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/i
THE
CHEMISTS' MANUAL:
PRACTICAL TREATISE ON CHEMISTRY,
\
QUALITATIVE AND QUANTITATIVE ANALYSIS,
STOICHIOMETRY, BLOWPIPE ANALYSIS, MINERALOGY,
ASSAYING, TOXICOLOGY, ETC., ETC., ETC.
BY
HENRY A. MOTT, Ju., KM., Ph.D.,
MxNnro ElNoimesR and Amalttioal CmnnsT, Mkxber or the American Chemical
80CTBTT, MsMBEB or THE New Tork Academt op Scibhceb, Fellow of
THE Obogbapbioal Sooiett, Etc, Eto., Eto.
't/
\^
NEW YORK
D. VAN NOSTRAND, PUBLISHER,
28 MURRAY STREET & 27 WARREN STREET.
Jf^^rll
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1^
^fe
Copyright, 1877, by Henry A. Mott, Jr.
30^
Electrotyped by Printed by
SMITH & McDOUGAL. J. J. UTTLE & CO.
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1
^^ry H E literature of Analytical Chemistry, in the Tarious
-■- branches of qualitative, quantitative, blowpipe and tech-
nical analysis, ^nd assaying, has expanded to such a degree
as to make it impossible for students, and even for most pro-
fessional chemists, to possess a complete library in these depart-
ments of the science : moreover, much of the literature is sealed
to many chemists by being published in French and German,
or in jonmals and transactions of Societies which are inac-
cessible. A further embarrassment arises from the multiplicity
of methods given in special woAs, from which few can select
without first testing several.
This carefully prepared Manual of Dr. Mott will prove
especially valuable, as containing a judicious selection of the
most important methods, most of which have been tested by
laboratory experience, and found to give satisfactory results.
These are presented in a concise form, with reference to original
authors. The numerous tables of constants will also be found
of great value.
This work will possess a special value for the student and
laboratory worker, and will serve as a useful reference book for
the general scientific reader.
CHAS. F. CHANDLEB, Ph.D., M.D., LL.D., F.C.S., Etc.
\
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/
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PREFACE.
/^If the principle that every scientific man " should compile
^^ his own pocket-book, as he proceeds in study and prac-
tice, to suit his particular business,** the Author accumulated
from time to time a large number of valuable notes and tables,
which became too voluminous to be carried in the pocket, and
soon grew in the form of manuscript. After repeated requests
by a number of prominent scientific men, the Author has
decided to present the manuscript, greatly enlarged and im-
proved, to the public The object of the Author has been to
accumulate only matter which has a practical value attached
to it.
Under the Department of Qualitative Analysis, the Author
has adopted the method or classification presented in a work
commenced by Tuttle and Chandler, and has consulted various
works on the subject, especially Fresenius' Qualitative Analysis
and Watts' Dictionary of Chemistry. It has been the object of
the Author to furnish formulae for all compounds and precipi-
tates considered, as they have recently been determined. The
Schemes presented will be found very practicable and accurate,
as has been demonstrated by frequent use.
Under the Department of Mineralogy, only the principal
minerals of those elements which have found use in the Arts
are considered. Free use has been made of Dana's Mineralogy,
as also Egleston's Lectures on Mineralogy.
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vl PREFACE.
Under the Department of Quantitative Analysis, Schemes
are presented for the most frequent occumng compounds met
with in e very-day analyses, all of which have been frequently
tested and found accurate.
Under the Departinent of Assaying y brief and accurate meth-
ods are described for the assay of those ores usually met with
in the laboratory. In preparing the method described for the
assay of gold and silver ores, the Author was greatly assisted
by a valuable pamphlet (reprint from the "American Chemist"
for 1870) by T. M. Blossom, E.M.
In the Miscellaneous Departmenty the Author has compiled
a large number of tables which cannot help but possess a prac-
tical value.
It has been the intention of the Author to furnish the author-
ity for all analyses and tables presented m this work; and if
any have been omitted, by communicating direct to the Author,
all claims will be promptly acknowledged.
The various subjects considered in this work opens a channel
for it among Chemists, Pharmaceutists, Physicians, and Scien-
tific men in general.
The Author is quite familiar with the fact that a work of.
this character must open much room for criticism; still he
hopes it will prove on the whole acceptable to all.
AUTHOR
98 Waix Stkbbt, Feb, 7, 1877.
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TABLE OF CONTENTS.
PAOS
tabiieb of the elements 3, 4, 5, 6
Specific Heats 7, 10
QUALITATIVE ANALYSIS 11
Defobtment of the Metals and theis Salts with
Reagents 18-154
Scheme for Qualitativb Analysis 138-146
Detection of Acids 147-154
Table of Analytical Chemistry 155-169
Zettnow's Scheme for Qualitatite Analysis 170
Scheme for the Alkaloids 172
Reactions of Fat Oils 176-179
Fat Oils 180-184
Pharmacopcbial Preparations — Tests for Impurities. 185-192
Organic Substances — Influence on the Precipitation
of Metallic Oxides 193
BLOWPIPE ANALYSIS 195
Casamajor's Table 196
Table of Volatile Elements 198
Scheme for Blowpipe Analysis 200
SPECIFIC GRAVITY DETERMINATIONS 207-212
Hydrometer Degrees , . . 213, 214
Alcohol—Specific Gravity of Solutions 210
Hydrochloric Acid— Specific Gravity op Solution... 220
Nitric Acid — Specific Gravity op Solution 221
Phosphoric Acid— Specific Gravity of Solutions 223
Sulphuric Acid " " " " 225
Ethylic Ether " ** " " . 226
Ammonic Hydrate " " " " 227
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viii TABLE OF CONTENTS.
PAGS
PoTABSic Hydratjb— Specific Gkavitt op Solutionb ... 229
SoDic Hydrate " " " " ... 230
Acetic Acid *' " *' " ... 231
Glycerin " " " " ... 232
Specific Gravity of Official Liqcidb 232
Table of Specific Gravity and Weights 235
MINERALOGY 241
Principal Minerals 243.
Coal 836
Petroletik 348
Scale of Hardnesb 850
STOICHIOMETRY 858
Table of Solubility 860
Table of Reduction of Compounds found to Con-
stituents Sought 862
QUANTITATIVE ANALYSIS 871
Iron Ore Analysis 873
Cast Iron " 884
Chromic Iron " i 888
Pig Lead ** 890
Nickel Ore " 892
Copper Ore " 893
Zinc Ore " 894
Pyrolusite " 895
Ilmenite " 897
Orthoclase •• 898
DOLOMITB * 899
• White Lead " ^ 400
Type Metal " 401
Silver Coin " 402
Fertilizer " 408
Water " '.. 404
Coal '* , 421
Gunpowder " 423
Glass « 425
Chlorimetet 427
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TABLE OF CONTENTS. ix
PAQB
Oroahic Analtbis .... . 431
Urikb " 450
BiX)OD ** 447
Milk ** 457
SnoABS 462
" Examinations 472-486
ASSAYING 487
Iron Okb Asbat 480
Gold and Silver Assay 494
Lead Ores, Assay ov 614
Antimony, " 616
Plattntm, " 616
CHEMISTRY OF MAN 617
Analysis of Secretions 620-{»44
BOSCELLANEOUS department 645
Elements, Classification of 647
Table of the Defunct Elements 664
Price of Metals 656
Agricultural Products 667
Fruits, Composition of 672
Glycerin as a Solvent 678
Formula of FREQUENTLY-oocuRRiNa Substances 678
formulib of frequently-occurrina acids 581
Artificial Formation of Organic Bodies 584
Alcohols 585
Alloys and Compositions. 587
Available Oxygen in a few Oxygen Compounds .... 689
Old Names for a few Salts 590
Poison and their Antidotes 592
Thermometers 598
Different Remarkable Temperatures 602
T M. . - T>^^^,,p Tv>TVTs OF Saturated Solutions 608
t'Ai'.'Mni 11 l)!:(.s».. • 604
W:'.l;> ^y Mk\ r iiES 605
r^'. . <. TiiK .. of Standard Coins in Circula-
...y !* ^ > • h SY 614
o
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TABLE OF SPECIFIC HEATS.
TABLE OF SFECmC HEATS OF ELEIENTARY SUBSTANCES.
KAMx or njasTAXcm.
AlaminiuzD,
Antimonj, .......
Anenic,
(ciystalliaed), - - -
" (amorphoas), - - -
Bismnth,
Boron (uDorpbouB), ....
" (crystalliaed), - - - -
Cbdmiom,
Caldmn.
Carbon (natural graphite)^ - -
" (purified),
M M U _ _
" (gas carbon), - - - .
(purified),
tf M ft a
M « u
(iron graphite), - - -
a « « ...
(diamond),
popper,
Indium, - -
Iron.
L«id,
Magnesium,
Rutnenium,
Selenium, (ciystalline), - - -
'* (amorphoufi), - - -
Silicon (graphitoYdal), - - -
« (crystalline), ....
" (fused),
surer.
** .........
Salphur (rhombic), . . - .
Tellorium,
Tin,
" (cast),
" (allotropic).
Zinc,
0.202
i .0495
.0523
.0680
.0758
.0805
.254
.280
.0542
.0548
.1670
.2019
.1977
.1955
.174
.1968
.2000
.2040
.185
.1961
.166
.1488
0.0930
.0570
.112
.0315
.245
.0611
.08401
.0860
.0958
.181
.165
.138
.0560
.0559
( .163 )
KbetrA40f
.1712
.0475
.0548
.0559
.0545
.0932
.0935
▲UTHOBITT.
Kopp.
Bunsen.
Kopp.
i Neumann (Pogg. Ann.
cxxvi. 137).
BettendorfTand WUllner.
do. do.
Kopp.
do.
do.
do.
Bunsen.
do.
j Regnault (Ann. Ch. Pbys.
} p], vii, 46).
Regnault.
BettendorfiTand WUllner
Kopp.
"^ ault
BettendorfiT and WaUner.
Kopp.
Bettendorff and Wtlllner.
Kopp.
Bettendorff and Wtlllner.
Kopp.
Bunsen.
do.
do.
do.
do.
Bettendorff and WtQlner.
Neumann.
Bettendorff and WQllner.
Kopp.
do.
do.
do.
Bunsen.
Kopp.
Bunsen.
Kopp.
do.
Bunsen.
do.
Kopp.
Bunsen.
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DEPORTMENT
OF
THE METALS AND THEIR SALTS
WITH REAGENTS.
GROUP I
Win contain Silyeb Salts, Mebcitbofs Salts, and Lead
Sali^ the Chlorides of which, namely, Abgentio Chlobibe,
Mebcitbous Chlobibe, and Plumbic Chlobide, are insoluble
or bnt sparingly soluble in water and in dilute acids, and are
therefore precipitated by Hydboghlobic Acid.
SILVER.
Sjmbol A^r.— Atomic weight, 108.— Equivalence, I and m.— Positive
Monad.— Electric condnctivity at 82" F. 100.00.— Specific gravity, 10.58.—
Specific heat, 0.0570.— Atomic volume, 10.04.— Fusing point, 1028" C—
Color, white. — Cat with a knife. — Order of malleability commencing with
gold, second ; ductility commencing with gold, second ; tenacity commencing
with (iron as 1000, silver as 849) ; heat-condncting power commencing with
gold, third.
SILVER OXIDES.
There are thbbe silveb oxides known.
Abgentio Oxide, AgjO, made by heating argentic car-
bonate to 200° C. ; it is a brown-black powder, having a Sp.
Gr. 7.143 (Herapath).
Abgentio Dioxide, Ag202, formed when concentrated
AgNOg is electrolyzed, with two thick platinum wires for
poles, and is deposited in crystals on the positive pole, while
metallic silver separates at the negative pole.
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14 THE CHEMISTS' MANUAL.
Abgentous Oxide, Ag^O,* is made by passing hydrogen
gas over argentic oxalate or citrate heated to 100° C. ; half the
acid is set free, leaving the asgentous oxide ; remove the acid
by water.
SILVER SALTS.
The silver salts are non-volatile and colorless; most of
them acquire a black tint when exposed to the light. Vege-
table colors are not altered by the soluble neutral salts, but
the salts are decomposed at red heat.
METALLIC SILVER.
1. Heated on Chabgoal, it fuses, and gives after a time
a red incrustation of argentic oxide (AgaO).
3. Hydrochloric Acid has very little, it' any, action on it.
3, Nitric Acid dissolves it slowly when cold, rapidly when
hot, evolving nitrogen dioxide (NjOg).
6Ag+8HN03=6AgN03 + N^+4H20.
4, Sulphuric Acid, when concentrated, dissolves silver
if heated, evolving sulphurous oxide (SO2). The solution
contains argentic sulphate (Ag2S04). Dilute acid has no
effect. .^A^
2Ag+2H2S04=Ag2S04 + S02 + 2H20.
I^ote.'^The silver of commeTce is usuaUy alloyed with copper ; it also
contains a trace of gold, which remains behind as a black powder when the
silver and copper are dissolved in nitric acid.^TuTTLE and Chandler.)
SALTS OF SILVER.
Solution best fitted for reaction :
Argentic Nitrate (AgN03).
6. Htdrochlorio Acid, when added to argentic nitrate,
produces a white precipitate of argentic chloride (AgCl) insol'
uhle in water and in nitric acid; readily soluble in am-
MONio HYDRATE and rcprecipitatcd by nitric acid.
AgN03 + HCl=AgCl+ HNO3.
* If this formula kgfi is correct, oxygen is a tetrad.
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THE CHEMISTS' MANUAL. 15
Note. — The argentic chloride becomes violet when ezpoeed to the light.
When mixed with a certain quantity of mercoroiiB chloride or fuming sul-
phuric add, this change of color does not take place. — (Tuttlb and
Chahbleb.)
6. Soluble cHLosmEs, Buch as NaCX KCl, etc, produce the
same result as hydrochloric acid.
AgN03 + NaCl=AgCl+ NaNOj.
SoDiG Thiosulphate (NagSjOa) dissolves ai^ntic chloride,
and prevents precipitation by potassic chloride ; but potassic
or sodic bromide or iodide added to the solution, precipitates
ABOENTIC BBOMmE Or lODmE.
2AgCl + 2Na2S203 = (NagSgOa + AgaSgOg) + 2NaCl.
(NaaSaOa'+AgaSaOg) + 2NaCl + 2NaBr=2AgBr + 2Na2S203 + 2NaCL
Potassic Cyanide dissolves argentic chloride forming
aboento-potassio cyanide,
AgCl + 2KCN=AgCN,KCN + KCl.
7. nTDEOSULPHTjRio AcH) produccs a black precipitate of
ARGENTIC SULPHIDE (AggS) iusoluble in dilute acids and in
ammonic sulphide (NH4HS), soluble in boiling nitric acid with
separation of sulphur.
2AgN03 + H2S=Ag2S+2HN03.
8« Ahmonio Sulphide ^acts the same as hydrosulphuric
acid.
2AgN03 + NH4SH=:Ag2S+NH4N03 + HN03.
9. Potassic Hydrate, when added, produces a light-brown
precipitate of argentic oxide (Ag20), insoluble in excess,
soluble in ABOfONIC HYDRATE.
2AgN03 + 2KH0=Ag20+2KN03 + H20:
10. Ammonic Hydrate added to neutral solutions pro-
duces a brown precipitate of argentic oxide soluble in excess,
No precipitate is produced in acid solutions.
2AgN03 + NH40H=Ag20 + NH4N03-fHN03:
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16 THE CHEMISTS' MANUAL.
U. P0TAS810 Beomtoe precipitates aegentio bbomide (AgBr)
yellowish in color, insoluble in water and acids, and much less
soluble in ammonic hydrate than the chloride, soluble in sodic
hyposulphite.
AgNOg + KBr= AgBr+ KNO3.
13. PoTASsio loDmE produces a pale-yellow flocculent
precipitate of argentic iodide (Agl), slowly acted on by light,
insoluble in acids and almost so in ammonic hydrate, soluble
in a concentrated solution of potassic iodide, and soluble in a
solution of sodic hyposulphite.
AgN03 + KI=:Agl + KN03.
The FOLLOWING are a few miscellaneous reactions :
3AgN03 + Na2HP04=Ag3P04 + 2NaN03 + HN03.
Ag3P04= Argentic Orthophosphate or Phosphate is a
canary-yellow product. Solution is acid.
AgN03 + NaP03=AgP03 + NaN03.
AgP03= Argentic Metaphosphate is a gelatinous mass.
4AgN03 + Na4P207= Ag^PgOj + 4NaN03.
^84^2^7= Argentic Pyrophosphate is a white precipitate.
*
2AgN03 + KaCr^Oy^^i^gaCraOy + 2KNO3.
Ag2Cr207= Argentic Bichromate, red-brown.
2AgN03-hK2Cr04=Ag2Cr04-f2KN03.
Ag2Cr04= Argentic Chromate, dark-brown precipitate, sol-
uble in ammonic hydrate and in dilute acids.
AgN03 + KCN=AgCN + KN03. ..
* ^ ^
AgCN= Argentic Ctanide is a white curdy precipitate, sol-
uble in excess of reagent, insoluble in dilute acids.
2AgN03 + Na2C03 = AgaCOs -f 2NaN03-.
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THE CHEMISTS' MANUAL. 17
Ag2C03=ABGBNTio Cabbonate, Bolublc in ammonic hydrate
and ammonic carbonate.
2AgN03+C2Hg04=Ag2C204+2HN03.
Ag2C204=ABGENTiG OxALATE, wlutc precipitate, soluble in
ammonic hydrate and sparingly in nitric acid.
3AgN03+C«H8K307=C,H5Ag30,+3KN0a.
'^ ^ '
C5H5Ag307= Aroentio CrrEATE, white powder.
C«H4Ag205= Aegentio Tabtbate, curdy precipitate, produced
^ t *
by mixing a dilute solution of argentic nitrate with a dilute
solution of Eochelle-salt (C3H4KNa05.4H20 potassio-sodic
tartrate) slightly acidulated with nitric acid.
Metallic Silver is PREciprrAXED by Zn, Cu, Fe, Hg, P, etc.,
SnCla, FeS04, ^^'
2AgN03+Zn=2Ag+Zn2N03.,
2AgN03+Cu=2Ag+Cu2N03.
4AgCl + 2Na2Co2+ A<5*=4Ag+4NaCl + 2C62+C)2.
AgN03+C+A<J=Ag+C02+N0.
13. Blowpipe. — Dry compounds of silver, mixed with
Bodic carbonate and fused before the blowpipe on charcoal,
yield malleable, metallic globules of pure silver without
forming an incrustation. — Chabacteeistio Eeaction, No. 5,
LEAD.
Sfinbol, Pb.— Atomic weight, 207. — Equivalence, II and IV.— Color,
binish white.— Cut by a knife.— Spedfic gravity, 11.36.— Fuses at 335" C.
(or 6\T F.—RUDBEBO).— Specific Heat, 0.0814.— Atomic volume, 18.24.—
Electric conductivity at 82° F. 8.32.— Order of malleability commencing
* Ad — Heat or fuse.
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18 THE CHEMISTS' MANUAL.
with gold, is the seventh; for dactility oommencing with gold, is the
eighth. — TeDacit7, iron as 1000, — Pb=50.— ^rder of heatroonducting power
commencing; with gold, is the seventh.
LEAD OXIDES.
Lead unites with oxygen to form five oxides:
Plumbic oxide, PbO ; Plumbous oxide, PbjO ;
Plumbic peroxide, PbOj ; Plumbic orthoplumbate, Pb304 ;
Plumbic meta plumbate, PbgOa.
PbgO Plumbous oxide may be produced if plumbic *ox-
alate is heated in a retort from which air is excluded, viz. :
2PbC204= PbgO +C0 +3C0^.
PbO Plumbic oxtoe (Litharge) may be obtained pure by
igniting basic nitrate or the carbonate or oxalate in a platinum
crucible in contact with air, taking care the oxide does not
fuse, otherwise it would take up the metal from the crucible.
Pure oxide, lemon-yellow color, Sp. Gr. 9.4214.
Pb02 Plumbkj peroxide may be formed by exposing the
protoxide (PbO) suspended in water to the action of a stream
of chlorine gas. It is a brown powder; when heated gives
off oxygen, and is converted into red lead or protoxide.
PbaO^ Plumbic orthoplumbate = (2PbO.Pb02 or PbO.
PbjOa) Pb2Pb04, and is sometimes called red oxide; it is
formed when the protoxide is kept at a low red heat for a
considerable time in contact with air. It is a scarlet crystal-
line granular powder, Sp. Gr. 8.62 (Karsten).
PbjOg Plumbic meta plumbate (Pb.PbOg) may be obtained
by precipitating a solution of red oxide in acetic acid with
caustic alkalies or alkaline carbonate. It is a reddish-yellow
precipitate.
LEAD SALTS.
The salts of lead are non-volatile ; most of them are color-
less; the neutral soluble salts redden litmus-paper, and are
decomposed at a red heat.
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THE CHEMISTS' MANUAL. 19
Plumbic chloride, when heated with accesB of air, partially
Yolatilizea, and oxychloride of lead remaing behind.
METALLIC LEAD,
14. Heated on chasgoal, it ftises and gives an incrusta-
tion of plmnbic oxide, which is deep-yellow when hot, pale-
yellow when cold.
15. Hydbochloric acto has very little action on lead.
16. Nitric acto, when concentrated, acts very slowly on
lea^ ; but if it be diluted, especially if heated, it rapidly dis-
solves it, forming plumbic nitrate, which separates from the
solution sometimes in white crystals.
3Pb+8HN03=3Pb|N03-|-NX+4H20.
17. SuLPHUBic ACID, whcu hot aud concentrated, dissolves
lead and forms plumbic sulphate with evolution of sulphurous
oxide. Dilute acid does not act on lead.
Pb + 2(H2S04)= PbSO^-h S0^+ 2H2O.
LEAD SALTS
Solution best fitted for the reactions:
Plumbic "NriRATE (PbjNOa).
18. Hydbochlobic acid, when added to a solution of plum-
bic nitrate, produces a white precipitate of plumbic chloride
(PbCl2)5 which is soluble in a large amount of wateb ; there
is therefore no precipitate found in dilute solutions of lead.
In. every case a little lead escapes precipitation. Ammonic
hydrate does not dissolve or blacken the precipitate.
Pb2N03 + 2HC1= PbCla + 2H NO3.
19. Htdbosulphubic acid produces a black precipitate of
plumbic sulphide, which is insoluble in cold dilute acids, in
alkalies, alkaline sulphides, and^potassic cyanide.
Hot dilute nitric acid dissolves (if dilute enough) the precipi-
tate, forming plumbic nitrate, and separates sulphur. Fuming
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20 THE CHEMISTS* MANUAL.
nitric acid oxidizes the sulphur and converts the precipitate
into insoluble plumbic sulphate. If in the solution to be pre-
cipitated from, there is any excess of concentrated mineral acid,
such acid must be neutralized by the addition of water or an
alkali before the hydrosulphuric acid will precipitate the lead.
If the solution corftains an excess of free hydrochloric acid
the paecipitate may be red, consisting of plumbic sulphide and
plumbic chloride, which in time, with the addition of hydro-
sulphuric acid in excess, will be converted into plumbic sul-
phide.
Pb2N03 + H2S= PbS + 2H NO3.
30, Ammonio sulphide acts the same as hydrosulphuric
acid.
Pb2N03 + NH4SH=PbS+NH4N03 + HN03.
31, SuLPHUEio ACID produccs a white precipitate of plumbic
sulphate, which is nearly insoluble in dilute acids and water ;
concentrated nitric acid partially dissolves it; concentrated
hydrochloric acid, when boiling, dissolves it with difficulty;
a solution of potassic hydrate dissolves it more readily. Am-
monic acetate or citrate dissolves it, and dilute sulphuric acid
precipitates it again. In very dilute solutions of lead an ex-
cess of dilute acid should be added, as the precipitate only
forms after standing. Precipitate is blackened by hydrosul-
plmric add, 'which distinguishes it from baric and strontic
sulphate, which are insoluble. Plumbic sulphate, in the cold,
is soluble in watdr to the extent of ^^^ Fresenius ; in dilute
sulphuric acid, 'ishnf Fresenius ; almost absolutely insoluble
in alcohol. -
• Pb3Na3-fH2S04=PbS04 4-2HN03.
' ^ '
33« Potassic Hydbate produces a white precipitate of
plumbic hydrate (PbgHO), readily soluble in excess, and
almost insoluble in ammonic hydrate.
Pb2N03 4- 2KHO»Pb2HO + 2KNO3.
^ ^ ^
23. Ammonia produces a white precipitate of plumbic
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THE CHEMISTS' MANUAL. 21
hydrate (Pb2H0), insoluble in excess, but readily soluble in
nitric acid. In solutions of plumbic acetate, ammonic hydrate
(free from carbonate) does not immediately produce a precipi-
tate, owing to the formation of a soluble plumbic triacetate.
The filtrate from the precipitation should be examined, for
it will contain some lead if the ammonic hydrate is in excess
and there are ammonic salts present.
Pb2N03 + NH4H0=Pb2H0 + NH4N03+HN03.
24. PoTASsic Chromate or Dichromate produces a yellow
precipitate of plumbic chromate (PbCr04) which is insoluble
in acetic acid; sparingly soluble in dilute nitric acid, but
readily so in potassic hydrate. ^
Pb2N03+K2Cr04=PbCr04+2KN03.
2Pb2N03 + K2Cr207+H20=2PbCr04 + 2KN03 + 2HN03.
25. SoDic Carbonate produces a white precipitate of
PLUMBIC carbonate, together with plumbic hydrate, which
is insoluble in excess of the precipitant, and also in potassium
cyanide.
7Pb2N03 + 7Na2C03 + H20=(6PbC03 + Pb2HO)+ liNaNOj
+CO2.
26. Potassium Iodide precipitates plumbic iodide as a
beautiful light-yellow precipitate.
2KI + Pb2N03 = Pbig + 2KNO3.
Metallic lead is precipitated by zinc and iron out of its
soluble salts.
Pb2N03+Zn = Pb+Zn2N03.
Pb2N03 + Fe= Pb+ Fe2N03.
When plumbic sulphate is heated with carbon in the right
proportion, metallic lead is produced.
PbS04+C=Pb-fC0^ + S07.
27. Blowpipe. — Dry compounds of lead, when frised with
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22
THE CHEMISTS' MANUAL.
sodic carbonate on charcoal in the inner (reducing) flame, fur*
nishee very Boft, malleable globules of metallic lead, which
produces a mark on paper like a pencil. A yellow incrustation
is formed at the same time, which becomes quite pale when cold.
LIMIT OF REACTIONS OF TESTS FOR LEAD.
asm PABT OF
m WATBB.
BMJLQWn.
AT7TBOBITT.
Lead
100,000 or more.
900,000
800,000
100,000
90,000
96,000
70,000
SalphydrlcAdd.
ii u
it u
H.SO« in exceea.
Na,S0«iiil5inin.
Chromate of Potaestom.
A. S. Taylor.
LaaMl^De.
Hardng.
PftUr.
Pfhff A Harting.
LaatAlgne.
Harting.
Lead as Nitrate
Oxide of Lead ae Nitrate
Nitrate of Lead
Oxide as Nitrate
Leadaa ''
Oxide as "
Chaeaotebibtio
EEAOnONS,
MERC
18, ai, 27.
JURY.
Symbol Hg (Hydnagyram from Mopapyvpov, Uquid silver or quickBilveT).
—Atomic weight, 200.— Equivalence (Hg,) and II.— Density, 100.— Mo-
lecnlar weight, 206.— Molecular volume, 2. — One litre of mercury vapor,
weight 8.96 grains (100 criths).— Specific gravity, 18.696 at 82° F.— Solidifies
at -40** F. ; boils at SSO** F.— Vapor, Sp. Gr. 6.976.— Electric conductivity,
1.68 at 78** F.— Atomic volume, 14.66.
MERCURY OXIDES.
There are two mebourt oxides known:
Meboubic OXIDE HgO, or red mercnric oxide, also called
binoxide and deutoxide.
When mercurous or mercnric nitrate is exposed in a glass
vessel surrounded with sand, to heat, as long as nitrous oxide
is evolved, mercuric oxide is formed. The commercial oxide
has a bright brick-red color, shining crystalline grains. Sp.
Gr. 11.074 (Herapth) of precipitated.
Mebcuboub Oxide HgsO. Black mercurous oxide, also
called dioxide and suboxide.
When a solution of mercurous salt is mixed with an excess
of caustic alkali, mercurous oxide is precipitated. Brown-black
powder. Sp. Gr. 10.69 (Herapth) of that obtained from calomel.
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THE CHEMISTS' MANUAL. 23
METALLIC MERCURY.
28. Heated m a tube, having one end closed, it boils,
and in the cool part of the tube minute shining particles con-
dense.
29. Htdbochlobio acid does not attack metallic mercury.
30. NrrBic acid, if dilute and cold, dissolves the metal
dowlj, and the solution contains mercubous niibate.
Dilate. -.^A— .
6Hg+8HN03=3Hg2(N03)2+N202+4H20.
Concentrated acid, when hot, dissolves the metal rapidly,
forming mebgusio NrrBATE.
3Hg+8HN03=3Hg(N03)2 + N202+4H20.
31. SuLPHUBio Acm, when concentrated and in excess, if
heated, dissolves the metal with evolution of sulphurous oxide,
forming meboubic sulphate.
Hg+2H2S04=HgS04+S0^+2H20.
When the metal is in excess of the acid, a mixture of mer-
cnrous and mercuric sulphate is obtained. Dilute acid does
not act upon the metal.
SALTS OF MERCUROUS OXIDE.
The mercurous salts volatilize on ignition ; most of them are
decomposed by this process. Mercurous bromide and chloride
volatilize unaltered. Mercurous nitrate is decomposed on the
addition -of much water into a pale-yellow insoluble basic and
soluble acid salt. The soluble salts in the neutral state redden
litmus-paper. Most of the salts are colorless.
ScltUion best JUied far reactions :
MEBCtJKOUS NrniATE Hg2(N03)2.
32« Htdrochlobio Acm precipitates a powder of dazzling
whiteness, mebcubous ohlobide (Hg2Cl2) (calomel).
Hg22N03 + 2HCl=Hg2Cl2+2HN03.
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24 THE CHEMISTS' MANUAL.
Insoluble in water and dilute acids. Hydrochloric and
nitric acids, after long boiling, dissolves it. Nitrohydrochloric
acid and chlorine dissolve it readily, converting it into mer-
curic chloride. Amnionic hydrate and potassic hydrate hlackev
mercurous chloride ; when potassic hydrate is used, the black
mercurous oxide is precipitated (§ 36) ; when amnionic hydrate
is used, MEBCUBOUs-AHHONicM CHLOBiDE (NH3Hg)2Cl2 is pro-
duced.
Hg2Cl2+2NH40H=(NH,Hg)2Cl2 + 2H20.
33. Soluble chlorides produce the same precipitate as
hydrochloric add.
Hg2(N03)2 + 2NaCl = Hg2Cl2 + 2NaN03.
34. Hydrobtjlphuric acid produces a black precipitate of
MERCUROUS SULPHIDE (Hg2S) ; insolublc in ammonic sulphide,
dilute acids, and potassic cyanide ; easily soluble in nitrohydro-
chloric acid, but not by hailing concentrated NirRio Acm, which
does NOT ATTACK IT.
Hg2(N03)2 + H2S=Hg2S+2HN03.
35. Ammonic SULPHIDE produces the same precipitate as
hydrosulphuric acid.
Hg2(N03)2 + N H4HS= Hg2S + N H4NO3 + H NO3.
36* Potassic hydrate produces a black precipitate of
MERCUROUS OXIDE.
Hg2(N03)2 + 2K0H = Hg20 + 2KN03 + H20.
Precipitate is insoluble in excess. Sodic hydrate produces
the same precipitate.
37« Ammonic hydrate produces a black precipitate of
2NH3.3Hg2O.N2O5, which is a hydrated trimercurous am-
monium NrrRATE. 2(NHHg3)N03.2H20 (according to C. G.
Mitscherlich), but according to Kane, 2(NH2Hg2)N03.H20 (di-
mercurous ammonium nitrate). The precipitate is velvet-black,
and is known as " Hahnemann's Soluble Mercury."
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THE CHEMISTS' MANUAL. 25
METALLIC MERCURY PRECIPITATED.
38, Stannous chloride produces a gray precipitate of mb^-
TALLic MERCURY, which may be united into globules by boiling
the metallic deposit, after decanting the fluid with hydro-
chloric acid, to which a drop of stannous chloride may be
added with advantage.
39. Metallic copper, when introduced into a solution of
mercury, becomes covered with a lustrous coating of metallic
mercury. K the coated copper be dried and heated, it as-
sumes its original color, the mercury being volatilized,
Hg22N03-fCu=2Hg+Cu2N03.
"Copper wire or foU, in pieces aboat one inch in length, may be used for
this test. They shooid be first^lipped into etrong nitric acid, and well washed.
The mercarial solution should be acidulated with a few drops of dilate nitric
add, and then boiled for a few minutes with the strips of copper. These
ate then to be removed, washed, dried between folds of paper, and grently
heated in a small glass tube, closed at one end. A shining ring of minute
globules of mercury will condense above the copper, which now resumes its
original color. This method is often used to separate mercury from organic
substances, in examining vomited matter, and in case of poisoning." — (TuT-
TXB AND CHANDIiEB.)
40, PoTABSio CYANIDE precipitates mercury.
( Hg22N03 + 2KCN=Hg2(CN)2+2KN03-
(Hg2(CN)2=Hg+Hg(CNV
There is first formed Hgj (CN)2, which is resolved into mer-
curic cyanide Hg(CN)2 and metallic mercury.
Mbtallig mebcust is separated as a gray powder by zinc,
sulphurous add, and phosphorous acid.
41. NriEic ACID converts all mercurous salts into mercuric by
boiling.
A FEW MISCELLANEOUS REACTIONS.
PoTASsio IODIDE, whcu added to mercurous nitrate, forms a
greenish-yellow precipitate of mebcubous iodide (always, how-
ever, mixed with mercuric iodide), soluble in excess.
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26 THE CHEMISTS' MANUAL.
PoTASBic FBBBOOYANiDE, wlien added to mercurous nitrate,
forms a white, and fotasbio FEBBioYAKmB a reddish-brown
precipitate.
Sodic phosphate and oxalic acid form white precipitates
with mercurous nitrate.
Hg22N03 + C2H204=C2Hgb4 -f 2HNO3.
3Hg22N03 + QNa^H P04=2Hg3P04 -f ^NaNOa + 2H NO3.
PoTAssio CHROMATE produces a brick-red precipitate when
added to mercurous nitrate.
Gallic acid produces a brownish-yellow precipitate when
added to mercurous nitrate.
42. Blowpipe. — ^Dry compounds of mercury mixed with
ten to twelve parts of dry sodic carbonate, and heated in a dry
glass tube, closed at one end, yield metallic mebcuby, which
condenses in minute globules in the cool part of the tube.
These may be united together into larger globules by rubbing
with a glass rod.
" To make this test more delicate, the meicuiy oompoimd should he <
folly dried ; the sodic carbonate should be ignited (on platinam foil) just
previous to ose. To prevent sublimation of any undecompoeed mercufy
compound, a layer of sodic carbonate should be placed above the mixture."
— (TUTTLB AND CHAin>LEB.)
Chaeacteristic Eeactions, 32, 39, 42.
DETECTION OF MEMBERS OF GROUP I.
Having noticed the different respective behaviors of the
chlorides of the members of this group, with water and am-
monic hydrate, we are able to make a scheme for their scparsr
tion and detection.
SCHEME FOR THE SEPARATION AND DETECTION OF
MEMBERS OF GROUP I.
The solution to be examined is supposed to contain a salt of
silver, mercurous oxide, and lead.
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THE CHEMISTS' BIANUAL.
27
Add to the Bolution hydrochloric acid; there is produced a
precipitate of argentic, plumbic, and mercorous chloride.
AgCl+PbCla + HgaCla.
Filter the precipitate and wash it) then boil the precipitate
in water and filter :
FiLTBATB.
The filtrate wUl oon-
tain PbCl, in aolntion.
Add salphnric add if a
precipitate is produced;
it is plumbic sulphate
PbSO^. (See §18; §27.)
BlBBinCB.
The letaodae wUl oontian AgCl + Hg^Clt.
ammonic hTdrate, and filter.
Add
Soivtian,
Solution will contain
the aUver salt. Add
nitric acid, which will
precipitate (AgCl) ar-
gentic chloride.
§6.)
(See
Betidue.
If black (see § 82) dia-
Bolve in (8HC1 + HN0.)
nitrohydrochloric acid.
Add stannous diloride
(SnCl,) in excess, which
will deposit metallic
mercury (Hg). (See
§88.) ^
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G-ROUP II.
This group contains the metals not peecipita.tbd by Hydbo-
CHLOBio Acid, but precipitated from their acid solutions by
Hydbosulphubio Acid.
FIRST DIVISION.
Salts of the metals, the sulphides of which are inboluble m
AHHONIC sulphide.
SECOND DIVISION.
Salts of the metals, the sulphides of which are soLtrBLB in
4MMONIC SULPHIDE.
FIRST DIVISION.
Salts of Lead,* Mercury, Copper, Cadmium, and Bismuth.
SALTS OF MERCURIC OXIDE.
Solution heat fitted for the reactions :
Meeoubio Chlobidb (HgCl2).
The SALTS of MERCuKio OXIDE volatilizc upon ignition ; most
of them are decomposed by this process. Mercuric chloride,
bromide, and iodide volatilize unaltered. Mercuric nitrate
and sulphate are decomposed by water (added in large quan«
tity) into soluble acid and insoluble basic salts. The soluble
neutral salts redden litmus-paper. Most of the salts of mer-
curic oxide are colorless.
* The reactions of the salts of lead have been given § 18 et seq. ; it is
introduced here for the reason that very dilate lead solations give no pre-
cipitate with hydrochloric add, bat are precipitated by hydrosulphoric acid.
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THE CHEMISTS' MANUAL. 29
43. HYBBOfiiTLPHTTBio ACID, when added to a solution of
mercuric chloride in small quantities, produces a white or
yellow precipitate (HgCl2+2HgS). On the addition of more
of the precipitant, the precipitate formed passes from white to
yellow, to orange, to brownish-red color, and finally to black
if enough has been added. I%is distinguishes the mercuric
ooffide from all other bodies.
HgCl2 + H2S=HgS+2HCl.
Mescubio sulphide is not dissolved by ammonic sul-
phide, potassic hydrate, or potassic cyanide; insoluble in
boiling nitric or hydrochloric acid. Dissolves completely in
potassic sulphide, and is readily decomposed and dissolved
by nitrohydrochloric acid.
44. Amhonio sulphids produces the same precipitate as
hydrosalphuric add.
HgCl2+NH4HS=HgS+NH4Cl + HCl.
45. Potassic hydrate, added in small quantities to a
neutral or slightly acid solution, produces a reddish-brown
precipitate, which acquires a yellow tint, if reagent is added in
excess. The reddishrbrown precipitate is a basic salt; the
yellow precipitate consists of iqercuric oxide.
HgCl2+KH0=Hg0-t-^KCH-HCl. ^^
In very add solution the precipitation is very incomplete.
When the solution of mercuric chloride contains an excess of
ammonic chloride, the precipitate is analogous to that pro-
duced in § 40.
46. Ammonic hydbate produces a white precipitate, if
ammonic hydrate be in excess [HgCl2(NH2)2] ; if mercuric
chloride be in excess [2HgCl2(NH2)2].
47. Potassic iodide produces a scarlet predpitate of mer-
curic iodide (Hgig).
HgCl2 + 2KI = Hgl2 + 2KCl.
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30 THE CHEMISTS' MANUAL.
Soluble in excess of either salt. This difficnltj may be
avoided by adding a drop of potassic iodide to the white pre-
cipitate by amnionic hydrate, § 40, which will change to a
chocolate-red Hgl^.
48. Stannous chloiude, when added in small quantities,
produces a precipitate of mercurous chloride.
SHgCla + SnCl2= HgaCla + SnCV
If added in excess and boiled, the mercurous chloride at first
formed is reduced to metal.
HgaClj + SnCla = Hgj + SnCl^.
The metal may be united into globules by boiling with
hydrochloric add and some stannous chloride.
49. Blowpipe. — The behavior of the mercuric salts is the
same as the mercurous salts ; therefore see § 36.
CHABAOrEKISTIO REACTION, 39y 43, 47, 42, 49.
A FEW MISCELLANEOUS REACTIONS.
FoBiao AOiD REDUCES metcurio chloride to mercurous
chloride.
Ahmonio garbonatb produces a white precipitate with
mercuric nitrate.
Potassio carbonate produces a yeUow precipitate of HgO.
Hydro-potassio carbonate and hydrosodic carbonate pro-
duces a brown-red precipitate in mercuric nitrate^ and a white
precipitate turning red in mercuric chloride. Precipitate
(2HgO,HgCl2).
Some phosphate produces a white precipitate.
Potassio ferrooyanide produces in solutions not too dilute
a white precipitate turning blue, prussian blue being formed
while filtrate contains mercuric cyanide.
Potassio ferricyanidb produces a white precipitate with
mercuric nitrate, and none with mercuric chloride.
Tincture of galls forms an orange-yellow precipitate in
all solutions except m^curic chloride.
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THE CHEMISTS' MANUAU 31
COPPER.
Symbol, Cu. (Latin, Cuprinm, Cnpiiis).— Atomic wdght, 88.5.— EqnivBr
lenoe (Cu,)°- and IL — Color, flesh-Ted. — Crystols, isometric. — Specific ^ravitj,
a952.— Auymic yolnme, 7.10.— Specific beat, 0.0951.— Fnaiiig point, 1096^ F.
—Electric oondnctivity at 32" F. ia 99.95.-^rder of maileability commeno-
iDg witb gold is tbiid ; Ductility, flfUi ; Heat-condnctiiig power, fourth. —
Tenadt7=650.
COPPER OXIDES.
There are two well-determined copper oxides, and two un-
certain oxides.
CuPBous OXIDE, CU2O9 also called dioxide, suboxide, and
red oxide of copper. Found native in two forms as (rothkup-
ferey and) red copper and copper hlooniy chalotrechite (kupfer-
bluflie). Ignite 29 pts. copper-filings with 24 pts. anhydrous
cupric sulphate, and cuprous oxide is obtained. Hydrochloric
acid forms, with cuprous oxide, cuprous chloride, which is
easily decomposed by water. Kitric acid converts it into
cupric nitrate ; most other acids decompose it, forming cupric
aalts and depositing metallic copper. Very few oxygen salts
known ; sulphites and double sulphites with alkaline metals.
CuFBio oxiDB, CuO, black oxide of copper. Found native as
malaoonite. Prepared by exposing cupric sulphate to an in-
tense heat, or cupric carbonate or nitrate to a moderate heat
Seduced to metal by hydrogen, when ignited with it, or char-
coal. Potassium or sodium also reduce it to a metallic state.
Sesquioxidb of oopfbb, CU2O3; not known in a separate
state. Mix chloride of lime with a solution of cupric nitrate
and there is formed calcic cuprate, a beautifiil rose-colored
substance ; it decomposes but slowly. Most other salts are de-
composed with violent evolution of oxygen, soon after formation.
Pjsboxidb of ooppeb, CuOg ; formed by agitating cupric
hydrate with a large excess of hydrogen peroxide at 0** C. It is
a yellowish-))rown powder. Insoluble in water, with acids it
forms ordinary cupric salts and hydrogen peroxide. It may
only be a compound of cupric oxide and hydrogen peroxide,—
(Thenabd.)
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32 THE CHEMISTS' MANUAL.
METALLIC COPPER.
50* Heated on ohasooal it becomes coated with capric
oxide ; it fuses with difficulty, and gives no incrustation.
51. Htdboohlobio acid has very little action on metallic
copper.
63. NriEio Aom dissolves it readily, forming cupric nitrate
and evolving nitrogen dioxide.
3Cu + 8HN03=3Cu2N03 + n5^+4:H20.
53. SuLPHUBic ACID, wheu hot and concentrated, rapidly
dissolves copper, forming blue cupric sulphate (CUSO4), and
evolving sulphurous oxide. Dilute acid has but little action
on copper. .^^j^
Cu+3H2S04=CuS04+S02 + 2H20.
54. NrrEOHYDEOCHLOEic ACID dissolves copper, forming
cupric chloride and evolving nitrogen dioxide (NgOj).
3Cu'+2(3HCl + HN03)=8CuCl2 + N^+4:H20.
SALTS OF COPPER.
" Most of the neutral salts are soluble in water ; the soluble
salts redden litmus-paper, and suffer decomposition when
heated to gentle redness, with the exception of the sulphate,
which can bear a somewhat higher temperature. They are
usually white in the anhydrous state ; the hydrated salts are
usually of a blue or green color, which their solutions continue
to exhibit even when much diluted,''
Solutions heat fitted for the reactions:
Cupric Sulphate (CUSO4).
55. Hydrosulphuric Acro produces a black precipitate of
cupric sulphide.
CuS04+H2S=CuS+H2S04.
Cupric sulphide is slightly soluble in ammonic sulphide,
completely soluble in boiling nitric acid, and dissolves com-
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THE CHEMISTS' MANUAL. 33
pletelj in potassic cyanide ; not solnble in dilute sulphuric or
hydrochloric acid.
56. Ammonic 8TjLPHn>£ produces the same precipitate as
hydrosulphuric acid.
CUSO4+ NH^HS=CuS + NH^HSO^.
57. PoTABSic HYDRATE producos a light-blue bulky precipi-
■ tate of cuPMC hydbate (Cu2H0).
CuS04+2KH0=Cu2H0+ K2SO4.
Insoluble in excess. When heated, turns black, forming cu-
PRic oxms.
"* The preeienoe of fixed organic matters (sogta, tartaric acid) causes the
hjdiate to rediseolve in excess of potassic hydrate with a deep-blue color." —
(TUTTLE AND ChAKDLGR.)
68. Ammonio hydbate produces a greenish-blue precipitate
of a BASIC SALT (CuS04.+2Cu2HO), when added in a small
quantity; in a large quantity the precipitate dissolves, im-
parting to the liquid a deep azure-blue color, forming (NH3)2
CuO-f(NH4)2S04.. This test distinguishes copper from most
other substances.
3CuS04+4NH^H0=2Cu2H0+CuS04-f2(NH4)2S04.
69. SoDic CAEBONATE produccs a greenish-blue precipitate
of cupric carbonate and cupric hydrate (CuC03-f-Cu2H0),
with the evolution of carbonic oxide.
2CuSO4 + 2Na2C03-hH20=CuC03 + Cu2H0-|-C02 + 2Na2S04.
This precipitate, on boiling, is converted into cupric oxide.
60. Potassic febrocyanide produces a chocolate-colored
precipitate of cupric ferrocyanide (CugFeCgNg).
2CUSO4 + H4FeCfiNg=Cu2FeCfiNfi -t-2H2S04.
Insoluble in dilute acids, but readily soluble in ammonic
hydrate. Decomposed by potassic hydrate, with the forma-
tion of cupric hydrate and potassic ferrocyanide.
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34 THE CHEMISTS' MANUAL.
To very dilute solutions of copperj potassic ferrocyanide
imparts a reddish color, which is a more delicate indication
than the ammonic hydrate reaction, being still visible in a
solution containing 1 pt. of copper in 400,000 pts. of liquid
(Lassaigne), and in 1,000,000 pts. (Sarzeau).
Dissolves in ammonic hydrate, and forms on evaporation,
which produces a most delicate test. Thus, if a solution con-
taining copper and iron be treated with anmionic hydrate in
excess, a few drops of potassic ferrocyanide added, the liquid
filtered, and filtrate evaporated in a small porcelain crucible
or capsule, cupric ferrocyanide is left behind, exhibiting char-
acteristic red color (Warrington Chem. Soc., Qu. J. v. 137).
Before applying the test, the solution should be acidulated
with acetic acid. If strong mineral acids present, they should
be neutralized by adding excess of potassic or sodic acetate.
61. Potassic CYANroE produces a precipitate of cupbio
CYANmE Cu(CN)2, which is yellow-green.
CuS04+2KCN=Cu(CN)2-|-K2S04.
Solvhle in excess. Hydrochloric acid throws down from this
solution cuprous cyanide soluble in excess of acid ; hydrosul-
phuric acid and ammonic sulphide produces no precipitate
with this solution.
62. Potassic iodide produces a yellow precipitate of cupbio
IODIDE with separation of iodine.
63. Metallic ikon, when introduced into a solution of
copper, acidulated with a few drops of hydrochloric acid, be-
comes coated with a characteristic film of metallic copper of
coppery-red color.
CUSO4 -h Fe = Cu 4- FeSO^.
If the solution containing copper be introduced into a plat-
inum dish with a little free hydrochloric acid and a piece of
zinc introduced, the platinum becomes rapidly covered with a
coating of copper.
Pt+CuS04+Zn=ZnS04+Pt4-Cu.
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THE CHEMISTS' MANUAL. 35
64* Blowpipe. — ^If a dry compound of copper is fused with
a little Bodic carbonate and potassic cyanide on charcoal in the
reducing flame of the blowpipe^ there is produced a globule
of METALLIC COPPEB. No incrustatiou is formed. If the fused
mass is triturated with water in a mortar, the charcoal particles
are washed ofl*, leaving shining scales of metallic copper per-
fectly visible when only a minute quantity of the compound
is used.
65. Borax and sodio phosphate readily dissolve cupric
oxide in the outer flame. Beads are green while hot, and blue
when cold. Any compound of copper imparts to borax bead
fused on platinum wire in the outer flame, a green color while
hot, and hltic when cold. If this bead is detached and heated,
on charcoal, with a little metallic tin, the bead becomes red
and opaque^ and colorless when only a minute quantity of
copper is present.
In the inner flame the borax bead is made colorless, that
produced with sodic phosphate and ammonia turns dark-green ;
both acquire a brownish-red tint upon cooling.
Chabactebibtic Eeachons, 58, 60, 63, 64, 65.
CADMIUM.
Symbol, Cd. (Greek, Cadmia— Calomine). — Atomic weight, 112. — Equiva-
lence, IL — Density, 60. — Molecular weight, 112. — ^Molecular volume, 2. —
Discovered in 1817 by Hermann and also by Stromeyer. — Specific gravity,
8.604.— Becomes brittle at 82" C— Boiling point, 1580° F.— Fusing point,.
442' F.— Calculated Sp. Gr. of vapor, 3,869 ; observed spedfic gravity, 8.94.
—Atomic volume, 12.06.— Electric conductivity, at 82'' F., 23.72.— Order of
ductility commencing with gold, eleventh.— Color, grayish- white.
CADMIUM OXIDES.
Cadminm forms two oxides^ viz. : CdgO and CdO.
Cadmous oxide CdjO, or suboxide. This oxide may be ob-
tained by heating the oxalate to about the melting-point of
lead. ^ .^^
2C2Cd04+ A<J=Cd20-|-C0-|-3G02.
It is a green "powder resembling chromic oxide, and is re-
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36 THE CHEMISTS' MANUAL.
solved by heat or by acids into metallic cadmium and cadmic
oxide. It does not yield metallic cadmium with mercury,
hence it appears to be a definite compound and not merely a
mixture of the metal with cadmic oxide.
Cadmio oxtoe, CdO, or protoxide, may be obtained by heat-
ing metallic cadmium in the air, when it takes fire and is
converted into cadmic oxide. Formed also by igniting the
hydrate, carbonate, or nitrate. Sp. Gr. 6.9502. Insoluble in
water.
METALLIC CADMIUM.
66. Hydrochlobio acto, when hot, converts the metal into
CADMIC OHLOBTOE (CdCl2), liberating at the same time hydrogen
gas. ,o^
Cd+2HCl=CclCl2 + 2H.
67. SuLPHtTEio ACID, whcu dilute, converts the metal into
CADMIC SULPHATE and liberating hydrogen gas.
Cd + H2S0^=CdS04 + 2H.
68. NriRio ACID is the best solvent for the metal, convert-
ing it into CADMIC NiTEtATE (Cd2N03) and liberating at the
same time nitrogen dioxide.
3Cd + 8HN03=3Cd(N03)2 + NS+4H2O.
69. Heated on charcoal, it fuses and deposits a reddish-
brown incrustation of cadmio oxide.
CADMIUM SALTS.
Most of the cadmium salts are colorless ; they have a dis-
agreeable metallic taste, and act as emetics. The solutions,
even of the neutral salts, redden litmus-paper. The salts are
decomposed by heat.
Solution best fitted for the reactions:
CADmC NlTBATE (Cd2N03).
70. HYDRosuLPnuRic ACID producos in a solution of cadmic
nitrate a bright-yellow precipitate of cadmic suLPHroE (CdS).
Cd2N03-|-H2S=CdS+2HN03.
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THE CHEMISTS' MANUAL. 37
The Bolatioii, if acid, must be largely diluted, as the precipi-
tate CdS is soluble in concentrated hydrochloric acid ; not sol-
uble in very dilute hydrochloric, sulphuric, or nitric acid, but
soluble in boiling hydrochloric and sulphuric acids ; not soluble
in alkalies or ammonic sulphide. Cadmic sulphide is the only
yeJJUfW sulphide not soluble in cmimonic sulphide.
71. Ammonic sulphide produces the same precipitate as
hydroeulphuric acid.
Cd2N03 + NH4HS=CdS+HN03 + NH4N03.
72. PoTAssic HYDRATE produccs a precipitate of cadmio
HYDRATE, which is whitc ; insoluble in excess of precipitant.
Cd2N03-h2KHO = Cd2HO-|-2KN03.
73. Ammonic hydrate produces a white precipitate of cad-
mio HYDRATE, solublc in cxcoss.
Cd2N03+2NH4H0=Cd2H0+2NH4N03.
\ y i/
74. Ammonic carbonate produces a white precipitate of
CADMIC carbonate, insolublc in excess. Dissolves readily in
potassic cyanide.
Cd2N03+(NH4)2C03=CdC103 + 2NH^N03.
^ ^ '
75. SoDic phosphate precipitates cadmic orthophosphate
(CdgPjOe). A white powder.
3Cd2N03 + 2Na2HP04=Cd3P208+4NaN03 + 2HN03.
76. Ammonic oxalate produces a white precipitate when
added to cadmic chloride of cadmic oxalate (CdC204..3H20);
soluble in ammonic hydrate.
CdCl2 + C2(NH4)204+3H20=CdC204.3H20 + 2NH4Cl.
*■ ^ *
77. Potassic ferrocyanide produces a white precipitate.
2Cd2N03 -h K4Cfy=Cd2Cfy+4KN03.
78. Potassic ferricyanide produces a yellow precipitate,
soluble in hydrochloric acid.
3Cd2N03-t-KgFe2C,2N,2=Cd3Fe2C,2N,2 + 6KNOs.
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38 THE CHEMISTS' MANUAL.
METALLIC CADMIUM PRECIPITATED.
Zd^o precipitates metallic cadmium from its salts (in den«
drites).
Ccl2N03+Zn=Cd-|-Zn2N03.
79. Blowpipe. — When a cadmium compound is mixed
with sodic carbonate and fused on charcoal in the inner flame
of the blowpipe, there is produced a reddish-brown incrusta-
tion, of cadmic oxide, which becomes very distinct on cooling;
no metal is produced.
Chasactebibtio Beactions, 7O9 79.
BISMUTH.
Symbol, Bl. (German, towTRo^).— Atomic weight, 210.— EqoiTalenoe, m
find v.— Specific gravity of solid, 9,830.— Fusing point, 607^ F.— Atomio
volume. 21.84— Specific heat, 0.0808.— Electric conductivity at 82" F., 1.24S.
— Order of brittlenees oommenciug with antimony ib third.
BISMUTH OXIDES.
Bismuth forms two definite oxides, and two others.
BisMUTHOus OXIDE, BijOa, or trioxide. — Formed when bis- .
muthous nitrate is gently ignited. It is a pale-yellow powder,
which melts at red-heat. It occurs native as bismuth ochre.
BisMUTHio OXIDE, BigOs, or protoxide. — ^Prepared by passing
chlorine through a concentrated solution of potassic hydrate
which contains bismuthoub hydrate (BiHOa, or BijOa-HjO) in
suspension ; a blood-red substance then separates, which is a
mixture of hydrated bismuthic acid and bismuthic oxide.
This is treated with dilute nitric acid, which dissolves the
oxide, but in the cold does not attract the acid. Bismuthic
oxide is a bright-red powder. "Bismuthates are but little
known. Hydropotassic bismuthate, Bi2KH05 = BiK03 BiHOs,
is known." — ^Abppe.
Bismuth dioxtoe, Bi202. — This oxide is formed when a solu-
tion of a bismuth-salt is treated with stannous chloride. (A
corresponding sulphide is known.)
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THE CHEMISTS' MANUAL. 39
BisHiiTHATE OF BISMUTH, Bi204. — When bismuthic oxide is
heated to lOC C. it becomes converted into bismuthate of bis-
muth (Bi203.Bi205=2Bi204).
METALLIC BISMUTH.
80. Heated on ohabooal it fuses and deposits a deep-
yellow incrustation of bismuthous oxide (BijOs).
81. Hydbochlobic Acm does not act upon bismuth.
82. Nmao Acro dissolves it rapidly, converting it into
bismuthouB nitrate (BiSNOs).
2Bi + 8HN03=2BI(N03)3 + N^+4:H20.
If water is added to the solution, a white basic nitrate
(Bi203.N205 + H20=Bi2N208 + H20) is precipitated.
83. SiTLFHUBic Acn) dissolves it when concentrated and
aided by heat, forming bismuthous sulphate, Bi2(S04)3, and
Hberating sulphurous 02dde. Dilute sulphubio acid does not
dissolve bismuth.
2Bi + 6H2S04= Bi2(S04)3 + 2SO2 + 6H2O.
BISMUTH SALTS
The salts of bismuthous oxide are non-volatile, with the ex-
ception of a few (bismuthous chloride). The soluble salts, in
the neutral state, redden litmus-paper, and are decomposed
when treated with a large amount of water, insoluble basic
salts separating, the greater portion of the acid and a small
quantity of bismuth remaining in solution.
Soltition best fitted for the reactions :
Bismuthous NrrBATE, Bi (N03)3.
84. Htdbosulphukic acid produces a black precipitate of
bismuthous sulphide (Bi^Ss).
2Bi(N03)3 + 3H2S= BiaSa + 6H NO3.
Insoluble in alkalies, alkaline sulphides, and potassic cyanide.
Nitric acid decomposes and dissolves it when hot. If the
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40 THE CHEMISTS' MANUAL.
BolatioDB to be precipitated from are very acid from the pres-
ence of free hydrochloric or nitric acid, they must be first
diluted.
85. Ammonio suLPHroE produces the same precipitate as
hydrosulphuric add.
86. PoTAssio HYDEATE precipitates a white bibmuthofs
HYDBATE (BigOg.HgO).
2Bi(N03)3 + 6KH0=Bi203.H20-|-6KN03 + 2H20.
' » '
Insoluble in excess, but soluble in dilute acids.
87. Ammonio hydrate produces the same precipitate as
potassic hydrate.
2Bi(N03)3 + 3NH4H0=Bi203.H20 + 3NH4N03 + 3HN03.
88. SoDio CARBONATE producos a precipitate of basic bis-
MUTHOUS carbonate.
2Bi(N03)3 + 3Na2C03 = BiaOg^a + 6NaN03 + icOj.
The precipitate is white ; insoluble in excess and in potassic
cyanide.
89. Potassic dichbomate, or chromate, produces a yellow
precipitate ; when in excess it has the composition of SBijOs-
SCrgOg. If this be treated with a small quantity of acid, a
yellow salt remains undissolved, consisting of Bi203.2Cr203 ;
this may be precipitated when bismuth salt is in excess. —
(Lowe.) This last precipitate, according to Pearson, consists
of Bi203.Cr203. Compare § 89 with § 24.
90. Water, when added to solutions of bismuth, precipi-
tate WHIIE BASIC SALTS. (Bi203.N205 -|- H20=2BiN04+ H2O)
is precipitated from the nitrate; from the chloride a basic
chloride (Bi2Cle.2Bi203-|-6H20) is precipitated.
** This reaction is very characteristic, and distinguiBhes bieannth from all
other metals, except arUimcny. Bismnthons chloride exhibits this reaction
in the most striking manner, and it is best to convert the bismuth compound
into this salt by adding an excess of hydrochloric acid and evaporating to
dryness. The residue is dissolved in as little hydrochloric acid as poeeible,
and the solution poured into a large quantity of water.
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THE CHEMISTS' MANUAL. 41
"Bismutbons snlphate is not decomposed by bydrochloric acid. Wben a
solution is to be tested, therefore, which is known to contain salpburic
add, it is best to predpitate bismnthoos oxide by an excess of ammonia,
filter, wash, and dissolve in hydrochloric add, and then proceed as above."
— (TCTTLE AWD CHANDLEB.)
A FEW MISCELLANEOUS REACTIONS.
Ptkophosphoric acid, when added to a solution of bismuth-
OUB nitrate, produces a precipitate of bismuthous diphosphate
(2Bi203.3P205=Bi4Pe02,).
4Bi(N03)2 + 3H^P207= Bi^PeOa , + 12H NO3.
Phosphobio acid produces a precipitate of bismuthous phos-
phate (orthophosphate) when nitric acid is present.
Bi(N03)3 + H3P04+HN03=BiP04+4HN03.
OxAuo acid precipitates bismuthous oxalate ; a white pre-
cipitate (Bi3C«0,2.15H20).
3Bi(NO3)3 + 3C2H204+15Hg0=C6Bi30,2.15H20 + 6HN03.
Tabtabic acid added to hot moderately strong bismuthous
nitrate, produces a white precipitate of bismuthous tabtrate.
C,2Hi2-Bi20,8.6H20=Bi203.3C4H405.6H20.
METALLIC BISMUTH PRECIPITATED.
Metallic bismuth is precipitated from its solutions by metal-
lic iron, copper, lead, and tin, viz. :
2Bi(N03)3 + 3Pb= 2Bi + 3Pb2N03.
2Bi(N03)3+3Cu=2Bi + 3Cu2N03.
91. Blowpipe. — When solid compounds of bismuth are
fused with sodic carbonate in the reducing flame of the blow-
pipe, BBrrxLE metallic globules of metal are produced, as
also an incrustation of BisBiUTHous oxide, which is yellow.
Chakactebistio Ebactionb, 89, 90, 91.
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43
THE CHEMISTS' MANUAL.
SCHEME FOR THE SEPARATION AND DETECTION OF THE
MEMBERS OF THE FIRST DIVISION OF GROUP II.
The solution to be examined is supposed to contain a salt
of mercuric oxide, copper, cadmium, lead, and bismuth.
Add hydrochloric acid — ^no precipitate. Add to the solu-
tion hydrosulphuric acid (HgS) ; there is produced a precipitate
of bismuthous sulphide (BisSs), plumbic sulphide, (PbS), cad-
mic sulphide (CdS), mercuric sulphide (HgS), and cupric sul-
phide (CuS).
BijSa + PbS+HgS+CciS+CuS.
* *
Wash completely to expel the chlorine in the mixture; add
moderately strong nitric acid (free from hydrochloric), and
warm, then filter.
RssrouB.
Is composed of
HgS + S. "Black."
Dissolve in a little
aqoa-regia. Add
stannoiiB chloride ;
a precipitate is
^ercuric chloride,
^Hg, CI,. Heat. Me-
tallic mercury is
formed. See §48.
Solution.
The solution contains the Pb. Cu, Bl, and Cd. Add
dilate sniphnric acid; concentrate solution to expel
HNO, ; add H,0 and filter.
Bstidue,
PbS04.
See §21.
8oliaion
Contains the Cu, Bl, and Cd. Add NH4HO
and filter.
FiUraU Blue
Contains the Cu and Cd. Divide^
gd Part.
Add KCN to de-
stroy bine color.
thenH.S. Pro-
cipiute CdS.
See §70.
PredpUate.
Bi,0,.H,0.
Wash, dis-
solveinHCl.
Te8tas§9a
lit Part,
Acidulate with
acetic acid. Add
K4Cfy, a preci-
pitate Cu,Cfy.
See §60.
SECOND DIVISION OF GROUP il.
Metals, the sulphides of which are soluble in ahmonic
SULPflroE.
Absenic, antimony, tin, gold, platinum.
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THE CHEMISTS' MANUAL, 43
ARSENIC.
Symbol, Aa. (Greek, arienicon, potent). ^Atomic weight, 76.— Equivalence,
III and V. — Density, 150. — ^Molecular weight, 300. — ^Molecular volume, 2. —
1 litre of arsenic vapor weighs 18.44 grams (150 criths). — Specific gravity,
5.7 to 6.059 (Miller).— Atomic volume, 12.96.— Specific heat, 0.0814.— Elec-
tric conductivity at 82'' F., 4.76.— Volatilizes at SSO** F.— Order of brittleness
commencing with antimony, Becond.«<!V>lor, dark-gray ; bright only when
freshly fractured.
ARSENIC OXIDES.
Arsenic forms two well-defined oxides, viz.: Arsenious
oxide AS2O3, and arsenic oxide AS2O5. The black film which
forms on the sur&ce of the metal is supposed to be a sub-
oxide, but it is more probably a mixture of metallic arsenic
with arsenious oxide.
Absenious oxmE, AS2O3, in the hydrated state absenious
ACID. Occurs native in the mineral arsenite or arsenolite.
Formed when arsenic is volatilized in contact with free
oxygen, as when the metal is heated in a glass tube through
which a current of air is passing.
3As-t-03 + A^=As203
It is a white solid. Sp. Gr. 3.7385 (Guibourt). Volatilizes at
about 218® C. Insoluble in ether; nearly so in alcohol.
Absenio OXIDE, AS2O5, in the hydrated state arsenic acid.
This compound is formed by oxidizing arsenious oxide or
arsenious acid with nitric acid, aqua-regia, hypochlorous acid,
or other oxidizing agents. Dissolve AS2O3 in hot HCl and
oxidize by adding HNO3, ^^ latter being added as long as red
vapors are produced, the whole then cautiously evaporated to
complete dryness, and the residue heated to low redness. Ar-
senic oxide is produced as a white anhydrous mass which has
no action on litmus-paper. Strongly-heated arsenious oxide
and free oxygen are produced.
As205-hA<J=As203-f-20.
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44 THE CHEMISTS' MANUAL.
METALLIC ARSEIQIC.
93. Heated on chaeooal, it does not fiise, but gives off
fiunes of arsenious oxide (AS2O3), a portion of which is deposited
as a white incrustation. A peculiar alliaceous odor is emitted
at the same time.
93. Heated m a tube which has one end closed, the
arsenic sublimes, forming a blacky shining metallic bing on
the glass.
94. Hydrochloric acid does not attack metallic arsenic.
95. Sulphuric acto, dilute, does not attack metallic ar-
senic, but boiling concentrated acid oxidizes it to arsenious
oxide, evolving sulphurous oxide.
2As + 2H2S04=As203+2S02 + H20.
96. Nrnuc acid, when dilute, converts arsenic by the aid
of heat into arsenious acid«
2As+2HN03=As203 + N^-|-H20.
Concentrated nitric acid converts the metal partially into
arsenic oxide (AsgOg).
6As+10HNO3=3As2O5 + 6N2O2 + 5H2O.
Arsenious acid (2H3As03=3H20.As203).
Solution best fitted for the reactions:
Arsenious Acid, H3ASO3.
97. Hydrosulphuric acid produces no' precipitate with
arsenious acid, but imparts to the solution a yellow color.
If hydrochloric acid be added, a precipitate of arsenious sul-
phide (AS2S3) is produced, which is soluble in ammonic sul-
phide, from which it may be reprecipitated by acids.
2H3As03 + 3H2S-t-HCl=As2S3-|-6H20 + HCl.
Ammonic carbonate dissolves arsenious s'ulphide, especially
when heated, from which it can be reprecipitated by means
of acids. It is readily dissolved by hot nitric acid ; also by
hydrochloric acid, with potassic chlorate.
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THE CHEMISTS' MANUAL. 45
98. Ammonio sulphide produceB no precipitate; simply
imparts to the solution a yellow color. If hydrochloric acid
be added, a yellow precipitate of aesenious sulphide is pro-
duced, soluble in excess.
SHaAsOa+SNH^HS+SHClrsAsaSa + SNH^Cl+eHaO.
99. Abgentic ntieate produces no precipitate in arsenious
acid, but if ammonic hydrate be cautiously added, a yellow
precipitate of abgentic arsenite is produced, which dissolves
easily in excess of ammonic hydrate and in nitric acid.
2H3As03+4AgN03+2NH4H0=Ag4^205 + 2NH4N03+2HN03
+ 3H2O.
" In making this test, add the argentic nitrate, and then (incline the test-
tnbe) let one or two drops of ammonia run down so as to form a layer on the
surface of the liquid to he tested. AVliere the two liquids are in contact a
bright jeUow ring of argentic ars^nlte (2Ag,0. AsgO, =Ag4As,05) will be seen/'
— {ToTTLE Aim Chandler.)
100. CuPBio SULPHATE produccs no precipitate, but if
nmmonic hydrate be added, as in § 94, a yellowish-green
CTjPEio ARSENTiE (Scheclc's grccu ; 2Cu0.As203=Cu2As205) is
precipitated.
2H3As03 + 2CuS04+2NH4H0=Cu2As205 + (NH4)2S04+H2S04
+ 3H2O.
101. Eeinsoh's Test. — If a solution of arsenious acid,
mixed with hydrochloric acid, be heated with a clean strip of
METALLIC copper, an iron-gray film or incrustation is de-
posited on the copper even in highly diluted solutions, which
is METALLIC ARSENIC ; this film may be detached in black scales
by long boiling. The thickness of the film depends on the
concentration of the solution and the amount of arsenious
acid present. The film may be separated from the copper by
boiling the strips in ammonic hydrate, when minute spangles
fleparat^. If the film separated by boiling water be dried,
and introduced into a tube closed at one end, on the applica-
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46 THE CHEMISTS' MANUAL.
tion of heat the arsenic is caused to sublime as a shining ring^
if much is present, or as a white crystalline ring of arsenioug
oxide, if the quantity is small.
103, Metallic Zinc — ^If arsenious acid is introduced into
a flask in which hydrogen gas is being evolved from pure zinc
and dilute sulphuric acid, the zinc oxidizes not only at the ex-
pense of the oxygen of the water, but also at the expense of
that of the arsenious acid, and the arsenic separates accordingly
in the metallic state ; but a portion of the inetal combines in
the moment of its separation with the liberated hydrogen of
the water, forming hydrogen arsenide or arsine (HgAs).
This reaction affords a means for the detection of even the
most minute quantities of arsenic.
103. Marsh's Test. — ^This experiment is best conducted
in the apparatus here figured. Into the flask (a) containing
granulated (pure) zinc and distilled water, dilute sulphuric
acid is introduced. Hydrogen is liberated, which, passing
through the calcic chloride tube (J), where it is dried, escapes
at the extremity of the apparatus. As soon as the air is com-
pletely expelled the hydrogen may be ignited.
If the solution containing the arsenic be now poured into
the flask, hydrogen arsenide will be evolved, and the flame
changed to a livid Mice.
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THE CHEMISTS' MANUAL. * ' 47
104* 1. If a piece of cold porcelain (the cover of a porcelain
cradble) be held in the flame, a black deposit of metallic
arBenic is produced. The stain disafpeabs, when moistened
with calcic hypochlorite (Ca2ClO).
105. 2. If one or two drops of strong nitric acid be poured
on an arsenic stain, and then gently evaporated, it is converted
into arsenic oxide. By adding a drop of argentic nitrate, and
cautiously neutralizing with ammonic hydrate, a brick-red
argentic arseniate (3Ag20.As205=Ag5As208=2Ag3As04) is pro-
duced. An excess of ammonic hydrate dissolves the red ar-
seniate.
106. 3. If tube Cj d, (which should be of hard glass and
free from lead) be strongly heated between the points e and d,
the hydrogen arsenide is decomposed, metallic arsenic being
deposited in the form of a shiiono bijlck mibbob on the cold
part of the tube.
107. 4. If a short tube be adjusted, by means of a caout-
chouc connector, to the extremity of the tube c, dy and the gas
passed into a solution of abgentic kitrate, a black precipi-
tate of metallic silver is produced, while the arsenic passes
into solution. On neutralizing the filtered liquid (see § 99)
with ammonia, the tellow argentic arsentie is precipitated.
12AgN03 + 2AsH3+3H20=12Ag+As203-fl2HN03.
r 108. Fleetman's Test. — If a solution containing arsenic
be mixed with a large excess of a concentrate solution of
potassic hydrate, and boiled with granulated zmc, hydrogen
arsenide is evolved. A piece of filter-paper moistened with a
solution of argentic nitrate, assumes a purplish-black color
if exposed to this gas. This experiment may be conducted in
a small flask, or large test-tube, supplied with a cork, through
which passes a small tube, drawn to a point.
109. Blowpipe. — Dry compounds of arsenic, when heated
with sodic carbonate on charcoal in the inner flame of the
blowpipe, emit a peculiar garlic odor. This odor has its
origin in the reduction and re-oxidation of the arsenic ; very
minute quantities may be detected in that way.
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48 THE CHEMISTS' MANUAL.
110. Heated witli sodic carbonate and a little potassic
cyanide, in a dry tnbe closed at one end, a black mirror of
METALLIC AssENio sublimes.
Charactebistio Eeactionb, 93, 93, lOO, 101, 104,
105, 106, 107, 109, 110.
Aesenio Acid, H3ASO4.
Solution best fitted for the reactions :
Arsenic Acid H3As04.(3H20.As205=2H3As04).
111. Hydrosulphuric acid fails to produce a precipitate in
arsenic acid, but if the acid be acidified with hydrochloric acid
and the solution warmed and allowed to stand, a yellow pre-
cipitate of ARSENIC sulphide, AsgSg, is produced, which is sol-
uble in ammonic sulphide. It is re-precipitated from this
solution by acids.
2H3As04+5H2SH-HCl=As2S5-h8H20-hHCl.
112. " In order to separate arsenic oxide completely by
hydrosulphuric acid, it is necessary first to reduce it to arseni-
ous oxide by adding a little sodic sulphite to the solution.
The excess of sulphurous acid is then to be removed by boiling
the liquid." — (Tuttle and Chandler.)
113. Ammonio sulphide produces arsenic sulphide, which
is held in solution as ammonic-arsenic sulphide,
2H3As04+6NH4HS=NH4HS.As2S5 + 5NH4H0H-3H20.
If to this solution an acid be added, the double sulphide is
decomposed and arsenic sulphide is precipitated ; this precipi-
tate separates more rapidly than in the case of hydrosulphuric
acid (§ 111).
2H3As04 + 6NH4HS+5HCl=As2S5-h5NH4Cl + 8H20.
114. Argentic nitrate produces, under the circumstances
stated in § 105, a brick-red precipitate of argentic arseniate,
easily soluble in nitric acid and in ammonic hydrate. When
free nitric acid is present, therefore, it is necessary to neutralize
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THE CHEMISTS' MANUAL. 49
very carefdlly with ammonic hydrate. As argentic arseniate
is slightly soluble in ammonio nitrate the precipitate is not
always produced.
2H3As04+6AgN03 + 3NH4H0=2Ag3As04+NH4N03 +
SHNOa + SHaOT"^
115. Hydrochloric acids or chlorides, if present, should be
removed by precipitation with argentic nitrate, a little nitric
acid being added to retain the arseniate in solution. If am-
nionic hydrate is now added to the filtered liquid, the brick-
red argentic arsenite (3Ag20.As205=2Ag3As04) is precipitated.
116. CcPRic SULPHATE, uudcr the same circumstances as in
§ 95, produces a greenish-blue precipitate of cupric arseniate
(2Cu0.H20.As205=Cu2H2As208=2CuHAs04), soluble in nitric
acid and in ammonic hydrate.
117. Metallic zinc behaves the same as with arsenious
acid. (See §97, 98.)
118. Metallic copper (Reinsch's test) acts as with arseni-
ous acid, except that much more hydrochloric acid is to be
added in order to insure reduction. (See § 96.)
119. AMMOmo-MAGNESIC ARSENIATE [2MgO.(NH4)20,As205 +
12H20 = Mg2(NH4)2As208 = 2Mg(NH4)As.04) is precipitated
when arsenic acid is added to a clear mixture of (magnesic
Sulphate, ammonic chloride, and a sufficient quantity of am-
monia). It separates from concentrated solutions immediately,
from dilute solutions after some time.
2H3As04+2MgS04 + NH4Cl + 6NH4H0=2Mg(NH4)As04
+ NH4Cl+2(NH4)2S04+6H2a
The above magnesia mixture may be prepared by dissolv-
ing in water 24.6 grams of crystallized magnesic sulphate and
33 grams of ammonic chloride, adding some ammonic hydrate
and diluting to the volume of a litre.
120. Blowpipe.— (See Arsenious Acid, § 109, 110.)
4
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50 THE CHEMISTS' MANUAL.
ANTIMONY.
Symbol, Sb. (Arabic, aUthruidem).— Atomic weight, 122. — Equivalence^
ni and v.— Density, 244 (?)— Molecular weight, 488 (?)— Molecular volume, 2,
— 1 litre of antimony vapor weighs, 21.86 grams (244 criths) (?) — Sp. Gr. 8.715.
—Melts at 450" C— Atomic volume, 18.16.— Specific heat, 0.0508.— Fusing
point, IISO** F.— Electric conductivity at 32° F., 4.65.— Order of brittleneas,
first. — Bluish-white color.
ANTIMONY 0XIDES.
Antimony unites with oxygen to fbrm thbee definite com-
pounds, SbaOg ; Sb204 : SbjOj.
Antimonious oxide, SbjOa, occurs as a natural mineral (Val-
entinite, white antimony, antimony-bloom, weisspiessglanzez).
It may be prepared by burning the metal in the air.
2Sb-|-30 = Sb203.
Easiest mode of obtaining it is to heat antimonious sulphide
with strong hydrochloric acid, as long as hydrosulphuric acid
goes oflF, and pour the resulting solution of antimonious chlo-
ride into a boiling solution of sodic carbonate. A crystalline
powder is then deposited consisting (according to Graham) of
antimonious oxide.
SbgSa + 6HCl=:2SbCl3 + SH^.
2SbCl3 + 2Na2C03 = SbjOg -f 6NaCl -f 3C07.
HegnauUj however, states ("Cours de Chimie," iii., 239)
that the oxide obtained is a hydrate containing SbgOg, HgO, or
SbHOj (meta-antimonious acid).
Antimonious oxide dissolves sparingly in water; more
freely in strong hydrochloric acid. Dissolves when boiled
with AQUEOds TARTARIC ACID, and very easily in hydropotassic
tartrate (cream of tartar), forming antimonio-potassic-tartrate
C4H4KSb07 (tartar emetic). It is quite insoluble in nitric
acid of ordinary strength, but dissolves in cold filming nitric
acid, forming a solution which deposits pearly scales of a
nitrate (N205.2Sb203 = Sb4N20,,). It dissolves in fuming
sulphuric acid, the solution depositing shining scales of a
sulphate containing 3S03.Sb203 = Sb2S30,2.
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THE CHEMISTS* MANUAL. 61
AimMONio oxn)E, SbgOg ; in the hydrated state antimonic
acid. This compound is obtained as a hydrate by treating
antimony with nitric acid, or with aqiiBrregia containing an
excess of nitric acid ; by precipitating a solution of potassic
antiinonate with an acid ; by decomposing antimonic chloride
with water. The hydrate oxide obtained by either of these
methods gives oflF its water at a heat below redness, and yields
antimonic oxide as a yellowish powder.
The hydrated oxides obtained by the three methods given
above are by no means identical. That obtained by the first
and second methods is monobasic, and, according to BerzeliuSy
contains SbjOs-HjO, or SbHOa; according to Fremy^ SbgOs-
SHjO, or SbHgOs, when dried at mean temperature; but the
acid obtained by the action of water on antimonic chloride is
dibasic, and contains, according to Fremy^ Sb205.4H20. The
acids are antimonic HSbOa ; met-antimonic, pyro-antimonic, or
di-antimonic, H^SbgOy ; ortho-antimonic, H3Sb04.
Aa'timonoso - ANTIMONIC OXIDE, Sb204. — Somo cousidcr
this oxide as (Sb203 + Sb205=2Sb204) a compound of the
antimonious and antimonic oxides. This oxide forms salts
with the alkalies (often called antimonites), which may be ob-
tained solid. Potassic antiinonite, K20.Sb204, by mixing the
solution of this salt with hydrochloric acid, a precipitate of
hydrated antimonoso-antimonic oxide, H20.Sb204,is produced.
The salt K20.Sb204 may be regarded as (K20.Sb203)+(K2a
Sb205)or KSbOa-KSbOa.
METALLIC ANTIMONY.
121. Heated on chakcoal it bums brilliantly, emitting
copious white inodorous vapors, and if left to cool before it is
completely burnt away, becomes covered with a white net-
work of the crystallized antimonious oxide. The white fumes
form an incrustation on the charcoal.
12S. Hydrochlorio acid does not attack antimony in the
solid (compact) state even on boiling; but if the antimony is in
a fine powder it is dissolved by the boiling acid, and hydrogen
gas is given off.
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52 THE CHEMISTS' MANUAL.
133. NrrBio acid rapidly oxidizes it, forming a white
powder, which differs in composition according as the acid
used is dilute or concentrated.
Moderately dilute acid, the product consists of antimoni-
ous oxide mixed with antimonic oxide (Sb203.Sb205).
12Sb + 16HN03=3(Sb203.Sb205)+8N202+8H20.
Dilute acid converts it ahnost entirely into antimonious
OXIDE.
Concentrated acid converts it almost entirely into anti-
monic oxide. The acid oxidizes it, but does not dissolve it.
134. NrrROHYDRocHLORTO ACID dissolves the metal when
hot, forming antimonious chloride (SbCl3) when the acid is not
very concentrated, and antimonic chloride (SbCls) when the
acid is very concentrated.
2Sb+2(3HCl + HN03)=2SbCl3+4H20 + N^2'
135. SuLPHURio ACID, whcu dilute, does not attack anti-
mony ; but if heated concentrated acid be employed, the metal
is converted into antimonious sulphate (Sb203.S03=Sb2S0g)
with evolution of sulphurous oxide.
2Sb+4H2S04 (conc.)-h A<5=Sb2S05+3S02+4:H20.
SALT OF ANTIMONIOUS OXIDE.
Most of the salts of this oxide are decomposed upon ignition.
The soluble neutral salts redden litmus-paper. When heated
with a large amount of water, they are decomposed into basic
salts and acid solutions. Thus: water precipitates from a
hydrochloric acid solution of antimonious chloride (SbClg),
antimonious oxy chloride (2 SbCl3. 5 SbgOs) (powder of algaroth).
This precipitate is soluble in tartaric acid, therefore it is not
precipitated in the presence of this acid.
Solution heat fitted for the reactions:
Antimonious Chloride, SbCl3.
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THE CHEMISTS' MANUAL. 68
126. HTDBOsiiLPHrsic Acm produces an orange-red precip-
itate of ANTQCoNious SULPHIDE (SbsSs) when added to an acid
solution of antimonious salts.
2SbCl3+3H2S=Sb2S3+6HCL
From alkaline and neutral solutions the ANTEBfONioTTS-strLr
PHTOE is only partially precipitated.
Antimonious sulphide dissolves readily in potassic hydrate
and ammonic sulphide, sparingly soluble in amnionic hydrate.
Boiling hydrochloric acid (concentrated) dissolves it with
evolution of hydrosnlphuric acid gas. Boiling nitric acid dis-
solves a portion, and converts the rest into a white insoluble
powder.
127. Ammonic sulphide produces an orange-red precipitate
of antimonious sulphide.
2SbCl3+3NH4HS=Sb2S3-f3HCl+3NH4CL
^ ^ ^
This precipitate is soluble in excess, especially when the
precipitant is rich in sulphur.
138. WATEjt, when added in large quantities, produces a
white precipitate of antimonious oxychloride (2SbCl3.5Sb203)
(according to-Duflos and Bucholz), which is soluble in tartaric
acid, whereby it is distinguished from bismuth (§ 85). The
formation of this precipitate is prevented if tartaric acid or
much fi-ee hydrochloric acid is added before the addition of
the water.
129. Potassic hydrate produces a white precipitate of
antimonious acid (HSbOg or Sb203.H20), which is soluble in
excess. This solution precipitates from argentic nitrate, black,
metallic silver — the antimonious oxide being changed into anti-
monic oxide.
This precipitate is readily distinguished from that which is
produced by potassic hydrate alone, in silver solutions, by its
insolubility in ammonic hydrate. (See §9.) The presence of
tartaric acid prevents the precipitation.
130. Ammonic hydeate produces the same precipitate as
potassic hyarate.
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54 THE CHEMISTS' MANUAL.
131* Ammonio oabbokate produces a precipitate of white
HYDRATKD ANTIMONIOU8 OXIDE or ANTIMONIOU8 ACID, HSb02.
2SbCl3+3(NH4)2C03 + H20=2HSb02 + 6NH4Cl+3C02.
The. precipitate is partially soluble in excess. The presence
of tartaric acid prevents the precipitation.
133. SoDio OABBONATB produccs the same precipitate as
ammonic carbonate, viz. : HSbOg. — (Regnault.)
2SbCl3+3Na2C03 + H20=2SbH02 + 6NaCl+3C02.
133. Metallic zmc precipitates antimony from its solution
in the form of a black powder. If free acid be present, anti-
MONious HYDRIDE, SbH3, (Stibine) is evolved. This experiment
is conducted precisely as in the case of arsenic (§ 102).
134. 1. K a piece of cold porcelain is held in the flame, a
BLACK DEPOSIT of metallic antimony is produced, which does
not dissolve when treated with calcic hypochlorite (Ca2C0).
135. K one or two drops of nitric acid be poured on the
antimony stain, and gently evaporated, it is converted into
white ANTiMONic OXIDE. Aroentic NITRATE producos no
change. (See § 100.)
136. If the tube c, d^ be strongly heated, a metallic ring is
deposited, as in the case of arsenic (§ 101).'
137. K ANTiMONioirs hydrtoe be passed into a solution of
ARGEinic NTiRATB, A BLACK PREdPTTATE of argentic antimonlde
is produced (SbAg3).
3AgN03+SbH3=SbAg3 + 3HN03.
On neutralizing the filtered liquid by ammonic hydrate, no
precipitate is produced. (Comp. Arsenic, § 107.)
To detect antimony in argentic antimonide it should be
washed, boiled with nitric acid (which dissolves only the anti-
mony), and filtered. Hydrosulphuric acid should then be
added to the filtrate, and on boiling, orange-red antimonious
sulphide separates.
138. Metallic zinc boiled with a solution of antimony, to
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THE CHEMISTS* MANUAL. 55
which a veiy large excess of potassio hydrate has been
added, liberates pure hydrogen, which does not discolor paper
moistened with a sohition of argentic nitrate. (See § 103.)
139. Auric chloride, when added to a solution of antimoni-
ous chloride or other antimonious salts, forms a yellow pre-
cipitate of metallic gold, antimonic oxide at the same time
being precipitated as a white powder, unless the solution con-
tains a large excess of hydrochloric acid.
4AuCl3 + SSbaOa + 6H2O =4Au + 12HC1 + SSbaOg.
The reduction is slow at ordinary temperatures, but is acceler-
ated by heating. In a solution of antimonious acid in potassic
hydrate, auric chloride produces a black precipitate which
forms a very delicate test for antimonious oxide.
140. Metallic copper precipitates antimony from its solu-
tions, in the form of a bright metallic film, which may be
dissolved off by a solution of potassic permanganate, yielding a
solution which will give the characteristic red precipitate with
hydrosulphuric acid. — (Odlino.)
141. Blowpipe. — Solid compounds of antimony, mixed
with sodic carbonate (and potassic cyanide), and fused on
charcoal in the inner flame, yield BRnrLE globules of metal-
lic antimony, forming at the same time a whtie incrustation
of antimonious oxide.
Characteristic Beactions, 123, 128, 129, 134, 135,
136, 137.
ANTIMONIC OXIDE.
Antimonic oxide (SbgOg) is pale-yellow, its hydrates or acids
(HjSbOs ortho-antimonic acid; HSbOa dimeta-antimonic acid;
H4Sb207 diantimonic acid) are white. The oxide and acids
are slightly soluble in water, and almost insoluble in nitric
acid, but dissolves pretty readily in hot concentrated hydro-
chloric acid, forming antimonic chloride, which becomes turbid
on addition of water.
Sohition best fitted for the reactions :
Potassic Antimoniate, KjSbaOg.
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66 THE CHEMISTS' MANUAL.
143. NiTRio ACID produces a white precipitate of htdbated
ANTIMONIO ACID (Sb205.4H20).
143. Htdboohlobio Acm precipitates the same as with
nitric acid soluble in excess.
144* Hydbosulphubic acid, in a neutral solution, produces
no precipitate. If an excess of hydrochloric acid is present,
an orange-red precipitate of antimonic sulphide (SbgSg) is pro-
duced.
K2Sb205 + 5H2S-f2HCl = Sb2S5 + 2KCl + 6H20.
Antimonic sulphide is soluble in amnionic sulphide, from
which it may be precipitated by acids.
146. PoTAssic hydrate in acid solutions precipitates a
white hydrate of antimonic acid (Sb205.4H20), soluble in
excess.
146. Argentic nitrate produces in solutions of anti-
monic OXIDE to which an excess of potassic hydrate has been
added, a black precipitate of argentic oxide, which is readily
soluble in ammonic hydrate. This reaction distinguishes
antimonic oxide from the salts of antimonious oxide. (See
§129.)
147. Antimonic oxide, when boiled with hydrochloric acid
and potassic iodide, liberates iodine, which dissolves in the
hydriodic acid present, giving a brown color to the solution.
148. Potassic metantimoniate (K2H2Sb207.6H20) is a sol-
nble salt, whilst sodic metantimoniate (Na2H2Sb207.6H20) is
insoluble. This diflFerence in the two salts make the potassic
metantimoniate valuable as a test for sodic salts.
149. Metallic zmc acts as with antimonious salts (§ 137).
160, Blowpipe. — See Antimonious Salts. (See § 141.)
TIN.
Symbol, Sn. — ^Atomic weight, 118.— Equivalence, II and IV.— Molecular
weight, 236.-- Brilliant white metal.— Specific gravity, 7.292.— Melts at
230*' C— Atomic volume, 16.20.— Specific heat, 0.0562.— Fusing point,
442" F. —Electric conductivity at 32'' F., 12.36.— Order of raaUeabmty com-
mencing with gold, fourth ; of ductility, seventh ; heat^jonducting power,
seventh. — ^Tenacity, 63 (iron as 1000).
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THE CHEMISTS' MANUAL. 57
TIN OXIDES.
Tin unites with ozygen to fonn three oxides, SnO ; SnsOa ;
SnOj.
Stannous ohdb, SnO, or protoxide, may be prepared by
heating stannous oxakte out of contact with the air (Liehig).
By precipitating stannous chloride with sodic carbonate, and
heating the washed and dried precipitate of stannons hydrate
in an atmosphere of hydrogen or carbonic oxide to a tempera-
ture not exceeding 80° C, the anhydrous oxide is thus obtained
as a brown or black powder (Berzelius). According to Otto,
the hydrate sometimes changes to the black oxide on the filter,
or the sides of the precipitating vessel, whence it is touched
with a glass rod. Stannous oxide is a black powder of specific
gravity 6.666 (Berzelius). Permanent in the air at ordinary
temperatures, but easily oxidized to stannic oxide when heated.
Stannous hydrate, Sn2H203=2SnO.H20.
Ten sESQUioxmE, SngOs. — This oxide was obtained by Fuchs
in combination with water, by diffusing recently-precipitated
ferric oxide in a solution of stannous chloride not containing an
excess of acid, and afterward boiling the mixture. Sesquioxide
of tin is then precipitated.
2SnCl2 -f Fe203=Sn203 + 2FeCl2.
Thus obtained is a slimy gray matter ; ammonic hydrate dis-
solves it readily (not so stannous oxide). This oxide produces
a purple precipitate with auric chloride (not so stannic oxide).
Stannic oxroE, Sn02, or dioxide, occurs native in tinstone or
cassiterite. May be prepared by burning metallic tin in con-
tact with the air. May also be prepared by igniting either of
the other oxides or their hydrates in contact with the air. It
is a white or yellowish powder, assuming when heated a darker
color. Specific gravity, 6.6 to 6.9.
Stannic acid, Sn02.H20=H2Sn03.
Metastannic acid, Sn50,o.5H20=H,QSn50,5.
The first acid is capable of exchanging the whole of its
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58 THE CHEMISTS' MANUAL.
hydrogen for a metal, and forming stannates, whereas the
latter exchangee only one-fifth of its hydrogen metals forniing
metastannates.
METALLIC TIN.
151, Heated on chabcoal, in the outer flame of the blow-
pipe, it is converted into stannic oxide (Sn02) ; in the inner
flame it remains unchanged.
Sn + 0=Sn02.
153. Htbeoohlorio acid, when dilute and cold, dissolves
tin but slowly; when hot and concentrated it is easily dis-
solved, forming staics^ous chloride, and liberating at the
same time hydrogen.
Sn-f2HCl=SnCl2 + 2H.
The presence of much stannous chloride in the solution re-
tards the action of the hydrochloric acid to some extent.
153. Nitric acid when concentrated (Sp. Gr. 1.5) does not
act on tin, the metal even preserving its metallic brilliancy ;
but if the acid be dilated it attacks the metal very violently,
converting it, when heated, entirely into metastannic acid=:
Sn5H,oO,5 = Sn50,o.5H20 + 5Sn02.5H20.
According to Weher^ nitric acid of Sp. Gr. 1.2 converts tin
at ordinary temperatures into stannous nitrate, stannic acid,
and metastannic acid, which is colored yellow by admixed
stannous metastannate.
With nitric aeid Sp. Gr. 1.2 it converts tin into (if the liquid
is well cooled) metastannic acid [stannic ?] and stannic nitrate ;
by dihition and heating the stannic acid is converted into in-
soluble metastannic acid, which indeed is always produced
under influence of heat. Wlien this product is heated to red-
ness it is converted into stannic oxide.
154. Sulphuric acid, when dilute, dissolves tin slowly
(with the aid of heat), and converts it into stannous sulphate,
SnS04, and liberates hydrogen at the same time.
Sn + H2S04 = SnS04 + 2H.
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THE CHEMISTS' MANUAL. 59
When the acid is concentrated and hot (with plenty of tin)
it is dissolved, and converted into stannic sulphate, and
liberating sulfhubous oxide at the same time.
Sn+4H2S04=Sn(S04)2 + iS02+4H-j0.
STANNOUS SALTS.
The stannous salts are colorless and are readily decomposed
hy heat. The soluble salts in the neutral state redden litmus-
paper. The stannous salts, when exposed to the air, rapidly
absorb oxygen, and are converted into salts of stannic oxide.
The crystallized stannous chloride only dissolves to a clear
liquid in water acidulated with hydrochloric acid.
Solution best fitted for the reactions :
Stannous Chloride, SnClg.
155. Htdbosulphumo acid produces, when added to stan-
nous chloride, a brown precipitate of stannous sulphide (SnS).
SnCl2 + H2S=SnS+2HCL
The precipitate is dissolved by ammonic sulphide (in excess),
which first converts it into stannic sulphide, from which solu-
tion it may be precipitat^ed by acids. Nitric acid converts it
into insoluble metastannic acid. In alkaline solution, the tin
18 only partially precipitated by hydrosulphuric acid.
156« Ammonic sulphide produces the same precipitate as
liydroBulphuric acid, soluble in excess if the ammonic sulphide
<x>Dtains an excess of sulphur (known by its bright-yellow
color).
167. PoTAssio hydkate precipitates stannous hydrate
(2SnO.H20) as a white compound which is soluble in excess.
2SnCl2-f-4KHO=2SnO.H20+4KCl+H20.
168. Ammonio hydrate produces the same precipitate as
potassic hydrate (2SnO.H20 + Sn2H203).
2SnCl2+2NH4HO-fH20=2SnO.H20 + 2HN4Cl-f-2HCl.
The precipitate is insoluble in excess of ammonic hydrate.
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60 THE CHEMISTS' MANUAL.
159* SoDiG OABBONATE produces the same precipitate aa
ammonic hydrate.
2SnCl2 + 2Na2C03 + H20=2SnO.H20+4NaCl+C02.
S . y /
160. Merourio CHLOBmE produces a white precipitate of
mercurous chloride.
2HgCl2 + SnCl2= Hg2Cl2 + onCl4.
When much stannous cHLOBmE is present, the precipitate is
reduced to metal.
Hg2Cl2 + SnCl2= Hg2 + SnCV
This is a very delicate reaction for salts of stannous oxide.
(See §42.)
161. POTASSIO FERRICYANIDE and FERRIC CHLORIDE, whcU
added to a solution of stannous chloride in hydrochloric acid,
produces a precipitate of prussian blue, owing to the reduction
of the ferricyanide to ferrocyanide.
. • K^(FeCeN^)2 + Fe2Clfi = Fe2(FeCeN,)2 + 6KCL
\ KgCfya + FeaClg + FeaCfya + eKCl.
2Fe2(FeCg Ng)2 + 2SnCl2 + 4HCl=Fe4(FeC6Nc)3 + 2SnCl4 + H^
(FeC.N,): ' '
2Fe2Cfy2 + 2SnCl2 + 4HC1 = Fe^Cfya + 2SnCU + H^Cfy.
The reaction is extremely delicate, but it can be held to be
decisive only in cases where no other reducing agent is present.
163. Metallic zinc produces a gray precipitate of tin (Sn),
soluble in hydrochloric acid after the removal of the zinc.
163. Blowpipe. — If solid compounds of tin be fused on •
charcoal with sodic carbonate (and potassic cyanide) in the
reducing or inner flame, metallic globules of tin, which are
white and malleable, are produced.
Characteristic Reactions, 163, 160, 163.
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THE CHEMISTS* MAMJAL. 61
STANNIC SALTS.
The salts of stannic oxide are colorless; they are decom*
posed at r^ heat. Anhydrous stannic chloride is a Tolatile
liquid, strongly filming in the air. The soluble salts of stan-
nic oxide in the neutral state redden litmus-paper.
Solution best JUted far the reactions :
Stannic CHLomoE, SnCV
364. Hydbosulphubic acid produces in neutral or acid
solutions a ykllow PREciprrATE of stannic sulphide (SnS2).
SnCl4+2H2S=SnS2-|-4HCL
The precipitate dissolves readily in potassic hydrate, am-
monic sulphide, concentrated hydrochloric acid, and aqua-
regia. Soluble with difficulty in ammonic hydrate, and
insoluble in ammonic carbonate and dilute acids. If the pre-
cipitate contains arsenic sulphide, ammonic carbonate will
dissolve it. Boiling nitric acid converts it into insoluble
stannic oxide, but is dissolved by hot hydrochloric acid to
which a little nitric acid has been added.
165. Ammonic sulphide produces the same precipitate as
hydrosulphuric acid, soluble in excess, repredpitated by acids
unaltered.
SnCl4+2NH4HS=SnS2 + 2NH4Cl+2HCL
166. Potassio hydrate and sodio hydrate produce a
white precipitate of stannic acid (Sn02.H20=SnH203) if acid
be present, soluble in excess of potassic or sodic hydrate.
SnCl4+4KH0 + HCl=Sn02.H20+4KCl+H20 + HCl.
SnCU + 4NaH0 + HCl^SnOg.HgO + 4KC1 + HCl 4- HjO.
167. Ammonic and some carbonate produce a white pre-
cipitate of an ACID 8TANNATE.
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62 THE CHEMISTS' MANUAL.
168. Babio or oalcio cakbonate produces a precipitate of
STANNIC ACID (SnHjOa), soluble in excess.
SnCU + 2BaC03 + H20== SnHaOg + 2BaCl2 + CO^.
SnCl^ + 2CaC03 + H2O = SnOg. H 2O + 2CaCl2 -I- CO^.
^ ^ '
169. SoDic SULPHATE produccs a white precipitate of stan-
nic acid hydrate, insoluble in excess.
SnCl4+4Na2S04+4H20=Sn02^H20+4NaCI+4(NaHS04).
170. Blowpipe.— Same as § 163.
PLATINUM.
Symbol, Pt — Atomic weight, 197. — Atomic volame, 9.12. — Specific heat^
0.0324.— Specific gravity, 2.15.— Equivalence, II and IV.— Electric conduc-
tivity at 69.2° F., 10.53. — Order of malleability commencing with gold,,
sixth ; of ductility, third ; of heat-conducting power, second.— Tenacity, 494
—Color, white.
PLATINUM OXIDES.
Platinum forms two oxides, Pt"0 and Pt'^Og, both of which
are salifiable bases. According to E. Davy, there is also an
oxide of intermediate composition.
Platinous OXIDE, PtO, is obtained as hydrate (PtO.H20 or
PtHgOg) by digesting platinous chloride in a warm solution of
potassic hydrate, and washing the precipitate formed.
PtCl2 + 2KH0+ AcJ=PtO.H20-|-2KCL
* ^ ^
Part of the hydrate remains dissolved in the alkali, and may
be precipitated by neutralizing the liquid with sulphuric acid.
According to Berzelius, it may be converted by a gentle heat
into anhydrous platinous oxide (Pt02).
Dissolves slowly in acids forming unstable salts. Boiling
hydrochloric acid resolves it into platinic chloride and metal-
lic platinum. When recently precipitated, it dissolves in
potassic hydrate or sodic hydrate, forming platintfes, which
are formed when metallic platinum is treated with caustic
alkalies.
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THE CHEMISTS' MANUAL. 63
Platinio Oxtoe, Pt02. — Dobereiner mixes platinic chloride
with an excess of sodic carbonate, evaporates to dryness, heats
the mixture gently, and dissolves out the chloride and excess
of sodic carbonate with water. There then remains a sodic
platinate containing Na2O.3PtO2.6H2O, from which nitric acid
removes the soda without dissolving the platinic oxide. When
platinic hydrate (Pt02.2H20) is gently heated, it is converted
into anhydrous Pt02, which is a black powder. Platinic oxide
imites with strong bases, forming salts called platinates
PUTIN UM SALTS.
The platinic salts are decomposed at a rea heat. The solu-
tions redden litmus-paper. Platinic chloride, if heated, is
resolved into platinous chloride, then into metallic platinum.
The color of most of the salts, yellow; platinic chloride, a
reddish-brown ; solution, reddish-yellow.
METALLIC PLATINUM.
171. Heated on chabcjoal, it does not fiise, nor does its
surface become tarnished.
173. Hydeochlokic acid has no eflfect on platinum when
pure.
173. NrrRic acid has no effect on platinum.
174. WrrRo-HYDKocHLORic ACID dissolvcs the metal slowly,
forming a reddish-yellow solution of platinic chloride (PtCl^).
3Pt-t-4(3HCl+HN03)=3PtCl4+2N^2 + 8H20.
175. SuLPHiTBic Acm has no effect on metallic platinum.
176. SiLVEB alloyed with platinum, the alloy becomes sol-
uble in nitric add.
PLATINUM SALTS.
SoltUion heat fitted for the reactions :
Platinic Chlortoe, PtCl^.
177. Htdbosulphitric acid produces a brownish-black pre-
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64 THE CHEMISTS' MANUAL.
cipitate of Platinio sulphtoe (PtS^), slowly when cool, rapidly
when hot. PtCl4+2H2S=PtS2+4HCl.
The precipitate is soluble with diflSculty in* amnionic sul-
phide ; insoluble in dilute acids, but soluble to some extent in
concentrated nitric acid, and completely dissolved by nitro-
hydrochloric acid.
178. Ammonic sulphide precipitates platinic sulphide (PtS2) 9
soluble in excess.
PtCl4-|-4NH4HS=PtS2 + 2NH^Cl+2HCl.
Acids reprecipitate the sulphide unaltered.
179. Ammonio CHLORmE produces a yellow crystalline pre-
cipitate of ammonic chloro-platinate [(NH4Cl)2PtCl4=(NH4)2
PtClg], slightly soluble in water, insoluble in alcohol.
PtCU+2NH^Cl=(NH^)2PtClg.
If the solution be very dilute, the precipitate does not ap-
pear for some hours.
Ignite the precipitate, and metallic platinum is left in a
spongy state.
180. Stannous chlomde produces a deep brown-red color
(if acid be present), due to the formation of platinous chloride
(PtCla). .
If the platinum solution be very dilute, the color is yellow,
becoming darker on standing.
Very minute quantities of platinum may be detected by this
tesL.
181. PoTAssic lODmE first colors platinum solutions deep-
red ; then, on standing, or on the application of heat, a brown
precipitate of platinic iodide separates.
PtCU-f-4KI = Ptl4 + 4KCl.
182. Metallic copper or zinc (or formic acid on heating)
precipitates platinum as a black powder (Pt), soluble in aqua-
regia, but insohible in either hydrochloric, nitric, or sulphuric
acid. It is not removed from the copper by heat. (See § 33, 96.)
Charactefistic REAmoxs, 170, 172, 173, 175, 176, 182.
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THE CHEMISTS' MANUAL. 66
GOLD.
Symbol, Au. — Atomic weight, 197. — Eqaivalenoe, I and III. — Specific
gravity, lOJM.—Orange-yellow metal.— Fuaes at 1102" C. (2015.6'' F).— -Atomic
volume, 10.04.— Specific heat, 0.0548.— Electric conductivity at 82" P., 77.96.
—Older of malleability, first ; ductility, first ; heat-oonducting power, first. —
Taiadty, 273 (iron, as 1000.)
GOLD OXIDES.
Gold forms two well-defined oxides, AugO, AujOa, ^^^ ^^^
of uncertain composition (AuO ?).
AuBous OXIDE, AujO, is obtained when anrous chloride is
decomposed by a cold potassic hydrate solution.
2AuCl+2KHO=Au20 + 2KCl=H20.
' — » — '
Aurous oxide is obtained as a green powder, partly dis-
solved by the precipitant, and soon begins to decompose, being
r^olved into auric oxide and metallic gold, which is deposited
on the sides of the vessel as a slim film, appearing green by
transmitted light, like gold-leaf. Potassic hydrate produces
no precipitate from auric chloride unless some organic matter
is present ; if tannic add is added, the precipitate (deep-black)
is aurous oxide (AusO).
AuBic OXIDE, AujOa, may be produced by adding potassic
hydrate to auric chloride, then acetic acid, then boiling the
mixture ; the precipitate, when dried, is auric oxide (AugOa).
AuCla + GKHOmKaOaAu + SKCl + SHgO.
K2O3AU + SCaH^Oam H3O3AU -f- SKC^H 3O2.
2H3O3AU -f- A (J= AU2O3 + 3H2O.
The oxide may also be prepared by digesting zinc oxide in
auric chloride, and decomposing the resulting zinc compound
with nitric acid. — (Pelletier.)
It is a brown-black powder ; when exposed to sun-light it is
veiy quickly reduced.
5
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66 THE CHEMISTS' MANUAL.
Intermediate oxide, AuO? — When stannous chloride and
organic substances act on solutions of gold, this oxide (AuO)
seems to be produced. Auric chloride stains the skin purple,
probably in consequence of the formation of this oxide.
METALLIC GOLD.
183. Heated on Chabcoal, it fuses with some diflSculty,
its surface remains bright, and no incrustation is produced.
184. Hydeochloric acid, when pure, does not act on gold.
185. NiTEic acid does not act on gold.
186. NrrBo-HYDKOCHLOEio acid dissolves the metal slowly
when cold, more rapidly when aided by heat, producing auric
chloride, and liberating nitrogen dioxide.
2Au + 2(HN03 + 3HCl)=2AuCl3+4H20 + N202.
"The gold of commerce, and also that which is found native, con-
tains more or less silver and copper. If the amount of silver present
be small, the gold is readily dissolved in aqua-regia, while the silver
remains undissolved as chloride.
" If the proportion of silver be more considerable, the gold is protected,
and its solution prevented, bj the argentic chloride formed.
" If the silver amount to more than three-fourths of the whole, it may
be entirely extracted by nitric acid, leaving the gold undissolved."— (Tirr>
TLE AND ChAIYDLEB).
187. SuLPHUBio ACID docs not attack gold.
GOLD SALTS.
The oxygen salts are few; there is a sodio-aurous htpo-
SULPHITE (sulpho-Bulphate), Aug Sj O3 . 3 Nag Sg O3 . 4 Hg 0, or
1 ^U^^lu 1 ^^'^^^Oy or Na3Au(S203)2.2H20 ; the solution of this
salt is used for fixing daguerreotype pictures. There is a
baryto-aurous hyposulphite (sulpho-sulphate) j g ^ a f O45 ^^
Ba3Au(S203)2 ; sulphuric acid removes all the barium from this
last salt, and forms hydbated aueous HYPOSCLPHirE (sulpho-
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THE CHEMISTS' MANUAL. t)7
sulphate). The haloid salts of gold are yellow, and their
solutions continue to exhibit this color up to a high degree of
dilution. The whole of them are readily decomposed on igni-
tion. Neutral solution of auric chloride reddens litmus-paper.
Solution hest jUied for the 7'eacti07is :
Auric Chloride, AUCI3.
188. Hydrosulphuric acid precipitates from dilute neutral
or acid solutions in the cold auric sulphide (AujSa).
2AUCI3 + 3H2S = AU2S3 + 6HCI.
■- ^
From boiling solutions the precipitate is aubous suLPHmE,
AujS.
2AuCl3-f 3H2S = AU2S+6HCI+2S.
Auric sulphide (AU2S3) is a black precipitate; dissolves, as
also does aurous sulphide, in yellow ammonic sulphide, par-
ticularly if heated. Acids reprecipitate it from this solution.
Auric sulphide and aurous sulphide are insoluble in hydro-
chloric, nitric, and sulphuric acid, but dissolves in nitrohydro-
chloric acid.
189. Amnionic suLpnroE produces a brownish-black pre-
cipitate of AURIC SULPHIDE (AugSj), solublc in excess if precipi-
tant is rich in sulphur.
2AUCI3 + 3NH4HS = AU2S3-I-3NH4CI + 3HCI.
190. Oxalic acid on boiling produces even in slightly
acid solutions a precipitate of finely divided metallic gold,
appearing first as a purple or brown powder, which atlerwards
separates in the form of flakes. If these flakes are rubbed,
they assume a metallic appearance.
2AUCI3 4- 3H2C2O4. = 2Au + 6HC1 + 6CO7
" If free hydrochloric or nitric acid are present this precipitate does not
occur, bat quickly makes its appearance if a Uttle ammonic hydrate be
added to the boiling solution. If but a small quantity of gold is present,
the liquid simply assumes a purple col6r."— (Tuttle and Chandler.)
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68 THE CHEMISTS' MANUAL.
191. Ferrous sulphate produces a precipitate of metallic
GOLD from its solutions, as a bluish-black powder, which be-
comes yellow and lustrous when rubbed. (The solution must
not contain an excess of nitric acid.)
2AuCl3 + 6FeS04 = 2Au + Fe2Clg + 2Fe23S04.
192. Antimonious CHLORmE precipitates metallic gold
from acid solutions of its chloride, by means of acid solution
of antimonious chloride. — (Lovel.)
3SbCl3 + 2AuCl3 = 3SbCl5 + 2Au.
193. SuLPHLTioDS ACID, or 8ulj}hurous oxide gas^ when
added to a solution of gold, precipitates metallic gold com-
pletely.
2AuCl3 + 3H20-f 3H2SO2 = 6HCI+3H2SO4+2AU.
194. Reaction, which takes place during the process of
gilding. ^
6AUCI3 + 3K2CO3 + 6Cu = 6Au + 6CUCI2 + 5KC1 4- KCIO3 4- 3C0^.
195. Stannous chloride and stannic chloride, when
mixed together, produce in very dilute solutions of gold a
PURPLE PRECIPFTATE knOWn aS " PURPLE OF CASSIUS."
An acid solution of tin sesquioxide, Sn203, produces the
same precipitate : this distinguishes stannic sesquioxide from
STANNIC OXIDE (SnO^- SnOg = 50303).
^BerzeliuH found that when " purple of cassius " was ignited
there remained a mixture of stannic oxide and metallic gold ;
he proposed to represent it as a compound of the purple gold
DIOXIDE, AuO, combined with stannic SESQunoxiDE, 50303;
hence, AuO.Sn203. A glance at its formula shows how readily
the " purple of cassius," as thus represented, may pass into
gold and stannic oxide :
AuO.Sn203=Au + 2Sn02.
" Purple of cassius " is considered by Figuier to consist of
a iirnRATEi) double st annate of gold and tin (Sn"Au20g.4H20
=Au20.Sn02.SnO.Sn02.4H20).
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THE CHEMISTS' MANUAL, 69
"A very delicate method of making this reaction is as follows : Ferric
chloride is added to stannous chloride, until a permanent yellow color is pro-
duced ; the solution is then considerably diluted. The gold solution, having
been likewise very much diluted, is poured into a beaker, which is placed
on a sheet of white paper ; a glass rod is dipped into the tin-iron solution,
and afterwards into the gold solution, when, if even a trace of the precious
metal is present, a blue or purple streak will be observed in the track of the
glass rod.-'— < Abel and Bloxah.)
The reaction will indicate by a feint coloring 1 pt. of gold in
64,000 pts. of liquid.
196. PoTAssic IODIDE produces, when added to a neutral
solution of auric chloride, a dark-green precipitate of aubio
IODIDE, Aulg.
When first added the liquid acquires a dark-green color, and
yields a dark-green precipitate of auric iodide, which redis-
Bolves on agitation ; but after 1 at. of the auric iodide has
been added to 4 at. of potassic iodide, a further addition of
the gold solution decolorizes the liquid, and fonns a permanent
precipitate of auric iodide, because the auric and potassium
iodide at first produced are thereby decomposed.
AuCl3-h4KI = KI.Aul3.
3(KI.Aul3)-f-AuCl3=4Aul3-|-3KCl.
Characteeistic Reactions, 183, 184, 185, 187, 188,
189, 195.
SCHEME FOR THE SEPARATION AND DETECTION OF THE
MEMBERS OF THE SECOND DIVISION OF GROUP II.
The solution to be examined is supposed to contain a salt
of ARSENIC, ANTIMONY, TIN, GOLD, AND PLATINUM.
Add HYDROCHLORIC ACID^NO PRECIPriATE.
Add to the acidified solution hydrosulphuric acid ; there is
produced a precipitate of
AsjSx -I- SbgSx + SnSx 4- AujSg -|- PtSg.
Wash the precipitate well, then add hydrochloric acid and
potassic chlorate, and heat gently and filter. Eesidue is sul-
phur.
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70
THE CHEMISTS' MANUAL.
SOLUTION.
AsClg + SbCla + SnCl^ 4- AuClg + RCI4.
Divide the solution into two parts.
F1B8T Pabt.
Test this portion for As« Sb, and
Sn.
Concentrate the solution ; intro-
duce some of it into a flaak contain-
ing zinc, water, and dilute sulphuric
acid. (§ 133, 102.) Then pass the
gas thus generated into a solution
of argentic nitrate ; a precipitate
is produced consisting of silver
and argentic antimonide. Ag +
Ag,Sb. Filter
Sbcx)nd Pabt.
Test this portion for Au and Pt
IMvlde into halves.
I0t Half.
Add hydrochloric
acid, then ferrous
sulphate ; boil the
mixture; there is
precipitated metal-
lic gold. Filter,
wash, dry the pre-
cipitate, and fuse
on charcoal with
borax to a globule,
yellow. (See §11>1.)
2d Half.
Add a little am-
monic chloride,
evaporate to dry-
ness over a water-
bath, and treat with
alcohol. An or-
ange-red residue
(NH4Cl),.PtCl4 in-
dicates platinum.
(See § 182.)
FZLTBATB.
Add argentic
nitrate, neutral-
ize the clear solution with dilute ammonic hydrate ; a pre-
cipitate of argentic arsenite is produced. Yellow Ag^As^
O,. (See §99, 107.)
Prbcepitatb.
Wash precipi-
tate well, intro-
duce filter, and
precipitate in a
test-tube; add
tartaric acid, and
boil for a few minutes. The antimony will dissolve ; filter. Residue. Ag.
Filtrate will contain the antimony : add hydrosulphuric acid, and boil, when
a fiocculent orange-red precipitate wiU be produced : antimonic sulphide.
(See § 126.) By this process Hoffman readily detected one part of antimony
in the presence of 199 parts of arsenic.
Detection of Tin. — The tin is precipitated in the flask by
the zinc, as a gray metallic powder. It is necessary to detach
the tin from the zinc, etc., by agitation ; then transfer the tiu
to another vessel ; wash it ; then boil in hydrochloric acid ; filter
if necessary. Add mercuric chloride ; there is produced a pre-
cipitate of mercurous chloride. (See § 160.)
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THE CHEMISTS* MANUAL.
71
SCHEME FOR THE SEPARATION AND DETECTION OF
THE MEMBERS OF GROUP II.
The solution to be examined is supposed to contain mer-
curic oxide, copper, cadmium, lead, bismuth, arsenic, antimony,
tin, gold, and platinum.
Add hydrochloric acid — ^no PEECiprrATE.
Add hydrosulphuric acid, and pass the gas through the solu-
tion ; there is precipitated
BiaSa + PbS + HgS+CdS+CuS+AsaSx + SbaSx-f AuaSs + PtSj.
Filter, and wash the precipitate well; then add yellow
AHMONio SULPHIDE ; warm gently and filter ; wash.
Rbsidub.
Wm contain the PbS, CuS, BiS,—
HgS — CdS. Wash well to remove
chlorine. (Teat with argentic ni-
trate.) Boil the precipitate with
nitric add; filter- wash.
Besidue,
HgS + S.
Sdutitm.
Contains the Pb,
Cu, Bi, and Cd,
Treat according
to Bchem& .
Solution.
Will contain the As, Sb, Sn, Au, and
Ft Add dilate sulphuric acid ; there
is precipitated
As.Sj +Sb,S8 +SnS, + Au,S, + PtS,+S.
filter and wash; dissolve in hydro-
chloric acid and potassic chlorate.
AsCl, + SbCl, + SnCl4 + AuCla + PtCl^.
Treat according to scheme.
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GROUP III.
Metals NOT peecipitated by hydrochloric acid, nor from
th^r add solutions by hydrosulphueic acid, but precipi-
tated BY AMMONIC SULPHIDE:
Aluminum, chromic oxide salts, zinc, iron, cobalt, nickel,
manganese.
ALUMINUM.
Symbol, Al. (Latin, alumen, alum). — Atomic weight, 27.4 — ^EqniTalenoe
(AIb)^!.— Specific gravity, 2.5 to 2.67.— Specific heat, 0.202.— Electric con-
ductivity at 67.2'' F., 23.76.— Atomic volume, solid, 10.56.— Malleable white
metal.
ALUMINUM OXIDE.
Aluminum unites with oxygen to form one oxide, AI2O3.
Aluminic OXIDE, AI2O3, may be prepared by biiraing metal-
lic aluminum in a fine state of division, either in the air or in
oxygen.
2Al+30 = Al203.
By precipitating d boiling solution of common alum
(Al3033S04+K2S04 = Al2S30,5.K2S04), free from iron, with
ammonic carbonate, washing the precipitate well with water,
and igniting it to expel the combined water. — (Watts.)
By igniting aluminic sulphate or ammonia alum. In the
former case sulphuric oxide is given off; in the latter, that
compound, together with ammonic sulphate; an almninic
oxide remains.
AI23SO4+ A<J = AI2O3 + 3SO3.
Al2(NH4)24S04+ Ac5 = Al203+(NH4)2S04 + 3S03.
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THE CHEMISTS' MANUAL. 78
Artificially prepared aluminic oxide is white, Sp. Gr. 3.87
and 3.90.
Alnminic monohydrate, AI2O3.H2O = AljHjO^.
Aluminic dihydrate, AI2O3.2H2O = AI2H4O5.
Alumiuic trihydrate, AI2O3.3H2O = Al2Hg0g.
Al2Cl6 + NagOeAl2 + 6H20 = 2Al203.3H20 + 6NaCl.
Alurainic hydrate (trihydrate, AI2O3.3H2O or /^^^^e^e) forms
compounds called aluminates ; the hydrogen can be replaced
by an equivalent quantity of various metals.
METALLIC ALUMINUM.
197. Heated on chabcoax, it fuses, and becomes tarnished
on the surfiM», owing to the formation of aluminic oxide
(AI2O3).
198. Hydrochloeio Acm, either dilute or concentrated,
dissolves it readily, even at low temperatures, forming alu-
minic chloride (Al2Clg), with evolution of hydrogen.
2Al + 6HCl = Al2Clg + 6H.
199. NrrRic Acro, either dilute or concentrated, does not ^
attack aluminum, at ordinary temperatures, and very slowly
even at the boiling heat.
200. Sulphuric Acro, when /wt and dilute^ dissolves it
slowly, evolving hydrogen. Neither concentrated or dilute
acid attacks aluminum in the cold.
201. PoTASSic HYD«ATE dissolvcs it readily ; caused by the
rapid oxidation of the metal, evolving hydrogen, and forming
FOTASSio AJLUHiNATE, which remains in solution.
AI2 + 6KHO = (KO)6Al2 + 6H.
Al2 + 6NaH0 = (NaO)6Al2 4-6H.
ALUMINUM SALTS.
Some of the aluminum salts are soluble, and some not ; most
of them are colorless. Aluminic chloride (AlaClg) is a yellow
crvstalline volatile solid.
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74 THE CHEMISTS' MANUAL.
The soluble salts have a sweetish, astringent taste, redden
litmus-paper, and lose their acid upon ignition. The insoluble
salts are dissolved by hydrochloric acid with the exception of
certain native compounds.
Solution best fitted for the reactions :
Alum [AI2.3SO4+K2SO4+I2H2O = Al2K2(S04)4.12H20].
203. Ammonic sulphide produces a white precipitate of
ALUMiNio HYDRATE (AlgOa.SHjO or AlgH^Og), hydrosulphuric
gas being evolved. The precipitate is insoluble in excess, but
soluble in hydrochloric and other acids.
Al2K2(S04)4+6NH4HS+6H20=Al2Hg0e+3(NH4)2S04+
K2S04-f6H2S.
203« Ammonic htdrate produces a white, gelatinous pre-
cipitate of ALUMnac HYDRATE (AlgH^Og), but slightly soluble
in excess. Insoluble if ammonic chloride be present, but solu-
ble in hydrochloric and other adds.
AI23SO4. K2SO4 + 6NH4H0 = AlgH^H- K2SO4 + 3(N H4)2S04.
" In very dilate solutions the precipitate can bardlj be distingnished by
the eye. On boiling, or shaking, however, it becomes visible, being fre-
quently carried to the surface of the liquid by entangled air-bubbles/' —
(TUTTLB AND CHAITDLER.)
204. Ammonic caebonate produces a white precipitate of
ALUMINIC HTDRATE and HYDBO AMMONIC CARBONATE {^2^6^ 6"^
NH4.H.CO3), the ammonic salt not being removed by washing.
— (H. EosE.) (Pogg. Ann. xli. 462.)
205. SoDic CARBONATE produces a white precipitate, which
after being washed and dried, then triturated with water, again
washed and dried over sulphuric acid, consists of pure aluminic
hydrate {^2^6^6)' — (James Barret, Ohem. News, i. 110.)
206. PoTAssic hydrate produces the same precipitate as
ammonia, soluble in excess, and forming at the same time
POTASSIC ALUMINATE.
AI23SO4.K2SO4 + 6KHO = Al2Kg0« + K2S04 + 3H2S04.
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THE CHEMISTS' MANUALl 75
If the solution now containing potassic aluhinate be mixed
with aluminic chloride, the aluminum from both compounds
will be precipitated as aluminio oxm£ :
AlaK^Oe+AlaCle = 2AI2O3 + 6KCL
» ^ ^
The aluminum may be precipitated as aluminic hydbate,
by first acidulating with hydrochloric acid, and then adding
ammonic hydrate.
Al2K606 + 6HCl + NH^H0 = AlaH^Oe + eKCl+NH^HO.
Sodic silicate, NasO.SiOs, precipitates when added to a solu-
tion of potassic aluminate, alumd^io silicate (AlsSigOp or
AljOa.SSiOa ?).
207. Some PHOSPHATE (ortho), when added to a solution
of alum, produces a precipitate which, in the anhydrous state,
has the composition (8AI2O3.9P2O5). — (Ludwig.)
But when the alum solution is carefully added to the sodic
phosphate, a precipitate of the neutral salt (AI2O3.P2O5.6H2O
or A1™P04.3H20, or with 4 at. or 4^ at. of H^O) is produced.
2Na2HP04+Al23S04.K2S04+6H20 = AI2O3.P2O5.6H2O
+ 2Na2S04+ H2SO4+ K2SO4.
The precipitate varies in composition, according to the
proportions of the acting solution, the temperature at which
they are mixed, and the extent to which the precipitate is
washed.
The precipitates are soluble in hydrochloric acid and re-
precipitated by ammonic hydrate. Precipitates are soluble in
excess of potassic hydrate, and reprecipitated by an excess of
acetic acid, in which they are nearly insoluble. By this be-
havior they are distinguished from aluminic hydrate (^2^6^^).
If sodic silicate (Na20.Si02) is added to the solution of
aluminic phosphate in potassic hydrate, the aluminum is pre-
cipitated as silicate (Al203.3Si02 ?), while the phosphoric acid
remains in solution.
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76 THE CHEMISTS' MANUAL.
208. Blotvtipe. — If any of the compounds of aliuninum be
heated on charcoal, then moistened with a few drops of co-
baltic nitrate (C02NO3) solution, and again strongly ignited,
an infused mass of deep sky-blue oolob is produced, which
consists of a compound of the two oxides.
By candle-light it appears violet. MB,nj ficsihle compounds,
free from aluminic compovmds^ assume the same color.
CHARAcrTEBisTio Keactions, 203, 206.
CHROMIUM.
Symbol, Cr. (Greek, erama, color). — ^Atomic weight, 52.12.— Equivalence^
II, rv, VI.— Also a pseudo-triad (Cr,)^. — ^Specific gravity, 7.01. — Discovered
by Vauqaelin in 1797. — Atomic volume, 7.00.
CHROMIUM OXIDES.
Chromium unites with oxygen to form several compounds :
CrO ; CrgOa ; CrOa ; Cr304, which is intermediate between CrO
and CfgOa ; and several oxides intermediate between CrgOa
and CrOg.
Chromous oxtoe, CrO. — This compound exists in some speci-
mens of chromic iron and in pyrope. It is precipitated as
HYDKATE by the action of potassic hydrate on a solution of
chromous chloride (CrCl2). Chromous hydrate, 2CrO.H20 or
Cr2H203, is very unstable, decomposing water at ordinary
temperatures ; unless protected from the air by precipitating
from a well-boiled solution of potassic hydrate, it is converted
as soon as formed into cheomoso-chromic oxtoe, with evolution
of hydrogen. Yellow when precipitated, brown when dry.
(Dry in atmosphere of hydrogen.) When ignited it gives off
hydrogen forming chromic oxtoe (CrgOg).
2CrO.H20+ A^=Cr203 + 2H.
The anhydrous chromous oxide (CrO) has not as yet been
obtained.
Chromoso-chromic oxtoe, Cr304 or CrO.Cr203, may be pre-
pared by precipitating chromous chloride (CrCl2) with potassic
hydrate, without excluding the air. After washing in water
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THE CHEMISTS' MANUAL. 77
and drying in the air, it has the color of Spanish tobacco. It
is but slightly attacked by acids.
Cheomic oxide, CrgOa- — This oxide exists in chrome-iron
ore and in chrom-ochre. It may be prepared by igniting mer-
curons chromate (Hg2Cr04), or ammonic di-chromate [(NH4)2
Cr^O^]. .^^
4Hg2Cr04+A<5=2Cr203+ 8Hg+100.
(NH4)2Cr207+ A<y=Cr203+4H20 + 2N.
By passing chlorochromic anhydride (Cr02Cl2) through a
red-hot porcelain tube :
4Cr02Cl2+ A<5=2Cr203 + 8Cl + 20.
By passing chlorine gas over ignited potassic di-chromate :
K2Cr207-h A<J+2Cl=Cr203+2KCl + 40.
Chromic oxide obtained by any of these processes has a
dark-green color.
Chromic Hydrates. — When chromic chloride (Cr2Cl5) is
boiled with an excess of potassic hydrate, a precipitate of
(Cr203.4H20 or Cr2H807) (Ordway) is produced.
Cr2Clc + 6KH0 + 4H20=Cr203.4H20H-6KClH-3H20.
By treating the chloride with sufficient potassic hydrate to
redissolve the precipitate first formed, and neutrahzing the
excess of alkali with hydrochloric acid, another hydrate is ob-
tained. A third hydrate is obtained by precipitating a solu-
tion of a chromic salt with excess of ammonic hydrate. The
dried precipitate thus obtained is, according to Schafiher,
CraOa-CHgO or HjgCrgOp.
Cr23S04 + 3NH^H0 + 6H20=Cr203.6H20 + 3NH4HS04.
When chromic salts are treated with an excess of sodic
hydrate, and heated, a gelatinous hydrate (Cr203.5H20 or
H ioC''208) of fine green color is precipitated.
Cr23S04+6NaH0 + 5H20-f A<^=Cr203.5H20 + 3Na2S04
+ 3H2O.
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78 THE CHEMISTS' MANUAL.
The same hydrate is obtained by pouring a chromic salt of
eitlier modification into excess of the boiling alkali solution.
When a solution of violet chrom-alum [K2Cr2(S04)4.12H20]
is poured into an excess of ammonic hydrate, and heated not
above 50° C, a grayish-green pulverulent precipitate is formed
having the composition (CrgOg.THgO or Hj^CraOjo) (Lefort).
Dissolves in acids with violet color.
K2Cr2(S04)4 + 7H20 + 3NH4H0+A<5=Cr2H,40,o-f3NH4HS04
+ K2SO4.
If the ammoniacal solution is left to evaporate in the air or
over oil of vitriol, a hydrate (CrgOg-OHgO or HjgCrjOig) is
obtained. When dry, it forms a grayish-violet, very light
powder; when dissolved in acids, it yields red salts. — (Le-
FOKT.)
Emerald-gbeen of Panetier is obtained by melting in a
crucible a mixture of equivalent quantities of boric-anhydride
and hydropotassic cbromate, and treating the fiised mass with
water, when mono-metachromic hydrate (Cr203.2H20=Cr2
H4O5) is obtained. By washing this hydrate and triturating
it, a brilliant green powder is obtained. — (Guignet.)
CnROMirM PEROXIDE, Cr203.Cr03=Cr30g or 2(Cr02). The
precipitate formed by ammonic hydrate, when added to chromic
sulphate mixed with hydropotassic chromate is (2Cr02.H20)
(Vogel). The black substance obtained by heating chromic
anhydride (trioxide) to 200^C. is, according to Traube, normal
chromic chromate, Cr203.3Cr03 or Cr50,2. The precipitate
formed by mixing the solution of chrom-alum and neutral
potassic chromate, when dried at 100° C. is (3Cr403.2Cr203.
9H2O =Cr,gO,5.9H20 = Cr,gH,8024). Chromic hydrate di-
gested with excess of chromic acid, yields a dark-brown solu-
tion, which dries up to a residue containing according to Maua
(Cr203.4Cr03 = 3Cr205).
Chromic TRioxroE (anhydride), Cr03, may be prepared by
pouring 1 vol. of potassic di-chromate in a Ain stream into
1^ vol. of sulphuric acid, stirring all the while. As the liquid
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THE CHEMISTS' MANUAL. 79
cools, chromic trioxide crystallizeB from it in crimson needles
often an inch long.
Chbomic tbioxjde melts at 190° C, and begins to decom-
pose at 250° C. ; gives off oxygen, leaving a brown oxide
CHBOMIC CHROMATE, whlch, whcn FUETHEE HEATED, is BEDUCED
to CHBOMIC OXIDE. Cbromic trioxide is a powerful oxidizing
agent, being qnickly reduced to chromic oxide by sulphydric
acid, zinc, arsenious acid, tartaric acid, sugar, alcohol, and
various other organic bodies, especially when heated.
2Cr03 + 3H2S = CraOa + SHaO + Sg.
2Cr03 + 12HC1 = CraCl^ + GHgO + Cl^.
Sulphurous acid added to a solution of a chromate throws
down a brown precipitate, consisting of (Cr203.Cr03=Cr305=
3Cr02), which is chromium peboxide.
PfiBCHBOioo acid, HjCraOg, or (HCr04). — When hydrogen
peroxide dissolved in water is mixed with a solution of chromic
acid, the liquid assumes a deep indigo-blue color, but often
loses this color very rapidly, giving off oxygen at the same
time. The same blue color is obtained by adding a mixture
of aqueous hydrogen peroxide and sulphuric or hydrochloric
acid to potassic di-chromate, but in a very short time oxygen
is evolved, and chrom-alum is left in solution. For each atom
of potassic di-chromate 4 at. oxygen are evolved, provided an
excess of hydrogen peroxide be present. We may therefore
suppose that peechbomic Acro, HgCrgOg, is first formed by the
union of HO (HjOa) with Cr03, and afterwards resolved into
oxygen and chromic hydrate. — (Baebeswiu)
HgCrjOg = H2Cr204-f O4.
According to Storer^ the coloring power of perchromic acid
is so great, that when a solution of 1 pt. potassic di-chromate
in 30.000 to 40.000 pts. water is shaken up with ether con-
taining hydrogen peroxide, the ether acquires a perceptible
blue tint ; he therefore recommends this reaction as a veby
DELICATE TEST for CHBOMIC ACID. Schonhein applies it as a
test for hydrogen peroxide.
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80 THE CHEMISTS' MANUAL.
METALLIC CHROMIUM.
209. Heated. — ^Wohleb's chkomium, when heated in the
air to redness, acquires yellow and blue tarnish like steel, and
gradually becomes covered with a film of green oxide f but
the oxidation is bj no means complete.
Peligot's chromium oxidizes with great facility, taking fire
in the air, even at a heat below redness, and being converted
into green chromic oxide, CrgOs-
Deville says when chromium is pure it is even less fusible
than platinum.
" The properties of chrominin differ considerably, according to the man-
ner in which it is prepared, the peculiarity doubtless depending chiefly on
the state of aggregation."
210. Htdrochlokic acid dissolves Wohler's chromium,
forming blue chromous chloride (CrCla) and evolving hydrogen.
CrH-2HCl = CrCl2 + 2H.
PELiGcrr's chromium also dissolves in hydrochloric acid.
Fremy's crystals of chromium ai:e not attacked by any acid,
not even by NrrROMUBiATio acid.
211. Nitric acid does not attack Wohler's chromium
when either pilute or concentrated.
Peligot's chromium is oxidized by nitric acid.
2Cr+8HN03 = Cr26N03 + N^+4H20.
Fremy's chromium is not attacked.
212. Sulphuric acid when dilute and heated dissolves
Wohler's and Peligot's chromium, forming chromic 8ULPHATe(?)
{Cr23S04) and evolving sulphurous oxide.
2Cr+6H2S04 = Cr23S04 + 3S02 4-6H20.
Fremy's crystals are not attacked.
213. Nttromuriatic acid dissolves Wohler's and P^igot's
chromium, but does not even attack Fremy's crystals of
chromium.
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THE CHEMISTS' MANUAL. 81
CHROMIUM SALTS.
The chromic salts exhibit two principal modifications, the
green and the violet. Most of the salts dissolve in hydro-
chloric acid retaining their color, but if heated, a green color
is produced. Many of the salts are soluble in water, which
salts redden litmus-paper. Chromic salts containing a volatile
acid are decomposed upon ignition. Chromous salts are but
little known, but chkomous cHLOBroE (CrCl2i is one of the
most powerful deoxidizing agents known. )
Solution best fitted for the reactions :
Chbom-Alum or Potassic Chkomic Sulphate [CraOa.SSOa.
K20.S03.12H20 = Cr2K2(S04)4.12H20].
214. Ammonic sulphide produces a white precipitate of
htdrated cheomio oxide (Cr203.9H20).
Cr2K2(S04)4 + 3NH4HS+12H20=Cr203.9H20 + 3NH4HS04 +
K2S04 + 3H^.
The precipitate is insoluble in excess, but soluble in acids.
215. Ammonio hydrate produces in solutions of the green
chromic salts, a oeayish-green PBEciprrATE; in solutions of
the violet chromic salts, a orayish-blue precipitate, both of
which yield green solutions with sulphuric or hydrochloric
acid. The liquid above the precipitate has a reddish color,
and contains a small quantity of chromic acid, which may be
precipitated by boiling the mixture. The precipitate formed
when amnionic hydrate is added in excess is (Cr203.6H20), or
H,2Cr209 w^hen dried. — (Schaffner.)
Cr2K2(S04)4+3NH4H0+6H20=Cr203.6H20 + 3NH4HS04 +
K2S04.^ *~
Lefobt states that if a violet solution of chrom-alum be
poured into excess of ammonic hydrate, and heated to a tem-
perature not exceeding 50° C, a grayish-green pulverulent
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82 THE CHEMISTS' MANUAL.
precipitate is produced, Laving the composition (Cr203.7H20
= H7Cr05), dissolving in acids to a violet color.
Fbebiy states that when ammonic hydrate is added to a
violet chromic salt, there is a precipitate produced, which,
when dried in vacuo, has the composition (CraOg.OHgO).
Cr2K2(S04)4+3NH4H0 + 9H20=Cr203.9H20 + 3NH4.HS04+
K2S04.^
It dissolves in acetic acid, ammonic hydrate, and dilute
potash-ley. Its properties are liable to considerable altera-
tions ; thus, by the action of boiling water, or by prolonged
contact with cold water, by the action of concentrated saline
solutions, by desiccation for several days in the air or in vacuo,
and trituration, it is rendered insoluble in liquids in which it
was previously soluble. Fremy is of the opinion that these alter-
ations result from an aUotropio modification of the chromic
oxide, and 7iot from loss of water. He applies the terra chbomio
oxmE to the oxide which has been rendered insoluble in acetic
acid, potassic hydrate, and ammonia in the manner just men-
tioned, and METACHROMic OXIDE to that oxide which is soluble
in these reagents, and is precipitated by ammonic hydrate from
a violet chromic salt.
216. PoTASsio HYDRATE produces a precipitate of hydrated
CHROMIC OXIDE, which is soluble in excess, but reprecipitated
by boiling, as (Cr203.5H20=CrH504, according to Lefort).
Cr2K2(S04)4+6KH0 + 5H20=Cr203.5H20+4K2S04-f3H20.
Cr2K2(S04)4-h6NaH0 + 5H20=Cr203.5H20 + 8Na2S04+K2S04
+3H2O.
According to Fr6my, the precipitate is (Cr203.9H20=2Cr
H,0«).
Cr2K2(S04)4+6KH0+9H20=Cr203.9H2q+4K2S04+3Ha0.
Cr2K2(S04)4+6NaH0+9H20=Cr2O3.9H20+3Na2S04+KaSO4
' r '
+ 3H2O.
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THE CHEMISTS' MANUAL. 88
If the green solution of chromic oxide in potassic hydrate
be boiled with plumbic oxide (or plumbic orthoplumbate), the
chromic oxide is converted into chbomic tbioxide, plumbic
oxide at the same time being dissolved. If the liquid be fil-
tered and then acidulated with acetic acid^ yellow plumbic
GHBOMATE (PbCr04) is precipitated.
" When the chromic oxide is mixed with much ferric oxide, it is not dis-
eolTed bj excess of potasrac hydrate." — (TuTTiiS and CHAin^LER.)
217. Zmc, immersed in a solution of chrom-alum or chromic
chloride, excluded from the air, (jradually reduces the chromic
saU to a chromous salt^ the liquid after a few hours acquiring
a fine blue color, and hydrogen being evolved by decomposi-
tion of the water. If the zinc be left in the solution for some
time, the whole of the metal is precipitated in the form of a
basic chromous salt, and its place taken by the zinc.
Tin likewise, at a boiling heat, reduces the chromic salt to a
chromous salt, but only to a limited extent ; and on leaving
the liquid to cool after the action has ceased, a contrary action
takes place, the chromous chloride decomposing the stannous
chloride previously formed, reducing the tin to the metallic
state, and being itself reconverted into chromic chloride.
Iron does not reduce chromic salts to chromous, but simply
precipitates a basic chromic svlphate or an oxychloride as the
caee may be.
218. Blowpipe. — If any compound of chromium be fused
on charcoal or on a platinum-foil with a little potassic nitrate
and sodic carbonate, a yellow mass of potassic gkromate is
obtained. If this be dissolved in a little water, an excess of
acetic acid and a few drops of plumbic acetate added, a yel-
low precipitate of plumbic chbomate (PbCrO^) is obtained.
219. Borax. — Compounds of chromium are dissolved in
borax, both in the oxidizing and reducing fiame, to clear beads
of a faint yellowishrgreen tint, which, upon cooling, changes
to emebald-oreen.
Chabacteristic Eeactions, 315, 216, 218, 219.
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84 THE CHEMISTS' MANUAL.
ZINC.
Symbol, Zn. — Atomic weight, 65. — Eqaivalenoe, IL — Density, 32.5. —
Molecular weight, 65. — ^Molecular volume, 2. — Hard and brittle at ordinary
temperatures and at 200" C, but between lOO** C. and IdO*" C. it is malleable
and ductile.— -Melts at 412" C— -Boils at 1040° C, evolving vapor having half
the nominal density. — Atomic volume, 18.76.— Specific heat,0.0d85. — Specific
gravity, 7.18.— Electric conductivity at 32'' F., is 29.02.
ZINC OXIDES.
Only one well-defined oxide is known — ^zmcio oxtob, ZnO.
BerzeUua regards the gray film which forms on zinc when ex-
posed to the air as the suboxide (ZngO). Thinard also states
that a glntinoas peroxide (Zn02) is produced by the action of
hydric peroxide on hydrated zinc oxide.
ZiNCio OXIDE, ZnO, occurs native contaminated with man-
ganese oxide as zincite^ and comprised with ferric and man-
ganic oxides as FranJcUnite. When zinc is burnt in the air,
this oxide is produced.
Zn-fO=ZnO.
Ordinary oxide is a white amorphous powder. Specific
gravity, 5.6. When heated, assumes a yellow color, but be-
comes white again on cooling.
ZINC SALTS.
Zincic salts are colorless ; part of them are soluble in water,
and the rest in acids. The neutral salts which are soluble in
water redden litmus-paper, and are readily decomposed by heat,
with the ej^eption of zincic sulphate^ which can bear a dull red
heat, without being decomposed. Zincic chloride is 'Volatile
at a red heat.
METALLIC ZINC.
320. Heated on chabcoal, it fuses and bums with a
white flame, forming zincic oxide (ZnO), some of which is de-
posited as an incrustation, yellow while hot, and white when
^^^^- Zn.fO=ZnO.
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THE CHEMISTS' MANUAL. 85
Z21» Hydbochlobic acid dissolves zinc, forming zincio
CHLOBiDE (ZnCl2), with evolution of hydrogen.
Zn + 2HCl=ZnCl2 + iH.
If a strip of platinum or copper be put into the solution, a
galvanic current is formed, and the zinc dissolves very rapidly.
222. Nftbic acid dissolves it readily, forming zincig
NiiBATE (Zn'iNOa). I^ *he acid be concentrated, nitrogen di-
oxide (N2O2) is given off; if very dilute, nitrogen monoxide
(NjO) is given off. ; ' , . 1/
Zn+4HN03==Zn2'N03.H-N^2 + 2H20. ^
4Zn + 10HN03=4Zn(N03)2 + N^ + 5H20.
223. SuLPHUBic acid, when diluted, readily dissolves it,
forming zincio sulphate (ZnS04) ^^^ liberating hydrogen.
' Zn + H2S04=ZnS04+iH.
Concentrated acid has scarcely any action in the cold.
** AU acids soluble in water, feven the organic acids (if not too diluted),
dissolve zinc. Hydrogen is liberated in every case, except where sulphurous
acid is ena ployed. In this case ziNCic hyposulphite (ZnS,04) a°d zikcic
SULPHATE (ZnSO^) are formed, and no gas liberated."— {T\:TnjB and Chan-
dler.)
224. POTASSIC HYDBATE, 80DIC HYDRATE, and even AMMONIC
HYDRATE, whcH boilcd with zinc, dissolve it, forming potassio
ziNCATE (K2Zn02), soDic ziNCATE (NagZnOj), and ammonic zmo-
ATE [(NH4)2Zn02], with evolution of liydrogen.
Zn + 2KH0 = K202Zn + iH.
Zn + 2NaH0=Na2Zn02-f2H.
Zn + 2NH4H0=(NH4)202Zn+2H.
225. Many metals — silver, copper, tin, for example — are
precipitated from their solutions in the metallic state by zinc,
soluble salts of zinc being formed at the same time. (See
Metallic Silver Precipitate, and § 63-162.)
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86 CHEMISTS' MANUAL.
ZINCIC SALTS.
Solution best fitted for the reactions:
Zmcio Sulphate (ZnS04).
S26. Hydbobttlphubio acid produces no precipitate in a
mineral add solution not too dilute ; but on neutral solution
it precipitates part of the zinc. From acetic acid solutions all
of the zinc may be precipitated as ZnS.HgO.
337. Ammonio sulphide produces a wliite precipitate of
HTDRATED ZINCIC SULPHmE (ZnS.HjO). — (WacKENBODEE.)
ZnS04+NH4HS+HaO=ZnS.H20H-NH4HS04.
The precipitate is insoluble in excess, but soluble in hydro-
chloric, snlphuric, and nitric acids, and in a very large excess
of acetic acid. — (Wackeneodeb.)
328. Ammonio hydbate, in neutral or but slightly acid
solutions, produces a white gelatinous precipitate of zmao
HYDBATE, solvblc in cxccss^ and reprecipitated by boiling ; also
soluble in acids and in ammonic salts.
ZnS04+2NH4H0=ZnH202 + (NH4)2S04.
339. PoTAssio HYDBATE and 8ODI0 HYDBATE produce the
same precipitate as ammonic hydrate.
ZnS04 + 2KH0=ZnH202 + K2S04.
The precipitate is soluble in excess, and from its sodic or
potassic solution it may he precipitated as ^phide by hydro-
sulphuric acid.
330. Ammonic cabbonate produces a white basic zmac
CABBONATE. If the solutious are very dilute^ or if concen-
trated and boiling, the precipitate has the composition (Zn2
COa-ZoHO + xHaO or Zn3HC04.xH20). Soluble in excess^ in
ammonic salts, and in acids.
331. SoDic CABBONATE, samc precipitate as ammonic car-
honate, but not soluble in excess, but soluble in ammonic salts
and in acids.
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CHEMISTS' MANUAL. 87
Fresenius gives the composition of the precipitate fonned
by ammonic and Bodic carbonate as (3ZnH202 + 2Zn + C03 +
4H2O or Zn5HgC20,2.4H20).
232. DisoDic 0BTHOPHO8PHATE prodnces a white precipi-
tate of DISONCIG OBTHOPHOSPHATE (Zn2H2P20e-2H20) froHl hot
solutions.
2ZnS04+2NaHP04+2H20=Zn2H2P208.2H20 + 2NaS04.
233. P0TA8810 FESBOCYANmE produccs a precipitate in the
form of a white powder of zmcic fekeocyanide (Zn4Fe2Cy5
+3H2O). The precipitate is insoluble in hydrochloric acid.
234. Blowpipe. — When oompoimds of zinc are treated
with the reducing flame on charcoal, an incrustation of zinc
oxide is formed ; yellow while hot, white when cold. If this
oxide be moistened with a little cobaltic nitrate, and then
heated, an infused mass having a green color is produced.
IRON.
Symbol, Fe.— -Atomic weight, 66.— Equivalence, II, IV, VI.— Also a
paeudo-triad (Fa,)^.— White pig-iron, Sp. Gr., 7.5— Gray pig-iron, Sp. Gr.,
7.1.— Specific gravity of iron, 7.844. — Atomic volume, 7.10.— Specific heat,
0.112.— Electric conductivity at SS** F., 16.81.
IRON OXIDES.
Iron forms two oxides corresponding to the chlorides:
Ferrous oxide, FeO, and ferric oxide, FcgOs, *^^ several oxides
of intermediate composition, called ferroso-ferric oxides, which
may be regarded as compounds of the two just mentioned ;
the most important of these is the magnetic oxide, Fe304 =
FeO.FcjOa. A trioxide may be supposed to exist in the fer-
rates (FeOa), ^ ^ potassic ferrate (KjO.FeOa), but it has not
as yet been isolated.
Ferrous oxide, FeO. Found in nature in the form of car-
bonate (FeCOg), in spathic iron ore, and in chalybeate waters.
May be obtained, according to Dehray^ by passing a mixture
of equal volumes of carbonous oxide (CO) and carbonic oxide
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88 THE CHEMISTS' MANUAL.
(CO2) over red-hot ferric oxide. It is not easily prepared in
the pure state, on account of the avidity with which it absorbs
oxygen.
Ferrous hydrate may be precipitated from a solution of
pure ferrous salt, perfectly free from air, with potassic hydrate,
also free from air, in a vessel filled with de-aerated water.
Precipitate must be washed by decantation with recently
boiled water, then dried and preserved in an atmosphere free
from oxygen. — (Schmtot.)
Ferric oxide, FegOg, occurs in nature as specular iron
ore, as martite, and as red hematite. May be obtained in
small crystals by decomposing ferric chloride with lime at a
red heat (Daubrd). May be obtained as an amorphous powder
by igniting ferrous sulphate with -^ pt. of saltpetre and
lixiviating the product; by dissolving iron in nitric acid,
evaporating, and heating the resulting nitrate to redness.
The amorphous powder is nearly black; has a specific
gravity 5.04 to 5.17. — (Rose.)
Ferric oxide is reduced to the metallic state by hydrogen
gas at a heat below redness, and at a red heat by charcoal,
carbonous oxide, and ammonia gas. Ferric oxide dissolves in
acids ; best solvent, strong, boiling hydrochloric, much facili-
tated by presence of zinc or stannous chloride ; the oxide then
dissolves as ferrous chloride.
Fe203-h6HCl-fZn = 2FeCl2-hZnCl2 + 6H.
Ferric hydrates are most, easily prepared by precipitating
a moderately dilute solution of ferric chloride with excess of
ammonic hydrate (with a smaller quantity a basic salt would be
thrown down) ; the precipitate formed in the cold (the ferrum
oxidatum fuscum of the pharmacopoeias) has the composition
Fe203.2H20, according to Gmelin (Handbook, v. 198) and
Lefort (J. p. Chem., liv. 305); Fe203.3H20, according to
Wittstein (Farm. Centr. 1853, p. 367); or 2Fe203.3H20, ac-
cording to P^au de Saint-Gilles (Ann. Ch. Phys. [3], xlvi. 47) ;
the proportion of water doubtless varying according to the
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THE CHEMISTS' MANUAL. S9
degree of dilation, the mode of precipitation, and the tempera-
ture at which the hydrate has been exposed in drying. The
hydrate precipitated from hot solutions is Fe203.2H20, accord-
ing to Lefort. — (Schaffnee, Ann. Ch. Pharm., li. 117.)
Native ferric hydrates are also of various composition.
Gothite is FejOa-HgO; and a variety of bog iron (Quellery)
from Kussia consists, according to Hermann (J. p. Chem.,
xxvii. 53), mainly of FegOj.SHgO.
If the ordinary yellow hydrate, 2Fe203.3H20 (precipitated
fix)ra chloride by ammonic hydrate), be boiled in water for seven
or eight hours, it changes to a brick-red (Fe203.H20), and is
scarcely acted on by boiling nitric acid, but dissolves slowly in
hydrochloric acid. This hydrate is precipitated when ordinary
hydrate is boiled in acetic acid (Peau de Saint-Gilles).
Ferroso-fereio oxmES and hydrates. Iron oxides inter-
mediate between ferrous and ferric oxide are called ferroso-
ferric oxides ; they may be regarded as compounds of the two.
The principal ones are the scale oxide and viagnetlc oxide.
Scale oxide, Fe809=GFeO.Fe203. If iron is heated to
redness in the air, layers of scale oxide are formed, which may
be separated. The inner layer is a blackish-gray, porous,
brittle substance, attracted l)y the magnet, and has the compo-
sition 6FeO.Fe203. The outer layer contains a larger amount
of feme oxide, 32 to 37 per cent, and on the very surface,
52.8 per cent (Mosander). The outer layer is of a reddii?h
iron-black color, dense, brittle, yields a black powder, and is
more strongly attracted by the magnet than the inner oxide.
• Magnetic oxide, Fe304=FeO.Fe203, occurs native; when
pure contains nearly 72 per cent of iron (the richest ore). It
is produced when iron is heated to redness in aqueous vapor
(Regnault, Gay Lussac). When ferrous chloride is heated to
redness with excess of sodic carbonate. — (Liebiq and Wohler).
Ferroso-ferbic hydrate ; — there are two hydrates :
Dingy-green hydrate. Made by exposing white ferrous
hydrate to the air for a short time ; or by precipitating a mix-
ture of ferrous salt with a little ferric salt by ammonic hydrate,
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90 THE CHEMISTS' MANUAL.
a dingy green hydrate of ferroso-ferric hydrate is obtained,
which is converted by the air into rusty-brown ferric hydrate.
Black hydrate. This hydrate (FeO.FeaOg+xH^O nearly) is
precipitated from a solution of magnetic oxide in hydrochloric
acid by ammonic hydrate. This black precipitate is magnetic
in the liquid if a magnet dipped in it, and the precipitate
collects around it. It contains about 7 per cent of water, and
when heated in a retort, leaves anhydrous ferroso-ferric oxide;
when heated in the air, it is converted into ferric oxide.
Fereio trioxide, FeOa, ^ ^^^ known in the free state, but
is supposed to exist in the ferrates, viz.: Potassic ferrate,
K20.Fe03=K2Fe04.
METALLIC IRON.
235. Heated on chabcoal, it is slowly converted into the
black magnetic oxide (ferroso-ferric oxide), Fe304, without
fusing.
236. Htdroohlobio acid dissolves iron, forming a pale-
green solution of FEBBOus CHLOBIDE with cvolution of hydrogen.
Fe + 2HCl=FeCl2+iH.
" a small reddae, consisting of carbon and silicon, which are constant
ingfredients of iron, remain undissolved in the fonn of a black powder." —
(TUTTLE AND CHANDLER.)
237. NrTEio acid, when concentrated, has very little action
on iron ; but if diluted, it dissolves the metal very rapidly,
forming febbic NrrBATS (FcsONOs) and liberating nitrogen
dioxide (N2O2).
2Fe + 8HN03:|fe26N03 + N^+4H20.
" Iron, which has been plunged into strong nitric acid, is said to become
passivef and is unaffected by dilute acid. The same is true of iron-wire,
one end of which has been heated to redness."— (Tuttlb and Chandlkb.)
238. SuLPHTJBic ACID, whcu concentrated, dissolves iron,
forming febbous sulphate and generating sulphurous oxide.
Fe ^2S04^= FeS04^ + S07+ 2H2O.
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THE CHiailSTS' MANUAL. ^l
If the acid used be dilute, hydrogen gas is generated.
Fe + H2S04=FeS04+2H.
239. NrrBOMUsiATio acid dissolves iron, forming febbio
CKLOKiDE (FesCl^) and liberating nitrogen dioxide (N202)-
2Fe+2(3HCl+HN03)=Fe2Cle + fS+*H20.
FERROUS SALTS.
Most of the ferrous salts are soluble and ciystallizable ; they
are white in the anhydrous state, and pale greenish>blue in the
hydrated state. The solutions have a sweetish taste, with an
inky after-taste; they quickly absorb oxygen, and are eon-
verted into basic ferric salts — ^thus: 2FeS04-|-0=Fe20.2S04
(Fe203.2S03). Ferrous salts containing a volatile acid give
up on ignition, leaving a residue of ferric oxide. The soluble
neutral salts redden litmus-paper.
Solution hest fitted for the reactions :
Febbous Sulphate (FeS04).
!340. Hydbosulphubio acid, in acid solution, produces no
precipitate, nor in neutral solutions, provided the iron is in
combination with a mineral acid. In neutral solutions, where
the iron is combined with acids such as carbonic, oxalic, tar-
taric, or acetic, part of the iron is precipitated in the form of a
BLACK HYDBATED FEBBous SULPHIDE. The precipitation in the
last three-mentioned salts going on only until a moderate quan-
tity of acid is set fi-ee.
241. AiocoNiG SULPHIDE produccs a black precipitate of
PEBBOUS SULPHIDE (FcS) (perhaps containing water) :
FeS04-fNH4HS=FeS+NH4HS04.
Soluble in dilute hydrochloric acid. The precipitate oxid-
izes rapidly in the air, being first converted into ferrous sul-
phate, then into yellow-brown boMc ferric sulphate.
242. AicMomo hydbate precipitates part of the iron as
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92 THE CHEMISTS' MANUAL.
FEBEOUB HYDRATE (FeHgOj), the rcfit reinainfl diasolved in the
liquid :
2FeS04 + 2NH4H0=FeH202+(NH4)2S04.FeS04.
The precipitate at first is nearly white ; it changes to a dirty
green ferroso-ferric hydrate (Fe304.04H8) by absorbing oxygen
from the air, then to a reddish-brown feme hydrate (FeOs.SHjO
= Fe2H,0^).
*' If the Bolation oontains free acid, or ammonic salts, amnionic hydrate
produces no precipitate, a soluble double aniraonic salt and ferrous salt being
formed [FeS04+(NH4),S04]. But on exposure to the air, oxypjen is ab-
sorbed, and ferric hydrate gradually separates." — (Tuttlb and Chandler.)
243, PoTAssic Hydeate completely precipitates the iron as
a dirty white fereous hydeate :
FeS04+2KH0=Fe(0H)a + K2S04.
The precipitate changes the same as in the case of amnionic
hydrate, absorbing oxygen from the air.
244. Potassic ferrocyanide produces in solutions per-
fectly free from ferric salts a white precipitate of potassio-
FERROUS-FERROCYANIDE (KgFegCyg) :
FeS04 + K^FeCy^ = KaFejCyg + K2SO4.
This precipitate absorbs oxygen from the air, which acquires
a blue color, and prussian blue [ferric ferrocyanide, Fe7Cyis=
Fe™4Fe"3Cyi8 or 2(Fe2/'Cy5.3Fe"Cy2, w^hich, in combination
with 18 molecules of water, constitute prussian blue] is formed,
probably thus :
eKaFeaCye + O3 = Fe^Cy , s + 3K4Fe°Cyg + FeaOg.— (Fownes.)
The oxide is dissolved by the free acid present. Nitric acid
or chlorine converts potassio-ferrous-ferrocyanide immediately
into prussian blue.
24:5. Potassic ferricyanide produces a deep-blue precipi-
tate of ferrous FERRicYANiDE, Fe°(Fe2)^Cy,2 + xH20 :
3FeS04-f-KgFe2Cy,2 + xH20=Fe3Fe2Cy,2.xH20-h3K2S04.
L
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THE CHEMISTS' MANUAL. 93
The precipitate is insoluble in hydrochloric acid^ but is de-
composed by potassic hydrate. This precipitate is known
under the name of " TurnbulFs blue."
** This is an extremely delicate test for ferrons salts. Before adding the
ferricyanide, the eolation should he addalated with aeetie acid; or if it
already contains free mineral acid, potassic or sodic acetate should he added,
in order to replace the free mineral acid, which might produce a blue color
by decomposiDg the ferticyanide." — (Tuttlb and Chandler.)
246. " NriRio acid, in the cold, imparts a brown color to
solutions of ferrous salts, due to the formation of a compound
of the ferrous salt with nitrogen dioxide (N2O2) ; thus (4FeS04.
N2O2). On applying heat this compound is destroyed — ^the
ferrous salt changed to a ferric salt, and the solution assumes a
yellow color.''
If ferrous sulphate is added very carefully to a solution con-
taining a nitrate (with the same volume of pure sulphuric acid
as the nitrate), so that the fluids do not mix, the stratum,
where the two fluids are in contact, shows a purple, after-
wards a brown, or, in cases where only minute quantities of
nitric acid are present, a reddish color. If the fluids are
mixed, a clear brownish-purple liquid is obtained.
247. Potassic and sodic carbonate and ammonic sesqui-
CABBONATE precipitate white hydrated ferrous carbonate in
thick white flakes, which, on exposure to the air, absorb oxygen
and give oflF carbonic oxide, first assuming a dirty green color,
and ultimately changing to yellowish-brown ferric hydrate.
The precipitate may be rendered more permanent by mixing
it with a little sugar when moist. Dissolved by aqueous car-
bonic acid. Exists in chalybeate waters.
248. Potassic sulphocyanate neither alters the color of
pure ferrous solutions, nor forms any precipitate in tliein.
249. Tincture of galls neither colors nor precipitates
ferrous salts, when they are quite free from ferric oxide ; but
the mixture acquires a violet-black color on exposure to the air.
250. Blowpipe. — Metallic iron may be obtained by
fusing ferrous salts on charcoal with sodic carbonate and po-
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94 THE CHEMISTS' MANUAL.
tassic cyanide. If the fused mass is washed with water in a
mortar, a black powder is obtained, which is readily attracted
by the magnet.
251. BosAx dissolves ferrous salts in the outer flame, form-
ing a yellow bead ; in the inner flame a bottle-green bead,
owing to reduction.
FERRIC SALTS.
Most of the ferric salts in solution are yellow or reddish-
yellow. The soluble neutral salts redden litmus, and are
decomposed by heat. Ferric salts are easily reduced to fer-
rous salts by various deoxidizing agents; as by sulphydric
acid, sulphurous, hyposulphurous, and phosphorous acids;
by stannous chloride ; by metallic iron, and even by silver at
the boiling heat.
Solution best Jitied for the reactions :
Fbbbio CnLOEmE (FcaClg).
252. Htdbosulphubic Aom reduces the ferric salts to the
ferrous and deposits sulphur:
Fe2Cle + H2S=2FeCl2 + 2HCl+S.
It will be seen from the reaction that the hydrogen of the
hydrosulphuric acid acts as the reducing agent.
" When in combination with a weak organic acid (as acetic acid), iron is
precipitated as sulphide (FeS) by hydroealphoric add."— (Tuttub ahd
CHA17DLBB.)
253. Ammonio suLPHmE produces, in strong solutions of
ferric salts, a black precipitate of ferrous siTLPHmE mixed
with sulphur.
Fe2Cle + 2NH4HS=FeCl2+2S+2NH4Cl + 2HCL
FeCl2 + NH^HS=FeS+NHjl + HCl.
The presence of ammonic chloride favors the precipitation.
The precipitate is easily soluble in dilute adds, the sulphur
remaining undissolved.
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THE CHEMISTS' MANUAL. 95
In very dilute Bolutions of ferric salts, hydrosulphtiric acid
only produces a blackish-green coloration, which, if kept for a
long time, deposits ferrous sulphide in black flocks.
254. Ammokio hydrate added in excess produces a pre-
cipitate of FEBBic HTDBATE, FcsOs.SH^O (Wittsteiu). (See
Ferric Hydrates under Ferric Oxide.)
The precipitate is of a brownish-red color, insoluble in am-
nionic salts, but soluble in acids.
Fe2Cle + 6NH4H0=Fe2Hg0e + 6NH4Cl.
255. PoTAssic HYDBATE produces the same precipitate as
ammonic hydrate.
Fe2Cle + 6KHO=Fe2HgOe + 6KCl.
256. PoTASsic FEBEocTANiDE produccs in very dilute solu-
tions a deep blue precipitate of Febbio FEBBocYAinDE, FcyCyig
or 2Fe2Cyj.3FeCy2 :
2Fe2Cle + SK^FeCye = Fe^Cy^ + 12KC1.
(FcyCyis i^ combination with 18 molecules of water constitute
Prussian blue.) See § 242. The precipitate is insoluble in
acid, but decomposed by potassic hydrate, with separation of
ferric hydrate :
''e7Cy,8+12KH0 = 2Fe2Hg06 + 3K4FeCye.
"This is one of the most delicate tests for iron. Neatral solutions
fihoQld be addulated with acetic acid before applying it. As strong adds
decompose the potassic f errocyanide, giving rise to a blue color, it is best to
add potassic or sodic acetate to acid solutions, in order to replace the free
mineral acid by acetic add :
HCl + KCgH,0,=KCI + H.C,H,0,."— (TuTTLE ahd Chahdleb.)
357. Potassic febbicyanide produces no precipitate in
absolutely pure ferric salts, but changes the color of the solu-
tion to a GBEENisH-BBOWN. If there is the least trace of ferrous
salt present, a blue precipitate is produced. This test distin-
guishes the ferric salts from the ferrous salts.
258. Potassic sulphoctanate does not produce a precipi-
tate, but colors the solution a deep blood-red; the color is
i
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^^ THE CHEMISTS' MANUAL.
very distinct in very dilute solutions, and is probably the most
sensitive test for ferric salts. The color is due to the forma-
tion of a soluble ferric sulphocyanide ; it appears in solution
not too acid; if much free hydrochloric or nitric acid is
present, the hydrochloric acid nearly destroys it, and a certain
quantity of nitric acid, after a while, completely destroys it.
Ammonic hydrate instantly decolorizes the red solution, and
precipitates ferric hydrate rFe2(0H)g]. Ammonic sulphide
produces a black precipitate of ferric sulphide (FegSg).
" A similar red coloration is prodaced hj potassic sulphocyanate in solu-
tion containing molybdic oxide (MoO,)or liTponitric acid."— (Frksenius.)
259. Bario carbonate, when shaken up with a ferric solu-
tion, produces a precipitate of ferric hydrate :
Fe2Cl6 + 3BaC03 + 3H20 = Fe2H60g + 3BaCl2-f3C07.
In FERROUS SALTS (sulphato excepted), baric carbonate pro-
duces no precipitate.
260. Some ACETATE. "When a solution containing a
ferric salt is rendered nearly neutral by sodic carbonate, and
then heated to boiling with addition of excess of sodic acetate^
all the iron is precipitated as a (reddish) brown basic sesqui-
acetate, and may be completely removed from the solution by
jUtering hot and washing with boiling water. If it is allowed
to remain in the solution, it jmrtiaUy redisaolvea as the latter
becomes cohl.'^^
261. Blowpipe.— See §§ 249, 250.
COBALT.
Symbol, Co.— Atomic weiflrht, 60.— Equivalence, II, IV, and probably VI.
—Also a pseudo-triad ( Co j)^.— Specific fcravity, 8.71 (to 8.95).— Malleable at
red heat— Atomic volume, 6.94.— Specific heat, 0.1069.— Electric conduc-
tivity at 82" F., 17,22.
COBALT OXIDES.
Cobalt unites with oxygen to form several oxides: CoO,
C0O2, CO2O3, CO3O4, COgOy, COgOj.
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THE CHEBflSTS' MANCTAL. 97
CoBALTous oxTOE, CoO, OT protoxide, may be obtained by
igniting cobaltous hydrate, Co(0H)2, or carbonate, C0CO3, in
close vessels, by igniting the protochloride (cobaltons chloride)
in a stream of aqueous vapor. — (Schwabzenbebo.)
Co(0H)2+ A<J=CoO + H^.
C0CO3+ A<J=CoO+C02.
CoCl2 + H20+A<J=CoO+(2H+2Ci).
The pure cobaltous oxide is a light greenish-gray or olive-
green non-magnetic powder. It is reduced to the metallic
state at a red heat by hydrogen, charcoal, carbonous oxide (CO),
potassium, and sodium.
Cobaltous hydrate, CoO.HjO or Co(H0)2, is produced when
a cobaltous salt is decomposed by potassic hydrate out of the
air. A blue basic salt is first produced, which changes slowly
(quickly on heating) to the rose-colored hydrate. If ignited
out of the air, cobaltous oxide is formed as above; but if
Ignited in the air, a higher oxide is formed. Dissolves readily
in acids, and forms cobaltous salts.
CoBALTic oxroE, C02O3 (sosquioxidc). — ^It may be prepared
by passing chlorine through water in which cobaltous hydrate
is suspended ; itis then precipitated as cobaltic hydrate :
2Co(QH)2 4\3H^+2Cl=Co203.3H20 + 2HCl.
The water is decomposecj'irf^the chlorine, and hydrochloric
acid is produced, while the oxygen of the water preoxidizes
the cobalt. "*
When this black hydrate is cautiously heated to 600° 0. or
700° C, the black cobaltic oxide is produced.
Cobaltic oxide acts as a weak base.
Cobaltic acetate is the most permanent cobaltic salt.
CoBALToso-coBALTic OXIDES. — The oxidc Co304 = (CoO.
C02O3) may be prepared by heating to redness in contact
with the air, cobaltous nitrate, oxalate, or cobaltic hydrate
(Hess, Ramraelsberg), but according to Beetz and Winkel-
blech, the oxide thus obtained is CogOy or Co, 20,4.
7
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98 THE CHEMISTS' MANUAL.
If the residue obtained by gently igniting the oxalate in
contact with air, is digested in strong hydrochloric acid, the
oxide C03O4 remains in hard, brittle, grayish-black micro-
scopic octahedrons having a metallic lustre. The same
crystalline compound is obtained by igniting dry cobaltous
chloride alone, or mixed with ammonic chloride, in dry air
or oxygen gas.— (Sohwakzbmbbbg.)
CoBALTio ANHYDKiDE, C03O5 or CoeOjo, ifl obtained in
combination with potassic oxide, by strongly igniting the
oxide C03O4, or the pure cobaltous oxide or carbonate, .with
pure potassic hydrate. A crystalline salt is formed which
contains, when dried At 100° C, KaO.SCoaOg-f-SHaO.
CoBALTio DIOXIDE, CoOg, has uot yet been obtained in a free
state, but may be supposed to exist in the oxycobaltic salts.
Co02.N205.5NH3 + H20=the nitrate.
METALLIC COBALT.
262. Heated on ohabcoal, it takes fire, and is converted
into cobaltoso-cobaltic oxide (C03O4) :
3C04-O4+ A<J=CoO.Co203 or C03O4.
It decomposes aqueous vapor at a red heat.
263. Hydrochloric acid dissolves the metal slowly in the
cold, more rapidly when heated, forming cobaltous chloiude
(C0CI2) and liberating hydrogen.
Co-|-2HCl=CoCl2+2H.
264. NriRio acid dissolves the metal easily, forming cobal-
tous nitrate [Co (N 03)2] and liberating nitrogen dioxide:
3Co + 8HN03=3Co(N03)2 + n5^+4H20.
265. SuLPHURio ACID, whcu dilute, dissolves the metal,
forming cobaltous sulphate (C0SO4), with evolution of hydro-
gen gas: ,^^
Co-|-H2S04=CoS04+2H.
If heated the metal dissolves more rapidly.
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THE CHEMISTS' MANUAL. 99
COBALTOUS SALTS.
CobcdtoiiB salts in solution have a rose-red color, except when
they are very concentrated or contain a free acid, in which
case they are blue; dilution with water changes the Uue
color to red. The neutral solutions faintly redden litmus-
paper. Cobaltous sulphate is the most pennanent, all others
being decomposed at a red heat; the sulphate can stand a
moderate red heat. Cobaltic oxide dissolves in hydrochloric
acid, forming cobaltous chloride and liberating chlorine.
Co203+6HCl=2CoCl2+icr+3H20.
Solution best fitted /or the reactions :
Cobaltic NrrEAXE, Co(N03)2.
266. HTDEoeuLPHTJBio ACID produccs no precipitate in solu-
tion containing an excess of any strong acid ; but in solutions
of the acetate, or of any cobalt salt mixed with potassic acetate,
it forms a black precipitate of cjobaltous sulphide (CoS) when
cobaltous acetate is used, and cobaltic suLPHmE (C02S3) when
cobaltic acetate is used.
267. Ammonio sulphide precipitates completely the cobalt
as cobaltous sulphide, insoluble in excess:
Co(N03)2 + NH4HS=CoS+NH4N03 + HN03.
Ammonic chloride greatly favors the precipitation. The
precipitate is with difficulty soluble in hydrochloric acid, but
dissolves in nitromuriatic acid very easily, especially when
heated.
268. Ammonio hydrate precipitates a portion of the co-
balt as a bluish basic salt [6Co(OH)2.Co(N03)2], a portion
remaining in solution as a double salt [Co(N03)2.NH4N03]
If the solution contains free acid or ammonic salts, no pre-
cipitate is produced. The precipitate in contact with the air
becomes green. If more ammonic hydrate be added, it dis-
solves and forms a brownish-red liquid, which, by the action
of the air, changes to red-brown, and then consists of the ele-
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100 THE CHEMISTS' MANUAL.
ments of ammonic hydrate united with the higher oxides of
cobalt If the precipitation is performed out of contact with
the air, cobaltous hydrate is precipitated. (See Cobaltous
OXIDB.)
269. PoTAssio HTDEATB produccs a blue precipitate of a
basic salt [6Co(0H)2.(CoN03)2], which is insoluble in excess,
assuming a green or dirty bluish-green color when exposed to
the air, from formation of cobaltic oxide ; but if protected
from the air, is converted into cobaltous hydrate of a dingy red
color. A solution of cobaltous and cobaltic chloride produces
a precipitate with potassic hydrate which does not change to
dingy red even on boiling, but merely acquires a darker color.
270, PoTAssio CYANIDE produces a red-brown precipitate of
cx)BALTO[Js CYANIDE [Co(CN)2 or CoCy2], solublc in excess,
forming a double cyanide (4:KCy.CoCy2), from which acids pre-
cipitate cobaltous cyanide :
Co(N03)2+2KCN=Co(CN)2+2KN03.
Co(CN)2 + KCN=CoKCy3 or Co(CN)2.KCN.
CoK4Cye-h4HCl=CoCy2 + 4:KCl-h4HCy.
If the solution containing an excess of potassic cyanide be
boiled with free hydrocyanic acid (generated by adding a few
drops of hydrochloric acid), a compound potassio-cobaltic
cyanide is formed (KgC,2N,2Co2=6KCy.Co2Cy5); in the solu-
tion of which acids produce^ when added, no PBECiprrATE.
(Important distinction from nickel.)
4Co(CN)2 + 12KCN-h4:HCN-h20=2KeC,2N,2Co2+2H20.
271. Potassic febrocyanide produces a pale-blue precipi-
tate of hydrAted cobaltous febrocyanide, which, when care-
fully treated, gives off the greater part of its water, and
assumes a dark-green color. Dissolves in ammonic hydrate
and carbonate; not in chloride. Insoluble in hydrochloric
acid.
272, Potassic ferricyanide produces a purplish-brown
(brown-red) precipitate of cobaltous ferricyanide, insoluble
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THE CHEMISTS' MANUAL. 101
in hydrochloric add, and in ammonic hydrate. This precipi-
tate may beprodtcced in an ammonic solution of cobalt.
373, Basic cabbonatb in the cold does not precipitate
cobaltous salts (sulphate excepted, which precipitates the
greater part of the cobalt after a long time). No precipitate
is found when cobaltous chloride is used in the cold, but when
heated to boiling, after a long time all the cobalt is pre-
cipitated.
274. Potassic NnRiTE when gradually added to cobaltous
nitrate acidified with nitric or acetic acid, precipitates a beau-
tiful OEANOB- YELLOW COMPOUND, whlch cousists, according to
A. Stromeyer, of C02O3.2N2O3.6KNO2.2H2O, and contains 13.6
per cent of metallic cobalt :
2Co(N03)2 + 12KN02 + 2C2H402-f2H20=
Co203.2N205.6KN02.2H20 + 4KN03-h2KC2H302 + NS.
*
By this reaction cobalt may be distinguished from nickel ;
dilute solutions should be concentrated before adding the
potassic nitrite. The precipitate is only slightly soluble in
water; insoluble in saline solutions and in alcohol. When
boiled with water it dissolves, though not copiously, to a red
fluid, from which alkalies precipitate cobaltous hydrate.
275« Potassic carbonate, if added hot to a hot solution of
cobaltous nitrate, produces a precipitate of 5CoO.2CO2.4H2O.
When added at the ordinary temperature, a precipitate
4C0O.2CO2.7H2O is formed ; if either of these precipitates be
boiled, they assume an indigo blue color, and the precipitate
is then 4CoO.CO2.4H2O, becoming green during washing by
absorption of oxygen.
276. Blowpipe. — When compounds of cobalt are ftised on
charcoal with a little sodic carbouate and potassic cyanide in
the inner flame, and the fused mass pulverized in the cold in
a mortar, on treating with water, metallic cobalt is obtained
as a gray powder, which is attracted by the magnet.
277. Borax, Any compound of cobalt imparts to a borax
bead in either flame a beautiftil sapphibe blue color.
CHARAcrrEBisTic REACTIONS, 267, 272, 270, 274, 277.
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102 CHBMISTS' MANUAL.
NICKEL.
Symbol, Ni.— Atomic weight, 58.— Equiyalence, II, IV, probably VI.—
Also a pseudo-triad (Ni,)^'.— Magnetic ; loses this property at 350"* C. —
Atomic volume, 6.94.— Specific hefkt, 0.1069.— Specific gravity, asa.—
Electric conductivity at 82" P., 17.23.
NICKEL OXIDE&
Nickel unites with oxygen to fonn two oxides, NiO, NI2O3 ;
the first is a salifiable base, the other is not.
NicKELous OXIDE, NiO (protoxido), may be obtained by cal-
cining nickelous nitrate, hydrate, or carbonate :
Ni(OH)2+A<J=NiO + H^.
It may be freed from traces oi peroxide^ which it sometimes
contains, by heating it to about 100*^ C. in hydrogen gas. —
(Eedmann.)
It is a dense green or grayish-green non-magnetic powder,
which does not absorb oxygen from the air, either at common
or high temperatures. It is reduced to the metallic state by
hydrogen at a red heat, and by charcoal at a white heat.
NicKBLOus HTDBATE, Ni(0H)2, is obtained as an apple^reen
precipitate, by treating the solution of a nickelous salt with
excess of potassic or sodic hydrate :
Ni(N03)2 + 2KH0=Ni(0H)2 + 2KN03.
N'(N03)2 + 2NaOH = Ni(OH)2 + 2NaN03.
Dissolves easily in acids; also in amnionic hydrate^ form-
ing a violet solution.
A crystalline hydrate [Ni(0H)2.H20] has been found as an
incrustation on chrom-iron in Texas, Pennsylvania.
NicKELic OXIDE, NigOs {sssquioxtdc and peroxide). This
oxide is produced by calcining the nitrate at a moderate heat.
2Ni(N03)2+ A<5=Nl203 + (2N202 + 50).
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THE CHEMISTS' MANUAL. 103
It is a black powder of Sp. Gr. 4.84 (Herapath), which is
resolved by ignition into oxygen and nickelous oxide.
Ni203+A<J=2NiO + a
NicKELio HYDKATB, NigOa-SHjO OT Nl2(0H)^. By passing
chlorine gas through an alkaline solution of nickelous hydrate,
a precipitate of nickelic hydrate is produced. If a nickelous
salt is mixed with an excess of caustic alkali, then with an
alkaline hypochlorite, this hydrate is produced. It is dark-
brown when suspended in water, but forms a black shining
mass when dry. When heated it readily gives oflF water and
oxygen. Dissolves in ammonic hydrate with evolution of
nitrogen^ the solution cx>nta]ning nickelous hydrate.
Anotheb hydbated nickelic oxide of a dingy light-green
color is obtained by treating the nickelouB hydrate with hydro-
gen peroxide. — (Thenabd.)
METALLIC NICKEL
278. Heated on charcoal by the outer flame, it is rapidly
oxidized and converted into nickelous oxide (NiO) without
fusing or forming an incrustation.
In the inner flame the metal is not changed.
279. Hydbochlomo acid, if not too dilute, dissolves the
metal slowly with evolution of hydrogen, forming at the same
time nickelous chlobide (NiCl2)*
Ni-i-2HCl=NICl2 + 2H.
280* NrrBio acid rapidly dissolves the metal, forming
nickelous nitrate [Ni(N03)2], and liberating at' the same
time nitrogen dioxide (N2O2).
3Ni + 8HN03=3Ni(N03)2 + NX+4:H20.
281. SuLPHURio acid dissolves the metal slowly when
dilute and aided by heat, fopning nickelous sulphate and
liberating at the same time hydrogen.
Ni + H2S04=NiS04-|-iH.
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104 THE CHEMISTS' MANUAL.
NICKELOUS SALTS.
The solutions of the nickelous salts have a light-green color.
The salts are mostly green in the hydrated state, and yellow in
the anhydrous state. The soluble neutral salts slightly redden
litmus-paper, and are decomposed at a red heat.
Solution best fitted for tlie reactions :
Nickelous NrrEATB [Ni(N03)2].
282. Hydeosulphuric acid produces no precipitate in acid
solutions, and only partially precipitates the nickel from neutral
solutions (such as sulphate or chloride) ; but if nickelous ace-
tate or any nickelous salt be mixed with sodic or potassic
acetate, the metal is completely precipitated as nickelous sul-
phide (NiS) on boiling, unless a large excess of acetic acid is
present.
283. Ammonio sulphide produces a dark-brown precipi-
tate of nickelous sulphide (NiS), which is slightly soluble in
excess, forming a dark-brown solution, from which it may be
completely precipitated by boiling :
Ni(N03)2 + NH^HS=NiS+NH4N03 + HN03.
Nickelous sulphide is solvhle with difficulty in hydrochloric
add or acetic acid, but easily soluble in nitric or nitrohydro-
chloric acids.
284* Ammonio hydrate produces no precipitate if the solu-
tion contains ammonic chloride or free acid. If the solution
is neutral, a partial precipitate of nickelous hydrate [Ni(0H)2]
is produced, a portion remaining in solution as a double salt
with the ammonic salt [Ni(N03)2 + 2NH4N03]. The precipi^
tate formed is soluble in excess, forming, after standing, a blue
solution, from which nickelous hydrate may be precipitated
by sufficient potassic hydrate.
285. Potassic hydrate produces an apple-green precipi-
tate of nickelous hydrate, insoluble in excess, soluble in am-
monic salts.
Ni(N03)2+2KH0=Ni(0H)2+2KN03.
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THE CHEMISTS' MANUAL. 105
286. F0TA8810 FEBRocYANiDE produoes a greenish-white
precipitate in flocks, consisting of nickelons fenroejanide
(Ni2Fe2Cye) and some potassic ferroejanide, soluble in am*
rnoDic hydrate, insoluble in ammonic salts and in hjdro^
chloric acid.
287. Potassic FSBSiCTAinDE prodnoes a yellowish-green pre-
cipitate of nickelons ferricyanide (N 12^620x12)7 insoluble in
hydrochloric acid; soluble in ammonic hydrate. No precipi-
tate is produced in ammonic solutions of nickel. This dis-
tinguishes nickel from cobalt. (See § 276.)
288. Potassic ctanidb produces a jellowish-green precipi-
tate of nickeUma cyanide [Ni(CN)2] :
Ni(N03)i + 2KCN=Ni(CN)2-|-2KN03.
Soluble in excess, forming a brownish-yeUow solution consist-
ing of a double cyanide of nickel and potassium [Ni(CN)2+
2KCN]:
Ni(CN)2+aKCN=2KCN.Ni(CN)2=K2NiCy4.
If sulphuric or nitric add be added to the solution, the
potassic cyanide is decomposed, and nickelons cyanide is
reprecipitated, which is only soluble with difficulty in these
acids, but more so on boiling. (See § 274.)
M^xmric oxide decomposes the solution of the double salt
[2KCN.Ni(CN)2], precipitating nickelons hydrate :
Hg0-|-2KCN.Ni(CN)2 + H20=NiH202 + 2KCN.Hg(CN)2.
' — » — '
Cobaltocyanide is not decomposed by mercuric oxide or
alkaline hypochlorites.
289. Potassic NrrBrrB produces no precipitate, even in
concentrated solutions. This distinguishes nickel from cobalt.
(See §278.)
• 290. Basic cabbokate produces no precipitate (sulphate
excepted).
291. Blowpipe. — All nickel salts, when fused on charcoal
in the inner flame with a mixture of sodic carbonate and potas-
sic cyanide, are reduced to a gray metallic powder, which is
<
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106 THE CHEMISTS' MANUAL.
attracted by the magnet. The fused mass is best washed with
water in a liiortar, when the metallic nickel (Ni) may be ob-
tained.
292. BoBAx. — Compomids of nickel give in the outer flame
a clear bead of a reddish-brown color while hot, and a pale or
dark yellow when cold. In the inner flame the bead changes
to gray and opaque, owing to reduction of the metal.
Chabactkristio Eeactions, 283, 287, 288, 292.
MANGANESE.
STinbol, Mn. — ^Atomic weight, 56. — Equivalence, 11, IV, and VI. — ^Also ft
pseudo-triad, (Mn,)vi.— -Specific gravity, 8.02.— Specific heat, 0.1217.—
Atomic volume, 7.
MANGANESE OXIDES.
Manganese unites with oxygen to form four different defi-
nite oxides :
Manganous Oxide MnO.
MANGANOSO-MANGAinO OxiDE . . Mn304.
Manganic Oxide Mn^Os.
Manganese Dioxide MnOj.
Manganous oxide, MnO (protoxide), may be obtained by
igniting manganous hydrate^ carbonate, or oxalate, at a mod-
erate heat in a dosed vessel, or better, in a stream of hydit^n,
and allowing the product to cool in that gas. Liebig and
Wohler recommend mixing equal parts of fused mangancyus
chloride and sodic carbonate with a small quantity of sal
ammoniac^ heating the mixture until it fuses, and exhausting
the fused mass with water when cold. It is a grayish-green
powder, which, according to Despretz, melts at the heat of a
forge-fire to a fine green-colored mass.
Manganous hydbate is obtained by precipitating a man-
ganous salt with " caustic potash," as a white, milky, floccu-
lent precipitate, which, on exposure to the air, turns brown by
oxidation, and is ultimately converted into manganic hydrate.
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THE CHEMISTS' MANUAL. 107
According to H. Davy, the hydrate contains 24 per cent of
water.
Makoanio Oxide, Mn203 (sesquioxide). This oxide occurs
native as hraunite (91-97 per cent MnjOa). May be obtained
by heating manganic hydrate to low redness. According to
Schneider, all the lower oxides are converted iato sesquioxide
by strong ignition in oxygen gas. Manganic oxide, when
strongly ignited in the air or in a closed vessel, gives off
oxygen, and leaves manganoso-manganic oxide. Hot strong
solphuric acid reduces it to inanganous oxide^ and dissolves it
with evolution of oxygen gas.
Manganic hydrate, Mn2H204. Found native as mangor
nite or gray manganese ore. It is found when manganous
hydrate is exposed to the air. Artificially prepared, it is a
dark-brown powder, light, and capable of soiling very strongly.
When boiled with concentrated nitric acid, it is resolved into
manganous oxide, which dissolves, and a hydrated peroxide as
« residue (Berthier). Dissolves in cold hydrochloric acid,
forming manganic chloride,
Manganoso-manganio oxide, Mn304 = MnO.MnjOa (red
oxide of manganese), occurs native as hausmannite (98-99.44
per cent Mn304). When manganous oxide, nitrate or carbonate
is strongly ignited in contact wtih air, or when either of the
other oxides is subjected to very strong ignition. This oxide
is very easily prepared. When heated to whiteness with char-
coal, it is reduced to metallic manganese. Hot sulphuric acid
dissolves it, forming manganous sulphate and liberating oxygen :
Mn304+3H2S04+ A<5=3MnS04+8H20 + 0?
Sot hydrochloric acid dissolves it with liberation of chlorine.
Mn304+8HC1+ A(J=3MnCl2 + 4H20 + 2CL
Manganese dioxide (MnOg) (peroxide), occurs native as
pyrolusite or polianite. When manganoso-manganic oxide or
manganic oxide is boiled with strong nitric acid, manganese di-
oxide is produced, or when manganous carbonate is heated in an
open vessel to 260° C. ; and any portion of carbonate that may
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108 THE CHEMISTS' MANUAL.
then remain nndecomposed, may be removed by cold and very
dilute hydrochloric acid ; whereupon, according to Forchham-
mer, pure manganese dioxide remains behind. When heated
alone, manganese dioxide is converted into manganoso-man-
ganic oxide. When drenched with strong sulphuric acid, it gives
up one-fourth of its oxygen, and yields a dark-red solution of
MANGAJsrio SULPHATE (M 023504). With cold hydrochloric acid^
it forms manganic chloride (MnjClg); ow heating^ manganous
chloride (MnClg) is obtained with evolution of chlorine.
Hydbates of manganese dioxide. In the spontaneous de-
composition of manganates or permanganates dissolved in
water or in dilute acid, a black-brown hydrated dioxide is pre-
cipitated, which cakes together to a black coherent mass
containing MnOa-HjO (Mitscherlich). The same hydrate is
formed when manganous carbonate suspended in water i&
treated with chlorine, and the black-brown residue is well
washed with dilute acid (Berthier). A hydrate containing
2Mn02.H20 is obtained when a solution of a mangjmous salt
is precipitated by a mixture of potassic hydrate and potassic
hypochlorite. — (Winkelblech).
The hydrate SMnO.HjO is deposited on evaporating a
solution of manganous bromate (Rammelsberg). The hydrate
4Mn02.H20 is obtained by treating manganoso-manganic hy-
drate with strong nitric acid (Berthier). (See Gmelin's Hand-
book, iii. 206.)
Manganese oxides, intermediate in composition between
the sesquioxide and dioxide are mostly mixtures of different
oxides (which cannot be regarded as definite chemical com-
pounds or distinct mineral species), although there are one or
two of definite composition. Psilomelane, Varvacite, Wad,
Earthy Cobalt, Cupreous Manganese, Wad or Bog Manga-
nese, Groroilite, Pelokonite.
METALLIC MANGANESE.
293. Heated on charcoal, it rapidly oxidizes, but does
not melt. Manganese oxidizes very easily when it is exposed
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THE CHEMISTS' MANUAL. 109
to the air at ordinary temperatures, and must therefore be
kept under rock-oil, or in sealed tubes. Decomposes water at
ordinary temperature, being itself oxidized.
294. Hydeochlobio acid dissolves the metal, forming
HAjroANOus CHLORIDE (MnCl2) and liberating at the same time
hydrogen. -*»-.
Mn + 2HCl=MnCl2 + 2H.
295. NrTRic acid, when dilul;e, dissolves the metal.
296. SuLPHumo acid, when dilute, dissolves the metal,
liberating hydrogen and forming manganous sulphate,
MnSO^: .^
Mn + H2S04=MnS04+2H.
The metal prepared by Brunner's process, when immersed
in strong sulphuric acid, liberates but a small quantity of
hydrogen at ordinary temperatures, but dissolves on boiling
with evolution of sulphurous oxide. In dilute sulphuric acid
it dissolves readily ; also in nitric acid, in very dilute hydro-
chloric, and in acetic acid.
MANGANOUS SALTS.
Manganous salts have a pale rose tint, which is not de-
stroyed by sulphurous or hydrochloric acid, and is therefore
chara(5teriBtic. Some of the salts are soluble in water, the rest
in acids. The ones soluble in water are decomposed at a red
heat (sulphate excepted). The solutions do not alter vege-
table colors.
Solution best fitted for the reactions :
Manganous Sulphate (MnS04).
397. Hydeosulphueio acto produces no precipitate in acid
solutions, but from a neutral solution of manganous acetate a
flesh-colored precipitate is formed after a while; but not if the
solution contains free acetic acid.
298. Ammonio suLPHroE produces in neutral solutions a
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110 THE CHEMISTS' MANUAL.
flesh-colored precipitate of hydrated kanganous sitlphidb
(MnS.xH20):
MnS04 + NH4HS+xH20=MnS.xH20 + NH4HS04.
The precipitate is insoluble in excess, but dissolves in adds,
even in acetic acid. The precipitate, on exposure to the air,
oxidizes, and its surface turns brown. The separation of the
precipitate is much fitcilitated by the presence of anunonic
chloride.
299. Ammonio hydrate produces in neutral solution &
white precipitate of manganous hydrate [Mn(0H)2] :
MnS04 + 2NH4H0=Mn(0H)2 + (NH4)2S04.
In solutions containing free acid or amnionic salts it pro-
duces no precipitate; but if sufficient anmionic hydrate is
added, and the solution exposed to the air, all the manganese
is deposited as brown manganic hydrate (MnjOg-HgO).
Manganous hydrate, on exposure to the air, oxidizes, and is
converted into manganic hydrate.
300. PoTAssiG hydrate produces a white precipitate of
MANGANOUS HYDRATE I
MnS04 + 2KH0=Mn(0H)2 + K2S04,
The precipitate soon absorbs oxygen frou) the air and turns
brown; if collected on a filter and washed, it ultimately
changes to manganic hydrate.
301. PoTASsic or soDic CARBONATE produccs a white pre-
cipitate, which, after washing with boiling water and dried in
vacuo of sulphuric acid, has the composition 2MnC03.H20 :
2MnS04+2K2C03-|-H20=2MnC03.H20+2K2S04.
, * — — I '
. If atomic quantities of manganous chloride and sodic car-
bonate are mixed together, the precipitate will contain 5Mn
C03.2Mn(0H)2.
302. PoTAssic FERRocYANiDE produccs a whitc precipitate,
soluble in hydrochloric acid. When the manganous salt is
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THE CHEMISTS' MANUAL. Ill
poured into the potassic ferrocyanide, the precipitate contains
both manganese and potassium. Both precipitates are tinged
with red.
303. PoTAflsio FEKRioYANiDE produccs a hro\jon precipitate
which is insoluble in acids.
304« Plumbic dioxidb (or red lead), when saturated with a
fluid containing manganous oxide (free from chlorine) and a
little nitric acid (firee from chlorine), and the mixture boiled
and allowed to settle, the fluid is of a purple-red color from
the formation of perma7iganic acid (Crum) or manganic ni-
l/rate (Rose).
The color is very perceptible after the excess of lead-oxide
has settled, and is the most delicate test for manganese in the
wet way.
305. Basic oaebonatb produces no precipitate except with
the sulphate.
306. Febboub salt. To determine the amount of ferrous
salt in a solution, by adding potassic permanganate and sul-
phuric (or hydrochloric) acid, the reaction is as follows :
10FeS04+K2Mn208 + 8H2S04=5Fe23S04+K2S04+2MnSO^
-I-8H2O.
K2Mn2O8-fl0FeCl2+16HCl=2MnCl2+2KCl-f5Fe2Clg + 8H2O.
307. Manganese salts of any oxide, when boiled with
hydrochloric acid, exhibit the reactions of manganous salts.
308. Manganates. Potassic manganate^ when boiled
with water, decomposes and precipitates Mn02.H20 :
3K2Mn04+3H20=Mn02.H20 + K2Mn208+4KH0.
This change is retarded by excess of alkali. Nitric, sul-
phuric, or hydrochloric acid, effects the change at once ; with
hydrochloric acid the red solution gradually becomes broWn,
and when heated, colorless, owing to .the formation oimangdn-
(ms chloride. The solution is also decolorized by sulphurous
and solphydric acid and other reducing agents.
K2Mn04+2H2S04 = MnS04+K2S04+2H20.
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112 THE CHEMISTS' MANUAL.
309. Pebmanganates form a deep purple-red colored soln-
tdon. They are very easily reduced by organic compounds,
and by all reducing reagents, such as hydrochloric, sulphur-
ous, arsenious, nitrous, and sulphydric acids, and ferrous salts
(see § 310), stannous salts, etc. ; the solution first becoming
green and ultimately colorless.
310. Manoanio salts in solution are red, and yield with po-
tassic hydrate, in the absence of ammonic chloride^ a black pre-
cipitate of manganous hydrate. They are easily reduced to
manganous salts by merely heating, also by hydrochloric, sul-
phurous, or nitrous acid or any organic compound ; the liquor
then becomes colorless. Ammonic sulphide first reduces them
to manganous salts, then precipitates the flesh-colored sulphide.
311. Blowpipe. — ^If a manganese compound be fused on
charcoal or on a piece of platinum-foil in the outer flame of
the blowpipe with sodic carbonate, there is produced sodic
manganate (Na2Mn04), which is green while hot, and bluish-
green when cold.
Potassic nitrate may be added with advantage. The mix-
ture should be heated on the under-side of the platinum-foil
in the hottest part of the flame.
313. Borax. Any compound of manganese, when heated
with borax or phosphorous salt, in the outer blowpipe flame,
forms an amethyst-colored bead containing manganoso-man-
ganic oxide, which becomes colorless in the inner flame, by
reduction of that compound to manganous oxide. This test is
very sensitive, and serves to distinguish manganese from other
metals, when not disguised by other metals forming colored
beads.
Charactebistio Eeactions, 297, 298, 304, 307, 311,
312.
SCHEME FOR THE SEPARATION AND DETECTION OF
THE MEMBERS OF GROUP III.
The solution to be examined is supposed to contain a chro-
mic SALT, a salt of ALUMINUM, ZINC, IRON, COBALT, NICKEL and
MANGANESE.
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THE CHEMISTS' MANUAL.
113
Add AMMONiG CHLOBiDE, then AMMOinc HYDBATE {until olko^
Une)^ and then ammonic sulphide. There will be precipi-
tated:
Alg(OH),4-Cr,0,.9H,04-ZnS.H,04-FeS.(xH,0?)+CoS + NiS + MnS.xH,a
Filter off the precipitate, and wash it ; dissolve it in the
fiinnel with hydrochloric acid ; then wash. There will be a
Residue.
The residue will contain
CoS + NiS + a
Test the reeidue with
borax bead (after wanh-
ing^weU).
Blae bead slgniflea^
Cobalt.
Brown bead signlflei
Kkkel.
See H 877, S98.
Place precipitate in a
porcelain cmcible, paper
and all; bum it: dissolve
residue in hot nitric acid ;
dilate, filter, and concen
trate filtrate to a few
drops. Add acetic acid^
then potassic nitrite, filter
off the precipitate and
wash.
Pbscipitati.
A Tellow
precipitate
C0,0,.2N,0..
6KNO,jgH,0.
See $974.
Test pre-
cipitate with
borax bead,
to be sore.
See ^377.
Solution.
The solution will contain the Zn, Mn, Fe, AI, Or, and H,S.
Add a few crystals of potassic chlorate, and boil to destroy H,S,
and to change FeO to Fe,0.. Add an excess of potasoic hydrate,
filter off the precipitate and wash.
SOLUTIOK.
Solution will con-
tain some of the Zn,
Al Or. Boil the so-
lution ; a precipitate
Witt be Cr.0,.6H,0.
See S 216- Filter,
wash, and test the
precipitate with bo-
rax bead. See $ 219.
Divide filtrate into
two parte.
l8T Past.
Add hv.
drosu I-
phu ri c
acid or
a m monic
sulphide ;
a precipi-
tate is
ZnS.H,0.
SeeK326,
897. Test
according
to)288.
3dPabt.
Add hy-
drochloric
acid, then
aromonic
hydrate;
a precipi-
tate is
A1,(0H)..
See $203.
Test ac-
cording to
sao8.
Pbboipttats.
Divide precipitate into three parte.
8d Part.
Dissolve
in warm
1st Pabt.
Dissolve
in hydro-
chlo r i c
acid. Then
add potas-
sic sulpho-
cyanate,
which col-
ors the
solution
a deep
blood -rea,
8 h o w i og
the pres-
ence of
IRON. See^
$358. Test
also with
p o t a s s ic
rerrocyan-
ide, S m
2d Part.
Fuse on platinum-
foil with sodic ni-
trate and sodic car-
bonate. If green,
manganese is pres-
ent. See §810. Dis-
solve residue in
water and filter.
Solution, i Rxsidux.
Contains Contains
Cr. Mn. Zn. Mn.Fe.Zn.
Add acetic ' Dissolve
acid and. in hydro-
divide inlchloric
halves. acid. Add
Add plum- inexcess,
bic ace- 1 filter, add
tate; ato filtrate
yellow hydrosul
p reel pi- *
tate Is
PbCrO,
phu ri c
acid* a
precipi-
See last ^^teis
I a r t of
$ 216.
gd ffa(f.
Add alco-
hol. Boll:
filter if
necessary:
then add
hydrosul-
p h u r i c
acid: a
precipi-
tate is
ZnS.H,0.
See $288
ZnS.H,0.
See $226.
hydrochlo-
ric acid.
Add sodic
carbonate,
a m m onic
hydrate
and l)aric
carbon-
ate : shake
well; a pre-
cipitate is
a greenish
chromic
hydrate
and baric
salt. Fil-
ter, add
a m m onic
hydrate to
filtrate;
then a m-
monic sul-
p h i d e .
which will
show the
presence
uf manga-
nese by a
precipi-
tate
MnS.xH.O.
See$29&
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G-ROUP IV.
Metals KOT precipitated by Hydrochloric Acid, Hydro-
SULPHURIC Acid, or Ammokic Sulphide.
FIRST DIVISION
Will contain the metals which are precipitated by ammonic
CARBONIC in presence of ammokic chloride, yiz.: Barium,
Strontium, and Calcium.
SECOND DIVISION
Will contain the metal which is not precipitated by ammonic
carbonate in presence of ammonic chloride, but is precipi-
tated by Bodic phosphate, viz., Magnesium.
.FIRST DIVISION.
BARIUM.
STinbol, Ba.~Atoinic weight, 187. EquiTiilSnce, IT and IV.— Beoog-
nized first hj Scheele in 1774.— IsolatcMi hj Davy in 1808.— 8p. Or,, 400.
BARIUM OXIDES.
Barium unites with oxygen to form two oxides : BaO and
BaOa-
Baric oxide, BaO. When baric iodate is ignited, all the
iodine is given oft* and f of its oxygen, there then remaining
baric oxide. .^^^
Ba(l03)2 + A<5+ BaO + I2O5.
When baric carbonate is exposed to the strongest heat of a
forge-fire, baric oxide and carbonic oxide are produced.
BaCOg + A (5= BaO + COj.
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THE CHEMISTS' MANUAL. 115
Baric oxide is a grayish-white, friable mass, having a specific
gravity of 4.7 (Karsten). 6.54 (Filhol). Heated in vapor of
carbon disulphide, it forms baric carbonate and sulphide *
8BaO + CS2 + A <5= BaCOa + 2BaS.
Bario htdbate, BaO.HgO or Ba(0H)2. When baric oxide
is moistened with water, it combines into hydrate with great
evolution of temperature. May be prepared by boiling the
sulphide with water and cupric oxide :
6BaS + 6H20 + 8CuO+A(5=5Ba(OH)2+BaS2H204+4Cu2S.
As the last two compounds are insoluble if the liquid is fil-
tered and the filtrate allowed to cool, crystals of hydrate are
deposited as the liquid cools [Ba(0H)2.8H20].
Baric dioxtoe, Ba02, may be obtained by heating baric
oxide or hydrate to low redness in a current of pure oxygen
or of air free from carbonic oxide. It is a gray powder. When
thrown into water it diffuses itself, forming a hydrate which
probably contains Ba02.3H20.
Argentic oxide, chloride, sulphate or carbonate introduced
into an acid solution of baric dioxide, is partly reduced to
metallic silver. Silver compounds in small quantities or other
similar compounds are capable of reducing large quantities of
baric dioxide. Iodine, on the other hand, decomposes it in
exactly atomic proportions:
Ba02-{-l2=Bal2-{-20.
METALLIC BARIUM.
313. Watkb. Barium decomposes water at ordinary tem-
peratures, forming bawo oxtoe and evolving hydrogen :
Ba + H20=BaO + 2H.
314. Heated in the aib, it bums with a dark-red light
(Davy), but heated before the oxyhydrogen blowpipe, it bums
with a greenish fiame (Clarke).
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116 THE CHEMISTS' MANUAL.
315* Sulphuric acid converts the metal very rapidly into
BAEio SULPHATE, with evolution of hydrogen.
Ba+H2S04=BaS04-f2H.
BARIC SALTS.
All baric salts are colorless, except those which have a
colored acid. Most of the salts are insoluble in water, but
dissolve in hydrochloric acid, with the exception of baric sul-
phate and silicofluoride, which are insoluble in any acid.
The soluble salts do not affect litmus-paper. Baric nitrate
and chloride are insoluble in alcohol. All but baric chloride
are decomposed upon ignition.
Solution best fitted for the reactions :
Baric Chloride, BaCl2.
316. Ammonio hydrate (pure) forms no precipitate even
in the most concentrated solutions.
317. PoTASsic HYDRATE (free from carbonate) produces in
concentrated solutions a precipitate of baric hydrate:
BaCl2 + 2KHO + 8H20=:Ba(OH)2.8H20-f2KCL
Water dissolves the bulky precipitate [Ba(0H)2.8H20].
318. SoDio or AMMONic CARBONATE produccs a white pre-
cipitate of BARIC CARBONATE :
BaCl2 + Na2C03 = BaCOg 4- 2NaCl.
BaCl2 + (N H4)2C03 = BaCOg + 2N H^Cl.
Baric carbonate is slightly soluble in ammonic chloride, so
that if the solution is very dilute no precipitate is produced.
With ammonic carbonate, in acid solution, a precipitate is
only produced upon heating the fluid when the last reagent is
319. Sulphuric acid and all soluble sulphates throw
down from all baric salts, whether neutral or acid, a white
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THE CHEMISTS' MANUAL. 117
polyerolent precipitate of basic bulphate, which is insoluble
in nitric or hydrochloric acid even at a boiling heat :
BaCl2 + HaS04=BaS04+2HCl.
BaCla + NagS04=r^S04 + 2NaCl.
According to Harting, a solution of baric chloride containing
1 pt. of barium in 71,000 pts. of water becomes turbid with sodic
sulphate after the lapse of half an hour. A solution of nitrate
in 200,000 to 400,000 pts. of water, after some minutes gives
a cloudiness, but in 800,000 pts. of water the reaction is no
longer visible. — (Lassaione.)
330. SoDic PHOSPHATE produccs, in neutral or alkaline
solutions, a white precipitate of baric phosphate (BaP04), which
is soluble in free acid. If ammonic hydrate is added, a por-
tion of the precipitate is converted into basic baric phosphate
(SBaO.PaOj or BaaPaOg).
331. PoTAssic CHBOMATE produccs a yellow precipitate of
BASIC CHBOMATE (BaCr04) :
BaCla + K2Cr04= BaCr04 + 2KC1.
The precipitate dissolves in nitric, hydrochloric, or excess
of chromic acid, forming a reddish-yellow colored solution,
from which it may be precipitated by ammonic hydrate.
PoTASsic BicHKOMATE may be used.
333. PoTASsic OXALATE produces a white precipitate of
BARIC OXALATE (8320409. 2 HgO), solnblc in hydrochloric and
nitric acid :
BaCl2 + 2KC204+H20 = Ba2C408^0 + 2K01.
This precipitate dissolves in oxalic acid and acetic acid ; but
the solution rapidly deposits in the form of a crystalline powder
of an HYDBOBABIC OXALATE (8820404 Hj. 4 HjO).
333. Hydbofluosilicxc acid, when added, produces a pre-
cipitate of microscopic crystals, insoluble in excess of the acid,
composed of babio silicofluobide (8aSiFg).
8a0l2 + SiHjFg = 8aSiFg 4- 2HC1.
2HF.SiF4=SIH2F6.
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118 THE CHEMISTS' MANUAL.
The precipitate is nearly insoluble in nitric and hydrochloric
acid. This reaction will detect one part of baric chloride in
3800 pts. of water. Alcohol fevors the precipitation. Stron-
tium compounds 7iot heirig precipitated by silicofluoric acid,
are therefore easUy detected from barium compounds and vice
versa,
324. Heated. Baric salts, when heated with dilute alco-
hol, impart to the flame a gbebnish-tellow color (not very
characteristic). When heated in the inner blowpipe flame,
the outer flame is colored yellowish-green. This flame, when
viewed through green glass, appears blue-obeen.
Chabagtebistio Beactioks, 316, 319, 320, 324, 323.
STRONTIUM.
Svmbol, Sr.— Atomic weight, 88.^EqmyBlenoe, II and IV.^DiBtiiigaished
by Hope in 1792.— Prepared pure bj Matthiessen in 1855. — Atomic volmne,
84.66.— Specific gravity, 2.54.— ^Electric conductivity, 6.71 (at 68-62*" F.).
STRONTIUM OXIDES
Strontium unites with oxygen to form two oxides : Stbontio
OXIDE and stbontig feboxide.
Stbontio oxide, SrO, may be prepared by heating strontic
nitrate to redness, or by exposing the carbonate, either alone
or mixed with charcoal, to the strongest heat of a forge-fire.
It is a grayish- white porous mass of specific gravity, 3.0 to
4.0 (Davy), 3.932 (Karsten), infusible, not volatile, and glows
in the blowpipe flame with a dazzling white light.
Stbontio Hydbate, SrO.H20=Sr(OH)2, may be produced by
adding atomic quantities of water to strontic oxide, when the
mass becomes hot, and the strontia hardens to a crystalline
hydrate. On dissolving the hydrate with five or six pts. of
boiling water, filtering hot, and leaving the solution to cool,
needle-shaped transparent crystals of [Sr(0H)2.8H20] are de-
posited, which deliquesce when exposed to the air. When
heated to 100** C, or above, they give off fifty per cent, of
water and leave strontic hydrate [Sr(0H)2].
Stbontig peboxide is obtained as hydrate in shining scales by
mixing " strontia water " with hydrogen peroxide. — (Thenabd.)
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THE CHEBdlSTS' MANUAL. 119
METALLIC STRONTIUM.
325. Heated in the air, it burns with a beautiful red light,
strontic oxide being formed.
3!36. Acids. Hydrochloric, sulphuric, and dilute nitric
act upon strontium, nitric acid often causing it to ignite.
Concentrated nitric add does not act upon it below the boil-
ing beat.
337. Water is readily decomposed by metallic strontium,
strontic oxide and hydrogen gas being formed.
H20 + Sr=SrO + 2H.
STRONTIC SALTS.
Strontic chloride deliquesces in moist ah*, and dissolves in
absolute alcohol; but strontic nitrate does not dissolve in
absolute alcohol, nor does it deliquesce when exposed to the air.
Solution best ^fitted for the reactions :
StBONTIO NriBATE [Sr(N03)2].
328. Ammonio hydbate does not produce a precipitate
when added to strontic nitrate.
329* PoTAssic HYDRATE producos a precipitate of strontic
hydrate [Sr(0H)2.8H20] :
Sr(N03)2-f2KH0 + 8H20 = Sr(0H)2.8H20 + 2KN03.
This precipitate of crystals dissolves more easily in water
than the corresponding baric salt.
330. SoDic or ammonio carbonate produces a white pre-
cipitate of STRONTIC carbonate :
Sr(N03)2 + Na2C03 = SrCOj + 2NaN03.
SKN03)2 4-(NH4)2C03=SrC03-f2NH4N03.
Strontic carbonate dissolves in ammonic chloride with more
difficulty than baric carbonate.
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120 THE CHEMISTS' MANUAL.
331. SuLPHUBiG Acm and sulphates produces a precipitate
of STEONTic SULPHATE ill the form of a white powder :
Sr(N03)2 + H2S04=SrS04 + 2HN03.
Sr(N03)2 + Na2S04=SrS04 + 2NaN03.
If the solution is heated, the precipitation is greatly pro-
moted.
Strontic sulphate is &r more soluble in water than baric
sulphate, therefore from dilute solution it takes a longer time
for it to separate ; even in concentrated solutions, if a calcic
sulphate solution is used, the precipitate takes some time in
forming. As strontic sulphate is insoluble in alcohol, if it be
added the precipitate will form far more rapidly. If the solu-
tion is acid with nitric or hydrochloric acid, the reaction is not
so delicate, as strontic sulphate is perceptibly soluble in those
acids.
If baric chloride is added to a solution of baric sulphate in
hydrochloric acid, then water, the mixture becomes turbid.
Strontic sulphate decomposes by long digestion in solutions of
ammonic carbonate or dicarbonate ; also, and far more rapidly,
in a boiling solution of one part of potassic carbonate and
three parts of potassic sulphate. (This is an important dis-
tinction from baric sulphate.)
332. HYDROFLuostticio Acro fails to produce a precipitate
in dilute or concentrated solutions. (See § 326.)
333. Ammonic oxalate produces a white precipitate from
even dilute solution of steontio oxalate (SrC204.H20).
S<N03)2 + (NH4)2C204+H20=SrC204.H20 + 2NH^N03.
Strontic oxalate dissolves readily in nitric and hydrochloric
acid, and slightly in ammonic salts, but very slightly in oxalic
or acetic acids. .
334. SoDic phosphate produces a white precipitate of
stbontio phosphate (Sr2H2P209 or SrHP04) :
Sf<N03)2-hNa2HP04=SrHP04+2NaN03.
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TRE CHEMISTS' MANUAL. 121
Strontic orthophosphate is a white powder, insoluble in
water, bnt solnble in water containing acids or ammonic
335* Heated with alcohol, and the mixture ignited and
stirred, the flame will be a beautiful carmine color. If strontic
salts be exposed on platinum-wire to the inner flame of the
blowpipe, the outer flame is colored red, which, when viewed
through a blue glass, appears purple to rose-colored, which dis-
tinguishes it from calcic salts, which, under the same circum-
stances, has a faint green-gray tint.
CuABAOTERisTio Beachons, 331, 332, 335.
CALCIUM.
Symbol, Ca. — Atomic weight, 40. — EquivaleDce, II and IV. — Specific
giavitj, 1.6778. — Atomic volume, 25.28. — Discovered by Davy in 1808, and
in 1855 by Matthieasen in a pure state.
CALCIUM OXIDES.
Calcium nnites with oxygen to form two oxides : CaO and
CaOa-
Calcic oxroE, CaO (Lime), may be prepared by heating
any calcic salt containing an easily expelled acid, such as calcic
nitrate or carbonate, etc. :
CaC03+ AcJ=CaO + C02.
Lime or calcic oxide, when pure, forms a white porous mass
of specific gravity 2.3 to 3.08. Lime takes up water very
rapidly, generating steam, then falling to a powder (known as
slaked lime), which is calcic hydrate (or hydrate of lime) [Ca
(0H)2=Ca0.H20]. This powder is soft, and at a red heat
gives oS its water and is converted again into qiiick-lime.
Calcic DioxroE, Ca02 (peroxide), is known only in the state
of hydrate, which falls down in fine crystalline scales when
lime-water is mixed with an aqueous solution of hydroffen
peroxide. — (Thenaed. )
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122 THE CHEMISTS' MANUAL.
METALLIC CALCIUM.
336. Water is decomposed by calcium; oalcio ozidb
(CaO) being formed and hydrogen being liberated.
H20 + Ca=CaO + 2H.
337. Acros, snch as dilute nitric, hydrochloric, and sul-
phuric, rapidly act upon the metal. Nitric acid acts so rapidly
sometimes that the metal ignites. Concentrated nitric acid
will not act upon the metal unless heated to boiling.
338. Heated in the air on platinum, it bums with a
bright flash, oxidizing and forming calcic oxide.
CALCIC SALTS.
All calcic salts dissolve in nitric or hydrochloric acid (calcic
sulphate excepted). Calcic bromide, iodide, nitrate, acetate,
and many other organic salts disaplve in water. Calcic car-
bonate, borate, phosphate, arsenate, and oxalate are insoluble
in water ; the sulphate is sparingly soluble. Calcic chloride
and nitrate are soluble in absolute alcohol, and deliquesce in
the air.
Solution best fitted for the reactions :
Calcic Chloetoe (CaCl2). (Hydsated Calgio CnLOBmE,
CaCla.SHgO.)
339. Ammonic hydrate produces no precipitate.
340. PoTAssio HYDRATE produccs a white gelatinous pre-
cipitate of calcic hydrate [Ca(0H)2], unless the solution is very
dilute.
CaCl2+2KOH=Ca(OH)2 + 2KCl.
341. SoDio CARBONATE produccs a white precipitate of
CALCIC CARBONATE (CaCOs) :
CaCla + NagCOa = CaCOg + 2NaCl.
Calcic carbonate is soluble with effervescence in nitric, hydro-
chloric, and acetic acids.
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THE CHEMISTS' MANUAL. 123
Hjdroeodic carbonate produces no precipitate in the cold ;
but on boiling, a pulverulent precipitate is produced with
escape of carbonic oxide.
342. SuLPHUBio ACID and soluble sulphates produce im-
mediately a white precipitate of hydeated calcic sulphate,
unless the solution is t*oo dilute, in which case if alcohol be
added, the precipitate is soon deposited, as calcic sulphate is
insoluble in alcohol.
CaCla + H2S04Hr 2H20=CaS04.2H20 + 2HC1.
CaClj + Na2S04 + 2H20=CaS04.2H20 + 2NaCl.
' ^ '
Hydrated calcic sulphate is slightly soluble in water, the
anhydrous salt nearly insoluble. 1 pt. of hydrate dissolves
in 332 pts. of water at any temperature (Lassaigne). The
solubility is increased by the presence of acids and sodic
chloride.
343. Hydbofluosujoio acid produces no precipitate. (See
§326.)
344. Ammonic oxalate " precipitates hydrated calcic
OXALATE (CaC204.H20) as a white pulverulent powder, at the
boiling heat or in the cold from concentrated solutions. From
very dilute solutions (provided there is no free mineral acid
present), in the cold the precipitate is always a mixture of
(CaC204.H20 and CaC204.3H20)."— (Souchay and Lessen.)
CaCl2+(NH4)2C204+H20=CaC204.H20 + 2NH4CL
345. Sodic phosphate precipitates hydrated dicalcic ortho-
phosphate (Ca2H2P208.xH20 or CaHP04.xH20) :
CaCl2 + Na2HP04+xH20=CaHP04.xH20-h2NaCl.
\» ^ *
K the solution is very slightly add, the precipitate forms
more rapidly. The precipitate is more or less soluble in acids
according to the manner of precipitations.
346. Heated. When alcohol is burnt on soluble calcic
salts, the flame is red tinged with yellow ; viewed through a
green glass, the flame appears siskin-green; through a blue
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1^ THE chemists; manual.
glass, a faint green-gray tint. The hydrated chloride and a
iew other calcic compounds, when heated in the blowpipe-
flame on platinum-wire, impart a red color to the flame, similar
to that of strontium, but less intense ; the color disappears as
soon as the salts are dehydrated, smd does not appear at all if
baric salts are present.
Characteristic Reactions, 341, 342, 343, 344, 345,
346.
[The separation and detection of the members of the first
division of Group IV will be given combined with the mem-
bers of the second division.]
SECOND DIVISION.
MAGNESIUM.
Symbol, Mg. — ^Atomic weight, 24. — Equiyalenoe, II. — ^A wire 0.297 mm.
in thickness gives a light equal to 74 stearine candles, five of which weigh a
pound.— Atomic volume, 18.76.— Specific heat, 0.245.— Specific gravity, 1.74.
—Electric conductivity at 62.6" F. is 25.47.
MAGNESIUM OXIDE.
Magnesio oxide, MgO (Magnesia), may be produced by
burning the metal in the air or in oxygen gas, or when car-
bonate or nitrate is ignited in the air. It is a white powder,
having a specific gravity of 3.07 to 3.200, increased by ignition
in a pottery-furnace to 3.61 (H. Eose). It melts under oxy-
hydrogen blowpipe, and is converted into an enamel which
scratches glass like a diamond (Clark).
Magnesio htdbate, Mg(0H)2, occurs native as brucite, and
is precipitated as a white powder on adding potassic or sodic
hydrate or baryta water in excess to the solution of a magnesic
salt.
MAGNESIUM.
347. Heated to redness in the air or in oxygen gas, it
bums with a bluish-white light, forming magnesic oxide.
Mg+0 = MgO.
348. Water is decomposed by the metal very slowly, but
if the water be acidulated the decomposition is very rapid.
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THE GH£M)STS' MANUAL. 125
349. Hydboghlobio acid. When the metal is thrown on
this acid, it takes fire momentarily.
350. Sulphuric acid, when Qoncentrated, dissolves it
dowlj) forming maonesio sulphate (MgS04) •
Mg+H2S04=MgS044-2H.
A mixture of sulphuric acid and fuming nitric acid does not
act upon it at ordinary temperatures.
MAGNESIC SALTS.
Magnesium salts are colorless unless they contain a colored
acid. They^U dissolve in hydrochloric acid, with the exception
of magnesic nietaphosphate. Magnesic carbonate, borate, phos-
phate, arsenate, arsenite, and many organic salts are insoluble in
water, but most of these salts are soluble in ahmonic cHLORmE ;
most of the others are soluble in water. They have a bitter taste.
They are decomposed on ignition (magnesic sulphate excepted).
Solution best fitted for the reactions :
Magnesic Sulphate (MgS04).
351. Hydrosulphuric acid or ammonic sulphide produce
BO precipitate.
352. A3fM0Kic HYDRATE, whcH added to an aqueous pure
solution of a magnesic salt, produces a precipitate of magnesic
HYDRATE [Mg(0H)2], which is insoluble in excess:
MgS04+2NH^0H = Mg(0H)2+(NH4)2S04.
If the solution were made previously acid (no excess), no
precipitate would be produced, owing to the formation of an
ammonic salt. Even if the solution is neutral, only part of
the magnesia is precipitated, owing to the formation of a
double ammonic salt.
353. PoTAssio HYDRATE produccs a white precipitate of
MAGNESIC HYDRATE [Mg(0H)2] :
MgSO^ + 2K0H = Mg(0H)2 + K2SO4.
The precipitate is insoluble in ammonic salts^ especially in
AMMONIC CHLORIDE.
354. SoDic CARBONATE produccs a white precipitate of
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126 THE CHEMISTS' MANUAL.
BA8I0 MAGNE8I0 CARBONATE [4MgC03 + ^fi(0H)2 + lOH^O],
" One-fifth of the carbonic oxide liberated in the process com-
bines with a portion of the magnesic carbonate and forms
a dicarbonate, which remains in solution. But if the solution
be boiled, further precipitation takes place (MgCOa-hSHgO is
produced)." Ammonic chloride and other ammonic .salts pre-
vent the precipitation and dissolve the precipitate formed.
355. Ammonio carbonate produces, after a time, a white
precipitate of ammonio-maqnesic carbonate [(NH4)2C03-|-
MgC03+4:H20=(NH4)2Mg(C03)2.4H20] in concentrated solu-
tion, but not in very dilute solutions. Ammonic chloride
only hinders the precipitation, but does not prevent it in con-
centrated solutiona
356. Baric hydrate and calcic hydrate both precipitate
magnesic hydrate :
MgS04+ Ba(0H)2=Mg(0H)2 + BaS04.
MgS04-hCa(0H)2=Mg(0H)2+CaS04.
This reaction affords an easy means of separating magnesia
fix)m the alkalies.
367. SoDic PHOSPHATE, whcu added to neutral solutions,
produce a white precipitate of maonebic phosphate (MgHP04.
7H2O). If this precipitate be boiled, trimaqnesic phosphate
[Mg3(P04)2.7H20] is produced:
MgSO^ + Na2H PO4 + 7H20= MgH PO4.7H2O + Na2S04.
•^ ^ '
If ammonic hydrate and ammonic chloride be added before
precipitating, the precipitate will be ammonic dimaonesic
orthophospiUlTE [(NH4)2Mg2(P04)2.12H20], which is a crystal-
line precipitate. This is a very delicate test for magnesic salts.
If the solution is very dilute, the crystals attach themselves
to the glass, on the sides. According to Harting (J. pr.
Chem., xxii. 60), a solution containing only ^(^^(^^(^ of mag-
nesia gives a precipitate after twenty-four hours with am-
monic phosphate mixed with free ammonic hydrate, provided
the latter solution is highly concentrated and added in equal
quantity.
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THE CHEMISTS' MANUAL.
12T
358. Ammonic oxalate, in concentrated solutions, pro-
duces a white precipitate of maonesic oxalate (M£C204.
^HjO), mixed with various ammonig-maonesic oxalates.
359. SuLPHUBio ACID produccs no precipitate.
360* Hydrofluosilicio acid produces no precipitate.
361, Heatsd on chabooal, when moistened with water to
rednessj then moistened with one drop of cobaltic nitrate;
heated again, first gently, then intensely, in the oxidation
flame, a pinJdsh mass is obtained which becomes apparent on
cooling. The salt must be free from alkalies, alkaline earths,
and heavy metallic oxides to manifest this reaction.
362. Flame. Magnesic salts impart no color to the flame.
CHASACTTEfiiSTio Eeactions, 357, 356, 359, 360, 362.
SCHEME FOR THE SEPARATION AND DETECTION OF THE
MEMBERS OF GROUP IV.
The solution to be examined is supposed to contain a salt
of BABIUM, OALCIUM, STBOimTIM, and MAGNESIUM.
Add AMMONIC CHLORIDE, then AMMONio HYDRATE, and thcu
AMMONIC CARBONATE, there will be precipitated baric, stron-
TIC, and CALCIC cajebonate ; filter and wash the precipitate.
Prbcipitate.
BaCO, + SrCO, + CaCO,.
IMsaolye in hydrochloric acid ; add
iodic acetate, and then potaasic di-
chromate; a yeUow precipitate (Ba
CrO,) is prodnoed ; filter and wush.
PmTRATB.
Test for magnesic salt by adding
Bodic phosphate; there will be pre-
cipitated magnesic phosphate [Mg»
(P0J.7H,0]. (See §367.)
Precipitatb.
BaCrO,.
(See §821.)
dnoed ; filter and wash thoroughly.
Filtrate.
Add to a portion of the filtrate calcic sulphate, and
wait ten minutes, if a precipitate forms. Add to the re<
maining portion potasedc sulphate ; a predpitate is pro-
PBECnTTATB.
Strontic sulphate, SrSO^.
§§331.885.)
(See
Pn^TRATE.
Add ammonic hydrate and oxaUo
acid ; a white precipitate is CaCgO^.
(See §§344, 346, 342.)
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G-ROUP V.
To this Groap belong PoTASSiUHy Sodium, and Ahmokia,
neither of which are precipitated by Hydroghlobic Acid,
Htdrosulphurio Acid, Ammonio Sulphide, Ammonio Cab-
BOKATB, or SODIO PHOSPHATE.
POTASSIUM.
Symbol, K.— Atomic weight, 89.1.— Equivalence, I, III and V.— Atomic
yolome, 44.96.— Specific heat, 0.16956.— Fusing point, 144.5** F.— SpedAc
gravity, 0.860. Electric conductivity between e8"-7V F., 20.85.
POTASSIUM OXIDES.
Potassium unites with oxygen to form three oxides, KgO.
K2O2, K2O4. " A gray suboxide is said also to be found during
the gradual oxidation of the metal in the air, but it is proba-
bly a mixture of the protoxide with potassium." — (Watt.)
POTASSIC PROTOXIDE, (KjO), Or ANHYDROUS POTASH. When
potassium is exposed to air free from moisture in thin slices,
potassic protoxide is produced,, or when 1 at. of potassium is
heated with 1 at. of potassic hydrate.
2KH0 + K2=2K20+iH.
It is white, very deliquescent and caustic, volatilizes at a
high temperature, melts at a low heat. Combines with water
very rapidly.
Potassic peroxide, (KjO^), or tetroxide, may be prepared
by heating pure potassium in a current of dry air moderately,
and then in dry oxygen gas. It is a chrom-yellow powder
which cakes together about 280® C. It absorbs moisture from
the air, and is decomposed by water forming potassic dioxide,
K2O2.
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THE CHEMISTS' MANUAL. 129
FoTABSio DIOXIDE, Kp029 18 fomied at a certain stage in the
preparation of the peroxide, but it is difScult to obtain it free
from the yellow peroxide. It is a white powder ; its aqueous
solution is prepared by dissolving potassic peroxide in water
as stated above.
POTASSIUM.
3,63. Heated in the air to its point of volatilization, it
bursts into flame and burns rapidly with a violet light, forming
potassic oxide (KgO).
K2 + 0=K20.
364. Water is decomposed with great violence by potas-
sium, displacing half the hydrogen and forming potassio
HrDBATE. ..A^
2H20 + K2=2KHO + H2.
** The escaping hTdrogen carries with it a small portion of the yola-
tllized metal, and takes fire from the heat evolved, burning with a beauti-
fal rose-red flame, while the metal floats on the water, and finally disap-
peais with an explosive b.orst of steam as the globule of melted potash
becomes cool enough to come into contact with the water."
POTASSIC SALTS.
' Most of the salts are readily soluble in water. They are
colorless, unless colored by their constituent acid. Potassic
sulphate, carbonate, phosphate, arsenate, and borate are not
decomposed by heat. Potassic chloride, bromide, iodide, and
hydrate volatilize without decomposition at a very high tem-
perature. Most other potassic salts are decomposed by heat.
Sdution best jUted for the reactions :
Potassic Chloride, KCl.
365. Plahnic DicHLORroE produces a yellow crystalline
precipitate of potassic chloro-platinate (2KCl.PtCl4=K2PtClg)
in neutral and acid solutions :
2KC1+ PtCl4=2KClPtCl4.
» ^ *
2KN03+2HCl+PtCl4=K2PtCl6 + 2HN03.
2KCIO3 + 2HCI+ PtCl4= KgPtCle + 2HCIO3.
9 " '
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130 THE CHEMISTS' MANUAL.
In concentrated Bolution the precipitate forms immediately,
in dilute solution only after standing for some time, and in
very dilute solution the precipitate is only discernible under
the microscope.
The dilute solution is best to be evaporated to a small bulk,
then add alcohol and a little ether (as potassic chloroplatinite
is not soluble in alcohol or ether, but is to some extent in
water). As amhonio cHLOBOPLATmrrE greatly resembles po-
tassic CHLOROPLATiNrrE, caxc must be taken not to confound
the two.
366. SoDic HTDBOTARTRATB, NaC4H506, produccB a white
crystalline precipitate of Acro potassic tartrate (KC4H5O5):
KCl+NaC4H506 = KC4H505 + KCl.
•■ •
The precipitate is soluble in 180 pts. of cold water, readily
soluble in acids or in alkaline solutions, ivisoluhle in alcohol.
In dilute solution the precipitation is facilitated by addition
of alcohol, also by agitating the solution or scratching the side
of the vessel with a glass rod. Better evaporate to small bulk,
add alcohol, then the acid sodic tartrate.
367. Tabtabio acid produces the same precipitate as sodic
hydrotartrate in neutral or alkaline solutions. If the solution
is acid, the acid must first be neutralized. The precipitate
forms very rapidly in concentrated solutions, but not in very
dilute solutions; they must first be evaporated to a small
volume.
KCl+H.C4H50^=KC4H50g + HCl.
' -* '
368. Flame. Any potassic salt that is volatile at a red
heat when brought in contact with the outer blowpipe flame,
colors the flame violet.
Alcoholic solutions of potassic salts bum with a violet flame.
The color is not visible in the presence of sodium or (lithium) ;
but if viewed through a plate of dark-blue glass, the sodium
flame is cut ofi^, and and the potassium flame becomes dis-
tinctly visible as a rich reddish-violet color.
Characteristic Eeactions, 365, 366, 368.
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THE CHEMISTS' JtfANUAL. 131
SODIUM.
STmbol, Na.— Atomic weight, 23.— Specific gmvity, 0.972. Atomic vol-
imie, 28.60.— Specific heat, 0.29840.— Fusing pgint, 207.7'' F.— Electric con-
ductivity between OS'-Tl" F., 37.48.
SODIUM OXIDES.
Sodium unites with oxygen to form two oxides : NasO and
NagOj.
SoDic oxTOE, NajO (protoxide or anhydrous soda). When
metallic sodium is burnt in the air, sodic protoxide and dioxide
are produced. If the dioxide be exposed to a very high tem-
perature, the protoxide is produced, or if sodic hydrate be
heated with atomic quantities of metallic sodium.
NaOH + Na=Na20+lHL
The specific gravity of the protoxide is 2.805. — (BIabsten.)
SoDio DIOXIDE, NajOg (peroxide). This oxide may be pre-
pared by igniting the metal in oxygen gas until constant
weight. It is a pure white powder, which becomes yellow on
heating, and on cooling, white again. When thrown into
water little by little, a solution of dioxide is obtained. If this
solution he evaporated over oil of vitriol, crystals of some
DIOXIDE HYDRATE are obtained (Na202.8H20). These crystals
left to effervesce for nine days over oil of vitriol, form another
hydrate, Na202.2H20.
SODIUM.
369. Heated in the air, it bums with a yellowish flame,
forming sodic pbotoxide and dioxide.
Na^ + O3 = NagO + NagOj.
When simply exposed to the air, it oxidizes like potassium,
but not so rapidly.
370. Water is decomposed when sodium is dropped on it ;
hydrogen is evolved while the metal runs around on the sur-
face of the water; the hydrogen does not take fire unless the
water is previously heated.
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132 THE CHEMISTS' MANUAL.
SODIC SALTS.
Sodic salts are more generally soluble than potassic salts.
They are colorless unless colored by some colored acid.
Sodic carbonate crystallizes readily whilst potassic carbonate
crystallizes with difficulty. The tabular crystals of sodic car-
bonate effervesce rapidly when exposed to the air. The same
applies to sodic sulphate, but not to potajssic sulphate.
Solution best fitted for the reactions:
Sodic Chloetoe (NaCl).
371. Taetabio acid or sodic DnABTBAXE produce no pre-
cipitate even in concentrated solutions.
373. SiLicoFLuoEio acid produces in concentrated solutions
a gelatinous precipitate of some silicofluobide (4NaF.SiF4) :
4NaCl+4HF.SiF^=4NaF.SIF^4.4HCl.
The potassic salt (4KF.SiF4) is prepared in the same way.
373. Potassic Acro metantimoniate (K2O.Sb2O5.7H2O)
(sometimes called granular antimonate of potassium). ' This
salt may be prepared by treating antimonic trichloride with
an excess of potassic hydrate sufficient to redissolve the pre-
cipitate first formed, and adding potassic permanganate till
the solution acquires a faint rose color. The liquid filtered
and evaporated, yields crystals of granular metantiomonate
(E-eynoso). This salt dissolves readily in water between 45°
and 50° C, but sparin^y in cold water. It must be preserved
in a solid state, and only dissolved as required. When this
solution is added to a sodic solution (if not too dilute), the
precipitate of sodio acid metantimoniate (Na20.Sb205-|-7H2O
or 2NaOH.Sb05 4-6H20) is flocculent at first, but finally be-
comes crystalline.
2NaCl+K20.Sb205.7H20=Na20.Sb205.7H20 + 2KCl.
If the solution to be examined contain 1 pt. of sodic salt in
800 pts. of water, the precipitate is produced immediately.
In dilute solutions the precipitate is gradual, and is deposited
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THE CHEMISTS' MANUAL. 133
as eryBtal on the sides of the glass; in solutions containing
TuW pt**of sodie salt the effect is apparent after twelve hours.
The presence of alcohol helps the precipitation. Alkali in a
free state retards it, and the presence of lithium and am-
monia Id diluted solution spoils the test ; as they themselves
fonn similar precipitates, they should first be removed, and
also earth metals if present.
The solution to be tested should be neutral, or slightly alka-
line, for free acid would separate antimonic acid from the
potassic salt.
374. Platinig dichlobide produces no precipitate with
sodic solutions.
SoDic CHLOROPLATiNATE is Very solublc in water and alcohol.
It may be prepared by slowly evaporating a drop of sodic
chloride with an excess of platinic dichloride on a piece of
glass, when crystals of sodic chloroplatinate appear, which
may be seen sometimes with the eye, and readily by the help
of a magnifier.
376. Flame. Any sodic salts colors the outer blowpipe
flame with a rich yellow color, which entirely destroys the
color produced by any other metal. Alcoholic solutions of
sodic salts bum with a yellow flame. The sodic flame is char-
acterized by its rendering a crystal of potassic dichromate,
which is illuminated by its light colorless. Paper covered
with mercuric iodide when seen by the sodic flame appears
yellowish-white (Bunsen). Viewed through green glass, its
color is orange-yellow. — (Merz.)
Chabagtesistio Beaotions, 373, 374, 375.
AMMONIA.
Symbol, NH,.— Molecular weight, 17.— Molecular volume, 3.— Density,
8.6.— One litre weighs 0.702 grams (8.6 criths).— Specific heat (H,0=1) is
0.608 (Regnault).— Specific gravity, 0.6893 (calculated by H. Davy).— Re-
fractive power (air=l) is 1.309 (Dulong). — Faraday obtained solid ammonia
by exposing the dry gas to a pressure of 20 atmospheres and to a cold of
—75'* C. — It is a white, transparent, crystalline body, which melts at 76° C.
and has a higher specific gravity than ammonia in the liquid state, which
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134 THE CHEMISTS* MANUAL.
has a specific gravity, 0.76 ; boiling point at 749 mar., barometric pressure,
-33.7^ C. (Bunsen).— Its tension at —17.78'* C. =2.48 atmospheres; at
0° C. = 4.44 atm. ; at 10.8' C. = 6 atm. ; at 19.44'' C. -= 7.60 atm. ; at 28.81*' C.
= 10. atm.
AMMONIC HYDRATE.
When ammonia gas is passed into water it is rapidly ab-
sorbed, with considerable evolution of heat and with great
expansion.
"Davj found that 1 vol. water at 10" G. and 29.8 inches barometric
pressure absorbs 670 vols, ammonia, or nearly half its weight ; the specific
gravity of this solution is 0.875. According to Dalton, water at even a
lower temperature absorbs even more ammonia, and the specific gravity of
the solution is 0.85. According to Osaun, 100 pts. water at 24" C. absorbs
8.41 pts., at 55** C, 6.96 pts. ammonia. 1 vol. water, by absorbing 505 vols,
ammonia, forms a solution occupying 1.5 vols., and having a specific
gravity 0.9 ; this, when mixed with an equal bulk of water, yields a liquid
of specific gravity 0.9455, whence it appears that aqueous anmionia expands
on dilution."— (U»B1.)
Ammonio hydeate or aqueous ammonia (NHg-hHjOrs
NH4.OH) is a colorless transparent liquid, smelling of ammonia,
and having a sharp, burning taste.
Its specific gravity varies from 1.000 to 0.86, according to
amount of ammonia it contains ; its boiling point varies simi-
larly. A perfect saturated solution freezes between —38** C.
and —41° C, forming shining, flexible needles ; at —49® C. it
solidifies to a gray gelatinous mass without smell (Fourceroy
and Vauquelin). It lost almost all its ammonia at or below
100® C. The following table, on next page, shows the amount
of real anmionia contained in ammonic hydrate of difiTerent
densities.
AMMONIC SALTS.
When ammonia or ammonic carbonate is brought in contact
with an acid, the salt corresponding to the acid is directly pro-
duced. Ammonic salts have a pungent, saline, bitter taste.
They are soluble in water generally with facility ; less soluble
in alcohol and ether. They are colorless if their acids are
colorless. They are volatile at a high temperature with or
without decomposition.
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THE CHEMISTS' MANUAL.
135
DALTON.
H. DAVY.
1 URE.
If
li
ll
ll
Speciflc
Gravity.
f|i
Speciflc
Gravity.
^
ll
is
0.85
85.8
-4** C.
0.8750
32.3*
1 0.8914
27.940
0.9363
15.900
0 86
82.6
+ 3.5^
0.8857
29.25
0.8987
27.633
0.9410
14.575
, 087 ' 29.9
10^
0.9000
26.00
0.8967
27.038
0.9455
13.250
0.88 27.3
17'
0.9054
25.37»
0.8983
26.751
0.9610
11.926
0.89 , 24.7
28'*
0.9166
22.07
09000 ' 26.500
0.9564
10.600
0.90 1 22.2
30'
0.9255
19.54
0.9045 1 25.175
09614
9275
0.91 19.8
37'
09326
17.52
0.9090 ' 23.850
0.9662
7.950
0.92
17.4
44'
0.9385
15.88
0.9133 22.525
0.9716
6.626
0.93
15.1
50'
0.9435
14.53
0.9227 1 19.875
0.9768
6.500
0.94
12 8
57*
0.9476
13.46
0.9275 ' 18.650
0.9828
3.975
,0.95
10.5
63'
0.9513
12.40
0.9320 ! 17.225
0.9887
2.660
0.96
8.3 70"
0.9645
11.56
0.9945
1.325
• 0.97
6.2 79'
0.9573
10.82
0.96
4.1 , 87*"
0.9597
10.17
0.99
2.0
92'
0.9616
1 0.9692
9.60
960»
Solution hest fitted for the reactions :
Ammonio Sulphate (NH4)2S04.
376. PoTASsio HYDRATE. If a solution containing an am-
nionic salt be treated with potassic hydrate, ammonia is liber-
ated : , « ,
(NH4)2S04+2KH0=2NH3H-K2S04+2H20.
The ammonia thus liberated may be detected by the smell,
or by the fumes generated when a volatile acid is brought in
contact with it. As, for example, hydrochloric acid pro-
duces WHITE FUMES of AMMONIC CHLORIDE :
NH3 + HCl=NH4a
The gas generated may be detected by moistened test-paper.
Calcic or sodic hydrate may be used in place of potassic
hydrate.
377. Platinio dichloride, when added to a solution con-
* These nnmberB were detenniiied by experiment ; the rest is Davy
table by calculation.
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136 ' THE CHEMISTS' MANUAL.
taining an amnionic salt, produces a yellow precipitate of ah-
MONIO CHLOBOPLATINATE [(N H 401)2 PtCl4 = (N H ^)2 PtCl g] .*
NH4Cl+PtCl4=(NH4Cl)2.PtCl4.
(NH4)2S04+ 2HC1+ PtCl4=(NH4Cl)2+PtCl4+ H2SO4.
This precipitate is somewhat lighter in color than the cor-
responding potassic precipitate. Where the precipitate is
ignited it is converted into pure metallic platinum perfectly
free from chloride.
378. Nessleb's Test. If to a solution containing an am-
monic salt, potassic hydkate be added, and a solution of mbr-
cuBio IODIDE in POTAssio IODIDE, -a. J^rowu PEEOiprrATE or
OOLOKATION is immediately produced :
NH3 + 2Hgl2=NHg2l+3HI.
(NH4)2S04+4Hgl2=2NHg2l +6HI + H2SO4.
This reaction is by far the most delicate test for ammonia.
379. SODIO ACID TABTKATE Or TAETABIC ACID produoeS a
white precipitate of ammonic acid tartrate (NH4C4H5OJ):
(N H4)2S04 + 2NaC4H jOj = 2N H4C4H jOj + Na2S04.
This precipitate is slightly soluble in cold water, readily sol-
uble in alkaline solutions and mineral acids. If this precipi-
tate be ignited the carbonaceous residue obtained will have no
alkaline reactions.
380. SoDIO PHOSPHO-MOLYBDATE produCCS a YELLOW PKB-
ciprrATE, soluble in alkalies and non-volatile oi^anic acids, but
insoluble in mineral acids.
381. Flame. Alcoholic solutions of ammonic salts bum
with a blue or violet flame.
382. Heated. Any ammonic salt, if heated, either alone
or with a fixed alkali, baryta, lime, plumbic oxide, etc., evolve
ammonia. Magnesia expels only half the ammonia, forming a
double salt.
Characteristic Reactions, 376, 378, 382.
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THE CHEMISTS' MANUAL.
137
SCHEME FOR THE SEPARATION AND DETECTION OF
MEMBERS OF GROUP V.
The solution to be ezamiiied is supposed to contain a salt
of potassium, sodium, and ammonia.
Divide the solution into two parts :
First Part.
Add potanic hydrate
and boil, Aid test for
ammonia Vith hydro-
chloric add^ also by
smell and . test-paper.
(See §376.) 'Test also
with Nessler's solution.
(§378.) ^
SB00in> Pabt.
If ammonia has been found in '* First Part/'
evaporate to dryness the '* Second Part " to ex-
pel aU ammonia. Dissolve nssidue in water;
add hydrochloric acid, then platinic dichloride;
there will be precipitated potassic chloroplati-
iiate ; filter and wash.
Pbectpitatb.
KjPiCl,. (See §365.)
Test as in § 368.
Filtrate.
Evaporate filtrate to
dryness: the presence of
red circular crystals indi-
cate the presence of a
sodic salt. Add alcohol,
and test by flaibe. (See
§376.)
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SCHEME FOR
QUALITATIVE ANALYSIS.
THE SUBSTANCE FOR EXAMINATION IS A SOLID.
PRELIMINARY EXAMINATION*
This consists in an accurate observation of the physical prop-
erties of the substance, its form, color, hardness, gravity, and
odor, and of its deportment at a high temperature, either alone
or in contact with some chemical compound which produces
decomposition.
1. The substance is heated m a dby kabbow tube.
{a). Organic compounds carbonize and blacken, evolving
empyreumatic, inflammable gases.
* The majority of the preliminary tests are taken from Manual of Chem.
Anal., by Fred. Hoffman, Ph.D.
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THE CHEMISTS' MANUAL. 139
(i). The sxibstance remains unaltered ; indicating absence
of organic matter, of salts containing water of crystallization,
and of volatile compounds.
(c). The sttbsiance fuses, eosfpelUng aqueous vapors^ which
condense in the cooler parts of the tube ; indicating salts with
water of crystallization (these will generally re-solidify after
the expulsion of the water) or decomposable hydrates, which
often give off their water without ftising.
(//)• Oases or f nines are evolved; smell of iodine from
iodine compounds ; smell of sulphurous oxide from decomposi-
tion of sulphates ; smell of nitrogen oxides from the nitrates ;
fimell of ammonia from ammonic salts, from cyanides, or from
nitrogenous organic compounds, in which latter case carboniza-
tion takes place, and either cyanogen or empyreimiatic fumes
escape with the ammonia.
(e). Stdflimates are formed by volatile substances, as sul-
phur and compounds of ammonium, mercury, arsenic, and
antimony. In this case the sublimate is removed to the bot-
tom of the test-tube, and, together with the substance, is
covered with a few small pieces of charcoal, and again heated ;
mercury and arsenic form metallic sublimates, the latter with
the characteristic garlic odor, the former without. In another
tube part of the substance is heated, and the sublimate is
moistened with solution of potassic hydrate ; mercurous chlo-
ride turns black; mercuric chloride red; and anmionic salts
evolve the odor of ammonia.
2. The substance is mixed with dried sodic carbonate,
and heated on oharooal in the reducing-flame of the
BLOWPIPE.
(a). Fusion and absorption into the coal indicates alkalies.
(b). An infusible white residue, either at once or aft«r pre-
vious fusion in the water of crystallization, indicates com-
pounds of calcium, barium, strontium, magnesium, aluminium,
zinc, or tin.
(c). A reduction to the metallic state takes place, without
formation of a peripheric incrustation upon the charcoal. Com-
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140 THE CHEMISTS' MANUAL.
pounds of tin, silver, and copper give malleable shining scales.
Compounds of irou, manganese, cobalt, and nickel are reduced
to a gray infusible powder ; all visible upon cutting the iiise
from the coal, and triturating and levigating it in an agate
mortar.
(d). Reduction with incruatation : Antimony compounds
give a brittle metallic globule and a white incrustation ; bis-
muth, a brittle globule and a brown-yellow incrustation ; lead,
a malleable globule and a yellow incrustation ; zinc and cad-
mium are reduced, but give, the former a white incrustation,
not volatile in the oxidizing flame, the latter a brown-red in-
crustation.
(e). Arsenic compounds give the smell of garlic.
(/). Borates and aluminates swell up.
(ff). Sulphur compounds give an alkaline sulphide, which^
when moistened, leaves a black stain upon a clean piece of
silver.
3.* Fuse a small portion together wiih a bead op
miorocosmio salt, and expose for some time to the ot7ter
flame of the blowpipe.
{A). The substance dissolves readily, and rather
LARGELY, TO A CLEAR BEAD (WHILE HOT).
(a). The hot bead 18 colored :
Blue, by candle-light inclining to violet — cobalt.
Green, upon cooling, blue; in the reducing-flame, after
cooling, red— COPPER.
Green, particularly fine on cooling, unaltered in the reduc-
ing-flame— CHROMIUM.
Brownish-red, on cooling, light-yellow or colorless ; in the
reducing-flaine, red whilst hot, yellow whilst cooling, then
greenish — iron.
Dark-yellow to reddish, turning lighter or altogether col-
orless on cooling ; in the reducing-flame unaltered — ^nickel.
Yellowish-brown, on cooling, changing to light-yellow or
losing its color altogether ; in the reducing-flame almost col-
♦ From "Qualitative AnaljsiB," Freeeniua, 1870, p. 252.
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THE CHEMISTS' MANUAL. 141
orless (especially after addition of a very little tin-foil), blackish-
gray on cooling — ^bismuth.
Bmght-yellowish to opal, when cold, somewhat turbid ;
in the reducing-flame, whitish-gray — silver.
Amethyst-bed, especially on cooling; colorless in the re-
dncing-flame, not quite clear — manganese.
(^B). The hot bead is colorless :
It bemains gleab on cooling: antimont, alttmina, zmc,
CADMIUM, LEAD, LIME, MAGNESIA ; the latter five metals, when
added in somewhat large proportion to the microcosmic salt,
give enamel white beads ; the bead of oxide of lead is yellow-
ish when saturated.
It BECOMES enamel-white on cooling, even when only a
small portion of the powder has been added to the microcoi|^ic
salt — ^BABYTA, STBONTIA.
(J). The substance dissolves slowly and only in small
<juantity:
{a). The bead is colorless, and remains so even after cooling ;
the undissolved portion looks semi-transparent; upon addition
of a little ferric oxide, it acquires the characteristic color of an
iron bead — snjcio acid.
(J). The bead is colorless, and remains so after the addition
of a little ferric oxide — tin.
(c). The substance does not. dissolve, but floats (in the
metallic state) in the bead — gold, platinum.
" As the body under ezamination may consist of a mixture of the most
^asimilar elements, it is impossible to give well-defined cases that shaU offer
at the same time the advantage of general applicability. If, therefoi^*eac-
tions are observed in an experiment which proceed from a combin^Bi of
two of several cases, the conclusions drawn from these reactions nRt of
course be modified accordingly." — (Fresenius.)
4. Dissolve a portion of the finely powdeeed sltb-
8TANCE in HjO, and FILTER:
If not soluble in HgO, dissolve in HCl.
« « " " HCl, " " HNO3.
« « « " . . . . HfDa, " " (3HCI+HNO3).
« « « "(3HCI+HNO3), it must be rendered sAuble
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142
THE CHEMISTS' MANUAL.
hj other means. This is generally accompanied by fusion with
three to four parts by weight of alkaline carbonates, in the case
of baric, strontic, calcic, and plumbic sulphate, and also of silicic
oxide and silicates, or by fusion with hydropotassic sulphate
in the case of aluminic oxide or aluminates.^
HaO SOLUTION.
Test with red and blue litmus-paper. Add HCl. If solu-
tion was acid, the precipitate may be either PbCl2, AgCl, or
Hg2Cl2. If solution was alkaline, it may be either 2SbCl3.
6Sb203, Sn02.H20, H4Si04, etc. Filter if precipitate forms.
Add to filtrate HjS ; if precipitate is produced, saturate the
Itquid with H2S gas and precipitate PbS, CuS, HgS, CdS, BigSj,
SbjSx, SnS^, AujSg, PtSj. Filter and wash; test accord-
Group II.
in^;o
ACTUAL ANALYSIS.
Substance to be examined is soluble in water; also such
as are insoluble in water, but soluble in HCl, HNO3, (3HCL
HNO3).
GROUP I.
SCHEME FOR DETECTING.
Ag. salts. — Hg2 salts. — Pb salts. r\
Add HCl. Free. = AgCl + HggCla + PbCla- »W^^
Filter and wash ; lay filtrate one side to be further treated
(as in Group II). No precipitate ; pass on to Group II.
Boil precipitate in HjO and filter.
FiLTRATK
PbCl, in H,0.
Ad^dilute H,S04, ^Wch wlU
precipitate PbSO^. (See §g 18, 27.)
Rbsidttb.
AyCI + Hg.Cl,.
Add NH4OH and filter.
SomnoN.
Add HNO,
which will pre-
cipitate AgCl.
(See §5.)
Rbbidub.
If black (see
§ 82). Dissolve
in (8HC1.HN0,).
Add SnCl, and
boil ; Hjr precipi-
tated. (See §88.)
* Se(» Scheme I'or Analvsis of Insoluble Sabstances.
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THE CHEMISTS' MANUAI^
143
GROUP «•
SCHEME FOR DETECTING.
Pb, Co, Bi, Hg, Cd, As, Sb, Sn, Au, Pt
Add to filtrate from Group I (after testing with HCl). WjS
until filtrate smells distinctly of the reagent; filter o^tiie
{H^pitate (after passing H^S gas through solution) ; wash it.
Lay filtrate aside (test according to Group III). If no pre-
cipitate forms, pass on to Group III. The precipitate may be :
PbS, CuS, BigSa, HgS, CdS, AsjS,, SbjS,, SnS,, Au^S^, PtSj.
Add yeUow NH4HS, warm gently and filter. ^
REsrouB. I SoLunoir.
PbS, OuS, B1,S„ H^, Cdg. { As.Bs, 8b,S., SnS., An,8s,
Wa^h well to remove 01. (Test; Add dilate H.SO. ; there ie precipitatedl
wlthA^NO,.) - +Sb,8, + SnS. + Au,S, + PtS, + S.
BoU prec. wHbHNQJ; Alter; wuh. Filter andjuab: dii*t<o)Ye iu HCl and^ao, by
' ^^ '^ gentle heat7T5ci,+8bCl,+SnCl.+Aa*+PtCl*.
Divide In two parts.
>itated^^p9.
BiSTDCB.
(bbck). Die-
Joh-e in
aeci.HNO,
«Dd boU
with Sna,
Prec.=Ilg.
(8eeS4g.)
SOLTTTIOir.
Pb, Cu, BI, Cd.
Add dUate U,SOv,
cone. 8oL to expel HSiO,
A J J n rk i At^ — z^ Test thifl , portion ftir
Add H,0 and Altar, -jt^ As, S\)\^n. ^
RssmuB.
PbSO,.
(See|$L)
Pbbcifi-
TATti
BI,O.HjO.
WMb. Diet-
idve in HCl
test (SW.)
FiLTBATI.
Cn, Cdl'.
Divide in two parts.
2o PABT
Concentrate ; Introdoce
r^ ni ^^ some into flask contaiD
Co, Bi, Od, jng Zn + H.O + H,SO,.
*^^^ See $1 laH, l(tt. Fft^esas
f^enerated into AgNO,.
Prec.=A«+Ag,Sb. Fil
ter; wash.
SoLunoir.
Add
NH^OH
and Altec. .
iBT Past.
Acidolate
with acetic
acid. Add
K.Cfy: a
AddKCN
to dbetroy
blue color ;
then add
precipitate ,H.S, which
Iff Go, ay. Iwfllprecipl.
(See nag.)! tato OdS.
; (See fm)
l8T PaBT.
FiLTRATS.
TVdd
AgNO,.
Noatralize
2d Pabt.
this portion
for
PSBOIFI-
TATB.
Wash wen
introduce
filter and i with dilate
precipitate NH.OH; a yellow pi
In a teet- (See $8 99,107.)
tabe. Add-
Test
Au, Pt
Divide in halves.
Ut Ha{f. I fdBa{f.
Add HCk Add NH.CL
then Fe80j Evaporate to
and bolL dryneMH over
Prec. eooal . water batb;
Ao. (Sec \ treat with
S 191.) alcohol.
' OraD£|«-red
rcPidae Ib (NH,ri),.PtCU
indicates Pi (See $ 188.)
tec, = Ag,AB,0,.
tartaric acid and boil for a few minates, filter (resi-
due Kg). Add H,S and boil ; an orange-red prec. :
Sb,8r (See $126.) ^
DsTBcnoN OP Tm. Detach tin
flask by auritation, then transfer the tii
boll with HCl; filter, if necessary. Add HgCl,. There is
' "'^ " (Seefiea)
TetSel; wash K J w**!* wim ii\^i, um-r, II uc^'cciNirj.
Hg.Clg ; boil Hg is precipitated, which indicates Sn,
GROUP
SCHEME FOR DETECTING.
AljOa, CrjOg, ZnO, CoO, ^^MnO, FeO, FcaOg, Append^
''Add to filtrate from ^^B II (after testing wi|jB||2S)
NH4CI+NH4OH (uDta alkSlie)+NH4HS. FUter off ^R)r©.
l^PRbcI
by Google
144
THE CHEMISTS' MANUAL.
cipitate. Lay filtrate to one side to be tested according to
Group IV. If no precipitate forms, pass on to Group IV.
The precipitate may be : ,
Al2(0H)c + Cr203.9H20+ZnS.H20 + FeS(xH20?)+CoS +
# NiS+MnS.xH20.
Wash, and dissolve in the funnel with HCl, then wash again.
There will be a
1 to
phate? and o:
and filter.
txolat
.tef> of Ca, Ba, Sr, Mg. Dissolve precipitate to acetic acid
FiLTBATI.
Divide in two parts.
IsT, Pabt,
part
I to a
am-
datc
^.1 in
TNd^fl^ulverii-
lent pale yellow
precipitate indi-
cates presence of J^JJj
phosphoric acid '
2d Pabt.
Add Fe,Cl« and
sodic acetate.
Warm gently and filter.
Prbcipitatk.
Fe,0,.P,0,=FePO..
White powder. Indicates
the presence of phosphoric
Rbbidus
Consisttf of oxalates. Wash dry and
ig:nite. Dissolve in dilate Ha. lEffer
vescence of CO, indicates the pres-
ence of phosphoric acid.
FtLTRATB
Will contain Ba, Sr, Ca, Mg.
Test according to Groop IV.
I"
two
id/9.
Dis-
arm
Add
and
lake
pre-
s a
hro-
[rate
nith
Ball,
add
»fil.
then
hich
the
presence of
Mn by a pre-
cipitate
MnS.xH.O.
(See $ «98-)
ad. 0. Fuse
on Pt foil with
NaNO, and
Na,CO,. If
green, Mn ie
present. (f*ee
S 811.) Dis-
solve resldne
in H,0 and
filter.
Solution.
Cr, Mn, Zn.
Add acetic acid and divide.
(^ Ut Haif,
Add jriunbic ace-
tate ; I^^W precipi-
tate i^^^p)«. (See
last pHM S16.)
td Half.
Add alcohol ; boil :{
filter if necesnary ;
then add H^S; a pre-
cipitate is ZnS.HaO.
(See § 22ti.)
Rbsiditv.
Mn, Fe, Zn.
Dissolve iir HCl. Add KOH in excess,
add to filtrate H,8; a precipitate is
,0. (See 8 236.)
w
,\ ▼This
filtrate may be tested for any of the
'metals of this Group.
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THE CHEMISTS' MANUAL:
GROUP IV.
«
. *
145^
SCHEME FO^IJETECTING
Ba, Sr, Ca, Mg. •
Add to filtrate from Group III (after testing with NH4HS),
NH4CI+ NH4OH +(NH4)2C03 ; a precipitate is prodoeed ; filter
and wash. *
^^o precipitate is produced, pass on to Group Y.
PRBdPrrATB.
Filtrate.
BaCO, + SrCO, + CaCO,.
Mj
DiflBolve in HCl ; add M>dic acetate.
Add NaHPO^ ; a
then KjCftO, ; a yellow pfrecipitate
iflprodnoed; filter.
(P04),.7H,0. (Sa
Prrtipitatb.
FiLTIL
BaCrO^ (See § 321.)
Add to a portion
an#wait ten minal
forms. Add to the remaining portion
K^SO^; a predpitate is prodaoed;
filter and wash thoroughly.
PRBCnETTATO.
Filtrate. ^
Ad^NH^OH and oxalic Kd; a
whiArecipitate is CaCsO^. (See
§§33^346,342.) ^
SrSO^. (See §§331, 835.)
GROl
IP V. •
SCHEME
FOF
I DETECTING
®
NH3, K, Na.
* Divide a portion of the original solution in two
First Part. « Second Part.
Add KOH and boil: test aonia has been found in "First '
HCl ; smeU, and try test-pftp vaporate to dryness the " Sec- ^
tjip
§376.)
Test also with Nessler's
(See §378.)
10
rt" to expel
as salts). DissoJ
; add HCl, then
forms ; filter ani
#
•
all ami]^^^
oogle
$
< ^
,146
«
HE CHEMISTS' MANUAL.
Precipitate.
^KagtCl«. (See §365.) Test as in
f
§368.
Filtrate.
Evaporate filtrate to drTness; the
presence of red circular crystals indi-
^ ^^cates the presence of Na. Add alco-
^hft, and test by flame. (See § 375.)
May also test with K,0.Sb,0j.7H,0.
(See § 373.)
g>
INSOLUBLE SUBSTANCES.
^SCHEME FOR THEIR DETECTION. ^
licates, BaSO*, PbSO^, SrSO^, SnOj, CrOg.
•
,x bead — green =Cr203. Fuse part of insoluble
bh NajCOa ^^ charcoal with reducing flame, then
bright silver coin when cold, and moisten with
Jl black spot on silver, after standing, indicates
ash the fused mass a little, then grind to a powder,
and carefully look for metallic scale8=Pb^04). Boil original
substance with NH4C2H3O2, and filter ai^wash.
i
^LUTION.
^Contains the Pb(S04 ?).
•
•
Vbsidub.
Fuse some with Na^Co, on char-
coal; metallic gl<^ule— Sn. Black
spot on silver coi]fcBaS04 + SrS04.
Fuse some of residue on Pt foil with
Na.CO, ; boil with water and filter.
"-"' moN.
RKsrouE.
HCl ; evaporate to
with HCl ; dissolve
Dissolve in HCl ; evaporate to dry-
ness; moisten with HCl; dieeolve in
H,0 and filter.
Residue.
Solution.
Residue. «^
Test for HgSO^ Test for SnO,
with BaCl,. with phosphorous
bead.
Ba,Sr. Testae-
cording to Group
IV.
Test for SiO,
with pIiifMphorouB
bead.
Digiti
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t
THE CHEMISTS' MANUAL.
14T
DETECTION OF THE INORGANIC AND ORGANIC
ACIDS JN SUBSTANCE^ SOLU0E IN WATER.
^ SULPHURIC ACID (H2SO4).
Add baric chloride to a portion of the original solution [if
Pb.Ag. or Hg2 salt have been found, add Ba(N03)2], which, if
acid, first make neutral or slightly alkaline with NH^OH. If
a pnecipitate fdi-nis, add HCl ; if it does not dissolve, sulphuric
acid (HfBO^) is present.
H2S04 + BaCl2=Ba604+2HCl.
To detect free H2SO4 in presence of a sulphate, mh^roe
fluid under examination with a very little cane-sug^^nd
evaporate to dryness at 212° F. If free H2SO4 wailprSHT, a
black residue remains, or in the case of most mini^p quan-
tities, a blackish-green residue. Other ^oee acids do not de-
compose cane-sugar in this way. — (Rtjnge.)
Hydrochloric (HCl); Hydrobromio (HBr); Hydriodic (HI);
Hydrocyanic (HCN) ; Hydroferrocyanic (H4Fe"Cy<^HY-
DROFERRiCYANic [Hg(Fe2)^Cy,2]; and Sulphur. ^^k
Add to a portion of the origins^^solution argentic mtrate
(AgNOg) ; there will be precipitated :
;^l-^AgBr-|-Agl -f AgCy-f Ag4FeCyg-hAgcF5!yi2-
Observe the color of the precypitate :
AgCl, AgBr, AgCy, Ag4FeCyc are white precipii
Agl is a yellow precipitate,
AggFe2Cyi2 is a hrownhh-red j^recipitate.
Add HNO3 to the precipitate and shake it; if it does not
dissolve, one or all of the above acids may be present. If the
precipitate is blackish, this points to hydrosulphuric acid or a
soluble metallic sulpfcidc^Wphur may easily be detecte^|^
testing a fresh solution ^^^^B304. ^^^^
If hydrosulphuric acid ^^Hgnt in the solutioti to ^^^ted,
DigrHPSy *
Google
t
148 THE CHEMISTS' MANUAL.
it must first be removed by boiling. Alkaline sulphides must
be removed by a is^tallic salt^ such as will not precipitate
any of the other JRs, or at least will not precipitate them
from acid solutions. ^
Hydriodio aoid (HI) and hydbooyanio Acm (HCN), in the
presence of hydrochloric or hydrobromic acid, may be detected,
viz. : The hydbiodio ach) solution is mixed with some thin
clear starch-paste, then made distinctly acid with dilute H2SO4
or HCl, and a drop or two of a concentrated'solution ofjj>otassic
nitrate (KNO2) is then added, when the starch iodide^ blue
col^ makes its appearance ; if the hydriodic acid present is
v^^dilute, the fluid turns reddish instead of blue. This re-
acU^fe^ more delicate when the solution is quite cold.
^^^HYi^BocYAi^io Aom solutiou (or the solution containing
it) is mfced with ferrous sulphate, which has been exposed to
the air lor a while ; ^en potassic hydrate is added, when a
bluish-green precipilme forms, which consists of prussian blue
and ferric hydrate. Heat, then add HCl, when the hydrate
will dissolve and leave prussian blue undissolved. If hydro-
cyai^^cid is present in only minute quantities, the fluid
sim^^ftppears green afl;er adding HCl, and it is only after
longl^mding that a smalL:precipitate falls.
For the detection of hydbochlobio and hydeobbomig acid,
hydrocyani|fc,nd hydriodic acid must be removed. All the
radicals present in the solution to be tested must be con-
verte^Jnto silver salts and ignited. The argentic cyanide
wy^^^Wpy be decomposed, leaving the aigentic chloride,
bi^^^^Bnd iodide imaltered. The residue is then fused
wi^^^P&Oa + KgO, then boiled with HgO; sodic and potas-
sic chloride, bromide, and iodide are then in solution ; or
the fused silver salts may be easily decomposed by means
of zinc and H2SO4, and the whole allowed to stand for some
time. The solution, containing the soluble zincic chloride,
l]fl|pide, or iodide, is filtered o||^^n the metallic silver. If
to tb||^xed sodic or zincic ^^^H solution of one part of
cuprflHphate and two and a ffll^^arts of ferrous sulphate
#
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THE CHEMISTS' MANUAL. 149
be added, the sodic or zincic iodide will be decomposed and
cuprous iodide (Cu2i2) will be precipit^|;ed as a dirty-white
precipitate. The'addition of a little ammonic hydrate helps
the complete precipitation.
From HTDBOBBOikao Acm, hydriodic acid is separated most
accurately by palladious chloride, which only precipitates the
hydriodic acid as palladious iodide. From hydrochloric it is
separated by palladious nitrate.
Htdrobbomic acid, in presence of hydriodic acid and hydro-
chloric acid, may be detected, viz. : " Mix the fluid with a few
drops of dilute H2SO4, then with some starch-paste, and add a
little red fuming nitric acid or, better still, a solution of hypo-
nitric acid in sulphuric acid, whereupon the iodine r^|Jion
will show itself immediately. Add now chlorine wate^Trop
by drop, until that reaction has disappeared; and then add
some more chlorine water to set the bromine also free, which
may then be separated and identified," viz. : The substance to
be examined is placed in a test-tube, and a little carbonic di-
sulphide or chloroform is added, which gathers as a globule at
the bottom ; dilute chlorine water is then added drop b;;^rop,
the whole being agitated. When bromine is present Ir con-
siderable quantities {e. y., 1 of bromine to 1000 of water), the
globule acquires a reddish-yellow color; with very minute
quantities {e. g.^ 1 of bromine to 30,000 of water), it still has a
perceptible pale-yellow tint.
ihe^TOci]
HYDROCHLORIC ACID.
Hydrochloric add may be said to be present wl^^Here
traces of iodine and bromine have been found ; if the^Kcipi-
tate by argentic nitrate is quite large, and is not soluble in
nitric acid.
METALLIC CHLORIDE.
Metallic chlorides are detected in the presence of metallic
bromides, viz. : The metaUtauchlorides and bromides are trit-
urated with potassic chroiSfc, the mixture treated yqA^ sul-
phuric acid in a tubulated retort, and a gentle heat applied ;
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150 THE CHEMISTS' MANUAL.
a deep brownish-red gas is evolved, which condenses into a
fluid, and passes over into the receiver. If this distillate is
mixed with amnionic hydrate in excess, if a metallic chloride
is present, a yellow tint is imparted to the liquid by the am-
monic chromate which forms ; upon the addition of an acid,
the color of the solution changes to a reddish-yellow, owing to
the formation of anunonic dichromate. In the case of a metal-
lic bromide, the distillate does not turn yellow, but becomes
colorless upon supersaturation with ammonic hydrate.
NITRIC ACID (HNO3).
If ferrous sulphate is added very carefully to a solution con-
tainA^ a nitrate (with the same volume of pure sulphuric acid
as the nitrate), so that the fluids do not mix, the stratum,
where the two fluids are in contact, shows a purple, afterward
a brown, or in cases where only minute quantities of nitric
acid are present, a reddish color. If the fluids are mixed, a
clear brownish-purple liquid is obtained.
^ CHLORIC ACID (HCIO3).
When sulphuric acid is poured into a solution containing a
chlorate (as, for example, potassic chlorate), there will be pro-
duced potassic perchlorate (KCIO4), potassic hydrosulphate
(KHSO4) ; and a bright yellow gas, perchloric oxide (CI2O4), is
evolved :
;;i03 + 2H2S04=KC104+2KHS04+H20 + cCor-
has an aromatic odor, and colors the solution yel-
low, ^f the solution be heated (which should be done with
only a small quantity, and with a great deal of care), a crack-
ing sound occurs.
PHOSPHORIC ACID (H3PO4).
Add to the solution supposed^p contain phosphoric acid,
amm<^ic hydrate in excess, thenlmmonic chloride, and then
magnesic sulphate ; there will be precipitated ammonio-mag-
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THE CHEMISTS' MANUAL. 151
nesian phosphate (NH4)2Mg2P208. The precipitate is white,
and if kept in a warm place (not too hot) it subsides quickly.
If a solution containing phosphoric acid be added drop by
drop to a solution of ammonic niolybdate in nitric acid, there
is formed in the cold, either immediately or after the lapse of
some time, a pulverulent pale-yellow precipitate^ which gathers
on the sides and bottom of the tube. If the phosphoric acid
is only present in quantity (0.0002 grm.), it is necessary to
heat gently (not above 100° F.), and to wait a few hours. j
OXALIC ACID (C2H2O4).— HYDROFLUORIC ACID (HF).
Add ammonic hydrate, then calcic chloride ; if a precipitate
is produced, add acetic acid ; if not dissolved, test a portion of
the original solution by adding some finely-pulverized man-
ganese dioxide and a few drops of sulphuric acid for oxalic
ACID. If present, a lively eflfervescence ensues, caused by
escaping carbonic oxide :
Mn02 + C2H204 + H2S04=MnS04 + 2Cd^-|-2H20.
Test another portion of the original substance for htdroflf-
ORic ACID. Mix together the substance to be tested with sul-
phuric acid (so that a thin paste is made) in a platinum
crucible, and cover with a watch-glass which has been coated
on the convex side with bees-wax, and a few marks made
with a pin through the wax to the glass ; fill the concave side
with water, and heat the crucible gently for an hour or so,
when the marks made by the pin will be etched into Uie glass
by the action of the hydrofluoric acid evolved, and the marks
will not be removed by washing.
BORACIC ACID (H3BO3).
Add to a portion of the original solution, hydrochloric acid
until distinct acid reaction ; then dip a slip of turmeric paper
in the solution ; then dry the paper at 112° F., when, if boracic
acid was present, the paper will show a peculiar red tint
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152 THE CHEMISTS' MANUAL.
(H. Rose). If this peculiar red-tinted paper be moistened
with an alkali or alkaline carbonate, its color passes into
bluish or greenish-black. Hydrochloric acid restores the red
tint (A. Vogel; H. Ludwig). Malvern W. lies, Ph.B., has
discovered what may be called the most reliable test for
boracic acid and borates known. It consists in simply dipping
a platinum-wire in glycerine, then into the finely-powdered
substance, and then holding the same in a gas flame, when the
flame will be colored green. By this method boracic acid has
been detected in substances when, by all other tests, its pres-
ence could not be demonstrated.
SILICIC ACID {H^S\0^).
This acid has probably been found already. Evaporate
some of original substance with hydrochloric acid to dryness ;
moisten with hydrochloric acid, and dissolve in water. If
Si02 remains, silicic acid is present. (Phosphorous bead.)
CHROMIC ACID (H2Cr04).
The yellow or red color of the original solution, or the
purple-red color of the precipitate produced by argentic
nitrate, points to the presence of chromic acid. If there re-
mains any doubt, add plumbic acetate to a portion of the
original solution acidified with acetic acid, when basic plumbic
chromate will be precipitated (Pb2Cr05=2PbO.Cr03).
ORGANIC ACIDS.
Before testing for organic acid, remove, first, Group I, II,
III, according to Scheme, as their presence might disturb the
reactions.
Make a portion of the fluid from which Group I, II, III
have been removed slightly alkaline by adding NH^OH ; add
some NH4CI, then CaCl, and shake vigorously, and let the
mixture stand at rest for some minutes (ten to twenty).
A precipitate forms ; filter.
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THE CHEMISTS' MANUAL.
163
FUOIFITATE.
Digeet and ehake the pre-
cipitate with NaHO; dilute
with water ; filter, and boil fil-
trate for some time. If a pre-
cipitate separates, tabtabic
ACiD(C«H«Os) maybe aAvnmed
to be present. Pour over the
precipitated calcic tartrate
NH«6h in a test-tube, then
add AgNOs, and heat, when
pulverulent metallic silver
will sepante.
PBBCIFITATB. FfLTBATS.
Calcic cit- Add alcohol
trate dissolve again, which
in HCl: add vRll precipi-
NH«OH, and tate calcic
boil ; if calcic malate ; dis-
cltrate is pre- solve in acetic
cipitated acid ; add al-
again, Cit- cohol, and
BIO ACID filter if neces-
(C.H.O,) is ' pary. The
present. ; filtrate is pre-
, cipitated with
— ' plumbic ace-
tate, and neutralized with ammonic hydrate; wash precip-
itate; stir In water decomposed by H,S, and evaporate ,
filtrate to dryness. |
The malic acid thus obtainedMf heated in a glass tube, is {
converted Into makie add (C«H«0«), which will condense
to crystals in the colder part of the tube. This indicates
the presence of malic acid (C«H«0,). '
FiLTBATB.
Add some more calcic chloride, then add alcohoL
cipitate forms ; filter.
FiLTBATB.
Apre-
Pbbcifitatb.
Wash with some alcohol,
dissolve on filter with HCl ;
add NH«OH to feeble alka-
line reaction, and boU for
some time. A heavv white
precipitate forms ; filter.
Heat to expel alcohol, neu-
tralice exactly with HCl, and
addFe.Cl«. If a light-brown
flocculent precipitate is pro-
duced, filter, digest, and
heat.the washed precipitate
witV NH.OH in excess;
filter, evaporate filtrate near-
ly to dryness, and divide in
halves.
1st
Add alcohol
and baric
chloride; a
white precipi-
tate will con-
sist of baric
succinate,
BaC«H,0„
which indi-
cates the pres-
ence of SDC-
citrio acid
(C.H,OJ.
3d halt.
Add hydro-
chloric acid,
when BKN-
20IC acid
(CH.O.) will
be precipi-
tated as a dax-
aliug white
sparkling
powder.
" Benzoic acid
may generally
be detected
by pouring a
little hydro-
chloric acid
over the orig-
inal solution, when the benzoic acid vrill remain undissolved ; if this be heated on a
platinum-foil, it will fhse. and afterward volatilize completely. The fhmes of benzoic
acid cause a peculiar irritating sensation in the throat ana provoke coughing : when cau-
tSonsly cooled, they condense to brilliant needles ; when kindled, they burn with a lumin-
ouB sooty flame.^*
ACETIC ACID (C2H4O2).
Introduce a portion of the original solution in a Bmall
tube, pour some alcohol over it, add about an equal volume
of sulphuric acid, and heat to boiling. Evolution of the odor
of acetic acid demonstrates its presence, increased by shaking.
FORMIC ACID (CH2O2).
When neither chromic or tartaric acid have been found, add
to solution argentic nitrate in excess the sodic hydrate until
the fluid is exactly neutralized, and boil.
If formic acid is present, the argentic formiate which was
produced is decomposed and metallic silver precipitated
If chromic and tartaric acid have been found, mix the orig-
inal solution with some nitric acid ; add plumbic oxide in ex-
cess ; shake the mixture ; filter ; add to the filtrate dilute sul-
phuric acid in excess, and distil. Add to the distillate ferric
oxide (FegOa), ^^^^ ^h© A^^id will become a blood-red color,
owing to the formation of a soluble neutral salt.
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154
A COMPLETE TABLE OF
BY JAMES
(OLD SYSTEM OF
NAXS.
Salts Of Potash,
Soda, • - . .
Lithia, . . . .
earyta.
No precipitate.
No precipitate.
No precipitate.
A volaminoas
precipitate, eola-
' Die in a large
I quantity of wa-
' ler.
Strontia, •
time, - •
•Magnesia,
Alumina, •
Clucina, -
Thoria,
Yttria,
Zirconia, •
Cerium,
(Protoxide,
Peroxide)
No precipitate
unless left for
some days.
Same as Stron-
tla.
▲ bulky preci-
pitate complete-
ly soluble in Mu-
riate of Ammo-
nia.
A wliite preci-
f>ftate, insoluble
n Muriate of
Ammonia in ex-
cept, but soluble
in Potash.
A white precl-
{titate, insoluble
n excess and in
Muriate or Am-
monia.
A eelatinons
precipitate, in-
soluble inexcess.
A white, volu-
minous precipi-
tate, Id soluble in
excess.
A white preci-
gitate, insoluble
1 excess.
A white preci-
pitate, turning
Drown, insoluble
in excess. j
OABBONATB OF
POTASH.
The same.
Same as Bary-
ta: not quite so
soluble.
The same, not
quite so soluble.
A white preci-
pitate, insoluble
m excess; solu-
ble in Muriate of
Ammonia.
A precipitate
sohible in ex-
cess, insoluble
in Muriate of
Ammonia.
A precipitate
completely solu-
ble in excess.
The same.
The same.
The same, per-
fectly Insoluble
In excess.
The same.
No immediate
precipitate, bat
after a time a
granular one.
A white preci-
pitate, soluble
with, etrervesces
in free acids.
Same as Baryta.
The same as
Baryta & Stron-
tia.
A white precl-
Sitate, BoluDle In
Luriate of Am-
monia.
A white preci-
pitate, soluble in
caustic potash.
A precipitate,
soluble in a great
excesB of preci-
pitant.
A white preci-
pitate, soluble in
excess.
A white preci-
pitate, slightly
soluble in a great
excess.
A white preci-
pitate, slightly
soluble in a great
excess.
A white preci-
pit,ate, slightly
soluble In ex-
BICARBONATl
OF POTASH.
The same.
The
Same aa Baryta.
The same.
No precipitate
unless solution
Is boiled, then a
strong one.
The same ; Car*
t>onic Acid gaa
la disengaged.
The
The
The same, com-
pletely soluble In
a great excess.
The same.
The
Digiti
ized by Google
/ •
i >
ANALYTICAL CHEMISTRY.
156
HAYWOOD.
NOMENCLATU RE.)
CABBOHATB OF
AnONIA.
BUI^FHUBETTSD HTDBOBULPRATB TXLLOW PBUB8X- BID F11UB8IATE
HTDBOGIN. OF AJOfOHIA. ATB OF POTASH. OF POTASH.
No precipitate.
Tbei
The same.
The same.
Seme as the Bi-
carbonate of Pot-
ash, eoloble in
Muriate of Am-
monia.
The same.
A white prcci-
pStoie, Bohible in
<ezce8s.
The I
Thefl
The same, nore
«s»U7 Bolnble in
excess.
The same.
No precipitate.
No precipitate.
No precipitate.
No precipitate.
No precipitate.
No precipitate
in any eolation.
No precipitate.
No precipitate.
No precipitate.
No precipitate.
No precipitate.
No precipitate if
the test is pure.
A white precipi-
tate of Alumina,
soluble in Potash.
A white precipl-
tate,soluble in Pot-
ash.
A white precipi-
tate of Thoria.
A precipitate
fttria.
of
A TohiminooB
precipitate.
A white precipi-
tate of Protoxide.
No precipitate.
No precipitate.
A white, heavy
precipitate, solu-
Die in acids.
A white preci-
plUte.
A white preci-
pitate.
A white preci-
pitate.
No precipiute.
No precipitate.
No precipitate.
No precipitate.
No precipitate.
Digiti
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156
A COMPLETE TABLE OF
BY JAMES
(OLD SYSTEM OF
SalU Of Potash, •
Soda,
Lithla,
BtryU, .
Strontit, •
Lime,
MagnesU,
Alumina, •
Gluclna, -
Thoria,
Yttria,
Zirconia,
Cerium,
(Protoxide,
Peroxide)
OXAUO AOID.
No precipitate
No precipitate
UDleftg left for
some days.
A troubling in
BtTODjr solutions;
if Ammonia be
added, a precipi-
tate.
An immediate
precipitate, sola-
ble in Nitric or
Muriatic Acid.
No precipitate
unless Ammonia
be added.
No precipitate.
No precipitate.
A white preci-
titate, Insoluble
exceed.
El'
A white preci>
Sitate, soluble in
[nriatic Acid.
A white precip-
itate, soluble In
a preat excess or
in Muriatic Acid.
A white precip-
itat«,eveninacid
solutions; spar-
in(;ly solnble in
Muriatic Acid.
IODIDE OF
FOTASaiUK.
No precipitate.
BULFHATS OF
POTASH.
A wliite preci-
pitate, if Ammo-
nia be added.
A Toluminous,
white precipi-
tate, insoluble in
strong acids.
The same as
Baryta ; rather
more soluble in
water.
No precipitate
in dilute solu-
tions, but a white
one if strong.
No precipitate.
After a time
crystals of Alum
are formed.
No crystals are
formed.
Thrown down
as a double salt,
insoluble in ex-
After a time a
precipitate is
formed, but is
easy soluble in
an excess.
A white preci-
pitate. %lmo8t in-
soluble in water
and acids.
After a time a
precipitate, in-
soluble in ex-
FHOePHATB OF
SODA.
No precipitate;
but if Ammo-
nia be added, a
strong one.
A white preci-
uitate, soluble in
nee acids.
Same as Baryta.
SameasBaiTta.
A white precipi-
tate, particularly
if Ammonia be
added.
A white precipi-
tate, soluble io
Acids or Potash.
A voluminous
precipitate.
A white, flaky
precipitate.
A white pre-
cipitate, soluble
in acids, but is
again precipita-
ted by boiling.
A voluminoua
precipitate.
Awhitepiedpi-
Ute.
Digiti
ized by Google
ANALYTICAL CHEMISTRY.
HAYWOOD.
NOMENC];.A.TURE )
16T
BIFOBE TUB BLOWPiPB.
On Platinum wire tingOB
oat«r flame Tiolet : with Bo-
rax and Oxide of Nickel, a
blue bead.
The bead of Nickel and Bo-
rax is not changed by Soda ;
heated on Platinum wire
tinges outer flame yellow.
TiDfceB OQter flame of a car-
mine color ; the doable phoe-
pbate is fluible.
Cannot easily be dlstin-
gnlshed : the Cnloride tinges
onter flame greenish ; Invisi-
ble alone; Visible with flaxes.
Tinges outer flame carmine
red wnen heated on Platinum
wire.
Same as Stroutia, only not
so bright: gives a powerltd
white light when strongly
heated.
When a salt of Magnesia,
that has been heated, !» mois-
tened with Nitrate of Cobalt,
it acquires a pale red color.
Treated as the above on
Charcoal, a fine blue color is
communicated to the assay.
When moistened with Ni-
trate of Cobalt, becomes dark
gray, or nearly black.
Not easily distinguished:
produces a colorless bead
with Borax.
Yttria behaves in the same
manner as Oluclna.
Obnnot easily be distin-
guished ftom similar sub-
stances.
OBSKBTAnOBS.
Give a white precipitate with Tartaric Acid,
a yellow one with CVilorlde of Platinum, and
a gelatinous one with Hydroflnosilicic Acid,
which distinguishes it from other substances.
Gives no precipitate with Tartaric Acid, or
Chloride of Platinum, by which it may be ais-
tinguiflhed.
No precipitate with Chloride of Platinum ;
can easily oe distinguished from the former.
Basily distinguished by forming a white
precipitate with Sulphates and Carbonates.
The Chloride is insoluble In Alcohol.
Distinguished from Baryta by criving a pre-
cipitate with Hydroflnosilicic Acid, and by the
filtered liquid of the still Alkaline Sulphate
giving a precipitate with fiazyta water.
Distinguished firom Baryta and Strontla by
giving no precipitate with Sulj)hates when
diluted ; separated in the state of Nitrates and
C*hlorldes by Alcohol.
Easily distinguished and separated by Sul-
phates from the above, or by tne precipitates
being all soluble in Muriate of Ammonia.
Distingnished from the Alkalies by giving a
white precipitate with Ammonia. andmay be
separated irom most other suDstances by
Caustic Potash.
May be distingnlphed from Alumina by the
Carbonates, from Magnesia by being insolu-
ble in Muriate of Ammonia, and from Lime
and the Alkalies by Ammonia.
Thorla maybe distinguished and separated
from the above substances, as it is perfectly
insoluble after Ignition In all acids except the
Sulphuric.
Distinguished from Thorla by Sulphate of
Potash, and from the other subi*tances de-
scribed by the same means as Thorla.
Distinguished from Thorla by Sulphate of
Potash and Oxalic Acid, and from Yttria by
its Oxide, after ifrnition, being insolable in
all Acids except the Sulphuric.
Converted to Peroxide, sol- Distinguished from other substances pre-
uble in Borax, producing a viously cTescribed by tuming Into a red Per-
red bead ; color flies on cool- oxide when heated in contact with the atmos-
Ing. phere.
Digiti
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158
A COMPLETE TABLE OP
NAXS.
AJOIOMIA.
POTASH.
POTASH.
BICARBONATE
OF POTASH.
Manganese, - - -
(Protoxide)
A white preci-
pitate, solnble in
Muriate of Am-
monia, turning
brown at the 8ur-
Ikce.
A precipitate,
turning brown,
insoluble in Mu-
riate of Ammo-
nia.
white precipi-
Ute, slightly sol-
uble in Muriate
of Ammonia.
The same, im«
less Tery dUute.
Manganese,- - -
(Sesqoioxlde
and
Peroxide)
A dark-brown
precipitate, in-
soluble in Muri-
ate of Ammonia.
The same.
A brown, volu-
Ute.
The same.
Zinc.
A white, gelat-
inous precipi-
tate, Boluble in
excess.
The same as
Ammonia.
A white preci-
pitate, insoluble
in excess, but
soluble In lluri-
ate of Ammonia
or Caustic Alka-
lies.
A white preci-
piUte, which be-
haves in the
same manner.
Cobalt, - - - .
(Protoxide
or
Peroxide)
A blue precipi-
tate, soluble in
excess, forming
a greenish so-
lution, turning
brown.
A blue preci-
pitate, insoluble,
turning green
and pale, red
when boiled.
A red precipi-
tate, which boU-
ing renders blue.
A red precipi-
Ute.
Hickel,
(Protoxide
and
Peroxide)
A slight green
troubling, then a
clear, blue solu-
tion, precipitate
green by Potash.
An apple-green
preciuitate, in-
soluble in ex-
cess.
A light-green
precipitate.
The same; Oar-
bonic Acid gaa
is given off.
Iron,
(Protoxide)
pitate, soluble in
Muriate of Am-
monia, turning
brown in contact
with the air.
A green preci-
piute, insoluble
in excess, turn-
ing brown at the
Burf^tce.
A white preci-
pitate, soluble in
Muriate of Am-
monia.
.
The same.
Iron,
(Sesqnioxide
and
Peroxide)
A reddish-
brown precipi-
tate, insoluble in
Muriate of Am-
monia.
The same.
A light-brown
precipitate.
The same : Car-
bonic Acid is dis-
engaged.
Cadmium, - - -
A white preci-
pitate, soluble in
a slight excess.
A white preci-
pitate, insoluble
in excess.
A white preci-
pitate, insoluble
in excess.
A white preci-
pitate: Carbonic
Acid is disen-
gaged.
Lead, - - - - •
(Protoxide
Peroxide)
A white preci-
pitate, insoluble
in an excess, ex-
cept with Ace-
tates.
A white preci-
pitate, soluble in
a great excess.
A white preci-
pitate, insoluble
in excess, but
soluble in Pot-
ash.
A similar preci-
pitate with an
evolution of gas.
Bismuth, • • - -
A white preci-
pitate, insoluble
!n excess.
The same.
The same.
The same.
(Deatoxide)
pitate and deep
purple solution ;
again precipi-
tated by Potash
if boiled.
A green preci-
pitate, which
Boiling renders
black
A green preci-
pitate, which
boiling rendera
black.
A light-green
precipitate, solu-
ble in excess.
Digiti
ized by Google
ANALYTICAL CHEMISTRY.
159
CAKBONATS OF
▲JIMONIA.
TlieHune.
The I
A white preci-
pitate, eolable in
A red precipi-
tate, eolable in
Mariate of Am-
monia.
A green preci-
pitate, eolnole in
ezce^c, forming a
blnidh solution.
The flune.
A Hgbt-brown
piecipitate.
A white preci-
Eitate, infoluble
lexoese.
Tbei
Thei
A green preci'
pitate, eolnole in
esceM, sa
Ammonia.
SULPHTBKTTED
HYDBOOSN.
No precipitate
nnle(f>8 Ammonia
be added.
A milk-white
precipitate of
Solphnr ; solu-
tion then con-
tains a Proto-
salt
A white preci-
pitate if nentral,
bat none if acid.
No precipitate;
solntion tarns
darker.
No precipitate;
solution tarns
darker.
No precipitate.
A milkr-wtiite
precipitate of
sulphur ; solu-
tion then con-
tains Protoxide.
A jellow preci-
pitate.
A black preci-
piUte, in both
neutral and acid
solutions.
A black preci-
pitate, in both
neutral and acid
solutions.
A black or dark-
brown precipi-
tate, in both neu-
tral and acid so-
lations.
HTDROSITLFHATE
or AXJCONIA.
A flesh-red pre-
cipitate, turning
brownish in con-
tact with the air.
The flesh-red pre-
cipitate ; the precl-
ftitate by Ammonia
a turned flesh-red
by it.
A white precipi-
tate, insoluble in
excess.
A black precipi-
tate, insoluble in
excess.
A black precipi-
tate, slightJy sol-
uble in excess.
A black precipi-
tate,tumingbrown
at the Burfhce.
A black precipi-
tate, same as Pro;>
toxide.
A yellowish pre-
cipitate, insoluble
in excess.
A black precipi-
tate, insoluble in
excess.
A black precipi-
tate, insoluble in
excess.
The same ; insol-
uble in excess.
TSLLOW PBUSSZ-
▲TE OF POTASH.
A pale-red pre-
cipitate, soluble
in tree acids.
A grayish-green
precipitate.
A gelatinous,
white precipi-
tate, insoluble in
Muriatic Acid.
A green preci'
to t '
gray, ini
ID Muriatic Acid.
pitaU
turning
insoluble
A white preci-
pitate, slightly
tending to green,
insoluble in Mu-
riatic Acid.
A light-blue
f)recinitate, tuni-
ng darker, in-
»oTuble in Muri-
atic Acid.
An immediate
dark-blue precl-
Eitate, insoluble
1 Muriatic Acid.
A slightly yel-
low precipitate,
soluble in Muri-
atic Acid.
A white preci-
pitate.
A white preci-
Sltate, polnole in
[uriatic Acid.
A r e d d i s fa-
brown precipi-
tate, inpoluble in
Muriatic Acid.
BED FRUSSZATB
OF POTASH.
A brown preci-
Eitate, insoluble
1 Aree a<.*.ids.
The same aa
the Protoxide.
A yellowish-red
Ereciiiitate, solu-
le in Muriatic
Acid.
A reddish-
brown precipi-
tate, insoluble in
Muriatic Acid.
A yellowish-
green precipitate,
in soluble in Mu-
riatic Acid.
An immediate
dark-blue preci-
Eitate, insoluble
1 Adds.
No precipitate.
A yellow preci-
Sitate, soluble in
[uriatic Acid.
No precipitate.
A pale-yeHow
precipitate, sol-
uble in Muriatic
Acid.
A yellowish-
green precipitate,
Insoluble in Mu-
riatic Acid.
Digiti
ized by Google
160
A COMPLETE TABLE OF
Manganese, - - -
(Protoxide)
Manganese, - - -
^Sesquioxide
and
Peroxide)
Zinc,
Cobalt,
(Protoxide
or
Peroxide)
Nickel,-
(Protoxide
and
Peroxide)
Iron,
(Protoxide)
Iron,
(Sesqaioxlde
and
Peroxide)
Cadmium, -
Lead,
(Protoxide,
Peroxide)
Bismuth, •
Copper,
(Deatozide)
OXAUO AOID.
A white cry*-
talline deposit,
unless very di-
lute.
No precipitate,
but the Bolntlon
is soon rendered
colorless.
A white preci-
pitate, sola Die in
free Acids and
Alkalies.
A slight troub-
ling and shortly
a pale-red preci-
pitate.
No immediate
precipitate, but
a slow deposit
A yeUow color,
and shortly a
precipitate.
No precipitate ;
solution turns
yellowish.
An immediate
precipitate, solu-
ble in Ammonia.
An immediate,
white precipi-
tate.
IODIDE OF
FOTASaiUK.
No precipitate.
No precipitate.
A yellow preci-
pitate, soluble In
a great excess.
No immediate Abrownpred-
precipitate, but i pltate, soluble in
after a time a excess,
granular one.
A greenish pre-
cipitate.
A white preci-
pitate, soluble in
a great excess.
8ULPHATV OF
FOTA8B.
No precipitate.
No piedpitate.
No predpltaie.
No precipitate.
No precipitate.
A white preci-
pitate, very in-
soluble.
No precipitate
except from the
water of solu-
tion.
No precipitate.
FHOSFSATB OF
SODA.
A permanent,
white predpl
tate.
A brown preci-
pitate in neutral
eolutlona.
A white prod-
ultate, soluble In
firee Acids and
Alkalies.
A bine precipi-
tate.
A white precipi-
tate, slightly ten-
ding to green.
A white preci-
pitate, tnming
green.
A white precipi-
tate, which Am-
monia turns
brown, and at
length dissolves.
A white preci-
pitate.
A white precipi-
tate, soluble in
Potash.
A white preci-
pitate.
A greenlsb-
whlte preclpitatei,
soluble in Am-
monia.
Digiti
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ANALYTICAL CHEMISTRY.
161
nTALUOORO.
No precipitate.
b precipitated
u fman metallic
Precipitates in
t crystalline me-
tallic slate.
^Precipltatee it
from the mitt^
•elation, even as
aspoDgymaBS.
^ Zinc and Iron
Vrth precipitate
metaDfc Copper
from all its lola-
BSFOSB TBM BLOWFIPI.
Prftducesa bead of an am&-
thTHt color in the outer flame
with Borax, which diaap-
peara in the Inner flame.
Same aa Protoxide.
On Charooal with Soda a
coat of white Oxide la formed;
with Nitrate of Cobalt they
aasome a green color.
The amalleat portion colon
Borax atrongly bine: reduced
to a metallic state with Soda;
magnetic.
With Borax In the outer
flame, a reddish color, which
disappears when cold; with
Soda, a white magnetic
powder.
With Borax in the onter
flame, a red bead, turning
lighter as It cools : interior
flame a green bead, turning
llc^ter on cooling.
Peroxide behaves in the
same manner; with Soda,
a magnetic powder Is ob-
tained.
Heated on Charcoal, in the
Inner flame a brownlah-red
powder sublimes.
Heated on Charcoal with
Soda, is reduced to metallic
giobnlee, which are mallea-
le; a yellow powder sub-
limes: produces clear glass
with Borax.
On Charcoal are easily re-
duced to brittle metallic glo-
bules ; a vellow oxide sub-
limes ; with Borax, a clear
glass.
Outer flame with Borax, a
fine green bead ; inner flame
dirty red ; with Soda is re-
duced.
OBaSBTATIOHB.
The reaction of these salts with Hydrosul-
phate of Ammonia is so well characterized
that they cannot be miataken.
The Peroxide is always converted into the
Deutoxide by solution in an Acid. Muriatic
Acid converts it into Protoxide by boiling.
The solution in Potash is precipitated by
Hyd. Sul. 'Am., which distinguishes it fh>m
earthy salts, and mav easily be separated
from other metals by Ammonia.
Easily distinguished from all other salts by
their behavior with Hydroeulphate of Am-
monia.
Dlstinguiehed ftom Cobalt by Ammonia and
Potash, aad from other substances in the same
way as Cobalt.
The Salts of Iron are easily distinguished
by their behavior with the Prusslates ; may
be separated from Manganese by Succinate
of Soda.
Peroxide is distinguished and separated
from Protoxide by red Prussiate of Potash
and Ammonia.
Distinguished by Sulphuretted Hydrogen,
and maya>e separated from all the above oy a
bar of Zinc.
Solutions of Lead give a precipitate with
Sulphuric Acid and sulphates, and therefore
may be distinfirnished from most other metals.
Muriatic Acid aloo precipitates Lead, but
water dissolves the precipitate.
May be detected by giving a precipitate
with water alone.
Salts of Copper can be easily distinguished
from other safta by their behavior with Am-
monia and Potash.
Digiti
ized by Google
162
A COMPLETE TABLE OP
OABBOHATB OF
POTASH.
BIOABBONATB
OF POTASH.
SUver,
Marcury, - - - -
(TOtoxide)
Mercury, - - - -
(Peroxide)
Plttint,
Gold,
Tin,
Tin,
(Protoxide)
(Peroxide)
Antimony, -
Chromium,
Vanadium, - -
Columbium, -
Iridium,
A brown preci-
pitate, vary solu-
ble in excess, bnt
is reprecipitated
by Potash.
A blaclE preci-
pitate, BolQDle in
excess.
El'
A white preci-
Itate, inoolnble
excesB.
A yellow preci-
j;>irate, Bolable in
excels, int«olable
in free acidB.
A yellow preci-
pitate.
A white preci-
Eitate, Insolable
1 excess.
A white preci-
pitate, rolaDle Id
acids and in ex-
cess.
A white preci-
f>itate, insolnble
n excess and in
Mni-iatic Acid.
Af^eenieh-blne
precipitate, in-
solDDie in ex-
A grayish-
white precipi-
tate, turning red
and dissolving.
Is readily dis-
solved, ano may
be again precipi-
tated by acids.
A brown pre-
cipitate, partly
solnble, forming
a pnrple solu-
tion.
A brown preci-
filtate, insolnble
n excess, but
solnble in Am-
monia.
A black preci-
pitate, BoluDle in
excess.
A yellow or
white precipi-
tate, soluble in
excess.
A yellow pre-
cipitate, soluble
in excess when
boiled, and again
precipitated by
acidtf.
At first no
precipitate, but
shortly a black
one.
A white preci-
pitate, solnble in
excess ; decom-
posed by boiling.
The same, sol-
nble in excess.
The sane, sol-
nble in Muriatic
Acids.
A green preci-
pitate, soluble in
excess : again
thrown down by
boiling.
The same.
The same, in-
soluble in strong
acids.
A dark-brown
precipitate.
A white preci-
pitate, soluble in
Ammonia.
A dirty yellow
precipitate,
which boiling
renders black.
A reddis fa-
brown precipi-
tate; if it con-
tains Muriate
of Ammonia, a
white one.
A yellow preci-
Eitate, insoluble
1 excess.
No precipitate.
A white precl-
Eitate, insolable
1 excess.
The same;
deposits slowly
aeain after solu-
tion.
The
A green preci-
pitate, slightly
soluble in ex-
cess.
A grayish-
white precipi-
tate, soluble in
excess.
The same, and
maybe dissolved
by Acetic Acid.
No precipitate;
color destroyed.
The same.
A white preci- \
pitate. rendered
black by boiling.
A reddish-
brown precipi-
tate, either im-
mediate or after
a time.
The same; Mn-
riatic Acid must
be added in all
cases.
No precipitate
The same.
A white preci-
Eitate, insoluble
1 excess.
The
The same; lath-
er lighter.
The same.
The same.
The
Digiti
ized by Google
ANALYTICAL CHEMISTRY.
163
CABBOHATS OF
▲nONIA.
BULPU UKBTTKD
HTDBOGKK.
HTDBOSULFHATB
or AMKOKIA.
TBI.LOW FRU88I-
ATB OF POTASH.
BXD FBUB8IATB
OF POTASH.
A white preci-
pitate, soluble in
exce««.
Amy or black
precipitate.
A white preci-
pitate.
A yellow precl-
A yellow preci-
pitate. If neutral.
Thsiame.
Thei
The
The same; ap-
;to Tio-
proaehiogt
The same, in-
soluble In excess.
The
The same.
A black precl-
plute, in both
nentml and acid
solutions.
A black preci-
pitate, in acid
and neutral solu-
tions.
A black preci-
pitate, turning
white, and again
black by an ex*
cess, soluble in
Potash.
A brown color
and shortly a
precipitate.
A black preci-
pitate, in both
acid and neutral
solutions.
A dark-brown
precipitate. In
both acid and
neutral solu-
tions.
No immediate
precipitate, but
shortly a yellow
one.
A red precipi-
tate in acid so-
lutions.
No precipitate
in any solutions.
Generally a
brown precipi-
tate, in ether,
acid: or neutral
solutions.
A dark-brown
precipitate.
A black precipi-
tate, insoluble in
excess.
A black precipi-
tate, insoluble in
excess, partly sol-
uble in FotasD.
The same; solu-
tion must be neu-
tral.
A brown precipi-
tate, soluble In a
large excess.
A brown precipi-
tate, soluble in ex-
cess.
A brown precipi-
tate, soluble in ex-
cess, reprpcipita-
ted by Muriatic
Acid.
A yellow preci-
pitate, soluble in
excess.
A red precipitate,
soluble in an ex-
cess.
A greenish preci-
pitate.
A grayish-white
precipitate.
No action with
the Acid, but a
brown precipitate
with the Oxide.
The same; solu-
ble in excess.
A white preci-
pitate.
A white, gelat-
inous precipi-
tate.
A white preci-
pitate, turning
blue.
A yellow preci-
pitate, solution
turns darker.
An emerald-
green color.
A white, gelat-
inous precipi-
tate.
No precipitate
atflrst,butshort-
]▼ the whole
forms a thick
Jelly.
A white pred-
Eltate, insoluble
1 Muriatic Acid.
No precipitate.
A reddish-
brown precipi-
tate.
A reddish-
brown precipi-
tate, turning
white.
A yellow in most
solutions. but
none with the
Perchloride.
The same.
No precipitate.
A white precl-
Eltate, soluble in
[uriatic Acid.
No precipitate.
No precipitate,
but shortly a
slight opacity.
No precipitate.
yeDowish-
1 preclpl-
No precipitate.
Digiti
ized by Google
164
A COMPLETE TABLE OF
OXAUO AOID.
IODIDE OF
FOTASBIUM.
eULPHATV OF
POTASH.
PHOSPHATE OF
80DA.
Sliver, •
Mercui
thoto
ttozlde)
Marcury.
(Peroxide)
Plttlna,
A white preci-
pitate, soluble in
Ammonia.
A white preci-
pitate.
A white preci-
{>itate, bat none
n the Perchlo-
ride.
No precipitate.
Gold,
ATellowish pre-
cipitate, soluble
in excesB.
A greenish-yel-
low precipitate,
rendered black
by an excess and
at length dis-
solves.
A line scarlet
precipitate, sol-
uble in excess
and in Muriatic
Acid.
A deep-brown
color and preci-
Kitate, which
oiling reduces.
A dark color, A dark color
and shortly the ' and a yellowish
Gold is precipi- precipitate,
tated.
A White preci- j A yellow preci-
pitate^ unless the
solution be di-
luted ; soluble in
water.
A whito preci-
pitate. /
pitate, soluble In
Ammonia.
A white preci-
pitate.
A white preci- A white preci-
pitate. pitate in most,
but not in the
Perchloride.
No precipitate.
No precipitate.
Tin,
(Protoxide)
Tin,
(Peroxide)
A white preci-
pitate.
No precipitate.
Antimony,
Chromium,
Vanadium,
Columbium,
iridium.
yellowish A white precl-
. ltate,tum- ipitate, partial.
Ing red, soluble
in excess.
preciplfa
Ing red,
No precipitate.
A white preci- The same,
pitate, caused by
water.
No precipitate. A greenish pre-
I cipitate, soluble
iu Muriatic Acid.
DissolTOS the
Oxides.
No precipitate.
The same.
No precipitate.
No precipitate.
Fused with it,
the Oxide re-
mains after boil-
ing.
No
or act
precipitate
No precipitate.
No precipitate.
A wliite preci-
pitate.
A white preci-
pitate.
The same.
A light-green
precipitate.
No precipitate
Digiti
ized by Google
ANALYTICAL CHEMISTRY.
166
UTAIXIO XOfC.
BirOBB THB BLOWFIPB.
OBBEBYATIONa.
Is precipitated
in ft metallic state.
Fonns a gray
coating, which u
an *in^igaTn-
Same as Pro-
toxide.
A black, metal-
lic powder.
A brown, bulky
coating.
Small grayish-
white spangles
of Tin.
A white Jelly;
Hydrogen gas is
Ptecipitated in
the form of a
Uack powder.
No precipitate.
Pradpltatad as
a dark powder.
With Borax in the enter
flame, a milky elSAs ; with
Soda IB easily reanced.
Heated in a glass tnbo with
a little Soda, Mercury sab-
limes and condenses in small
globnles.
Same as Protoxide.
Completely rednced, bnt
rives no color to flaxes or
Same as Platlna, insolnble
in all acids except Nitro-Ma-
riatic.
Easily reduced with Soda ;
deprives a bead of Copper
and microcosmic salt of its
green color.
Bedaced on Charcoal, forms
a white enamel with glass ;
does not dissolve easily in
Borax.
Redoced with Soda, rapidly
oxidizes and sublimes In the
outer flame as a thick, white
smoke.
A fine emerald-green bead,
both in the inner and outer
flame, with fluxes.
In the inner flame, with
Borax, a green glass, outer
becomes yellow.
Effervesces with Soda; a
dear glass with Borax, or
the Phosphoric Salt.
No action with fluxes : no
odor ; may be coupled with
lead.
Muriatic Acid throws down a white preci-
pitate, insoluble in acids, but soluble in Am-
monia, which dlBtinguishes it trom all other
substances.
Muriatic Acid gives a white precipitate,
insoluble in acids, which Ammonia renders
black, but does not dissolve ; by this it may
be distinguished.
Persalts of Mercury are easily recognised
by Sulphuretted Hydrogen and iodide of Po-
tassium.
Easily recognixed by its behavior with Pot-
ash and Ammonia ; may be separated by Mu-
riate of Potash.
Protochloride of Tin gives a deep purple
color and precipitate ; Sulphate of Irou throws
down the gold, which distinguishes it l^om
most other metals.
The behavior of these ealts with Gold, as
above, is sufficient to distinguish them.
The Peroxide is insolnble in all Acids after
ignition ; Nitric Acid oxidizes Tin, but does
uot-diseolve the Oxide.
The Oxide is volatile and insoluble in
Nitric Acid ; may be diBtinguished ttom Tin
by Sulphuretted Hydrogen ; water only pre-
cipitateB part of the Oxide.
Its solutions are usually green, and may be
diBtinguished ttom most other solutions by
Snlphnretted Hydrogen.
All its Baits have a blue color : distingulBhed
trom Iron by Hydrosulphate of Ammonia.
__ Ihsed with Csustic or Carbonated
les, the whole is soluble In water.
Fnsed with Carbonate of Potash, the reBult
is not Boluble in water, but disBoIvcB in Mu-
riatic Acid, producing various colore.
Digiti
ized by Google
166
A COMPLETE TABLE OP
Rhodium,
Palladium, -
Osmium, -
Tellurium,
Titanium,
Tungsten,
Uranium,
Molybdenum,
Shortly a lem-
on-yellow color.
A yellowista
precipitate,
Blightly soluble
in
No precipitate ;
Bolation turns
yellow.
A white preci-
pitate, Boluole In
excess.
A white precl-
Sitate, insoluble
1 excess.
The Acid dis-
solves, but is
again pi-ecipita-
ted by stronger
acids.
A brown, flaky
precipitate, in-
soluble in ex-
cess.
The Acid is dis-
solved, and the
Protoxide forms
a brown precipi-
tate.
A yeUow preci-
pitate, soluble In
acids.
An orange-col-
ored precipitate
from the Nitrate.
Fused ^vith the
whole, is soluble
in water.
A white preci-
pitate, soluble in
excess; reprecl-
pitated by acids.
The same.
The same.
A yellowish
precipitate, in-
soluble in ex-
cess.
The same ; pre-
cipitate insolu-
ble in excess.
GABBONATS OV
POTASH.
A gelatinous
Krecipitate when
oiled with the
double Chloride.
A deep-brown
precipitate, iu-
srlubie in ex-
cess.
No precipitate ;
solution turns
yellowish.
The same.
The same.
Is insoluble in
water when
flised in it.
The same,
slightly soluble.
A brown preci-
pitate, soluble in
excess.
H0AB80NATB
or POTASH.
No precipitate
The
The same.
The
Thei
The
The
Digiti
ized by Google
ANALYTICAL CHEMISTRY.
167
CABBOHATB OV
▲MMONIA.
No precipitate. — ' — —
The same.
The
The
Theeame.
A yeUowish
precipitate, mIh-
ble in excel
The
A dark-brown
precipitate.
A brown preci-
pitate.
A black preci-
pitate, Boinble in
Potash.
No precipitate.
No precipitate.
No precipitate.
A brown preci-
pitate, in Alka-
line solatione.
BTOROSULPHATB
or AHXOMIA.
No precipitate.
The
The eame; boIq-
ble in excesB.
The eame, or in
exceed.
A dirty-green pre-
cipitate, nnieee
Tartaric Acid be
present, then no
precipitate.
A precipitate, Bol-
nbleln
A black precipi-
tate. Bli^tly Boin-
ble in excess.
The eame. if Hn-
rlatlc Add be
added.
TXLLOW PRUBSX-
▲TK or POTASH.
No precipitate.
An orange or
olive yellow pre-
cipitate.
No precipitate.
No precipitate.
A deep orange
precipitate.
AbrowniBh-red
precipitate.
A brown preci-
pitate.
BED FBUBSIATI
or POTASH.
No precipitate.
No precipitate.
The
The same.
Digiti
ized by Google
168
A COMPLETE TABLE OF
HAVS.
OXALIC ACID.
lODiDX or
FOTASBIUM.
BULPHATV OP
rOTABH.
PBOSPBATB OF
SODA.
Rhodium, - - -
Palladium, - • -
Osmium, - • • -
Fused with the
Bisnlphate, the
whole dissolves
in water.
An oranee-yd-
low precipitate.
No precipitate
or acuon.
No action.
Tarns darker,
but Is not preci-
pitated.
- - -
_ - —
Titanium, ...
Tungsten, ...
Uranium, . - -
Molybdenum, - -
lent precipitate.
Does not form
a doable salt.
No doable salt
Digiti
ized by Google
ANALYTICAL CHEMISTRY.
169
XKTALUC nHO.
BKFOmS THX BLOWTIPS.
0B8KBTATI0NB.
Precipitated
from double
Chloride of Hho-
dinm and Soda.
Precipitated in
a metal&c state.
Precipitated at
a dark powder.
Is precipitated
olack po
IS a
der.
pow-
A deep-bine
color is produced.
In Muriatic
Add a bine Oxide
b Conned.
In a Mnriatic
solution of the
Add a blue and
red powder.
No action with flnxee.
Same aa Bhodlnm.
Oivee a strong odor of
Chlorine ; has no action
with fluxes ; may bo cupelled
with Lead.
A white glass, when cold ;
with fluxes; rames when
heated alone.
With Soda, a yellow glass,
opaque when cold ; wiw Bo-
rax and inner flame, a blue
glass.
With Borax, a clear gbws
in the outer flame, yeUow in
the inner: blood-red with
Iron and Phosphorous salt.
On FlatiDum with Borax,
a desr. yellow glass, outer
flame, dirty green, not Tola-
tile.
Insoluble in acids after ignition; distin-
guished and separated bj Bisulpnate of
Potash; the double Cbloride is soluble in
Alcohol,
The Cyanide of Mercury will easily sepa-
rate Palladium as a yellow precipitate ; the
Chloride is soluble in Alcohol.
Tincture of Galls gives a purple precipi-
tate; separated by distillation.
May be separated from most other metals,
combined with Chloriae or Hydrogen, both
compounds being volatile.
Is precipitated by boiling ; distinguiphed
from other metals by its behavior with Tar-
taric Acid and Hydrosolphate of Ammonia.
Sulphuric, Nitric, and Mnriatic Acid preci-
pitate its Alkaline solutions white, turning
yellow when boiled with Nitro-Murlatic
Acid.
Separated ftt>m most metals by dissolving
in Carbonate of Ammonia or Soda ; its solu-
tions are green.
Sublimee aa a white pow- Distinguished by Carbonates, but separated
der ; a clear glass with Bo- by Hydrosulphate of Ammonia,
rax.
Digiti
ized by Google
170 ZETTNOW'S SCHEME FOR QUALITATIVE ANALY
ARRANaED BY
FOR THE STUDENTS OF THE SCHOOL
Add hydrochloric acid to the iiolation, wash, and Alter.
PreHpUaU.
Boil with water and
Alter.
Add exoeM of dilate
Sblu-
tion.
Add
HaSO.
JlsHdue.
Treat with
(NH«)HOr
PrwApUaU.
Agitate with conBiderable cold
water and filter.
Plr»-
Solu-
dp-
tion.
UaU
Add
Pb.
HI90..
Pr$-
dp-
Uaie
A».
BeHdtu
tarns
gray
or
black,
PVtraU.
Add exceaa
of
(NH.),C,0,
PredpUaU
Ca.
Add (NH^fiO and
(NH.).C.H,0..
digest and filter.
Besidue.
Boil with Na,00„
filter, wash, dissolve
on filter with HCl,
neatraliae filtrate
with (NH«)HO, and
dlYlde into two
I>art8.
FUtraU,
Add
H(C,H,0,)
ind K,CrO
PredpUats
lit Half.
Add ezce«is
of Bolation
ofSrSO*.
PredpUaU
Ba.
Second Haiff.
Add excess of
H.Si,F]« and alco-
hol. Shake, filter,
dilate with water,
expel alcohol by
evaporation, add
solution of CaSO«,
and after one or
two miuotes a
precipitate
Sr.
In this scheme regard is had to the following sab-
stances in aqueons solution :
I.
PbO, Ag,0. HgO.
n.
CaO, BaO, SrO.
m.
(NHJ.O, Na.O. K,0.
IV.
As.Os, As.O,. 8b,0„ Sb.O., 8nO, 8nO.,
Hg.O, CuO, CdO, BUO,.
V.
PeO, Fe,0„ Cr,0„ A1,0..
VI.
MnO, MgO. Ck)0. NiO.
vn.
ZnO.
To \ add BaH.O.
andboiL
VdaWixed. Solution.
(NHJ,0.
Test gas
withBa
and lltmas.
Add
excess
of
(NHj.CO,
and
warm, filter,
evaporate to dryness,
and ignite residae.
Test on platSnam
wire in colorless
flame : intense yellow
color indicates
Ka.
Violet color seen
throagh blae glaaa
indicates
Flacei
when
^wash
Voior
tUaed,
Collect
spots on
cold
porce-
lain,
and
treat
with
NaClO.
Spoto
dissolve;
As.
Spots
do not
dissolve ;
8b.
Test
abo with
AgNO.
I
N. B.— To test for sine mix
Ha, H.SO«, filter, add NaHO In
and NH«C1 to filtrate, boil antU
ter. Add K«Fe«Cy« to eolation.
Digiti
ized by Google
SIS WITHOUT THE USE OF H2S OR (NH4) HS. m
H. C. BOI.TON, FI1.D.,
OF MIKES, COLUMBIA COLLEGE.
jnUrats.
HaSO« and waeh on Alter.
FUtrau,
Divide the eolation tnto two unequal parti>, \ and {.
- - •
of tbe foiutloo in a Marnh^s apparatan, add pieces of elnc and a strip of pintinnm foil,
bni little dnc remains heat 16 or SO minutes, and throw contents of flasK on a Alter ;
thoroughly.
Treat with strong HNO„ and filter.
Filtrate.
Boil with a little UNO, and divide in two
nnequal parts.
BetiOm.
Wash, boil
with HCl,
and filter.
8olU' \ BeH-
Hon. > due.
Put In Add
a platl- to »o-
nnm lution
dish
with a
ofzlnc.
A dark
spot
on the
nnm
Indl-
catee
8b.
lu
plati-
nam
dish,
boil
with
HCl,
filter
and
add
dpi-
UUe
Sn.
FiUraU.
Diyide Into two parts.
UtPorOtm.
Add KCvS.
Bed ColoT,
Add
SnCl..
tote
Second PorOtm,
Neutralize with (NU«)HO, add ex-
cess of BaCOa, ngitate 10 minutes,
filter and wash thoroughly.
Second Half.
Add HCl, boil,
then add excess of
NaHO, wash the
precipitate on fil-
ter with water,
tben with
(NH«)HO contain-
ing NH«CL
SeHdve.
Dissolve
on filter
in very
litUe
HCl and
add
large
of Ht(
to the
filtrate.
A cloudy
precipi-
tate in-
dicates
Bi.
IWrale.
Divide into two
parts.
IMffaO-.
Acidilv-
with HCl
and add
K.Fe.Cy.
Jrrectpi'
tote
On.
Add
excess
of
NaHO.
a white
f^latln-
oas
Precipi-
tate
Gd.
a portion of the original solution with
excess, and boil. Add a little (NH«),CO.
all odor of (NH«)HO is expelled, and fil-
« dond or precipitate indicates Zn.
PredjAtate.
Boll in a porcelain
dish with dilute
H,80« and filter.
Add excess of NaHO
to filtrate, a few drops
ofK,Mn,0.,anda
little NH«C1. boil
filter, and divide the
solution.
Ut Ha^.
Add some
HlCH.O.)
and
Pb(C,H,0,).
PreeipUate
Cr.
MdHalf.
Add ex-
cess of
NH«C1.
Precipi'
taU
AL
• To determine de-
gree of oxidation of
Pe, examine the ori-
ginal solution with
K«Fe.Cy« and ECyS.
PreeipUate
Mix a por-
tion with
Na,CO.
andNaNO.,
fuse on
platintmi
fbil.
Oreen color,
Mn.
Filtraie,
Add excess of dilute
H,SO„ filter, and sat-
urate filtrate with
(NH.),CO„ warm, filter,
and wash.
Sduiion.
Add
Na.HPO..
Dissolve
another
portioQ in
HCl, neu-
tralize
with
(NH,)HO,
add con-
siderable i
NH.Cland
(NH,),C,0,
Pre^)itate
Pnh
cipi-
tate
Solu-
tion.
Evap-
orate
to
dry-
ness, dis-
solve in
HCl, add
KNO, and
H(C»H,0.),
filter.
Pre
Hpi-
fate
Co-
Solrt-
tUm.
Add
Na
HO.
Pre-
dpi-
tote
Ni.
Digiti
ized by Google
172 STAS-OTTO'S SCHEME FOR THE
TRANSLATED FROM THE CERMAN
Taken np by ether in acid
BolutionB.*
Taken ap by ether
With tannic add.
Solid
Precipitated.
NoacUon.
With concentrated Bolphnric acid.
COLCHI-
OXN.
DlOITA-
UK.
MUedwith
a BOlation
of galls
concentra-
ted H.SO.,
hbriffht-
rMl Btratam
ie fonped
and finally
a red
Uqnid.
PlOBOTOX-
nr.
The dUnte
alkaline
(NaHO)
eolation U
eobfrteu
and
reducoB
Fehling'e
copper
Bolatlon.
InthecoUL
On heating.
TheyOlmD
Bolutlon iB
colored
violet by
concen-
trated
HNO,.
Roae-red.
Brown-red.
YeUow,
then or-
ange, and
cherry-red.
Yellow, then
Tiolet-blae,
and dark-rod.
BBUom.
Soluble in
concentra-
ted HNO.,
with a
color,
which
becomes
uettotoon
heating.
On addGig
Btannic
chorlde to
thie eola-
tion, a
vioUt color
is formed.
Dblphzh-
IN
forme with
concentra-
ted H.SO.
and bro-
mine water
Ared^sA-
Ho^ color.
The same
coloration
appeare on
evaporat-
ing with
phoephoric
acid.
VniA-
TBIH
forme with
concentra-
ted HCl a
colorlete
eolation,
which
becomee a
fine dark'
red on
heaUng.
NABoomr
on diesoMng
in H.SO,
with a little
HNO., forme
a red color.
Concentrated
H.SO. with
a trace of
Bodic molyb-
date forme a
oreen color.
Dleeolvee in
HCl, forming
tk pale-men
eolation
which tome
on adding
NH.HO.
On dilating
the nitric
acid Boln-
tion and
making it
alkaline
withNaHO,
an oranfi^
fwl colora-
tion iB
obtained.
OndieeolY-
ing in con-
centrated
H.SO«and
mixing
with a drop
of bromine
water, a
violet-red
coloration
is
produced.
Aoozomv
dieeolvefi
color.
* Also a Bmall quantity of atropin.
tAle
0 partially
* Pharmaceatieche Poet,
Digiti
ized by Google
DETECTION OF ALKALOIDS, ETC. 173
BY H. CARRINOTON BOLTON, PH.D.*
in alkaUne 8olntiODB.t
Insoluble in
ether.
<odorieM).
Liquid (strongly odorous).
MoBFHnr. ' .
With concentrated HaSO«
and K.Cr,0,.
With
concentrated
phosphoric
acidand
application
of heat.
With chlorine water.
The ammonia-
cal solution
gives a arau-
green solution
on heating
with cupram-
moninm
(Nadler).
Ck>ncentrated
In the cold.
•
On heating.
VIolet-blne.
Characteris-
tic odor.
FredpiUted.
No action.
HNO, colors it
blood red,
neutral Fe,Cl«
colors it
darMlw.
On dissolving
in concentrated
HsSO^heatlng,
allowing to
cool, and then
adding a little
HNO,, an in-
tense red color
is produced.
Reduces an
acid solution
of iodic acid,
the iodine
dissolving out
in C8, with a
vMet color.
tomB B tfellow
solation with
HNO,.
TheffMet
coloration also
obtains when
either potassic
plumbic and
manganic
dioxides, or
potasslc iodate
Isnsed
in place of
K.Cr,0,.
Atbohot.
The
odor is better
formed by
placine the
alkaloid on a
few crystals
of chromic
acid and .
heaSng antil
the green
oxide of
chromiom
b<»;in8to
ibnn.
Aoomnv
produces a
vioAff color.
Dissolves in
concentrated
U.SO.witha
color.
CoRor.
Aqneoas
solntions
become
colored on
heating.
NlCOTIH.
Aqueoos
solutions do
not become
colored on
heating.
Dklphinin
and
behave In the
same manner
withH.PO«.
DiT HCl gas
colors it red
and then
On gently
heating with
hA,
becomes
violet, KudoD
adding
HNO,
the color
changes to
orange.
Note,
CUBAHIN
gives similar
reactions to
sti7chnin,
bat forms a
red color with
H,SO« alone,
and is more-
over insoluble
In ether in the
presence of
acids and
alkalies.
colcfaicinanddigitalin.
YoL VI., No. 11, June, 1878.
Digiti
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■ Yellow^ Blue Colorlegs.
174 THE CHEMISTS' MANUAL.
DETECTION AND SEPARATION OF ALKALOIDS.
According to J. Trapp (Jahresb., 1863, p. 702).
The yellow pulveralent or flocculent precipitates produced
in the acid solution of many organic bases by phosphomolybdic
acid are insoluble in dilute nitric acid, but easily soluble in
amnionic hydrate and the fixed alkalies. The solutions of the
several precipitates in ammonic hydrate exhibit the following
color-reactions :
Aconitin ''
Atropin
Bebeeriu
Berberin
Bracin Orange Yellow-green. Brown.
Codein Yellow Green Orange-red.
QSiSid*m!!.".!*.;!!;f^®"^^ Insoluble Colorless.
Caftein Yellow Colorless , .
Conia Yellowish- white Light-blae Colorless.
With digitalin (yj^ of a grain) and phosphomolybdic acid,
there is formed a yellow liquid, which becomes green on boil-
ing ; deep-indigo on addition of ammonic hydrate ; green again
on heating ; then colorless.
NEW REACTION OF THE ALKALOIDS.*
If strychnin be dissolved in concentrated sulphuric acid, to
which is added a little eerie oxide (sesquioxide of cerium), an
intense Blue color is developed, similar to that produced in the
ordinary mode of testing by potassic dichromate. The color
is, however, more durable, and passes gradually into a cherry
red, which remains unchanged for several days. Other alkar
loids, treated in the same manner, give rise to a variety of
color-reactions, as follows :
Brucin (C21H22N2O2) — Orange, and finally yellow.
Morphin (C34 H 33 N2O6)— Brown, olive-green, and finally
brown.
Narcotin (C5H7N) — ^Brown, passing to cheny-red.
• Vierteljahresschrift fuer Prak. Pharm.
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THE CHEMISTS' MANUAL.
175
I8H21NO3
or CagH^aNjOg) — Olive-green, and
Codein (C,|
finally brown.
Quinin (C20H24N2O2) — ^Pale-yellow.
Veratrin (C32H52N2O8) — Eeddish-brown.
Atropin (C, 7 H 23 NQ3)— Yellowish-brown.
Solanin (C43H71 NO,g ?)— Yellow and finaDy brown.
Emetin (C30H44N2O8)— Brown.
Colchicin (CiyHj^NOg) — Green, and finally dirty-brown.
Conin (CgH jgN)— Clear yellow.
Piperin {C,7H,9N03) — Colors the sulphuric acid blood-red ;
an addition of eerie oxide, dark-brown.
STRYCHNIN.
The following table comprises the various tests for strych-
nia made by Mr. W. T. Wenzell (Am. Jour. Phar., Sept. 1870).
The solution of strychnin was made by dissolving the alkaloid
in water with the aid of sulphuric acid :
GRAINS
KCaCrO, and
BO.H test (solid).
CtO, and SO«H
test (1-JX)0).
KO.Hn.Or and
SO.Htesta-SOOO).
1-100,000.
Color -reaction,
distinct and
well-defined.
Color of reac-
tion, very fine
and distinct
Reaction very
brilliant and
durable.
1-300,000.
Reaction weak
and evanes-
cent.
Color fine and
distinct.
Colors brilliant
and reaction
distinct.
1-600,000.
No reaction.
Colors still de-
finable, bat
weak.
Reaction dis-
tinct and col-
ors fine.
1-900,000.
No reaction.
Reaction faint,
but succession
of colors weU-
defined.
1-1.200,000.
Reaction very
faint.
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176
REACTIONS
OF FAT
(WATTS DIG
OILS
1. CHEM.,
OILS.
OUve
OalllpoU
India nut
Pale Bape-0eed
Poppy
Frenoh nat
SoMine
Oastor
Hemp-seed
Linseed
Lard
Keat's-foot
Spenn
Seal
Cod-liver
Caubtio
Soda.
Sp. Gr.,
1.840.
SUUPHUBIO
AOID.
Sp. Or.,
1.476.
SuLPHnmo
Acid.
Sp. Gr.,
1.580.
SULPHUXIO
ActD.
Sp. Gr.,
1.685.
NiTBIO
Acid.
Sp. Gr,,
LlSOi
Slight
yellow.
Ditto.
Thick and
white.
Dirtv
yeUowish
white.
Ditto.
Ditto.
Ditto.
White.
Thick
brownitih
yellow.
Phiid
yellow.
PlnkiBh
white.
Dirty
yellowish
white.
Dark red.
Ditto.
Ditto.
Green
tinge.
Ditta
Brownish.
Green
tinge.
Intense
green.
Green.
Dirty white.
Yellow
tinge.
Light red.
Ditto.
Parple.
Greenish
white.
Gray.
Dirty white.
Pink.
Dirty white.
Gray.
Greenish.
Dirty white.
Dirty white.
Intense
green.
Dirty green.
Dirty white.
Brownish
dirty white.
Red.
Ditto.
Purple.
Light
green.
BrowiL
Light
brown.
Brown.
Brown.
Intense
green.
Green.
Light
brown.
Brown.
Intense
brown.
Ditto.
Ditto.
Greenish.
Ditto.
Yellow.
Orange
yellow.
Dirty
green.
YeUow.
Light
yellow.
Slight
yeuow.
Pink.
Digiti
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177
"WITH ACIDS AND ALKALIES.
Vol. IV, p. 188.)
NlTRBU
Acid.
Acid. Soda.
Sp. Gr., Sp. Or.
*1.8a 1.84.
Phosfhobio
Acid.
Syrupy.
SULPHUBIC
Acid +
NiTBIC
Acid.
Aqua
Bbgia.
+ Caustic
Soda.
Greeniata.
Greenish.
Fluid
white
mass.
Orange
yellow.
Fluid white
mass.
Ditto.
Ditto.
Fibrous
ditto.
Ditto.
Dark
brown.
Fibrous
yellowish
wnite mass.
Ditto.
Orange
whitl
Fibrous
white mass.
Fluid ditta
Dark
brown.
Fibrous
yellowish
white mass.
Orange
yellow.
Red.
Light red
mass.
Slight
yellow.
Fluid intensA
rose-colored
mass.
Bed.
Dark red.
Fibrous
red mass.
Brown
yellow.
Dark
brown.
Yellow.
Fibrous
orange mass.
Ditto.
Ditto.
Fluid red
maps with
brown
liquor
underneath.
Fibrous
white
mass.
Green be-
coming
intense red.
Brownish
red.
Ditto.
Fluid oranse
mass with
brown liquor
beneatn.
Fibrous pale
rose-colored
mass.
Greenish
dirty
brown.
Greenish
dirty
brown.
light brown
mass.
Green.
Green
becoming
black.
Green.
Fibrous
light brown
mass.
TeBow.
Green
becoming
brown.
Fluid
yellow
mass.
Brown
yellow
green.
Ditto.
Greenish
yellow.
Fluid orange
mass.
^K^^^
Fluid
mass.
Brown.
Fluid pink
mass.
Light
yellow.
Light
brown.
Fibrous
white
mass.
Dark
brown.
Slijght
yellow.
Fibrous
brownish
yellow mass.
Ditto.
Bed.
Fluid
mass.
Dark red.
Ditto.
Ditto.
Fluid orange
yellow mass.
Light Rd.
Ditto.
Ditto.
Ditto.
Ditto.
Ditto.
Ditto.
Ditto.
Ditto.
Ditto.
Ditto.
Yellow.
Dit'U).
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178
SCHEME FOR THE ANALYSIS OF FATTY
ARRANGED BY
6 volB. oU mixed
with 1 vol. potash
lye of 1-84; and
etrongly a^tated.
The maes Is—
Snow white.
Oil of almonds,
very good rape-seed
oD, bleached
oUveoiL
yellowish,
sesame oiL
Greenish.
Linseed oU,
hemp-seed oil,
oils containing Co,
and arti£ dyes.
Mix in beaker care-
ftilly equal vol. of
oil and red Aiming
nitric acid. A mid-
dle zone forms on
point of contact.
This la
Narrow and light
green ; oil becomes
flocculent and
opaque.
Oil of almonds.
Dark-green;
pink above.
Poppy-seed oiL
Broad and beantiftal
light-blue green.
OUve oil.
Mix in a beaker the
oil with concen-
trated enlphnric
acid. Layers where
oil and acid meet
10 drops of oil, 8 of concentrated sulphuric acid.
Beautifhl green,
with brown stripes,
Rape-seed oil.
Yellow; after
agitating, brown
Poppy-seed oil,
madia OiL
Bed, soon changing
to black, Ftri pes
undulating through
the liquid.
Train OiL
In the elaidine test
the oil masB la-
Solidified, crumb-
ling, and white.
Olive oU, oil of
aimonds, bleached
rape-seed oiL
Solidified,
crumbling, and
yellowleh.
Bape-seed oiL
Solidified and red.
Sesame olL
in bollinfl: with wa-
ter and oxide of
lead a plaster is
formed, the consis-
tence of which is—
Solid.
Olive oil.
Smeary.
Bape-seed oil,
oil of almonds,
sesame oU.
Smeary, but drying
after some time.
Drying oils.
Solubility of 1 part
oil in alcohol-
1:1
Castor oU.
1:86
Poppy-seed oiL
1:80
Hemp-seed oO.
Specific grayity of
oils is
0-918
Poppy-seed oil,
and oil of brass.
nap.
0-014
Oil of almonds,
oil of brass, camp.
0^8
OUveoiL
No. of degrees Centi-
grade at which the
oils change fh>m
solid to liquid
state.
—87'
HempHBeed oil.
-18"
Castor oil.
+S-6+6*to+8'.
Olive oU, lard oil.
-16" to -80*
Linseed oil.
-80- to -85-
OUofalmoDdf.
NoTB.-See JfTMT. CSIk^n., December, 18T8.
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179
OILS AT ORDINARY TEMPERATURES.
G, GLAS SN ER.
Pink color.
Brown and stiff.
Hemp-Beod oU.
Yellowleh-brown
and tlnid.
Linaeed oiL
Red.
Train oiL
Brown-red.
Cod-llTerolL
Lineeed oil.
Brown-red,
ffreeni»h below.
Kape-seed oil.
The oil colon
throo^hont red,
after some time.
Linseed oa
Eqoal Tolnroes oil and acid.
Without bisnlphide of carbon.
With blsnlpfaide of
carbon.
When agitated,
line dark-green.
Bape-seedoiL
Green.
Linseed oU,
hemp-seed oiL
Bed.
Train oil.
With 80 timee its
vol. C8„ splendid
violet, quickly
changing to brown
coloration.
Train oil.
Waz-llke and white.
Castor oa
The elaidine mass
shows oil drops
and stripes.
Oil mixtures con-
taining drying oils.
Unchanged.
Llnseed^oil,
poppy-seed oil,
nut oil.
Ethereal oils, added
to the olive to
correct the smell,
float on the elaidine.
1:40
Linseed oU.
1:60
Oil of ahnonds.
0-988
Sesame OIL
o-aw
Sonflower oil.
0-9B0 — O'TO
Castor oa
0-«80
Linseed oil.
-16-
Sonflower ofl.
-6'
Oil of brass, napns.
—40'
Oil of brass, camp.
-6*
Sesame oa
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180
THE CHEMISTS' MANUAL.
FAT OILS.
The following table* exhibits a list of the priocipal vegeta-
ble fat oils, together with their specific gravities and solidify-
ing points. The specific gravity marked with an asterisk are
according to the determinations (taken as 15° C.) by Cloey
(Bull. Soc. Chem. 1865, p. 46) ; the rest and the solidifying
point.s are taken from OnidMa Handboolc, The numbers in
the last column denote the temperatures at which the oils
become perfectly solid ; nearly all of them, however, become
viscous or semi-solid at temperatures somewhat higher.
Naxs of Oil.
Spboipic
GBAYTrT.
SOUDIFTINO POIKT.
1. Drying Oil.
Oress-seed oil
Oil of deadly night- 1
shade f
Oil of gold off
pleasure seed. . . )
Gourd-seed oil
Grape seed oil
Hemp seed oil
Oil of honesty
Linseed oil
Oil of madi
Lepidium sativum....
Atropa belladonna. ...
Camelina sativa
Cucurbita peps
Vitis vinif era
Cannabis sativa.
Hesperis matronalis. . .
Linura usitatissimum.
Madia sativa
0.924
0.936
0.93075*
0.9381
0.9203
0.93075*
0.9232
0.93515*
0.9286 at IS*"
0.92702*
0.92504*
0.9313
0.926
0.9283
0.904
0.9232
0.92878*
0.9358
0.91844*
0.923
0.917
0.943
6.9639*"*
0.9306
0.9136atl5"'
-15° C.
-27.5°
-19°
-16°
-ir
-27.6°
below —15°
below -20°
below —10°
PODDV oil
Papaver somnif erum. .
Helianthus aunuus...
Finns sylvestus
Abies picea dec
Abies excelsa dec
-18°
Sunflower oil
Oil of Scotch fir seed
Oil of silver fir cones
OU of spruce fir
Fatty oil of spruce fir
Tobacco-seed oil
Walnut or nut oil . .
Weld-seed oil
Non-Drying Oils.
{Vegetable.)
Almond oil
-16°
-80°
below —15°
Nicotiana tabacum
Juglans regia
Reseda luteola
Amygdalus communis.
Fagus sylvatica
Butea f rondosR
jCalophyllum ino-|
\ phyllura )
Canarium commune . .
Ricinus communis
Gossypium barbadeuse
j Bra^sica campes- _
\ tris oleifera
-15°
-18°
below -16°
—21°
Beech-nut oil
Oil from seed of
Oil from seed of. .. .
Oil from seed of . . .
Castor oil
-17.5°
4-10^
+ 5°
+5 to 3.6-
—18°
Cotton-seed oil
Colza oil
—6.25°
* Watt's Die. Chem., vol. iv, p. 180.
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THE CHEMISTS' MANUAL.
181
PAT OlLB^Contintied).
I OF Oil.
Naxb of Plant whxoh
TIBI.D8 IT.
spbcifio
Gbavitt.
SouDDTniG Point.
Croton oil
Oil of cyperus-graBS.
Oil of Daphne....)
Oleum seminom V
coooognidii )
Earth-nut oil
Ergot oil
Hfl^l-nut oil
Henbane-seed oil . . .
Horse-chestnut oil..
Mesua oil
Black mnstaid oil . .
White mustard oil. .
Oil from seed of . . . .
Oil from root and)
seed of )
Parsley oil
Plum-kernel oil
Oil from seed of . . . .
Summer rape-seed )
oil S
Winter rape-seed oil
Sesame oil
Spindle-tree oil
Spurge oil
Oil from seed of . . . .
Oil from Tarious)
kinds of -..]
Croton tiglium
iCyperus esculen- )
tus (root) )
Daphne mezereum . . . .
Arachis hypogoea; . . . .
Secale comutum
Coiylus avellana.
Hyoscyamus nigra. . . .
( .Slsculus hippo- )
7 castanum )
Mesua ferrera
Sinapis nigra
Sinapis alba
Nigella sativa
Finns quadrif olia. .
Petroselinum sativum,
Prunus domestica
Pougamia glabia
Brassica proecox
Brassica napus
Sesamum orientale
Euonymus europoeus.
Euphorbia lathyris. . .
Sterculia fcetlda
Thea and camellia. . .
0.94268*
0.018
0.014-0.921
0.918
0.922
0.91987*
0.913*
0.915
0.964
0.92102*
O.fi
0.92
0.935
1.078 at 12*
0.9127
0.915
0.91555*
0.91648*
0.92415*
0.95717*
0.92613*
0.923
0.927
-37"
-lO**
+ 8''
below 0°
does not solidify.
+ 2'
(becomes turbid
at -12% but
does not solid-
ify.
-8.7''
+8°
a little below 0°
-5"
-12° to -15'*
-llj"
below -1-3°
if orms an emul-
sion at 4.5°
The following table * exhibits the rotary power of a con-
siderable number of volatile oils, together with their refractive
indices A, D and H, as determined by Gladstone (Chem. Soc.
J., xvii, 3). Also their specific gravities. The rotary power
was determined for a column of liquid 10 inches long ; the same
length of a solution of equal parts of cane-sugar and water
produced a deviation of + 105*^.
» Watt's Die. Chem., vol. iv, p. 186.
Digiti
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182
THE CHEMISTS* MANUAL.
SPECIFIC GRAVITIES AND OPTICAL PROPERTIES OF
ESSENTIAL OILS.
CRUDE OTUB.
Anise
Atherospenna moschatam
Bay
Bergamot
** Florence.
Birch-bark
Cajeput
CaJamus
" Hamburg
Caraway
' * Hamburg, 1st dist.
" " 2d dist.
Cascarilla
Cassia
Cedar
Cedrat
Citronella
«' Penang.
Cloves
Coriander
Cabebs
Dill
Elder
Eucalyptus amygdalina. .
** oleosa
Indian Qeranium
Lavender
Lemon
Lemon grass
*' Penang
Melaleuca ericifolia
'' linarifolia
Mint
Myrtie .',
Myrrh
Neroli
u
Nutmeg
" Penang
Orange-peel
'* " Floi-ence
Parsley
Patchouli
*• Penang
" French
Peppermint
Spkoifio
GBAVITr
AT
16'.5 C.
1.0425
.8825
.8804
.0005
.9203
.9410
.8845
.9121
.8956
1.0297
.9622
.8584
.8847
1.0475
.8775
.9414
.8584
.8812
.9322
.9043
.8908
.8498
.8766
.9080
.9016
.9342
.9105
.8911
1.0189
.8789
.8743
SBniACTIYB InDIOBB.
.9069
.8509
.8864
.9936
.9554
.9592
1.0119
.9028
Temp.
16°.5
14*'
18°.5
22^*
26^5
8°
25^5
10°
IV
19"
10**
10°.5
10°
19°.5
23°
18°
21°
15°.5
17°
10°
10°
11°.5
8^5
13".5
13°.5
21°.5
20°
16°.5
24°
13 .5
9°
9°
19°
14°.5
14°
7°.6
18°
10°
124°
j 16°
20°
20°
I 8'.5
21°
21°
1 14°
14°.5
1.5483
1.5172
1.4944
1.4')59
1.4547
1.4851
1.4561
1.4965
1.4843
1.4601
1.4829
i!4844
1.5002
1.4978
1.4671
1.4599
1.4604
1.5218
1.4592
1.4953
1.4764
1.4686
1.4717
1.4661
1.4653
1.4685
1.4667
l!4756 !
1.4665 >
1.4710 !
1.4767 I
1.4756 ,
1.4623 I
1.5196
1.4614
1.4673
1.4644
1.4749
1.4638
1.4707
1.5068
1.4990
1.4980
1.5074
1.4612
1.5566
1.5274
1.5022
1.4625
1.4614
1.4921
1.4611
1.5031
1.4911
1.4671
1.4903
1.4784
1.4918
1.5748
1.5035
1.4731 I
1.4659 1
1.4665
1.5312
1.4652
1.5011
1.4884
1.4749
1.4788
1.4718 '
1.4714 I
1.4648 1
1.4727
1.4705 i
1.4837
1.4712,
1.4772 I
1.4840
1.4822 I
1.4680!
1 5278 :
1.4676 i
1.4741
1.4709 '
1.4818 .
1.4699
1.4774
1.5162
1.5050
1.5040
1.5132
1.4670
1.6118
1.5628
1.5420
1.4779G.
1.4760G.
1.5172
1.4778
15204G.
1.5144
1,4886
1.5142
1.5158
1.6243G.
1.5238
1.4952
1.4866
1.4875
1.5666
1.4805G.
1.5160G
1.5072
1.4965
1.5021
1.4909
1.4868G.
1.4862
1.4946
ROTATIOV.
1.5042
1.4901
1.4971
1.5015G.
1.5037
1.4879
1.5472G.
1.4835G.
1.4831F.
1.4934
1.5053
1.4916
1.4980 ,
1.5417G.I
1.5194G.'
1.5183G.
1.5202F.I
1.4854
1°
7°
6°
23°
40°
88°
0°
43°.5
42° t
63°
-h 26°
0°
+ 3°
-1-156°
- 4°
- 1°
- 4°
+ 21°?
+206°
+ 14°.6
-136°
+ 4°
- 4°
- 20°
+ 164°
+ 3°t
0°
+ 26°
+ 11°
-116°
- 13!
+ 21°
-136°
+ 16°
+ 28°
+ 44°
+ 9°
+ 32°?
+ 216^
- 9°
-120°
- 72°
Digiti
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THE CHEMISTS* MANUAL.
183
SPECIFIC GRAVITIES, ETC., OF ESSENTIAL OILS {Continued).
CRUDE OILS.
Peppermint, Florence,
Petit grain
Rose
Roeemary
Rosewood
Sandalwood
Thyme
Turpentine
Verbena
Wintergreen
Wormwood
Sfboific
Gbatitt
AT
15'.6 C.
.9118
.8766
.8912
.9080
.9064
.9750
Rbvractiye Ikdicbb.
Temp.
.8727
.8813
1.1423
.9122
14*'
2V
25°
16^6
17°
24°
19°
13°
20°
15°
18°
1.-
1.4536
1.4567
1.4632
1.4843
1.4959
1.4695
1.4672
1.4791
1.5163
1.4631
1.4682
1.4600
1.4627
1.4688
1.4903
1.5021
1.4754
1.4732
1.4870
1.5278
1.4688
1.4867
1.4808
1.4836
1.4867
1.5113
1.5227
14909G.
1.4938
1.5059G.
1.5737
1.4756F.
Rotation.
- 44°
+ 26°
- 7°
+ 17°
- 16°
- 60°
- 79°
- 6°
+ 3°
SPECIFIC GRAVITIES, BOILING POINTS, AND OPTICAL
PROPERTIES OF HYDROCARBONS FROM ESSENTIAL
01 LS.*— (Gladstoite.)
SOVBCX OB Htdbooabboh.
Orange peel
'* " Florence...:
Cedrat
Lemon
Bergamot
" Florence
Neroli
Petit grain
Caraway, Hamburg, Istdist.
Dill
Caficarilla
Elder
Bay
Ganltherilene
Nutmeg
** Penang
Garverie
Hamburg, 2d dist.
Wormwood
Terebene
Anise
Mint
Peppermint
.8460
.8468
.8466
.8466
.8464
60
II
.8470
.8466
.8467
.8467
.8468
.8508
.8510
.8518
.85271
.8530
.8645
-8565
.a583i
.85801
.86001
174° C
174°
173°
173°
175°
176°
173°
174°
176°
173°
172°
172°
171°
168°
167°
166°
166°
160°
160°
160°
160°
175°
1.4645
1.4650
1.4660
1.4660
1.4619
1.4602
1.4614
1.4617
1.4645
1.4646
1.4652
1.4631
1.4542
1.4614
1.4630
1.4634
1.4610
1.4641
1.4590
1.4670
1.4607
1.4622
1.4577
Id
1.
.0277
.0281 1
.0280 i
.0295
.02S7\
.0291
.0282
.0286
.0288
.0305
.0260
.0271
.0284
.0274
.0261 1
.0263!
.0253
.0275
.0255
.0267
.0048
.0049
.0049
.0049
.0049
.0048
.0047
.0046
.0048
.0046
.0049
.0047
.0047
.0049
.0047
.0049
.0048
.0048
.0047
.0048
.9047
.0048
.0047
s^6
vac?
.549
.5491
.5602
.6466
.6487
.5450
5439
.5486
.5480
.6494
.5468
.5338
.5422
5435
.5434
.5440
.5431
.5359
.5440
.5368
.5374
.5321
I
+ 164°
+ 260°
+ 180°
+ 172°
+ 76°
+ 82°
+ 76°
+ 60°
+ 180°
+ 242°
+0°
+15°
-22°
+ 49°
+ 4°
-20°
+ 86°
+ 46°
0°
+ 30°
-60°
Digiti
ized by Google
184
THE CHEMISTS' MANUAL.
SPECIFIC GRAVITIES, ETC., HYDROCARBONS— (Ciw«»ntt«f.)
SovBOB or Htdrocabbok.
Laurel turpentine
Thyme
Turpentine, I
II
Ill
IV
Eucalyptus amygdalene.
Myrtle
Parsley
Rosemary
Cloves
Rosewood
Cubebs
Calamus
** Hamburg
Cascarilla
Patchouli
" Penang
French
Colophene
m
.8818
.8685
.8644
.8555
.8614
.8600
8642
8782
.8805
.9041
.9042
.9180
.9275
.9212
.9211
.9255
.9891
160°
160'
il60°
.160*
!l60''
I 160*'
!l71'
lOS''
160'
163°
249'
249'
260'
260'
260'
254'
254'
257'
260'
315'
1.4637
1.4617
1.4612
1.4590
1.4621
1.4613
1.4696
1.4565
1.4665
1.4583
1.4898
1.4878
1.4950
1.4930
1.4976
1.4926
1.4966
1.4963
1.6009
1.5084
Jo-
.0266
.0249
.0264
.0248
.0291
.0241
.0284
.0277
.0302
^1
.0337
.0807
.0274
.0275
.0309;
.0047
.0048
.0047
.0047
.0047
.0049
.0047
.0046
.0046
.0045
.0045
.0041
.0042
.0043
.0042
.0042
.0044
.0042
.0041
III
.5380
.6346
.6335
.6365
.5364
.5364
.6434
.5253
.5865
.5205
.5417
.6395
.6462
.6370
.6366
.6347
.6891
.6849
.6412
.6413
I
+ 94'
-75'
+ 48'
-87'
-90'
-88'
-142'
+ 64'
-44'
+ 8'
-11'
+ 59'
+65'
+ 22'
+ 72'
-90'
0'
* This table exhibits the densities and optical properties of a consider-
able number of polymeric hydrocarbons. The oils are arranged according
to their specific gravities at 20' C. The column headed ** Disperaion at
£0" C." gives the difference between the refractive indices of the lines
H and A. The "sensitiveness" is the amount of diminution of the refrac-
tive index when the temperature rises 10'; it is calculated for the line A.
The ** Specific refracHte energy" is the refractive index minus unity,
divided by the density. In this table it is taken for A ; that is, the column
represents ^—^' (Watt's Die. Chem., vol. iv, p. 187.)
Gladstone proposes (Chem. Soc. J. [2], x, 1) to distinguish the several
hydrocarbons by the following names :
Hydrocarbon from Bay Laurylene.
" " Calamus Calamene.
" Dill Anethene.
" " Elder Sambucene.
** " Eucalyptus amygdalina . Eucalyptene.
" Myrtle Myrtene.
'• " Nutmeg Myristioene.
" << Rosewood Rhodine.
Digiti
ized by Google
THE CHEMISTS' MANUAL.
185
TABLE OF OFFICIAL TESTS FOR IMPURITIES IN
PHARMACOPCEIAL PREPARATIONS.
ATTFIELD'S TABLE.
XAm OF FBBFABATIOH.
IMFUBITIBB.
AcMdae Gnmmi
Acetam
Addam Aoeticnm —
Acetic Add
Add. Acetic. Qlac. . . .
Addam Boradcum..
Addum CStriciun .
■I
Addam Ga11icam<
Addam Hydrochlori- 'i
com 'i
Addam Hydrocyani- <
com Dilatom
Acidum Nitricom ...
Acidam Oxalicam. . . .
Addam PhoBphori- ^
cam Dilatam ....
Addam Salphoricom •'
Addum Tannicam . .
Addam Tartaricam. ^
Aconitia
Adepe Preparatas. . . j
jEther.
^ther paras
Alcohol I
Alcohol Amylicam. . . .
Alam
Starch
More than one thou-
BandthH8S04
Traces of Pb or Cu. . .
H,S04
HCl
Sulphurous Add
Sulphurous Acid
Alkaline Salts
Traces of Cu. or Pb. .
Tartaric Acid
Sulphuric Acid
Mineral Matter
Tannic Add
Sulphuric Add
Arsenic
Sulphurous Acid
Sulphuric Add
Hydrochloric Acid . . .
Mineral Matter
Sulphuric Add
Hydrochloric Add . . .
Mineral Matter
PborPt
Sulphuric Add
Hydrochloric Acid . . .
Meta phosphoric Acid.
Nitric Add
Phosphorous Add. . . .
Mineral Matter
Nitric Acid
As or Pb
Mineral Matter
Metallic Matter, as Pb
Oxalic Add
Calcium Tartrate ....
Caldum Sulphate. . . ,
Mineral Matter
Mineral Matter
NaCl
Starch (flour)
Alcohol
Alcohol and Water . .
Resin or Oil
Water
Other Spirit. Matter .
Iron (Sulphate)
Iodine.
y Quantitative Analysis.
Sulphuretted Hydrogen.
BaCl, or Ba2N08.
AffNO,.
Nascent Hydrogen.
Nascent Hydrogen.
Insolubility in AlcohoL
H,S.
Acetate of K.
BaCl, or Ba2N08.
Indneratioru
Gelatine.
BaClj or Ba2N0,.
H,S.
Nascent Hydro^n.
Baa, or Ba2N08.
AgNOg insoluble in HNOg.
Evaporation and ignition.
BaCl, or Ba2N0s.
AgNO,.
Incineration.
H,S.
BaCl, or Ba2No,.
AgNO, and HNO,.
Albumen.
FeSo4 and H,S04.
Corrosive Sublimate.
Evaporate and ignite.
FeS04.
H,S.
Incineration.
HjS.
CaS04.
Ammonia Oxalate^
41 i(
Indneration.
Incineration.
AgNOa.
Iodine.
Boiling- point and 0p. Gr.
Sp. Gr.
Opalescence on dilution.
Anhydrous CUSO4.
Boiling-point and Sp. Gr.
Yellow or Red Prussiate*
Digiti
ized by Google
186
THE CHEMISTS' MANUAL.
NAXB or FBBPARATIOir.
•i
Ammonia Benzoas
Ammoniffi CarbonaB.
Ammonis Chloridam..
Amylum <
Antimoniam Nigrum.
AntimoDii Oxidum. . . .
Antimoniam Tartrate.
Aqua Aurantic Floris.
Aqua Distillata .
Argenti Nitras .....
Argenti Oxidam -I
Argentum Porificatom
Atropia
AtropisB Sulphas
Balsamum
num . . . .
Peru via-
Beberiae Sulphas. .
Bismuth Carbonas. .
Bismuth Subnitras. . ^
Bismuthum Purifica-)
turn )
Borax
Bromum .
\
Oadmii lodidum. .
Calcii Chlpridum. . . .
Calcis Carbonas Pre-
cipitata.
Calcis Phosphas. . .
Fixed Salts
Fixed Salts
Ammonium Sulphate.
** Chloride.
Fixed Salts.
Alkaline Matter
Acid Matter
Silica
Higher Oxides of Sb..
General
Pb.CuSn
Fixe<i Salts
Sn, Pb, and Cu
Calcium Salts
Chlorides
Sulphates
Carlmnates
Other Nitrates, etc. . .
Metallic Silver
General
Copper
Mineral Matter
Mineral Matter
Fixed Oil...
Alcohol
Mineral Matter
Bi3N0, or NH^NOg.
Lead Carbonate. . . .
Oxychloride of Bi . . .
Oxy nitrate of Pb
Oxychlorideof Bi...
Copper.
General
General
Iodine
Zinc Iodide..
General (
Ca Hypochlorite
Carbonic Oxide
AlgOa.FeO and Phos-
phates
' Chlorides.
I Carbonate of Ca
I Alumina
Sand
Calx.
j I Carbonate of Ca .
j| Al.^Oa, FeO. et<;.
Calxchlorata | General
Cambogia Starch
Non-volatility.
Non-volatility.
BaCl, orBa2NO,.
AgNO,.
Non-volatility.
Red Litmus.
Blue Litmus.
Insoluble in HCL
Tartrate of K.
Quantitative Analysis.
H,S.
Evaporation and Ignition.
HgS.
Ammonium Oxalate.
AffNO,.
BaCl, orBa2N0,.
Lime Water.
Quantitative Analysis.
Effervescence with HNO,.
Quantitative Analvsis.
NH4HO to HNO, 'solution.
Incineration.
Incineration.
Invisibility with Alcohol.
Non-diminution of volume
when mixed with Water.
Incineration.
Indigo Sulphate.
Dilute H-SO4.
AgNO,.
Dilute H.SO..
AgNO,.
NH4HO to HNO, adntion.
Quantitative Analysis.
Sp. Gr. Boiling-pomt.
Starch.
EHO in excess, then snl-
phydrateof NH4.
Quantitative Analysis.
Quantitative Analysis.
HCl.
Saccharine solution of OaO
to solution in HNO..
AgNO, -I- HNO,.
Efiervesces with Adds.
Solution of Potash.
Insoluble in Acids.
Effervesces with Acids.
Saccharine solution of Lime
to solution in Acids.
Quantitative Analysis.
Iodine (green).
Digiti
ized by Google
THE CHEMISTS MANUAL.
187
HAXB or PKBPAKATIOM.
Camphora
Carbo Animalis Puri-
ficatus
Carbo Ligni
Catechu Pallidum. . .
Cera Alba
mpUBITUB.
Fixed Salts .
Earthy Salts.
More than i
Starch
Soft Fats. .
Soft Fats. .
JAsh.,
CeiaFlaTa.
CeriOxalas.
Gataoeum. . .
Chloiof orm .
Oopaiba
Creasotnin . . . .
Capri Sulphas.
Elatrium.
Fel Bovinum PurifiO
catum )
Ferri Arsenias ]
Ferri Carbonas Saccha-
lata
Ferri et AmmoniflB
atias
Ferri et Qainie CStras -j
Ferri Oxidum Magneti-
cum
Ferri Peroxidum Hu-
midum
Ferri Phoephas a
Ream ]
Flour I
Carbonate and Oxa- {
lates J,
Alumina ( ;
w
General.
Soft Fats
General
Hydrocarbons
Non-volatile matter. . ,
Wood oa.
Carbolic Add.
Ferrous Sulphate.
Chalk. . .
General.
Mucus, crude bile. . . .
Sodium Sulphate....
General
UNH,).SO,
(General
Tartrate of Fe and
NH4
General
EorNa Salts
K or Na Salts
General
Other Alkaloids y
( Metallic Iron
/ General
j Ferrous Hydrate —
{ Ferric Oxy hydrate. .
Ferri Arsenias -j
General
Non-volatility.
Incineration by help of red
oxide of Hg.
Incineration.
Iodine.
Melting point.
Melting point.
Soluble m Alcohol.
Insoluble in Turpentine.
Iodine.
Ash, soluble in acids with
effervescence.
Ins. of Hydrate in NH4HO.
More or less of 48 per cent.
Ash.
Melting point.
Specific Gravity.
Sulphuric Acid.
Residue on evaporation.
Gelatinous at 270^ F.
Incomplete sol. in Benzol.
Oxidation.
Non-vol. at 212'' F.
Dextro rotation of Polar-
ized ray.
Crystallization on cooling.
HNO, and NH^HO.
Effervesces with Acids.
Quantitative Analysis.
Incomplete sol. in Spirit.
Baa, or Ba2N0,.
Quantitative Analysis.
Baa^ or Ba2N0j,.
Quantitative Analysis.
Ebullition with KHO and
saturated with HgO.A =
KHC,H,Oe.
Quantitative Analysis.
Alkalinity of Ash.
Alkalinity of Ash.
Quantitative Analysis.
Insolubility of precipitated
Alkaloid in Ether.
Effervesces with Acids.
Quantitative Analysis.
Acid solution.
Insol. in cold, dilute HCl.
Slip of Cu in Acid solu-
tion.
Quantitative Analysis.
Digitized by VjOOQIC
188
THE CHEMISTS' MANUAL.
HAXB OF FBSPABATION.
Ferric Sulphas
Ferri Sulphas
Granulata
Ferrum Radactum.
Ferrum Tartaratum.
Glycerinum.
Hydrargyri lodidum)
Rubrum f
Hydrargyri lodiduiu)
Viride
Hydrargyri Oxldum i
Rubrum
Hydrargyri Subchlo-
ridum
Hydrargyri Sulphas .
Hydrargyrum
Hydrargyrum Ammo )
niatum )
Hydrargyrum Cum )
Creta )
lodum .
JalapsB Resina.
Llmonis Succus...
Liquor Ammonise.
Liquor Ammonise
Fortior
Liquor Autimonii Chlo-
ridi
Liquor Arsenicalis
Liquor Arsenici Hydro-
chloricus
Liquor Bismutlii et
AmmonisB Citrate. . .
Liquor Calcia
Liq. Calcis Chloratae. )
Liquor Calcis Saccha- >
ratus )
ZMPURXTIK0.
r Ferric Ozysulphate.
i Ferric Compounds. \
[Copper, &c
Less than 50;^
Ferrous Compounds..
Ammoniacal Salts.. . .
General
General .
Fixed Salts.
Red Iodide. .
Fixed Salts. Nitrate)
of Mercury J
Corrosive Sublimate..
Fixed Salts
Insoluble in H.O.
Precipitate of S in aqaeowi
solution by H.S.
H,S.
Quantitative Analysis.
Red Prussiate to Acid boL
Soda.
Quantitative Analysis.
Specific Gravity.
Non-volatility.
Insoluble in Ether.
Non-volatility. Orange vft-
por on heating in tube.
Treatment with Ether.
Non-volatility.
Fixed Salts , Non-volatility.
Pb, Sn, Zn, Bi, Cu .
Fixed Salts
Mercuric Oxide.
Fixed Salts
Cyanide of Iodine
General
Resin .
of
atric)
Deficiency
Acid...
General .
General impurity or
deficiency
(NHJ.CO,
Calcium Salts
Iron Salts
Sulphur Salts
NH,a
(NH,)«SO,
General impurity )
or deficiency. . . . )
Non-volatility.
Non-volatility.
Stannous Chloride to eola-
tion in HCl.
Non-volatility.
Physical characteristics^
Quantitative Analysis.
Soluble in Turpentine.
Quantitative Analysis.
Sp. Gr. and Quant. AnaL
Sp. Gr. and Quant. AnaL
Lime Water.
Oxalate of Ammonia.
Sulphydrate of Ammonium.
Ammonio Sulphate of Cop-
per.
AgNO, to Acid solution.
BaCI, to Acidified solution.
Specific Gravity and Qoan^
titative Analysis.
Quantitative Analysis.
General impurity or ( Specific Gravity.
Deficiency in strength
eneral impurity or ( .
deficiency ) Quantitative Analysis..
Digiti
ized by Google
THE CHEMISTS' MANUAL.
189
Liquor Chloii.
Liquor Ferri Perchlo-
rideFort
Liquor Ferri Pemi-
trates
Liquor Ferri Persul-
phates
Liquor Hydrargyri )
Nitric Acid J
Liquor Lithis Effer- {
veaceDB )
Liquor Magnesia Car-
bonae
Liquor Plnmbi Sub-
aoetatis
Liquor PotaaeflB .
Liquor Potasne Ef-
fenrescens
Liquor Sod» •*
Liquor Sodse Chlo-
rate
Liquor Sods Effer-
veBoena
Litlu» Carbouas .
Lithi»Citras
Magnesia.
Magnesia Levis.
Magnesia Carbonas.
Magnesia Carb. Levis 1
uunnaTin,
Qeneral quality
Fixed matter
Deficiency in strength
Ferrous Salts
► General impurity >
or deficiency.... f
Deficiency in strength
Mercurous Salts
General impurity or /
deficiency^ (
Other Mg Salts j
General impurity or )
deficiency f
General impurity or i
deficiency )
General impurity or i
deficiency J
K,ro,
Calcium Salts
Silica....
More than
traces of
Sulphates
Chlorides
^Alumina.
Deficient in strength.
Na Bicarbonate
Gen. imp. or def. ....
Calcium salts
Na.CO,
More [Silica
than J Sulphates. . . .
traces I Chlorides. . . .
of I Alumina
Saltsof KorNH^...
Gen. imp. or def
Calcium salts. .......
Deficient in strength.
Gen. imp. or def
Calcium salts
Alumina
Deficient in strength.
MgCo,
Ca2H0 orCaCOg
MgSO^ orNa,S04...
Alumina
MgS04 orNajSO^...
CaCOg
Fe,Pb, etc
Gen. imp. or def
Specific Gravity.
Residue on evaporation.
Quantitative Analysis.
Red Prussiate.
Specific Gravity and Quan-
titative Analysis.
Specific Gravity.
Specific Gravity.
Quantitative AJaalysis.
Bitter taste (MgO, or
MgSOJ.
Quantitative Analysis.
Specific Gravity and Quan-
titative Analysis.
Specific Gravity and Quan-
titative Analysis.
Effervesces Acids Ca2H0.
Oxalate of Ammonia.
\ Insoluble in Acid after
) evaporation.
BaClg or Ba2N0,.
AgNOg to Add solution.
Ammonia to Acid solution.
Quantitative Analysis.
Tartaric Acid, etc.
Sp. Gr. and Quant. Anal.
Ammonia Oxalate.
Efierves. Acids and Ca2H0.
Insol. in Acids after evap.
BaClg to Acid solution.
AgNO, to Acid solution.
Ammonia to Acid solution.
Perchloride of Pt to Acids.
Sp. Gr. and Quant. AnaL
Ammonia Oxalate.
Quantitative Analysis.
Quantitative Analysis.
Ammonia Oxalate, etc.
Lime-water, etc.
Quantitative Analysis.
Effervesces with Acids.
Ammonia Oxalate, etc.
BaCl, to Acid solution.
Ammonia to Acid solution.
BaClg to Acid solution.
HgO.O to NH4HO solution.
HgS to Acid sol. + NH^HO.
Quantitative Analysis.
Digiti
ized by Google
190
THE CHEMISTS* MANUAL.
HAXE OF FBKPABATIOK.
MagneaiaB Sulphas
•1
Manna
Mel
Morphiffi HydrocliJo- (
rafl t
OleaDistillata.
Opium
Plumbi Acetas
Plumbi Carbonas.. . .
Potassa CauBtica. . . .
Potassa Sulphurata..
PotasssB Acetas
Potass8B Bicarbonas. . .
Potass» Carbonas. . . i
Potassse Chloras |
Potassffi Citras
PotasssB Nitras \
Potassse Permanganas.
PotasssB Sulphas j
PotassBB Tartraa )
Potass8B Tart. Adda. )
Potassii Bromidum. . j
Potassi Fenidcyanide
Potassii lodidum. ... J
Quinie Sulphas \
Rhei Radix
CaSo.
FeSO^
Genend impurity. . . .
Deficiency of Mannite
Starch (flour)
General impurity. . . .
Fixed oiL
Alcohol
Deficient in Morphia.^
General
PbS04, BaS04, or)
Silicates )
Calcium (chalk) \
More than j Chlorine .
traces of (Sulphate.
Gen. imp., H^O. etc. .
Excess of Carbonate )
or Sulphate )
Fe,etc
K.CO, j
General
More (Silicates...
than -< Sulphate . .
traces of (Chloride.. .
General
KCl
CaCl,
General
»::::::::::::::
General.
KHSO4
CaS04
General
Free Bromine
KI ,
General
Ferrocyanide of K. . .
lodateof K
Ka
K.CO.
Salidn...
General. .
Ammonia Oxalate.
Chlorinated NaO.
Quantitative Analysis.
Quantitative Analysis.
Iodine.
Quantitative Analysis.
Permanent greasy stain on
paper.
Loss in volume on shaking
with water.
Quantitative Analysis.
Quantitative Analysis.
Insoluble in Acetic Acid.
Ammonia Oxalate, after re-
moving the Pb.
AgNOs to Acid solution.
BaCl, to Acid solution.
Quantitative Analysis.
More than 25^ insoluble
in Spirit.
Ammonium Sulphydrate.
Effervesces with Acids. In<
sol. in Spirit. Alkalinates.
Quantitative Analysis.
Insol. in Acids after evap.
BaCl, to Add solution.
AgNO, to Acid solution.
Quantitative Analysis.
AgNO,.
Ammonia Oxalate.
Quantitative Analysis.
BaCl,.
AgNo,.
Quantitative AnalyslB.
Test Paper.
Ammonia Oxalate.
Quantitative Analysis.
Odor.
Chlorine Water and Stardu.
Quantitative Analysis.
Ferric Salt.
HgO.T and Starch.
AgNO,, etc.
S^c. solution of Lima
H.SO^.
Quantitative Analyris.
Turmeric I Boracic Add.
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THE CHEMISTS' MANUAL.
191
KAVS OF PRgPABATIOW.
Sods Sulphas
SocUb Yalerianas.
Santoninum -|
Sapo Dams.
Sapo Mollis
Scammonis Resina . .
Scammonium
Smapis
Soda Caustica i
Soda Tartaiata
Sods Acetas
SodsB Anezuas
Sod» Bicarbonas . . .
Sode Hyposulphic . .
Sods Nitraa
Sods Phospbas ....
Spiiitus iBtheris Ni-
trosi
Spiiitiis Ammonio'
Atomat
Spiritiis ChloTofor-
mii
Spiiitus Tenoior . .
Strychnia
Spiritns Bectificatas.^
mPUKlTlEB.
Mineral Matter
Earthy, Soap, etc
Oil
K compounds
Earthy, Soap, etc. . . .
Oil
Resin of Guaiacum. . .
Resin of Jalap
CaCo.,MgCO,
Starch (flour)
Starch (flour)
More than j Chloride.
traces of J Sulphate.
Gen. imp., Water, &c.
General
Acid or Alkaline imp.
Na,S04 or CaSO^
NaClorCaO,
Excess of H,0 of)
crystallization. . . . )
General
Na.CO,
More than J Chlorides
traces of ( Sulphates
General
NaCl
Na,SO.
More than traces of )
Sulphates )
Def. of H,0 of crys- [
tallization or excess )
Ammonium Salts. . . )
Ferric Salts )
General
NaOorNa,CO, j
General
More than trace of Add
Free Add
Defidency of Nitrite of
Ethyl
General
Gen. (excess of HgO).
Brucia
Mineral Matter
Gen. (excess of H,). . .
Resin or Oil
More than trace of)
Fusel OU \
Indneration.
Insoluble in Spirits.
Oil stain. Paper.
Deliquescence of Ash.
Insoluble in Spirits.
Oily stain. Paper.
Inner surf, of potato paring.
Insoluble in Ether.
Eifervesces with Acids.
Solution of Iodine.
Solution of Iodine.
AgNOj to Acid solutions..
BaCl, to Acid solutions.
Quantitative Analysis.
Quantitative Analysis.
Test Paper.
Baa, to Acid solution.
AgNOg to Acid solution^
Quantitative Analysis.
Quantitative Analysis.
Mercuric Chloride,
AgNOg to Acid solution^
BaClt to -^ci^l solution.
Quantitative Analysis.
AgNO..
Baa, or Ba2N0a.
BaCl, to Add solution.
Quantitative Analysis.
Solution EHO heated.
Quantitative Analysis.
Test Paper.
Insoluble in Spirits.
Sp.Gr.
Effervesces with Bicarbon^
ate of Soda.
More than feeble eflferves.
( with Bicarb, of Soda.
[ Quantitative Analysis.
Spedfic Gravity.
Specific Gravity.
Nitric Add.
Indneration.
Specific Gravity.
Opalescence on dilution*
AgNO,.
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192
THE CHEMISTS' MANUAL.
KAXB OF PBIPABATIOK.
DCPUBITIBB.
Sulphur Predpitatum.
Sulphur Sublimatum
Sulphuris lodidum.. . .
Syrupi
Tamarindus. .
Veratria
Zind Acetas.
Zind GarbonaB.
Zind Ghloiidum . . .
Zind Ozidum.
Zind SulphaB
Zind Valeiianas. . . .
CaSO^
Earthy Matter
HjS04orH,S08....
Sulphide of Arsenicum
Dendency of Iodine...
Defidency of Sugar. . .
Traces of Cu.
liGneral Matter......
Sulphates
Chlorides
As, Cd, Cu, Pb
Acetate of Iron
Copper Acetate
Chlorides
Sulphates
Copper Carbonate. . . .
As.Cd, Cu, Pb
Sulphates
CaClj
FeCl,
Fe.Cie
ZnCO,
Na,s64 or ZnSO^ . . .
ailorides,
Copper Oxide
As, Cd, Cu, Pb
Iron Sulphate
Copper Sulphate
ZnSO^
Butyrate of Zinc
(Appear, under microeoope
j — residue on ignition.
Indneration.
Litmus-paper.
Ammonia.
Quantitative Analysis.
Spedfic Gravity.
Iron.
Incineration.
Baa, orBa2NO,.
AgNO,.
HNO.+NH^HO.
NH.HO.
AgNO, to Add solution.
BaCls to Add solution.
NH.HO to Acid solution.
H S
BaCi, or Ba2N08.
Ammonium Oxalate.
Ferridcyanide of K.
Ferrocyanide of K.
Effervesces with Acids.
BaCl, to Add solution.
AgNO, to Add solution.
NH.HO to Add solution.
H.S.
Tincture of Galls.
CuSO^ add NH.HO.
BaHg or Ba2N0,.
Acetate of Cu, etc.
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THE CHEMISTS' MANUAL. 193
INFLUENCE OF FIXED ORGANIC SUBSTANCES ON THE
PRECIPITATON OF METALLIC OXIDES FROM
SALINE SOLUTIONS BY ALKALIES,
The following results have been obtained by H. Grothe
(J. pr. Chem., xcii. 175) : 1. The alteration produced in the
reactions of different metallic solutions with alkalies by the
presence of fixed organic bodies, exhibit great diversities,
scarcely any two metallic bodies being similarly affected ; so
that these alterations do not afford properties characteristic
of groups of metallic oxides, but rather of individual oxides.
2. Of non-volatile organic substances, citric acid acts most
strongly in modifying these reactions ; then follows tartaric
acid ; then sugar, starch, and gum, which, however, act but
feebly, and require to be added in large excess. 8. The pre-
cipitating action of ammonic hydrate is diminished by these
bodies much more than that of sodic carbonate. 4. Solutions
which are not precipitated in presence of fixed organic bodies
by alkaline hydrates or carbonates, are for the most part pre-
cipitated by alkaline orthophosphates, pyrophosphates, arse-
nates, and borates. 5. Sodic orthophosphate may be used as
a reagent in nearly all the cases in which the precipitation of
a metallic oxide is hindered by the presence of non-volatile
organic substances.
The following table exhibits the reactions of the more im-
portant metallic salts with ammonic hydrate, and with sodic
carbonate, borate, phosphate, pyrophosphate, arsenate, and
borate, in presence of tartaric acid, citric acid, and sugar:
p denotes perfect precipitation ; i, imperfect precipitation ; a
clash, no precipitation :
13
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194
THE CHEMISTS' MANUAL.
II
S'SL
OS
It
•28
5"
1
1-
I--
—
—
P-
p.
i.
i.
p.
p.
—
P-
1.
1.
p.
1.
p.
P-
p.
p.
p.
p.
—
P-
P-
1.
—
p.
1.
p.
p.
1.
P-
P-
1.
1.
p.
p.
—
1.
p.
P-
p.
p.
P-
1.
p.
—
—
1.
—
i.
i.
i.
i.
i.
I
i.
—
i.
i.
i.
i.
i.
i.
i.
—
p.
P-
p.
i.
i.
P-
P-
—
p.
P-
P-
~~
~~
p.
P-
—
P-
p.
p.
—
—
P-
1.
i.
p.
]*•
P-
—
1.
P-
p.
1.
P-
P-
p.
—
p.
p.
P
1.
P-
p.
p.
1.
p.
P-
P-
—
i.
P-
P-
—
p.
p.
p.
—
p.
p.
p.
i.
I
P-
P-
p.
p.
P-
P-
p.
p.
p.
p.
p.
p.
p.
P-
P-
I.
I
Aluminium Salts.
Manganous Salts. .
Manganic Salts...
Zinc Salts.
Nickel Salts.
Cobaltous Salts. . .
Uranic Salts.
Ferrous Salts. . . . .
Ferric Salts
Cupric Salts.
Cadmium Salts. ..
Lead Salts
Bismuth Salts.
Chromic Salts.. ..
(Green solution.)
Chromic Salts
(violet solution.)
I Tci.taric Acid
•'Citric Acid
I Sugar.
I Tartaric Acid
• 'Citric Add
I Sugar.
Tartaric Acid
-Citric Acid
Sugar
I Tartaric Acid
•Citric Acid
I Sugar
I I Tartaric Acid
•Citric Acid
Sugar
Tartaric Acid
• 'Citric Acid
I Sugar.
I Tartaric Add
•Citric Acid
I Sugar
r Tartaric Acid
■ Qtric Acid
I Sugar.
I'Sugar.,
I Tartaric Acid. .
• 'Citric Add ..
I ' Sugar
Tartaric Add..
• Citric Acid....
I Sagar
Tartaric Acid..
• I Citric Acid
I Sugar
Tartaric Add. .
■Citric Acid....
I Sugar
Tartaric Acid..
i Citric Acid
Sugar
Tartaric Acid. .
Citric Acid ....
Sugar
Tartaric Acid.
Citric Add. .
p.
p.
P-
P-
p.
p.
p.
P-
p.
P-
?:
i.
i.
i.
i.
P-
P-
p.
P.
P-
V'
p.
p.
P-
P-
P-
P-
P-
P-
i.
p.
p.
P-
P-
P-
p.
P-
P-
P-
p.
P-
^.
i.
L
L
L
P-
p.
P-
P-
p.
P-
P-
P-
P-
P-
P-
p.
P-
P-
p.
P-
P-
P-
Digiti
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|Uqi;, ln.l,>i>.
Digiti
ized by Google
196
THE CHEMISTS' MANUAL.
UJ
Q-
Q.
^
ad
3
U
ill
s
X
w
1-
H
Ul
^
tr
m
o
P
CO
^
PE3
g
OQ
s
o
I
UJ .
X X
I- 0 QQ
Q < 9
«? a
h- o PS
z . o
Ld n. «
" I
Ld M
Ll. PP
O Q
pi]
</) H
C/) H
UJ OS
I- »
o ^
o
<
cc
<
X
o
^
i .1 .iiii s
Ot3
l8l
J22
•5 Q Q
fl o o
c, ^ o
o o o •
a a fl ja ^ j3 "S
I
i
1
-2 b» b * b
i
1^6
«2 .
8 :8
l8
§
fl fl
^88
^ i i
o o o
V O) V
fe o "S "S ^
1
o
>-^
9i
ft,
PQ
3
S
1
1^
a
1
1 +
5
Q
ntube)
tiibe)B
BW.
I QQ
'•s
^ fl ^ ^ti
O M O O "»•
'C _ ts "^ 5
9 9 fl fl 4»
ft, SDft,Ct,ft,
m
6 SpqE
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THE CHEMISTS' MANUAL.
197
&"25 Sog tl S^^ I
P.P.5 5 5 o4
§§1111-
'8:2'^-^
* « © © g^
rhl!!llli
"3*3^ © © — " -'>■
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198
TABLE OF VOLATILE ELEMENTS
FROM WATT'S DICT.
Mbtallzo Film.
OZIDB-FIUI.
OXIDB-FILM
WITH
Stamnovs
Chlobzdb.
OZISB-FIUE
Stannoub
Chloudb
AND Soda.
OZIDB-FILM
WITH
Abobntio
NiTBATB ABB
Ajemobla.
Te.
Black;
thin part brown.
White.
Black.
Black.
YeUowiBh.
white.
8e.
Chenrred;
thin part brick red.
White.
Brick-red.
Black.
White.
Sb.
Black;
thin part brown.
White.
White.
White.
Black;
insoluble in
Amm3niA.
Ab.
Black;
thin part brown.
White.
White.
White.
Lemon-yellow or
reddish-brown;
soluble m
Ammonia.
Bi.
Black;
thin part brown.
YellowlBh-
white.
White.
Black.
White.
Hit.
Gray;
non-coherent thin
film.
Fe.
Black;
thin part brown.
White.
White.
White.
White.
Pb.
Black;
thin part brown.
Yellow-ochre
color.
White.
White.
White.
Cd.
Black;
Blacki$>h.
brown ; thin
part white.
White.
White.
White ; in the
thin part tarns
bloish-black.
Zn.
Black;
thin part brown.
White.
White.
White.
White.
Sn.
Black;
thin part brown.
YellowiBh-
white.
White.
White.
White.
Digiti
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199
WHICH CAN BE REDUCED AS FILMS.
OF CHEMISTRY.
lOMDI-nLM.
Iodide-film
Sttlphidx-filx.
WITH AXXONIO
SULFHIDS.
Bbmabks.
Brown ;
disappears for a time
Disappears
altogether on
blowing.
Black to
blackish-brown.
Disappears
for a time.
Brown;
does not wholly dis-
appear on breathing.
Does not
disappear on
blowing.
Yellow to
orange.
Orange and
then disappears
for a time.
Element!
whose reduc-
tion-films
are scarcely
' dissolved in
dilute
Nitric Add.
Orange-red to yellow ;
disappears
on breathing.
Disappears
altoeetner on
blowing.
Orange.
Disappears
for a time.
Orange-yeHow ;
disappears Tor a time
on breathing.
Disappears
altogether on
blowing.
Lemon
colored.
Does not
disappear.
Blnish-brown ;
^, thin parts pink ;
disappears for a time
on breathing.
Pink to orange ;
chectnnt
colored when
blowing.
Burnt nmber
color to
coffee color.
Does not
disappear.
Elements
^nnine-colored and
iemon-yellow ;
Qoe« not difiappear on
breathing.
Disappears
for a tfme on
blowing.
Black.
Does not
disappear.
whose rednc-
tion-fllma
are with
■ difficulty
dispolved in
dilute
Nitric Acid.
J
t
Lemon-yellow ;
oeK not disappear on
breathing.
Does not
dlHappear on
blowing.
Black;
thin parts
blnlsh-gray.
Does not
disappear.
1
Oi^nge-ycllow to
lemon color;
■^s not diwippear on
breathing.
Disappears
for a time on
blowing.
Brownish-red
to black.
Does not
disappear.
White.
White.
Lemon
colored.
Does not
disappear.
Elements
whose rednc-
tion-fllms
' are instantly
dissolved In
dilute
Nitric Acid.
U
White.
White.
White.
Does not
disappear.
I
"Yellowish-white.
Yellowish-
white.
White. Does not
' dl^»appcar.
I 1
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200 THE CHEMISTS* MANUAL,
SCHEME* FOR THE QUALITATIVE DETERMINATION OF
SUBSTANCES BY THE BLOWPIPE.
The substance may contain As, Sb, S, Se, Fe, Mn, Cu, Ni,
Pb, Bi, Ag, Au, Hg, Zn, Cd, Sn, CI, Br, I, CO^, SiOj, HNO3,
HgO, etc. ^
1. Treat on Ch (charcoal) in the O.F. (oxidizing flame) to
find volatile substances such as, As, Sb, S, Se, Pb, Bi, Ag, Zn,
Cd, etc. (p. 66, et seq.) [This number, and all others, refer to
the pages of Plattner's Manual, translated by H. B. Gomwall,
1872. Owing to the additions to this scheme, as also Casa-
major's table on the preceding page, reference to Plattner's
Manual will be unnecessary.]
a. If there are volatile subBtances present, form a coating and test it
with S.Ph (salt of phosphorus) and tin on Ch for Sb (p. 99), or to distin-
guish between Pb and Bi (p. 280).
b. If there are no volatile substances present, divide a part of the
substance into three portions and proceed as in A.
a. Yellow coat, yielding with S.Ph a black bead; disappearing with
blue flame, no part of it yielding green Sb flame ; Pb and Bi.
b. Yellow coat, generally with white border, yielding black or gray bead
with S. Ph, disappearing with blue flame ; also the border disappearing
with green flame ; Pb and Sb.
c. Yellow coat, very similar to b, but yielding no blue flame ; Bi and Sb.
(See note at end of Scheme.)
3. If As, Sb, S, Se are present, roast a lai^ quantity
thoroughly on Ch (p. 77). Divide the substance into three
portions and proceed as in .4.
A. Treatment of the First Portion. — Dissolve a veiy
small quantity in borax on platinum-wire in the 0. F. and
observe the color produced. Various colors will be formed
by the combination of the oxides. Saturate the bead and
shake it off into a porcelain dish ; repeat this once or twice
(p. 79).
a. Treat these beads on Ch with a small piece of lead, silver or gold In
a strong R. F. (reducing flame), p. 113.
* Scheme is by T. Egleston, E. M., with a few additions by Author.
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THE CHEMISTS' MANUAL. 201
h. Fe, Mn, Co, etc., remain in the bead (p. 115).
If the bead spreads out on the Ch, it most be collected to a globule by
continued blowing.
Hake a borax-bead on platinum-wire and dissolye in it some of the
frag^MnU of the head, reeerring the rest for accident.
c. Ni, Cu, kg, Au, Sr\, Pb, Bi are reduced, and collect bj the lead-button
(p. 115).
BemoTe the lead-button from the bead while hot, or by breaking the
latter, when cold, on an anvil between paper, carefuUj preserving all
the fragments.
d. If Co is present the bead will be blue.
If a large amount of Fe is present, add a little borax to prove the presence
or absence of Co (p. 222).
If Mn is present, the bead, when treated on platinum- wire in the O.F.,
will become dark- violet or black.
e. If no Co is present, the bead will be almost colorless.
Look here for Cr, Ti, Mo, U, W, V, Ta. Mo will give a cloudy -brown or
black with the borax-bead in the R. F., owing to the molybdic acid being
reduced.
/. Treat the button « on Ch in the 0. F. until all the lead, etc., is driven
off, Ni, Cu, Ag, Au remaining behind ; or separate the lead with boradc
acid (p. 442).
g. Treat the residue ^ on Ch in O.F. with S.Ph bead, removing the but-
ton while the bead is hot.
A. If Ni and Cu are present, the bead will be green when cold (p. 292).
If Ni only, yellow. If Cu only, blue.
Prove Cu by treating with tin on Ch in R.F. (p. 298).
i. For Ag and Au, make the special test No. 8.
B. Treatment of the Second Pobtion. — Drive off the
voktile substances in the O.F. on Ch. Treat with the R.F, or
mix with soda, and then treat with R.F. for Zn, Cd, Sn. If a
white coating is formed, test with cobalt solution (pp. 251, 256,
276). Tin gives greenish-blue ; zinc, green. If Zn is found,
it is not necessary to look for Sn and vice versa^ as they very
rarely occur together. Cd gives a brown coat and variegated
tarnish.
C, Treatment of the Third Portion. — Dissolve some of
the substance in S.Ph on platinum-wire in O.F., observing
whether Si is present or not, and test for Mn with nitrate of
potassa and soda (p. 210).
3. Test for As with soda on Ch in the R.F., or with dry soda
Digiti
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202 THE CHEMISTS* MANUAL.
in a closed tube (p. 345 et seq.). On charcoal it gives garlic
odor ; in the tube, a metallic mirror.
4. Dissolves in S.Ph on platinum-wire in the O.F. (if the sub-
stance is not metallic and does not contain any S), and test
for Sb on Ch with tin in the R.F. (See 1, a, p. 99.)
6. Test for Se on Ch ; it gives a horse-radish odor (p. 368).
6» In absence of Se, fuse with soda in the R.F., and t^st for
S on silver-foil (p. 365). By moistening the fused mass, and
letting it stand on the foil, the latter turns black if S be pres-
ent. In the presence of Se, test in open tube (p. 366).
7. Test for Hg with dry soda in a closed tube; a metallic
mirror is formed (p. 304).
8. Mix some of the substance with assay lead and borax
glass, and fuse on Ch in the R.F. (p. 401). Cupel the lead-
button for Ag (p. 407). Test with nitric acid for Au, dissolv-
ing the silver (p. 320).
9. Test for CI and 1 with a bead of S.Ph saturated with
oxide of copper. CI gives blue flame; I, intense green (pp.
373, 374, 375).
10. Test for Br with bisulphate of potassa in a matrass,
gives brownish-yellow fumes ; test also for CI (p. 374).
11. Test for H2O in a closed tube ; drops collect on the in-
terior (p. 353).
13, Test for borates : dip substance in glycerine and hold
in flame — ^green color. If barium is present, remove the same,
then apply the test. Discovered by Mr. lies. (See Amer.
Chem., Apr. 1876.)
13. Test on platinum-wire, or in platinum-pointed forceps,
for coloration of the flame (p. 72 et seq.).
14. Test for CO2 with hydrochloric acid, letting the gas
pass over lime-water (p. 360).
15. Test for HNO3 ^^^^^ bisulphate of potassa in a matrass;
yellow-colored fumes and acid reaction (p. 354).
16. Test for Te in an open tube; forms a grayish-white
sublimate, which fuses to clear transparent drops when strongly
heated. Te burns with a bluish-green flame (p. 354).
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THE CHEMISTS' MANUAL. 203
DETECTION OF BISMUTH IN THE PRESENCE OF LEAD
AND ANTIMONY.
By H. B. CORNWALL, E. M.
One part teroadde of Uamuth^ fifty parts oxide of lead^
and fifty parts teroxide of omUmony are mixed with an
equal volume of sulphur, and treated B.B. in a deep cavity on
coal with the blue flame for a few minutes. The resulting
fused sulphides remove to a flat coal, and treat alternately
with O.F. and R.F. until the antimonial fiimes cease to come
off, and an impure blue lead flame appears. Powder the
residue and treat a portion of it with iodine mixed on coal.
No bismuth will be detected. But if the other portion is
treated in an open tube (4 in. long and not less than J in.
wide, over a Bunsen gas-burner) with a mixture of 6 parts
sulphur and 1 part iodide of potassium by weight ; and about
equal volumes of this and of the metallic oxide, a distinct bis-
muth sublimate will be formed about one-third of an inch
above the lower edge of the yellow sublimate.
The bismuth sublimate forms a red ring. If sulphides are
under treatment, remove the excess of antimony on coal.
Care must be taken not to confound with the bismuth sub-
limate a sublimate of iodine, which may condense on the upper
part of the tube, but at a greater distance from the assay.
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\^t,^i^t^ Irattitip.
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DETERMINATION OF SPECIFIC GRAVITIES.
SPECIFIC GRAVITIES OF POWDERS OR SMALL SOLIDS.
(Brand and Tajfior'a Chemistry,)
The specific gravity of solids in powder or im, small pieces
may conveniently be determined by the bottle. Thus : weigh
the powder, pour it into the bottle, and fill it with water at
62° F., taking care to dislodge all adhering bubbles of air.
Then weigh it and deduct the known weight of the bottle j
the remainder is the conjoint weight of the powder and water.
Deduct fi-om this last sum the found weight of the powder,,
and the difference is the weight of the water ; deduct this dif-
ference irom the known weight of the water required to fill
the bottle, and the remainder is the weight of a volume of
water equal to the volume of the solid in powder ; then as this
18 to the known weight of water, required to fill the bottle
: : Sp. Gr. water : Sp. Gr. powder. Example :
Grains.
Weijfht of water iu the bottle 1000
" of natiye platinam grains (in air) 40
1040
Weight of water and platinam in bottle 1087.5
Difference = Volame of water displaced 2.6
40 -I- 2.5 = 18 Sp. Gr. of native platinum.
When the substance is soluble in water, another liquid of
known specific gravity which does not act upon the solid,,
must be employed. Alcohol, oil of turpentine, or olive oil
may be used, or, in some cases, the substance may be coated
with varnish. Example — Eequired Sp. Gr. of Sugar :
Graing.
Weight of sugar in air 400
*• " " in oil of turpentine 182.5
Weight of an equal bulk of oil 217.5
Known Sp. Qr. of turpentine 0.870
Then 0.870 : 1000 : : 217.5 : 250, and 400 -r- 250 = 1.6,
which is the Sp. Gr. of the sugar.
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308 THE CHEMISTS' MANUAL.
SPECIFIC GRAVITY OF SOLIDS HEAVIER THAN WATER.
{Brcmd and Taylor^ b Chemistry,)
Weigh the solid in air, then suspend it by a fine thread
(horse-hair) to one arm of a balance ; exactly counterpoise it,
and immerse the solid so counterpoised in distilled water at
62° F., and note how much less it weighs now than when
weighed in air. The diflference between the two is the weight
of a volume of water, exactly equal to that of the immersed
solid. Divide the weight of the solid in air by this differ-
ence, and the result is the Sp. 6r. of the solid. Thus in refer-
ence to a small bar of aluminum :
OralDB.
Weight of Alnminum in air 48.8
** of " in water 29.0
Difference = Volume of water 17.8
46.3 -I- 17.3 = 2.6 Sp. Or. of Aluminum.
A knowledge of the Sp. Gr. of solids enables a chemist to
ascertain the weight of bodies from their volume. A cubic foot
of water contains 1728 cubic inches, and weighs 1000 ounces
(strictly 998 ounces 62.4 pounds Av.) ; hence a cubic foot of
sulphur (Sp. Gr. 1.957) would weigh 1957 ounces, and a cubic
foot of marble (Sp. Gr. 2.5) would weigh 2500 ounces. A
cubic foot of air weighs 535.161 grains.
SPECIFIC GRAVITY OF SOLIDS LIGHTER THAN WATER.
{Brcmd and Taylor's Chemistry,)
1. Find the weight of the solid (a) in air. 2. Take a piece
of metal heavy enough to make (a) sink in water, and find its
weight in air and in water. 3. Tie together (a) and the metal,
and find the weight of the compound mass in water. The
difference between the weight of the metal in air and in water
is the weight of a volume of water equal to that of the metal ;
deduct this from the difference between the weights in air and
in water of the compound mass, and the remainder is the
weight of a volume of water equal to (a). Now divide the
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THE CHEMISTS' MANUAL. 209
weight of (a) by the remainder, and obtain the Sp. Gr. Thufl
with reference to beef-fet :
Grains.
Weight of fat in air .* 117.3
Add brass weight to sink it 1000.0
Weight of compound mass in air 1117.8
GraioB.
LoflB of weight by the compound mass in water. 245.5
" •* brass weight (1000) in water 119.4
Weight of the water displaced by the fat 126.1
Hence 117.8-4-126.1 = 0.980 Sp. Gr. of beef&t.
SPECIFIC GRAVITY OF GASES.
The weighing of the air and gas should take place at the
same temperature and pressure, or a calculation should be
made. In reference to gases and vapors, air is taken as the
standard of unity.
Gases. — A light glass flask, of about forty or fifty cubic
inches capacity is employed. This is capable of being screwed
to the air-pump plate, and of being suspended to a scale-beam
and accurately balanced. The flask is exhausted, balanced,
filled with dry air, and again balanced. The increase in weight
represents the weight of the volume of dry air in the flask, at
the pressure and temperature at which it was filled. The ex-
periment is repeated with the dry gas, the Sp. Gr. of which it
is proposed to determine. The following is the Sp. Gr. of car-
bonic oxide (COg) :
GninB.
Wdght of the flask with dry air 2aS3.8
" exhausted 2021.4
Weight of dry air in flask 12.4
Grains.
Weight of the flask with dry carbonic oxide 2040.24
'' exhausted 2021.40
Weight of dry carbonic oxide in flask 18.84
Hence, 18.84 -i- 12.4 = 1.520 Sp. Gr. of carbonic oxide.
The weight of 100 cubic inches of any gas may be found by
multiplying the specific gravity of the gas or vapor by 31 [one
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210 THE CHEMISTS' MAJ^UAL.
hundred cubic inches of dry air at a mean temperature of
(62° F.), and a mean pressure (30 inches), are considered to weigh
31 grains]. Thus, nitrogen has a Sp. Gr. of 0.967 and 0.967
X 31=29.98 grains, the weight of a hundred cubic inches of
the gas.
A knowledge of the Sp. Gr. of gases enables a chemist to
control the results of an analysis of a compound gas. Thus, if
2 volumes of ammonia consist of one volume of nitrogen and
three volumes of hydrogen, it follows that the sum of the spe-
cific gravities of its constituents, divided by 2, should exactly
represent the Sp. Gr. of the gas.
SPECIFIC GRAVITY OF VAPORS.
{BraTid and Taylor^ s Cfiemititry,)
The weights of equal volumes of vapor and air are com-
pared under the same temperature and pressure. A thin glass
globe of about three inches diameter is drawn out at its fleck
to a narrow tube, six or seven inches long, the point of the
tube being cut across with a file, but not sealed. The globe
is then weighed, and the temperature and pressure at the time
observed. In order to introduce a volatile liquid, the globe is
warmed so as to expel a portion of its air, and the end of the
tube is then dipped into the liquid. As the globe cools, the
air within contracts and the liquid is forced into it by atmos-
pheric pressure. When a suflScient quantity (fix)m 100 to
150 grains) of liquid have entered, the globe is finally enclosed
in a wire-holder, and immersed in a bath of water, oil, or other
medium, heated to 50** or 60** above the boiling point of the
liquid in the globe. Under these circumstances, a stream of
vapor rushes rapidly through the orifice, carrying with it the
air of the globe. When this ceases the point of the tube is
sealed by a blowpipe flame, the temperature being observed at
the same minute. The globe is removed from the bath, and
when cool is cleaned and weighed. The next point to be
determined is the capacity of the globe. For this purpose the
neck is broken under the surface of water or mercury, when
Digiti
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THE CHEMISTS' MANUAL. 211
the cold fluid enters the globe and fills it completely, if the
operation has been properly conducted, and all the air has
been expelled by the vapor. By pouring out the water or
mercury into a graduated vessel, the capacity of the globe is
accurately ascertained. The data necessary for the calculation
is thus obtained :
1. The weight of the globe full of air at the common tem-
perature and pressure.
2. The weight of the globe, and of the vapor filling it, at
the temperature of the batli, and under the same pressure.
3. The capacity of the globe.
Having these results, there can be obtained by calculation :
4. The weight of the empty globe.
5. The weight of the vapor filling the globe at the tempera-
ture of the bath, as well as its volume at this or at any other
temperature that may be required.
Let it be assumed that the object is to determine the specific
gravity of the vapor oi chloroform,
1. The weight of the globe full of air at 60° F. and bar. 30,
is found to be 2012.4 grains.
2. The liquid chloroform having been introduced into the
globe in the manner described, the globe is maintained at a
temperature of 200° in the bath until nothing but vapor re-
mains in the interior. The aperture of the small tube is then
sealed. The globe, when dry and cooled to 60° F., is found to
weigh 2040 grains. This gives the weight of the globe and
vapor together.
3. The capacity of the globe is determined by breaking the
point of the tube under water. The liquid rushes in and
entirely fills the vessel. When this liquid is poured into a
graduated glass, it is found that at 60° F. there are 40 cubic
inches ; hence, 40 cubic inches of air were contained in the
globe at common temperature and pressure.
4. The weight of this air would be 12.4 grains (100 cubic
inches : 31 grs. : : 40 cubic inches : 12.4 grs.), and as the globe
and air weighed together 2012.4 grains, then 2012.4 — 12.4 =
2000 grains, the weight of the empty globe.
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213 THE CHEMISTS' MANUAL.
5. The weight of the vapor filling the globe may now be
determined. The globe was found to weigh, on cooling, 2040
grains ; hence, 2040 — 2000 = 40 grains, the weight of the
vapor. It is now necessary to determine either the weight .of
the air which would fill the globe at the temperature of the
bath, or the volume of vapor which, by calculation, would be
contained in the globe when cooled to 60** F. The reduction of
the volume by cooling from 200° F. to 60° F. is the more sim-
ple process. Thus 40 cubic inches at 60*^ F. (648 : 508 : : 40 :
30.78). According to Gay-Lussac, 1000 volumes of air at
32° are increased to 1375 volumes at 212° F. Hence, the
increase is |Jf or 2.08, for each degree between 32° F. and
212° F.; and 1000-5-2.08 = 480. Hence, the increase for
each degree is equal to l-480th part of the volume at 32° F. ;
or, assuming that the volume of gas at this temperature is 480
cubic inches, there will be an addition of one cubic inch for
every degree of increase of temperature up to 212° F.
The mean temperature is taken at 60° F., and 480 cubic inches
at this temperature would become (60 — 32 -f 480) 508 cubic
inches. The number 32 is deducted from the temperatures,
because it is from this degree (32° F.) that the rate of expan-
sion, on which the calculation is based, commences. Hence,
assuming that chloroform vapor was cooled to 60°, and could
still exist as vapor at that temperature, it is obvious that its
specific gravity would be determined by ascertaining the
weight of 30.78 cubic inches of air at the same temperature
and pressure. 100" cubic inches of air weigh 31 grains ; hence,
100 : 31 : : 3078 : 9.54. Hence, at the same temperature, 60°,
30.78 cubic inches of chloroform would weigh only 9.54 grains ;
and 40 ~- 9.54 = 4.19, which is nearly the specific gravity of
the vapor of chloroform, as determined by calculation from its
elementary composition. The following is a summary of the
results:
Capacity of the globe at 60** =40 cubic inches.
Weight of the globe with diy air = 3012.4 grains.
" " air by calculation = 12.4 "
Weight of the globe without air = 2000 "
Digiti
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THE CHEMISTS' MANUAL. 213
Weight of the globe with chloroform rapor = 2040 grains.
•* " chloroform yapor =40 **
40 cubic inches of air or vapor at 200°, zednoed to 80.78 cubic inches
steo^
Weight of 80.78 cubic inches of air at eO"* = 9.54 grains.
" " chloroform vapor at 60** =40 "
Hence,
Wt of air. Wt. of chlor. yapor. Sp. Gr. air. Sp. Qr. ctilor. vapor.
9.64 40 1.000 4192.
It may be observed that the ascertained Sp. Gi*. of chloro-
form vapor is 4.20 ; and the Sp. Or. of the vapor calculated
from its elementary composition is 4.1805 ; diflTerences which
are comparatively unimportant.
c
Google ^
Digitized by VjOOQ
I
SPECIFIC GRAVITY
Corresponding to Degrees of BAUME'S HYDROMETER.
144
14^ K. 17.5^ C. (Sp. Gr. = — — - correct.)
144 — B"
DBGRSB.
GBAYITT.
DBOBBB.
1
BPBCinC
GKAVITY.
DVGBBB.
BPBCmO
.0
1.0000
24.5
1.2050
48.5
1.5079
0.5
1.0035
25.0
1.2101 ;
49.0
1.5158
1.0
1.0070
25.5
1.2152 .
49.6
1.5238
1.5
1.0105
26,0
1.2203 1
500
1.5319
2.0
1.0141
26.5
1.2255 1
50.5
1.5401
2.6
1.0177
270
1.2308 '
51,0
1.5484
3.0
1.0313
27.5
1.2361 1
51.5
16568
8.5
1.0249
28.0
1.2414
52.0
1.5652
4.0
1.0286
28.5
1.2468 '
52.5
1.5737
4.5
1.0323
29.0
1.2523
53.0
1.5824
5.0
1.0360
29.5
1.3576
53.5
1.5911
65
1.0397
80.0
1.2682
54.0
16000
6.0
1.0435
30.5
1.2687
1 64.5
1.6089
6.5
1.0473
81.0
1.2748
65.0
1.6179
7.0
1.0511
81.5
1.2800
55.5
1.6271
7.5
1.0549
32.0
1.2857
56.0
1.6363
8.0
1.0588
32.5
1.2915
56.5
i;6457
8.5
1.0827
83.0
1.2978
, 57.0
1.6551
9.0
1.0667
33.5
1.3032
' 57.5
1.6647
9.5
1.0706
84.0
1.3091
58.0
16744
10.0
1.0746
84.5
1.8151
58.5
1.6842
10.5
1.0787
85.0
1.8211
69.0
16941
11.0
1.0827
85.5
1.8273
59,5
1.7041
11.5
1.0868
86.0
1.3333
60.0
1.7143
13.0
1.0909
36.5
1.8895
60.5
1.7245
12.5
1.0951
37.0
1.8458
61.0
1.7349
130
1.09^2
37.5
1.3531
61.5
1.7454
13 5
1.1034
88.0
1.8585
62.0
1.7560
14.0
1.1111
88.5
1.3649
, 62.5
1.7668
14.5
1.1120
89.0
1.3714
63.0
1.7777
15.0
1.1163
89.5
1.8780
63.5
1,7888
15.5
1.1206
40.0
1.3846
640
1.7999
16.0
1.1250
40.5
1.8918
64.5
1.8112
16.5
1.1294
41.0
1.8981
65.0
1.8227
17.0
1.1339
41.5
1.4049
65.5
1.8348
17.5
1.13S3
42.0
1.4118
.66.0
1.8461
18.0
1.1429
42.5
1.4187
66.5
. 1.8580
18.5
1.1475
4S.0
1.4367
67.0
1.8701
19.0
1.1530
48.5
1.4838
67.6
1.8828
19.5
1.1566
44.0
1.4400
68.0
1.8947
20.0
1.1613
44.5
1.4473
68.5
1.9071
20.5
1.1660
45.0
1.4545
69.0
1.9200
21.0
1.1707
45.5
1.4619
69.5
1.9828
21.5
1.1755
46.0
1.4694
70.0
1.9459
23.0
1.1803
46.5
1.4769
70.5
1.9591
235
1.1852
47.0
1.4845
71.0
1.9726
23.0
1.1901
47.5
1.4932
71.5
1.9862
3a.r,
1.1950
48.0
1.5000
72.0
2.0000
24.0
1.2000 '
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THE CHEMISTS* MANUAL.
215
SPECIFIC GRAVITY
FOR OaUIDS LIGHTER THAN WATER.
144
14 4
B" + 184
TABLE BY DR. W. H. PH.E.
= Sp. Gr.
DWISBBS
Spbcifio
DXOBBBS
Specdio
DXOBEES
Stbcifio
Dbgrbbs
Htdbom-
RBB.
(Banmd).
IlTDBOX-
BTXB.
Gbavitt I
(Baame). 1
Htdbox-
ETXB.
(Gravity
(Bauin6).
Hydsox-
ETXB.
Gbatity
(Baum^).
10
1.0000
27
.8917 '
44
.8045
61
.7329
11
.9029
28
.8860
45
.8000
62
.7290
12
.9859
29
.8805 1
46
.7954
68
.7258
13
.9t90
30
.8750 '
47
.7909
64
.7216
14
.9722
31
.8695
48
.7865
65
.7179
15
.9655
32
.8641
49
.7821
66
.7142
16
.9589
33
.8588
50
.7777
67
.7106
17
.9523
34
.8533
51
.7734
68
.7070
18
.9459
35
.8484
52
.7692 -
69
.7035
19
.9395
36
.8433
53
.7650
70
.7000
20
.9333
37
.8383
54
.7608
71
.6965
21
.9271
38
.8333 .
55
.7367
72
.6930
22
.9210
39
.8284
66
.7526
73
.6896
23
.9150
40
.8235
57
.7486
74
.6863
24
.9090
41
.8187
58
.7446
75
.6829
25
.9032
42
.8139
59
.7407
76
.6796
26
.8974
43
.8092
60
.7368
77
.6763
DEGREES TW^ADDLE'S HYDROMETER
AND THE CORRESPONDINO SPECIFIC GRAVITIES.
DTCBKBfl.
Sracmo
DSOBKBB.
Gravitt.
DlORSSS.
SPBOiric
Gravity.
1.075
Beorexb.
Spbcipio
Gravity.
1
.1.005
8
1.040
15
22
1.110
2
1.010
9
1.045
16
1.060
23
1.115
8
1.015
10
1.050
17
1.085
24
1.120
4
1.020
11
1.055
18
1.090
25
1.125
5
1.026
12
1.060
19
1.095
26
1.130
6
1.030
18
1.065
20
1.100
27
1.135
7
1.035
14
1.070
21
1.105
28
1.140
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216
THE CHEMISTS' MANUAL.
PROPORTION OF ABSOLUTE ALCOHOL
BY WEIGHT IN lOO PARTS OF SPIRIT,
OP DIFFERENT SPECIFIC GRAVITIES AT W P. (15°. 5 C.)
(FowNBS. Phil. Trans,, 1847.)
AliCOHOL
Sfbcuic
Alcohoi.
Sfboific
Alcohol
Spbcifio
Alcohol
Bfbcifxo
FIBCKHT.
FBBCXHT.
Gbxtttt.
PUCBNT.
Qbatttt.
PEBCBKT.
GBAvnr.
0
1.0000
25
.9652
51
.9160
76
.8581
0
.9991
26
.9638
52
.9135
77
.8657
1
.9981
27
.9623
58
.9118
78
.8533
2
.9965
28
.9609
54
.9090
79
.8508
8
.9947
29
.9593
55
.9069
80
.8488
4
.9980
30
.9578
56
.9047
81
.8469
5
.9914
81
.9560
57
.9025
82
.8484
6
82
.9544
58
.9001
83
.8408
7
.9884
38
.9528
59
.8979
84
.8382
8
.9869
34
.9511
60
.8956
85
*357
9
.9855
35
.9490
61
.8982
86
.8331
10
.9841
36
.9470
62
.8908
87
.8805
11
.9828
87
.9452
63
.8886
88
.8279
12
.9815
88
.9434
64
.8863
89
.8254
13
.9802
89
.9416
65
.8840
90
.8228
14
.9789
40
.9396
66
.8816
91
.8199
15
.9778
41
.9376
67
.8793
92
.8172
16
.9766
42
.9856
68
.8769
98
.8145
17
.9753
48
.9886
69
.8745
94
.8118
18
.9741
44
.9314
70
.8721
95
.8089
19
.9728
45
.9292
71
.8696
96
.8061
20
.9716
46
.9270
72
.8672
97
.8031
21
.9704
47
.9249
' 73
.8649
98
.8001
22
.9691
48
.9228
74
.8625
99
.7969
23
.9678
49
.9206
75
.8603
100
.7988
24
.9665
50
.9184
In this table every alternate number is the result of a direct synthetical
experiment ; absolute alcohol and distilled water being weighed out in the
proper proportions, and mixed by agitation in stoppered bottles ; after a
lapse of three or four days, each specimen was brought exactly to 60" P.,
and the specific gravity determined with great care.
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THE CHEMIST'S MANUAL.
217
TABLE
Of thb Proportion bt Volume of Absolute or Real Alcohol or
100 Volumes of Spirits of different Specific Grayities (Gat-
LussAC) at 59** F. (15' C).
100 VOLUXW
100 YOLUXKS
OF 6PlftiTS.
> 100 YoLums
1
OF Spibtts.
CONTAXR
Contain
Contain
SPBCino
YOLUIUEB
SPBcnfic
YOLUMXS
Spbcifio
YoLUXBfl
QRAYXTy.
OF BBAL
Gratitt.
or BBAL
Ausosou
Alcohol.
Alcohol.
l.OOGO
0
09608
84
0.8956
68
.9085
1
.9594
35
.8932
69
.9970
3
.9581
86
.8907
70
.9956
3
.9567
87
.8882
71
.9943
4
.9553
38
.8857
73
.9929
6
.9538
39
.8831
73
.9916
6
.9523
40
.8805
74
.9903
7
.9507
41
.8779
75
.9891
8
.9491
42
.8753
76
.9878
9
.9474
43
.8726
77
.9867
10
.9457
44
.8699
78
.9855
11
.9440
45
.8672
79
.9844
12
.9422
46
.8645
80
.9833
13
.9404
47
.8617
81
J)822
14
.9386
48
.8589
82
M12
15
.9367
49
.8560
83
.9802
16
.9348
50
.8531
84
.9792
17
.9329
51
.8502
85
.9783
18
.9309
52
.8472
86
.9773
19
.9289
53
.8442
87
.9763
30
.9269
54
.8411
88
i>753
31
.9248
55
.8379
89
.9743
33
.9237
56
.8346
90
.9732
33
.9206
57
.8812
91
.9721
34
.9185
. 58
.8278
92
.9711
25
.9163
59
.8242
98
.9700
26
.9141
60
.8206
94
.9690
37
.9119
61
.8168
95
.9879
38
.9096
62
.8138
96
.9668
39
.9073
63
.8086
97
.9657
30
.9050
64
.8043
98
.9645
31
.9027
65
.8006
99
.9633
83
.9004
66
.7947
100
.9621
33
.8980
67
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218
THE CHEMISTS' MANUAL.
QUANTITIES OF ABSOLUTE ALCOHOL BY WEIGHT,
IN MIXTURES OF ALCOHOL AND WATER OF THE FOI^
LOWING SPECIFIC GRAVITIES.-HDbihkwatbr.)
Spbodio
Alcohol
Alcohol
Specific
Alcohol
SPKcnno
Alcohol
Gravitt
byW'ght
Gravity
byW'oht
byW'oht
Gravitt
btW'qht
AT 60' F.
iw 100
AT flO' F.
IN 100
AT flO' F.
IK 100
AT »)' F.
IN 100
(15*.5 C.)
PARTS.
(16'.5 C.)
PARTS.
(15".6 C.)
PARTS.
a6".5 C.)
PARTS.
1.0000
0.00
0.9959
2.22
0.9918
4.64
0.9877
7.80
.9999
0.05
.9958
2.28
.9917
4.70
.9876
7.37
.9998
0.11
.9957
2.34
.9916
4.76
.9875
7.43
.9997
0.16
.9956
2.39
.9915
4.82
.9874
7.60
.9998
0.21
.9955
2.45
.9914
4.88
.9873
7.67
.9995
0.26
.9954
2.51
.9913
4.94
.9872
7.64
.9994
0.32
.9953
2.57
.9912
5.01
.9871
7.71
.9993
0.37
.9952
2.62
.9911
5.07
.9870
7.78
.9902
0.42
.9951
2.68
.9910
5.13
.9869
7.86
.9991
0.47
.9950
2.74
.9909
5.20
.9868
7.93
.9990
0.53
.9949
2.79
.9908
5.26
.9867
7.99
.9989
0.58
.9948
2.85
.9907
5.32
.9866
8.06
.9988
0.64
.9947
2.91
.9906
5.39
.9865
8.13
.9987
0.69
.9946
2.97
.9905
5.46
.9864
8.20
,9986
0.74'
.9945
302
.9904
5.51
.9863
8.27
.9985
0.80
.9944
8.08
.9903
5.68
.9862
8.34
.9984
0.85
.9943
8.14
.9902
5.64
.9861
8.41
.9983
0.91
.9942
3.20
.9901
5.70
.9860
8.48
.9982
0.96
.9941
8.26
.9900
5.77
.9869
8.56
.9981
1.02
.9940
8.32
.9899
5.83
.9868
8.62
.9980
1.07
.9939
3.37
.9898
6.89
.9857
8.70
.9979
1.12
.9938
8.43
.9897
6.96 1
.9856
8.77
.9978
1.18
.9937
8.49
.9896
6.02
.9855
8.84
.9977
1.23 ,
.9936
355
.9895
6.09
.9854
8.91
.9976
1.29 !
.9935
8.61
.9894
6.15
.9863
8.98
.9975
1.34 1
.9934
3.67
.9898
6.22
.9862
9.05
.9974
1.40
.9933
3.73
.9892
6.29
.9a5i
9.12
.9973
1.45
.9932
8.78
.9891
6.35
.9860
9.20
.9972
1.51
.9931
8.84
.9890
6.42
.9849
9.27
.9971
1.56
.9930
8.90
.9889
6.49
.i7o4o
9.84
.9970
1.61
.9929
8.96
.9888
6.56
.9847
9.41
.9969
1.67
.992d
4.02
.9887
6.62
.9846
9.49
.9968
1.73
.9927
4.08
.9886
6.69
.9845
9.66
.9967
1.78
.9926
4.14
.9885 .
6.75
. .9844
9.63
.9966
1.83
.9925
4.20
.9884
6.82
.9843
9.70
.9965
1.89
.9924
427
.9883
6.89
.9842
9.78
.9964
1.94
.9923
4.38
.9882
6.95
.9841
9.86
.9963
1.99
.9922
4.39
.9881
7.02
.9840
9.92
.9962
2.05
.9921
4.4,5
.9880
7.09
.9889
9.99
.9961
2.11
.9920
4.51
.9879
7.16
.9888
10.07
.9960
2.17
.9919
4.57
.9878
7.23
This Table is founded on synthetic experiments, in which eleven differ-
ent mixtures of alcohol and water were made, containing respectively 0.5,
1, 2, 3, 4, 5, 6, 7, 8, 9, and 10 per cent of alcohol by weight : the alcohol em-
ployed had a specific gravity of 0.7938 at 60° F. or 15^6 C.
Digiti
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THE CHEMISTS' MANUAL.
TABLE*
qq^ Q^-^^fTiTY ov ReaIj Alcohol contained m 1
tp*,:®^^^ ^^^Ij€X)hou sy Weight and by Volume a'
(Teznfpera.tixTe, 15" C.)
100 Voi^trxEB
coKTAJor :
o.oo
1.2S
2.54:
3.77
4.97
e.io
7.S2
a4s
11.&&
IS ai
15. S3
17.42
1B.S»
10.01
20-03
^3-00
33.03
33.30
34=--l4
35-4'^
3B-^1
3T.&^
3«.&»
30.00
^^-^^
i^3-0^
4^.Tr3
100 PABT8 I
sy Wkioht
coif TAIN :
Spscific
Gravity.
100 VOLUMEI
CONTAIN :
u±loohol.
Alcohol.
WaU
lOO-OO
.9348
50
53.7
98-38
.9366
49
54.7
96.83
.9385
48
55.6
95.35
.9403
47
56.6
93.89
.9421
46
57.6
9!3.45
.9439
45
58.6
91.08
.9456
44
59.5
B0.72
.9473
43
60.5
SS.37
.9490
42
61.5
8T.04
.9506
41
62.4
S,"5.74
.9522
40
63.4
e^4.47
.9538
39
64.3
e3.22
.9553
38
65.^
ei.96
.9568
37
66.^
eo.72
.9582
36
67.2
-TO 51
.9595
35
68.1;
'78-29
.9607
84
69.0
'77.09
.9620
33
69.9
-75.91
.9633
32
70.8
-74/75
.9645
31
71.8
-73 59
.9657
30
72.7
•72.43
.9668
29
73.6
•71.80
.9679
28
74.5;
•70.16
.9690
27
75.4:
e9.04
.9700
26
76.3;
67.93
.9711
25
IIZ
66.82
.9721
24
78.1;
65.72
.9731
23
79.0
64.64
.9741
22
79.9
63.58
.9751
21
80.8
62.50
.9761
20
81.7
61.43
.9771
19
82.6
60.38
.9781
18
83.5
69.33
.9791
17
84.3
58.29
.9801
16
85.2
57.25
.9812
15
86.1
66.23
.9822
14
87.0
55.21
.9833
13
88.0
54.20
.9844
12
88.9
53.19
.9855
11
89.8
52.20
.9867
10
90.7
51.20
.9878
9
91.6
50.21
.9890
8
92.5
i 49.24
.9902
7
93.4
\ 48.26
.9915
6
94.3
I 47.29
.9928
5
953
\ 46.33
.9942
4
96.2^
1 45.37
.9956
3
971
44.41
.9970
2
98.1
\ 43.47
.9985
1
99.0
Bxam. Med. Chemicals, Hofftnann, p. 119.
Digiti
ized by Google
220
THE CHEMISTS' MANUAL.
TABLE*
Of thb Quantitt bt Weight of Htdbochlobio-Acid Gas ooirrAiNED
IN 100 Parts bt Weight of Aqueous Htdbochloric Acid at
DIFFERENT DENSITIES. (Temperature, 16° C)
Pkb osst
PXBCBHT
Pbboknt
SFBCino
Gravity.
OF
Htdbo-
CHLOBIO
Sfboifio
OF
Hydro-
OHLORIO
Gravity.
OF
Hydro-
OHLORIO
Sfscifio
OF
Hydbo-
Acid.
Acid.
Acid.
I
1
ACID.
1.2013
41
1.1551
31.25
1.1056
21.5
1.0573
11.75
1.2002
40.75
1.1539
31
1.1044
21.25
1 1.0661
11.6
1.1991
40.5
11526
30.75
1.1031
21
1 1.0M9
11.25
1.1930
40.25
1.1513
30.5
1.1019
20.75
10637
11
1.1969
40
1.1501
30.26
1.1007
20.5
' 1.0524
10.75
1.1918
39.75
1.1488
30
1.0994
20.25
1 1.0512
10.5
1.1917
39.5
1.1475
29.75
1.0982
20
1 1.0500
10.26
1.1936
39.25
1.1462
29.5
1.0969
19.76
1 1.0488
10
1.1935
39
1.1450
29.25
1.0957
19.5
' 1.0475
9.76
1.1913
38.75
1.1437
29
1.0946
19.26
1 1.0463
9.6
1.1902
385
1.1424
28.75
1.0932
19
1 1.0451
9.26
1.1890
38.25
1.1412
28.5
1.0920
• 18.75
' 1.0439
9
1.1878
38
1.1399
28.26
1.0907
18.5
' 1.0427
8.75
1.1867
37.75
1.1386
28
1.0895
18.26
1 1.0414
8.5
1.1855
37.5
1.1373
27.75
1.0883
18
1 1.0402
8.25
1.1841
37.25
1.1361
27.5
1.0870
17.76
17.6
1.0390
8
1.1833
37
11348
27.25
1.0858
1.0378
7.75
1.1831
36.75
1.1335
27
1.0845
17.25
1.0866
7.6
1.1810
38.5
1.1323
26.75
1.0833
17
1.0853
7.25
1.1793
36.25
1.1310
26.5
1.0821
16.76
1.0841
7
1.1787
38
1.1297
26.25
1.0807
16.6
1.0329
6,75
1.1775
35.75
1.1284
26
1.0795
16.26
1.0317
6.6
1.1763
35.5
1.1272
25.75
1.0783
16
1 1.0306
«.26
1.1752
35.25
1.1259
25.5
1.0770
15.76
10292
6
1.1739
35
1.1246
25.25
1.0758
15.6
1 1.0280
6.75
1.17:37
34.75
1.1234
25
1.0746
15.26
1 1.0268
5.6
1.1714
34.5
1.12-21
24.75
1 1.0733
15
1.0256
5.25
1.1703
34.25
1.1208
24.5
1 1.0721
14.75
1.0244
6
1.1689
34
1.1196
24.25
1 liy709
14.5
1.0231
475
1.1677
,38.75
1.1183
24
1 1.0696
14.25
1.0219
4.5
1.1684
88.5
1.1170
23.75
1 1.0684
14
1.0207
425
1.1652
33.25
1.1157
23.5
1 10672
13.76
1.0196
4
1.1639
33
1.1145
23.25
i 1.0869
13.6
1.0170
8.6
1.1637
32.75
1.1132
23
, 1.0647
13.26
1.0146
3
1.1614
32.5
1.1119
22.75
' 1.06a5
13
1.0122
2J5
1.16^2
32.25
1.1107
22.5
1 1.0622
12.76
1.0097
2
1.1589
32
1.1094
22.26
1.0010
12.6
1.0073
1.5
1.1577
31.75
1.1081
22
, 1.0598
12.25
10048
1
1.1564
31.5
1 1.1069
21.75
1.0585
12
1 1.0024
0.5
♦ Taken from " Manual Chem. Anal.," by Fred. Hoffmann, p. 87.
Digiti
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THE CHEMISTS' MANUAL.
221
The density of the aqueous add being decreased by an increase of tem-
perature, and increased by a decrease of temperature, the consequent
change of the specific gravity amounts for each degree of the Centigrade
thermometer in either direction —
For acids of a specific gravity of 1.17d9 to those of 1.1886 to about 0.0005
- '* 1.1385 •* 1.0982 " 0.0004
1.0082 • " 1.0636 •* 0.0008
For in$tanee : An acid of a specific gravity of 1.1234 at lO"" C, containing
25 per cent of hydrochloric-acid gas, will have at 18.5° C. a specific gravity
of (1.1284 - 0.004 X 2.5 = ) 1.1224, and at ISS** C. a specific gravity of
(1.1284 + 0.004 X 2.5 =) 1.1244.
T A BLE*
Of thb Quantitt by Weight of Nitric Oxide (N,Oj) and of Mono-
htdrated nitric acid coktained in 100 parts by weight op
AqiTEOUB Nitric Acid at different Densities. (Temperature,
17.5* C.)
6RAY1TT.
Pra
CBKT OF
N.O..
Pebckiit
OF N.O,
+ H,0.
Obayxtt.
Pkb
csht of
N,0..
Pbbciht
OF N,0,
+H,0.
SPBCIFf O
Gravitt.
PBH
CEKT OF
N.O..
Pkiscemt
OF N.O,
+ H,0.
1.528
85
99.16
1.472
72
84.00
1.417
59
68.83
1.521
84.5
98.58
1.470
71.5
83.41
1.414
58.5
68.25
1.519
84
98.00
1.469
71
82 83
1.412
58
67.66
1.517
83.5
97.41
1.467
70.5
82.24
1.409
67.5
67.08
1.516
83
96.88
1.465
70
81.66
1.406
57
66.50
1.514
82.5
96.24
1.462
69.5
81.08
1.403.
56.5
65.91
1.612
82
95.66
1.460
69
80.50
1.400
56
65.33
1^10
81.5
95.08
1.458
68.5
79.91
1.397
55.5
64.75
1.508
81
94,50
1.456
68
79.33
1.394
55
64.16
1.506
80.5
93.91
1.454
67.5
78.76
1.392
54.5
63.58
1.504
80
98.33
1.451
67
78.16
1.389
54
63.00
1.502
79.5
92.74
1.449
66.5
77.58
1.386
53 5
62.41
1.500
79
92.16
1.447
66
77.00 1
1.383
53
61.83
1.498
78.5
91.58
1.444
65.5
76.41 .
1.380
52.5
61.25
1.496
78
91.00
1.442
65
75.83
1.377
52
60.66
1.494
77.5
90.41
1.440
64.5
75.25
1.374
51.5
6C.08
1.492
77
89.83
1.438
64
74.66
1.371
51
59.50
1.490
76.5
89.24
1.436
63.5
74.08
1.368
50.5
58.91
1.488
76
88.66
1.434
63
73.50
1.364
50
58.33
1.486
75.6
88.08
1.432
62.5
72.91
1.361
49.5
57.75
1.484
75
87.50
1.430
62
72.33
1.358
49
57.16
1.482
74.6
86.91
1.428
61.5
71.75
1.355
48.5
56.58
1.480
74
86.33
1.426
61
71.16
1.352
48
56.00
1.478
73.5
85.74
1.424
60.5
70.58
1.349
47.5
55.41
1.476
73
85.16
1.422
60
70.00 1
1.345
47
64.83
1.474
72.5
84.58
1.419
59.5
69.41 '
1.343
46.5
54.25
* Taken from " Man. Chem. Anal.," by Fred. Hoffinann, 1873, p. 94.
Digiti
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222
THE CaraiMISTS* MANUAL.
Sfkoifio
Qbavitt.
Pkr
CENT 07
N.O..
Pebcxnt
OF N,0,
+ H,0.
1
1 SPEcmc
Gravity.
1 PKH !
CENT OF
1.338
46
53.66
1 1.236
32.6
1.334
45.5
53.08
1.282
82
1.330
45
52.50
1.228
31.6
1.327
44.5
51.91
1.224
81
1.323
44
51.33
1.220
30.6
1.319
43.5
50.75
1.217
80
1.315
43
50.16
1.213
29.6
1.312
42.5
49.58
1.209
29
1.308
42
49.00
1.206
28.5
1.304
41.5
48.41
1.201
28
1.301
41
47.a3
1.198
27.5
1.297
40.5
47.25
1.194
27
1.294
40
46.66
1.190
26.5
1.290
39.5
46.08
1.186
26
1.287
39
45.50
1,182
25.5
1.283
38.5
44.91
1.178
25
1.279
38
44.33
1.174
24.5
1.275
87.5
43.76
1.170
24
1.271
37
43.16
1.167
23.5
1.267
36.5
42.58
1.163
28
1.263
36
42.00
1.159
22.5
1.259
35.5
41.41
1.155
22
1.255
35
40.83
1.151
21.6
1.251
345
40.25
1.147
21
1.247
34
39.66
1.143
20.5
1.243
33.5
39.08
1.140
20
1.239
33
88.50
1.136
19.5
Pes cent,
OF ISaOm I
+ H.0.
37.91
37.83
86.75
86.16
85.68
35.00
34.41
83.83
83.25
32.66
82.08
31.60
30.91
80.33
2974
29.16
28.58
28.00
27.41
26.83
26.26
25.66
25.08
24.49
28.91
28.83
22.74
SPBdFIO
Oratitt.
1.132
1.129
1.126
1.122
1.118
1.114
1.111
1.107
1.104
1.100
1.096
1.092
1.089
1.086
1.082
1.078
1.075
1.071
1.068
1.064
1.060
1.066
1.C68
1.050
1.045
1.038
1.C32
P«B 'PEBcxirr
CENT of! OF N,0,
N,0.. +H.O.
19
18.6
18
17.6
17
16.5
16
15.6
15
14.5
14
18.6
13
12.6
12
11.6
11
10.6
10
9.6
9
8.5
8
7.6
7
6
6
22.16
21.58
21.00
20.41
19 bS
19 25
18.66
18.08
17.50
16.91
16.33
16.74
15.16
1468
14.00
13.41
12.83
12.25
11.66
1107
10.60
9.91
983
8.84
8.16
7.00
6.83
Note. — With the decrease and increase of temperatare, the density of
Nitric Acid suffers a corresponding increase or decrease, amounting for each
degree of the Centigrade thermometer in either direction —
For adds of a sp. gr. of 1.492 to those of 1.476 to 0.00213 in the average.
I<
1.472
1.466 " 0.002
((
1.464
1.434 « 0.00186
((
1.430
1.412 " 0.00171
<l
1.406
1.888 " 0.00166
"
1.877
1.352 " 0.00141
' <i
1.845
1.815 " 0.00128
« .
1.808
1.279 « 0.00114
((
1.271
1.239 " 0.001
<i
1.282
1.201 « 0.00086
((
1.194
1.163 " 0.00071
<i
1.156
1.125 " 0.0006
For instance: An acid of 1.178 specific gravity at 17.6" C, containing^
26 per cent of anhydrous, or 29.16 per cent of monohydrated. Nitric Add,
will have, at 20" C, a specific gravity of (1.178 - 0.00072 x 2.5 =) 1.762.
and at 16" C. 41 specific gravity of (1.178 + 0.00072 x 2.5 =) 1.179a
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THE CHEMISTS' MANUAL.
TABLE*
Of thb Quantity by Wkioht op Phosphoric Oxide (PjOj) and of
TrI HYDRATED PHOSPHORIC ACID CONTAINED IN 100 PARTS BY WEIGHT
OF Aqueous Phosphoric Acid at different DENsmE&
(TSXPBBATUBB, 17.5* 0.)
Feb CENT or
SPBCiric
Pkk cent of
Gbatitt.
P.O..
P.0,+8H,0.
Gbatity.
P.O..
P.0,+8H,0.
1.809
68
93.67
1.469
46.5
64.06
1800
67.6
92.99
1.462
46
63.37
1.792
67
92.30
1.455
45.5
62.68
1.783
66.5
91.61
1.448
45
61.99
1.776
66
90.92
1.441
44.5
61.30
1.766
65.5
90.23
1.435
44
60.61
1758
65
89.54
1.428
43.6
59.92
1.750
64.5
88.85
1.432
43
69.23
1.741
64
88.16
1.415
42.5
58.55
1.733
63.5
87.48
1.409
42
57.86
1.726
63
86.79
1.402
41:5
67.17
1.717
62.5
86.10
1.398
41
50.48
1.709
62
85.41
1.389
40.5
55.79
1.701
61.5
8472
1.383
40
55.10
1.693
61
84.03
1.377
39.5
54.41
1.635
60.5
83.34
1.371
39
58.72
1677
60
82.65
1.365
38.6
53.04
1.669
59.5
81.97
1.359
38
52.36
1.661
59
81.28
1.354
37.5
51.66
1.653
58.5
80.59
1.348
37
50.97
1.645
58
79.90
1.342
86.5
50.28
1.637
57.5
79.21
1.336
36
49.59
1.629
57
78.52
1330
36.5
48.90
1.621
56.5
77.83
1.325
35
48.21
1.613
56
77.14
1.319
34.6
47.62
1.606
55.5
76.45
1.314
34
46.84
1.597
55
75.77
1.308
33.5
46.15
1.589
54.6
75.08
1.303
33
45.46
1.581
54
74.39
1.298
32.6
44.77
1.574
53.6
73.70
1.292
32
44.08
1.566
68
73.01
1.287
31.6
43.89
1.559
52.6
72.32
1.281
31
42.70
1.551
62
71.63
1.276
30.6
42.01
1 1J543
51.6
70.94
1.271
30
41.33
1.536
61
70.26
1.266
29.5
40.64
1.528
60.6
69.57
1.260
20
39.96
1.521
60
68.88
1.255
^.6
39.26
1.513
495
68.19
1.249
28
88.57
1.505
49
67.60
1.244
27.5
37.88
1.488
48.6
66.81
1.239
27
37.19
1.491
48
66.12
1.233
26.6
86.50
1.484
47.6
65.48
1.228
26
36.82
1.476
47
64.75
1.223
26.5
36.13
• Loc dt. (Hoffman), p. 101.
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224
THE CHEMISTS' MANUAL.
Table of thb
' Weight, 'Ertc.^Gontinued.)
Sntomo
Pkbcknt of
Per cent of
Specxfio
PXBOBHTOF
Gbavitit.
P.O..
P.O.+8H.O.
P.O..
P,0»+8H,0.
1.218
25
34.44
1.109
13.6
18.60
1.213
24.6
83.75
1.104
13
17.91
1.208
24
88.06
1.100
12.5
17.22
1.203
28.5
32.87
1.096
12
16.63
1.198
28
81.68
1.091
11.5
15.84
1.193
22.5
30.99
1.087
11
15.16
1.188
22
80.31
1.088
10.5
14.46
1.183
21.5
29.62
1.079
10
1377
1.178
21
28.93
1.074
9.5
18.09
1.174
20.5
28.24
1.070
9
12.40
1.169
20
27.55
1.066
8.5
11.71
1.164
19.5
26 86
1.062
8
11.02
1.159
19
26.17
1.058
7.5
10.38
1.155
18.5
25.48
1.053
7
9.64
1.160
18
24.80
1.049
6.5
8.95
1.145
17.5
24.11
1.045
6
a26
1.140
17
23.42
1.041
6.6
7.57
1.136
16.5
22.73
1.037
6
6.89
1.180 .
16
22.04
1.083
4.5
620
1.126
15.5
21.35
1.029
4
6.61
1.122
16
20.66
1.025
3.5
482
1.118
14.5
19.97
1.021
3
4.18
1.113
14
19.28
1.017
2.6
8.44
Note. — With the decrease or increase of temperature, the density of
phosphoric acid suflPers a corresponding increase or decrease, amounting for
each degree of the Centigrade thermometer in either direction :
For acids of a specific gravity of 1.809 to those of 1.613 to about 0.601.
" " " *• " 1.597 " 1.462 " 0.00082.
** " " " " 1.448 " 1.836 " 0.00068.
" « « " " " 1.325 " 1.228 '* 0.00052.
•• '* " « *' " 1.218 " 1.122 " 0.0004
« " « *' " " 1.113 " 1.079 " 0.00035.
For instance: An acid of 1.130 Sp, Qr. at 17.5*' C, containing 16 per
cent, of phosphoric oxide (PtOg) or 22.04 per cent of tri-hydrated phosphoric
acid, will have, at 20° C, a Sp. Gr. of (1.130 - 0.0004 x 2.5 =) 1.129, and at
16° C, a Sp. Gr. of (1.130 + 0.0004 x 2.5 =) 1.131.
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THE CHEMISTS' MANUAL.
TABLE*
MONOHTDRATKD SUIiPHTJRIC AciD CONTAINED IN 100 PaKTS BT
Weioht ov Aqusocts Sulphubic Acids at different Densitibs.
(Temperature^ 17-5" C.)
Pkb
Obayitt.
OJSMT OT
SO..
1.559
53.8
1.547
58.0
1.536
52.2
1.525
51.4
1.514
50.6
1.503
49.8
1.493
49.0
1.482
48.1
1.471
47.3
1.461
46.5
1.460
45.7
1.440
44.9
1.480
44.0
1.420
43.2
1.411
42.4
1.401
41.6
1.892
40.8
1.382
40.0
1.373
39.2
1.864
38.3
1.354
87.5
1.345
86.7
1.336
85.9
1.328
35.1
1.319
84.3
1.310
38.4
1.302
82.6
1.293
81.8
1.285
81.0
1.276
80.2
1.268
29.4
1.260
28.5
1.251
27.7
1.243
26.9
Pkb
OSNT
OF 80,
+ H,0.
65
64
61
60
59
58
57
56
55
54
53
52
51
50
49
48
47
46
45
44
48
42
41
40
87
86
85
84
SpBcmo
Pbb
CBKT OF
SO..
1.285
26.1
1.257
25.3
1.219
24.5
1.211
23.6
1.202
22.8
1.194
22.0
1.186
21.2
1.178
20.4
1.170
19.6
1.168
18.7
1.155
17.9
1.147
17.1
1.140
163
1.132
15.5
1.125
14.7
1.117
ia8
l.llO
13.0
1.103
12.2
1.095
11.4
1.088
10.6
1.081
9.8
1.074
9.0
1.067
8.1
1.060
7.3
1.053
6.5
1.046
5.7
1.039
4.9
1.032
4.1
1.025
3.2
1.019
2.4
1.012
16
1.006
0.8
1.003
0.4
0.000
0.
Feb
OHNT
or so.
+ H.0.
31
30
27
26
25
24
21
20
19
18
17
16
16
14
13
12
11
10
9
8
7
6
5
4
3
2
1
0.5
0
lioc cit. (Hoffmann), p. 108.
15
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226
THE CHEMISTS' MANUAL.
Note. — With the decrease and increase of temperatare, the deDsity of
sulphuric acid suffers a corresponding increase or decrease, amoxmtixig for
each degree of the Centigrade thermometer in either direction :
For acids of a Sp. Gr. of 1.841 to those of 1.782 to about 0.0014.
1.774
<(
1.6d5
u
0.0012.
1.Q5S
i*
1.302
it
0.001.
1.293
«
1.219
t*
0.00075.
1.211
M
1.140
€t
0.00045.
1.182
M
1.067
Cf
0.00047.
TABLE*
Of the QuAitiTiTx BT Weight op Pure Ethtlio Ether coittainsd
IN 100 Parts by Weight of Ether at different Densitieb.
(Temperature, 17.5° C.)
Feb
Feb
Pbb
PKB
Bfxoifio
OBNT OF
OBNT OF
Sfboifio
CBKT OF
Sfioifio
CXBT OF
Bthtijo
Grayttt.
Ethtuo
Ethtuo
Gbatitt.
Etbtuc
BTTmt,
Ethbb.
Bthbb.
0.7185
100
0.7310
87
0.7456
74
0.7614
61
.7198
99
.7320
86
.7468
73
.7627
60
.7206
98
.7331
85
.7480
72
.7640
59
.7215
97
.7342
84
.7492
71
.7653
58
.7224
96
.7353
83
.7604
70
.7666
57
.7233
95
.7364
82
.7516
69
.7680
56
.7242
94
.7375
81
.7528
68
.7693
55
.7251
93
.7386
80
.7540
67
.7707
54
.7260
92
.7397
79
.7552
66
.7721
63
.7270
91
■ .7408
78
.7564
66
.7735
52
.7280
90
.7420
77
.7576
64
.7750
51
.7290
89
.7432
76
.7588
63
.7764
60
.7300
88
.7444
75
.7601
62
.7778
49
Note. — With the decrease and increase of temperature, the density of
ether suffers a corresponding increase or decrease, amounting for eaeh
degree of the Centigrade thermometer in either direction :
For ether of a Sp. Gr. of 0.7198 to that of 0.7331, about 0.0013.
.7342 " .7504, " .0011.
.7516 " .7627, " .0009.
.7640 " .7764, " .0008.
For instance : An ether of 0.7206 spedfic gravity at 17.6° C, containing
98 per cent ethyl oxide, will have, at 20" C, a specific gravity of (O.7206
-0.0013 X 2.5=) 0.7173, and, at 15° C, a specific gravity of (0.7206
+ 0.0013 X 2.5 =) 0.7239.
♦ Loc. dt. (Hoffmann), p. 116.
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J
.9
M
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THE CHEMISTS' MANUAL.
Table of the Quantitt by Weight op Ahmoioa, Enc.-^Oantinued.)
Sfbcitio
Pebosnt of
Bpbcipto
SPEcmo
PBBcmr OF
AnoiHA.
Gbavity.
Ajocohia.
Ajocokia.
0.9726
6.6
0.9815
4.4
0.9907
2.2
.9788
6.4
.9828
4.2
.9915
2.0
.9741
6.3
.9881
4.0
.9924
1.8
.9749
6.0
.9839
8.8
.9982
1.6
.9757
6.8
.9847
3.6
.9941
1.4
.9766
5.6
.9855
3.4
.9950
1.2
.9773
5.4
.9863
8.2
.9959
1.0
.9781
6.2
.9873
8.0
.9967
0.8
.9790
5.0
.9882
28
.9975
0.6
.9799
48
.9890
2.6
.9988
0.4
.9807
4.6
.9899
2.4
.9991
0.2
Note. — With the decrease and increase of temperatare, the density of
amnionic hydrate sufiers a corresponding increase or decrease, amounting
for each degree of the Centigrade thermometer in either direction :
For ammonic hydrate of a Sp. Gr. of 0.9001 to that of 0.9221 to about 0.00055.
0.9251 " 0.9414 " 0.0004.
0.9520 " 0.9670 '* 0.0003.
0.9709 " 0.9831 " 0.0002.
For instariee : Ammonic hydrate of 0.9598 specific gravity at 14' C,
containing 10 per cent of ammonia, will have, at 18° C, a specific gravity
of (0.9598 - 0.0008 x 4 =) 0.9581, and at 12^ C, a specific gravity of (0.9593
+ 0.0008 X 2 =) 0.9599.
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THE CHEMISTS' MANUAL.
229
TABLE*
Of the QuAimTT by Weight of Potassic Ozidb coittained in 100
Pabtb by Weight of Potassic Hydrate at different DENsnTsa
(Temperature, 17.6" C.)
Sracma
SpBcmo
PXR CENT OF
Pot. Ozids.
Pot. Ozidk.
Grayity.
Pot. Ozidr.
1.576
45
1.358
80
1.171
15
1.568
44.5
1.852
29.5
1.165
14.5
1.560
44
1.845
29
1.159
14
1.553
43.5
1.889
28.5
1.153
13.5
1.545
43
1.382
28
1.147
13
1.537
42.5
1.826
27.5
1.141
12.5
1.530
42
1.820
27
1.185
12
1.522
41.5
1.313
26.5
1.129
11.5
1.514
41
1.807
26
1.123
11
1.507
40.5
1.801
25.5
1.117
10.5
1.500
40
1.294
25
1.111
10
1.492
39.5
1.288
24.5
1.105
9.5
1.484
39
1.282
24
1.099
9
1.477
38.5
1.275
28.5
1.094
8.5
1.470
38
1.269
23
1.088
8
1.463
37.5
1.263
22.5
1.082
7.5
1.456
37
1.257
22
1.076
7
1.449
86.5
1.250
21.5
1.070
6.5
1.442
86
1.244
21
1.065
6
1435
85.5
1.238
20.5
t.059
5.5
1.428
85
1J281
20
1.054
5
1.421
34.5
1.225
19.5
1.048
4.5
1.414
34
1.219
19
1.042
4
1.407
33.5
1.213
18.5
1.037
8.5
1.400
33
1.207
18
1.031
8
1.893
32.5
1.201
17.5
1.026
2.5
1.386
82
1.195
17
1.021
2
1.379
31.5
1.189
16.5
1.015
1.5
U72
31
1.188
16
1.365
30.5
1.177
15.5
Note. — With the decrease and increase of temperature, the density of
the solution suffers a corresponding increase or decrease, amounting, for
each degree of the Centigrade thermometer, in either direction :
For solation of a specific gravity of 1.576 to that of 1.500 to about 0.00056.
" " *' 1.484 ** 1.358 " 0.0005.
" " " 1.345 " 1.231 " 0.0004
" " 1.219 " l.lll " 0.00033.
* Loc. dt. (Hoffmann), p. 254.
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230
THE CHEMISTS' MANUAL.
TABLE*
Op the QUAlffTITY BY WEIGHT OP SODIC OXIDB CONTAINED IN 100 PaBT8
BY Weight of Sodio Hydrate at different Denbitibb. (Tern-
perature, 17.5* C.)
Spicmo
Pbr ckst of
Spboifio
Pbbcxxtov
Gravity.
Sod. Ozids.
Sod. Ozids.
Sod Oxm.
1.500
85
1.858
25
1.210
15
1.492
34.5
1.845
24.5
1.208
14.6
1.486
34
1.838
24
1.195
14
1.477
88.5
1.881
28.5
1.188
1SJ5
1.470
88
1.324
28
1.181
18
1.468
32.5
1.317
22.5
1.174
126
1.455
32
1.809
22
1167
12
1.448
81.5
1.302
21.5
1.160
11.5
1.440
81
1.295
21
1.153
11
1.438
80.5
1.288
20.5
1.146
10.5
1.426
30
1.281
20
1.139
10
1.418
29.5
1.274
19.5
1.132
9J5
1.411
29
1,266
19
1.125
9
1.404
28.5
1.259
18.5
1.118
8.6
1.896
28
1.252
18
1.111
8
1.389
27.5
1.245
17.5
1.104
7.6
1.382
27
1.288
17
1.097
7
1.875
26.5
1.281
16.5
1.090
6.6
1.867
26
1.224
16
1.088
6
1.360
25.5
1.217
15.5
1.076
5.5
(Liquor Natri Caustici of the Pharmacopoea Gennanica has a specific
gravity of from 1.880 to 1.384, and contains from 80 to 81 per cent of sodic
hydrate, or about 23.5 per cent of sodic oxide.)
Note. — With the decrease and increase of temperature, the density of
the solution suffers a corresponding increase and decrease, amounting for
each degree of the Centigrade thermometer, in either direction :
For solution of a specific gravity of 1.500 to that of 1.858 to about 0.00045.
1.346 " 1.210 *' 0.0004
1.208 " 1.076 " 0.00089.
* Loc. dt (Hoffmann), p. 255.
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THE CHEMISTS' MANUAL.
231
DENSITY OF AQUEOUS ACETIC ACID.
By OUDEMAUS.
"IS
Dbnbitt.
^1
Dbksitt.
At 0- C.
At 16".
At40\
At 0" C.
At 16\
At 40'.
0
0.990
0.9009
0.9934
61
1.0740
1.0698
1.0416
1
1.0016
1.0007
0.0086
69
1.0749
1.0681
1.0438
»
1.0088
1.0099
0.0948 1
68
1.0768
1.0688
1.0490
8
1.0061
1.0087
0.9960 1
64
1.0W7
10646
1.0484
4
1.0060
1.0069
0.9079
66
1.0775
1.0668
1.0440
6
1.0088
1.0067
0.9984
66
1.0788
1.0600
1.0446
6
1.0106
1.0068
a9996
57
1.0791
1.0666
1.0460
7
1.0194
1.00B8
1.0008
68
1.0798
1.0678
1.0466
8
1.0149
1.0118
1.0090 1
60
1.0806
1.0679
1.0460
9
1.0160
1.0197
1.0089 1
60
1.0818
1.0685
10464
10
1.01T6
1.0149
1.0044 !
61
1.0690
1.0691
1.0468
11
1.0194
10167
1.0066
69
1.0696
1.0097
1.0479
IS
1.0911
1.0171
1.0067
68
1.0639
1.0709
1.0475
18
1.0988
1.0186
1.0079
64
1.0688
1.0707
1.0479
14
1.0946
i.oaoo
1.0090
66
1.0816
1.0719
1.0489
16
1.0969
1.0814
1.0101
66
1.0861
1.0717
1.0486
16
1.0279
1.0998
1.0119
67
1.0856
1.0791
1.0488
17
1.0i»6
1.0343
1.0128
68
1.0861
1.0795
1.0491
18
1.0311
1.0966
1.0184
60
1.0866
1.0790
1.0498
19
1.0897
1.0970
1.0144
70
1.0671
1.0788
1.0496
90
1.0348
1.0S84
1.0165
71
1.0875
1.0787
1.0497
91
1.0339
1.0998
1.0166 '
79
1.0879
1.0740
1.0498
99
1.0874
10311
1.0176
78
1.0663
1.0749
1.0499
9S
1.0890
1.0894
1.0187
74
1.0686
1.0744
1.0600
94
1.0406
1.0887
1.0197
76
1.0888
1.0746
1.0601
96
1.0480
10660
1.0907
78
1.0891
1.0747
1.0501
96
1.0t35
1.0068
1.0917
77
1.0693
1.0746
1.0601
97
1.0450
1.0876
1.09S7
78
1.0694
1.0748
1.0500
98
1.0466
1.0888
1.0986
79
1.0696
1.0748
1.0499
99
1.0479
1.0400
1.0946
80
1.0807
1.0897
1.0748
1.0497
80
1.0488
1.0419
1.0956
81
1.0747
1.0496
81
1,0607
1.0494
1.0964
89
1.0607
1.0746
1.0499
89
1.0BS0
1.0436
1.0974
63
1.0R96
1.0744
1.0469
88
1.0684
1.0447
1.0363
84
1.0694
1.0749
1.0486
84
1.0647
1.0460
1.0991
86
1.0699
1.0789
1.0481
86
1.0660
1.0470
L0600
86
1.0869
1.0796
1.0475
86
1.0678
1.0481
1.0808
87
1.0886
1.0781
1.0469
87
1.0686
1.0498
1.0816
88
1.0861
1.0796
1.0469
88
1.0698
1.0609
1.0894
89
1.0876
1.0790
1.0456
88
1.0610
1.0618
1.0689
90
1.0871
1.0718
1.0447
40
1.06U
1.0698
1.0640
91
1.0706
1.0488
41
1.0684
1.0688
1.0648
09
1.0696
1.0498
49
1.0646
1.0648
1.0865
96
1.0686
1.0416
48
1.0657
1.0668
1.0868
1 M
1.0674
1.0408
44
1.0668
1.0669
1.0870
95
1.0660
1.0388
46
1.0679
1.0671
1.0877
96
1.0644
1.0870
40
1.0690
1.0680
1.0384
«7
1.0696
1.0860
47
1.0700
1.0689
1.0891
96
10604
1.0897
48
1.0710
1.0698
1.0897
99
1.0580
1.0301
40
1.0790
1.0807
1.0404
100
1.0668
1.0978
CO
1.0780
1.0616
1.0410
1 .
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232
THE CHEMISTS' MANUAL.
TABLE*
Of the Quantity bt Weight op Wateb contained in 100 Pabtb
BY Weight op Glycebin at dipfebent DENSiTiEa (Temperature
17.6" C.)
fiPEcmo
li
SPECino
11
Spbcxfio
11
Sfbcifio
ii
Gravitt.
«^
GBAvmr.
n
Gravitt.
i\
Gbatitt.
^^
£S
£S
1.267
0
1.224
18 '
1.185
26
1.147
89
1.2«4
1
1.221
14 1
1.182
27
1.145
40
1.260
2
1.218
15
1.179
28
1.142
41
1.257
3
1.215
16
1.176
29
1.139
42
1.254
4
1.212
17
1.178
30
1.136
43
1.250
5
1.209
18
1.170
31
1.134
44
1^47
6
1.206
19
1.167
32
1.131
45
1.244
7
1.208
20
1.164
33
1.128
46
1.240
8
1.200
21
1.161
34
1.126
47
1.237
9
1.197
22
1.159
35
1.123
48
1.234
10
1.194
23
1.156
36
1.120
49
1.231
11
1.191
24
1.153
37
1.118
50
1^28
12
1.188
25
1.150
38
* Loc. cit.- (Hoffmann), p. 224.
THE FOLLO^VING ARE THE
SPECIFIC Gravities of official
LIQUIDS,
(B. P. = British Phannacy. U. S. P. = United States Pharmacy.)
ATTFIELD.
Name. Sp. Gb.
Acid, Acetic, B. P 1.044
U.S. P 1.047
diluted. B. P. and U. S. P 1.006
Glacial 1 .065—1 .066
" Carbolic 1.065
" Hydriodic, diluted 1.113
« Hydrochloric, B. P. and U. S. P 1.160
" " dauted,B.P 1.062
•* •* " U.S. P 1.088
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THE CHEMISTS' MANUAL. 233
Namr Sp. Gb.
Arid, Hydrocyanic, B. P. and U.S. P 997
" Lactic, U.S.P 12n
" Nitric, B. P. and U. S. P 1.420
" diluted, B.P 1.101
" U.S. P 1,068
" Nitrohydiochloric 1.074
" Phosphoric, diluted, B. P 1.080
U. S.P 1.056
« Sulphuric, B. P. and U. S. P 1.843
« « aromatic 927
diluted, B.P 1.094
U.S.P 1.082
•* Sulphurous, solution of , B. P 1.040
U.aP 1.035
Alcohol, U. a P 835
absolute 795
" (rectified spirit, 84^) 888
* (proof spirit, 49%) 920
« dilutum, U. S. P 941
foriiuB^U. S.P 817
« Amylic, B. P. and U. S. P 818
Ammonia, aromatic spirit of, B. P 870
•* stronger water of, U.S.P 900
" solution of, B. P 959
" strong solution of, B. P. 891
Antimony, solution of Chloride of , B. P 1.470
Arsenic, Hydrochloric solutions of, B. P 1.009
Arsenical Solution (Liquor Arsenicalis), B. P 1.009
Benzol, B.P 850
Bismuth and Ammonia, solution of Citrate of, B. P 1.122
Bromine 2. 966
Chlorine, solution of , B. P 1.008
Chloroform, B. P. and U. S. P 1.490
Spirit of, B. P 871
Onchonia, liquid extract Yellow, B. P. about 1.100
Creasote,B. P 1.071
U. S. P 1.046
Ether, HP 785
•* U.S.P 750
" pure B. P 720
" fortior, U. S. P 728
Glycerine, B. P. and U. S. P 1.260
Iron, solution of Pemitrate of, B. P 1.107
U.S.P 1.065
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334 THE CHEMISTS' MANUAL.
Name. Sp. Gr.
Iron, solution of Persulphate of, B. P 1.441
« " U.S.P 1.820
^ Bfcrong solution of Perchloride of, B. P. 1.388
** tinctoie of Perchloride of, R P. and U. 8. P 992
Lead, solution of Sub^oetate of, B. P. 1 .260
U.S.P 1J367
Lime, Sacchaiated solution of , B. P. 1.052
" solution Chlorinated, B. P 1.085
Mercury (at O** C. = 32'' P.) 18.696
(at 15^55 C. = 60* P.) ia560
add solution of Nitrate of 2.246
" « « •' U.S.P 2.165
Nitre, Sweet Spirit of 845
" " " U.S.P 837
Oil of Mustard, B.P 1.015
Potash, solution of, B. P 1.058
U. S. P 1.065
Soda, solution of, B. P 1.047
U. S. P 1.071
" Chlorinated, B. P 1.108
U.S. P 1.045
Squill, Oxymel of, B. P 1.330
^jrup, B. P 1.330
'* U.S.P 1.317
« of Buckthorn, B. P 1.320
" of Ginger
«* of Hemidesmus 1.835
« of Iodide of Iron, B. P 1.885
" ofLemon,B.P 1.340
* of Mulberries, B. P 1.330
" of Orange Flower, B. P 1.880
« " Peel, B. P
" of Phosphate of Iron, B. P
" of Poppies, B. P 1.820
" of Red Poppy, B. P 1.380
" of Red Roses, B. P 1.385
" of Rhubarb, B. P
* of Senna, B. P 1.810
« of Squill, B.P
'» ofTolu,RP 1.830
Treacle, B.P about 1.400
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THE CHEMISTS' MANUAL.
236
TABLE OF SPECIFIC GRAVITIES AND WEIGHTS
(Trautwinb.)
In this Table the Sp. Gr. of Gases and Air are compared with that
of Water, instead of that of Air.
Naxxb of Substancm.
Atebaob
Sp. Ob.
Atxb. Wt.
OF A CU. FT.
INLBB.
Air, atmoBpheric ; at 60° F., and ander pressure of
one atmosphere, 14.7 lbs. per sq. inch, weighs ^^
pan as much as water at 60**
Alcohol pure
*' of commeroe
*• proof spirit ....*•• •
Ash, perfectly dry
1000 ft. board-measure weighs 1.748 tons.
ABh, American white, dry , average
1000 feet board-measure weighs, 1.414 tons.
Aluminum
Antimony, east, 6.66 to 6.74 average
" native
Anthracite, 1.8 to 1.84 ; of Penn., 1.8 to 1.7, usually
A cubic vard of anthracite averages 1.75 cu. yards
when broken to any market size, and loose.
Anthracite, broken of any size, loose average
** " moderately shaken '*
" heaped bushel, loose, 77 to 88 pounds. . .
A ton loose averages from 40 to 48 cu. ft. ; at 54
Ibe. per cu. ft., a cubic yard weighs .651 ton.
Asphaltum, 1 to 1.8 average
^smnth, cast ; also native "
BzBfls (copper and zinc), 7.8 to 8.4 ''
** rolled *'
Bronze (Cu 8 parts + Sn 1 part), gun metal, 8.4 — 8.6
Brick, pressed
" common hard
•* soft inferior
Brick-work. (See Masonry.)
Caldte, transparent, 2.51^2.78 average
Carbonic anhydride gas is 1^ times as heavy as air. .
Charcoals of pines and oaks average
Chalk, 2.2 to 2.8 **
Clay, potter's dry, 1.8 to 2.1 **
** dry in lump, loose **
Coke, loose, of good coal '*
" a heaped bushel, loose, 85 to 42 lbs.
" a ton occupies 80 to 90 cubic feet.
In coking, coal swells from 25 to 50 per cent.
Equal weights of coke and coal evaporate about
equal weight of water ; and each about twice
as much as equal weights of dry wood.
Cherry, perfectly dry average
lOiOO feet board-measure weighs 1.562 tons.
.00128
.793
.884
.916
.762
.61
2.6
6.70
6.67
1.5
1.4
9.74
8.1
8.4
8.5
2.62
.00187
2.5
1.9
.672
.0765
49.43
52.1
57.2
47.
162.
418.
416.
52 to 56
56 to 60
87.3
607.
504.
524.
529.
150.
125.
100.
164.
15 to 80
156.
119.
63.
23 to 82
42.
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236
THE CHEMISTS' MANUAL.
Naxxb of Substavcm.
Atxbaos
8p. Ob.
Ayxb. Wt.
OF A CU. FT.
IN LBS.
Coal, bitammoQB, 1.2 to 1.5 average
** •* broken of any aize, loose. . . .average
*« " moderately shaken **
" '< a heaped bushel, loose, 70 to 78 lbs.
« " a ton occupies 43 to 48 cubic feet.
A cubic yard, solid, averages about 1.75 yards when
broken to any market size, and loose.
Chestnut, perfectly dry average
1000 feet board-measure, weighs 1.525 tons.
Cement, hydraulic, American, Rosendale; ground,
loose average
Copper, cast, 8.6 to 8,8 *'
rolled, 8.7 to 8.9
Cork
Diamond, 8.44 to 3.55 ; usually 3.51 to 3.55
Earth, common loam, perfectly dry, loose. . . . ,
*' slightly moist, loose
" common loam as a soft-flowing mud
u «. « « u .* « pressed in
a box
Ether.
Elm, perfectly dry average
1000 feet board-measure weighs 1.302 tone.
Ebony, dry average
Emerald. 2.67 to 2.73 *'
Fat **
Flint "
Feldspar, 2.4 to 2.6 "
Garnet, 3.5 to 4.3 ; precious, 4.1 to 4.3 •'
Glaas, 2.5 to 3.45 "
" common window "
«* Millville, N. J. , thick-flooring "
Granite, 2.62 to 2.76 "
Gypsum (plaster of pans), 2.26 to 2.35 "
Gravel, about the same as sand. (See.)
Gold, cast, pure 24 carat •'
** native, pure, 19.3 to 19.4 "
'* pure, hammered *•
Gutta-percha "
Hornblende, black, 3.1 to 3.4 "
Hydrogen cas is 14i times lighter than air ; 16 times
lighter than oxygen
Hemlock, perfectly dry average
1000 feet board-measure weighs .930 tons.
Hickory, perfectly dry average
1000 feet board-measure weighs 1.971 tons.
Iron, cast, 6.9 to 7.4. average
" ** usually assumed at "
At 450 lbs., a cubic inch weighs .2604 lbs. ; 8601.6
cubic inches a ton ; and a lb. = 8.840O cubic
inches.
Iron, wrought, 7.6 to 7.9 ; the purest has the great-
est spedlc gravity average
1.85
.66
8.7
8.8
25.
3.53
716.
56.
1.22
2.7
.93
2.6
2.5
4.2
2.98
2.52
2.53
19.258
19.32
19.5
.98
3.25
.4
.85
7.15
7.21
7.77
84.
47 to 52
51 to 56
41.
60.
542.
548.
15.6
72 to 80
70 to 76
104 to 112
110 to 120
44.6
35.
76.1
58.
162.
156.
186.
157.
158.
168.
1204.
1206.
1217.
61.1
203.
.00527
53.
446.
450.
485.
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THE CHEMISTS' MANUAL.
237
KAMBB of SUBSTAITOBS.
Iron, large rolled bars average
« « « " nsuallj assumed at. . . **
•* sheet "
At 480 lbs., a cubic inch weighs .2778 lbs. ; and a
lb. =3.6000 cu. in. Light iron indicates impurity.
Ivory average
Ice "
India-rabber , "
Lard "
Lead, 11.35 to 11.47 "
Limestone and Marbles, 2.65 to 2.85 "
Idme, <^ck **
Lime, Quick, ground, loose, per struck bushel,
71 lbs average
Mahogany, Spanish, diy* "
•* Honduras, dry "
Masonry of Granite or Limestone* well dressed
throughout average
Masonry of Granite, roughly scabbled, mortar rub-
ble average
Masonry of Granite, roughly scabbled, dry rub-
ble average
At 155 lbs. per cu. ft., a cu. yd. weighs 1.868 tons ;
and 14.45 cu. f t = 1 ton.
Masonry of Sandstone about | part less than the
Masonry oiBrick work, pressed brick, fine joint, aver.
•**'** medium quality "
** ** " coarse inferior "
At 125 lbs. per cu. ft., a cu. yd. weighs 1.507 tons ;
and 17.»2 cu. ft. = 1 ton.
Mercury, at 32" Pah
at 60** Fah
at 212" Fah
Mica, 2.75 to 3.1 average
Mortar, hardened, 1.4 to 1.9 "
Mud, dry, close
" wet, moderately pressed
** wet, fluid
Naphtha
Nitrogen Gas is ^r part lighter than air
Oak, Live, perfectly drv, .88 to 1.02 average
" White. " " .78 to .88 "
" Ked, Black, &c "
Oils, Whale, Olive "
" of Turpentine "
Oxygen Gas, a little more than -fg part heavier than air
Petroleum
Peat, dry, unpressed
Pine, White, perfectly dry, .35 to 45
1000 ft. board-measure weighs .030 ton.
Pine, Yellow, Northern, .48 to .62
1000 ft. board-measure weighs 1.276 tons.
AVBBAOB
Sp. Gb.
7.6
7.69
.94
.93
.95
11.41
2.75
1.60
.85
.56
.55
AVBB. Wt.
OF A CU. irp.
IKLBB.
474
480
485
114
58.7
58
59.3
711
172
100
57
53
35
165
188
125
,_«
140
125
—
100
13.62
849
13.58
846
13.38
836
2.93
183
1.65
103
—
80 to 110
—
110 to 130
104 to 120
.848
52.9
—
.0744
.95
59.3
.83
518
32 to 45
.92
57.3
.87
543
.00136
.0846
.878
54.8
—
20 to 30
.40
25
34.8
* Green timbers usually weigh from ^ to nearly i more than dry.
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238
THE CHEMISTS' MANUAL.
Najcbs of Sttbbtanceb.
Pine, Yellow, Southern, .64 to .80
1000 ft. board-measure weighs 1.674 tons.
Pitch
Plaster of Paris ; see Gypsum.
Platinum, 21 to 22
" native, in grains, 16 to 19
Quartz, common, pure, 2.64 to 2.67
" " finely pulverized, loose
Ruby and Sapphire, 3.91 to 4.l6
Salt, coarse, per struck bu.^ Syracuse, N. Y., 56 lbs.
" Liverpool, fine, for table use, 60 to 62 lbs
Sand, of pure quartz, perfectly dried aud loose,
usually 112 to 183 lbs. per struck bushel
1 measure of solid quartz makes 1.75 measures of
loose, rounded sand.
Sand well shaken, 128 to 147 lbs. per struck bushel.
" ** packed
At 130 lbs. per cu. ft., perfectly wet, 17.28 cu. ft.
weigh 1 ton ; and a cu. yd. = 1.567 tons.
Extremely fine, even -grained sand, perfectly dry,
may weigh as little as 70 to 80 lbs. per cu. ft.
Sandstone, fit for building, dry, 2.1 to 2.73
Snow, fresh fallen
" moistened and compacted by rain
Sycamore, perfectly dry
1000 ft. board-measure weighs 1.876 tons.
Slate. 2.7 to 2.9 average
Silver "
Soapstone or Steatite, 2.65 to 2.8 "
Steel, 7.8 to 7.9 "
The heaviest contains least carbon.
Sulphur «
Spruce, perfectly dry "
1000 ft. board-measure weighs .930 ton.
Spelter or Zinc, 6.8 to 7.2 "
Tallow «'
Tar "
Topaz •*
Tin, cast, 7.2 to 7.5 "
Turf or Peat, dry, unpreesed
Water, pure rain, or distilled, at 32"^ F., barom. 30 in.
M H it QQO -p ^ u it
" " 80° P.i ** *'
Sea, 1.026 to 1 .030 average
Although the weight of fresh water is almost in-
variably assumed as 62J lbs. per cu. ft., yet 62J
would be nearer the truth, at ordinary tempera-
tures of about 70* ; or a lb. = 27.759 cu. in. ;
and a cu. in. = .5764 oz. Avoir., or .4323 oz. Trojr,
or 252.175 grains. The grain is the same m
Troy, Avoirdupois, and Apothecaries' weights.
Wax, Bees average
Wines, .993 to 1.04 "
Walnut, Black, perfectly dry "
Zinc or Spelter, 6.8 to 7.2 **
Zircon, 4.5 to 4.75 "
ArXBAOB
Sp. Qb.
.72
1.15
21.5
17.5
2.65
4.04
2.65
.97
.998
.61
7.00
4.62
Atbr. Wt.
OF A CU. WV.
nriAB.
45
71.7
1342
165
90
45
49
90tolOe
99 to 117
101 to 11»
2.41
150
—
5 to 12
—
15 to 50
.59
87
2.6
162
10.5
655
2.78
170
7.85
490
2
125
.4
25
7
487.6
.94
68.6
1
62.4
8.56
7.35
459
—
20 to 30
—
62.375
1
62.331
—
62.190
1.028
64.08
60.5
62.3
38
487.5
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J[ini{ital«08.
Digiti
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Digiti
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MINERALOGY.*
It ifl my object under this division to consider only those
minerals which have found more or less use in the arts.
Ores of the following elements will be considered :
1. Aluminium.
2. Antimony.
3. Absenig.
4. Bismuth.
6. Cadmium.
6. Calcium.
7. Caebon.
8. Chbomium.
9. Cobalt.
10. Copper.
11. Gold.
12. Iridium.
13. Iron.
14. Lead.
15. Lithium.
16. Magnesium.
17. Manganese.
18. Mercury.
19. Nickel.
20. Phosphorus.
21. Platinum.
22. PoTAssnjM.
23. Silicon.
24. Silver.
25. Sodium.
26. Strontium.
27. Sulphur.
28. Tin.
29. Zmo.
30. Zirconium.
16
* See Author's Preface.
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242
THE CHEMISTS' MANUAL.
I. ALUMINIUM.
The principal Aluminium minerals are :
HiNERAL.
Habdness.
8p. Gb.
FOBXULA.
Coiawmox,
Corundum
9
8.909-4.16
M
Al = 53.4
Diaspore
6.5—7
8.3-8.5
AlH
Al.Oj = 85.1
Aluminite
1-2
1.66
A1S + 9H
A1,0, = 29.8
Alunogen
1.5-2
1.6-1.8
^8sl8H
A1,0, = 15.4
Alunite
8.5—4
2—2.5
2.58—2.752
1.75
KS + 8A1S + 6H
ks + MS,+24H
Al.O, — 87.18
KiOinite
Al 8 = 18.4
Cryolite
2.5
2.9-8
8Na P + AljPj
Al = 13
Tupquois
6
2.6-8.88
A1,P + H
A1,0, = 46.9
WavelUte.
8.26—4
2.387
ik.l?', +12H
Al.O, = 37.3
CTuysoberyl
8.5
3.5-8.84
BeAl
Al,Oj = 80.2
CORUNDUM.
St/n. — Corindon, Sapphire, Ruby, Oriental Amethyst,
Smirgel, Emery. Color is red, blue, purple, yellow, brown,
gray and white. Streak, colorless. Transparent, translucent
to opaque. Lustre vitreous, sometimes pearly on the base,
and occasionally showing a bright opalescent star of six rays
in the direction of the axis. Crystallizes in a rhombohedron
of 86°4'. Sp. Gr., 3.909-416.
The different varieties of corundum are much used in the
arts. Large crystals of sapphire have been found at New-
town, N. J. Imperfect rubies have been found at Warwick,
N. J., and bluish crystals in Delaware and Chester Co., Penn-
sylvania. In California, in Los Angeles Co., in the drift of
San Fransisqueto Pass. In Canada, at Burgess, red and bine
crystals have been found.
Red sapphire is the most highly esteemed. A ciystal
weighing four carats, perfect in transparency and color, has
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THE CHEMISTS' MANUAL.
243
been valued at half the price of a diamond of the same size.
Corundum, under certain conditions, absorbs water and changes
to diaspore, and perhaps also to the mica-like mineral, marga-
rite (Dana). Corundum may be found artificially by exposing
to a high heat, 4 pts. of borax and 1 of alumina (Ebelmen) ;
by decomposing potash alum by charcoal (Gaudin) ; by subject-
ing in a carbon vessel fluoride of aluminum to the action of
boric acid, the process yielding large rhombohedral plates
(Deville and Caron); by the addition to the last chromic
fluoride, affording the red sapphire or ruby, or with less of the
chromic fluoride, blue sapphire, or with much of this chromic
fluoride, a fine green kind, by action of aluminic chloride on
lime (Daubree).
The following are elaborate analyses by J. Lawrence Smith,
taken from elaborate papers in the Am. J. Sci., II, x, 354,
xi, 53, xlii, 83. The column of hardness gives the effective
abrasive power of the powdered mineral, that of sapphire
being as 100 :
1. Sftpphlre. /fuHa
i Raby, "
3. ComndxaxL, AHa Mitiar.
4. " India
•L Emery, Kttlah
e. " Oiegler.
Habdhess.
100
90
77
68
W
Sp. Gb.
4.06
8.88
8.89
4J»
97.51
97.82
92.89
98.13
44.01
Haonx-
TITB.
1.89
1.09
1.87
0.91
88.35
••• (88.35
'^^l 50.81
Ca.
1.18
1.08
0.98
Si.
0.80
1.31
2.05
0.96
1.61
8.13
— =100.80
— = 99.63
1.60 = 98.88
2.88 = 98.87
1.90 =101.18
2.00 = 99.85
CRYOLITE.
This mineral is only found in Greenland, and has a very
extensive use in the arts (Formula, SNaF.AljFg). Its compo-
sition is Al 13.0, Na 32.8, Fl 54.0. Sp. Gr. 2.9-3.
" It crystallizes as a doubly oblique rhombic prism 88° 30',
and has a perfect basal cleavage. Its lustre is vitreous or
slightly pearly, and is nearly the same on the three cleavages
on the crystid. Its fracture is lamellar or scaly. It is gener-
ally white, and has about the same kind of lustre as a stearine
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THE CHEMISTS' MANUAL.
caDdle on the fracture. It is sometimeB colored slightly red,
or may be even brick red, when it is mixed with partially
altered siderite. Occasionally it is black."
Heated in an open tube, it gives up HFl. Soluble in sul-
phuric acid, giving off MFl. It is easily fusible, even in the
jflame of a candle, without the aid of the blowpipe. If it is
then thrown into water, there seems to be a commencement
of decomposition, for an alkaline carbonate or lime-water
throws down M ? Cryolite is shipped in large quantities to
Europe and the United States (Pennsylvania), where it is used
for making soda, and soda and alumina salts ; also of late in
Pennsylvania, for the manufacture of a white glass which is a
very good imitation of porcelain.
a. ANTIMONY.
The principal Antimony minerals are :
Habdnssb.
8p. Gb.
FOBMULA.
CoxPosinoK.
Native Antimony
8.85
6.646-«.72
Sb (when pure).
Sb = 100
Senarmonite
2—2.5
5.22-5.3
Sb
Sb= as.56
Valentinite
2.5-8
5.566
Sb
Sb= 83.56
Stibnite
2
4.516-4.612
SbgSs
Sb= 71.8
Kermesite
1—1.5
4.5—4.6
Sb + 2SbS,
Sb= 75 3
NATIVE ANTIMONY.
Crystallizes in rhombohedra of 87° 35' (Rose). Lustre is
metallic. Color and streak is tin-white. It is very brittle.
It contains sometimes silver, iron or arsenic as impurities.
Composition of a specimen from Andreasberg gave, according
to Klaproth, antimony 98, silver 1, iron 0.25 = 99.25.
The mineral allemontite has the following composition
(SbAsg) = arsenic 65.22, antimony 34.78. Analysis by Ram-
melsberg of the Allemont ore: arsenic 62.15, antimony 37.85=
100 given ISb to 26As.
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THE CHEMISTS' MANUAL. ^5
Antimony has been found native in the Harz, in Mexico ;
Hnasco, Chili ; South Ham, Canada ; at Warren, N. J.
Allemontite occurs sparingly at Allemont, Przibram in
Bohemia ; Schladmig in Styria, and in the Harz.
STIBNITE.
Stibnite, or gray antimony, furnishes the antimony of com-
merce, and is therefore the principal ore. Sometimes the
oxides senarmontite and valentinite are found in suflScient
quantity to be mined. Stibnite is orthorhombic. Hardness
= 2. Sp. Gr. = 4.516 (Haiiy); 4.62 (Mohs). It is a lead-
gray ore, usually fibrous or in prismatic crystals ; it has a me-
tallic lustre which is often bright. Streak is same as color,
lead-gray. •
Composition, SbgSg = sulphur 28.2, antimony 71.8 = 100
when pure. Eight analyses of stibnite from Arnsberg, West-
phalia, gave Schneider a mean of Sb 71.48, S 28.52, excluding
0.33 per cent of quartz.
It fuses without the aid of a blowpipe. On charcoal it
fuses, giving off' sulphurous and antimonious fumes. On char-
coal, in R. F., it gives antimony coat, and colors the flame green-
ish-blue.
Occurs with spathic iron in beds, but generally in veins.
Often associated with blende, heavy spar and quartz. It is met
in veins at Wolfsberg in the Harz ; abundant near Padstow
and Jiutagel ; abundant also at Borneo. In the United States
it is found in Maine, New Hampshire, and Maryland ; abun-
dant in the granitic range, south side of Tulare valley, near
pass of San Amedio. Specimens found in Nevada are usually
argentiferous (Humboldt mining region). It is also found in
New Brunswick.
As stated above, this ore affords nearly all the antimony of
commerce. " The crude antimony of the shops is obtained by
simple fusion, which separates the accompanying rock. From
this product most of the pharmaceutical preparations of anti-
mony are made, and the pure metal extracted." " This ore
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THE CHEMISTS' MANUAL.
was used by the ancients for coloring the hair, eyebrows, etc.,
to increase the apparent size of the eye." The ore changes on
exposure by partial oxidation to antimony bUnde (2Sb2S3-h
5^203), and by further oxidation to vaUntinite (Sb203). Anff-
mony ochre (Sb203 + 86205), and also 56205 + 5H are other
results of alteration (Dana).
3. ARSENIC.
The principal Arsenic minerals are :
MiNBBAL.
Hardness.
8p. Gb.
Pee Cert
WHEN Pdbb.
Native Arsenic
Arsenolite
3.5
15
1.5—2
1.5—2
5.93
3.698
8.4-3.6
3.48
As
As
AsS
AsjS,
As = 100
As — 75.76
Realgar
As — 70.1
Orpiment . . . . ;
As — 61
NATIVE ARSENIC.
Native arsenic is one source of arsenic, but it is too rare to
amount to much. It is found in veins in crystalline rocks,
and in older scliists, and is generally accompanied by other
ores. It crystallizes as a rhombohedron of 85° 41'. Hardness
= 3.5. Sp. Gr. 5.93. When pure, is composed only of ai'senic ;
but it generally contains some antimony, and traces of iron,
silver, gold or bismuth. The arsenical bismuth of Wenier is
arsenic containing 3 per cent, of bismuth (Hardness = 2. Gr. =
5.36-5.39). An antimonial arsenic, containing, according to
Schultz, 7.97 per cent, of antimony, occurs at the Palmbaure
mine, near Marienberg, Saxony. A similar compound, con-
sisting, according to Genth, of arsenic 90.82 and antimony 9.18
(= 17As4-lSb), occurs at Washoe Co., California.
Native arsenic gives metallic arseific in a closed, and As in
an open tube. In the R. F. it volatilizes without residue and
without melting, coloring the flame blue. It is not attacked
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THE CHEMISTS' MANUAL. 247
by HClj but is soluble in HNO3. I^ ^^ found in considerable
quantity in the silver mines at Freiberg, Annaberg, Marien-
berg and Schneeberg. Abundant at Chauarcillo and else-
where in Chili. In the United States, it has been observed
by Jackson at Haverhill, N. H., in thin layers in dark-blue
mica slate, stained by plumbago, and containing also white
and magnetic pyrites ; found also at Jackson, N. H., and on
the east flank of Furlong Mountain, Greenwood, Me.
REALGAR.
Realgar has the following composition when pure: sul-
phur 29.9, arsenic 70.1 = 100 (AsS). A specimen from Spain
gave S 30.00, As 70.25 (Hugo Miller, J. Ch. Soc, xi, 242).
Hardness = 1.5-2. Sp. Gr. = 3.4^3.6. Lustre resinous. Color
is bright-red and vitreous. Streak red when not decomposed,
but generally orange-yellow.
In closed tube, it fuses and volatilizes without decompo-
sition ; in open tube gives sulphurous fumes and a white crys-
talline sublimate of arsenious acid. Soluble in caustic alkalies.
Realgar crystallizes as an inclined rhombic prism 74° 26'.
It is always crystallized or crystalline. It is found in the
Harz ; at Tajowa in Hungary in beds of clay, and at Bumen-
thal, Switzerland, in dolomite.
ORPIMENT.
Formula AsgSg = sulphur 39, arsenic 61 = 100. Hardness =
1.5-2. Sp. Gr.=3.48(Hoidinger) ; 3.4 (Breithaupt). Its color
is decided lemon-yellow; sometimes slightly orange-colored,
owing to admixture of realgar. Streak is yellow — generally
a little paler than color. Lustre pearly upon the faces of
perfect cleavage ; elsewhere resinous.
In a close tube it fuses and volatilizes, giving a dark-yellow
sublimate; acts otherwise like realgar. Dissolves in nitro-
hydrochloric acid and caustic alkalies.
Orpiment crystallizes as a right rhombic prism 100° 40'. It
is usually found in foliated and fibrous masses, and in this
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THE CHEMISTS' MANUAL.
form is fonnd at Kapnik in TranBylvama, and at Felsobanza
in Upper Hungary;, in Fohnsdorf, Styria, found in brown
coal. Small traces are met with in Edenville, Orange Co.,
N. T., on arsenical iron.
The arsenic of commerce is mostly obtained from the arsen-
ical ores of iron, cobalt and nickel, which see.
4. BISMUTH.
The principal Bismuth minerals are :
Habdivisb.
Sp. Qb.
CoxpoBmov.
PKBCbHT OF,
▼HXN PCBX.
Native Bismuth...
Bismuthinite
Alkinite
2-2.5
2
2-2.5
1.6—2
9.727
6.4^7.2
6.1-6.8
7.2—7.9
Bi
Bi.S.
8(CuPb)8+BigS,
Bi.Te,
Bi=100
Bi= 81.25
Bi — S6 2
Tetradymite
Bi= 61.9
NATIVE BISMUTH.
Native bismuth is the source of bismuth in the arts. When
pure contains only bismuth; it generally contains, though,
traces of arsenic, sulphur and tellurium. A specimen analyzed
by Genth (Am. J. Sci., II, xxvii, 247), gave Bi = 99.914,
Te 0.042, Fe trace = 99.956. A specimen analyzed by
Forbes (Phil. Mag., IV, xxix, 3), gave Bi 94.46, Te 5.09,
As 0.38, S 0.07, Au trace = 100.00. Hardness = 2-2.5. Sp. Gr.
= 9.727. Color silver-white, with a reddish tinge. Lustre
metallic. Opaque. Streak same as color ; subject to tarnish.
Sectile. Brittle when cold, but when heated somewhat mal-
leable. It melts in the flame of a candle. On Ch fuses and
is entirely volatilized, leaving a yellow coating. It is not
attacked by HCl. Fuses at 476° F. Dissolves in HNO3 ; ^^^
sequent dilution causes a white precipitate. Crystallizes
readily from fusion.
Bismuth is found native in veins in gneiss and other crys-
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THE CHEMISTS' MANUAL. 249
talline rocks and clay slate accompanjing yarious ores. It is
most abundant at the silver and cobalt mines of Saxony and
Bohemia. Has been found at Lane's mine in Monroe, Conn. ;
also at Brewer's mines, Chesterfield District, South CaroUna.
BiSMUTHINITE.
Bisthmuthinite when pure has the following composition :
Bismuth 81.25 -f sulphur 18.75 =^ Bi2S3. When impure, it
may contain in small quantities, Fe, Cu, Au, Pb, Te, Se. A
specimen (Oravicza) analyzed by Hubert (Haid. Ber. iii, 401)
gave Bi 74.65, S 19.46, Fe 0.40, Cu 3.13, Au, 0.53, Pb 2.26 =
100.33. Hardness = 2. Sp. Gr. 6.4-6.459 ; 7.2 : 7.16 Bo-
livia (Forbes). Color lead-gray or tin-white, with a yellowish
or iridescent tarnish. Streak same as color. Lustre metallic.
Opaque. CrystaDizes as a right rhombic prism 91° 30'.
In an open tube gives sulphurous fumes and a bismuth sub-
limate, which before the blowpipe fuses into drops, brown
while hot and opaque-yellow on cooling. Fus. = 1. Dis-
solves in nitric acid and gives a precipitate on diluting.
Sometimes found massive, with a foliated or reticulated
structure. Generally found associated with other minerals.
Accompanies molybdenite and apatite in quartz at Brandy Gill
in Cumberland. Occurs with gold, pyrite chalcopyrite in
Rowan Co., N. C. Found with chrysoberyl at Haddam, Ct.
(according to Shepard).
5. CADMIUM.
The principal Cadmium mineral is
GREENOCKITE.
When pure, Greenockite has the following composition:
Cd 77.7, S 22.3 = 100 (CdS or GdaSa). A sample analyzed
by Connel, gave cadmium 77.30 and sulphur 22.56 = 99.86.
Hardness = 3-3.5. Sp. Gr. = 4.8 (Brooke) ; 4.9-4.999 (Breit-
haupt) ; 4.5, the artificial (Sochting).
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THE CHEMISTS' MANUAL.
"Lustre adamantine. Color honey-yellow, citron-yellow,
orange-yellow, vein parallel with the axis, bronze-yellow.
Streak-powder between orange-yellow and brick-red. Nearly
transparent. Strongly double refraction." Not thermoelectric
(Breithaupt).
In a closed tube assumes a carmine-red color while hot,
fiiding to the original yellow on cooling.
In open tube gives sulphurous acid. Gives reddish-brown
coating on charcoal in R. F. Soluble in hydrochloric acid
with effervescence of hydrogen sulphide.
Found at Bishoptown, Scotland, in short hexagonal crystals,
136° 24'. Found at the Ueberoth zinc mine, near Friedens-
ville, Lebigh Co., Pa.
Named after Lord Greenock (late Earl Cathcart).
6. CALCIUM.
The principal Calcium minerals are :
MiNBBAL.
Hard-
NBse.
Sp. Gb.
FOBMULA.
CoxpoBinoH.
Anhydrite....
8-3.5 2.88^-3 895
CaS
08 = 41.2; '8 = 58.8
GypBum
1.5-8 2.814-8.28
1
CaS + aH
08 = 88.6; '8 = 46.6; H = aa9
Plnorite
4 8.01 -8.26
CaFl
Ca = 61.8; Fl = 4a7
Apatite
4.5-6
2.98 —8.25
Ca,P+iCa(Cl,F)
J Ca=48.43; >'=40.92 (=89.85 P,Ca),
1 Cl=6.81 ; Ca=8.84 (=10.65 Cl,Ca).
Pharmacolite.
2-2.5
2.64 -2.78
(jCa iH), As
Ca = 84.9 :'ab = 61.1; H = 84
Aragonitc...
8.5-4
2.987—2.947
CaO
Ca = 66;C = 44
Calcite
2.5-a5 2.508-2.729
. CaC
Ca = 66: C = 44
Dolomite
8JJ-4 ' 2.8 —2.9
CaC + MgC
6aC = 64.85; MgC = 45.66
Sclieelite
4.6-6.81 5.9 —6.076
CaW
Ca = 19.4; W = 80.6
GYPSUM.
Gypsum has the following composition when pure: Lime
32.0, sulphuric acid 46.5, water 20.9 = 100 (CaSH-2H).
The different varieties have the following composition :
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251
L Cryttamzea
2. Granular.
5. Alhay, flhrout
4. WIcnrode, oofTifKK^.
6. Ofiterode, **
a ** white
7. ** rtd
s.
1 .
Ca.
1
8l
44^
88.0
81.0
__
41.16
83.8B
21.0
—
44.19
89.41
80.18
6.48
46.76
81.87
19.90
8.80
45.95
82.63
80.70
0.43
46.61
8S.44
80.74
0.15
46.50
81.99
81.66
—
Ai'Fv.
— = 96.8 Bucbolz.
— = 99.04 Roso.
064 = 100.85 Trobe.
0.60 = 100.93 JOngsU
0.60 = 100.19
— = 99.94 Hampe.
0.46 = 100.80 "
Gypsum takes the form of a right rhombic prism of 138** 28',
and has three cleavages. Hardness = 1.5-2. Sp. Gr. = 2.314^
2.328, when pure crystal. Massive varieties sometimes glis-
tening, sometimes dnll earthy. It has a vitreous lustre which,
on some of the faces, may be adamantine.
Its colors are very variable,, generally not very sti'ong.
The color is usually white, although it may be gray, flesh-red,
honey-yellow, ochre-yellow, and blue; impure varieties are
often black, brown, red, or reddish-brown. It often has Fe
interposed when it is red. Streak is white. It is often trans-
parent or translucent.
Heat immediately expels the water from gypsum, and leaves
it white. It then fuses at 2.5 to 3, coloring the flame reddish-
yellow. On charcoal in R. F. it is reduced to sulphide. If
not ignited above 260° C, it will unite with water if moistened,
and becomes firmly solid. Soluble in muriatic acid and in
400 to 500 parts of water.
Gypsum often forms extensive beds in connection with
stratified rocks, especially limestones and marlites or clay-
beds. Fflle specimens of gypsum are found at Bex in Swit-
zerland ; large cuticular crystals have been found at Mont-
martre near Paris. A noted locality of alabaster occurs at
Castellina, 35 miles from Leghorn, whence it is taken to
Florence for manufacture of vases, figures, etc. This species
occurs in extensive beds in several of the United States, more
particularly New York, Ohio, Illinois, Virginia, Tennessee,
and Arkansas, and is usually associated with salt springs.
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THE CHEMISTS' MANUAL.
Also in Nova Scotia, Peru, etc. Handsome selenite and
snowy gypsum occurs near Lockport, N. Y. Large-grouped
crystals are found on the St. Mary's in clay in Maryland.
Large beds of gypsum are found with rock salt in Washington
Co., Virginia. Selenite and alabaster are found in Davidson
Co., Tenn. It has the form of rosettes or flowers, vines, and
shrubbery in Mammoth Cave, Ky. Abundant, also, w^est of
the Mississippi in many places.
" Plaster of Paris (or gypsum that has been heated and
ground up) is used for making moulds, taking casts of statues,
medals, etc., for producing a hard finish on walls ; also in the
manufacture of artificial marble, as the scagliola tables of Leg-
horn, aud in glazing of porcelain. The fibrous variety, when
cut en cabochon and polished, resembles cat's-eye."
The Montmartre gypsum quarries, near Paris, have been
famous for aifording browp gypsum, which, on account of
locality, is called Plaster of Paris.
CALCITE.
Calcite, when pure, is composed of carbonic acid 44, and
lime 56 = 100 (CaC). A portion of the lime of calcite is fre-
quently replaced by Mg, Fe, Mn, Sr, Ba, Zn, Pb. The color
of calcite is usually white, but is sometimes yellowish, gray,
red, green, blue, violet, yellow, brown, and black, fie pro-
duces different shades of red, from flesh-red or paler to opaque
blood-red, and brownish-red according to the proportions
present ; the latter, Hausmann names Hcematoconite, as in the
marble Rosseautico of Italy. ■Fe2*^3 causes yellowish to opaque
ochre-yellow and yellowi8h-bro\vn ; the deeper sideroconite of
Hausmann. Ferrous oxide, chromic oxide and ferric silicate
cause shades of green.
When calcite is perfectly pure, it crystallizes in rhombohedra
of 105° 5'. Hardness = 2.5-3.5 ; some earthy kinds (chalk,
etc). Sp. Gr. = 2.508-2.778; pure crystals 2.7213-2.7234
(Bend); fibrous camellar and stalactite 2.70-2.72, but when
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THE CHEMISTS' MANUAL. 253
palyerized, 2.729-2.7233. Streak is white or grayish. Lustre
vitreous, sub-vitreous, earthy. Transparent, opaque. Double
refraction strong.
When heated in a closed tube it sometimes decrepitates.
It is infusible, but gives a very luminous flame, coloring it
red (Ca). It is the same phenomena, on a small scale, that
is produced with the Drummond Light. When heated on
platinum foil with soda it fuses to a clear mass. The C is
expelled by heat and Ca remains ; when this is moistened on
the finger a sensation of heat is produced. It effervesces very
readily with acids, even in the cold.
Andreasberg, in the Harz, is one of the best European
localities of crystallized calcite. In Iceland, a single rhombo-
hedron over six yards long and three high has been observed.
Crystals are found also in many parts of the United States,
in New York in St. Lawrence and Jefferson counties, espe-
cially at Rossie lead-mine ; one nearly transparent is in the
cabinet of Tale College, weighing 165 pounds. In New
Hampshire, Massachusetts, New Jersey ; in Virginia, stalac-
tites are found of great beauty; also in the large caves of
Kentucky. At the Lake Superior copper-mines, splendid
crystals are found, containing scales of native copper.
CoEALS, of which reefe are formed, consist mainly of car-
bonate of lime (CaC).
B. SiUiman, Jr., obtained for a recent species of madrepora:
carbonate of lime, 94.807; phosphates, fluorides, etc., 0.745;
organic matter, 4.448. And the deposits of phosphates and
fluorides afforded the percentage. Si 12.5, Ca 7.5, Mg 4.2,
MgF 26.62, CaF 26.34, MgP 8.00, Al and fe 14.84.
Maeble. — ^Under this name a number of varieties of calcite
are included, which are sought after in the arts. In fact, when
the granular limestones are compact, and are fit for polishing
or for architectural or ornamental use, they are called marbles.
The colors are various. Statuary Marble is pure white, fine-
grained, and firm in texture. The Paiian marble, from the
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254 ;rHE CHEMISTS' MANUAL.
island of ParoB, and the Carrara^ of Modena, Italy, are among
the best statuary marbles.
What is sought after in marble is a uniform disposition of
the coloring material; these colore may be imiform white,
black, yellow, and red. Variegated marbles are also much
sought after. Marbles colored in veins of black and white are
called St. Anne.
The Porter^ called sometimes Egyptian marble, is of black
color, handsomely veined with yellow dolomite, and comes
from Porto-venere, near Spezzia. Marbles are not necessarily
exclusively composed of carbonate of lime ; thus, the marble
called verd-antique is iilled with veins of serpentine and talc.
Shdl Marbles include kinds consisting largely of fossil shells.
Madreporic marble contains corals. Encrinal contains cri-
noidal remains.
Euin Marble is a kind of compact calcareous marl, showing,
when polished, pictures of fortifications, temples, etc., in ruins,
due to oxide of iron.
Lithographic Stone is a very even-grained, compact lime-
stone, usually of buff or drab color.
Breccia Marble is made of fragments of limestone cemented
together. Colore are various.
Pudding-stone Marble consists of pebbles or rounded stones
cemented.
Hydraulic limestone is an impure limestone. The French
varieties contain 2 or 3 per cent, of magnesia and 10 "to 20 of
silica and alumina (clay). The varieties in the United States
contain 20 to 40 per cent, of magnesia and 12 to 30 per cent,
of silica and alumina. A variety worked extensively at Eon-
dout, N. Y., contains, COg 34.20, lime 25.50, magnesia 12.35,
silica 15.37, alumina 9.13, sesquioxide of iron 2.25. Accord-
ing to Prof. Beck (Min. N. Y., 78), oxide of iron is rather
prejudicial to it than otherwise.
Carrara Marble has the following composition, according
to Kseppel (J. Pr. Ch., Ivii, 324) : CaC 98.765, MgC 0.900,
Si 0.006, fe, Mti, Al 0.083, sand 0.1560, P and loss 0.090=100.
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THE CHEMISTS' MANUAL. 5^55
DOLOMITE.
When dolomite is pure, it has the following composition :
CaC 54.35, MgC 45.65 (CaC+MgC). Crystallizes in rhombo-
hedron, the angle of which, on account of its variation of
composition, varies between 106° 10' and 106° 20'. Hardness
= 3.5-4. Specific gravity, 2.8-2.9, true dolomite. Lustre
vitreous, inclining to pearly in some varieties. Colors are not
very decided, although it may be white, reddish, or greenish-
white ; also rose-red, green, brown, gray, and black. A very
rare variety, miemite, has a very decided green color (aspara-
gus green), owing to the presence of iron. Part of the
magnesia is replaced in some dolomites by protoxide of iron,
manganese, and, more rarely, oxide of cobalt and zinc.
A sample of dolomite from Westchester County, N. Y.,
gave, according to Akop (Ann. Lye, N". T., viii) : CaC 54.91,
MgC 43.63, FeC 1.23, insol. 1.30 = 100 oz.
A sample of miemo, miemite (Ranmielsberg, Min. Ch., 213),
gave: CaC 57.91, MgC 38.97, FeC 1.74, MnC, 0.57 = 99.19.
A sample of Jena, crystallized, uncolored, gave, according to
Suckow: CaC 55.2, MgC 44.7 = 99.9.
T. S. Hunt says that dolomites make up the chief part of
the Calciferous,. Clinton, Trenton, Guelp, Niagara, and Onon«
daga limestones of Canada. Thus we see that the limestone
strata of the globe is partly dolomitic.
Before the blowpipe it acts like calcite, but with nitrate of
cobalt the presence of magnesia can be ascertained. Dolomite
does not effervesce as easily as calcite, especially when pure.
If in a powdered state and heated, the acid dissolves it. Ter-
riferous dolomites become brown on exposure.
Dolomite is found at Salzburg, the Tyrol ; Hungary, Frei-
berg, in Saxony. Li the United States, in Vermont, at Box-
bury ; in Rhode Island, at Smithfield ; New Jersey, at Hobo-
ken ; New York, at Lockport, Niagara Falls, and Rochester.
Dolomite is sometimes used for making lime ; some varieties
are used as marble. It is also used in the manufacture of
Epsom salts.
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THE CHEMISTS' MANUAL.
7. CARBON.
Carbon occure in nature crystallized as the Diamond and
as Graphite.
DIAMOND.
The diamond is nearly, chemically, pure carbon. It ciya-
tellizes in the Isometric system. Its forms are various. Its
usual forms are, though, the octahedron and the hexoctahedron.
Hardness = 10. Sp. Gr. = 3.52955 (Thompson); 3.55 (Pe-
louze). Color white or colorless ; occasionally tinged yellow,
red, orange, green, blue, brown, and sometimes black. Lustre
brilliant adamantine. Transparent, translucent, and opaque.
Fracture conchoidal. Index of refraction 2.439. Exhibits
vitreous electricity when rubbed.
The crystals often contain numerous microscopic cavities, as
detected by Brewster, and some are rendered nearly black by
their number. The black planes of diamonds reflect all the
light that strikes them at an angle exceeding 24° 13', and
hence comes the peculiar brilliancy of the gem. In black
pebbles or masses called carhonada^ occasionally 1000 carats
in weight. Hardness = 10. Sp. Gr. = 3.012-3.416. Consist
of pure carbon, excepting 0.27 to 2.07 per cent.
The diamond was burned in the academy at Florence for
the first time in 1694, by a powerful burning-glass. The
crystalline colorless varieties gave only 0.01 per cent, of ash.
In the colored varieties the proportion is lai'ger, the black
diamond giving 2-3 per cent.
The Ancients knew nothing about cutting diamonds, and
wore the natural stone. Louis Berquen of Bruges in Belgium,
in 1456, discovered for the first time the method of cutting the
diamond so as to increase its lustre. Diamonds not fit to cut
are used for ends of tools for drilling or turning hard rocks,
such as granite or porphyry. The small stones which have a
very sharp edge are used for cutting glass. The clear stones
of diamonds have long been used as jewels for watches. The
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THE CHEMISTS' MANUAL.
257
black diamond has also been used for a long time for turning,
and lately in this country for drilling the harder rocks.
A diamond of 5-6 carats is a very large stone ; those of
12-20 are very rare, and very few are known that weigh more
than 100 carats.
WEIGHT OF THE LARGEST DLOfONDS KNOWN.
Naxs.
Baiah
Great Mofpil
Orioff
Koh-i-noor
Portogaeae
Florentine
Begent.
StaroftheSoath..
Koh-i-noor (recat)
Shah
SaUaoofTarkey..
Uhcut.
CtTT,
__
867 carats.
900 carats.
2T»A"
—
194i *«
798 "
186 "
—
148 **
—
WH "
410 "
186f •*
a5U "
1S5J "
—
106A"
—
96 "
—
84 "
Name,
Piggott
Naseac ,
Dresden ,
Saacy ,
Eugenie
Pa»ha
Dresden (green)
Hope (blae)....
Polar Star
Camberland ,
BasBian(red)....
Uhout. Cut.
801 carats.
carats.
As the diamond is very difficult to distinguish from some
closely allied stones, it is better not to trust to the judgment
alone, though some jewelers think they can detect the diar
mond with ease.
The following table, given by Prof. Egleston, affords a
scientific means :
TABLE FOR DISTINGUISHINa PRECIOUS STONES.
Storx.
DXHBITT.
Retbaction.
INDSX OT
Refraction.
Diamond
8.5a-a66
&»-4.8
8.5-8.8
84-^.6
8.8-8.5
8.ft-2.8
8.4-8.8
4.4—4.6
a6-«.8
Var. 8.5
Simple.'
Doable, 1 axis.
Doable.
Doable, 2 axes.
Doable.
Doable, 1 axis.
Simple.
Doable, 1 axis.
Doable, 1 axis.
Simple.
S.466
1.766
1.760
1.685
1.660
1.585
1.766
1.990
1.549
PoBitivc, not darable.
Bnby, 8«pphire, and
Oriental Amethyst
Chrysoberyl
White Topaz
Chrysolite
LastB BeTeral hoare.
LaetB several hoare.
More than 24 hoarc.
Poeitive.
Kmerald ....»-
Positive.
Spinel
Not tried.
Zircon.
Positive, not darable.
Onartz
Positive, not durable.
Strass
— Not darable. variable.
17
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258 THE CHEMISTS' MANUAL.
Some diamonds have red, white and black spots, and if the
diamond is heated to redness, protected from the air, these
spots disappear. This would seem to speak for the formation
of the diamond below red-heat. Jacqnelin transformed the
diamond into graphite by exposing it to an electrical current,
which seems to prove that diamond and graphite are only
allotropic conditions of carbon. The diamond has been formed
probably, like coal, by a slow decomposition of substances
containing carbon, whether vegetable or mineral, or even
animal matters. Many attempts have been made to make the
diamond artificially, but only very small crystals, if any, have
been formed.
The finest diamonds have been obtained from the mines of
India, which are no longer worked. There are diamond mines
in the Urals and in Brazil. The Brazil mines were opened in
1727, and it is estimated that at least two tons of diamonds
have been obtained from them. Diamonds are also largely
found in Africa, in the province of Constantine. In the United
States, a few crystals have been found in Kutherford Co., N. C,
and Hall Co. (Am. J. Sci., II, ii, 253, and xv, 373) ; they have
been found also in Portis mine, Franldin Co., N. C. (Genth) ;
one handsome one, over one-third of an inch in diameter, was
found in the village of Manchester, opposite ^Richmond, Va.
Diamonds have also been found in California, Kevada and
Colorado.
A diamond, when cut and polished, of the purest water
(perfectly colorless, without any defects), weighing one carat,
is valued at £12 in England ; and the value of others is calcu-
lated by multiplying the square of the weight by 12, except
for those exceeding 20 carats, the value of which increase at a
much more rapid rate. The slightest tinge or color, or defect,
affects greatly the conmiercial value.
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THE CHEMISTS' MANUAL.
259
GRAPHITE.
Graphite is also called Plumbago and Black Lead. Its
composition is pure carbon, with often a little oidde of iron
mechanically mixed.
The following analyses have been made of different graphites
by C. M6ne (C. R, Ixiv, 1091, 1867) :
Sp.Qb.
Cakbov.
Vol.
AilH.
CoMPOsmoK 100 Pabts Abb.
Si.
ib].
Fe.
MgCa.
A]k.aDd
I0B8.
Ural,Ht.AUbert.
Camberlnnd, Eag.
CeAA, Brazil
9.17B9
2J)4S6
S.8B66
94.08
91.55
77.16
O.W
1.10
S.56
6.S6
7.85
90.80
64j2
08.6
79.0
94.7
sas
11.7
10
19
7.8
0.8
«.o
1.6
0.8
1.9
Eegnault (Ann. Ch. Phys., II, i, 202) found :
LocAurm.
C.
H.
Abb.
Canada (I)
8&8
760)5
96.66
0.6
0.70
1.84
19.6 - 99.9
(ID
98.40 - 100 45
" (HI)
0.90 — 100.10
Hardness = 1-2. Specific gravity = 2.0891 ; of Ticonder-
oga, 2.229 (Kenngott); 2.14 (Wunsiedel, Fuchs). Color, black.
Streak, black and shining. Lustre metallic, opaque. Sectile ;
soils the fingers. Infusible. Bums at a high temperature,
without flame or smoke, leaving usually some oxide of iron.
Not acted on by acids.
Graphite in some places is coal altered by heat. It is
largely used in the arts for the manufacture of lead pencils
and crucibles, also as a lubricator. It is found at Burrowdale,
in Cumberland. Found in the United States in Massachu-
setts, Rhode Island, Connecticut, Vermont, New York, and
elsewhere.
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THE CHEMISTS' MANUAL.
8. CHROMIUM.
The principal Chromium mineral is chromite (Fe, Cr, Mg)
(M, Fe, €r). This mineral, called also chromic iron, is the
ore which furnishes the chromium in the arts. When pure,
contains oxide of iron 32, and oxide of chromium 68 = 100
(Fe -Gr).
The following table* contains a number of analyses of
chromic iron :
LocALimefl.
Pb.
Me.
•ek.
'id..
8l
1. Cheater County, Pa
2. •*
8. Baltimore (maeBlve)
4. " (cryBtolllaed)....
85.14
$^88.95
18.97
20.18
9.96
7.45
61.56
60.84
4491
60.04
9.72
0.98
18.85
11.86
2.90 = 99.82
0.62, Ni0.10
0.88 = 98.36
— =99.46
Hardness = 5.5. Specific gravity, 4.321, crystals (Thom-
son); 4.498, a variety from Styria ; 4.568, Texas, Pennsylvania.
Lustre is semi-metallic. Fracture uneven. Color, brownish-
black. Streak, brown. Opaque. Sometimes slightly mag-
netic. Chromic iron is one of the spinels of iron, a sort of
magnetite, and cannot be distinguished from magnetite with
certainty except by its chemical properties.
Chromic iron is not fusible before the blowpipe; in R. F.
becomes slightly rounded on the edges, as also magnetic.
With borax and salt of phosphorus when cool giv^e chrome-
green color ; the green color is heightened by fusion on char-
coal with metallic tin. It is not attacked by acids, but
decomposed by fusion with bisulphate of potash and soda.
Occurs in serpentine, forming veins, or imbedded masses.
It assists in giving the variegated color to verde-antique
marble.
* Analysis No. 1, Seybert (Am. J. Sci., iv, 321) ; No. 2, Starr (Am. J. ScL,
n, xiv); No. 3, Abich ; No. 4, Abich (Pogg., xxUi, 335).
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THE CHEMISTS' MANUAL.
261
It is found in large quantities in veins or masses in serpen-
tine, at Baltimore, Md. Found in crystals abundantly in
Pennsylvania. Found massive in New Jersey, Vermont,
Massachusetts, and California.
The ore obtained in England is procured mostly from Balti-
more, Drontheim, and Shetland Isles ; it amounts to 2000 tons
annually.
9. COBALT.
The principal Cobalt minerals are :
Naxb.
Habd-
KSBS.
Sp. Ob.
FOBXULA.
Unnsite
S.6
4.8-6
2Co 8 + Co S,
Co = 68; 8 = 48
Bieberite
-?-
1.934
(Co, Mg) 8 + 7H
Co = 26.6; 8 = 28.4; H = 46.1
Smaltite
6.6-6
6.4-7.2
(Co, Fe, Nl) Ab.
Co=9.4; A8=72.1; Nl=9.5; Fe=9
CJobaltite
6.6
6-6.8
Co (8, A8),
Co = 85.6 ; As = 46.2; S = 19.8
Erythrite
1.6-2.6
2.948
Co is + 8H
Co=87.65; *A8=88.48; H=84.02
-?-
-_f —
-?-
-?-
Earthy Cobalt.
j-w
8.16-8.20
(Co, Ca) Mn, + 4H
Sometlmea 825C Co
SMALTITE.
The composition of smaltite when pure is Co = 9.4 ; As =
72.1 ; Ni = 9.5 ; Fe = 9.0 (Co, Fe, Ni) Asg. The following are
a few analyses :
LocAums.
Ab.
Co.
Ni.
1.79
9.44
25.87
Fb.
Ccr.
S.
Bx.
1. Schneeberg
TD.87
TO.11
60.42
18.96
8.82
10.80
11.71
11.86
0.80
1.39
0.66
4.78
2.11
0.01 - 99.88
1 Chatbam, Conn
8. Hichelndorf, Conn...
- =100
— =100
AnaljBlB No. 1 was made by Uoflknann (Pog]^., xxr, 486) ; No. 2 by Genth ; No. 8 by
Bammelflbergr.
Hardness = 5.5-6. Specific gravity, 4.4-7.2. Color gen-
erally a silver or tin white, sometimes iridescent or grayish
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THE CHEMISTS' MANUAL.
frozntamiBb. Streak grayish-black. LoBtre metallic. Brittle.
Fracture granular and uneven.
On cbarcoal it gives off arsenic, and Aises to a globule. In
a closed tube gives a sublimate of metallic arsenic ; in an open
tube a white sublimate of arsenious acid, and sometimes traces
of sulphurous acid. With the fluxes it affords the reactions for
Co, Fe, and Ni. It is not attacked by the non-oxidizing acids.
Occurs with silver and copper at Freiberg and particularly
at Schneeberg, in Saxony. It has been found at Chatham,
Conn. ; also in crystals at Mine La Motte, Missouri. It is
used for making smalt ; hence its name.
COBALTITE.
Cobaltite has the following composition when pure : Cobalt
= 35.5 ; arsenic = 45.2 ; sulphur = 19.3 [CoSj 4- CoAsj or
Co (S, As)2]. The cobalt, though, is sometimes replaced
largely by iron, and sparingly by copper.
LOOALXTIBS.
S.
Ab.
Co.
Fb.
1. Skntternd
% "
ao.o6
S0.a6
19.06
48.46
42.97
48.14
38.10
8S.07
9.63
8.28 = 99.87
8.48, quartz 1.68 = 10084
8. Slegen pliimo8&
24.99, Sb 1.04, Ca 2.86, gangne 0.59=100.'2S
Analysis No. 1 was made by Stromeyer (Scbw. J., xlx, 886).
'* No. 2 '^ ^ Ebioghans (Ramm., 4th Suppl., 116).
'* No. 8 '' '' Heldlngsfdd (Bamm., 5Ui SappL)
Hardness = 6.5. Specific gravity = 6-6.3. Color silver
white, often a little rosy and also grayish, if much iron is
present. Streak grayish-black. Lustre metallic Fracture
uneven and lamellar. Brittle.
Not altered in a closed tube, but in an open tube gives
sulphurous fames, and a crystalline sublimate of arsenious
acid. On charcoal, affords fumes of sulphur and arsenic, and
ftises to a magnetic globule. With the fluxes gives the reac-
tions for Ni, Co, Fe. It is soluble in warm nitric acid, sepa-
rating arsenious acid and sulphur.
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THE CHEMISTS' MANUAL.
Found at Hokansbo and Tunaberg, in Sweden, in splendid
large crystals. Also at Skutterud, in Norway. The most
productive mines are those of Vena, in Sweden, where it
occurs in mica slate ; these mines were first opened in 1809.
This species and smaltite afford the greater part of the smalt
of commerce. Sometimes the black oxide of cobalt, a kind of
bog ore and very impure, is sometimes sufficiently abundant
to be valuable.
10. COPPER.
The principal Copper minerals are :
"Same.
Habd-'
HB88.
NatiYe Copper
a.6
Cnprite
&5-4
Chalcocite....
8.6-8
Bomlte
8
Chalcopyrlte..
8,6-4
TennaDtite . . .
8.5-4
T^tnhedrlte..
8-4.6
CauOcantliite..
15
Brodumtlte...
8.5-4
Atecsmite....
8-8.5
Libethenlte...
4
OleTenite
8
lirooonite ....
»-W
Milacbite
8.6-4
Asnrite
a6-4J6
8p. Qb.
FOBMUUL.
COMFOBinON.
6.85-6.16
4.4-6.6
4.1-4.8
Ca
■eu
•ens
(Ou Fe) B
thi 8 + Fe S + Fe S,
4.87-4.68 4 (t?u,Fe) S + As.S,
4.6-6.11
9.18
On = 100
Cii = 88.8; 0 = 11.8
Cu = 79.8; S = 80.8
j For (JCu + iFe) 8 =
lCu=70.18; Fe='f.78; 8=28.11
Ca = 84.6; Fe = 80.6; 8 = 84.9
j Cu = 47.7: Fe = 9.76;
\ Ah = 18.46; 8 = 80.25
Ca=19.86; Fe=«-7; Zn=l-7;
(8b;Ai)3r^ \ ^§ = ?i:?28; ^8 = 1^:^84
CnS + 6H
8.78-8.87 8Ca, 8 + Cn U + 4H
4-^8
&6^8.8
4.1-^.4
(8.868-
18.965
8.7-4.01
8.6-8.881
Ca a H + 8Ca H
Cu«*t' + H
Cu, (Ab,% + H
Ca = 81.8; 8 = 88.1; H = 86.1
Ca = e8: 8=19.9; H= 11.1
Cu = 68*6; CuCl = 80Ji; H= 16.8
Cu = e6.6; ¥ = 89.7; H = 8.8
Ca = 67.4; *Xb = 86.7;
'P'= 8.7; H= 8.8
Cu = 86.88; 'As = 88.06.
10.85; H =36.01
j Cu = 86.88;
( 'i>'=8.78; Al =
Cu = 71.9; C = 19.9; H = 8JI
Cu = e9.8; C = 86.6; H=5.8
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264 THE CHEMISTS' MANUAL.
NATIVE COPPER.
When perfectly pure, native copper consists of copper,
100 per cent., but it often contains some silver and bismuth.
Hautefeuille states that a Lake Superior specimen gave cop-
per 69.280, silver 5.543, mercury 0.0119, gangue 25.24S;
while r. A. Abel found in a specimen of same, which had a
thick vein of native silver running through it, 0.002 per cent,
of silver, with a trace of lead, and in another 0.56 silver (J. Ch.
Soc, II, i, 89). Abel obtained for a Uralian, from the
Kirghiz District, 0.034 silver,. 0.11 bismuth, a trace of lead,
and 1.28 of arsenic. Color, copper red. Streak, metallic,
shining; ductile and malleable. Fracture is hackly. Lustre
metallic.
Fuses easily ; on cooling becomes covered with a coating of
black oxide. Dissolves readily in acids.
Copper occurs native in beds and veins, and is most abun-
dant in the vicinity of dikes and igneous rocks. Sometimes
found in loose masses in the soil.
Found in fine crystals at Turinsk in the Urals. Brazil,
Chili, Bolivia and Peru afford native copper. Found also in
China and Japan. Found in Massachusetts, Connecticut and
New Jersey. The largest deposits in the world are found,
though, at Kewenaw Point, Lake Superior, where it occurs in
veins that intersect the trap and sandstone. The largest mass
of copper ever found was at the Minnesota mine ; it was 45 feet
in length, 22 feet at the greatest width, and the thickest part
was eight feet. It contained over 90 per cent, of copper, and
weighed about 420 tons. Found also in small quantities in
California and Colorado, and in large drift masses in Bussian
America.
CUPRITE.
The composition of Cuprite, when pure, is copper 88.8;
oxygen 11.2 (Cu). It sometimes affords traces of selenium.
Von Bibra found the tile ore of Algodon Bay, Bolivia, to con-
tain chlorine, and to be a mixture of atacamite, cuprite, hema-
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THE CHEMISTS' MANUAL.
26&
tite, and other earthy materials ; he obtained from one, ata-
comite 31.32, cuprite 10.85, sesquioxide of iron 20.50, gangue
34.42, water, antimony and loss 2.87 (J. pr. Ch., xcvi, 203).
Color is dark blood-red, Bometimee ahnost black. Streak
dark cochineal-red. Subtransparent, subtranslucent. Frac-
ture conchoidal, uneven. Brittle. Lustre adamantine or sub-
metallic to earthy.
In oxidizing flame, it is infusible, and gives a black scoria.
In the reducing flame, it gives a button of metallic copper,
which is malleable and ductile. Soluble in HCl and HNO3.
Unaltered in the closed tube.
Abundant in Chili, Peru and Bolivia. Crystals in this
region simply cubes (D. Forbes). When found in large quan-
tities, this mineral is valuable as an ore of copper. Found at
Sommerville, N, J., Cornwall, Pa., and Lake Superior.
CHALCOCITE.
Composition, when pure, copper 79.8, sulphur 20.2 (CuS).
It generally contains iron, and sometimes silica and silver.
L0CA11TZI8.
1 Siegen
2. Montagone, Tuscany,
a Bristol, Conn ,
19.00
21.90
90.26
Cu.
Fe.
79.50
71.81
79.42
0.75
6.49
0.88
Si.
1.00 = 100.26
— = 90.70
Ag0.11 = 100.12
Analysis No. 1 is by Ullmann (Syst. tab. Uebeis, 248).
" No. 2 (Ramm., 6th SnppL, 151, and Min. Ch., 997).
'* No. 8 (Private contribntion to Dana's Mineralogy).
Hardness = 2.5-3. Sp. Gr. = 5.5-5.8 ; 5.7522 (Thompson).
It crystallizes as a right rhombic prism 119° 35'. Color and
streak dark-blue, almost black. Lustre metallic. Streak some-
times shining. Ductile, easily cut with knife into curved
shavings.
Yields nothing volatile in closed tube. Melts in flame of
candle, giving off sulphurous fumes. Melts to globule of cop-
per on cliarcoal. Soluble in hot nitric acid.
Splendid crystals are found at Cornwall. Found massive
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THE CHEMISTS' MANUAL.
in Siberia, Tuscany, Mexico, Peru, Bolivia and ChiK. Found
massive at Bristol, Conn. ; also in New York, New Jersey,
Yirginia, and other States.
BORNITE.
The formula for Bornite is (Cu,Fe)S, with the proportion
of copper and iron varying. The following are some analyses :
LOOAUTIBS.
8.
Cu.
Pb.
1. St. Poocrace
SS.8
96.80
94.48
98.46
68.9
66.10
68.71
89.17
18.0, gangne 6.0 = 100
17.86, Si = 0.18 .-= 80.88
11.19, Md tnwe, Sl = 8.88 = 98.15
11.78, Ag = 9.68 = 100
"S. Delarne (mMslye)
8. Jenrteland Bwodon. t
4. BamoSf Mexico
Analysis No. 1 by Berthler (Ann. de M., in, vii, 640. 666).
" No. 9 by PUttner (Pogg., xlvii, 851).
" No. 8 by D. Forbes (Ed. N. PhU. J., 1. 978).
" No. 4 by C. Beigemann (Jahrb. Min., 1697, 864).
Hardness = 8. Specific gravity = 4.4-5.5. Specific gravity
of Analysis No. 3, 4.432. Color is reddish-brown, or a black
violet-blue, with a great variation in colors, owing to tarnish.
Streak pale grayish-black, or blackish bronze-yellow, slightly
shining. Lustre metallic. Fracture small conchoidal, uneven.
Brittle.
Gives in a closed tube a faint sublimate of sulphur. In the
oxidizing flame it is roasted with sulphurous odor; in the
reducing flame a half-melted globule, which is attracted by
the magnet. Soluble in nitric acid with separation of sulphur.
It is generally found compact, and owing to its variation of
colors, easily detected. It is a valuable ore of copper. Crys-
talline varieties are found at Cornwall, and mostly near
Redruth. It is the principal copper ore at some Chilian mines,
especially those of Tamayo and Sapos ; ako common in Peru,
Bolivia and Mexico. At the copper mines of Bristol, Conn.,
it is abundant, and often in fine crystals. It occurs also in
Massachusetts, New Jersey, Pennsylvania, and elsewhere.
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THE CHEMISTS* MANUAL.
267
CHALCOPYRITE.
The composition of Chalcopyrite, when pnre, is copper 34.6,
Bulphur 34.9, iron 30.5 (CuS+FeS+FeSa) =2(jCu-|-iFe)S+
FeSg. Some analyses give other proportions; but probably
from mixture of pyrite.
8.
Cu.
Fs.
Qttaxtz.
1. SaTn
35.87
88.88
86.10
84.40
8S.66
83.85
80.47
87.77
99.96
aS7 = 100.01
%. JemtelM, Sweden
Mn trace, Ui aSS - 99.69
SL Phenixrille
Pb 0.85 — 90.S8
Axudysis No. 1 by H. Roee (Gibb, Ixzli, 186).
No. 2 by D. Forbes (Bd. N. Phil. J., I, 378).
*« No. 8 by J. L. Smith (Am. J. Sci., n, zx, 349).
Hardness = 3.5-4. Specific gravity == 4.1-4.3. Color is
brass-yellow, with metallic lustre. It is subject to tarnish,
and is often iridescent. Streak is greenish-black, a little
shining. Opaque. Fracture conchoidal, uneven.
Decrepitates in a closed tube, and gives a sulphur sublimate.
On charcoal, before the blowpipe it melts, gives off sulphurous
acid, and yields a metallic globule. Dissolves in nitric acid,
with separation of sulphur.
Chalcopyrite is a very valuable ore of copper. At the Corn-
wall mines, it is the principal ore of copper, and 10,000 to
12,000 tons of pure copper are smelted annually from 150,000
to 160,000 tons of ore. There are large beds of this ore at
Fahlun, in Sweden ; it occurs also at Rammelsburg, in the
Harz. Found in fine crystals at Cerro Blanco, in Chili. It
is found in Maine, New Hampshire, Yermont, Massachusetts,
Connecticut, New York, Pennsylvania, Yirginia, North Caro-
lina, Tennessee, and California. The ore is extensively mined
at Bruce mine on Lake Huron.
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THE CHEMISTS' MANUAL.
TETRAHEDRITE.
The composition of Tetrahedrite is copper 19-25, iron 2-7,
zinc, 1-7, silver 0-31, arsenic 0-11, antimony 11-28, sulphur
19-26 [4(€u, Fe, Zn, Hg, Ag)S{SbAs)2S3].
LocALrms.
1. Bainmelsbei^(ma8eiTe) 96.8S 2a78
2. Arkaneas 96.71:26.50
8. Freiberg 81.17,84.68
4. PoraUch, Hungary ; 88.0C , 81.66
6. " " j 24.87 26.48
6. Kotterbach 28.68 19.84
7. MoBcheUandsberg , 81.90 28.45
Afl.
CIT.
__
87.96
1.08
86.40
—
14.81
—
89.04
trace 30.68 |
2.94
36.84
0.81
82.19
2.24
2.63
6.96
0.99
7.88
—
1.46
-
0.87
0.09
1.41
0.10
1
0.m = 97.98
2.80 = 99.02
81.29 = 96.87
0.12, Hg 0.62 = 100.62
0.09, Hg 16.69 = 98.67
5— Hg 17.27, Pb 0.81,
i Bi 0.81 = 100
( 0.10, Hg 17.38, Co 0.2&
( Bi 1.67, gangno 1.89
( =99.87
Analysis No. 1 by (B. H. Ztg., 1868, No. 2) ; Ajialysle No. 8 by J. L. Smith (Ann. J. Sd.,.
n, zliii, 67) ; Analysis No. 3 by H. Rose (Pogg., xv, 676) ; Analyses No. 4 and No. 6 are by
Haaer (Jahrb. g. Beichs, 1863, 96 ; J. pr. Ch., Ix, 65) ; Analysis No. 6 by G. v. Bath (Pogg.»
xcYi, 822) ; Analysis No. 7 by Oellacher (Jahrb. Min., 186^ 694).
Hardness = 3-4.5. Specific gravity = 4.5-5.11. Color is
a blackish-gray, which is more or less dark. Streak gener-
ally same as color ; sometimes inclined to brown and cherry-
red. Opaque. Lustre metallic. Rather brittle.
In the oxidizing flame, on charcoal, it is roasted, giving a
slight odor of arsenic and fumes of antimony, and in the
reducing flame, gives a brittle globule of copper. Decom-
posed by nitric acid, with separation of antimonious and arse-
nious acids.
It is found in masses with or without gangue. Tlie Cornish
mines, near St. Aust., have afforded large tetrahedral crystals
with rough and duU surfaces. More brilliant crystals occur
in Cornwall. The ore containing mercury occurs in Schmol-
nitz, Hungary. Tetrahedrite is found in Mexico, Chili, Ar-
kansas, California, and Arizona.
MALACHITE.
Composition of Malachite, when pure, is protoxide of copper
71.9; carbonic acid 19.9; water 8.2 (CugC + H =CuC-K:uH).
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THE CHEMISTS' MANUAL.
LOCAUTIBS.
C.
Cu.
H.
1. Tnijiusk, Ural
a. Chemy
lao
S1.85
m5
70.10
71.46
11.5=100
8.75 — 100 10
8- Fbenlxvitle
19.09
9.02. Fe 0.1S — 99.60
AaaljBiB No. 1 by Kaproth (Beltr., ii, 987, 1797).
^^ No. S by Vaaqnelin (Ann. da Mas., xz, 1).
** Na a by J. L. Smith (Am. J. ScL, n, zx, 949).
Hardness = 8.5-4. Specific gravity = 3.7-4.01. Color is
green, and may be of different degrees of intensity. Streak
paler than color. Translucent, opaque. Lustre of crystals.
Adamantine, inclining to vitreous ; of fibrous varieties more
or less silky ; often dull and earthy. Fracture subconchoidal,
uneven. It crystallizes an inclined rhombic prism of 104° 28'.
In a closed tube blackens and gives off water. It melts at 2,
coloring the flame green, and gives a scoriaceous mass. On
charcoal with the reducing flame gives a globule of metallic
-copper. Soluble in acids with effervescence.
Green malachite accompanies other ores of copper.* It is
usually found in concretionary masses, which have a fibrous
fracture, rarely conchoidal. Their lustre is silky and velvety.
Occurs abundantly in the Urals ; at Chessy, in France ; in
the old mine at Sandlodge, in Shetland ; in the Tyrol ; in
Cornwall and Cumberland, England ; also in handsome masses
at Bembe, on west coast of Africa ; also in Cuba, Chili, and
Australia. It is found in the United States at Cheshire, Conn.
In New Jersey, Pennsylvania, Maiyland, Wisconsin and Cal-
ifornia, Malachite is a valuable ore of copper, when found in
large quantities. It admits of a high polish, and when in
large masses is cut into tables, vases, etc. It is often employed
for veneering large articles, such as tables, doors, etc. A mass
weighing forty tons was found in Siberia.
AZURITE.
Composition of Azurite, when pure, is oxide of copper 69.2,
carbonic acid 25.6, water 5.2 (2CuC+CuH). Hardness =
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THE CHEMISTS' MANUAL.
3.5^.25. Specific gravity = 3.5-3.83. Color is azure-blue^
which is more or less dark. Streak is lighter than color.
Lustre vitreoug, abnoBt adamantine. Transparent, subtrans-
lucent. Fracture conchoidal. Brittle. It crystallizes as an
inclined rhombic prism of 99° 32'.
In closed tube blackens and gives off water. In the reducing
flame, on charcoal, a globule of metallic copper is produced.
Soluble in acids when heated, with effervescence.
It is sometimes found in concretionary masses in mamelons,
which are sometimes so close together as to become joined.
Found in splendid crystallizations at Chessy, near Lyons,
whence it derived the name Chessy copper. It is found in
Siberia ; in Cornwall, Devonshire, and Derbyshire in England.
Found in Pennsylvania, New York, New Jersey, Wisconsm^
and California.
When found in laige quantities, it becomes a valuable ore
of copper. When groimd to an impalpable powder, it forms a
bright paint with a blue tint ; but it is not used much as a.
pigment, as it is liable to turn green.
n. GOLD.
The principal Gold minerals are :
Naw.
Hard-
KBBS.
Sp. Gb.
FOBinTLA.
Coxposinov.
Native Gold
2.^
1.6-2
1-1.6
16.6-19.6
i 8.732; ]
1 aas (Pete). }
6.86-7.2
aiS-^-SS (Petz)
9-9.4 (KUstel)
16.6-16.8
Pure, An.
(An, Ag),Hg,
(Ag, Au) Te.
((Te, 8, Pb,»
1 An, Ag, Cu) f
AuTe + 44 AgTe
(Petz).
AnTe + 8AgTe
(QenthT
AnTe.
AnPd(Ag)
An Bd (Ag)
Pure, 100.
Oold Amalgam
Sylvanite
Tffanrvft.g^tA
(Gold 88.39: Merenrv
1 67.40; Silver, 6.0.
( An 88.&Te 66.8; Ag 16.7
! when7Ag:An=1:lV
Te8S.2; 8 8.0; Pb64.0:
' An 9.0; AgO.6; Cnl.8.
( Te 84.96: Ac: 46.76:
1 An 18.26; Fe,Pb,S, 7)r.
Petzlte
Cftlftverite t - r , , , t - - f - -
Te 66.63; An 44.47.
Palladium (Porpezite).
RliodlumQold
An8S.96;Pd9.86;Ag417.
An8a89; Ag6;Bd84-4i|t
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271
NATIVE GOLD.
The composition of native gold, when pure, is gold, but it
sometimes contains traces of copper, iron, palladium, and
rhodium.
Sp.Gb.
Au.
As.
F&
Cu.
1. Wicklow Conn^, Ireland..
«. BorMohka (N. TagUsk)....
& BoliYia, Tipnani
16.884
laae
16.07
14.16
98.88
94.41
91.96
6196
96.48
99.98
90.80
6.17
6.88
7.47
86.07
8.60
0.44
8.08
0.78
ao4
Trace.
OJM)
- =99.87
0.89 = 100
— gangne 0.97 = 100
- =100
— qaarts 0.10 = 09.17
0.07, Bl 0.01 - 100
4. New Grenada, Santa Rosa.
6- Anstralla.
A. "
7. Tfinnaniii^ Fingal . .
7y.,Sn,Pb, Co 1.0=99.91
Hardness :? 2.5-3. Specific gravity = 15.6-19.5 ; 19.30-
19.34 when quite pure (G. Hose). Color and streak different
shades of gold-yellow, sometimes inclining to silver-white.
Lustre metallic. Very ductile and malleable. Fuses easily^
but gives no reaction with fluxes. Not soluble in auy acid
except aqua-regia.
Gold is widely distributed over the globe, and occurs in.
rocks of various ages, from the Eozoic to the cretaceous or
tertiary. In Europe it is most abundant in Hungary at
Konigsberg, Schemnitz and Felsobanya, and in Transylvania.
Occurs in the sands of the Ehine, the Beuss, the Aar, the
Ehone, and the Danube. On the Alps, in Spain, in many
streams of Cornwall, in Scotland, Ireland and Sweden.
The large fragments found in sand are called nuggets, which
are of considerable size.
The following table gives the weight of the principal ones :
Nams.
Wkisbt.
Wekome Nugget 1 184 lbs. 8oz.
Ballarat, AoBtralla (valae,
•41,888). I
Blanch BarkieyKngget , 146 lbs.
Kia8k,UralB | 96 "
" , 87 "
Naiob.
Mlask, Urals
Paraguay
Cabarras County, N. 0.
Califomia.
Wkight.
27 lbs.
16 "
60 »'
87 "
27 **
17 **
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THE CHEMISTS' MANUAL.
The whole amount of gold in the auriferous sands of the
Bhine has been estimated at $30,000,000, but it is mostly cov-
-ered by soil under cultivation. In the Urals, they are prin-
cipally alluvia washings, and these washings seldom yield less
than 65 grains of gold for 4000 pounds of soil, and rarely
more than 120. The mines in the Ural became, after 1819,
the most productive in the world, until the discovery of the
California mines.
Gold is found in China, Japan, Africa, and South America.
It is found in the Eocky Mountains, Mexico, Sierra Nevada,
and California. In the Eastern States, it is found principally
in Virginia, North and South Carolina, and Georgia.
12. IRIDIUM.
The principal ore of Iridium is Iridosmine.
IRIDOSMINE.
Composition of Iridosmine is iridium and osmium in dif-
ferent proportions. Some rhodium, platinum, rutherium and
other metals are usually present.
LooAums.
IB.
Bd.
Pr.
Ru.
Os.
Cu.
Fs.
1. New Grenada
70.40
48.S6
13.80
6.78
0.10
0.08
&40
17J»
40.11
a78
— - 100
9. BaB8ia(Sp.Or.l8.9)...
0.90 = 100
Hardness = 6-7. Specific gravity = 19.3-21.12.
Color tin-white or steel-gray. Lustre metallic. Opaque.
Malleable with difficulty.
At a very high temperature gives off fumes of osmium.
With nitre gives the reaction for osmium.
It is found with platinum in the province of Choco, in
South America ; in the Ural Mountains ; in Australia. It is
rather abundant in the auriferous beach-sands of Northern
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THE CHEMISTS' MANUAL.
273
California. Also traces iu the gold washings on the Bivi^res
da Loap and des Plantes, Canada.
Iridium is used for the points of gold pens.
13. IRON.
The principal Iron minerals are :
Vamb,
Hard-
HB98.
8p. Qb.
FOBMUIA.
CoMPosinoH.
Native Iron
MeteoTitcB (
4.5
7.8-7.8
(When pnre) Fe.
Fe + Co + Ni
FelOO.
Ni from 1—20 per cent
Magnetite
6J5-6.6
4.9-&8
Fe,*e
Fe72.4; 0 27.6.
Frankllnlte
5.5-6.6
6.060
(Fe,Mn,Zn)(Pe,Mn)
Fe66;Mnl6; Znl7.
Hematite
5.5-65
4.6-5.3
^e
Fe70; 0 da
Golthite
5-^.5
5— fi.6
. 4—4.4
3.6—4
FeH
Fe.H.
Fe,8.
Fe 8.99 ; U 10.1.
Limonite ..... . .
F0,O.86.6; H 144
Fe60.5; 8 89.5.
Pjrrhotite
8.5— *.5
4.4-4.68
Pjrrite
6-6.5
4.83-5.2
FeS,
Fe46.7; S58.3.
Harcaeite
6-«.5
4.678—4.847
FeS,
Fe46.7; S 53.8.
Melanterite
3
1.883
FeS + 7H
Fe25.9; S38.8; H45A
Coplapite
1.5
2.14
Fe,S. + 18H
Ve$ + 8H
FeAs.
Fe.O, 842; 842.7; 1128.1.
FeO 48: 'P28.8; H 28.7.
Ylvianite
1.5—2
2.58—2.68
Lcncopyrite
5-6.5
6.8-8.71
Fe27.2; As 72.8.
Araenopyrlte
5.5-6
6-6.4
Fe (A», S).
Fe84.4; Ae48; 819.6.
Scorodite
3.6-4
3.1-3.3
Fe Ae + 4 H
Fe.O, 34.7; As 49.8: H 16.6.
Pharmacoslderite .
-
-
2»PeAB+'FeH.-i-12H
1-2
3.62-8.88
Ca»A9+4Fe3'AB -t- 15H
j Fe.O. 42.1; "As 87,9;
1 Ca 11.1 ;H 8.9.
Siderite
8.5—4.5
8 7—8 9
FeC
FeO 62.1; C87.9.
ife 1.2-83.47 ;Fe 1.5-60.17.
Menaccanlte
5.6
4.5-6
(Ti, Fo, Mn, Mg),0,
Chromlte
5.6
4821—4.496
(Fe,Cr,Mg) (Al,Fe,«r)
ForFeS-,Fe8a;'Cr68.
Colambite
6
6.4-6.5
(Fe, Mn) (Ca, *ta)
j For FeCb,
1 Fe 21.17 ;Cb 78.88.
WoUtamite
5-6.6
7.1-7 J56
j 2FeW + 8MnW,or
{ 4FeW + iCnW
Fe9.66; W 75.38; Mn 15.12
Fe5.6; W76.2; Mn 17.94
18
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2T4 THE CHEMISTS' MANUAL.
NATIVE IRON.
Native iron contains various quantities of other substances
than iron, principaUy nickel, associated with small proportions of
cobalt. The quantity of nickel may vary from 1 to 20;^. Pure
metallic iron has been reported to be found in certain pyrites
mines. Proust analyzed several specimens and pronounced
them to be pure. The metal in a pure state has also been
found in a mine in Dauphin^, Auvergne, and Brazil, but such
iron is very rare. It is found native as grains, disseminated
through volcanic rocks, at the Giant's Causeway and in Au-
vergne. It is easy to prove its presence by dipping the rocks
into a solution of cupric sulphate, when the rock becomes
coated with copper.
Iron is usually found native, however, as meteorites. Me-
teorites may be of two kinds :
First. Entirely composed of metallic iron, associated with
chromium, nickel, and sometimes with cobalt, manganese, and '
sulphur, and sometimes contain bituminous substances. In ,
the last case the masses are spongy, the cavities being filled
with chrysolite, or a substance analogous to it.
When a meteorite is polished and treated with acid, they
show the traces of crystallization. The following are some of
the principal meteorites :
I
The Gibbe Meteorite, in Yale College, weighs 1,635 lbs. |
The TuckBon Meteorite, in Smithsonian Institate, weighs 1,400 lbs. |
(1.) South America Meteorite weighs 82,000 lbs.
(2.) " " " " 14,000 lbs.
The Pallas Meteorite contains crystals of chrysolite, found in ffiberia;
weighs 1,600 lbs.
Second. Other meteorites, on the other hand, are of a stony
character, and contain the iron scattered through them in
bunches. The exterior of these meteorites is generally scori-
fied and covered over with a coating.
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276
MAGNETITE.
The compofiition of Magnetite, when pure, is iron 72.4,
oxygen 27.6 (Fe Fb) ; or ferric oxide (FejOa) 68.97, ferroua
oxide (FeO) 31.03, The iron ifi sometimes replaced in part
by titanium, magnesium, lime, silicic oxide, alumina, nickel,
copper, and manganese.
Fit.
5189
ti.
Mh.
Ctj.
Nl
ico.
Ca.
Sl
Al.
ffB,
1 Meicbes
21.75
24.95
1.75
_
_
_
i. Ytterby
6a54
8ai8
2.08
—
—
—
—
—
—
—
—
S. Ochreone.
fi6J20
18.87
—
17.00
O.0G
-
—
—
—
—
Sand.
4. LandAQ
69.27 ; 29.48
—
—
—
—
0.49
0.06
0.28
0.08 I -
i "
£6 90 11.97
—
—
—
—
0.17
0.38
0.18
0.22 1 —
f. NickeliferouB..
68.92
29.82 Tr.
Tr.
—
1.78
—
—
—
- 1 Tr.
Analyais No. 1 by A. Knop (Ann. Cbem. Fbarm., cxxlii, 848).
** No. 2 by J. A. Mlchaelron (J. p. Ob., xc, 107).
** No. 8 by P. A- Oentb (Ann. Cbem. Pbnrm., Ixvl, 277).
^ No0. 4 and 5, by Schwulbe (Zs. uat Ver. Halle, zx, 198).
" Na 6 by Feteraen (Jahrb. Min., 18OT, 886).
Hardness = 5.5-6.6. Specific gravity = 4.9-5.2 ; 5.168-
5.180, crystals (Kenngott), and 5.27 after long heating. Color
is black and streak is black. On its natural faces it has a semi-
metallic lustre. Generally opaque, but in very thin dendrites
is sometimes transparent. Fracture subconchoidal, shining.
Brittle. Strongly magnetic, sometimes possessing polarity.
It is fusible with difficulty. In oxidizing flame loses its
influence on the magnet. It is insoluble in nitric acid, but is
dissolved in hot hydrochloric acid.
Magnetite is mostly confined to crystalline rocks, and is
most abundant in metamorphic rocks, though found also in
grains in eruptive rocks. It sometimes happens that the
grains are covered with a superficial coating of oxide on the
surface, which makes them iridescent. Such ore is called
9horUor6 by the miner. The granular varieties, by the action
of the elements, often becomes a fine black sand. Such sand
is the only ore of iron in New Zealand, and it is found on
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276
THE CHEMISTS' MANUAL.
the sea-shore, where the constant action of the water has
washed out the impurities and made it quite pure.
The beds of ore at Arendal, and nearly all the celebrated
iron mines of Sweden, consist of massive magnetite ; Danne-
mora and Taberg, in Smaoland, are entirely formed of it.
Still larger mountains of it exist at Kurunavara and Gelwara,
in Lapland. Octahedral crystals are found at Fahlun, in
Sweden ; dodecahedral crystals occur at Normark, in Wermland.
The most powerful native magnets are found in Siberia and
in the Harz ; they are also obtained on the island of Elba.
In iNorth America, it constitutes vast beds. It occurs in
New York in several counties ; in Maine, in an epidotic rock ;
at Marshall's Island, masses are strongly magnetic. Also in
Vermont, Connecticut, New Jersey, Pennsylvania, Maryland,
and in California, Sierra Co., abundant, massive, and in crystals.
" No ore of iron is more generally diffused than the mag-
netic, and none superior for the manufacture of iron. It is
easily distinguished by its being attracted readily by the mag-
net, and also by means of the black color of its streak or
powder, which is some shade of red or brown in hematite and
limonite. The ore, when pulverized, may be separated from
earthy impurities by means of a magnet, and machines for this
purpose are in use."
FRANKLIN ITE.
Composition, when pure, is ferric oxide 66, manganic oxide
16, zincic oxide 17 (Fe, Mn, Zn)(fe, Mn).
The following are a few analyses :
Localities.
3PB.
to.
Zn.
Si.
'Jk
1. New Jersey
66.88
64.51
66.18
18.17
18.51
11.99
10.81
S5.80
81.77
0.40
0.38
a78 - 98.99
8. ** *^
— - 108.53
a " "
— — 100
Analysis No. 1 hj Abich (Pogg., zxiii, 848).
" No. 3 by RammelsbcrQ (Pog^., cvii, 818).
'' No. 8 by Steffens (B. U. Ztg. , xix, 468).
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THE CHEMISTS' MANUAL. 277
Hardness = 5.5-6.5. Specific gravity = 5.069 (Thompson),
5.091 (Haidinger). Color is black. Streak dark reddish-
brown. Very slightly magnetic. Lustre metaUic. Opaque.
Fracture conchoidal. Brittle.
Infusible. With borax in oxidizing flame gives a reddish-
amethystine bead (manganese), and in reducing flame changes
to bottle-green (iron). On charcoal with borax gives the
reactions for zinc and iron. Soluble in hydrochloric acid with
slight evolution of chlorine.
It is found in cubic crystals near Elibach, in Nassau; in
amorphous masses at Altenberg, near Aix-la-Chapelle.
It is only foimd in large quantities at Hamburg, New Jersey,
near the Franklin Furnace ; it is there found witli red oxide of
zinc and garnet, in granular limestone ; also at Sterling Hill,
in the same region, where it is associated with willemite in a
large vein, in which cavities occasionally contain crystals from
one to four inches in diameter.
Franklinite is used as an ore of iron and zinc.
HEMATITE.
Composition, when pure, is iron 70, and oxygen 30 (-Fe).
Some hematite contains titanium. Crystals \(rom Krageroe
afforded Eammelsberg (Pogg., civ, 528).
fe 93.63 - ti 3.55, Fe 3.26 = 100.44 = Fetl + 13fe or .
(FeTi)203 + 13fe.
The varieties depend on texture or state of aggregation, and
in some cases the presence of impurities.
Vae. 1. Specular. Lustre metallic, and crystals often splen-
dent.
(J.) When the structure is foliated or micaceous, the ore is
called micaceous hematite.
Var. 2. Compact, columnar, or fibrous. The masses often
long, radiating; lustre submetallic to metallic; color brown-
ish-red to iron-black. Sometimes called red-hematite.
Var. 3. Hed Ochreous, Eed and earthy. Reddle and red
chalk are red ochre, mixed with more or less clay.
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278 THE CHEMISTS' MANUAL.
Vab. 4. Clay Irori-stone ; Argillaceous Hematite, Hard
brownish-black to reddish-brown, heavy stone ; often in part
deep red ; of submetallic to unmetallic lustre ; and ajBbrding,
like all the preceding, a red streak.
{J}) When reddish in color and jasper-like in texture, often
cBlledjai<pe7^i/-clai/ iron-stone.
(c.) When oolitic in structure (consisting of minute flattened
concretions), it is called lenticular iron^ore.
Hardness = 5.5-6.5. Specific gravity = 4.5-5.3, of some
compact varieties as low as 4.2. Color dark, steel-gray or iron-
black ; in very thin particles, blood-red by transmitted light ;
when earthy, red. Streak blood-red or brownish-red. In thin
scales, it is transparent and of a blood-red color. Sometimes
slightly magnetic, and occasionally even magnetipolar.
It is infusible, but when exposed for a long time to the
reducing flame, it gives a magnetic globule. Dissolves with
difficulty in hydrochloric acid, more especially if it contains
titanium. This ore is found in rocks of all ages. The specu-
lar variety is mostly confined to crystalline or metamorphic
rocks, but is also a result of igneous action about some volca-
noes, as at Vesuvius.
The beds that occur in metamorphic rocks are sometimes of
very great thickness. In North America it is widely dis-
tributed ; occurs in beds in vast thickness in rock of the Eozoic
age, as in the Marquette region in northern Michigan, and in
Missouri at the Pilot Knob and the Iron Mountain; the
former, 650 feet high, consisting mainly of an Eozoic quartz
rock, and having specular iron in the upper part, the iron ore
in heavy beds interlaminated with quartz ; the latter 200 feet
high, and consisting at surface of massive hematite in loose
blocks, many ten to twenty tons in weight ; in Arizona and
New Mexico. Besides these regions of enormous beds, there
are numerous others of workable value, either crystallized or
argillaceous, in New York, Massachusetts, New Hampshire,
North Carolina and South Carolina ; a micaceous variety is schis-
tose rocks, containing the so-called specular schist or itabirite.
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279
" This ore aflTords a considerable portion of the iron manu-
factured in different countries. The varieties, especially the
specular, require a greater d^ree of heat to smelt than other
ores, but the iron obtained is of good quality. Pulverized red
hematite is employed in polishing metals, and also as a color-
ing material. The species is readily distinguished from mag-
netite by its red streak, and from turgite by its greater hard-
ness and its not decrepitating before the blowpipe."
LIMONITE.
Composition, when pure: ferric oxide 85.6, water 14.4
(fe2H2)* III t^® ^S ^^s ^^d ochres, sand, clay, phosphates,
oxides of manganese, and humic or other acids of organic
origin, are very common impurities.
The following are a few analyses of Limonite :
LooALinss. *
88.87
ttN.
H.
Si.
4.B0
?:
'^
Co.
1. HorhanseD
__
18.86
__
_„
Sl Salitfbary, Conn...
81.18
0.60
1881
868
Tr.
0.93
Tr.
8. Diet of Kandern i
(plsolllic) f
71.71
-
888
laoo
-
6.71
-
4 Dist. of Kandern }
(plaolitlc) f
68.70
-
11.63
1180
-
7.47
-
& Boffiilo, Mo.
84.80
—
11.09
8.88
—
0.64
—
Ca.
— =100.08
7V./8*71r. = 100.16
0.60 = 100.35
— = 99.60
— S 013 = 100.06
AnalyslB No. 1 by SchOnberg (J. pr. Ch., xix, 107).
•* Na 8 by C. S. Rodman.
^* Noe. 8 and 4 by Schenck (Ann. Cb. Fharm., xc, 138}.
'' No. 5 by Litton (Rep. G. Mo., 1866).
Hardness = 5-5.5. Specific gravity = 3.6-4. Color gen-
erally different shades of brown, sometimes nearly black in
the botryoidal varieties ; when earthy, brownish-yellow, ochre-
yellow. Streak yellowish-brown. Lustre silky, often sub-
metallic, sometimes dull and earthy.
The varieties are
1. Compact. Submetallic to silky in lustre.
2. Ochreous or earthy, brownish-yellow to ochre-yellow;
often impure from the presence of clay, sand, etc.
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280 THE CHEMISTS' MANUAL.
3. Bog Ore. The ore from marshy places, generally loose
or porous in texture, often petrifying leaves, wood, nuts, etc.
4. Brown Clay Iron-stone^ in compact masses, often in
concretionary nodules, having a brownish-yellow streak, and
thus distinguished from the clay iron-stone of the species
hematite and siderite ; it is sometimes («) pisoliticy or an
aggregation of concretions of the size of small peas (Bohnerz,
Germany) ; or {h) oolitic.
Gives oft* water and becomes red when heated. Soluble
in acids.
Limonite is in all cases the result of alteration of other ores,
through exposure to moisture, air, and carbonic or organic
acids ; and is derived largely from the change of pyrite, sid-
erite, magnetite and various other species. It is therefore
found in secondary or more recent deposits.
Extensive beds exist at Salisbury and Kent, Conn. ; also in
Beekraan, Fishkill, Dover, and Amenia, N. Y. ; also at Lenox,
Mass. ; in Vermont at Bennington, Monkton, Pittsford, Put-
ney and Kipton.
" Limonite is one of the most important ores of iron. The
pig iron from the purer varieties, obtained by smelting with
charcoal, is of superior quality. That yielded by bog ore is
what is termed cold-shorty owing to the phosphoiiis present,
and cannot therefore be employed in the manufacture of wire,
or even of sheet iron, but is valuable for casting. The hard or
compact nodular varieties are employed in polishing metallic
buttons, etc."
PYRITE.
The composition of Pyrite, when pure, is iron 46.7 ; sul-
phur 53.3 (FeSj). There are several varieties of pyrite.
Var. 1. Ordinartj. («) Indistinct crystals; {h) nodular,
or concretionary, often radiating within ; {c) stalactitic ; {d)
amorphous.
Var. 2. Nickellferous, Schnabel found 0.168 of nickel
in a kind from a silver mine near Eckerhagen. A pyrite from
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281
the Kearney ore-bed, Gouvemeur, N. Y., is Bimilar ; it is a
pale bronze in color, and radiated botryoidal. Hardness = 5.5.
Specific gravity = 4.863. (Am. J. Sei., II, xv, 444.)
Vab. 3. CobaUiferous, Specimens from Cornwall, Leba-
non County, Pa., afforded J. M. Blake 2 per cent, of cobalt.
Vak. 4. Cupriferous. A variety from Cornwall, Lebanon
County, Pa., gave J. C. Booth 2.39 per cent, of copper, afford-
ing the formula, (Fe, Cu) Sg. (Dana's Min., 1854, 55.)
Var. 5. Stanniferous ; BaUesierositey Schulz and Pail-
lette (Bull. G. Fr., II, vii, 16.) A kind in cubes, containing
tin and zinc, occurring in argillite, from Galicia.
Vae. 6. Auriferous. Containing native gold. Thepyrite
of most gold regions is auriferous.
Var. 7. Argentiferous from Hungary.
Var. 8. ThaUiferous. The pyrite of the Rammelsberg
mine, near Goslar, Pmssia, is especially rich in thallium.
The following are a few analyses :
8. Fe.
49.32 , 45.73
53.37 44.47
46.5 39.3
52.7 44.a
1.09
Co.
1.24
Cu.
118
2.89
Sl
10.0
2.5
Iai..
H.
1. Inveraiy
8.8
— insolnble 0.06
8l Cornwall
8. Chestfyand St. Bel ...
4. AUier
0.2
0.3
Analysis No. 1 by D. Forbes (Phil. Map., IV, xxxv, 178).
*• No. 2 by Booth (Dana's Min.. 1854, 55).
Nos. 8 and 4 by C. Mdne (C. K. , Ixi v, 870).
Hardness = 6-6.5. Specific gravity = 4.83-5.2 ; 5.185, pol-
ished crystals, Zepharovich. Color on its natural faces and on
its fracture is brass yellow, with a very decided metallic lustre,
and is quite uniform. This color caused it to be much sought
after at one time as an object of ornament. It was then
known to jewelers as marcasite. Streak is greenish or brown-
ish black. Opaque. Fracture conchoidal, uneven. Brittle.
It strikes fire with steel without giving out any odor. It can
be ftised in the flame of a candle. Heated in a tube, sulphur
sublimes. In the reducing flame a residue is obtained which
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THE CHEMISTS* MANUAL.
attracts the magnet. It is insoluble in hydrochloric acid, but
dissolves in nitric acid with evolution of HgS. Pyrite occurs
abundantly in rocks of all ages, from the oldest crystalline to
the most recent alluvial deposits. It usually occurs in small
cubes, more or less modified; also in irregular spheroidal
nodules and in veins, in clay, slate, argillaceous sandstones, the
coal formation, etc. Very large cubes are found in the Cornish
mines. Large octahedral crystals are found at Persberg, in
Sweden. Magnificent crystals come from Peru. Found as
crystal in Maine at Conia, Peru, etc., and massive at Bing-
ham, Brooksville. Found also in Xew Hampshire, at Unity,
massive. It is also found in Massachusetts, Vermont, New
York, Pennsylvania, Wisconsin, Illinois, North Carolina, Vir-
ginia, and Canada.
SIDERITE.
The composition of Siderite, when pure, is ferrous oxide 62,1
and carbonic oxide 37.9 (FeC). Part of the iron oxide is often
replaced by manganese, and often by magnesia and lime. The
principal varieties are :
(1) Ordinary. (a) Crystallized, (b) Concretionary =
Spherosiderite ; in globular concretions, either solid or con-
centric, scaly, with usually a fibrous structure, {c) Granular
to cojnpact massive, (d) Oolitic, like oolite limestone in
structure, {e) Earthy, or stony, impure from a mixture with
clay or sand, constituting a large part of the clay iron-stone of
the coal formation and other stratified deposits.
(2) In this variety the bases replace part of the iron.
The following are a few analyses :
Localities.
C.
36.90
88.41
40.31
88.16
Pb.
64.57
53.06
43.86
60.00
FeC.
79.87
Mn.
M«.
Ca.
H.
Fb.
1. Durham
1.15
4.20
2.57
MnC.
0.16
— > OKQ
2.68
8. Bieber (white)
8. Salzburg
8.36
10.46
MqC.
10.88
1.12
0.40
1.84
CaC.
* 11.91
— gangae0.4S
407
4. L.Laach
6. Erzberg, Stjria....
-
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THE CHEMISTS' MANUAL. 283
Aniklysls No. 1 by Thompsoo (Mfn., i, 445).
»' No. 2 by Qlasson (Ann. Ch. Pharm., 1x11, 89).
'' No. 3 by Sommer (Jahrb. Mln., 1866, 455).
**^ No. 4 by Blochof (Sammelvbarg, Min. Chemie, SSS).
** No. G by Sander (Kamm. Min. Cfa., 217).
Hardnees = 8.5-4.5. Specific gravity = 3.7-3.9. Color is
ivliite when just taken from the mine and when quite pure,
but it soon becomes altered in the air, and takes a grayish
color, which sometimes becomes brown, brownish-red, or green.
Streak is white. Translucent to subtranslucent. Lustre vit-
reous, more or less pearly. Fracture uneven. Brittle,
On charcoal it blackens and fuses at 4.5. Heated in a closed
tube gives off* carbonous and carbonic oxide, blackens, and
gives a magnetic globule. In the oxidizing fame the iron
becomes ferric oxide, in the reducing flame it becomes mag-
netic. Dissolves in acid in the cold slowly with effervescence,
but rapidly and with brisk effervescence with hot acid.
Siderite occurs in many of the rock strata, in gneiss, mica
slate, clay slate, and as a clay iron-stone in connection with the
coal formation and many other stratified deposits. It is often
associated with metallic ores. Siderite is one of the most
important ores of iron.
In Styria and Carinthia this ore forms extensive tracts in
^eiss. Clay iron-stone occurs in beds near Glasgow. It is
found in veins at New Milford, Conn., Plymouth, New Hamp-
shire, and Sterling, Mass.; also in New York, Oliio and
Pennsylvania.
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THE CHEMISTS' BfANUAL.
14. LEAD.
The principal Lead minerals are :
Mnmuu
Habd-
KIS8.
Bp. Gb.
Native ]ead
IJi
11.446
MIninm
2.8
4.6
GalcDite
8.6-2.75
7.25-7.77
Boarnonltc
2.5-8
5.7-6.91
Anglenlte
2.75-8
6.12-6.89
Clauethallte....
2.5-8
7.6-8.8
Pyromorphite. .
3.5-4.5
6.5-7.1
Minretite
3.5
7-7.25
Ceniseiite
8-8.5
6.465-^.48
Crocolte
2.5-8
5.9-6.1
Stolzite
2.73-^
2.75-8
7.87-8.13
6.05—7.01
Wnlfenite
FOBMULA.
Pb.
i»b + 2Pb.
FbS
8(Ca^)8-t-Sb.8.
FbS
PbSe.
8PbJ'+Pba
8Pb,*A8 + FbCL
PbC.
Pbc'r.
PbW.
PbMo.
Ck>xpo8inox.
Pb = 100.
Pb = 90.66 ; O = 984.
Pb = 86.6; 8 = 18.4.
( Pb=42.4; Sb>25; Ca=lS.9;
1 S = 19.7.
Pb = 78.6; 8 = 26.4
Pb = 72.4 ; Be = 27.6w
j Pb=74.1; P= 15.7;
1 CI = 2.6; Pb = 7.6.
Pbie = 90.60 ; PbCl = 9.84.
Pb = 88.5 ; C = 16.5.
Pb = Ga9 ; Cr = 81.1.
Pb = 49 ; W = 51.
Pb = 61.6; Mo = 835l
GALEN ITE.
The composition of Galenite, when pure, is lead 86.6;
sulphur 13.4 (PbS). It sometimes contains selenium, zinc,
cadmium, antimony, copper as sulphides, besides, also, some-
times native silver and gold, and even platinum.
The following are a few analyses :
LOCALITIEB.
8.
Pb.
SB.
Pb.
Cu.
Zh.
Ao.
1. Bottino
2. Argeutina —
12.SI0
15.63
80.700
72.90
8.807
5.77
1.877
1.77
0.440
1.11
0.024
1.88
0.825
0.72
Analyses No. 1 and 2 are by E. Bechl (Am. J. Sci., U, xiv, 60).
Hardness = 2.5-2.75. Specific gravity = 7.25-7.7. Color
is grayish-blue. Streak lead-gray. In its fresh fracture it has
a metallic lustre, which is quite bright, but becomes dull on
exposure. Fracture flat, subconchoidal, or even. Frangibla
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285
In an open tube it gives off eulphurous oxide. On charcoal,
decrepitates^ and then in oxidizing flame is roasted, giving off
snlphnrous odor and lead fumes, which coat the coal at a short
distance from the assay with a yellow ring. After being
roasted, gives a globule of metallic lead, which is malleable.
It is soluble in nitric acid, with evolution of HgS.
Occurs in beds and veins, both in crystalline and uncrystal-
line rocks. At Freiberg, it occurs in veins in gneiss; in
Spain, in granite.
Extensive deposits of this ore exist in Missouri, Illinois,
Iowa, and Wisconsin. The productive lead region is bounded
on the west, north, and east by the Mississippi, Wisconsin, and
Kock rivers. Occurs also in New York, Maine, New Hamp-
shire, Massachusetts, Virginia, Tennessee, etc.
Galenite is the only important ore of lead.
CERUSSITE.
The composition of Cerussite, when pure, is oxide of lead
83.5, carbonic oxide 16.5 (PbC).
The following are a lew analyses :
LocAunss.
C.
Pb.
Pb.
Ca.
1. LeadhlllB
16.0
16.0
8S.00
81.90
0.60
Sl Zellerfeld
0.90
AnalyBis No. 1 by Westrnnb, and No. 2 by Klaproth (Beitr., iil, 167).
Hardness = 3-3.5. Specific gravity = 6.465-6.480. Colors
are white, grayish-white, and does not interfere with an
adamantine lustre. Streak is uncolored. Transparent to sub-
translucent. Fracture conchoidal. Yery brittle.
Decrepitates when heated in a small tube, loses carbonic
acid, turns first yellow, and at a higher temperature dark red,
but becomes again yellow on cooling. After decrepitation on
charcoal, it becomes reduced to a metallic globule. Soluble,
with effervescence, in nitric acid.
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THE CHEMISTS' MANUAL.
It is found in beautiful crystals at Johanngeorgenstadt ; in
the Harz ; in England and Ireland.
Found in Massachusetts, Pennsylvania, North Carolina, and
Wisconsin.
15. LITHIUM.
The principal Lithium mineral is lepidolite, or lithia mica.
Its composition varies.
Localities.
Sl
Ax..
FB.
Mn.
0.41
Na.
Li.
8.59
k.
H.
Cl.
P.
8.40
Ca.
•p.
1. Bozena..
49.06
8&61
—
1.40
4.18
4.24
0.11
—
3. CornwaU
51.70
88.76
—
1.29
M.
0.94
1.16
1.27
10.29
—
—
7.12
0.40
0.16
8. Zinnwald
46.28
14.14
17.97
4.67
—
—
4.21
4.90
0.88
—
8.10
—
—
Analysis No. 1 by QmeUn ; No. 2 by Rammelsbnrg (5th SappL, 120) ; No. 8 by Omelin.
The formula for lepidolite is [(K, Li)3 (M, fB)2] Sig + 2Si.
Hardness = 2.5-4. Specific gravity = 2.84-3. Crystallizes
as a right rhombic prism of 120°. Color, rose-red, violet, gray,
lilac, grayish-white, white, or yellow. It is to these brilliant
colors, which resemble the wings of certain lepidoptera, that it
owes its name. Lustre pearly. Translucent. Streak iA
colorless.
In closed tube gives off water and reaction for fluorine.
Before the blowpipe ftises with intumescence to a grayish glass,
coloring the flame red. Attacked by acids, but not completely
decomposed. Gelatinizes, after fusion, with hydrochloric acid.
It is found near Oto, in Sweden, grayish-white ; in Zunn-
wald, in Bohemia, lilac or reddish ; violet at Rozena, in Mora-
via ; brown in St. Michael's Mount, in Cornwall.
Found in the United States at Paris and Hebron, Me. ; and
granular near Middletown, Conn.
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287
i6. MAGNESIUM.
The principal Magnesinm minerals are :
MlNEBAL.
Habdhsss.
Sp. Qb.
FOBXULA.
COXFOBITION.
Bracite
2^
9.86-8.46
MgH
Mg 68.97; H81.1S.
£pM>mite
2.SS
1.685-1.751
MgS+7H
Boracite
J7(only4when J
I maBsi^e) f
8.918-3.974
Mg.B.+*Mg01
ifg 96.8; B 684 ;Mga 10.6.
Magneeite....
SA-4J5
8-8.08
ifgc
Mg47.6; C54.4.
Spinel
8
8JJ-4.9
MgAl
Mga8;^'Ri.
MAGNESITE.
The composition of Magnesite, when pure, is magnesia 47.6^
carbonic acid 52.4 (MgC). Ferrops oxide often replaces some
magnesia.
The following are a few analyses :
C.
Fb.
Mb.
ico.
Ca.
H.
AL.
1. Snaroin (crystalUzed)....
51.46
0.79
^
47.29
0.47
2. " **
60.79
2M
—
46.86
—
028
1.12
8. Sateboig
49.67
'^8.68
0J»
44.58
0.66
—
— ineol. 0.68
4. Frankenatein (comi>act)..
60.83
—
ojsn
48.86
—
1.89
—
Bl ** " ..
58.10
—
—
47.90
—
—
—
6. Semmering (white)
60.46
8.19
—
48.49
8.18
—
— C1.99
■^ Han (Mark)
60.98
8.00
1.61
48.71
__
__
— can
a SLGothard (yeUow)
i».88
6.64
0.56
41.80
-
-
Analysis No. 1 hj Marchand and Scheerer (J. pr. Ch., 1, 896).
" No. 8 by MUnster (Pogg., Ixv, 899).
No. 8 by Sommer (Jabrb. Min., 1866, 466).
" No. 4 by Stromeyer (Kastn. Arch., iv, 488, tJnt).
" No. 6 by RammelBberg (Handw., 897).
No. 6 by Haner (Jahrb. O. Relche, iil, 164, 1868).
'♦ No. 7 by Stromeyer (Schw. J., 11).
** No. 8 by Stromeyer (1. c).
Hardness = 3.5-4.5. Specific gravity = 3-3.08 crystallized ;
2.8 earthy ; 3-3.2 when ferriferous.
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Color is white, yellow, or brown. Lustre vitreous ; fibrous
varieties sometimes silky. Transparent, opaque. Fracture
flat eonchoidal. The primitive form is a rhombohedron of
107° 29'.
Heated in a tube, it gives off water and acts like dolomite.
When reduced to powder, it is easily dissolved by warm hydro-
chloric acid, with effervescence, more easily than dolomite. It
is infusible, but glows intensely (Mg).
First discovered by Mitchell, at Hrubschtitz, in Moravia;
^found in Silesia, Norway, Styria, etc. In the United States it
is found at Bolton, Mass. ; at Barehills, near Baltimore, Md. ;
in Pennsylvania and California.
Magnesite is much used for making Epsom salts.
SPINEL
The composition of Spinel, when, pure, is magnesia 28,
alumina 72 (MgAl). The magnesia may be replaced by lime,
iron, manganese, or zinc, separately or in combination. Alu-
mina generally takes the part of a base ; in spinel, however, it
plays the part of an acid. Spinel is not really a mineral species,
but is rather the name of a family of minerals, which are simi-
lar in composition and crystalline form.
The varieties of spinel are :
Vab. 1. Ruhy^ or Magnesia Spinel. Clear red or reddish.
Transparent to translucent, sometimes subtranslucent. Specific
gravity = 3.53-3.58. Composition MgW, with little or no Fe,
and sometimes oxide of chromium as a source of the red color.
Varieties are called {a) spinel-ruby, deep red ; (J) balas-niby,
rose-red ; (<?), rubicelle, yellow or orange-red ; {d) almandine,
violet.
Yab. 2. Ceylonitey or Iron-magnesia Spinel, Color is
dark-green, brown to black, mostly opaque, or nearly so.
Specific gravity = 3.5-3.6. Composition, (Mg, Fe) VU or
(Mg. Fe) (^1, F).
Vab. 3. Magnesia-lhne SpiTiel, Color green.
Vab. 4. Chlorospinel^ or Magnesioriron Spinel. Color
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THE CHEMISTS' MANUAL.
grass-green, owing to the presence of copper. Specific gravity
= 3.691-3.594. Composition Mg (^M, fe), the iron being in
the state of ferric oxide.
Vab. 5. Piootite. Color black. Contains over 7 per
cent, of oxide of chromium, and has the formula (Mg, Fe)
(^, iFe, Cr). Lustre brilliant. Specific gravity = 4.08.
The following are a few analyses :
LooAumB.
is..
Fb.
F«.
Mo.
Ca.
Si.
69.01
__
0.71
96.91
^
9.02
88.M
—
8.40
96.79
—
925
78.31
—
—
18.68
7.49
6.69
OT.90
—
90.61
18.94
—
8.16
66.27
—
18.97
17.68
—
9.60
64.13
aTO
—
96.77
0.97
—
«"i-
94.60
10.18
—
1.98
«B.
1. Geylon (red)
9l Aker (blue)
8. Fnnklin, N. J. (green)
4. Cejlon (Ceylonite)
6. Ural (Pleonaste)
6.' '• (Cfhioroepinel)
7. L. Lhery (Picotite)
1.10
— CuO.97
7.90
AiulyMS No. 1 and 9 by Ablch (Pogg., xxill, 806).
" No. 8 by Thompson (Mio., i, 914).
" No. 4 by C. Qmelln ( Jahresb., Iv, 166).
" No. 5 by Ablch (1. c).
" No. 6 by Rose (Pogg., i, 659).
" No. 7 by Damour (Bull. G. Soc, II, xix, 418). «
Hardness = 8. Specific gravity = 3.5-4.1; 3.523, Hardin-
ger ; 3.576, red spinel. Color red of various shades, passing
into blue, green, yellow, brown, and black; occasionally
almost white. Streak is white. Transparent, nearly opaque.
Fracture conchoidal. *
Infusible, but changes color. Soluble in borax and salt of
phosphorus. Soluble with difficulty in concentrated sulphuric
acid. Decomposes by Aision with hydrosodic or potassic sul-
phate. It occurs in pebbles of beautiful colors at Ceylon, in
Siam, and other eastern countries. Pleonaste is found at
Candy, in Ceylon. A pale-blue and pearl-blue variety is found
at Aker, in Sweden. Small black splendent crystals in the
ancient ejected masses of Mount Somma.
It is found fipom Amity, N. T., to Andover, N. J., in a
granular limestone. It is also found in Massachusetts and
Canada West.
19
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THE CHEMISTS' MANUAL.
The varieties used in the arts are usually brought to this
country separated from their gangues. They come especially
from Ceylon and Birmah. These spinels are used by jewelers,
and are called balas-ruby ; they are much less esteemed than
the oriental ruby.
17. MANGANESE.
The principal Manganese minerals are :
MlNKXlAI..
Habd-
NEBS.
Sp. Gb.
FOBMULA.
CoxponnoK.
Braunlte
6-6.6
4.75-4.82
Mn,Mii,orMQ
Mn 86.96; 0 9^;Ba2.26; HaSB.
Hausmannite . .
6-5.5
4.722
Mii.Mn.
Mn 78.1 ;0 27.9.
Pyroluslte
9-2.6
4JS2
Mil
M1168JI; 086.7.
MaDganlte
4
4J8-4.1
MnH.
ICn 62.6 ;0 27.8; H 10.2.
PBilomelane....
6.6
8.7-4.7
j (Ba,Mn)Mn + )
1 Mn + nHHn. )
jiCn and Mn 81.8; 09.6; K4.5;
1 H4A
Wad
0.6-6
»-4.26
jRMn +H.B-J
(E,6a,Co,i[ii.)
jMnlfii 79,12; O 8.82; Ba 1.4;
( Hia66w
Alabandlte
8.6-4
8.96-^.04
MnS.
Mn68.8; S86.7.
Tripllte
466
8.44-a8
i4' + B.F.
j 1?"82.8 ; Fe 81.9 ; Mn 88.6; C» 8.1
j B=Fe and Mn ; R=Ca, Mg, Pe.
Bbodochroflite .
8.6-4.6
8.4-&7
MnC.
Mn6t4; 088.6.
"DisTmcnoN between the Oxides of Manganese. — The
oxides of manganese are very difficult to distinguish with the
blowpipe, as they all give the same violet bead with fluxes.
Manganite is distinguished by giving oif water, from braunite,
hausmannite, and pyrolusite. Wad is distinguished especially
by its lightness ; for all the others, the best distinctions are
taken from the color of their streaks.
Hausmannite, — Acute octahedra with plane faces; traces
of cleavage ; streak brownish-red.
Braunite. — Octahedra, curved faces without cleavage ; gran-
ular with a bluish-black color ; streak brown.
Pyrolusite. — Tender; stains paper black.
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THE CHEMISTS* MANUAL.
291
Manganite. — ^Black, with no bluish color ; fracture granular;
streak brown ; hardness greater than the others ; gives off
water.
Wad. — Light, soils the fingers chocolate brown, and gives
off water.
The only remaining oxide is Pailomelane, which has no
very distinct characters. It is generally necessary to make a
chemiccJ test for Ba, by treating with HCl and then with S.
Its hardness is generally greater than that of the other oxides."
PYROLUSITE.
The composition, when pure, is manganese 63.3; oxygen
36.7 (Mn).
Mn'Mn.
o.
Ba.
Sl
H.
9b.
Ca.
aL.
1. Elgersberg
2. nmenan
84.06
87.0
11.78
11.6
0.68
1.2
0.61
0.8
1.18
6.8
1.8
0.S
0.3
Analysis No. 1, by Tamer (EdlDb. Trans. , 1838).
" No. 8, by Scheffler (Arch. Pbarm., xxzv, 800).
Hardness = 2-5.5. Specific gravity = 4.82 (Turner). Color
iron-black or dark steel-gray. Lustre metallic. Opaque. Its
fracture is irregular and unequal. Streak black. Crystallizes
as a right rhombic prism of 93*^ 40'.
Pyrolusite is infiisible, not even giving off water. With
fluxes gives the reactions for manganese. Hydrochloric acid
dissolves it with evolution of chlorine. When it contains
rhodonite, gelatinous silica is deposited.
This ore is extensively worked at Elgersberg, near Ilmenan,
and other places in Thuringia; at Norderehrensdorf, near
Mahrish ; Traban, in Moravia, which place affords many hun-
dred tons of ore ; at Plateau, in Bohemia, and elsewhere.
Occurs in the United States with psilomelane ; abundantly
in Vermont, at Brandon, Irasburg, Bennington, etc., both
crystallized and massive; in Conway, Mass., in a vein of
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THE CHEMISTS' MANUAL.
quartz ; at Plainfield and West Stockbridge, Mass. ; at Win-
chester, N. H. ; at Salisbury and Kent, Conn., forming velvet-
like coating on limonite. Found also in California, New
Brunswick, and Nova Scotia.
Pyrolusite and manganite are the most important ores of
manganese. Pyrolusite is used extensively in glass works, for
making bleaching powders and also for the manufacture of
oxygen.
MANGANITE.
Composition of Manganite, when pure, is sesquioxide of
manganese 89.8 (=Mn 62.5, O 27.3), water 10.2 (MnH).
Mn.
0.
H.
Fb, Ba and iom.
1. Befeld
62.88
86.81
37.64
9.60
10.00
fL Cheverle
Qangue 1.14-2.05
Analysie No. 1, by Omelin (lb., xlii, 206).
" No. ft, by How (PhU. Mag., IV, xxxi, 166).
Hardness = 4 ; Specific gravity = 4.2-4:.4. Color dark-
brown or iron-black. Streak reddish-brown to nearly black,
darker than limonite. Lustre semi-metallic. Opaque; minute
splinters, sometimes brown by transmitted light. Fracture
uneven. Crystallizes as a right rhombic prism of 99*^ 40', with
an easy cleavage parallel to the brachypinacoid, and another
more difficult, parallel to the prism. It is usually well crys-
tallized. In a tube it gives off water when heated, and is
then infusible; this distinguishes it from the other oxides.
With fluxes gives the reaction for manganese. In acids,
even before calcination, it is dissolved and gives off chlorine.
Manganite occurs at Ilefeld, in the Harz; TJndennes, in
Sweden ; Christiansand, in Norway ; and Cornwall, etc. It is
found also in Nova Scotia and New Brunswick.
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THE CHEMISTS' MANUAL.
WAD.
The composition of Wad varies as follows :
LOCAUTIBS.
Mn. ifN.
0.
ftE.
Ba.
Cu.
H.
1. DeYODBhlre
79.13
60.8 -
68.50
66.16
8.82
11.17
16.75
3.70
1.4
16.84
-
10.66
%, YicdesMM
8. HUlHdale^N.Y.
4. SUdbeiY?
12.4 M 7.0
11.60, inso1.8.S6.
j Co 13.07, Si 0.92. 2i 0.75,
1ca0i59, Mg0.S8, KOJK.
AnalyfiiB No. 1 by Tamer (Edlnb. J. Scl.. N. S., li, 218).
No. 3 by Berthlv (Ann. Ch. Phya., U, 19).
•* No. 8 by Beck (Rep. Min. N. Y., 56).
^ No. 4 by Bahr (J. pr. Ch., Uil, 808 ; fr. OeiV. Ak. Stockh., 940, 1860).
Hardness = 0.5-6, Specific gravity = S-4.26. Color is
dull-bluish, or brownish-black, or reddish-brown. It is often
very light and soils the fingers.
In a closed tube, wad when heated yields water. Loses
oxygen by ignition. Gives the reaction for manganese. Yields
chlorine with hydrochloric acid. The varieties containing
cobalt and copper react for these metals.
When wad contains cobalt, it is called asbolite or earthy
cobalt.
When wad contains copper, it is called lampadite or cupro'
ous manganese.
Wad, or bog-manganese, is found abundant in Columbia
and Dutchess counties, N. T. ; at Austerlitz, Canaan Centre,
and elsewhere occurs as marsh deposits. Also found in New
Hampshire.
This ore, when abundant, is valuable*
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THE CHEMISTS' MASVAL.
i8. MERCURY.
The following are the principal Mercuiy minerals :
HABDirafla.
Bp. Gb.
FOBMTTLA.
Native Mercery
Clnnabftr ....
1-2
18.668
8.996
6.482
Hg
HgS
Hg.Cl
100
Hge6.2; S18.&
Hg84.9: C115.L
Calomel
CINNABAR.
The composition of Cinnabar, when pure, is mercury 86.2,
and sulphur 13.8 (HgS or HggSg).
LooAurm.
8.
Hft.
1. Neamarktel
14J»
17.6
11.88
86.00 - 99.26
2. Japan
78.4, 9e 1.7, M a7, Ga 1.8, %i OX
69.36, Fe 1.28» Ga 1.40, il 0.61. Ifg. 0.49, Si 14i».
8. Calitomia
AnalyslB No. 1 by Klaproth (Beltr.. It, 14).
No. 2 by John (John's Ch. Unt., i, 252).
" No. 8 by A. Bcaley (J. Ch. See., iv).
Hardness = 2-2.5. Specific gravity = 8.998. Color is
cochineal-red, inclining to violet. Streak characteristic ver-
milion-red. When it is impure, the color is often black, but
the streak is always red. It absorbs light easily, which often
makes it opaque. It is the most refrangent of all known
bodies. Sectile. Polarization circular. Ordinary refraction,
2.854; extraordinary, 3.201 (Descl.).
On charcoal it volatilizes without residue. In a tube gives
a red sublimate. It is not attacked by acids, and is the only
sulphide which is not acted on by aqua-regia.
The Idria mines are in the carboniferous formation ; those
of New Almaden, California, in partially cretaceous or tertiary
beds. It is found in Japan, China, Chili, Peru, etc.
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THE CHEMISTS' MANUAL.
295
Cinnabar is the principal ore of mercury, from which it is
obtained by sublimation. It is sometimes ground and used as
a pigment, called vermilion.
19. NICKEL
The J)rincipal Nickel minerals are :
HniBBAI..
Habdihess.
8p. Qb.
FOBMITLA..
Composition.
KUlerlte
8-8.6
4.6-6.66
NIB
Ni64.9; S86.1.
Niccollto
6-6.5
7.88-7.671
NlAe
Ni44.1; As 65.9.
Ulmannlte. . . .
6.6-6
6.2-6.61
NiS + Ni (Sb,AB),
Nia7.7; 8b 67.2; S 16.1.
AonAbez^te..
—
—
N1;1'b + 8H
Ni 87.2; As 88.6; H24.2.
Zaratlto
8-8.85
8.97-2.098
NIC + 2N1H + 4H
Ni69.4; C11.7;H28.9.
Chloanthite, or the niccoliferous smaltite, is sometimes very
valuable for nickel, as the cobalt is nearly absent in some
specimens.
MILLERITE.
The composition of Millerite, when pure, is nickel 64.9,
sulphur 35.1 (NiS).
LOCALITIKS.
8.
Ni.
Co.
Fa.
CXT.
1. Saalfeld
86.79
85.14
61.84
63.08
0.58
0.40
1.14 - 100
8. Gap Mine, Fa
0.87, gangue 0.28 = 100.86.
Analysis No. 1 by Rammelsberg (Ist Sappl., 67).
No. 2 by Genth (Ann. J. Sci., U, xxxiil, 195).
Hardness = 3-3.5. Specific gravity = 4.6-5.65 ; 5.65 fr.
Saalfeld Rammelsberg; 4.601 fr. Joachimethal Kenngott.
Color brass yellow, and often with an iridescent tarnish.
Streak bright. Lustre metallic. Brittle.
In an open tube gives, when heated, sulphurous fumes.
Fuses to a globule on charcoal before the blowpipe ; gives a
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THE CHEMISTS' MANUAL.
magnetic globule in the reducing flame. With fluxes most
varieties show traces of copper, cobalt, and iron.
It is fouDd in cavities at Bohemia, Przibram, Hummelfahrt
mine near Freiberg, Saxony, Cornwall, etc. It is found at
the Sterling mine, Antwerp, N. S. ; also at the Gap mine,
Lancaster Co., Pa.
NICCOLITE.
The composition of Niccolite, when pure, is nickel 44.1 ;
arsenic 55.9 (NiAs or NigAsg).
Ab.
Nl.
Fk
PB.
Co.
SB.
8.
Cu.
No. 1
54.73
0106
68.71
44.81
48.60
46.87
0.84
0.46
0.88
04S
0.06
0.40
8.18
0.48
No. 2
No. 8.
— gangae0.S0.
1.44
AnalyslB No. 1, by Stromeyer (OeL Anz. GOtt., 1617, 804).
" No. 8, by Ebelmen (Ann, d. M., IV, zl, 66).
'' No. 8, by Bchnabel (Bommelsberg, 4th SappL, 188).
Hardness = 5-5.5. Specific gravity = 7.33-7.671. Color
is a light copper-red, which is very characteristic. The inten-
sity of the color is, however, variable, and is subject to tarnish ;
those specimens containing antimony are much darker, while
those containing arsenic are paler. Streak is pale brownish-
black. Lustre metallic. Opaque. Fracture uneven. Brittle.
On charcoal it gives oflF a garlic odor with white vapors, if it
contains arsenic; when antimony is alone present, there is
only a coating of antimony without any odor. With fluxes
gives reactions for iron, cobalt, and nickel. Soluble in nitro-
hydrochloric acid.
It is found in the Saxon mines of Annaberg, Schneeberg,
etc.; found also in Styria, AUemont, Cornwall sometimes;
Scotland, Chili, and Argentine provinces. It is also found
at Chatham, Conn., in gneiss associated with smaltite.
Niccolite is a very important ore of nickel.
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297
20. PHOSPHORUS.
The principal Phosphorus mineral, or minerals containing
phosphorus, are :
Schreibersite..
CiyptoUte.
Apatite..
PBeadomAlachite .
BoTickite..
Callftmite.
Plibsphorgammite
or Omninlte
HABDHB88.
6JS
I^romon^ite.
J 6. (Some-
] ttmee 4.5)
4.5-*
8.6
85-4
j- 2.5-a
8.5-4.5
Sp. Ob.
7.oi-7.aa
{4.6
Cryptollte.
4.78
Phosphocerite.
«.ai-8J»
4-4.4
S.e96--8.707
S.5-S.BS
&9-4.20
6.5-7.1
FOBMULA.
P,Fe,Nl,C.
CoxpoeinoN.
^0neMmplevl
P7.a6: Fe 87.80;
C nndeterm
Oe, P (the
Ce replaced!^
in part by
1 (CI, Fl).
^; Ca, H.
Analyses
vary much.
\
{ (Pe,Ca,).
( i»*,+15H.
M'P+SH
sample yielded
Ni4.S4
undetermined.
One analysis gave
*? 87.87; Ce,DI 73.70;
Fe 1.51 (Cryp.);P 29.66;
Oe, i)l 67.88: Pe 8.95
^ (Phosphocerile).
Ca 48.48=89.86;
Ca8.84ori»*
43.96; Ca 60=99.96; Ca
P; F8.77; Ca 8.97.
r P 40.98; <
I a 6,81;
IM.^-"
rities.
I 8Pb,t»*+
) Pba.
t **»■ 94.65: Cn 67.96; H 8.90.
( Analysis of one sample.
ji>' 90.49; ¥e 62.29; Ca
\ 8.16; H 19.06.
'^49.89; Al 80.75; H 26.86.
iSF 72.0;^ 0.06; Ca 6.00;
Si 4.96 ;i^' 2.80 ;H 14.75;
F, As, (r.
iPb 74.1; $16.7; a 2.6;
1 Pb 7.6.
APATITE.
The composition of Apatite is phosphate of lime with
chloride or fluoride of lime or both; Ca3P + JCa(Cl,F); or
[-^Ca-f--j*^Ca(Cl,F)],oP3 = for chlorapatite. Phosphoric acid
40.92, lime 48.43 (= 89.35 P,Ca), chlorine 6.81, calcium 3.84
(=10.65 CljCa); and ior fluorapatite, f 42.26, Ca 50.00
(= 92.26 P,Ca), F 3.77, Ca 3.97 (= 7.74 F,Ca) ; and the analysis
should give for the former *P 40.92, Ca 53.81 ; CI 6.81 ; for the
latter, "P 42.26, Ca 55.56, F 3.77 (Rammelsberg).
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298 THE CHEMISTS* MANUAL.
The following analyseB are by G. Kose (Pogg., ix, 185) :
1. SXABVIE.
NOBWAT.
2. MUACTA,
Spain.
91.18
Se.066
4J»
0.886
4.60
7.049
8.174
S.986
8. Abbhbai.,
NOBWAT. "
Ttbol.
Phoephate of Lime. . ,
Chloride of Calcinm .
Fluoride of Calcinm.
Speclflc* Gravity
98.189
0.801
7.01
8.194
92.16
0.16
7.09
The following are a few other analyses :
f.
'#■.
Mo.
Ca.
Cl.
F.
H.
1. Bnarnm
41.64
1.T9
6a46
2.66
Not deter.
2.KragrOe,«A««...
41.86
0.S9
—
68.84
410
t<
J0.4S, ^ 0.88;alk.ai7;
1 iBBOl. 0.89.
A " red
41.81
1.06
—
64.60
1.08
(t
0.88, alk. 0.80; ineoLl.ia
4 PargaB, W««
40.76
0.81
—
64.74
Tr.
ti
- •#/Fe.Ail0.99.
6. m&BY,ydUno....
4s.oe
0.17
—
66.17
Tr.
«i
0.16
6. Staffel
84.48
6.43
0.16
45.70
-
8.45
(9.45, Al 1.06; Si 4.88;
(clJSl;Na049;K0.5eL
AnalyBis No. 1. by Weber (Pogg., Ixxziv, 806).
" No. 8 aDd 8, by VOlcker (J. pr. Ch., Ixxv, 884).
No. 4, by Arppe (An. Finska Min., 4).
" No. 5, by Rath (Pogg., xcvi, 881).
" No. 6, by Foster (R)., 1866, 716).
Hardness = 4.5-5. Specific gravity = 2.92-3.25. Apatite
is generally found in large crystals, which are yellow, green,
blue, or violet. The colors are never very bright. It may
also be white, red, flesh-red, and brown. Lustre vitreous,
inclining to subresinous. Streak is white. Transparent,
opaque. In the white varieties, there is sometimes a bluish
opalescence in the direction of the vertical axis. Cross frac-
ture conchoidal and uneven. Brittle.
Apatite fiises with difficulty on the edges at 4.5, coloring
the flame red (Ca). When moistened with sulphuric acid and
heated, colors the flame pale bluish-green (P). It is soluble in
hydrochloric and nitric acids, without residue, when CaFl is
absent. It is sometimes phosphorescent in the dark, especially
in powder.
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THE CHEMISTS' MAKCAL.
299
It is found in Sweden, Norway, Switzerland, Bavaria, Bo-
hemia, and in Cornwall.
In the United States it is found in Maine, New Hampshire,
Massachusetts, New York, New Jersey, l^ennsylvania, Mary-
land, and Delaware. Also found in Canada.
A compact variety, resembling impure limestone, has been
found near Charleston, S. C. It is used in making fertilizers.
PYROMORPHITE.
The composition of Pyromorphite is phosphoric acid 15.7,
oxide of lead 74.1, chlorine 2.6, lead 7.6 = phosphate of
lead 89.8, chloride of lead 10.2 = 100. [SPbg P + PbCl, or
(^TT Pb -f t*ir PbCl),o P]. Part of the lead is often replaced by
lime, part of the chloride of lead replaced by fluoride of cal-
cium, and arsenic acid part of the phosphoric acid.
The following are a few analyses :
LocALmsa.
pii;fe
PbCl.
CaF.
87^
10.28
ao7
89.16
10.47
—
80.18
9.94
—
90.09
9.91
—
TIM
10.84
1.09
f.
.V.
Ab.
PB.
[16.17]
s.ao
72.44
16.11
0.66
77.46
15.88
0.69
77.46
ca.y»:
1. Blelatadt (brown cryetalllsed) . . .
2. Kraoiiberg (green)
1L BeresovBk (jellowiBh-green)
4. LeadhiUs (oran^-red)
Polyephoerite (with mach phOBptaate
of lime).
6l Freiberg (brown)
CoHTAixDro Absksic Acid.
6. Ztchopan (white)
7. Badenweiler (wax-yellow)
& '' (dark-orange)
0.86, Fe,P0.77.
— Fe,tir0.60/V<r.
11.06
PbCl,
10.09
— Ca 2.40, (71 2.64.
— Ca 2.46, CI nndet.
AnalyslB No. 1 by Lercb (Ann. Cb. Pharm., xlv, 828).
" No. 2 by Sandberger (J. pr. CJh. , xlvii, 462).
'' No. 8 by Strnve (Kokech. MId. Rnsel., ill, 42).
" No. 4 by WGhler (Pogg., Iv, 161).
" No. 5 by Kersten (Schw. J., Ixi, 1 ; Pogg., xxvi, 489).
" No. 6 by WGhler (Pogg-, iy, 161).
'* Nob. 7 and 8 by Seidel ( Jahrb. Mln. , 1664, 222).
Hardness = 3.5-4. Specific gravity = 6.5-7.1, mostly when
without lime ; 5-6.5, when containing lime. The colors are
veiy variable, green, yellow, brown, or white, and are depend-
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THE CHEMISTS' MANUAL.
ent upon the compoflition. Streak white, sometimes yellowiflh.
Lustre resinous. Subtransparent, subtranslucent. Fracture
subconchoidal, uneven. Brittle.
Pyromorphite occurs principally in veins, and accompanies
other ores of lead.
It is found in Brittany, Saxony, Bohemia, at Sonnenwerbel
near Freiberg, and in Siberia. It is found green and brown
at Cornwall, gray at Devon, green and yellow at Derbyshire,
golden-yellow at Cumberland, red and orange formerly in
Scotland, clove-brown and yellowish-green at Wicklow.
In the United States it has been found at the Perkionen
lead mine near Philadelphia, and very fine at Phenixville;
also in Maine, New York, Massachusetts, and Bristol, Conn.
Good crystallizations of bright green and gray colors have
been found in Davidson County, N. C. It is a valuable ore
of lead.
21. PLATINUM.
The principal Platinum
minerals are :
MnrKBAL.
Habd-
NE88.
Sp. Gb.
FOBMULA.
CoMFOsmox.
Flatinum (PlatiDa).
PlatinirWlum
4—4.5
ft-7
16-19
».6-28
Pt+Pe,Ir,08,etc.
i Ft, Ir + {
j Ore« of Pt u saally con tain
( Pt 90^, ineol. lOH, Ir i%, Bu ff.
Pt 19.64-56.44
PLATINUM.
The composition of Platinum, or Platina, is platinum com-
bined with iron, iridium, osmium, and other metals.
The following are a few analyses :
IjOOALXTIBS.
Pt.
Au.
Fb.
IB.
Bh.
Pd.
Cu.
H.
08.
SAirn.
1. Ural
a. ChoGO,S.A.
8. OaliforDia .
4.
5.
9a87
86.16
79.85
76.50
68.80
0.66
1.^
0.80
ia98
&03
4.46
aio
6.40
0.06
1.09
4. SO
0.86
a70
4.44
2.16
0.65
1.95
1.80
1.80
0.85
1.95
1.80
0.10
2.80
0.40
0.75
1.26
4.25
0.11
1.91
496
7.66
[a.56]
0.06*
1.26*
0.97, MnaiO.
2.60
1.50,Pb(?)0m
- Hg0.«D.
Tbe loBB, with some osmium.
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THE CHEMISTS' MANUAL.
301
Aiia]7BiaNo.lbyO8aim(Pogg.,Tlli,605; zi«411: zlU,»3; xiv,8»; xy.ISB).
Na 2 by Svanberg (Institnt, U, SM).
« Kos. 8 and 4 by 8t C. DeyUle and Deb»y (Ann. Ch. Phys., IH, ItI, 44»).
^ No. 6 by Kiomayer (Arch. Fbarm., II, ex, 14 ; Jahreab., 18(B, 707).
Hardne88=4-4.5. Specific gravity = 16-19, 17.862, 17.759,
two masses (G. Eose) ; 17.200, a smaller ; 17.108, small grains
(Breith) ; 17.608, a mass (Breith) ; 17.60, lai^ mass from
Nischne Tagilsk, Sokoloff. Color and streak are whitish
steel-gray; shining. Lustre metallic. Opaque. Ductile.
Fracture hackly. Occasionally magneti-polar. When crys-
tallized, it is found in cubes and octahedra. Platinum was
found in pebbles and small grains in the alluvial deposits of
the River Pinto, in South America. It was first discovered in
1822, in Russia ; it occurs at Nischne Tagilsk and Gorobla-
godat in the Ural in alluvial deposits. Russia affords annually
about 800 cwt. of platinum, which is nearly ten times the
amount from Brazil, St. Domingo and Borneo, which last
place furnishes 600 to 800 lbs. annually. It is also found in
the sands of the Rhine ; in Ireland, in Honduras, in traces
with gold in Rutherford Co., N. C. ; at St. Francois Beauc,
etc., Canada East.
The prominent masses of Platinum are :
Weijfht.
Mass brought by Hnmboldt from S. A. (Berlin Museum). . 1.088 grains.
from Coudoto (Madrid Museum) 11.641 "
" " " Ural (weighed ICV^ Russian pounds).. 11. 67 lbs. Troy.
" in Demidoff Cabinet, the largest yet obtained 21 "
22. POTASSIUM.
The principal Potassium minerals are :
MnfBiuL.
Habd-
KB88.
Sp. Gb.
FOBMITUL.
CoxFOSinoir.
Kalinlte
a-a.6
1.75
KS'+^S, + d«H.
ESl&4;Ai 8 86.3; H46.5.
SyMte
3
i.»-a
KCl.
K6a.6; 01 47.5.
CamaUite.
KClf8MK01 + 13H.
KCl 36.88; M^d 84.30; H 88.89.
Nitre
%
1.087
kK
k46.6; ii*'58.4.
T»jk)rite
s
(|K0 + iNH.O^SO,.
K0 47; NH,0 5.8; SO, 47.8.
Aphthilallte....
8-8.5
1.781
KS.
K64.1; 8 46.9.
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THE CHEMISTS' MANUAL.
NITRE.
The compoflition of nitre, when pure, is potash 46.6 ; nitric
acid 53.4 (K N). Klaproth obtained for an African specimen
(Beitr., i, 317) nitrate of potash 42.65, sulphate of lime 25.54,
chloride of calcium 0.20, carbonate of lime 30.40.
A nitre crust from the vicinity of Constantino, Algeria,
afforded K N 86.00, CaN and MgR 3.00, NaCl 6.00, H 3.50,
insol., etc., 1.50 (Boussingault). Hardness = 2. Specific
gravity = 1.937. Crystallizes as a right rhombic prism 118® 50'.
It is usually white and transparent, or at least translucent.
Streak white. Lustre vitreous. Taste saline and cooling.
Nitre deflagrates on charcoal, coloring the flame violet (K).
Soluble in its weight of cold and half its weight of warm
water. It is not altered by exposure.
Nitre is found generally in minute needle-form crystals and
crusts on the surface of the earth, on walls, rocks, etc. It
fornjs abundantly in certain soils in Spain, Egypt and Persia,
especially during hot weather succeeding rains. It is found in
Madison Co., Kentucky ; it is found scattered through the
loose earth covering the bottom of a large cave ; also in other
caverns in the Mississippi valley; also in Tennessee. Nitre
is the saltpetre of commerce.
23. SILICON.
The principal Silicon minerals :
Habdnbbs.
Sp. Gb.
FOBMULA.
CoKPoaiTzoii.
Qnartz
7
8.6-2.8
81.
SI 46.67; 0 58.88.
OpaL
6.6-6.6
1.9—2.8
81 + xH.
H = 8-.21;(.
Wallavtontte..
4.6-6
2.78-2.9
CaSi.
rSSURmaybeCa,^
Ga 48.8; 8 61.7.
Pyroxene
6-6
8.28-^.6
- Mg,Pe,Mn,Zii, ■
^ Naandk.
—
8.2-8.88
(CaMg^i.
da26.8;ilg 18.6; 8166.7.
SaAlUe
—
8.26-8.4
(CaMgPe)SL
Oa24.9;Mg 18.4; SI 68.7.
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T..
THE CHEMISTS' MANUAL. <
The Pbincifal Silicok MrsmiAjjSh^Cantinued,)
Hasdmus.
Sp. Gr.
FOBXULA.
COXFOfllTIOH.
BsdendergUe..
-
8.&-&66
(4Ca + iFe)81.
Fe 87.01 ; Ca 82.96 ; Si 47.78.
81 44.4-51.79; Ca 14-84;
AvgUe,
—
a96-«JS
(OakgPexSlSl).
Mg 8.75-81.11; Fe4JM-
. l&08;ii 8.38-8.68.
Bhodomite...
6.5-«.5
8.4-8.68
HnSi.
Mn541: 8145.9.
Spodamene...
6.6-7
8.18-8.19
(LI, + 5i)fli,.
Li6.4; A189.4; 8164.8.
PetaUte
6-6.5
3.39-S.5
[(LlNa),+ii]Sl,+88l.
fRSl (R may bel
Li88;Nal.8; jid 17.8;
8177.7.
Amphibole...
5-6.5
9.9-&4
. Na, k. Ca. kg,
[ Fe,andifn). J
T^^mnoOie ....
5-6J&
ad-«.i
(6aMg)*81.
( da 18-15; Mg 84-86;
( " 8157-69.
-
8.65-8.47
(Three yarleties, J
< depending on the >
( qoantityofiron. )
f Ca 10-14 ; Mg 5-88;
A 5-15; Fe 8-89;
I 8140-^.
Ae^nolUe
-
8-8JI
(CaMgFe)Sl.
J 8155-69; Mg 9-84;
1 Ca 9-81 ; Fe 8-11.
Beiyl
7.6-«
8.68-8.76
(iBe. + jij)Si..
fie 14.1 ;A1 19.1; 8166.8.
Chrysolite....
6-7
8.88—8.5
(MfirFe).8L
Mg50J»; Fe9.86; S14a78w
WiUemite.....
5JJ
8.89-4.18
Zn.Si.
Zn'«.9; 8187.1.
Phenadte.
7.5-8
8.96-8
Be,Sl.
Be 46.8; 8154.81
Qamet
6J5-7.5
8.16-^81
(B,),81, + B,8i,.
Pmvp^
-
8.7-8.76
j[i(MgCaFeMn).l
1 + iXq.Si.. J
fMg ia48; M 88.47; Ca
6.58; Fe 9J»; Mn 6.97;
8148.45.
Qrx>3tukurUe..
—
8.4-8.7
(iCa,iAi).81..
Caa7.8;ii 98.7; 8140.1.
—
—
(iFe, + ^).Si..
E\)48.8; 1^80.5; 8186.1.
Bpeasartlte....
-
8.7-4.4
[KMnPe). + jii].8l,.
Mn 80.96; Fe 14.98; 3k
18.06; 8185.88.
OuvarovUe.,..
7.5
8.41-8.58
aCa. + K*).81,.
Zircon
7.5
4.06-4.76
Zr8L
Zr67;888.
Versavianite .
$Ji
8.49-8.45
j [| (Ca Mg Fe), + |
1 |(iiPe)],Sl,. )
jCa 87-88 jMgO-lO; Fe
1 0-16; id 10-98; 81 85-89.
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THE CHEMISTS' MANUAL.
The PBDrcil>AL Silicon Minerala— (Cim^niM^I.)
Sp. Qb.
Bpidote
6-7
8J»-«.5
lolite
7-7.5
8.fl6-».67
8.7-8.1
Biotlte
MMCOTite
a-«.6
2.75-8.1
LepidoUte....
2JJ— 4
2.84-8
Wemerlte....
5-6
2.68-2.8
NepheUte
5.6-6
2.5-2.65
XApiB-Lftznli. .
5-6.5
2.88-2.46
Haflynite....
5.5-6
2.4-2J^
Lencite
5.5-6
2.44-2.66
Anorthlte
6-7
2.66-2.TB
Labradorite...
6
2.67-2.78
Oligoclaae....
6-7
2.66-2.72
Alblte
6-7
2.60-2.65
ft
Orthodase....
6-6.6
2.44-2.62
Chrondrodite.
fr-6.5
8.118-8.24
Tourmaline ..
7-7.5
2.94-8.8
FOBMUXiA.
aGa,-t-|^M).8i».
2(MgFe)81-i'An8i,
i(idPe)1.81,.
[K.(AiFi)].8l, +
1481.
SI. + SBl.
Coxpoamcnr.
Ca 16-80; M 14-28;
Fe7-17; S186-W.
Mg8.8; Fe7.9; *ij 88.9;
8149.4.
[KKMgFe), + ) jMg 4-25; Fea-20; 'A
11—21; '#e4-25; Si 86-44.
E 5-12 ;M 81-39;
Fe 1-6; 8148-60.
E 4—14: LI 1-6; M
14-88; ¥e 0-11; Si 42-64.
H
[UCaNa).+|Al].
81, + Si.
j (Na.K.).8i.+ )'(
( 8AI.81. -1-881. ) i
Na 5; Cal8.1; ^28.5;
81484.
Nal6.9; K 6.2; A188.7;
8144.2.
Na 0-12; Ca 1-28;
ii 11-48; Fe 0-4;
8140^-66; 80-5; 80-4.
Na 16.6; Al 27.4; 81 82;
Ca9.9; 814.2.
K21.5;i^28.5; 8166.
Ca20; A186.9; 8148.1.
Na4.6; Ca 12.8 ; iy 80.8 ;
8162.9.
i<Na,Ca), + IM)\ i Ka 2-12 ; Ca 0.5-6 ;
81, -i- 8|Si. ) \ iy 19JM ; Si 69-64.
(iNa. ■^ fAl).81.
-i-(»l.
(iK. + |S).81,
•I-6SL
Mg.81..
Na,0a,Al,Fe,813,8.
J UNa. + |il). 1 j
J SI. + oas: n
KSi -i- iysi..
oca. + iAJ).8i,.
(Na,Ca)81 -i- AlSl..
[(Na, K, Ca, Kg,]
Fe).(Fe.MB)].
81..
Nall.8;Al lft6; S168.&
K16.9;M1&8;8164.&
One sample gave Mg 54.5 ;
Fe 6.TO ; 81 88.19 ; Fe 5.66.
fNaO-5; ko-4: GaO-2.
MgO-16; FeO-17; Ve
0-11 ;ii 80-44 ;B 4-11;
8i85-4a
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THE CHEMISTS' MANUAL.
The Pbiucipal Silicon MinERAiA-^Continued),
306
HABDNV88.
8p. Gb.
FOBinTLA.
COXPOSITIOH.
(15 (fori
tnuii»-
AndalDSite....
(for
toi»que)J
8.05-8.85
A)81.
A16&9; 8i8a8.
r'il 68.9 ; 'S.8a8 (£l may be
FRmdite
6-7
8J^-8ai
MBL
replaced by 9,;a1 oTO.Bi
[ Mg. H may be preMnt)
Cymnlte
6-7J»
8.45-8.7
A»l.
A168.9: S86.&
To]>u
8
8.4-8.66
iysicFi).
j 81 16.17 ;A1 99.68; 0 84.67;
1 Fl 98.68.
BnclMe
7.6
8.086
(iH, + |Be. + Hi>8i.
Be 17.4; ^86.8; 8141.1;
H6.9.
BAtottte
6-&5
2.g-8
(C8.3.JB)8L
Ca 86.0; H5.6; B 31.9;
8187.5.
Tlumita
6-A.5
8.4-8.56
(Ca,Ti)Sl.
Ca 91-98; Tl 88-48; 81 80.86.
Stauollte
7-7.5
8.4-8.8
J [i(4H + |M« + )
J iPe). |A1).SI.. )
H1.7; Mg9.6; Fo 15.8;
( & 61.7; Si 98.8.
PtetoUte
0
9.68-9.78
an + }Na f |6a)Si
JH9.7; Na9.8; Ca 88.8;
81 64.2.
Laamontlte...
8.5-4
9.96-9.86
(iCa,-i-{;^)Sl,+8H.
j Ca 11.9 ;& 91.9; 8160.9;
H 16.8.
Dioptose
6
8.978-8.48
CuSI + H.
Cu 60.4 ; 81 8a9;H 11.4
ChryBocoUa...
%-4
9-9.88
CnSl + 9H.
Ca4S.8;H90.6;8184JI.
CUamine
4.5-6
8.16-8.9
Zn,81 + H.
Zn67.6; H7.5; 8196.
Pr^hnite
6-«.6
9.&-S.96
(iH + |Ca + |A1),81,.
j(7a97.1; H4.4; A1919;
1 8148.6.
Chlonstrolite.
6.5-6
8.18
J (Ca,Na.)a81a + 1
(9(Al,iB^B),Si.+6H. S
(Na5.9; Ca 18.7; Fe 6.4;
( id 94.0; 8137.6; H7.6.
Apophylllte..-
4L6-6
9.8-9.4
J[iH+i(4i+«Ca)].J^
i Si + HSi. )
j H16.7; K4.8; Ca98;
81 66.6.
Natrolite
5-5JJ
9.17-&95
NaiiJ^i^iH.
Na 16.8; A197; 8147.9;
.H9.6.
Analdte
6-5.6
9.99-9.98
Na;il,48l,aH.
jNal4.1; AiaaS; 8154.4;
( il 8.2-
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306 THE CHEMISTS' MANUAL.
The Pbikcifai. Silicon UtsebaJj^— (Continued).
Hardnbbb.
Sp. Gb.
Chabazite
4.5
2.0-2.19
Hannotome...
4.6
2.44-2.45
Stelblte
8.6-4
2.094-2.206
Henlandlte. ..
8.5-4
2.2
Talc.
1.15
a-2.5
2.565-2.8
Seplollte
Serpentine....
-
Prochlorite....
1-2
2.78-9.96
FOBMin^A.
( [|Ca + 4(Na,K)]
( iy,4Si,6H.
Ba^,6Si +SH.
Ca,£l,6Sl,6H.
Ca,'Al,6Si,6H.
(jMg + JH)Si.
i[£:.Sl. + 2H.
aMg+iH).81 + 4H.
( [KMg,Fe). + m]
SiSH.
CoMFoainoN.
H
f Ca4-ll; NaO-4;
E0.17-2l66;^ 17-21;
8145-52; H 19-2&
Ba28.7; ^15.9; Si 46JS;
H18.9. When it containB
Ca7.4;iy 20.5; Si 47.9;
K 6.8 ;H 17.9.
Ca&9; 'A116.5; 81 ff7.4;
Ca9.2; M 16.9; 8109.1;
H14.8.
Mg 83.5; Si 62.8; H3.7.
Mg27.1; H12.1; Si 0O.&
Mg 42.97; Si 41.14; H 12.89.
Mg 15.8 ; Fe 27.5 ; M 19.7 ;
Si 28.8; H 11.7.
QUARTZ.
The composition of Quartz is pure silica or silicon 46.67,
oxygen 53.33 (Si02). The many different varieties of quartz
may be i-egarded as allotropie modifications. " Quartz may be
massive ; coarse or fine granular to flint-like or crypto-crystal-
line. Sometimes mamillary, stalactitic, and in concretionary
forms."
Colorless when pure ; often various shades of yellow, red,
brown, green, blue, and black. Streak is white, with pure
varieties ; if impure, often the same as color, although paler.
Transparent, opaque. Hardness = 7. Specific gravity =
2.5-2.8 ; 2.6413-2.641 (Bendant) ; 2.663 (Deville). It acquires
vitreous electricity by fiiction, but loses it very quickly.
Tough, brittle, fiiable. Polarization circular, there being a
colored centre instead of a central cross, and the rings of color
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THE CHEMISTS' MANUAL. 307
around enlarging as the analyzer is turned to the right in the
right-handed crj- stals, or left in the left-handed ; and colored
spirals are seen, which rotate to the right or left, when the
incident light and emergent light are polarized, one circularly
and the other plane.
It is infusible before the blowpipe. With soda it unites,
with effervescence; with salt of phosphorus no action takes
place. It is not acted upon by any acid except hydrofluoric.
The varieties of quartz are quite numerous, and may be con-
sidered as follows :
" Crystallized Quartz.
^' Concretionary Quartz, Agate, or Chalcedony.
" Jasper.
" SiLEX or Flint, which is more easily attacked by alkalies
than the other varieties. It is never pure.
" Earthy Quartz, sometimes in the shape of flour, and in
every way analogous to ihe silicic acid produced in the labo-
ratories. It is often formed of the skeletons of infusoria.
" QuARTzrrEs and Sand."
With respect to Crystallized Quartz, the form is a rhombo-
hedron of 94° 15', but this primitive form is rarely found, and
is always in very small crystals. The most general form is the
combination of two rhombohedra, by which the prism is appar-
ently terminated by a hexagonal pyramid. The rhombohedron
with the hexagonal prism is a form sometimes found.
Quartz is found penetrated by various minerals, " as topaz,
chrysoberyl, garnet, different species of hornblende and pyrox-
ene groups, kyanite, zeolites, calcite and other carbonates,
rutile, stibnite, hematite, gothite, magnetite, fluorite, gold,
silver, anthracite, etc."
Concretionary Quartz, Agate, or Chalcedobty is less
pure than crystallized quartz. A gray chalcedony from Hun-
gary gave, according to Redtenbaher (Eamm. Min. Ch., 1007),
Si 98.87, *f^ 0.53, CaC 0.62 = 100.02. Heintz analyzed a car-
nelian, which was a clear red, and found the red color to be
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808 THE CHEMISTS' MANUAL.
due to ferric oxide— fe 0.050, 'Al 0.081, Mg 0.028, K 0.048,
Na 0.075.
Klaproth analyzed a specimen of chrysoprase which was
apple-green, and found in that of Silesia (Beitr, ii, 127),
Si 96.16, /J 0.08, fe 0.08, Ni 1.0, Ca 0.83, H 1.85 = 100. The
color was due to the presence of nickelous oxide.
Redtenbaeher has analyzed a brown-banded agate with the
following results : Si 98.91, 'fe 0.72, CaC 0.31 = 99.94. Some
agates which are remarkable for their colors are made use of
in the arts, such as the blue variety called sappliirine. Besides
the camelian, which is clear red, and the chrysoprase, which is
clear apple-green, mentioned above, the phrase, which is dark-
green, and the sardine-stone, which is dark-brown, are much
used in the arts. When agates are used for cameos, they must
have parallel layers of different colors. These are often pro-
duced artificially. The zone or ribbon agate is much used in
the arts. When the zones or strata are in parallel layers, and
the colors in great contrast, this variety is called onyx.
Jasper is the name given to impure, opaque-colored quartz.
The red jasper is colored by ferric oxide — ^the brownish or
ochre-yellow jasper IB colored by hydrated ferric oxide, which
when heated loses water and becomes red. It may also be
dark-green and brownish-green ; grayish blue and blackish or
brownish-black. Striped or ribbon jasper has the colors in
broad stripes ; Egyptian jasper in nodules, which are zoned in
brown and yellowish colors. Jasper admits of a high polish,
and is used for vases, boxes, etc. Porcelain jasper is nothing
but baked clay, and differs from true jasper in being, before
the blowpipe, fusible on the edges. Red porphyry^ or its
base, resembles jasper, but is also fusible on the edges, being
usually an impure feldspar. Jasper is used extensively in the
manufacture of Florentine mosaics.
In the variety of quartz called Silex or Flint, there is no
trace of crystallization to be distinguished, not even under the
microscope. The colors are not so bright as in chalcedony.
Lustre is barely glistening. Subvitreous. It breaks with a
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THE CHEMISTS' MANUAL. 309
deeply conchoidal fracture, and a sharp cutting edge. It con-
tains more impurities than the agate. There is usually one
per cent, or so of alumina and peroxide of iron, with one or
ti^o of water. The coloring matter of the common kinds is
mostly carbonaceous matter.
Earthy Ql aetz. — This variety is another distinct allotropic
modification. It is sometimes called Flowers of Silica, and is
almost entirely soluble in alkalies.
Sand is the name applied to quartz in a finely-divided state.
Sand may be of difierent kinds ; sometimes each grain is a
complete ciystal, sometimes it is rounded or concretionary, and
sometimes it appears to have no form, but made up of frag-
ments of crystals.
When the grains of sand are united by a cement, such as
ferric oxide or lime, large and round fragments are formed
called pudding-stones. If the fragments are angular, it is
called breccia. When the cement is silicic acid, it forms a
rock which is called Quabtzite. At Fontainebleau, the sands
contain sufficient lime to cause them to crystallize with the
form of calcite, even when they contain as much as 80-85^ of
silicic acid. Quartz is found all over the United States.
Quartz crystals are sometimes found of enormous size. A
group in the Museum of the University of Naples weighs
nearly half a ton. A crystal belonging to Sig. Rafelli, of
Milan, measures 3J ft. in length and 5 J in circumference, and
its weight is estimated at 870 lbs. Another in Paris 3 feet in
diameter and weighs 8 cwt. A group from Moose Mountain,
N. H., at Dartmouth College, weighs 147J lbs. and contains
48 crystals, four of them from 5 to 5 J inches in diameter, ten
from 4 to 4| inches. A crystal from Waterbury, Vt., is 2 ft.
long and 18 inches through, and weighs 176 lbs.
' OPAL
The composition of Opal is Si, the same as quartz, but it
contains a varying quantity of water, from 3 to 21;rA
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310 THE CHEMISTS' MANUAL.
The following are a few analyses of opal :
LOOAUTIBS.
1. Czerwenltsa (precions opal) .
2. Zimapan (fire opal)
8. FarOe (fire opal)
4. Schiffenberg (eetni-opal)
6. Oberkassel (wood opal)
6. WaltBch, Bohem. (hyalite). . .
7. Iceland (geyeerlte).
8. Bilin (tripoUte)
9. Lnnebeig (InftiBorial earth)
la Paris (Q. nectique^floatstoDe) .
Sl
90
98
8B.78
10
7.75
7.97
90JH)| 2.7S
93.01 I 4.1S
96.94 1 8.06
91JWI 6.76
87.66 8.89
8786
94.00
8.4S
5.00
Al.
0.09
1.86
0.12
1.04
2.
5^.
0.25
4.11
0.37
0.18
04
0.18 I 0.78
0.6
Ca.
0.49
Na.
Mg.i 8.
0.84 1 1.48! —
0.90 0.800.86' OSL
0.88 0.16 0.19 0.47' 0.81
1.09
0.76
I
0.80 —
Oba.
— 2.28
I
Analysis No. 1 by Elaproth (Beitr.. ii, 161).
" " 2 " " a. c, Iv, 156).
" " 8 " Forchhammer (Pojjg., zxrv, 381).
u ** 4 u wrightson (Ann. Ch. Pharm., llv, 858).
" » 6 " R. Brandes (Nogg. Oeb. Rh. We^tph., i, 888).
•* " 6 " Damoar (Boll. G. Fr., H, v, 168, 1848).
** " 7 " BlckeU (Ann. Ch. Pharm., 1m, 290).
ii u 3 i4 Banmann (Ramm. Mln. Ch., 188).
*» '* 9 '* Haostein and Schnltx (Ann. Ch. Pharm., zcy, 298)
" " 10 *• Bucholz (Leouk- Tawdi., vi, 5, 8).
Opal may have the following colors: white, yellow, red,
brown, green, and gray; the colors are generally pale. It
often has a very bright play of colors. Streak is white. Lustre
is vitreous, pearly, or resinous. Transparent, translucent,
opaque. Its ^hardness is from 5.6 to 6.5. Specific gravity =
1.9-2.3. It is infusible before the blowpipe, but loses water
and becomes opaque. In some varieties the transparency may
be made to reappear by plunging it into water.
When the colors are very dark, they arise from foreign ad-
mixtures; in such cases, sulphuric acid will turn it black,
owing to organic matter. Some yellow varieties, containing
oxide of iron, turn red. It is soluble in alkalies.
In a vacuum it loses its water and becomes entirely opaque.
The variety known as precious opal is generally found dis-
seminated in trachytic or porphyritic rocks. Such opals are
greatly prized as objects of ornament. The play of colors of
the opal seems to depend on the hydration of the silicic acid ;
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THE CHEMISTS' MANUAL.
311
for if an opal is heated it loses fire, but often regains it to a
less degree if plunged into water.
Precious opal occurs in porphyry at Czerwenitza, near
Kasha w, in Hungary ; also in Honduras. Fire opal occurs at
Zimapan, in Mexico. Common opal is abundant at Telke-
banya, in Hungary ; in Moravia, Bohemia, Iceland, the Giant's
Causeway, and the Hebrides. Hyalite occurs at Schemnitz,
in Hungary. Wood opal forms large trees in the pumice con-
glomerate of Saiba ; also in Hungary, Faroe, and Tasmania.
The Luneberg earth contains many species of infusoria, and
is 10 to 18 feet thick.
In the United States, hyalite occurs sparingly in New York,
rarely in North Carolina, and in Georgia and Florida. In Wash-
ington County, Georgia, good fire opals have been found.
BERYL.
The composition of Beryl is silica 66.8, alumina 19.1, glu-
cina 14.1 (iBcg + 1^ Sig.
There are two prominent groups of beryl depending on the
color, the color varying as chromium or iron is present. When
the color is bright emerald green, it is owing to the presence
of chromium and is called Emerald. All other specimens are
called Beryly and owe their color to iron.
The following are a few analyses :
1. Roflenbach, Beryl.
i. Fo8«Qm "
8. Go9hen, Mass., "
4. Uxiso^ Emerald
Si.
"Al.
Be.
'#«
Ca.
66.61
S0.71
11.46
1.88
0.28
67.00
19.64
12.66
0.68
0.18
66.97
17.28
12.93
2.03
~
66.50
15.75
12.60
1.00
-
Mg.
0.12
Mn. tr.
€r 0.80, Ca 0.86.
Analyfiifl No. 1, by HofmelBter (lb., Izxxl, 1).
*• No. 2, by Schcerer (Po>?g., xlix, 533).
No. 8, by Mallet (Am. J. Sci., II, xvil, ISO).
No. 4, by Klaproth (Beitr., Hi, 215).
The colors of beryl are very variable; they are emerald
green, pale green, passing into light blue, yellow and white.
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312 THE CHEMISTS' MANUAL.
Streak is white. Brittle. Lustre vitreous or resinous; the
opaque varieties, however, have no lustre. Double refraction
feeble ; axis negative. Hardness = 7.5-8. Specific gravity =
2.63-2.76. At a high temperature before the blowpipe the
edges become rounded. Fuses at 5.5 (Kobell).
The colored varieties become white when heated and loee
in weight, which would seem to indicate that the color is due
to organic matter. Glass with borax clear and colorless for
beryl, a fine green for ememld. Unacted upon by acids.
Emeralds are found in clay-slate near Muso, New Grenada.
A perfect hexagonal crystal from this localityj two inches long,
is in the cabinet of the Duke of Devonshire. Emeralds of less
beauty but of lai^e size are found in Siberia, Mount Zalora,
and in Upper Egypt. Transparent beryls are found in Sibe-
ria, Hindostan and Brazil. Beryls of gigantic size have been
found in New Hampshire and in Massachusetts. One beiyl
from Grafton, N. H., weighs 2.900 pounds ; it is 32 inches
through in one direction and 22 in another. It is also found
in Maine, Connecticut, and Pennsylvania.
GARNET.
Garnet is a unisilicate, of sesquioxide and protoxide bases,
having the general formula (iR2 + i-l^)2Si3 or (R3)2Si3+^2Si3-
The following are the varieties (with the exception of the
last) which blend together more or less completely, through
varieties containing ciombinations of the protoidde bases and
also of the sesquioxide bases :
A. Grossularite or Lime-alumina garnet.
B. Pyrope or Magnesia-aZumiiia garnet.
C. Almandite or Iron-alxtmina garnet. *
D. Spessartite or Manganese-alumina garnet.
E. Andradite or Lime-iron garnet,
F. Bredergite or Lime-m.agneMa-iron garnet.
G. Ouvarovite or Lime-chrome garnet.
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THE CHEMISTS' MANUAL. 313
The following are a few analyses of the different varieties :
1. Shidiaiika R., Orett
9. Wilnl, GrouyiariU
8. Pyrope
4. Vthlun, AbnandUe
6. Haddom, Ct., SpetsartUe. . . ,
a. Westmoreland, AndradUe,
7. Sola, Bredergite ,
8. Bieeersk, OuvarovUe
Ai^
4099 14.90
88J25 19M
41.35 28.85
89.66 19.66
85.83 1&06
87.66; —
86.73
87.11
F«.
10.04
7.88
81.86
2.78 25.88
5.88 2.44
9.94
80.68
14.68
S8.54
Mn.
0.60
2J»
1.80
8a96
4.70
0.08
2.40
16.00
12.44
1.10
Ca.
82.94
81.75
6.29, Cr4.17
26.74
21.TO
80.84, H8.01
AoalyBis No. 1, by Ivanoff (Kokeich. Mln. Ru6i>l., Hi, 79).
" Ko. 2, by Karsten (Karet. Arch. Mln.. Iv, 888).
** No. 8, by MoberK (J. pr. Cb., xllll, 122).
" No. 4, by Hle^lnger (Schw. J., xxl, 258).
** No. 6, by H. Seybert (Am. J. Sci., vi, 166, 1888).
*' No. 6, HieiDf^r (Jahrefi>b., ii, 101).
'' No. 7, Bredberg (Ak. H. Stockh., i. 68, 1829).
'' No. 8, Koaroaen (Vech. Min. Gee. St. Pet., 1841-65).
Color of garnet. may be red, brown, yellow, white, apple-
green, black; some of the red and green colors are often
bright. Streak is white. Transparent, translucent, opaque.
Fracture conchoidal or uneven. Garnet is generally found
crystallized, l)ut the crystals are very often distorted. Hard-
ness = 6.5-7.5. Specific gravity = 3.15-4.3. It is brittle and
sometimes friable ; when granular, massive ; very tough, when
compact ; cryptocrystalline.
In the reducing flame of the blowpipe most varieties fuse to
a light- brown or black gloss, and often becomes magnetic,
owing to the presence of iron. The dark-red varieties are
easily fusible to a magnetic scoria, as they contain more iron.
Some varieties are partially decomposed by acids ; all except
ouvarovite are after ignition decomposed by hydrochloric acid,
and generally with separation of gelatinous silica. Decom-
posed on fusion with alkaline carbonates.
Common garnet is found in Sweden and Norway, Almanr
dite or precious garnet is found in Ceylon, Peru, Brazil and
Greenland. Other varieties are found in Bohemia, Saxony,
Hungary, and in the Urals.
In the United States, in Maine, beautiful yellow crystals or
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314
THE CHEMISTS' MANUAL.
cinnamon stones (with idocrase) are found. Garnets are also
found in New Hampshire, Massachusetts, Connecticut, New
York, New Jersey, Pennsylvania, Delaware, and California;
also found in Canada and New Mexico.
LAPIS LAZULI.
The composition of Lapis Lazuli is silicate of soda, lime
and alumina, with a sulphide, probably, of iron and sodium.
The following are a few analyses :
Si. j Ja.
Ps.
Ca.
Na.
H. '
1. Orient
46.0 14.6
45.50 , 81.76
45.70 1 85.84
8.0
TV.
1.30
17.5
8.52
7.48
9.09
10.55
2.0 '
1L Bucharel
«. Andes
0.12 1
4.0, C10.0.
5.80, Fe 0.88, 01 0.42, S O.K.
- 4.82, S 8.96, K 1.85.
AnalyBla No. 1, by Klaproth (Beltr. i, 189).
*' No. 2, by Varrontrapp (Pogg., zUz, SIS),
" No. 8, by Schultz.
Color of lapis lazuli is azure-blue, violet-blue, red, green,
or colorless. Streak, same as color. Translucent, opaque.
Fracture uneven. Hardness, 5-5.6. Specific gravity, 2.38-2.4^5.
When heated in a closed tube, gives off moisture; the
variety from Chili glows with a beetle-green light, but the
color of the mineral remains blue on cooling. Fuses easily at
3 with intumescence, and gives a bluish bead. In acids it is
more or less easily attacked, and gelatinizes, evolving at the
same time a little HgS. The action of acids is frequently to
decolorize it ; sometimes it is not attacked by acids except
after calcination.
It is usually found in syenite or erylallien limestone, associ-
ated often with pyrite and mica in scales.
It is found in Siberia, of a dark-blue color ; also in Transyl-
vania, Persia, China, Thibet, Tartary, and near the Kio
Grande.
It is much used by jewelers, especially when it contains
pyrite. It was formerly used to make ultramarine, but is now
superseded by a clieap artificial preparation.
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316
ORTHOCLASE.
The oompofiition of orthoclase or feldspar is (jkg + | ii)^
Si3 + 6Si, or else with half the excess of silica basic = silica,
64.6; alumina, 18.5; potash, 16.9, with soda sometimes re-
placing part of the potash. The orthoclase of Carlsbad con-
tains rubidium.
There is a large number of varieties. The following are a
few analyses :
LocAunxB.
Si. Ai..
1. Lomnitz, Sile»U 06.76
5. Siberia | 6B.8S '
«. Radebeig, Sax. (wh.)' 65.94
4. Schemnitz | 64.00 .
6. Davidfloii Co., N. C. 65.a0
«. Zircon— Syenite . . . . | 66.08 '
7. Ischia 67.00
8. Lococlase | 65.40 I
U Lochwald 66.87
17.50
17.80
ao.4o
18.00
90.90
19.17
1&88
19.48
19.96
iht.
M8.
Ca.
1.76
1.95
o.ao
0.09
0.10
—
0.84
—
0.68
0.81
0.78
Trace
Trace
0.06
0.81
—
0.90
1.25
0.08
0.86
1.36
0.90
9.96
Trace
0.40
-
Na. , E. Zk.
— 19.0 —
— ! 9.81 18,06, Mn 0.19, Ca^.
— I 0.27 12.86-0.52, Li 0.71
— ; 0.79 15.48, Pb and Caa89
4.85 —
0.78
6.88
4.50
7.98
9.64
6.96
7.68
9.76
8.49
0.91
0.76
Analysis No. 1 by Rose (Scheerer*B J., Till, 948).
*» 9 " Ablch (Pojrg., li, 6% ; B. H. Ztg. Jahrg., 19).
•• " 8 " Jenzsch (Po^g., xcv, 804).
♦' 4 »» C. BiMjhof (Bischoi; Lehrb. Geol., li, 9171-2187).
** ♦^ 6 " P. A. Gentli (Keller and Tied, ill, 486).
" •* 6 •* Scheerer (Pogg., cviii, 496).
♦» M 7 *. G. Biechof (Lehrb. Geol., 1. c).
" •• 8 " Smith and Brush (Am. J. Sci.. H, xvi, 48).
*^ »( 0 it B>. Sandbeiger (OeoL Beschr. Baden, Carlsmhe, 181, 48).
The color of orthoclase is flesh-red, white-gray, greenish
or bright-green. Streak colorless. Transparent, translucent,
opaque. Fracture conchoidal, uneven. Lustre vitreous on
cleavage; surfiice sometimes pearly. Hardness, 6-6.5. Spe-
cific gravity, 2.44-2.62 ; mostly, 2.5-2.6.
Before the blowpipe, the colored varieties whiten. In tbin
scales it is fusible between 4 and 5 to white glass. With
borax it gives a transparent glass, and with salt of phosphorus
a silica skeleton. It is not acted on by acids. Orthoclase is
an essential constituent of many rocks. It is found in fine
crystals at Carlsbad and Elbogen in Bohemia ; also in Siberia,
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316 THE CHEMISTS' MANUAL.
Norway, Silesia, and Cornwall, etc. In the United States,
orthoelase is found in crystals in Maine, Connecticut, New
York, North Carolina, etc. Massive orthoelase is abundant
in the above places, as also in Mt. Desert, Me.; Eockport,
Mass. ; Norwich, Conn. Kaolin at Andover, Mass., and abun-
dantly in New Milford, Kent, and Cornwall, Conn., et<;.
Under the influence of atmospheric agencies the silicates
undergo a peculiar decomposition. When decomposition
has taken place in a rock, the elements of which are well
separated as large-grained granites and pegmarites, the quartz
is unaltered and the mica is not decomposed ; the feldspar or
orthoelase only has undergone decomposition. The mica,
however, undergoes certain changes, and takes on a silvery
look, which it did not have in the unaltered rock.
The products of decomposition may be separated as follows :
1. Kaolins or porcelain clays, resulting from the decom-
position of rocks in places.
2. Ordinary Clays, formed as sediments.
3. Clays, produced by chemical decomposition.
KAOLIN.
In the decomposition of orthoelase to form kaolin, it loses
ik -I- f Si. Part of the silica set free may go off* with more or
less of the potash, or may form opal, quartz, or siliceous sinter.
Kaolin is generally a simple hydrous silicate of alumina,
expressed by the formula ^ Sig + 2H = silica 46.3, alumina 39.8,
water 13.9. It is usually white, and somewhat plastic, not
very coherent, earthy, and without argillaceous odor when
breathed upon. It is easily separated from the accompanying
undecomposed materials by crushing and washing. It is very
much sought for, when free from iron, for the manufacture of
porcelain. For this purpose, it is indispensable that all the
mica should be washed out.
Brougniart analyzed a great number of kaolins used in the
arts, and arrived at the following limits :
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THE CHEMISTS* MANUAL. 317
Si 23-46; metallic oxides 0.5-1; ii 21-43; Ca, MgO-6;
alkalies 0-05 ; H 5-12 : residue not argillaceous 0-3.
ORDINARY CLAYS.
" Clays seem to have been formed from the product of decom-
position, carried off by water and deposited in beds in the
stratified formations. They do not "have any well-defined
character. When dry, they rapidly absorb water, which they
lose easily, and then contract and crack in every direction."
Lustre is somewhat pearly or waxy, to dull. Color white,
grayish, greenish, bluish, reddish. When taken from the
earth, they are sometimes somewhat translucent on the edges,
and have a soapy look and a slight lustre. When breathed
upon, they give a peculiar odor, called argillaceous, like the
smell of ground after a rain. Fracture is conchoidal. Hardly
plastic. Hardness = 1-2. Specific gravity = 1.8-2.4.
Tlie composition of clays is very variable, but they can all
be arranged around two types, represented by the following
compositions :
I. n.
Si 45—50 60—66
Al 84—38 18—25
H 9—16 9—15
These may be represented by the formulae :
Ai Sia + 4H ; Si 51.83, Al 35.36, H 12.46, and
M Sis + 3H ; Si 65.64, Al 22.54, H 4.82.
"These clays are generally plastic enough to allow their use
in moulding and for pottery. When they contain but little
iron, they can be used for fire-brick. They absorb water rap-
idly, and have a very distinct argillaceous odor, and are only
partially acted on by acids."
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THE CHEMISTS' MANUAL.
CHEMICAL CLAYS.
Under this head is considered the varieties known as fuller^a
earth or smectic clay.
Their composition is as follows :
LocAums.
Si.
'Ax..
F*.
Mo.
Ca.
H.
1. CiUejr (smectite) 61.21
2. Riegate (ftaUer's earth). . 1 58.00
8. StelDdOrfel (malthacite).| 50.17
12.25
10.00
10.06
2.07
9.76
8.15
4.80
1.25
2.18
aso
0.25
2r.80
24.00, K/r,NaCl 0.10
85.88
Analyeis No. 1 by Jordan (Pogg., Ixxvil, 691).
" 2 " Klaproth (Beitr., iv, 888).
" 8 '' O. Melsaner (L c).
Color is white, gray, and various shades of green to moun-
tain green and olive green, or brownish. Softens in water.
In the fracture their lustre is quite bright; they may even be
translucent on the edges. They do not absorb water as easily
as kaolin and ordinary days, but they unite with fets, even
when cold, and saponify. They are largely used for soap in the
countries where they are found.
Before the blowpipe the malthacite is inftwible; but the
smectite and the Kiegate fuller's earth, owing to the impurities
present, fuse rather easily. They are decomposed by hydro-
chloric acid.
Malthacite is found at Steindorfel, in Lausitz ; and Beraun,
in Bohemia. Smectite is found in Cilley, in Lower Styria.
TOPAZ.
The composition of Topaz is silicon 15.17, aluminium 29.58,
oxygen 34.67, fluorine 20.58 (A (JSIO2 + iSiFg)].
The following are a few analyses :
L00AUTIB8.
81. AiM
F.
L Anerbach, Saxony ... ,
2. Brazil (yellow)
& Finbo (pyrophyealite)
4. Trumbull, Conn ,
6. AltenbergCpycnlte)..,
84.24
8101
8486
86.80
85.00
ffr.46
66.88
W.74
66.96
4&00
14.99
1&06
15.09
17.85
16.6
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THE CHEMISTS' BIANUAL. 319
Audyses No. 1, 2. 8« by Berzellns (Schweifc J., zrl, 4S8 ; AibandL, Iv, 286).
AiuUysiB No. 4 by Forchhammer (J. pr. Cta., xxx, 400X
» 6 '' Bochobs (Bchw. J., i, 886>
The color of topaz may be blue, green, yellow, oraDge-
yellow, red, and colorless. The colors vary with the locality
and crystalliue ibrm, and appear to be generally owing to
organic substances. Streak colorless. Hardness = 8. Spe-
cific gravity = 3.4-3.65. Lustre vitreous. Pyro-electric.
Transparent, subtranslucent. Crystallizes as a right rhombic
prism of 124^7'.
It is infusible before the blowpipe. The yellow varieties,
when heated, take a pink or red color, and are then known as
burnt topaz. Fused in the open air with salt of phosphonis
gives the reaction for fluorine. Only paiily attacked by sul-
phuric acid. Fine topazes come from the Urals, near Katha-
rinenburg and Miask ; in Nertschinsk, beyond L. Baikal, in
the Adun-Tschilon Mountains, etc., one crystal from near the
Biver Urulga, now in the imperial cabinet at St. Petersburg,
being llf in. long, 6J in. broad, weighing 22J lbs. Av., and
magnificent also in its perfect transparency and wine-yellow
color. Found also in Kamschatka; Yilla Bica, in Brazil;
Aberdeenshire ; Altenberg, Norway ; Broddbo, Sweden. One
crystal found at this last place weighed 80 pounds.
In the United States it is found at Trumbull, Middletown,
and WiUimantic, Conn. ; also in North Carolina and Utah.
TALC.
Syn. — Steatite, soapstone, or potstone.
The composition of talc in some cases may be represented
by the formula (^Mg + ^H) = silica 62.8, magnesia 33.5,
water 3.7. In other cases (|Mg + ^H) §i + i^H = silica 62.0,
magnesia 33,1, water 4.9. The formula is commonly written,
MgeSis + 2H.
The following area few analyses :
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THE CHEMISTS' MANUAL.
L00AIJTIB8.
81.
^.
Fb.
Me.
H.
1. Chamounl (foliated talc)
% China f amliDat)
68JS6
«IS9
60.76
ei.75
69.60
0J»
0.40
1.96
ftSt
8.40
l.TO
4.60
86.40
81.tt
82.90
81.0B
99.16
0.04
0.18, Mn a»
4. Rhode Island rtalc)
9.66, Ca 1.00
8.88
6. Potton, Canada (steatite)
4.40, Ni ir.
Analysis No. 1 by Marignac (Blbl. Univ., 1844).
'" 8 '" J. Schneider (J. pr. Ch., xUii, 816).
" 8 " Beck (Mln. N. Y., 207>
44 *. 4 w DetejiBe (Rev. Scientlf., etc).
•• " 6 ** T. 8. Hunt (Rep. Q. Can., 18W, 464).
The color of talc may be green, white, red, and gray.
Streak white, or lighter than color. It is flexible, but not
elastic, which allows of its being distinguished from mica. Its
touch is unctuous and soapy, on account of the large quantity
of magnesia it contains. Lustre is pearly. Sectile in a high
degree. Hardness= 1-1.5. Specific gravity =2.565-2.8. Crys-
tallizes in a right rhombic prism of 120°.
Before the blowpipe it whitens, swells, and sometimes
decrepitates a little, fusing with difficulty on the edges. With
nitrate of cobalt it gives the reaction for magnesia. Not
decomposed by acids. Eensselaerite is decomposed, though,
by concentrated sulphuric acid.
Talc, or steatite, is a very common mineral, and constitutes
beds in some regions. Apple-green talc occurs in the Greiner
Mountain, in Saltzburg; in Saltzburg, Valais, Cornwall,
Scotland, Ireland, and Shetland Islands, etc.
In the United States, it is found in Maine, New Hampshire,
Massachusetts, Ehode Island, New York, Staten Island, New
Jersey, Pennsylvania, and North Carolina, Also in Canada.
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321
24. SILVER.
Tbe principal Silver nunerals are :
MlHUAI..
Baxd-
mas.
Sp.Ob.
FOBHITLA.
CoxpoamoR.
NatlTe silver
S.4--8
10.1-llJ
Ag (when pure)
AglOO.
Anudgam
3-8.5
10.6-14
A«%,
A«84.8: Hg65.2.
Aigcntlte
a-M
7.196-7.886
AgB
Ag 87.1; 812.9.
Pronstite
2-2.6
6.4S2-6l66
8AgS-fAfl,S,
Ag66.4; 819.4; A0l6Ji.
Pyiargyrite
%-%.6
6.7-6.9
8AgS-4-8b,S,
Ag 69.8; 8b 28.6; 817.7
Stephanite
Polybaslte
2-2.5
2-8
6JH9
6.214
6AgS+Sb.S«
9(Ag,€u)S+(8b,AB).8.
Ag68.6; 816.2; Sb 16.a
jAg647; CT19.8; 814.8;
' Sb9.7.
Cemrgjrite.
1-1.5
• 6.81-6.48
AgCl
Ag 76.8; CI 24.7.
Bromyiite
2-8
&8-6
AgBr
AgOT.4; Br 42.6.
Embolite
1—1.5
6.81-6.81
Ag(Cl,Br)
Agl
Age9J»; Br 1480; CI 16.42
lodyrite.
1-1.6
6.6-6.71
Ag46; 164.
NATIVE SILVER.
The composition of Native Silver is silver, with some copper,
gold, and sometimes platinum, antimony, bismuth, and mer-
cury. The varieties are :
1. Atjkifeeous. — Kuatelite contains 10-30 per cent, of sil-
ver. Color is white to pale brass-yellow.
The name ktistelite was given to an ore in Nevada. Hard-
ness = 2-2.5. Specific gravity = 11.32-13.10. Eichter found
in it silver, lead, and gold.
2. CuPEiFEBOUS. — Contains sometimes 10 per cent, of copper.
4. Antimonial. — John found in silver from Johanngeorgen-
stadt (Chem. Unt., i, 285) 1 per cent, of antimony, and traces
of copper and arsenic.
The color of native silver is white, but is subject to tarnish
and to become grayish-black. Streak silver-white. Ductile,
sectile. Lustre metallic. Hardness = 2.5-3. Specific grav-
ity = 10.1-11.1 ; when pure, 10.5.
21
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THE CHEMISTS* MANUAL.
Native sflver has all the characteristics of silver on charcoal;
fuses easily to a metallic globule. In the oxidizing flame
gives a brown coating. Soluble in nitric acid, and deposited
again by metallic copper, or precipitated by hydrochloric acid
as argentic chloride.
The mines of Konigsb^^, in Norway, have furnished mag-
nificent specimens of native silver. A mass weighing 60 lbs.
was obtained from the Himmelsfiirst mine, near Freiberg,
which had a gravity of 10.840. It is also found in the Harz,
Hungary, Dauphiny, and in some of the Cornish minea
Mexico and Peru have been the most productive countries in
silver. A Mexican specimen from Batopilas weighed, when
obtained, 400 lbs. ; and one from Southern Peru (mine of
Huantaya) weighed over 8 cwt.
In the United States, it is disseminated through the copper
mines at Michigan. It has .also been found in New York,
New Jersey, California, Nevada, and Idaho. Also found in
Canada.
ARGENTITE.
The composition of Argentite, often called vitreous silver
and silver glance, is sulphur 12.9, sUver 87.1 (AgS).
The following are a few analyses :
LooAunxs.
S.
A8.
1. Joachlmsthal
2. HlmmelBftlreL
15
14.7
14.46
86
86.8
8, JoftTrh^'nttthftl T.
77.68, Pb8.88, Cnl.58, PelA
AnalTses No. 1 and 3 by Klaproth (Beitr., i, 168).
AnalyaiB No. 8 by Lindaker (VogFa Min. Joach., 78).
Color, deep iron-black, with very little lustre on the natural
faces. The lustre is, however, bright on the fracture. Streak
same as color, and shining. Opaque. Perfectly sectile.
Hardness = 2-2.5. Specific gravity = 7.196-7.365.
Argentite melts when held in a flame, without the aid of a
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323
blowpipe. In the oxidizing flame it is roafited; in the reduc-
ing flame gives a metallic globule. Soluble in nitric acid.
It is found as amorphous masses disseminated in gangues,
which are usually limestones. It is a very valuable ore of
silver, and is found at Freiberg, Annaberg, Joachimsthal of
the Erzgebirge ; at Schemnitz and BIremnitz, in Hungary ; in
Norway, in the Urals, Cornwall, Bolivia, Peru, Chili,, and
Mexico.
Occurs in Nevada, at the Comstock lode, at diflferent mines,
along with stephanite, native gold, etc. ; in the vein at Gold
Hill ; common in the ores of Eeese Kiver ; probably the chief
ore of silver in the Cortez district ; in the Kearsarge district,
silver sprout vein.
PYRARGYRITE.
The composition of Pyrargyrite is sulphur lY.T, antimony
22.5, silver 59.8 (3AgS + Sb^Sg).
The following are a few analyses :
s.
SB.
A«.
1. Mexico
18.0
17.45
laei
81.8
88.16
88.85
60.8
2. Chili
6aoi
8. Andrcseberar. . . . « .
68.96, gangae 0.aa
ADalysis No. 1 by WOhler (Ann. d. Pbarm., xxvli, lOT).
" 8 " P. Field (Q. I. Ch. Soc.. adi, 18).
*' " 8 '' Bonedorif (Ak. H. Stockh., 1821, 888).
The color of pyrargyrite is black or very dark red. Streak
cochineal-red. Lustre metallic, adamantine. Translucent.
Opaque. Fracture oonchoidaL Hardness = 2-2.5. Specific
gravity = 5.7-5.9.
In a closed tube, gives a red sublimate of sulphide of anti-
mony ; in an open tube, sulphurous fumes are evolved, and a
white sublimate of oxide of antimony. On charcoal it fuses
and coats the coal. Heated for some time in the oxidizing
flame, or with soda in the reducing flame, a globule of silver is
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THE CHEMISTS' MANUAL.
obtained. Decomposed by nitric acid, with separation of snl-
phur and antimonious acid.
It is found at Andreasberg, in the Harz ; also in Saxony,
Hungary, Norway, in Spain and in Cornwall. In Mexico, it
is worked extensively as an ore of silver. It is also found in
Nevada, at Washoe, in Daney Mine ; and at Poorman lode,
Idaho, in masses sometimes of several hundredweight, along
with cyraxgyrite. It is a valuable ore of silver.
STEPHANITE.
The composition of Stephanite is (5AgS-f SbgSa) sulphur
16.2, antimony 15.3, and silver 68.5.
The following are two analyses :
LOCAUTUCIS.
S.
8b.
Ao.
Fb.
Cu.
1. Schemnitz
16.42
16.61
14.68
15.79
68.M
GS.88
0.14
0.S4
9. Androftsb^nr , . . .»»...- » . . . -
Analysis No. 1 by Roee (Pogg., xv, 474).
u gt* Kerl (B. U. Ztg., 1868, No. «).
The color and streak of Stephanite is black. Lustre metallic
Fracture uneven. Hardness = 2-2.5. Specific gravity =
6.269 (Pryebram).
In a close tube, it decrepitates and fuses, and after long heat-
ing gives a faint sublimate of sulphide of antimony. On
charcoal it decrepitates and fuses, giving the rose-colored coat-
ing of silver and antimony. After long treatment, a globule
of silver is obtained.
It is found at Freiburg, Saxony, Bohemia, Hungary, in the
Harz, Mexico, and Peru.
It is an abundant ore in !Nevada^ in the Comstock lode; it
is also found in Idaho. •
It is a valuable ore of silver.
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325
CERARGYRITE.
The composition of Cerargyrite (called also Horn Silver) is
chlorine 24.7, silver 75.3 (AgCl). The color is white, gray,
grayish-green, or colorless when perfectly pure. Streak color-
less and shining. Transparent, feebly translucent. Fracture
somewhat conchoidal. Sectile. Lustre resinous, passing into
adamantine. Hardness = 1-1.5. Specific gravity = 5.552 ;
5.31-5.43 (Domeyke).
In a closed tube fuses without decomposition. Fuses in a
flame of a candle. On charcoal, gives a globule of silver.
Insoluble in nitric acid, but soluble in anunonia.
The largest masses, particularly green, are found in Peru,
Chili and Mexico. It is also found in Norway, Brittany,
Nevada, California, Idaho and Arizona. It is mined as an ore
in South America.
125. SODIUM.
The principal Sodium minerals are :
MnnsRAL.
Habdnxas.
S?. Gb.
1.987
FORXXTIJL.
COMFOSXnON.
Soda Nitre....
3
NaS:
Na 86.6 ;"&' 63.6.
Thenardlte. . . .
2-8
2.6-2.7
Nas".
Na66.8;'^'43.7.
Mimbllite
1.6-2
1.481
NaS + lOH.
Na 19.8; 8 24.8; H56.9.
Qlaaberlte....
2.6-8
2.64-2.86
(|Na + 4Ca)8.
8 67.6: Ca20.1; Na2».4.
Halite
2.5
2.1-2.257
NaCl.
Na 38.3; 01 60.7.
Bvraz .»T
2.26
1-1.6
1.716
1.423
NaB, + lOH.
NaC + lOH.
Na 16.2 ; B 86.6 ; H 47.2.
Natron
Nal8.8: C26.7; H64.6.
SODA NITRE.
The composition of Soda Nitre is nitric acid 63.5, soda
36.5 (NaN). Hochstetter obtained from the Chilian minerals
(v. Leonh., 1846, 235) NaN 94.291, NaCl 1.990, KS 0.239,
k N 0.426, MgN 0.858, insoluble 0.203, H 1.993.
The color of soda nitre is white ; also reddish-brown, gray,
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and lemon-yellow. Lustre vitreous. Fracture indistinctly
conchoidal. Taste cooling. Crystals strongly double refract-
ing. Transparent, translucent, or opaque.
Deflagrates on charcoal ; colors the flame ydlow. Dissolves
in three parts of water at 60° F.
It is found in Peru in great abundance ; also in Chili and
India.
GLAUBERITE.
The composition of Glauberite is sulphate of soda 51.1,
sulphate of lime 48.9 (JNa + JCa)S.
The following are a few analyses : —
S.
Ca.
Na.
Cl.
Fs.
1. villa RubU
66.6
67.52
67.23
2C.2
20.37
20.68
28.8
21.87
21.83
0.81
8. Ischl
_
& Tarapaca
0.14
Analyetiji No. 1, by Brouffclart.
" No. 2, by V. Haaer (Ber. Ac. Wlcn).
'' No. 8, by Hayee (J. Nat H. Soc. Boat., iv, 498).
The color of glauberite is generally yellow, somewhat gray,
but when ^ is present it is red. Streak is white. Fracture
conchoidal ; brittle. Taste slightly saline. Hardness = 2.5-3.
Specific gravity 2.64-2.85.
Decrepitates and melts into a bead, which is transparent
when hot, but opaline when cold. Water separates the sul-
phates by dissolving the sulphate of soda. It is soluble in
hydrochloric acid.
Glauberite is found at Villa Eubia near Ocana in New
Castle, also at Ausse in Upper Austria, and in Bavaria. Near
Madrid a large mass of glauberite was found fourteen to fif-
teen miles thick and several leagues square.
HALITE.
The composition of Halite (common salt) is chlorine 6017,
sodium 39.3 (NaCl).
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The following are a few analyses :
327
NaCl.
MeCL.
CaS.
NaS.
MgS.
1 Vic, white
90.3
90.8
96.70
96.37
aS8
OJW
0.6
60
1.21
1.09
8.0
- Clay 0.2.
— " 1.9.
a. ** CTBT
8. " red
— " as.
4. " yellow
ft. " <?reen
a66
aeo
AoalyBee Na 1-6, by Berttaier (Ann. d. M., x, 260).
The colors of halite are very variable. When pure it is
colorless, but generally it is colored by some earthy or organic
matter. It may be gray, red, violet, blue or green. The
cause of these colors is not very well understood ; they may
be owing to traces of Ni, Co, Cu, or organic matter. Streak
is white. Lustre vitreous. Hardness = 2.5. Specific gravity
2.1-2.257 ; of pure crystals 2.135 (Hunt). Transparent, trans-
lucent. Fracture conchoidal. Kather brittle. It is soluble,
and has its own peculiar saline taste.
When heated it at first decrepitates and then melts; when
fused, colors the flame deep yellow.
Halite or common salt occurs in irregular beds in rocks of
various ages. At Durham, Northumberland, and Leicester-
shire, England, salt springs rise from the carboniferous series ; in
the Alps, some salt works are supplied from oolitic rocks. In
the United States, the brines of New York come from upper
Silurian; those of Ohio, Pennsylvania and Virginia mostly
from Devonian and subcarboniferous beds. Salt also occurs
as eflSorescences over the dry prairies and shallow ponds or
lakes of the Rocky Mountains and California. The principal
mines of Europe are at Wieliczka, in Poland ; at Hall, in the
Tyrol ; Stassfurt, in Prussian Saxony. Also in Bavaria, Salz-
berg, Transylvania, Upper Silesia, France, Valley of Cardona
and elsewhere in Spain, forming hills 300 to 400 feet high.
Also occurs, forming hills, near Lake Oromiah, the Caspian
Lake, etc. It is also found in Algeria, Abyssinia, India,
China and Russia. In the United States, it has been found in
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THE CHEMISTS' MANUAL.
Virginia, Oregon and Louisiana. Brine Bprings are very
numerous in the Middle and Western States. These springs
are worked at Salina and Syracuse, N. T. ; in the Kanawha
Valley, Va. ; Muskingum, Ohio; Michigan at Saginaw and
elsewhere, and in Kentucky.
a6. STRONTIUM.
The principal Strontium minerals are :
MiNBBAL.
Habdnsbb.
8p. Gb.
FOBMULA.
CoMToernox.
Celestlte
Strontianite
8-«.6
8.93-8.975
8.«6-8.718
SrS!
SiC.
Sr 56.4; '8 4^6.
SrTaS; C29.&
CELESTITE.
The compoBition of Celestite is sulphuric acid 43.B, strontia
56.4 (Sr§).
The following are a few analyses:
LOOAUTIBB.
's.
SB.
Ba.
Ca.
F.
1. Frankfltown, Pa
2r Sflntel. Hanover. ..-■.»-
42
43.74
42.94
43.95
66
56.18
56.01
66.26
0.86
0.64
0.81
0.04, CaC 0.02, H 0.06.
0.66, Si 0.11, H OJK.
8. Dehraelf.
4. Dombms^.
a08, JA 0.06, CaC 0.10, H, Bit., O.lSw
AnalysiB No. 1 by Klaproth.
*^ No8. 2, 8, and 4 by Stromeyer (Unters., 200).
The color of celestite is white, often faint bluish, and inclin-
ing to pearly. Streak is white. Hardness = 3-3.5. Specific
gravity = 3.92-3.975 ; 3.9593, crystals (Bendant) ; 3.973, fr.
Tharaud (Breith) ; 3.96 fr. Kingston (Hunt). Its lustre is
very bright, often pearly. Fracture is lamellar and sometimes
conchoidal.
Decrepitates and fuses, coloring the flame red. Insoluble
in acids.
It is found in Sicily, Spain, France, Hmigary, Hanover,
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Austria, Torkshire, and New Grenada. It is found about
Lake Huron, particularly about Strontian Island; and at
Kingston, Canada; also in Chamnont Bay, Schoharie, and
Lockport, N. T.
Celestite is used in the arts for making nitrate of strontia,
which produces the red color in fireworks.
STRONTIAN ITE.
The composition of Strontianite is carbonic acid 29.8, and
strontia 70.2 (SrC). The strontia is often replaced in a small
degree by lime.
The following are a few analyses :
Localities.
C.
SB.
Ca,
S^.
MX.
H.
1. Strontian
80.0
29.94
80.66
80.81
69.6
67.53
66.68
65.60
1.88
8.68
8.47
0.01
0.
0.09
71
05
9. Brftonmlorf, Saxony
& Strontian
0.07
4. •*
0.07
Analyfiia No. 1 by Klaproth (Beitr., 1. 270; ii, 84).
'* 2 " Stromeyer .Untew, i, 198).
•» ** 8 " Thomson (Min., 1, 106).
* '* 4 " Stromeyer (1. c).
The color of strontianite may be gray, white, yellow, brown-
ish, and pale green. Streak white. Hardness = 3.5-4. Spe-
cific gravity = 3.605-3.713. Lustre vitreous, inclining to
resinous on uneven faces of fracture. Transparent, translu-
cent. Fracture uneven. Brittle.
Before the blowpipe it swells, arboresces, and fuses on the
thin edges, and colors the flame red. With soda, on charcoal,
the pure mineral fuses to a clear glass, and is entirely absorbed
by the coal. Soluble in hydrochloric acid.
It is found at Strontian, in Argyleshire, in Yorkshire,
England ; in Ireland, Harz, Saxony, and Saltzburg.
In the United States, it occurs at Schoharie, N. T. ; at
Muscalonge Lake ; Chaumont Bay ; and Theresa, in Jefferson
County, New York.
Strontianite is used for pyrotechnics.
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orj. SULPHUR.
The composition of Native Sulphur is pure sulphur, which
is often contaminated with clay and bitumen.
When it is quite pure, it is of a yellow color, called sulphur-
yellow, sometimes having a greenish tint. It is sometimes of
a reddish color, which has been attributed to traces of selenium.
Streak is sulphur-yellow, reddish, or greenish. Hardness =
1.5-2.5. Specific gravity = 2.072, of crystals from Spain.
Lustre is resinous. Transparent, subtranslucent. Fracture
conchoidal, more or less perfect. Sectile. Crystallizes as a
right rhombic prism, 101° 40'.
Heated in a closed tube it fuses and volatilizes, leaving no
residue, if it is pure. In an open tube, it burns with a blue
flame, and gives off sulphurous ftimes. Becomes strongly
electrified by friction. Insoluble in water, and not acted on
by acids.
The great repositories of sulphur are either beds of gypsum
and the associated rocks, or the region of active or extinct
volcanoes. It occurs in the valley of Noto, and Mazzaro in
Sicily ; at Conil, near Cadiz, in Spain ; at Bex, in Switzerland.
Also at Hanover, Egypt, Tuscany, and in the Chilian Andes.
Sulphur is found near the Sulphur Springs of New York,
and in Virginia, in limited quantities ; also in North Caroh'na
and Nevada.
28. TIN.
The principal Tin minerals are :
MnnBRAL.
Hardkess.
Sp. Ge.
FORMVUk.
CoMPosinoir.
Casslterlte
Stannite
6-7
4
6.4—7.1
4.8-4.582
Sn.
2(Cn,Pe,Zn)S4-SnS,.
Sn 78.67, 0 21.33.
j8n*7.2,Cn99AFc,6jB,
1 zi7.6.SSi.fl.
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331
CASSITERITE.
The composition of Cassiterite is tin 78.67, oxygen 21.33 (Sn).
The following are a few analyses :
LOCAUTDES.
Sn.
tA.
^B.
Mk.
Si.
Ial.
1. Finbo
98.6
96.96
91.81
2.4
1.4 0.8
2.41 -
l.OS
0.84
6.48
«. Wlcklow, Ireland
8. Tipmiiii, BollTla (ftuA)
0.7B
Analysie No. 1 by BerseUnP (Afh., iv, 164).
" " 2 " Mallet (J. O. Soc., Dubl., It, 276).
•* " 8 '* Forbes (PhU. Mag., iv, xxx, 140>
Cassiterite is sometimes found colorless, in a few localities,
bnt generally its color is of every gradation, intermediate
between gray, white, and yellow. The color is generally in
bands not equally diffused. Streak white, grayish, or brown-
ish. Hardness = 6-7. Specific gravity = 6.4-7.1. Lustre is
adamantine, and crystals usually splendent. Nearly transpa-
rent, opaque. Fracture subconchoidal, uneven. Brittle. It
is infusible before the blowpipe. In the reducing flame it is
with difliculty reduced ; but if soda be added, the reduction is
facilitated. With borax it melts easily, and becomes the base
of an enamel. It is only slightly acted on by acids.
It occurs in remarkable crystals in Cornwall. It is found in
Ireland, Bohemia, Saxony, Greenland, Sweden, and in Fin-
land. In the East Indies it is found near Borneo, and in
Australia.
In Bolivia, S. A., at Oruro tin mines ; in Bolivia, and in
Mexico.
In the United States, found sparingly at Paris, Maine ; in
Massachusetts, New Hampshire, Yirginia, and California.
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29. ZINC.
The principal Zinc minerals are :
Habdhisb.
8p. Gb.
FOBMULA.
CoMFosmoir.
Zlnclte
4-4.6
8.6-4
8-2.6
6
»-2.6
6.48-5.7
8.9-4JI
2.086
4-4.6
8.6&-8.8
Zn
ZnS
ZnS+TH
Zn'c
ZnO+SZnH
Zn 80 86, 019.74.
Zn 67.0, S £8.0.
ZnSa8,'s 87.9, H 48.91
Zn 64.8, C 86Jt
Zn 75,8,0 18.6, H ILL
Sphalerite
GoBlarlte
Bmithsonite
Hydrozincite
ZINCITE.
The composition of Zincite is oxygen 19.Y4, zinc 80.26 (Zn).
The following are a few analyses :
VAXtntTIBS.
Zm.
Mk.
iiiN.
fa.
L Bed
98
88
98.48
99.47
fl
8. **
18
6.60 -
_ O.fiS
8. "
0.S6, scales Fe 0.44.
- ign.0.88.
4. YeUow
AnalysiB No. 1 by Bruce.
.1 u 2 '* Berlhier (Ann. d. M., iv, 488).
" " 3 " A. A. Hayes (Am. J. 8c!., xlvHl, 861).
ii 4 it y^ p ])j^]^e (Mining Mag., H, ii, 94, 1860).
Color of zincite is characteristic; it is a deep red, sometimes
orange-yellow. Streak orange-yellow. Translucent, subtrans-
lucent. Fracture subconchoidal. Brittle. Hardness =4-4. 5.
Specific gravity = 5.43-5.7 ; 5.684, orange-yellow crystals
(W. P. Blake). Bleaches if heated in a closed tube, but on
cooling resumes its natural color. In the reducing fiame it
gives metallic zinc, which volatilizes, oxidizes, and forms a
white ring. Gives a green color with nitrate of cobalt. Show^s
reaction for manganese. Soluble in acids.
It occurs with Franklinite at Stirling Hill and Mine HiD,
Sussex County, N. J.
It is used as an ore of zinc.
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SPHALERITE.
The composition of Sphalerite is sulphur 33, zinc 6Y (ZnS).
The following are a few analyses :
LocAunss.
8.
Zn.
Fb.
CD.
1, Praibram (flbrouB)
88.16
8S.23
83.04
82.10
88.67
61.40
67.46
65.89
64.23
44.67
2.29
1.18
1.82
18.26
1.60
9. New Jersey (white)
Trace.
a. Clauf^thal n)]ack)
0.79, On 0.18, Sb 0.68.
4 CoriBthia Balbe] (rh. crystal).
6. CbryBtophite G>lack)
Trace ; 8b and Pb 0.72, H 0^
0.26, Mn 2.66, Sn trace.
Asalysis No. 1 by LeOwe (Pogg., zxxviii, 161).
u »» 2 w T. H. Henry (Pbll. Mag., IV, i, 28).
" » 8 " C. Knhlemann (Ze. nat. Ver. Halle, vUl, 409).
" " 4 " Kersien (Popg., IxH, 189).
** '• 6 '' Heinichen (B. H. Ztg., zzii, 27).
The color of sphalerite is very variable ; it is rarely color-
less, but is generally honey-yellow, brown, black, red, and
green. When pure it is generally white or yellow. Streak
is white, reddish-brown. Hardness = 3.5-4. Specific grav-
ity = 3.9-4.2 ; 4.063, white, New Jersey. Lustre resinous to
adamantine. Transparent, translucent. Fracture conchoidal.
Brittle.
In the open tube it gives off sulphurous fumes, and generally
changes color. In the oxidizing flame it gives off sulphurous
fumes and often a cadmium coating. The roasting is long and
difficult, and after it, in the reducing flame, it gives a coat of
zinc, which is yellow when hot and white when cold. Soluble
in hydrochloric acid. With nitric acid, very little red vapor
is given off, but much sulphydric gas.
Occurs in Derbyshire, Cumberland, Cornwall, Transylvania,
Hungary, Harz ; Salila, in Sweden ; Ealiebozitz, in Bohemia,
etc. Abounds with the lead ores of Missouri, Wisconsin,
Iowa, and Illinois. Found in New York, Massachusetts, New
Hampshire, Maine, New Jersey, Pennsylvania, Michigan, and
Tennessee.
Sphalerite is one of »tbe most abundant ores of zinc.
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THE CHEMISTS* MANUAL.
SMITHSONITE.
The composition of SmithBonite is csarbonic add 35.2, oxide
of zinc 64.8 (ZnC).
The following are a few analyses :
LOCALTTIBS.
c.
Zn.
Fb.
Pb.
8i3
648
—
—
86.18
64.56
—
0.16
8a78
68.06
0.84
-
ZkC.
FbC.
MhC.
MoC.
96M
0.62
0.15
0.98
90.10
-
-
L74
98.74
-
1.60
0.39
1. Somereetehire
8. Altenbeig
8. Moresnet, Belgium.,
4 Alte^beig (w. cryet) .
6. Algiers...
6. AIl)ran8don, Mez . . . .
0.16
1.63, H IX.
CaC.
0.90, ioBol. 0.07.
j 8.80, PbC 0.44, As SJSO^
{ Fe 1.60, sand a45.
1.48, CnC 8.48.
AnalysiB Xa 1 by Smithson (Nicholson's J., Ti, 76).
u i» 9 .* HeidlDgsfeld (Bamm., 6th Soppl.)
" ** 8 " Schmidt (J. pr. Ch., ii, 867).
** 4 " H. RiBse (Verrh. nat Ver. Bonn., 86, 1886).
" " 6 " Marigny (Ann. d. M. V., xl, 678).
" " 6 " Genth (Am. J. Scl., xx, 119).
Color of smithsonite may be white, green, yellow, or brown*
Streak white. Haixlness = 5. Specific gtavity = 4-4.45 ;
4.45 (Levy) ; 4.42 (Haidinger). Lnstre vitreous, inclining to
pearly. Subtransparent, trandocent. Fracture uneven, im-
perfectly conchoidal. Brittle. Crystallizes in rhombohedra
of 107° 40'. In a closed tube, when heated, loses its carbonic
acid. Infusible. On charcoal, with soda, gives vapors which
are yellow while hot and white when cold. Soluble in hydro-
chloric acid with effervescence.
It is found at If ertschinsk in Siberia, at Dognatzka in Hun-
gary, Altenberg near Aix la Chapelle, at Ciguenza, in Soot-
land, and in Ireland.
In the United States it is found at Brookfield, Conn., in
Kew Jersey at Mine Hill, in Pennsylvania at Lancaster, in
Wisconsin, Minnesota, Missouri, and Arkansas.
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335
30. ZIRCONIUM.
The principai ZircoDium mineral is Zircon.
ZIRCON.
The compoeition of Zircon is zirconia 67, silica 38 (ZrSi).
The following are a few analyses :
Bi.
Zn.
'Sk
Ca.
H.
1. Ceylon
82.6
88.85
88.'ZO
64.6
84.81
66.80
1.6
1.56
0.67
0.88
1 Fredericksyarn ?)
8. Buncombe Co., N. C
0.41
AnalyeiB No. 1, by KJaproth (Beitr., v, 196).
" No. 2, by Hemieberg (J. pr. Ch., xxxvlll» 508).
" No. 8, by C. F. Chandler (Am. J. Sci., n, zxiy, 181).
Zircon may be colorless, pale yellow, brownish-yellow, yel-
lowish-green, reddish-brown, gray or blue. Streak colorless.
Hardne88=7.5. Specific gravity = 4.05-4.75. Lustre adaman-
tine. Transparent to subtranslucent and opaque. Fracture
conchoidal, brilliant. Double refraction strong, positive. It
is infiisible. The red varieties before the blowpipe lose their
color without losing their transparency, and the dark-colored
varieties become white. It is thought possible, therefore, that
the color is due to organic matter. Acids do not aflfect it, but
it is decomposed by fusion with alkaline carbonates.
It is found in the alluvial sands in Ceylon, in the gold
regions of the Ural near Miask, at Arendal in Norway, in
Transylvania, in Bohemia, Tyrol, France, Scotland, Ireland,
Greenland and Australia.
In North America it is found in Maine at Litchfield, in
Vermont, Connecticut, New York, New Jersey, Pennsylvania,
North Carolina and California.
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836
THE CHEMISTS' MANUAL.
COAL •
Coal is produced by the spontaneotis distillation of wood,
etc., after life has left the material acted on. The following is
the Coal Series.
Ligneous.
Peat.
Lignite.
COAL SERIES. ■
Bituminous.
Semi bituminous.
Anthbacitb.
GbAFHTTIC ANTHRACnTE.
w Graphite.
CUVBKRLAND.
^^^^""^
A = Bitaminous Coal, containing 50 fo of Volatile Matter.
B = Semi " " " 17-26J&
C = Inflammable Anthracite " 10-20%
D= Lehigh " '• a-10%
E = Newport Coal, " 0-7%
COAL MEASURES.
The following sections, general and local, as shown on
p. 337, will serve to give an idea of the mode of occurrence of
coal in the carboniferous rocks, and of the nature of the asso-
ciated strata. (J. S. Newberry, Johnson's Cjc, Article Coal.)
The Brier Hill coal is the best bituminous coal in this
country ; it has the following composition :
Bbier Hill Coal. ^
Water 1 to 8%.
VolatUe Combustible. . 30 to 33%.
Fixed Carbon 62 to 05%.
Ash 1.5 to 3%.
Sulphur 6 to 1%.
The Brazil coal is the best coal in Indiana.
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THE CHEMISTS' MANUAL. 337
CarbonifleroiiB Btrata— W. PennsylTaDia and Ohio.
Coal MeaPureH— N. Ohio.
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338
THE CHEMISTS' MANUAL.
8
8
o
o
QQ
O
1^
i
;3
Is
^ is
eg N^ S'
S
eg
w
a
I
1
U)
II
^
I-
I
S3
J
s s
S"' s
QQ tj
g"^ ^
C»1-l 1-1
o
•9
n
•»
«■
s* ^
gssis
o
n
n
e
«■
o
^1
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THE CHEMISTS' MANUAL.
339
If the empirical formula C34H48O22 b® assigned to wood,
founded on die analysis of oak, as shown above, the approxi-
mate empirical formula for peat will be C20H22O8 j for Bovey
lignite C27H2a07 ; for Wigan cannel C26H20O2 ; and for Welsh
anthracite C^qH i^O.
Kow, if a small amount of oxygen, such as might be sup-
plied by solution in water, be supposed to act upon the woody
tissue, each of these varieties of fuel might be formed by the
separation of marsh gas, carbonic oxide, and water in the
following proportions (Miller) :
Wood.
Peat.
Marsh GUI. AiS^^rlde. ^^^''
4C34H48022-I- ^02 = 4C20H22O8 + 24CH^ + 32CO2+ 4H2O
Wood. Lignite.
4C34H48O22+ 2O2 ='4C27H2807 + 8CH4 -h.20C02 +24H2O
Wood. OBnnel.
4C34H^8022+ 4O2 = 4C2«H2o02 + 8CH4 +24CO2+4OH2O
Wood. Anthracite.
4C34H48O22+ 5O2 = 2C40H16O + 24CH4 + 32CO2+ 32H2O.
ESTIMATED AREAS OF COAL IN PRINCIPAL COUNTRIES.
(Pepper.)
L00ALITIB8.
Sq. MiLse I Totai.
Coix Abba. Sq. Milm.
United States
British Provinces of North America
Great Britain
France
Belgium
Rhenish Prussian SaarbrUcker coal-field .
Westphalia
Bohemia ,
Saxony
Bpwn
Roflsia
200.000
y 8,964
Assuming a thickness of 20 feet of coal over 200,000 square miles, North
America would contain 4,000,000,000,000 tons of coal.
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THE CHEJflSTS' MANUAL.
ANALYSIS OF COALS.
ANTHRACITE.
LooALinxB.
c.
N.
Abh.
1. Piesberg, Hanover.
3. Pennsylvania .
4.
6.
87.96
91.14
90.45
92.59
84.98
1.97
2.08
2.43
2.63
2.45
0.61
2.45
1.61
1.15
0.92
1.22
9.31
6.81
4.67
2.25
10.20
Nos. 1 and 2 by Hilkenkamp and Kempner ; 3 by Renault ; 4 and 5 by
J. Percy.
BITUMINOUS.
CAKING COAL.
C.
H.
0.
N.
8.
Arh.
1. Zweckan
72.27
78.65
82.42
87.45
89.27
4.16
4.65
4.82
5.14
4.85
10.73
14.21
11.97
8.93
4.47
0.34
1.70
0.88
0.55
0.86
12.50
2 Northumberland
249
8. "
4. River-de-Gier
0.79
1.78
5. Alais
1.41
No. 1 by Stein ; 2 and 8 by Dick ; 4 and 5 by Regnault.
LIGNITE OR BROWN COAL.
LooixmBB.
C.
H.
O.
N.
S.
Ash.
Pax, France
Bovey
Irkutsk
70.49
66.31
47.46
5.59
5.63
4.56
18
22.86
33.02
93
0.57
2.86
4.99
2.27
14.95
No. 1 by Regnault ; 2 by Vaux ; 8 by Woskressensky.
NON-CAKING COAL.
LooALrrxBs.
1. S. Staflfordshire.
2.
3. Scotland
4. Mous, France . .
6. Valenciennes. . .
c.
72.18
76.40 I
80.98
82.95
90.54
H.
0.
4.32
17.11"
4.62
17.43"
5.21
10.91
5.42
10.93
3.66
2.70
N.
8.
Nos. 1 and 2 by Dick ; 3 by Rowney ; 4 and 5 by Marsilly.
Abh.
_
0.54
6.44
—
0.55
1.55
1.57
0.63
6.75
—
—
0.70
—
3.10
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THE CHEMISTS' MANUAL.
341
CANNEL COAL.
LOCAUTIBS.
C.
H.
O.
N.
8.
Ash.
1. Wigan
8407
80.07
78.06
5.71
5.53
5.80
7.82
8.10
3.12
2T12
1.85
1.50
2.22
2.40
2. *•
2 70
3 Tvneside
894
Na 1 by Regnault ; 2 by Vaux ; 3 by Taylor.
Note. — (") signifies that the mtrogen is included in the oxygen.
The following table is taken from " Report on Cods to Con-
gress, 1844," by Prof. W. E. Johnson :
LOCAUTIBS.
Pennsylvania (anthracite)
Maryland (free-burning bitum. coal)
Pennsylvania "
Vir^nia
Pittsburg (bituminous coal)
Gannelton, Ind
Pictou, Nova Scotia , .
SpBcmo
Gravity.
1.590-1.610
1.3-1.414
1.3-1.407
1.29-1.46
1.252
1.273
1.318
1.826
VoLun
COXBUST.
Matter.
3.84
15.80
17.01
86.63
36.76
33.99
27.83
25.97
FiXXD
Cabbok.
87.45
73 01
68.82
50.99
54.93
58.44
56.98
60.74
ASHANB
Clihksbs
7.37
9.74
13.35
10.74
7.07
497
13.39
12.51
ANALYSIS OF THE ASHES OF COAL.
(Percentage of ash in the coal was 1.99.)
(Bt Ebbmer.)
Silica 15.48
Alumina 5.28
Peroxide of iron 74.02
Lime 2.26
Magnesia. 0.26
Potash 0.53
Soda —
Sulphate of lime 2^17
Total 100.00
\
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342
THE CHEMISTS' MANUAL.
DURABILITY OF DIFFERENT WOODS.
Experiments on this subject have been made on various
kinds of wood, of which sticks 2 feet long and 1 J inches square
were cut, and driven into the ground until but 1^ inches
projected.
The results were as follows :
HIND OF WOOD.
OOHDinON AJTXB Si TBS.
OOHDITIOK ATTKB 6 TBAB8.
Chestnut oak
Canada chestnut oak
Oak from Memel.. .
Oak from Dantzic. .
Hard mahogany. . .
Soft mahogany
Cedar of I^bajion. .
Virginia cedar. . ^ . .
Teak wood
Fir
Pine
Virginia pine
Hard pine
Soft pine
Larch
English elm
Canadian elm
American ash
Acacia
Very good
Very much attacked. .
The same
The same
Good
Much attacked
Good
Very good.
The same
Much attacked.
Very much attacked .
Attacked
i^in. attacked, the)
rest good • )
fuch rotted
r j^ in. on the surface )
■I attacked ; had lost >■
(in weight )
Much rotted
The same
The same
{Good, except loss)
in weight )
{Most specimens moderately,
some very much attacked.
Very bad, rotten.
The same.
Exceedingly had.
Tolerable.
Verv bad, entirely rotten.
Tolerable.
fVery good, the same as when
first put in.
Somewhat soft, but good.
Much rotted.
The same.
The same.
j \ inch attacked, the rest tot
I erable.
Much rotted.
{} inch much, the rest a little
attacked.
Entirely rotten.
Rotten.
The same.
j I inch rotted, the rest as
( sound as when first put in.
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THE CHEMISTS' MANUAL.
343
PRODUCTS OBTAINED FROM DISTILUTION OF COAL
Qm, IDaminatiDg, etc.
Tar.
Ammonia Water.
Coke, for fliel.
Oils, 80^.
Naphtha
Pitch, TQjt-
TVmmiP J B«n«oJe \ J Used to make
B«n«>»«"l Toluol, n Aniline.
Naphtha. . . .Used for Varnishes.
Xylole Used for Small Poz.
FUBHIBHB8
carbolic Acid J , Used for Dlsto-
CresylicAcldf^ '«^*^*«-
Naphthalene Dyes, etc.
Chrysene No use as yet
Used for Boofing and Pavements.
Anthracene, ft%.
Dead Oil
The following is a list of the products from the distillation
of coal (Chandler*) :
I. COKE.
Per cent.
1. Carbon 90—95
2. Sulphide of iron (¥e^St) 8—10
3. Ash 3—15
II. AMMONIA WATER
1. Hjdio-ammonic carbonate KH4HCO3.
2. Ammonio liydroBulphate NH4HS.
8. Ammonic sulphocyanide NH4CNS.
4 Amnionic cyanide NH4CN.
6. Ammonic chloride NH4CI.
IIL TAR.
1. Hydrocarbons,
Formula. Sp. Or.
1. Benzol CgHg 860
a. Toluol, methyl-benaol.... C7H8 870
8. Ethyl-benzol CpH,o —
4 Xylol, di-methyl-benzol. . . Cg H , 0 867
5. Cumol, propyl-benzol C9H, « 870
6. Methylethyl-benzol CgH, , —
Boiling Points.
82"C.=: 179^6P.
HI' = 2S\\S
132'' = 269^6
140° =284**
163" = 807°.4
160° =320°
* Johnson's Cycl., Article Gas-Lighting.
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THE CHEMISTS' MANUAL.
Fonnnla.
7. Tii-methyl-benzol (pseu-
documol, mesetylene. C9 H^
8. Isobutyl-benzo] Cj qHi 4
9. Cyniol, methyl-propyl-
benzol C,oHi4
10. Di-ethjl-benzol C| 0H14
11. Di-methyl-ethylbensol
(ethyl-xylol) C,oH,4
12. Amyl-benzol C,,H|6
13. Methyl-amyl -benzol C , ^H 1 ,
14. Di-methyl-amyl-benzol
(amyl-xylol) C , 3H, 0
15. Phenylene Cg H4
16. Cinnamene, styrolene... Cg Hg
17. Naphthalene C, oH,
18. Diphenyl C,,H,o
19. Anthracene C, ^H, 0
20. Pypene C,6H,o
21. Chryeene CjgH,,
22. Benzerytherene —
24.
25.
26.
27.
28.
29.
dO.
81.
84
85.
And probably :
Quintane CgHi t
Sextane CeHi4
Other paraffines CbHsd+s
Qaintene, amylene CaHj 0
Sextene CgH,,
Other olifines CnHs.
Quintine, valerylene. .. . CsHg
Sextine, diallyl CgH, 0
Other acetylenes CaHte-s
Dipropyl (CjHOf
Dibutyl (C4H9)j
Diamyl (C5HM)t
DicaproyI (CgHia),
Other alcohol radicals. . . (CoHta+i)«
8p. Or.
.861
Mi
1.158
1.147
0.60
.678
.706
.741
.757
Bofling Points.
166''C
.= 880".8P.
159'
= 818" J8
178"
= 852".4
178"
= 852".4
184"
= 863".2
198"
= 879".4
218"
= 415".4
282"
= 449".6
91"
= 195".8
145"
= 293"
220"
= 428"
240"
= 464'
800"
= 572"
80"
= 86"
68"
= 154".4
85"
= 95"
68"
= 154".4
46"
= 114".8
58"
= 186".4
68"
= 154".4
106"
= 222".8
158"
= 816".4
«»"
= 895".6
2. Ak(^iol8,
1. Phenol, carbolic acid C^ Hg OH . . .
2. Creaol, cresylic acid C7 H, OH . . .
8. Phlorol, phlorylic acid. . Cg H9 OH . . .
4. Xylenol C, Hg OH . . .
5. Thymol C, oH, 3OH . . .
1.065
1.087
180" = 856"
200" =892'
195" = 888"
218".5 = 416"
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THE CHEMISTS' MANUAL.
Fonniila. Sp. Or.
6. Methyl-thymol CnHj^OH.... — ..
7. Ethyl-thymoL Ci,HmOH.... — ..
8. Amylthymol CicHjaOH — ..
8. Acid%.
1. Acetic H.O,H,0, .... 1.062 ..
2. Bntyric H.C4HTO, 9817..
8. Roflolic GsoHigOa — ..
4. Bnmolic ? .... — . .
345
BoUiDg Pointo.
117^2 = 243'
184° = 827^2
4. Baw^
1. Ammonia H;iN
2. Methylamine CHgN . .
8. Ethylamine C^ H7 N . ,
4 Diethylamine C4 HuN .,
6. Aniline, phenylamine. . . Cg H7 N . ,
6. Toliudine Cg Hg N .,
7. XyUdine CgHi.N..
8. Cumidine C,oH,3N .
9. Cynudine CnH,aN .
10. Pyridine C^ H^ N ..
11. Picoline Cg Ht N .
12. Lutidine C7 H9 N ..
18. CoUidine Cg HmN .
14. Panroline Cg H^^N .,
15. Coridine C.oH.^N .
16. Bubidine C,,H,7N .
17. Viridine C.^H^gN .
18. Pyrrol C4 H, N .
19. Lenooline, chinoline.
Cg H7 N
Gaa
—
—
Qas
... ^^
—.
.696
... W
= 16°.2
—
. . . 57°.5 = 135°.5
1.028
... 182°
= 359°.6
—
... 205°
= 4or
— .
... 215"
= 419°
. .952
... 225^
= 487°
—
... 260°
= 482°
.985
... 117**
= 242°.6
. .961
... 138°
= 271°.4
.946
... 154°
= 309°.2
.921
... 179"
= 854°.2
— .
... 188°
= 870°.4
— ,
... 2ir
= 411°.8
1.017
... 280°
= 446°
1.017
... 251°
= 488°.8
1.077
... 188°
= 871°.4
1.081
... 288°
= 460°.4
.... 273°.9 = 526°
20. Iridoline, lepidine. C, oHg N
21. Cryptidine, dispoline. ... C, iH| ^N
5. Pitch.
Oxidised bitaminous bodies, whose nature has not been accarately de-
termined.
IV. GAS.
1. iMwinanU,
FormnUL Density.
1. Vapors of pftimflAnee CnHm+t —
2. Propyl (C3H-), —
8. Other alcohol radicals (CaHsn+is) —
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346 THE CHEMISTS' MANUAL.
Formnla. Denelty.
4. Olefiant g80, ethene C^H^ .976
5. Propene CaHg 1.490
6. Butene C4Hg 1.940
7. Vapors of other olifinee CHta —
8. Acetylene C,H, 920
9. Vapors of other aoetjlenee (?). GdHsq-i —
10. Valelene (?) CnHto-^ —
11. Benzole CgHg 2.71
12. Vapors of toluol, xylol, etc CdHsb-^ —
13. Phenylene, etc. (?) CnHto-g —
14. Cuinamene, etc. (7) GJ9sb-io —
15. Naphthalene CioHe —
18. Diphenyl. etc (?) Ci,H,o —
17. Anthracene (?) C,4H,o —
18. Pyrene(?) CigH^o —
19. Chrysene(?) CigHi, —
20. Phenol, etc. (Alcohols) CnHsn-TOH —
21. Bases above mentioned — —
2. DUuerUs.
1. Hydrogen H 0691
2. Marsh-gas, methene OH^ 5594
8. Carbonic oxide CO 9727
3. ImpuriHes.
1. Sulphuretted hydrogen H,S 1.1747
2. Ammonic Bulphydrate NH4H8 —
8. Carbon di-sulphide CS, —
4. Carbon oxysulphide CSO —
5. Sulphurous oxide SO, —
6. Mercaptan, etc C,H,HS —
7. Sulphur bases, etc. — —
8. Ammonic sulpho-cyanide NH4CNS —
9. Ammonic cyanide NH4CN —
10. Ammonic mono-caorbontAe NH4HCO, —
11. Carbonic oxide CO, 1.5240
12. Nitrogen N 9760
13. Oxygen O 1.1026
14. Aqueous vapor (water) H,0 6201
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TBE CHEMISTS' MANUAL.
847
PRODUCTS OF COAL
(MOLBStrOBTH.)
'Pao'DXjon.
NllVOABTLl.
Caxseu
From.
To.
From.
To.
Cube feet of gad per ton of coal
Pounds of coiLe
9,500
1,500
70
80
10,000
1,540
90
120
11,500
715
710
15,000
720
Pounds of tar
720
Fuel requiied for retorts, about 20 lbs. per cwt.
AVERAGE EVAPORATING POWER.
(MOLBBWOBTH.)
1 lb. of coal evaporates 9 lbs. of water.*
1 lb. of coke " 9
1 lb. of slack *' 4
1 lb. of oak (dry) " 4) "
1 lb. of pine " 2i *'
Goal loses about one-third of its weight in coking, but increases in bulk
•one-tenth.
PEAT.
br 100 Parts.
0.
H.
OaivdN.
Afln.
H.O.
Sp. Ob.
€ondensed Peat
Wood
47.2
39.6
91.3
4.9
4.8
2.9
22.9
34.8
2.8
5.0
0.8
3.0
20.0
20.0
1.20
0.75
Anthracite
1.40
(Taken from a book on Peat and its Uses, by S. W. Johnson, A. M.)
HEATING POWER OF DIFFERENT KINDS OF FUEL
(JOH1780N.)
(The comparison is made in units of heat,f and refers to equal weights
of the materials experimented on.)
Air-dried wood 2800
" " peat 2500—3000
Perfectly dry wood 3600
* Feed-water supplied at 212^ F.
f The amount of heat that will raise the temperature of one gram of
water one degree of the Centigrade thermometer, is agreed upon as the
unit of heat.
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THE CHEMISTS' MANUAL.
Perfectlydry peat 8000— 4000
Air dry lignite or brown coal 8900—4200
Perfectly dry lignite or brown coal 4000—5000
Bituminous coal 8800—7000
Anthracite 7500
Wood charcoal 8800—7500
Coke 6500—7000
PETROLEUM.
Coaim
Conglomerate.
LOWKR Cakbomifbbous.
OIL CREEK
BBGION.
Coal.
Conglomerate.
LOWXB CABBONTrBBOUB.
Flag Bock.
\
J Flag Hock.
Shale.
r
^ RhAlA
— -
SandBtone No. 1. £]
Sandatone No. 1.
Shale.
Shale.
Satadatone No. 3.
^
{ ^
J
Shale.
Shale.
Sandatone No. 8.
<
^ Sandstone No. 8.
Shale.
Shale.
Sandstone No. 4.
i
k
Sandstone No. 4.
Portage.
Portage.
PETROLEUM CAVITY.
If a petroleum cavity be struck at (a), it often happens that
the gas rushes out with such a velocity that all the tools are
blown out of the shaft. If struck at (b), petroleum oil will
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THE CHEMISTS' MANUAL.
349
rush out, having a specific gravity at the bottom of the shaft
of 50° B. ; and at the top 29° B. One cavity has been known
to give 100,000 barrels of oil before dry. If the cavity is
struck at (c), water will first come out, then oil.
The town of Fredonia, N. Y., has been lighted by gas
obtained from a petroleum cavity for tlie last 40 years. Several
buildings at Erie, N. Y., are also lighted from gas wells.
Petroleum is found all the time by the decomposition of
animal and vegetable substances. The formation of petroleum
may be noticed around the edges of stagnant pools, etc.
PBODUCTS OF THE DISTILLATION OP CRUDE PETROLEUM.
(By C. p. Chandler.)
Price in Bulk, 14 cents per Oailon.
U
ll
GMes.
to
106° B.
106«B.
to
95'' B. )
Naxb.
^CymogcDO..
^Hhigolene.
to [
80^ B. )
to
«6 B.
^Gftflotene.
Napltba .
°B. )
to V
;(
ae^B. ')
to V
««B. J
hBendiie.
66° B.
60^ B. ' ) Keroeene or
to V Bellned
aB"* B. ) Petroleum.
Paraffin oil.,
Coke, gas, and loss
Total
Gratitt,
BiAxncB.
110°
100°
86° to 90°
UircoNDBifssD, Loss.
10
71° to 76° 1
4
68° to 66°
66
46°
19*
89°
10
too
^ Condensed by pnmp, made
by one firm only for an ice
machine, bolls at 82^ F.
( Condensed by ice and salt, )
■{ uBed as an amesthetic, >
i bolls at 86^ F. )
r Condensed In worm by cold
i water, used in "air gas
1 machines " and gas *' car-
L bonlzers."
For oil cloths, cleaning, etc ;
so-called " Safety oil,'*
" Danforth'soil,'' ''Amer-
ican Safety Gas," etc. ;
for adnlteratinK kerosene;
cleaning oil wells.
prioi pbb.
Qaxlok.
\"
60
$1 00
86cto.
to
18 cts.
For paints and Tarnishes
,...j
16cts.
to
12 cts.
aocts.
to
26 cts.
'SemUeolld when cold.1 i.Q„t„
ChiUed and pressed tol;^°^J»
separate paraffin, oU used f I
Ordinary oil for lamps..
7 cts. 12ctB.
to to
6 cts. 90 cts.
to
for lubricating J "^^^e.
20 cts.
to
16 cts.
80 cts.
to
40ct&
Digiti
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850
THE CHEMISTS* MANUAL.
SCALE OF HARDNESS.
(MOHB.)
1. Talc.— Laminated light-green variety. Easily Bcratclied by the nail.
2. QTF8U1C. — Crystallized variety. Not easily scratched by the nail. Doea
not scratch a copper coin.
3. Calcitb. — Transparent variety. Scratches and is scratched by a cop-
per coin.
4 Fluor. — Crystalline varietur. Not scratched by a copper coin. Does
not scratch glass.
5. APATITB.—-Transparent variety. Scratches glass with difficolty. Easily
scratched by the knif&
6. Orthoclasb. — White cleavable variety. Scratches glass easily. Not
easily scratched by the knife.
7. Quartz. — Transparent variety. Not scratched by knife. Yields with.
difficulty to the file.
8. Topaz. — ^Transparent variety. Harder than flint.
9. Safphirg.— Cleavable varietiea Harder than flint.
10. Diamond.— Harder than flint.
THE HARDNESS OF A FEW SUBSTANCES ARRANGED.
Diamond 10
Ruby 9
Cymophane 8.5
Topas 8
Spinel 8
Emerald 8
Garnet 7.5
Dicroite 7.5
Zircon 7
Peridote 7
Quartz 7
Tourmaline 7
Opal 6.6-^.5
Lapis Lazuli 6
Feldspar 6
Amphibole 5.5
Phosphorite 5
Fluorspar 4
Coelestine 8.5
Barytes 3.5
Carbonate Ldme 8.
Mica 2.5
Qypsum 3
Chlorite IJH
Talc 1
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lot(liioitt«ti[g.
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V,
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STOICHIOMETRICAL CALCULATIONS.
Example.* — What is the percentage composition of calcic
snlphate, CaS04? ,
Molecular weight = m.
Atomic . " of any constituent = a.
Number of atoms of that constituent = n.
Percentage amount = x.
m : an : : 100 : x.
By the formula^ the molecule contains of
Calcmm^ one atom (atomic weight, 40) 40
Sulphur, " " ^atomic weight, 32) 32
Oxygen^ four atoms (atomic weight, 16) ..... 64
Molecular weight of calcic sulphate 136
an X 100.
From above proportion, x =
m
Substituting in this formula, the quantity of
>x 1'
136
xl
136
136
Calcium in 100 parts is — r-^-^ — = 29.41.
Sulphur « « « « ^^ = 23.53.
Oxygen « « « '' ^^ ^^^^^ = 47.06
100.00
Example. — What is the fnrm/^i?^ of quartz, its molecular
weight being 60, and its percentage composition being :
Silicon 46.67
Oxygen 53.33
100.00
• All the following examples are from Barker's Chemistry.
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354 THE CHEMISTS' MANUAL.
The atomic weight of silicon is 28 ; hence the nnmber of
atoms of
Silicon would he ln = jr^ \
60 X 46.67
100 X 28
mx \ 60 X 53.33
= 1
Oxygen « « (;, =-^). ^^^ ^^_ ^
The molecular formula of quartz is therefore SiOa-
Example. — The molecular weight of argentic nitrate is 170;
it contains 63.53 per cent, of silver, and has but one atom of
silver in a molecule. Wlmt is the atomic weight of silver ?
w u mx lIQx 63.53 ^^^
^^ ^^^^ ^ = 100;^ ^^ -lOOTT- = ^08'
Hence the atomic weight of silver is 108.
Example. — Salt contains 39.32 per cent, of sodium, whose
atomic weight is 23. In a molecule of salt there is but one
atom of sodium. Wha;t is the molecular weight of salt t
_ , an X 100 23 X 1 X 100 ^^ ^
We have m = or kk-^ = 58.5.
The molecular weight of salt is therefore 58.5.
Again, ferric oxide contains three atoms of oxygen, or 30
percent. What is its molecular weiahtl v
By the formula li^^-i^ = 160.
Therefore 160 is the molecular weight.
Example. — Amraonic nitrate NH4NO3, breaks up under the
influence of heat into one molecule of nitrogen oxide, NjO,
and two molecules of (H20)2. How much nitrogen oxide in
100 parts of ammonic hydrate f
In formula using {a) to indicate the weight of the group,
and (n) the number of such group in the molecule
an X 100 ^ , • 44 X 1 X 100 ^^
= formula, we have ^7^ = 5o.
m 80
Hence ammonic nitrate yields 55 per cent, of nitrogen
oxide.
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THE CHEMISTS' MANUAL. 355
Example. — How much iodine may be obtained from
grams of potassic iodide (Kl), the atomic weight of iodine
being 127, and the molecular weight of potassic iodide 166 ?
By proportion. — ^As 166 parts of Kl give 127 of I, it is
obvious that the quantity given by 236 parts would be given
by the proportion :
166 : 236 :: 127 : y-
y = 180.5, Answer, 180.5 grams iodine.
^ ^ , mi xs . . . - ^ 127 X 236
By formula, y = ; substitutmg therefore y = —;-z —
= 180.5. Hence 236 grams potassic iodide yield 180.5 grams
iodine.
Example. — How much potassic iodide would be required
to yield 78 grams of iodine ?
z = — —; substituting z = — z-^= — = 102. Answer, 102
grams potassic iodide.
CALCULATION FROM EQUATIONS.
Examples. — Nitric acid is prepared by the action of sul-
phuric acid upon potassic nitrate (KNO3), according to the fol-
lowing equation :
KN03 + H2S04=HN03 + HKS04.
101 + 98 = 63 + 136.
Ptxlhlem IsU — 125 grams of nitre yield 77.97 grams of
HNO3, whose molecular weight is 63. Wkatjs the* moUcul^r
weight of potassic nitrate?
E^pffesenting By M, the molecular weight of substance
given, by W, the absolute weight of this substance given in
the problem, by m, the molecular weight of the substance re-
quired, and by w^ the absolute weight of this substance, then,
M : W : : m \ w\ from which the following formulas may
be derived :
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356 THE CHEMISTS' MANUAL.
In Problem Uf, m = 63, W equals 125, and w = 77.97;
hence M = ^nn^ = 1^1> Answer.
Problem 2d. — The molecular weight of nitre is 101, and
that of nitric acid is 63 ; how much nitre would be required to
yield 77.97 grams nitric acid ?
Here the quantities being represented as before, we liave:
^ 101 X 77.97 ,^^ .
W = -^ = 125,' Answer.
Problem 3d, — 125 grams of nitre yield 77.97 grams nitric
acid. The molecular weight of nitre is 101. What is the
molecular weight of WHO ^i
T .^.' Ki 101 X 77.97 ^^ .
In this problem, m = r^^ = 63, Answer.
Problem ^th. — The molecular weight of nitre is 101, and
that of HNO3 5s 63. How much HNO3 would 125 grams of
nitre yield ?
We have w = — t-^j — = 77.97 grams, Answer.
Problem 5th. — How much nitre is necessary to yield 36
grams of HNO3?
W = ; W = — ^TTy — = 57.7 grams, Answer.
Problem Qth. — How much sulphuric acid required in last
problem ?
Here M = 98 ; hence W = — ttq — = 56 grams, Answer.
Problem 7th. — How much hydropotassic sulphate will be
produQcd in Problem \st ?
M = 136 ; hence W = - y.„ — - =■ 77.7 grams. Answer.
The last three problems were solved by formula (2) ; the
following ones will be solved by fonnula (4). Formula (2)
and (4) are usually employed.
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THE CHEMISTS* MANUAL. 357
PrMem 8t/i. — How mnch nitric acid may be produced
from 500 grams of KNO3 ?
mW 63 X 600 ^^, ^^
w = -^- = — yqI — = 311.88 grams, Answer.
Problejii 9th. — How much H2SO4 will be required to de-
compose 500 grams of nitre ?
Here w = 98 ; hence w = — j^T — = 485.15 grams, Answer.
ProUera 10th. — How much hydropotassic sulphate would be
yielded by the decomposition of 500 grams of KNO3 by H2SO4 ?
In this problem, m = 136 ; hence w = — ryj = 673.27
grams, Answer.
VOLUME CALCULATIONS.
Problem 1st. — How touch carbonic dioxide is farmed by
combustion of 1 litre of carbonous oxide ?
As 4 volumes carbonous oxide yield 4 of carbonic dioxide,
1 volume will yield 1 volume, and 1 litre of coui*se 1 litre,
Answer.
Problem 2<^.^How much oxygen is needed to convert 2
litres carbonous oxide to carbonic dioxide?
4 volumes by the equation require 2 of oxygen ; hence 2
litres will require 1 litre of oxygen,^ Answer.
Problem Sd. — To form 100 cubic centimetres of carbonic
dioxide, how much carbonous oxide must be burned ?
4 volumes of carbonic dioxide require the combustion of
4" of carbonous oxide ; 100 cubic centimetres will require its
own volume therefore, or 100 cubic centimetres. Answer.
RELATION OF WEIGHT TO VOLUME.
Example Ist. — ^What volume is occupied by 6.08 grams of
oxygen gas ?
The weight of 1 litre of oxygen is 1.43 grams ; hence in 6.08
grams there will be as many litres as 1.43 is contained times
in 6.08 ; or 4.25 litres, Answer.
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358 THE CHEMISTS' MANUAL.
Example 2d. — What is the weight of 25 litres of nitrogen
gas?
1 litre of nitrogen gas weighs 1.2C grams ; 1.26 x 25 = 31.5 ;
hence 25 litres of nitrogen weigh 31.5 gi-ams, Answer.
SPECIFIC GRAVITIES.
^Example. — What is the specific gravity of chlorine gas ?
The molecular weight of chlorine is 71 ; its density there-
fore is -^ or 35.5. 35.5 x 0.0693 = 2.46 (0.0693 Sp. Gr. of
hydrogen gas). Chlorine gas is therefore 2.46 times heavier
than air.
Problem. — The specific gravity of ammonia gas is 0.589.
What is its molecular weight?
If the specific gravity is 0.589, its density is 0.589 -r- 0.0693,
or 8.5. Hence its molecular weight is 8.5 x 2 or 17.
GASEOUS VOLUMES FOR PRESSURE.
JSxample.—'Wlist is the true volume which 250 cubic centi-
metres of hydrogen measured at 742 millimetres would have, if
measured at 760 millimetres ?
If the volume of a gas under' the height H of the barometric
column be represented by V, and under any other height H' by
V, then V: V':: H' : H; whence VH = V'H' or V = ^-
Substituting in the foriimla
742
V'= 250 X w^ = 244 cubic centimetres, Answer.
E,cample. — A certain volume of nitrogen dioxide gas, under
a pressure of 781 millimetres, measured 542 cubic centimetres*
What is its true volume^ measured at 760 millimetres?
Substituting in formula
781
V'= 542 X ^=^ = 578.3 cubic centimetres, Answer.
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THE CHEMISTS' MANUAL. 359
GASEOUS VOLUMES FOR TEMPERATURE.
In general, if V represent the known volume, V the un-
known volume, and t the number of degrees the temperature
is raised or lowered, the formula for calculating an increase of
volume will be : •
V'= V X (1 X ^ X -003665).
For lower temperature :
V
^^ (1 + ^ X -003665)-
.Example. — ^A gas measures 15 cubic centimetres at 0^. What
unU it measure at 60° ?
Substituting in formula,
V'= 16 X (1 + 60 X -003665) = 18.298 cc. Answer.
Example. — What will a gas measure at 0°, which, at 100,
measures 40.1 cubic centimetres ?
401
^= (1 + 100 X -003665) = 29-345 cc. Answer.
A gas measures 560 cubic centimetres, at 15°. What will
it measure at 95° ?
Here ^°= 95 - 15 = 80. Hence,
V'= 660 X (1 + 80 X -003665) = 724.2 cc, Answer.
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360
TABLE* OF
W or w— Bolnble in water. A or a->inBolab1e in water, eolable in acids (Ha,HNOs
but Bolable in acids. W-I— «i>aring]7 Bolable in water and acids. A-I-iniiolable in
refer to notes, p. a63.
♦
i
1
1
1
1
&
S
a
5
1
i
1
1
1
W
. 1
1
1
Acetote...
W
W
w
w
w
a
w
w
w
Areeniate .
a
w
a
a
a
a
a
a
a
a
a
Arsenltc. . .
w
a
a
a
a
A
a
Benasoate..
w
w
w
w
w
a
w
Borate
a
w
a
a
w-a
a
a
a
a
a
Bromide...
w
W
w-a
w
w-a
w
w
w&i
w
w
w
Carbonate.
a
W
A
A
a
A
a
A
A
A
Cblorate...
w
w
W
w
w
w
w
w
w
w
Chloride. .
w
w...
W-A»o
W
W-A,.
W
W
W&I
W
W
W
Cliromate..
w
a
a
a
a
w-a
a
a
w
1
Citrate...
w
w
a
a
w-a
w
w
w
"^ 1
Cyanide...
w
w-a
a
w
a
a-1
a
a-i
Ferricy'de.
w
w
1
I !
Ferrocy*de
w
w-a
w
I
i
1
Fluoride. . .
w
W
w
a-i
w
w-a
A
w
w^
a
w-a
Formate ..
w
w
w
w
w
w
w
w
w
w
Hydroxide
A
W
A
W
a
a
W-A
A
A
a
a
Iodide
w
W
w-a
w
a
W
w
w
w
w
W
Malate....
w
w
w &a
w&a
Nitrate....
w
W
W
w,.
w
w
W
W
W
W
Oxalate.. . .
a
W
a
a
a
A
w-a
A
a
Oxide
A&I
an
W
a
W&A
A&I
A
A
Phosphate.
a
w...
w-^
w&a
a
WAA
a
a
a
Silicate....
A-I
a
a
■
a
a
a
Succinate..
w-a
w
w-a
w-a
w-a
w-a
Sulphate . .
w,..
"••?••
a
A
w
W
W-I
W&A»J
w,.
W
w.
Sulphide..
a
W
Aja.ie
W
a
A
W-A
a-i '
a
A
Tartrate...
w
w.
Ai.
a
a
w-a
a
w
w
w
w-«
* From Qualitative Analysis (Freaeniiib).
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361
SOLUBILITY.
and aqua regla). I or 1— insolable in water and acids. W-A— spariDgly Bolable in water,
water, sparingly soloble In acids. Capitals indicate common f abstances ; smaU flgares
i
J
§
1
w
w-a
w
w
1
1
w
1
as
w
1
i
.
1
www
1
W w
w
w
W
Acetate.
a a a
»
a
a
a
1
W , a
w
a
a
a
An>en!ate.
a a a
a
a
a
a
w 1 a
w
a
»
Arsenlte.
a a w
1
w
a
w-o
w w-a
w
BenzoAte.
a
a 1 w-a
«
a
W a
W
a
a
a
Borate.
w
w-1 w
w
a-i
w
w
w; a
W
w
w
Bromide.
a A A
A
a
»
A
W a
1
W
A
A
Carbonate.
www
w
w
w
w
W ▼
w
w
w
w
Chlorate.
W. W-I W
W
A-1
w..
W
W„ I
w
W
W
W
W
Chloride.
w A-i; w
w
a
w-a
a
W 1 a
1
w W-a
a
w
Chromatc.
W a 1 w
a
a
w-a
w
w
a
W ] a
w-a
Citrate.
, » . ^
a
W
a-i
W
1
w
w
a
Cyanide.
w ;w^
w
i
i
W
i
w
a
Fcrricy'de.
I
. ' w
a
i
W
1
w
w
a-i
F'rrocy'de.
w
a ^1
a
w-a
w-a
w
w
w
a-i
w
w
W-tt
Flaoride.
w
W-a w
w
w
w
w
w
w
w
w
w
w
Formate.
A
a A
a
a
W
W
w
a
a
a
Hydioxide.
w
W-A w
w
A
A
w
W
i
w
w
w
w
w
Iodide.
w
w-a
w
w
a
w-a
w
w-a
w
w
w
w
w^
Malate.
w ! W
w
w
W
W
w
W
W
W
w
w
Nitrate.
a
a
a
w-«
a
»
a
w
a
W
'
a
w
a
Oxalate.
A
A
A
A.o
A
A
A
w
a
W
w
a
A&l
A
Oxide.
a
a a.
a
a
a
a
w
a
W
a
a
a
a
Phosphate.
a
a
a
a
a
W
W| a ,
a
Silicate.
a
w
w
a
w
w
w
a
w
w-a
1
a
w-a
Succinate.
W
A-I
W
W
w-a
w„
W
w..
W-A
W
I
1
w
W
Salphatt.
A
A
a
a
a
A,,
A„
w
a.,
W
w
a,.
A..
A„
Sulphide.
w..
a
w-a
w-a
w-a
>age4
a
a
w
a
w
a
a
a
Tartrate.
Edite
dbjJ
Fohnsi
on. I
r. (18
TO.)
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362 THE CHEMISTS' MANUAL.
NOTES TO TABLE OF SOLUBILITY.
1. Aluminic ammonic sulphate, W.
2. •' potassic " W.
8. Ammonio arsenic chloride, W.
4. " platinic " W— I.
5. " sodic phosphate, W.
6. " magnesic " A.
7. " ferrous sulphate, W.
8. " cupric " W.
9. " potassic tartrate, W.
10. Antimonic hypochlorite, A
11. Bismuthic " A.
12. " basic nitrate, A.
16. Calcic sulphantimonate, W — A.
17. Chromic potassic sulphate, W.
18. Cobaltic sulphide. Easily soluble in HNOg ; very slowly in HCl.
19. Ferric potassic tartrate, W.
20. Man^nese dioxide. Soluble in HCl ; insoluble in HNO,.
21. Mercurius solubilis Hahnemanni, A.
22. Mercurammonic chloride, A.
28. Mercuric sulphate basic, A. ^
24. Mercuric sulphide. Insoluble in HCl and in HNO3 ; soluble in aqua regia.
25. Nickelic sulphide. (See Cobaltic Sulphide.)
26. Potassic platinic chloride, W — A.
27. Argentic sulphide. Only soluble in HNO,.
28. Tin sulphides. Soluble in hot HQ ; oxidized, not dissolved by HNO, ;
sublimed stannic sulphide only soluble in aqua regia.
29. Zincic sulphide. Easily soluble in HNO, ; with diiBculty in HCl.
80. Auric sulphide. Insoluble in HCl and in HNO, ; soluble in aqua regia.
31. Auric bromide, chloride, and cyanide, W; iodide, a.
32. Platinic sulphide. Insoluble in HQ ; slightly soluble in hot HNO3 ;
soluble in aqua regia.
33. Platinic bromide, chloride and cyanide, nitrate oxalate and sulphate, W ;
oxide, a ; iodide, i.
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THE CHEMISTS' MANUAL. 363
REDUCTION OF COMPOUNDS
FOUND TO CONSTITUENTS SOUGHT BY SIMPLE
MULTIPLICATION OR DIVISION.
{FresenittM QuantikUive Analysis, p. 606. 1871 Eidition.)
The following table only contains some of the more fre-
quently occnrring compounds; the formulflB preceded by !
give absolutely accurate results.
FOR INORGANIC ANALYSIS.
Carbonic Acid.
I Carbonate of lime x 0.44 = carbonic acid.
Chlo7*ine
Chloride of silver x 0.24724 = chlorine.
Copper.
Oxide of copper x 0.79849 = copper.
. Iron.
\li^^ 1 Sesquioxide of iron x 0.7 = 2 iron.
! Sesquioxide of iron x 0.9 = 2 protoxide of iron.
Lead.
Oxide of lead x 0.9283 = lead.
Magnesia.
Pyrophosphate of magnesia x 0.36036 = 2 magnesia.
Manganese,
Protosesquioxide of manganese x 0.72052 = 3 manganese.
" " " X 0.93013 = 3 protoxide of
manganese.
Pliosphoric Acid.
Pyrophosphate of magnesia x 0.6396 = phosphoric acid.
Phosphate of sesquioxide of uranium (2 Ur203,P05) x 0.1991
= phosphoric acid.
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864
THE CHEMISTS' MANUAL.
Potassa,
Chloride of potassium x 0.52445 = potassium.
Sulphate of potassa x 0.5408 = potassa.
Potassio-bichloride of platinum x 0.30507
or
Potassio-bichloride of platinum
^3T2m
Potassio-bichloride of platinum x 0.19272
or
Potassio-bichloride of platinum.
5.188.
Soda.
Cliloride of sodium x 0.5302 = soda.
Sulphate of soda x 0.43658 = soda.
Sulphur.
Sulphate of baryta x 0.13734 = sulphur.
Sulphuric Acid,
Sulphate of baryta x 0.34335 = sulphuric acid.
I
( Chloride ot
I potassium.
= Potassa.
FOR ORGANIC ANALYSIS.
Carhon.
Carbonic acid x 0.2727
or
Carbonic acid
3.666.
or
Carbonic acid x 3
11
Hydrogen,
Water x 0.11111
= Carbon.
or
Water
9
= Hydrogen.
Nitrogen.
Ammonio-bichloride of platinum x 0.06269 = nitrogen.
Platinum x 0.1415 = nitrogen.
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THE CHEMISTS' MANUAL.
365
TABLE
SHOWING THE AMOUNT OF CONSTITUENT SOUGHT FOR
ONE PART OF THE COMPOUND FOUND.
Eldubntb.
Antimony . .
Anenic.
Burinm.
Biamuth. . .
Boron
Bromine. .
Oadmiom.
Found.
of
oi
Alumina,
Al.O,.
Chloride of Ammonium,
NH.Cl.
{Ammonio-bicbloride
Platinum,
NH4Cl,PtCl,.
(Anunonio-bicbloride
Platinum, f
NH4Cl,Pta,.
Teroxide of Antimony,
SbO,.
Tersulpblde of Antimony,
SbS,.
AntimoniouB Acid,
SbO^.
Arsenioufl Acid,
AbO,.
Arsenic Acid,
AflO,.
Arsenic Acid,
AsO,.
Tersulpbide of Arsenic,
AsSg.
Tersulpbide of Arsenic.
AsS..
{Arseniate of Ammonia I
and Magnesia. )
2MgO,NH^O,AsO.+Aq.
( Arseniate of Ammonia )
( and Magnesia.
2MgO,NH^O, AsOb + Aq.
Baryta,
BaO.
Sulphate of Baryta,
BaO, SO,.
Carbonate of Baryta,
BaO,CO,.
Silico-fluoride of Barium,
BaFl,SiFl,.
Teroxide of Bismuth,
BiO,.
Boracic Acid,
BO,.
Bromide of Silver,
AgBr.
Oxide of Cadmium,
CdO.
Sought.
Aluminium,
Al,.
Ammonia,
" NH,.
Oxide of Ammonium.
NH,0.
Ammonia,
NH,.
Antimony,
Sb.
Antimony,
Sb.
Teroxide of Antimony,
SbO,.
Arsenic,
As.
Arsenic,
As.
Arsenious Acid,
AsO,.
Arsenious Acid,
AsO,.
Arsenic Acid,
AsOg.
Arsenic Acid,
AsO,.
Arsenious Acid,
AsO,.
Barium,
Ba.
Baryta,
BaO.
Baryta,
BaO.
Baryta,
BaO.
Bismuth,
Bi.
Boron,
B.
Brominf,
Br.
Cadmium,
Cd.
0.53398
0.31804
0.11644
0.07614
0.83662
0.71765
0.948a5
0.75758
0.65217
0.86087
0.80488
0.93496
0.60526
0.52105
0.89542
0.65665
0.77065
0.54839
0.80656
0.31429
0.42660
0.87500
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366
THE CHEMISTS' MANUAL.
FOUKD.
Sought.
1.
Oaloium. . . .
Ldme,
Calcium,
0.71429
CaO.
Ca.
Sulphate of Liine,
Lime,
0.41176
CrO,So,.
CaO.
Carbonat^ of lAme,
Lime,
0.50000
CrO,CO,.
CaO.
Carbon
Carbonic Acid.
Carbon,
0.27273
CX),.
C.
Carbonate of Lime,
Carbonic Acid,
0.44000
CaO.CO,.
Chloride of Silver,
CO..
Ohlorine. . . .
Chlorine,
0.24724
Ago.
a.
Chloride of Silver,
AgCl.
Sesqnioxide of Chromium,
Hydrochloric Add,
HCl.
Chromium,
0.25421
Ohrominm..
0.68619
Cr.O,
Cr,.
Seaquioxide of Chromium,
Chromic Add,
0.31381
Cr.O,.
2CrOs.
Chromate of Lead,
Chromic Add,
0.31062
PbO,CrO,.
CrOg.
Oobalt
Cobalt,
Protoxide of Cobalt,
1.27119
Co.
CoO.
j Sulphate of Protoxide of (
i Cobalt. (
Protoxide of Cobalt,
0.48387
CoO.SO,.
CoO.
( Sulphate of Cobalt + Sul- {
phate of Potassa, )
Protoxide of Cobalt,
0.18015
2(CoO,SO,) + (KO.SO,).
2CoO.
( Sulphate of Cobalt + Sul- )
( phate of Potassa, f
Cobalt,
0.14171
2(CoO,SO,) + 8(KO.SO,).
2Co.
Copper
Oxide of Copper,
CttO.
Copper,
0.79649
SubBulphide of Copper,
Cu.S.
Fluoride of Calcium,
"^r*
0.79649
Fluorine. . . .
Fluorine,
0.4S718
CaPl.
Fl.
Fluoride of Silicon,
Fluorine,
0.73077
SiFl,.
2F1.
B3rdrogen . .
Water,
HO.
Hydrogen,
Iodide,
0.11111
Iodine
Iodide of Silver,
0.54049
Agl.
I.
Protlodide of Polladium,
Iodine,
0.70556
Pdl.
I.
Iron
Sesquioxide of Iron,
Iron,
0.70000
Fe.O,.
2Fe.
Sesqnioxide of Iron,
Protoxide of Iron,
O.90O00
Fe«0,.
Sulphide of Iron,
2FeO.
Iron,
0.63686
FeS.
Fe.
Lead
Oxide of Lead,
Lead,
0.92825
PbO.
Pb.
Sulphate of Lead,
Lead,
0.68317
PbO,SO,.
Pb.
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THE CHEMISTS' MANUAL.
367
IiOftd.
Uthimn.
Hagnesiom.
aHwcGoxy .
Nickel.. .
Nitrogen..
Oxygen.
Fouin>.
Salphate of Lead,
PbO,SO,.
Salphideof Lead,
PbS.
Carbonate of Lithia,
LiO,CO,.
Sulphate of Lithia,
LiO,SO,.
Basic Phosphate of Lithia,
8LiO,POe.
Maprnesia,
MprO.
Sulphate of Magnesia,
MgO,SO,.
Pyrophosphate of Magnesia,
2MgO,POe.
Protoxide of Manganese,
MnO.
( Protoeesquioxide of Man-)
1 ffanese. J
MnO + Mn^O,.
Sesquioxide of Manganese,
MnJO..
j Sulphate of Protoxide of )
( Manganese, )
MnO,SO,.
Sulphide of Manganese,
Mn&
Sulphide of Manganese,
MnS.
Mercury,
Mercury,
Hg.
Subchloride of Mercury,
HgjCl.
Sulphide of Mercury,
HgS.
Protoxide of Nickel,
NiO.
iAmmonio - bichloride of )
Platinum, f
NH,Cl,PtCl,.
Platinum,
Pt.
Sulphate of Baryta.
BaO.SO..
Cyanide of Silver,
A^.N.
Cyanide of Silver,
AgC.N.
Alumina,
Al.O,.
Sought.
Oxide of Lead,
PbO.
Oxide of Lead,
PbO.
Lithia,
LiO.
Lithia,
LiO,
Lithia,
8LiO.
Magnesium,
Mg.
Magnesia,
MgO.
Magnesia,
2MgO.
Manganese,
Mn.
Manganese,
8Mn.
Manganese,
2Mn.
( Protoxide of Man- )
( ganese. )
MnO.
{Protoxide of Man- )
ganese. j
MnO.
Manganese,
lln.
Suboxide of Mercnrr,
Hf.O.
Oxide of Mercury,
HgO.
Mercuiy,
Mercury,
Hg.
Nickel,
Ni.
Nitrogen,
N.
Nitrogen,
N.
Nitric Acid,
NO,.
Cyanogen,
C,N.
Hydrocyanic Acid,
Oxy^ei,
0.73597
0.98805
0.40541
0.27278
0.88793
0.60030
0.88850
0.86086
0.77465
0.72052
0.69620
0.47020
0.81609
0.68218
1.04000
1.06000
0.84940
0.86207
0.78667
0.06071
0.14155
0.46852
0.19410
0.20156
0.46602
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368
THE CHEMISTS' MANUAL.
SUEXBNTB.
Oxygen..
Found.
Teroxide of Antimooy,
SbO„.
Arsenious Acid,
AsO,.
Arsenic Acid,
AsO^.
Baryta,
BaO.
Teroxide of Biomatb,
BiO,.
Oxide of Cadmium,
CiiO.
Sesquioxide of Chromium,
CroO..
Protoxide^of Cobalt,
CoO.
Oxide of Copper,
' CuO.
Protoxide of Iron,
FeO.
Sesquioxide of Iron,
Fe,0..
Oxide of Lead,
PbO.
Lime,
CaO.
Magnesia,
MffO.
Protoxide of Mansunese,
MnO.
fProtoseequioxide of Man- )
ganese, J
MnO + MjOg.
Sesquioxide of Manganese,
Mn,0.,.
Suboxide of Mercury,
Hg«0.
Oxide of Mercurv,
HgO.
Protoxide of Nickel,
NiO.
Potassa,
KO.
Silicic Acid,
SiO,.
Oxide of Silver,
Ago.
Soda,
NaO.
Strontia,
SrO.
Binoxide of Tin,
SnO,.
Water,
HO.
SOUGIZT.
Oxygen,
30.
Oxygen,
30.
Oxygen,
Oxygen,
O.
Oxygen,
Oxygen,
Oxygen,
O.
Oxygen,
O.
Oxygen,
Oxygen.
Oxygen,
O.
Oxygen,
0.
Oxygen,
O.
Oxygen,
O.
Oxygen,
40.
Oxygen,
Oxygen,
O.
Oxygen,
O.
Oxygen,
O.
Oxygen,
Oxygen,
O.
Oxygen,
O.
Oxygen,
O.
Oxygen,
Oxygen,
O.
0.16438
0.24242
0.34783
0.10458
0. 10345
O.12500
8.31381
0.21333
0.20151
0.22222
0.30000
0.07175
0.28571
0.39970
0.22535
0.27947
0.80380
0.03846
0.07407
0.21333
0.16982
0.58333
0.06898
0.25810
0.15459
0.21338
0.88889
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THE CBEMISrS MANUAL.
369
ELKXKNT8.
Oxygen.
Phoflphonui.
PotaHinm.
Silicon
Sihrer.
Sodium
Strontitm. .
Salphnr.
Pound.
1
Oxide of Zinc,
ZnO.
Phosphoric Acid,
PO..
Pyrophosphate of Magnesia,
2MgO,PO,.
j Phosphate of Sesquiox- )
( ide of Iron, J
Fe,0.,PO,.
Phosphate of Silver,
3AgO,PO.
{Phosphate of ^squioz-
ide of Uranium,
2Ura08,P05.
Priophosphate of Silver,
2AgO,PO..
Potassa,
KQ.
Salphate of Potassa,
KO,SO,.
Chloride of Potassium,
KCl.
Chloride of Potassium,
KCl.
iPotassio-hichloride
Platinum,
KCl,Pta,.
fPotassio-bichloride
Platinum,
KCl,PtCl,.
Silicic Acid,
SiO,.
Chloride of Silver,
AgCl.
Chloride of Silver,
AgCl.
Soda,
NaO.
Sulphate of Soda,
NaSO,.
Chloride of Sodium,
NaQ.
Chloride of Sodium,
NaCl.
Carbonate of Soda,
NaO,CO,.
Strontia,
SrO.
Sulphate of Strontia,
SrO,SO,.
Carbonate of Strontia,
SrO,CO..
Sulphate of Baryta,
BaO,SO,.
SoueHT.
Oxygen,
O.
Phosphorus,
Phosphoric Add,
PO..
Phosphoric Acid,
PO..
Phosphoric Acid,
PO..
Phosphoric Acid,
PO,.
Phosphoric Acid,
PO..
Potassium,
K.
Potassa,
KO.
Potassium,
K.
Potassa,
KO.
Potassa,
KO.
Chloride of Potassium,
KCl.
Silicon,
Si.
Silver,
Ag.
Oxide of Silver,
Ago.
Sodium,
Na.
Soda,
NaO.
Soda,
NaO.
Sodium,
Na.
Soda,
NaO.
Strontium,
Sr.
Strontia,
SrO.
Strontia,
SrO.
Sulphur,
0.19740
0.43662
0.63964
0.47020
0.16949
0.19910
0.23437
0.83018
0.54080
0.52445
0.63173
0.19272
0.30507
0.46C67
0.75276
0.80854
0.74190
0.43658
0.53022
0.39337
0.58487
0.84541
0.56403
0.70169
0.18734
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370
THE CHEMISTS' MANUAL.
£LKXEHT8.
FOUXD.
■ Bought.
1.
Sulphiir
Tin
Zinc
Tersulphide of Arsenic,
AflS,.
Sulphate of Baryta,
BaO,SO,.
Binoxide of Tin,
SnO,.
Binoxide of Tin,
SnO,.
Oxide of Zinc,
ZnO.
Sulphide of Zinc,
ZnS.
Sulphide of Zinc,
ZnS.
Sulphur,
Sulphuric Add,
^••
Sn.
Protoxide of Tin,
SnO.
Zinc,
Zn.
Oxide of Zinc,
ZnO.
Zinc,
Zn.
0.39024
0.84385
0.78667
0.80333
0.80260
0.88516
0.67031
WEIGHT OF SWEDISH FILTER- PAPER ASH.
Aom.
No. 1 (8 hi.) 0.0008 grmB.
No. 2 (4 in.) 0.0006 grms.
No. 3 (5 in.) 0.0008 grms.
At.kat.ikk.
.0.0010 grms.
.0.0020 grms.
.0.0080 grms.
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SCHEMES FOR THE
OF THE PST FREQUENTLY OCCURRING COIjPOUNDS.
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SCHEME
FOR THE QUANTITATIVE ANALYSIS OF AN
IRON ORE OR SLAG.
The ore is sampled and prepared as described under Assay
OF Iron Ores. The ore may contain NagO, KgO, CaO, MgO,
AI2O3, CrgOg, Fe, Mn, Zn, Ni, Co, Cu, As, SO3, P2O5, TiOg, SiOg,
V2O5, WO3, CO2, CI, Fe, H2O— Organic matter.
Make a qualitative examination for CrgOa, Cu, As, and Ti.
I. SPECIAL DETERMINATIONS.
In 1 gram deter-
mine H,0 by direct
weight.
(Free. Qnant. An.,
§36.)
In 1 ffram deter-
mine COg by direct
weight.
(Frefl.,§139, II.e.)
For special determinations of
KjO, Na.O, Cr,0, FeO, As, S,
SO,. TiO„ V.O,, W0„ CI, Fl—
Organic matter. (See Appen-
dix.)
II. MAIN ANALYSIS.
Pulverize five grams to impalpable powder and fuse
thoroughly in platinum crucible (Note 2) with 20 grams
Na2C03 (increase to 30 grams as the ore contains more Si02
and Silicates) and 2 grams NaNOg (increasing to 5 grams as
the ore contains more FeO, sulphides, or organic matter).
After cooling, treat crucible and fused mass in a small
beaker with boiling water, until the mass is thoroughly dis-
integrated (Note 3). If the solution has a decided green
color, digest with a little alcohol; filter and wash with hot
water.— (Fres., §160, 10, a, and Note 4.)
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374
THE CHEMISTS' MANUAL.
I. WATER SOLUTION.
It must be clear, but may be colored. It may contain AljOj,
ZnO, SiOg, SO3, P2O5, CrOg, AS2O5. Add excess of HCl ; evap-
orate to dryness (Note 6); moisten residue thoroughly with
HCl ; digest with hot water; filter, and wash with hot water.
RBsmuao.
FiLTBATB a.
Dilate to 600 c.c, and divide in three portions.
SiO„ etc.,
to be added
to and re-
fused with
Residue h.
Solution a^— 300 cc
(If the ore ooatains As,
see Note 6.) Put into a
large flaak (to be after-
wards com bined with solu-
tion (2') after determining
Cr,0,, if present (Note 7).
Solution a*
100 cc.
Add BaCl,,
and determine
SO. asBaSO^.
(Fres., §183
and Note 8.)
Solution a»
100 cc.
Add to solu-
tion <{*, as a lit-
tle Fe often en-
ters the water
solution.
II. INSOLUBLE RESIDUE.
It may contain CaO, Mgi^. AlgOg, MnO, ZnO, NiO, CoO, Fe,
As, CuO, P2O5, SIO2, TiOg (itod Pt from crucible). Dry the
residue; transfer it to a casserole; dry and bum the filter and
add its ashes; moisten with HjO; treat with HCl; evaporate
to dryness, and add HCl (Note 9). Warm and digest with hot
water, with occasional stirring. When dissolved to a clear
solution, filter and wash. — (Fres., § 140.)
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THE CHEMISTS' MANUAL. 375
RMmUB d.
It maj contain
8IO„ TIO„ and
other sob^tanceft.
Combine It with
BxaiDuaa. Wash
thoroughly with
hot water; i^ite
and weigh. Add
a little H,SO, +
NH.Fl, and heat
gently; then lig-
nite to constant
weight. Lo»s =
8i0«. FoM now
with bisulphate
of soda, about 10
Earns, addins; a
tie more near
the end. When
crucible is per-
fectly cold, dis-
folve in a large
amount of H,0
400 c.c: when
dissolved to clear
Uquld, dilute to
60u C.C., and di-
Tide. Give 100
C.c. to Solution
<!*, and 800 c.c to
SoLunoM d^.
weight deduct P,
lared from d*y and
TIO, is present, d(
SoLunoH <l. Bei
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376 THE CHEMISTS' MANUAL.
NOTES.
[The references to Fresenins's Quantitative Analysis refer
to London edition of 1865.]
Note 2. Prelbninary fusion, — Thoroughly mix the ore
and its fluxes on glazed paper ; put about a third of the mix-
ture in a two-ounce platinum crucible, and heat over a Bun-
sen burner until the greatest violence of the eflfervescence has
ceased. Then add and treat the rest in the same way. Finally,
heat strongly over a blast-lamp until mass is in complete and
quiet fusion.
Note 3. Removal of the fused mass. — Let crucible cool
until just below red-heat, and place it on a clean and dry iron
plate, whose lower part is immersed in cold water. When
crucible is cold enough to hold in hand, put it in a small
beaker in which it can lie on its side, and digest with boiling
water. Heat over a water-bath until fused mass all comes out
of crucible, or will come out by inverting it. Remove the
crucible ; wash it ; treat it in a small beaker with a little con-
centrated HCl to remove any adhering particles, and add this
to that of the insoluble BEsrouE (2).
Note 4. Beduction of H2Mn04. — If alcohol is added, heat
over a water-bath. If there was no bluish-green tint, no alco-
hol need be added.
Note 5. Separation cf Si02. — In order to render Si02
entirely insoluble, the evaporation should be carried to perfect
dryness, until no odors of HCl can be detected, and the mass
is hard and crumbly. As the residue is to be re-fused with
Residue J, the drying may be conducted at a temperature
somewhat higher than 100° C.
Note 6. Removal of As. — The As has already been mostly
or completely volatilized in the foregoing evaporation. If a
trace still remains, saturate with HjS gas, filter, wash, add
a little KCIO3 to filtrate, and boil until S is completely oxi-
dized.
Note 7. Determination of Cr203. — Add KHO in excess,
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THE CHEMISTS' MANUAL. 377
and boil with sufficient Br. Cool, add HNO3 almost to neutrali-
zation, acidulate with acetic aciJy add some sodium acetate in
excess and boil. Filter out hot the basic aluminium acetate
precipitate, wash with hot water, containing a little sodium
acetate. To filtrate, add baH^irn acetate in slight excess, filter
and wash. This last filtrate and the precipitate of alnrni-
mum acetate contain all the P2O5 and AlsOs in the w^ater
SOLUTION. The latter is to be dissolved in HCl, the former to
be freed from the excess of bariutn acetate with dilute H2SO4,
and both to be added to solution d^. Digest the precipitate
of BaCr04 and BaS04 ^^^ concentrated H2S04,boil, filter and
wash. Boil the filtrate with concentrated HCl and alcohol to
reduce CrH204 to Cr203 and precipitate the latter with (N H4)20.
(Fres.,§106, l,a.)
Note 8. Precipitation of BaS04. — Add 5 cubic centimetres
of BaCl2 at first to hot solution ; when precipitate settles, add
a little more to see if there is any H2SO4 present. Filter,
digest with HCl, wash with hot water.
Note 9. Separation of Si02. — ^Evaporate as in Note 5.
Then add HCl pretty freely and warm for some time before
adding any water, as the high heat may have produced anhy-
drous Fe203, forming an oxychloride which is very slow to
dissolve, especially in dilute acid. If acid added be too dilute,
concentrate by evaporation, add concentrated HCl, and digest
at a moderate heat.
Note 10. Determivation of TiO^' — Pass H2S gas into
BOLunoN d^ until it is saturated, boil for an /tour, occasion-
ally adding H2S water. Filter oS the precipitate and wash.
Add a few grains of KCIO3 to the filtrate and boil. Precipi-
tate the iron with (NH4)H0. Dissolve it in H2SO4 acid, wann
dilute, etc., and test volumetricaliy for Fe. (Note 18.) The
precipitate obtained by boiling with HgS was Ti02 + S. Dry,
ignite, and weigh = Ti02 in one gram of ore.
Note 11. Precipitation of the Basic Acetates, — Dilute the
solution to about one litre for each gram of the sesquioxide
present. It is sufficient to boil from ten to fifteen minutes for
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378 THE CHEMISTS' MANUAL.
the complete precipitation of the acetates. The filtering should
be done as quick as possible — ^through a rib-filter. Wash the
precipitate with boiling water, containing a little sodium
acetate. Should any hade acetate separate upon concen-
trating the filtrate, add some sodium acetate^ boil, filter, dis-
solve the precipitate in HCl and unite to the solution of the
main body.
Note 12, Deterfnination of P2O5. — The following method
may be employed for the removal of HCl. Add (NH4)H0
suddenly in large excess, filter, wash once, and redissolve in
boiling HNO3. The solution containing concentrated HNO3
in large excess, and no more than a trace of HCl must be
diluted to about 400 cubic centimetres and heated to boiling.
Then add solution of (H4N)2Mo04 in large excess; with most
ores 100 cubic centimetres are sufficient. Keep near the
boiling point several hours and set aside over night in a
warm place. Then decant on a rib-filter, if the supemated
liquid is colorless, and transfer precipitate to filter by means
of small portions of the filtrate. Rinse the beaker and wash
the precipitate once with the diluted precipitant. Heat the
filtrate and washings to boiling, add a little more of tlie preci-
pitant and set aside to determine if any more P2O5 will be
precipitated. Dissolve the precipitate back into the original
beaker by pouring dilute (NH4)H0 through the filter. [If a
red residue of oxide of iron remains undissolved, pour dilute
HNO3 upon it, allow it to pass into (NH4)H0 solution, acidu-
late with HNO3, boil, add more of the precipitant, and set aside
as before, filter and wash several times with the diluted pre-
cipitant, then dissolve the precipitate on the filter and adhering
to the beaker in as little dilute (NH4)H0 as possible into a
small beaker.] Add from one to ten cubic centimetres of
magnesia mixture (Fres., § 62, 6,) and continue as in (Fres.,
§134,l,b,a.).
Note 13. Washing of Fe^Oa.eHaO.— Wash this precipitate
by boiling up with water and decanting until the wash-water
shows very little alkaline reaction with litmus-paper and
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THE CHEMISTS' MANUAL. 379
pves very little precipitate with solution of AgNOa. Then
transfer to filter and wash thoroughly with boiling water.
Note 14. Precipitation of the Sulphides. — Add no more
of the yellow amnionic sulphide than is required, as an ex-
cess will re-dissolve a portion of the precipitate unless much
NH4CI be present. But an excess of the latter reagent will
interfere with the concentration necessary to precipitate the
MgO in filtrate h. Cork the flask tightly before setting it
aside.
Note 15. Separation of Co and Ni. — Should these constitu-
ents be present in considerable quantity, which very rarely
happens, it is better, as the nickelous sulphate is likely to be
converted into NiO by too strong ignition, to dissolve the sul-
phides in aqua-regia, neutralize with KHO, precipitate and
determine the CoO by Genth and Gibbs' process (Fres., § 160,
12, and § 111, 4), and in the filtrate determine the Ni as oxide.
Note 16. Determination of Mn. — (Gibbs' process. Am.
Jour. Sci., xliv, p. 216.) To the HCl solution, free from
HjSjadd (NH4)H0 in excess and solution of Na2HP04 in large
excess. Then add dilute HjSO^ or HCl until the white preci-
pitate re-dissolves, heat to boiling, and add (NH4)H0 in excess.
Digest near the boiling point about an hour, when the precipi-
tate, at first white and gelatinous, becomes crystalline in rose-
colored scales. Filter and wash with hot water. If tinged
red, re-dissolve the precipitate in dilute HCl and repeat the
process. On ignition the precipitate is converted into Mn2P207,
a nearly white powder.
If Zn is present, it must first be separated as ZnS, as in the
Scheme.
Note 17. Precipitation (f dissolved NiS. — A trace of NiS,
which is somewhat soluble in ammonic sulphide, is often car-
ried through into this filtrate, but is completely thrown down,
along with the excess of S, by this acidulation.
Note 18. Volumeti^ic determination of Fe. — ^Put solution
rf*, after treating it according to Note 10, into a flask holding
200 cubic centimetres, cool, dilute with cold water exactly up
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880
THE CHEMISTS' MANUAL.
to the mark, mix by pouring back and forth several times
from the flask to a beaker, draw out 100 cubic centimetres
with a pipette known to deliver that quantity, empty it into
a reducing bottle of 250 cubic centimetres capacity, and cover
over with a ground plate of glass. Put in each bottle a piece
of amalgamated Zn free from iron, and a strip of platinum-
foil resting on it, add about 10 cubic centimetres of concen-
trated H2SO4, cover, and set aside over night; when reduction
is complete the solution will be colorless. Then in each of
two flasks, holding about 75 cubic centimetres, introduce
exactly two grams of flne iron wire, add an excess of dilute
H2SO4, and immediately adjust corks (having bent tubes
attached, with their ends immersed in small beakers of warm
water) and heat until the complete solution of the wire. By
this water-valve arrangement the entrance of the air and oxida-
tion of the FeClj solution are avoided, and when the water
begins to run back, after the evolution of H has ceased, its
warmth prevents the too sudden reduction of the temperature
and condensation of the vapors in the flask. After cooling,
pour and wash out the contents of each flask with the beaker
of water attached, into a large beaker, add dilute H2SO4 in
excess, dilute to about one litre, and titrate successively and
rapidly with the solution of KaMn^Oe, to determine its strength.
Now pour and wash the contents of each reduction bottle
into a large beaker, add dilute H2SO4, dilute to about one litre
and titrate successively as before. (In a HCl solution all pos-
sible excess of that acid must be avoided, and the solution
must be diluted to two litres.) Better evaporate the solution
previous to reduction with an excess of H2SO4 and drive ofi*
HCl.
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THE CHEMISTS' MANUAL. 381
APPENDIX.
SPECIAL DETERMINATIONS.
Alkalies. — Mix 5 grams of ore, very finely pulverized,
with 30 grams of CaCOa and about 3 grams NH4CI; calcine
at a bright-red heat in platinum crucible for thirty to forty
minutes; boil the cinter mass with water for two to three
hours, replacing the loss from evaporation; filter and wash.
(Fres., § 140, II, b, 8.) Separate all CaO by addition of (NH^)
HO and (NH4)2C03 in excess, and then a few drops of awr
monic oxalate ; filter and wash. In the filtrate the alkalies
occur as chlorides, and may be separated in the usual way.
(Fres., §152,1, a.)
Chkomicm. — Fuse, etc., as in Main Analysis, obtain filtrate
a of the WATEB solution, and determine the Cr as in Note 7.
But if the ore be chromic iron, either employ Hunt's method
(Fres., § 160, 10 a, a) or that of Gibbs (Amer. Jour. Sci., xxxix,
p. 59), as follows : Fuse over blast-lamp with 10 to 15 parts
KF, HF; digest with H2SO4 until F is expelled; add hot H2O
filter, and in the filtrate separate CrjOg from AI2O3, and de-
termine it as in Note 7.
Ferrous oxide. — ^Digest one gram of ore, finely pulverized,
in a flask with concentrated HCl, passing a current of carbonic
anhydride. After complete decomposition, cool in carbonic
anhydride, and immediately titrate the solution of FeCl2, with-
out removing the insoluble residue, with K2Mn208 (Note 18).
The presence of organic matter and of the higher oxides of Mn
will interfere with the accuracy of the process.
For a special determination of the entire amount of Fe in
an ore, either this method may be employed, omitting the use
of carbonic anhydride, or the ore may be decomposed by fusion,
as in the Main Analysis, without the use of Na2N03, or
Clarke's method may be employed as follows (Am. Jour. Sci.,
xlv, 178): Thoroughly mix 1 gram of ore with 3 grams
of NaF or pure powdered cryolite, put in large platinum cru-
cible, and cover with 12 grams of coarsely-powdered KHSO4.
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382 THE CHEMISTS' MANUAL.
Fuse about twenty minutes; ciool; add concentrated H2SO4;
fiise to homogeneous paste ; cool, and dissolve in cold water.
When cryolite is used, a bulky white residue of CaS04 gener-
ally remains. Reduce the solution obtained by either of these
methods and titrate in usual way.
Aesenic. — Fuse 5 grams of ore as in Main Analysis and
obtain the water solution, in which the As will be present as
sodium arseniate. Add a little Na2S04 and HCl to slight acid
reaction ; boil a few minutes until all the AsjOs has been re-
duced to AS2O3 ; saturate the warm solution with HjS gas;
filter, and wash with HjS water. Dry filter and contents, and
oxidize them in a beaker with fuming HNO3. Dilute, warm
gently with a little KCIO3, to oxidize organic matter, and pro-
ceed as in Fres., § 127, 2.
StJLPHUEio ACID. — Boil 6 grams ore with 50 c.c. HCl H- 50
c.c. H2O -f- 10 C.C. alcohol. Filter and precipitate with BaCl2
in the filtrate. The diflference between the sulphuric an-
hydride thus found and the total found in the Main Analysis
will give the amount equivalent to the S actually existing in
the ore as metallic sulphide.
TriANio ACID. — The ore must be decomposed and the Ti02
brought into solution in cold water by Clarke's method, de-
scribed under Fereous Oxide. Then proceed as in Fres.,
§ 107 and § 235, and Note 10.
Vanadio and tunostic Acros. — These acids, which occur in
very small quantities in some European ores, may be separated
and detected as follows: Treat Residue a, obtained fi'om 10 to
20 grams of ore, like Residue c in the Scheme, until all Si02 is
expelled. Any residue which remains may contain AI2O3,
Ti02, V2O5, and WO3. Ignite and weigh, fuse it with NajCOs,
dissolve in HCl, boil, add NH4HO in excess, and saturate with
H2S gas. A red color will denote the presence of V2O5,
and a brown precipitate that of WO3 (Pogg. Anal., 21, 47.
H. Rose's Handb. d. Anal. Chem., ii, 764).
Chlorine. — Proceed as in Fres., § 167, 3, c.
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THE CHEMISTS' MANUAL.
883
Fluokine. — ^Proceed as in Fres., § 166, 5, a, or if the ore
contains apatite, as in Fres., § 166, 6.
Oboanig matteb. — Eoast 1 gram in an open crucible, at a
red heat, and (when the protoxide of iron, the higher oxides of
manganese, sulphur, and arsenic are absent) the loss dimin-
ished by the amounts of carbonic anhydride and HjO present,
will be approximately equivalent to the amount of organic
matter.
ANALYSIS OF A.
Bbown Hkxatitb OB
LUfONITB.
Ferric oxide. 90.05
Ferrous oxide.
Manganous oxide. . .0.88
Alumina. 0.14
Lime 0.06
Magnesia 0.20
Potash.
Silica 0.92
Titanic acid.
Carbonic acid.
Phosphoric acid. 0.09
Oigaole matter.
Percentage of Iron, ^M
HmATiTB OB Sfboulab
Obb.
Ferric oxide 96.16
Ferrous oxide.
Manganous oxide. .0.24
Alumina 0.06
lime 0.07
Magnesia.
Potash.
Soda.
SUica 5.66
Carbonic add.
Phosphoric add )
Sulphuric add >• traces.
Iron pyrites )
Water iliyg««»Pi<5
^*^' } combined.
Organic sabstance.
Percen tage of Iron, 69.10
ILaonbtio Iboh Obb.
Ferric oxide 62.20
Ferrous oxide 17.82
Manganous oxide. . .0.14
Zinc oxide.
Alumina 3.81
Lime 5.52
Magnesia 1.82
Potash and Soda.. . .0.10
Silica 9.66
Carbonic acid.
Phosphoric acid 0.10
Sulphuric acid.
Iron pyrites 0.17
T»r„. _ j combined. . .0.28
^*^'^1hygroscopic.0.84
Insoluble in add.
Percentage of Iron.57 ,01
In the foregoing analysis, it may be seen that (for instance)
the magnesia in the given analysis of hematite does not exist,
neither the potash in the limonite or the zinc oxide in the
magnetite ; but in some ores these substances are present, in an
appreciable amount. The MAONEirrE of this state most always,
if not always, contains Ti02*
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384
THE CHEMISTS' MANUAL.
CAST OR PIG IRON ANALYSIS.
Total carbon : Rogers' process (see J. Chem. Soc., LoDdon,
May 1869). To 2.5 grams borings or filings add 50 c.c. of a
solution of CUSO4 (1 salt to 5H2O) ; heat gently for ten min-
utes. Fe dissolves, and Cu separates ; carbon remains. Now
add 20 C.C. of CuCla (1 to 2) + 50 c.c. strong HCl, and heat for
some time nearly to boiling until Cu dissolves; filter through
broken glass and asbestos; veash tlioroughly with boiling
water, and finally wash with small jet into flask (c), and add
three grams CrOs, and arrange apparatus as shown in the
Figure. Tlien add 30 c.c. of strong H2SO4, little at a time,
shaking constantly, closing cock of funnel tube each time.
Finally heat gently to boiling, not allowing more than three
bubbles of gas to pass per second. Boil one minute; attach
guard-tube {a)' and aspirator to guard tube (b) and draw air (3
bubbles per second). Increase weight of tube (y)=C02, etc.
AFPABATUS USED.
80.
and
H.80.
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THE CHEMISTS' MANUAL. 385
GRAPHITE AND SILICON.
Eggertz process. (Chem. News, Am. Eeprint, vol. iv,
p. 25.) Add 5 grains of fine borings to 10 cubic centimetres
of H2SO4 -f- 50 cubic centimetres HjO ; boil one-half hour,
evaporate one-third and cool. Add 10 cubic centimetres
HNO3, l^^ one-quarter hour, evaporate on water-bath until no
vapors pass oflf, to dry or nearly dryness, add 75 cubic centi-
metres HjO -I- 13 cubic centimetres HCl and boil one-quarter
hour. Add more HCl if anything remains undissolved.
(Filter through a filter washed with acid, dried and weighed.)
Wash first with cold water until no more iron appears in wash-
ings, then with boiling water -f 5 per cent HNO3. ^U ^^
100° C. and weigh. Ignite strongly and weigh again. Zos8
= GRAPHriE. Expel Si02 with NH^F. Loits = SiOj.
Note. — Si02 dried at 100° C. contains 6 per cent HgO,
which goes off on ignition, and must be deducted froj/i
ORAPHrrE after SiO^ is determined.
SULPHUR.
By Eggertz process. (Chem. News, Am. Reprint, vol. iii,
p. 1.) Dissolve 10 grams KCIO3 in 200 cubic centimeters HgO
and add 5 grams of borings ; boil and add 60 cubic centimetres
HCl (little by little), boil until Fe dissolves. Evaporate, dry
on bath to ensure oxidation of sulphur. Thorough dryness
not necessary, as SIO2 does not interfere in acid solutions.
Now add 10 cubic centimetres HCl + 30 cubic centimetres
HjO and leave on bath until all Fe2Clfi is dissolved. Then
add 20 cubic centimetres H2O and wash thoroughly. Add 2-
cubic centimetres saturated solution of BaCl2 (enough for
H2SO4 from 0.100 S) ; after cooling, add 5 cubic centimetres
(NH4)H0, stir and leave for twenty-four hours. Filter and
wash by decantation with cold water, two or three times, and
then with hot water. If precipitate shows iron after ignition,
treat with HCl, etc.
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386 THE CHEMISTS' MANUAL.
PHOSPHORUS.
Dissolve as in sulphur determination. Dry at 140° C,
some anhydrous FejOg will be left with SiOj. Fuse with a
little KaSjOy (bisulphate of potash), soften with H2SO4, and
dissolve in water. Filter out Si02 and determine it as a check
on regular determination. Add filtrate to main one, dilute
largely and precipitate sesquioxides + P2O5 by large excess of
(NH4)H0 cold, wash by decantation two or three times with
cold water, and then on a large filter. Dissolve on the filter
with' hot dilute HNO3. Boil out any CI remaining in the
solution, and precipitate P2O5, as in Kote 12 of Iron Ore
Scheme.
IRON.
Dissolve 0.200 grams in H2SO4, reduce with Zn and R, and
titrate with KMn04; when oxidation is nearly complete, use
solution one-tenth strength. Note 18, Iron Ore Scheme.
BASES OF GROUPS II. Ill AND IV.
Dissolve 10 or 20 grams in HCl. Extract Si02, and proceed
as in Iron Ore Analysis. It is better to determine aluminum
separately.
ANALYSIS OF FOREIGN MALLEABLE IRON.
/t SWXDISH. ^
Iron 99.803 99.220 — 98.78
Carbon 0.054 0.087— 0.84
Silicon 0.028 0.066— 0.12
Sulphur* 0.055 0.632— ....
Phoaphorus Trace 0.0O5— ....
Manganese Trace — 0.C5
Copper — 0.07
Arsenic Trace— 0.08
Total, 100.00 100.00 99.88
* Sulphur determinations are probab'y too hi^rh.
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THE CHEMISTS' MANUAL.
887
ANALYSIS OF CAST IRON.
Ore need
FoelaBed]
CbAf-
coaL
Fre-
seniiu.
netk.
Char-
ooaL
Henry.
Clay Iron Ore of Coal Measom
Coke.
Woolwich Araenal.
Iron
SOicon.......
Snlphnr
8S.880
4.8S8
0.979
0.014
0.060
10.T07
0.066
0.0T7
0.091
0.046
98.9Q6
4^
0.1TB
Trace.
0.199
1.987
CoIdBlaat.
No. 8
No.l
Pom
Pig.
}f»^gui€9e
Copper
Alnminnm ..........
Iron
98.01
0.04
810
9.16
0.11
0.68
0.50
0.06
94.69
£40
1.86
0.07
0.99
0.98
94.88
Cafclnm
IfAgiieeiiiiii
n-,Kft„ j Combined .
^^^''I Graphitic.
SUlcon :.
Snlphnr
j 9.87
109
Total
90JM6
100.00
0.78
Phosphomt
0.76
MancianeM
Nickel and Cobalt...
Total
0.98
99.60
100.09
100.00
ANALYSIS OF SUG FROM BLAST FURNACE.
Workft,
Ore need,
Fnel used,
Dowlaia. Dudley.
Clay Iron Ore of Coal Measure.
Coke.
Kind of Iron,
White
Foiige Pig.
Gray Pig.
Hot Blast
Analyit,
Riley.
Forbes.
Perey.
Fcrrouf oxide.
Alnniinn. . . . . ,
6.91
1.67
16.61
28.81
4.88
1.98
44.88
0.48
o.se
0 47
0.76
l.(H
16.18
88.89
7.44
1.99
88.48
0.16
1.98 I
0.99 f
0.98
9.79
18.01
81.48
7.97
9.60
87.91
8.65
1.97
0.40
14.11
Lime....... ........ :....
Ma^esia
86.70
7.61
Potash.
1 85
siHca..:::::::::;::::;;::"":;::"::
88.06
Phoaphorlcacld
Cftldom
Snlphnr
0.88
Total
100.68
100.54
99.69
99.81
Percentage Iron
6.87
0.60
0.69
0.99
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►
388 THE CHEMISTS' MANUAL.
CHROMIC IRON ANALYSIS.
T. S. Hunt and (F. A. Gknth. ZeUaehrift f. Anal. Chem,, 1, 498.)
Take 0.5 gram of the impalpable powder, and fuse in a
capacious platinum crucible with 6 grams potassic hydrosul-
phate for fifteen minutes, at a temperature scarcely above the
fusing of the latter ; then raise the heat somewhat, so that the
bottom of the crucible may just appear red, and keep it so
for fifteen or twenty minutes. The fusing mass sliould not
rise higher than half-way up the crucible. The mass begins
to fiise quietly, and abundant fumes of sulphuric acid escS^pe.
At the expiration of twenty minutes the heat is increased as
much as necessary to drive out the second equivalent of sul-
phuric acid, and even to decompose partially the iron and
chromic sulphate. To the fused mass now add 3 grams pure
sodic carbonate ; heat to fusion, and add a small portion from
time to time during an hour of 3 grams nitre, maintaining a
gentle red heat all the while ; then heat for fifteen minutes to
bright redness. Treat the cold mass with boiling water ; filter
hot ; wash the residue with hot water ; then digest in the heat
with hydrochloric acid. If anything remains undissolved, it
is a portion of the ore undecomposed, and must be subjected
again to the above operation.
To weigh such a residue and deduct it from the ore first
taken, is not good, as it never possesses the composition of the
original substance. The alkaline solution, which often con-
tains, besides the chromic acid, also some silicic, titanic, and
manganic acids and alumina, is evaporated with excess of am-
monic nitrate on a water-bath nearly to dryness, and till all
free ammonia is expelled. On addition of water, the silicic
acid, alumina, titanic acid, and manganic oxide, remain undis-
solved, while the chromic acid passes into solution. Filter
and thoroughly wash residue. To filtrate, add HCl and al-
cohol, when the chromic acid is converted into chromic oxide
(sesquioxide of chromium) by heating the solution for some
time.
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THE CHEMISTS' MANUAL. 389
All the alcohol must be expelled by heat. Then to the solu.
tion, which must not be concentrated, heated to 100° in a beaker,
is added ammonic hydrate in slight excess, and the mixture
exposed to a temperature approaching boiling-point, until the
fluid over the precipitate is perfectly colorless, presenting no .
longer the last shade of red ; let the solid particles subside ;
wash three times by decantation, and lastly on a filter, with
hot water, dry thoroughly and ignite and weigh as Cr^O^
(chromium sesquioxide). This method is very accurate.
ANALYSIS OF CHROMIC IRON.
Chester Co., Pa.
FeO 85.14
MgO
Cr.Oj 61.56
Al,0, 9.72
Baltimore.
FeO :. 30.04
MgO
Cr.O, 68.37
AlgO, 1.95
SiO, 3^ CaO 3.02
Total, 99.32 SiO, J^l
I Total, 99.59
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390
THE CHEMISTS' MANUAL.
SCHEME FOR THE ANALYSIS OF PIG LEAD.
(See Fbes., Zeit. Ann. Ch.)
Determine the silver by cupellation, or wet way, in
grams. For other metals present in the lead, dissolve 200
grams in 1.5 litres of water + 550 c.c. strong nitric acid, using
a large flask and filtering, should the solution be turbid.
RB8IDUE a.
Sb.Os - SnO, may be left. If bo,
disBOlve it in HCl, paes in H,S gap,
Alter and reserve the piec. to go with
Pbbc. r. ^Noto 1.)
SoLXTTzoir a.
Pbboifitatv e
= PbSO« and nerhaps Sb. Diffflolve
In HCl, add 10 Tolnmes H.S water,
paaa H.S gas In, and filter, etc.
8oi.imov d,
Bc^ect it.
PsaoiPiTAn d
= Sb^, •»- PbS, add
It to PBBOXPITATB /.
(Note 2.)
U boars for precipitate to settle ; filter, etc
PBBOIRTAn ff
= FeS, Zii8,_Co8, NIS.
Add 66 c.c. of pare H.SO«, shake and ellow to
stand till settled. Then filter and wash thoroaghlj.
PttBCIFITATB b. SOLtmON b.
Bqoal Pb80«. Bvaponte until fhmes of sal-
Reject pharic acid appear ; cool, and add
00 c c. of water ; filter and wash
with hot water.
SoLunoH e.
Dilate to 200 cc, heat to 70* C, pass H.S gas In,
allow to stand 18 hoars, filter, etc
SoLunoH /.
Evaporate to
600 c c, add
(NH.HO +
(NH«)H8, fiU
flask ana al-
low it to stand
Treat on the filter with a
mixtare of 6 partK Ha8
water + 1 part dilate HCl, I
pouring back several
times so as to avoid bulk ;
filter, etc.
SoLimaw ff.
Acidulate with HC.n^O,
and boil to recover NiS;
filter, etc.
Precitatk i
=Ni8,addto
Pbko. ff.
Rbsiditb a
=Oo8, NiS.
Dry, Ignite
to oxides r,
test with
the blow-
pipe
Feuo. i.
= Fe.O..
Solution h
= FeS. ZnS.
Add HNO.,
boil ; then
add(NH.)HO
in excess ;
filter, etc.
SoLUTioir i.
Add
(NH,>HO +
(NHJHS in
a flask and
allow to stand for twenty-
four hours ; filter, etc.
SOL.^. I PBBOIPITAni
= ZnS. Dis-
! solve in HCl
and boil with
Na.COs in excess : filter,
etc., ignite and weigh as
ZnO.
FiLTRATKil;.
Beject
Pbbcifttatk^
= SbxS., As.S., SnS,, Bi3», CnS,
Cd8,Pb8,etc. AddPssc. cl. Tx«at
with K.8, filter, etc (Note.)
Bbsidui I
= Bl-8,. CuS,
CdS. Pbs.
Spread the fil-
ter in a dish,
and treat nesirly
to boiling with
HNO, : when
dissolved, fil-
ter, wash, dry
and bum filter:
throw the ash
into the HNO.
solution. Then
add 8 c.c. HaSO« and evaporate till white
fhmes appear ; add HaO and allow to set-
tle ; filter, etc.
PBSOIFnATB tn,
PbSO, ; reject
SoLunoir tn.
Nentrallse nearly with
pure KHO : add Na.CO.
and a little KCy (tne
ft-om K,S) ; filter, etc. (N.B. Note 4.)
PBxoiprrATB n I
= Bi.O..
Dipsolve in dilute
HNO, and prec.
with (NH,),CO,
as above
SOLTTTION n.
Add a little more
KCy and then a few
drops K,R ; filter and
wash. Have Sol. o
and Prko. o.
SOLTTTIOV /
^ AstS,, 8b,St.
SnS, in K.S solu-
tion. Add HCl and
filter.
Pbbc. r.
6oL.r.
Beject
8b,8„
As, A,,
SnS,.
Add prcclp. tnm
Residux a \ dry,
treat with CJ^,, and
drv again. E^-apo-
rnte after adding
fhm]ngHNO„antfl
paper is destroyed
and most of the add
gone. Then dilute
a little and add
Na,CO, to alkaline
reaction, and then
NnNO, and evapo-
rate to drvness, and
heat careftiDy to fh-
sion. After cool-
insr. extract th(^ cake
with water, etc.
(Spo Fres., a. &,
p. 437.)
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THE CHEMISTS' MANUAL.
891
Add ft Httle HNO» -l- H,80«
-f HCl, mod erapomte undl no
odor of KCy U perceptibb.
Filter if neceftsaiy. PrecipiUte
the Ca with H,S.
FBBCXPITAra o
= Ag.8,CdS. Wash with dilate
HNO,. (Notes.)
RxarouB $. 8ol. t.
SOLlTTIOirX
= CdS. Evap-
orate nearly to
dryneft* and
add Na.CX),.
If no precipi-
tate appears,
add KHO, and if one then appears, Alter and waah ; filter with
NH.NO. and hum = GdO.
BttlDTJXX
= A«.S. Re-
iecteaaBAgfla
aetermined sep-
arately.
NaSbO..
Dissolve
in HCl •»-
H,C«H«0.
and pass
in H,8 =
8b,B. 4- 8,
oxidise
withHNO,
and weigh
as SbO,.
Add result
from Rbsi-
DUK t.
KiS and add large excess solution of snlphnrons acid, and digest
bftth, and then lM>il until two-thirds of water and all SO, is gone,
As, Sb, 8n.
Evaporate
off alcohol,
add dilute
H,SO«.
evaporate
until no
fbmes of
IINO. are
perceptible
and pass
H,0 gas in
at TO" C.
and filter,
wash, etc.
Dissolve in
for some time in a water-
filter, etc
Sh,8, -f SnS,. The SbaS, here win oulj
he a trace. Oxidize in a cmcihlo with HNO,
and weigh ; then ignite in hydrogen to expel
the SbO,, and oxidize again with HNO, and
weigh the 8nO.. The loss, ShO,.
SoLunoM I.
ASaS,. Fsas in H,9 gas, filter and wash,
oxidize with ftiming HNO., dilute a little,
warm gently with ITCIO, and precipitate aa
ammonio-magneslc arseniate. The washing
must he with NaCI, and the latter displaced
by (NH«)iD»HaO|, the latter washings being
rejected.
Note x. — In case no CdS be present, Bi and Cu may be
separated by (NH4)H0 and (NH^)2C03.
Note 1. — There will not (probably) be any Sn in the lead.
Should there be any it must be looked for in Filtrate 8.
Note 2. — If precipitate d contained much Pb, better treat
separately to the point of oxidizing with HNO3, and then add
to PBECIPriATB r.
Note 3. — Better dissolve thoroughly PBEciPrrATE r. The
Cd with (NH4)2C03, which will not dissolve the same.
Note 4. — If the KCy contains K2S, the precipitated car-
bonate may contain sulphides. Filter, wash, and dissolve in
boiling HNO3. Filter out any separated sulphur. Again pre-
cipitate with (NH4)2C03 in slight excess and hoil,
Ag will not be precipitated. Cd may be. Filter and wash
with water and then with a little KCy. The CdC03 is so
, readily soluble in KCy that it will be carried through the filter
into the solution.
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}
392 THE CHEMISTS' MANUAL.
ANALYSIS OF PIG LEAD.
Harz. Hatic.
Coppor 0.00476 0.0022
Antimony 0.00317 0.0052
Iron 0.00168 0.0007
Zinc 0.00265 —
Silver 0.00060 0.0006
Lead 99.98716 99.9913
Total lOO.OOOOD 100.0000
SCHEME FOR THE ANALYSIS OF A NICKEL ORE
Fuse 2 grams of finely-powdered niccolite (niccolite arsenide
4- cobalt + iron) with 2 parts of potassic nitrate and 2 parts
of carbonate of soda, in a platinum crucible, the bottom and
sides of which have been previously lined with NajCOa ; the
mass is then ignited for some time, and when cold, digested
in water ; tlie oxides formed are filtered off and thoroughly
washed. The solution contains all the arsenic in the form of
arsenates of the alkalies ; it is supersaturated with HCl, then
mixed with (NH4)H0 and MgSO^. Let the precipitate stand
for twenty-four hours, then filter through a weighed filter
washed with dilute (NH4)H0, dried at 100° and weighed.
The oxides are dissolved in concentrated HCl, and the cop-
per and bismuth, precipitated, by H2S. The filtrate from HjS
treatment is heated to boiling, and mixed with some KCIO3 in
order to peroxidize the iron, which may then be separated from
the nickel and cobalt in the same manner as from manga-
nese, by baric carbonate. From the liquid separated from
the baric carbonate, the dissolved baryta is precipitated by
H2SO4, and filtered. The filtrate contains the nickel and
cobalt, which are precipitated from a hot solution by potassic
hydrate.
The precipitate containing the hydrated oxides of Ni and Co
is gradually mixed with potassic cyanide (free from cyanate),
and a gentle heat applied until dissolved. By this process
the cobaltous and potassic cyanide, KCy,CoCy29 in the solution
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THE CHEMISTS' MANUAL. 393
18 converted into potassio-cobaltic cyanide (KgCojgCyg), whilst
the nickelous-potassic cyanide remains unaltered. Add to the
solution, while hot, levigated mercuric oxide. By this method
the nickelous-potassic cyanide is decomposed, and all the nickel
precipitated, partly as oxide and partly as cyanide. Filter and
wash ; ignite ; with excess of air, leaves pure oxide of nickel
behind, which weigh. Neutralize the filtrate with HNO3 and
solution of mercurous nitrate, as neutral as possible, added
as long as it produces a precipitate of mercurous-cobaltous
cyanide. After being filtered (through a weighed filter),
washed, and dried, it is ignited with excess of air, when it is
converted into cobaltic oxide, which, after weighing, must be
reduced by hydrogen to metallic cobalt.
ANALYSIS OF NICCOLITE.
As 54.05 54.89 52.71
Ni 43.50 43.21 45.87
Fe 0.45 0.54 —
Pb — — —
Co 0.32 — —
Sb 0.05 - —
S 2.18 1.35 0.48
Gangue 0.20 — Cu 1.44
Total 10075 99.09 "lOO.OO
Analysis by. . . Ebslicen. Gbtthow. Schhabkl.
SCHEME FOR THE ANALYSIS OF A COPPER ORE
Weigh out 2 grams of the powdered ore (impalpable powder),
and put into a beaker. Add concentrated HjSO^H-HNOa.
Cover with convex cover; heat gently until eflfervescence
ceases; remove the cover, and expel all the HNO3 ^^^^ ^
water-bath by evaporation, until fumes of H2SO4 are given off.
Wash dovm the sides of the beaker with hot water, then
filter into a weighed platinum dish ; after diluting with water,
throw in a piece of zinc (soluble in hydrochloric acid without
residue), and add, if necessary, a little more acid. Cover the
dish with a watch-glass, which is afterwards rinsed into the
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394 THE CHEMISTS' MANUAL.
dish. The separation of the copper commences immediately.
Heat, if necessary.
After an hour or two teat a portion of the snpemated liquid
with HjS water; if no brown tint is imparted, the copper is
all precipitated. Press the copper together with a glasa rod,
decant the clear fluid; wash; precipitate with boiling H2O9
and decant again; rinse the dish with strong alcohol; heat
over water-batli ; when Cu is dry, let it cool, and weigh. The
precipitation may be done in a porcelain or glass dish, but it
will take longer.
ANALYSIS OF COPPER PYRITES.
s
35.87
36.10
33.88
Cu
«1
Analysis by
34.40
80.47
3285
8265
Fe
... . 29.93
82.77
Quartz .
Mn
0.27
.. .. 0.32
Trace.
Pb. . . . .
... . 0.35
Tot
101.01
Bon.
09.28
SaiTH.
99.62
FOBBBB.
SCHEME FOR THE ANALYSIS OF A ZINC ORE.
The ore may contain Zn, Fe, AI2O3, CaO, MgO, PbO, SiOa,
S, H2O, CO2.
Dissolve 2 grams of pulverized ore in a mixture of 5 c.c. of
HNO3 + 5 C.C. of HCl at a gentle heat, then add 5 c.c, of N2SO4
and evaporate until fiimes of sulphorie acid are given off; then
add boiling HgO and filter.
PRECIPrrATB.
SlO. + PbSO^. Weigh; then boU
with ammonic citrate and filter. Res-
idue wiU be SiO,. The filtrate will
be Pb in solution ; add H,B and the
precipitate will be PbS ; put in cru-
cible, add HNO, +H,S04, and ifirnite,
which will fjriye PbSO^, which weigh.
The filtrate will contain in solution Zn, CaO, MgO. Add
H2S water; then pass in the solution H2S gas until Zn is all
FlLTBATB.
Fe,0,, A1,0,, ZnO, GaO, MgO, in
solution ; neutralize with Na^Co, ;
add sodic acetate and boil. Precipi-
tate wiU be Fe,0, and Alj^O.; filter
off
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THE CHEMISTS' MANUAL. 395
precipitated as ZnS. Filter and wasli with H2S water. Dis-
solve ZnS in HCl on filter; then wash into beaker with boiling
H2O ; add a few crystals of KCIO3 and boil; filter oft' the sul-
phur which may separate ; then add NajCOa, and the Zn will
be precipitated as ZnCO^ ; filter and wash ; ignite in a porce-
lain crucible and weigh as ZnO, from which the Zn may be
calculated. The solution filtered from ZnS will contain CaO
and MgO. Precipitate CaO as oxalate, and MgO as MgNH4P04.
Make special determinations for S, HgO and COg.
The above analysis is principally for the determination of Zn.
s
ANALYSIS OF
32.10
ZINC BLENDE.
83.82
8382
Zn
Fe
64.22 ....
1.82 ...
Trace
64.89
.... 54.17
11 19
Cd
0.98
. . . . 0.82
Cu
0.82
Pb»
0.72
0.78
Mn
088
H.O
0.80 ....
Total W.16 ....
100.29
Sjoth.
.... 100.88
ANALYSIS OF PYROLUSITE
FOR ITS COMMERCIAL VALUE.
The following analysis is founded on the fact that when
oxalic acid comes in contact with manganese in presence of
water and sulphnric acid, manganous sulphate is formed, and
carbonic add is evolved.
Mn02 + H2S04 + C203=MnS04+2C02 + H20.
Each equivalent of available oxygen, or, what amounts to
the same, each 1 eq. manganese dioxide = 43.5, gives 2 eq.
carbonic acid = 44.
As 44 parts by weight of CO2 correspond to 43.5 of manga-
nese dioxide, the CO2 found need simply be multiplied by
43.5 and the product divided by 44, or the COo mav be multi-
* Sb and Pb.
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396
THE CHEMISTS' MANUAL.
43.5
plied by -r^ = 0.9887 to find the corresponding amount of
manganese dioxide.
Take (0.9887) x 2 or 3 grams of ore, which is finely pulver-
ized, and introduce into a weighed flask A (capable of holding
120 C.C. up to the neck) ; now add 5-6 grams of sodic oxalate
or 7.5 grams potassic oxalate, in powder, and enough water to
fill the flask two-thirds full. Insert the cork into A and see
that it does not leaL
A = 120 C.C. to neck.
B = 100 c.c. to neck.
6 for sulphuric acid.
A for ores, etc.
a is closed at b with wax ball.
^0t0.— Exact weight of A and
6 must be known after they are
charged — that is, before CX), is
aUowed to come off.
Now make some H2SO4 flow from B to A, by applying
suction to d by means of a rubber-tube. CO2 goes oft' imme-
diately; when it ceases, let some more H2SO4 pass in, and
complete this imtil the manganese ore is completely decom-
posed. Take five to ten minutes.
Let the apparatus be weighed again after becoming cool.
The loss will equal CO2. The number of centigrams lost,
divided by 2 or 3, according to the multiple of 0.9887 gram
used, expresses the percentage of manganese dioxide in the ore
treated.
ANALYSIS OF PYROLUSITE.
Mn,Mn 83.56
O...
BaC
SiO,
H,0,
14.68
1.86
Total 100.00 ..
AnalyaiBby Ajbfvbdsok.
. a5.62
. 11.60
0.66
0.65
1.57
. 100.00
TUBHIB.
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THE CHEMISTS' MANUAL.
397
SCHEME FOR THE ANALYSIS OF ILMENITE.
Fuse 1 gram with 3 grams of NaF + 12 grams KgSgOy
thoroughly. Dissolve in large volume of cold water. If
there is any residue, fuse and dissolve as before. Neutralize
with NajCOa until a slight precipitate appeara, which dissolve
in H2SO4, so the fluid will be slightly acid. Saturate with
H2S gas ; boil one hour, adding from time to time HgS water.
Filter oflF the precipitate, and wash with water containing H^S.
The precipitate will be TiOj + S. Ignite and weigh =Ti02.
If the precipitate contains iron, fuse over again, etc.
ANALYSIS OF ILMENITE.
(Hystatlto.)
(Bmenite.)
TiO,. . .
Fe,0, .
FeO. . .
MnO. . .
MgO...
CaO...
SiOg...
Cr.O^.
(Hystatlte.)
2419
46.67
63.01
11.71
19.91
85.87
2.39
069
0.60
0.33
0.26
1.77
... . 2.80
0 .qft
Total 99.89
AnalysiB by MoeANDS
100.17
MoeAHDXB.
25.28
51.84
22.86
99.98
Kknsall.
SCHEME FOR THE ANALYSIS OF NATROLITE.
Moisten 2 grams of the pulverized mineral with water, and
digest in concentrated HCl ; heat, evaporate over water-bath ;
break up residue with stirring-rod, and get a powder.
It must neither be imder or over heated. Cover with paper
and put in air-bath, heat to 125° C' Let it dry for two or
three hours, moisten with concentrated HCl and let stand a
few minutes. Warm gently, then add water. The bases go
into solution and Si02 separates, which is weighed.
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398
THE CHEMISTS' MANUAL.
Divide filtrate into two parts :
iBT Pakt.
To detennine Na^O, add caustic
baryta, which precipitates Al, Fe,
Mg. The filtrate will contain fiaO,
GaO, and alkalies. To remove BaO
find CaO add (NH4),C0, and filter.
Test to see if CaO is present and
bum off (NH4)H0. Wash out evap-
orating dish with smallest amount
of water, add HCl and evaporate in
a weighed dish, and the residue will
be NaCl, which weigh.
2d Pabt.
To determine Fe, Al, Mg, treat
this 2d part in the usual manner.
Precipitate the Fe and Al by
(NH4)H8, etc
ANALYSIS OF NATROLITE.
SlO, . .
Al.O,.
Fe.O,.
CaO...
NaO. . ,
H,0. . .
48.00
2425
1.75
16.50
9.00
Total 99.50
AnalyBlB by. . . .Ki.apbotb.
4751 44110
25.60 aO-05
1.85 0.96
— 0.88
16.12 •-.. 18.58
o<oo •••••«•••»•.••• V«vu
99.16
FUCBS.
90.81
SCHEME FOR FELDSPAR OR ORTHOCLASE
ANALYSIS.
Mix the finely -powdered mineral, dried at 200°, with four
or five parts of baric carbonate ; this is then exposed to an
intense white heat by a blowpipe. When the contents are
aggregated into a cinder-like mass, the mass is then turned
out of the crucible into a capacious dish, a quantity of water
poured over it, and hydrochloric acid added in slight excess
until it is completely dissolved, with the exception of some
gelatinous Si02 which separates. The whole solution is then
evaporated to perfect dryness; then moisten with HCl and dis-
solve in HjO and filter off Si02, which weigh.
Precipitate the baryta in the filtrate with H2SO4 (very lit-
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THE CHEAUSTS' MANUAL.
899
tie); filter, and concentrate the filtrate, add (NH4)HS and
precipitate the ^2^99 ^^^ filter. Evaporate the filtrate to
dryness, and ignite it to expel ammonia salts. The residue is
sulphate of potash, and is weighed. If soda is present it must
be separated.
ANALYSIS OF FELDSPAR (ORTHOCLASE).
8iO,..
A1,0,.
Fe,0, .
MgO..
CaO...
NajO.
K,0..
66.75
17.50
67.01
18.60
1.76
0.85
125
.. .. 0.19
0.56
2.01
13.00
11.41
Total 99.25
AnalyBif by . . Boas.
100.63
DVBBSB.
65.10
20.12
2.42
12.80
100.44
SCHEME FOR THE ANALYSIS OF DOLOMITE
OR MARBLE.
It may contain CaO, MgO, Si02, AI2O3, Fe203. Dissolve
1.5 grams in HCl + HNO3, evaporate to dryness, moisten with
HCl, add H2O and filter.
Residub.
SiO, and silicates fuse in platinnm
enicible with Na,CO,; moisten with
H,0, add an excess of HCl, evapo-
late, dissolve in H,0 and filter.
BssmuE.
• SiO,, weigh.
PBBCIPrrATB.
A1,0, + Fe,0,
(CaO, MgO?).
Wash with a lit-
tle hot water, dis-
solve in HCl, re-
precipitate, filter,
add Filtrate (C) to Filtrate (E\ The precipitate = A1,0,
+-FeaO„ which weigh or separate.
B Filtrate.
Add to first Fil-
trate A.
A FiLTBATB + B.
Warm, add NH^a + (NH4)H0,
and filter.
E Filtrate + C.
CaO, MgO.
Concentrate if
too bullLy; acid-
ify with Ha if
cloudy ; then add
(XH,)HO.H
(NH,),C«04; al-
low the precipi-
tate to stand over
night ; pour the clear liquid through the filter ; wash the precipitate in the
heaker once or twice with H,0 ; pour the clear liquid through the filter
and dissolve the precipitate in HCl. Beprecipitate with (NH4),C,04 and
filter.
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400
THE CHEMISTS' MANUAL.
Pkbcipitatb,
CaCjO^. Moisten with HjSO^ =
2CaS04 and ignite in platinum cru-
cible ; cautiously moisten with dilute
H,S04 ; heat and weigh.
FiLTRATR.
MgO. Concentrate if too bulky,
and acidify if cloudy with HCl. Add
an excess of (NH4)H0, then add
NajHPO^. Filter off precipitate =
MgHPO* ; wash with [1(XHJH0 +
8H,0] ; dry and weigh.
For CO2 determination take about 1.5 grams, use apparatus
which is used in Pyrolusite.
For S and PO5 determinations, digest 6 grams in HNO3 and
divide.
ANALYSIS OF DOLOMITE.
(Jena^cryst)
CaCO, 55.22 ..
MgCOa 44.77 ..
FeCO, - ..
MnCO, — ..
H,0 — ..
FeO.... — ..
(Hiemite.)
.. 67.91 .
. . 88.97 .
.. 1.74 )
.. 0.57 )
ilA Valooclana.)
. . . . 53.18
.... 84.35
Total 99.99 .
ADalysifl by SuoKOW.
93.19
10.46
1.22
0.22
99.43
BOTB.
SCHEME FOR THE ANALYSIS OF WHITE LEAD,
The substances likely to be found are BaSO^, clay, ZnO,
PbSO^, PbCOa, CaCOg, CaSO^, HgO-foil. Digest 10 grams
of the material in a flask with ether ; filter and wash. Weigh
out of the powder 2 grams, and dissolve in HNO3; boil and
filter.
Rbsidtte a.
BaS04, clay ; weigh, and separate
If desirable.
PRBCIPrrATB B.
= PbS ; weigh as PbSO*.
REsmuE C.
= ZnS ; convert into ZnCO,, and
weigh as ZnO.
Filtrate A.
ZnO, PbO, CaO ; treat with H,S in
presence of considerable acid, and
filter.
SOUJTION B.
Zn + CaO in solution; add (XH4)
H0 + (NH)4HS; filter and wash.
Filtrate C.
CaO; add (NHJ.CjO^, and the
precipitate will be CaCgO^.
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THE CHEMISTS' MANUAL.
401
To determine SO3 in the shape of PbS04H-CaS04, dissolve
3 grams in boiling dilute HCl; add a little ammonic citrate
or acetate ; filter and determine SO3 as usual.
This scheme will apply also to zincic pigments.
SCHEME FOR THE ANALYSIS OF TYPE METAL
May contain Sb, Pb (Sn, Zn, Fe). Dissolve 1 gram of metal
in HNO3 + tartaric acid at a gentle heat; filter and wash.
Solution.
Sb, Pb (Zn + Fe); add H.SO^ to
eolation ; heat to boiling, and filter.
Residue.
SnO, xnaj contain a little Pb and
Sb; ignite the residue and weigh.
Fase with NagCO, + S ; dissolve in
hot H,0 and filter. Residue = PbS.
Heat in porcelain crucible with HNO,
which gives PbS04 ; ignite and weigh.
Add to Residue A.
Residue A.
WiUbePbSO^;
dry and weigh.
Precipitate.
SbS,+PbS; di-
gest with yellow
sulphide of ammo-
nia and filter.
Residue.
Will be PbS;
heat in a porce-
lain cmcible with
HNO„ which
gives PbSO^ ; ig-
nite and weigh,
and add to Resi-
due A.
Solution.
Sb, Pb (Zn and
Fe); pass in IlgS
gas and filter,
washing with
H,S water.
Solution.
Add(NHjHS;
precipitate = Fe
and Zn.
Solution.
(NH^niS, Sb,
S, ; precipitate
with HCl = SbS,
+ S ; evaporate
with HNO, in a
porcelain cruci-
ble; bum filter
paper with NH4
NOg and add ; ig-
nite the whole and
weigh as SbO^.
! Residue.
SnO, may contain a little Pb and
I Sb, ; ignite the residue and weigh.
I Fuse with NagCO, + S ; dissolve in
hot HaO, and filter. Residue = PbS.
Heat in a porcelain crucible with
HNO, which gives PbSO^ ; ignite
and weigh. Add to Residue A.
Solution.
Add Ha ; precipitate=:Sb,S,SnS, ;
oxidize with HNO, ; fuse with NaHO
in silver dish. Dissolve mass in 8
alcohol -I- 1H,0 and filter.
Residue.
NaSbO, ; warm
with HCl ; dilute
with H,0 and
precipitate with
n,S the Sb as
Sb,8, ; treat as
before.
Solution.
Sn as Na,Sn
O, ; acidulate with
HCl ; precipitate
by H,S = SnS, ;
ignite with SnO„
and weigh.
Note. — ^The above schemes show
only how to separate the constitu-
ents. For further information, see
Fresenius.
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402
THE CHEMISTS' MANUAL.
ANALYSIS OF TYPE METAL
Mbtals.
^
1
1
1
Type metal
15.5
20
50
56,8
14
16.7
69
80
75
17
7.4
89
15.5
Printing characters
Babbitt metal
—
Britannia metal
25 !2i5
White metal
28.4
86
8.3
74
Pewter
Metal that expands in cooling
—
SCHEME FOR THE ANALYSIS OF A SILVER COIN.
It contains Au, AgjS, Ag, Pb, Cu.
Boil in K HO to clean it ; then weigh, dissolve in HNO3 (^^^
from CI), and filter.
Prbctpitatb.
Au, AgjS. Dry; weigh; wrap In
a piece of Pb and cupel. This de-
stroys the AgS. Add also a little
piece of silver (the weight of which
must be known) ; dissolve the button
in HNO„ and filter.
Residue.
Au.
Filtrate.
AgNOg ; add to
Filtrate A.
Filtrate A.
AgNO.,Pb(NO,)„ Cu(NO,), ; add
Ha and filter.
Prbcifitatb.
AgCl.
Ftltratb.
PbCl, + Cua,;
add about 10 cc.
of HgSO^; evaporate to dry nets ; dis-
solve in H,0; filter and wash with
water containing a little alcohol.
Precipitatr.
= PbS04.
Filtrate.
= CUSO4.
Precipitate with
KHO,and test fil-
trate with HS.
ANALYSIS OF SILVER COIN.*
Ag.
Cu..
Pb.
Au.
51.49
47.91
.63
.02
Total 100.05
* Poor, Spanish coin.
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THE CHEMISTS' MANUAL. 403
SCHEME FOR THE ANALYSIS OF FERTILIZERa
Aspirator
■^
I I I
KITBOOEN TUBS.
Fertilizere owe their value to PjOg (soluble and inBolnble to
NH3 and K^O).
Ist Those that furnish insoluble P2O5 ; as bone ash, bone
black, rock guanos, apatite, green marl.
2d. Those that fiimish insoluble P2O5 + NH3; as bones,
meat scraps, dried blood, and almost all animal matter.
3d. Those that furnish NH3.
4th. Those that furnish soluble P2O5, as superphosphates.
To determine insoluUe P2O5, weigh out 2 grams, place in a
porcelain dish and evaporate with HNO3, ^^^ briug into solu-
tion. To destroy organic matter, add KCIO3. Divide the
solution in halves, and heat with Mo03. Wash the yellow
precipitate with M0O3 ^^^ dissolve it in (NH4)H0, and repre-
cipitate with magnesia mixture.
To determme the soluble P2O5, take 1.5 grams, pulverize
finely, and dissolve in cold H2O, and determine P2O5 as usual.
The determination of the nitrogen is conducted by mixing
the substance with soda-lime and heating. The H which is
formed goes to the N, and 0 to C, by splitting H2O.
The nitrogen tube, as shown in the figure, is placed in a
gas furnace, or in a charcoal fiimace. Determine NH3 with
PtCl4 or with a normal HCl solution.
Multiply the determined value of P2O5 in bone phosphate
by2.18 = Ca3(P04)2.
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404
THE CHEMISTS' MANUAL.
COMPLETE ANALYSIS.
May contain : SIO2, AI2O3, FegOg, CaO, MgO, KgO, NagO,
CO2, NH3, insoluble P2O5, soluble P2O5, H2SO4, H2O, organic
matter.
Use special methods for total P2O5, soluble P2O5, KjO,
NagO, NH3, H2O, CO2.
For SiOa, AI2O3, Fe203, CaO, MgO, H2SO4, dissolve 5 grams
in HCl, evaporate to dryness, moisten with HCl, add water,
and filter.
Residue A
SiO,, ignite and weigh.
Solution A.
Dilute to 500 C.C.
Divide in four parts.
l6t. 200 C.C.
Precipitate CaO
by H,S04 and
alcohol. (Not too
much alcohol nor
too little. About
2 vols, alcohol to
1 of solution was
with this solution.
Precip. = CaS04.
Test after weigh-
ing for AljOs and
Fe,Og.
2d. lOOcc.
3d. 100 c.c.
I
4th. 100 c.c.
Determine Fe Determine H ,804 Determine AlgO,
with KjMnaOg. with BaClg. by adding a solu-
tion of 4 grams of
metallic iron to liquid + Nag Co, + NaCgHjO,. The
precipitate = Al gOg -1- Fe,0, + P»Og. Ignite and weigh,
and deduct Fe,0, + PjO,.
To filtrate from Ist part add NaHP04 and (NH4) HO, and precipitate =
MgNH4P04. Ignite and weigh as MgePjO^, and determine MgO.
ANALYSIS OF WATERS.
BRIEF RULES WITH REGARD TO MINERAL WATERS.
I. If the water reddens blue litmus-paper before boiling,
but not afterward, and the blue color of the reddened paper is
restored upon warming, it is a carbonate.
II. If it possesses a nauseous odor, and gives a black precip-
itate with acetate of lead, it is sulphurous.
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THE CHEMISTS' MANUAL. 405
III. If, after the addition of a few drops of hydrochloric
acM, it gives a blue precipitate with yellow or red potassium
pnissiate, the water is a chalybeate.
IV. If it restores the blue color to litmus-paper aft«r boil-
ing, it is alkaline.
V. If it possesses neither of the above properties in a
marked degree, and leaves a large residue on evaporation, it is
saline water.
COMPLETE ANALYSIS OF MINERAL WATERS,
WHEN CONTAINING ALKALINE CARBONATES.
Fob Total Solids. — Evaporate 0.5 litre in weighed Pt dish ;
dry to constant weight at 130'' C, and weigh.
Fob FcaOa+AlaOa + CaO + MgO — SiOg, acidulate 1 litre
and evaporate to dryness in Pt dish ; moisten with HCl and
treat with hot water; filter, wash, etc. Dry residue, ignite
and weigh. Then expel SiOg with NH^Fl, and weigh again.
The loss is SIO2. Should any residue be left, examine it in
the SPECTBOSCOPE.
Treat the filtrate with (NH4)H0 and NH^Cl ; boil to precipi-
tate FcgOs, AI2O3, and P2O5 ; filter, etc. Dissolve the pre-
cipitate, and reprecipitate ; add the filtrate and washings to
the first, and in the combined filtrates determine the CaO,
MgO as usual.
Foe SO3, acidulate 1 litre with HCl, evaporate to small
volume in a porcelain dish, and precipitate with BaCla as
usual.
Fob Sodio Cabbonate, evaporate 1 litre of the water to
dryness ; treat with water and test with a standard solution of
H2SO4 or other acid-f-Na2C03 + Li2C03; or evaporate 1 litre
to dryness, dissolve in water, filter, wash. The sodic or
lithic carbonate go into solution. To the filtrate add a mix-
ture of CaCl2 + (NH4)H0 [prepared by dissolving 60 grams
CaCl2 in 250 c.c. water, adding 100 c.c. (NH4)H0] in excess;
filter and wash rapidly.
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406 THE CHEMISTS' MANUAL.
The CO2 goes to the lime ; the Boda and lithia are washed
out as chlorides. Dissolve the CaCO^ on the filter with HCl,
then precipitate as oxalate; either determine as CaS04 or
ignite to CaO, and estimate the corresponding amount of CaCOa ;
from this calculate the NagCOa by the proportion,
At. Wt. CaCOg : At. Wt. NagCOa : : CaCOg found : Na^COa.
Foe Potabsig oxtoe. — Take 1 litre of water ; evaporate nearly
to dryness in a silver dish; filter, wash with boiling water,
evaporate in Pt or porcelain dish with slight excess of HCl +
PtCl4 to dryness, or nearly so, on water-bath. Then dissolve
in a mixture of 2 parts alcohol and 1 part ether. Filter out
KCl, PtCl^ ; wash very completely with the same ; dry, trans-
fer to crucible, and ignite with oxalic acid. (See Fresenius.)
Total Chlorine. — Test -^^^ gallons with standard solution
AgNOg — (1 c.c. = 0.1 grain NaCl).
Fob Carbonic Acid. — Take 200 c.c. of the water previously
treated at the spring with "CaCl2+(NH4)H0 preparation,"
being careful to clear the neck of the bottle from all tat, etc.
Keep the bottle in boiling water until the eflFervescence ceases;
then filter out the CaCOs, rinsing the bottle thoroughly with
water. Keep the bottle for after treatment. Wash the CaCOg
on the filter, as long as the wash-water gives a reaction with
This washing should be done rapidly, to avoid the forma-
tion of CaCOs by the CO2 in the atmosphere, acting on the
CaH202 present. Then dissolve the CaCOg adhering to the
bottle with a little HCl, and wash into a beaker. Then punch
a hole in the filter and wash the CaCOg into same beaker,
cleansing the filter with HCl. Boil to expel CO2, and deter-
mine the lime as oxalate or caustic, and calculate the C02.
MAIN ANALYSIS.
Evaporate 10-20 gallons of the water to dryness in lai^
porcelain dishes (perfect dryness is not necessary). Treat the
residue in the dishes with water ; boil ; decant through a filter.
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THE CHEMISTS' MANUAL. 407
repeating the operation a number of times ; finally bring the
insoluble residue on the filter; wash with boiling water until
the residue gives only a faint trace of lithia in the spectroscope
(in case lithia is present).
Tbeatmbnt of the Kesedue. Insoluble in hot water (in
case lithia be not present in such quantity or in such a form
as not to be completely removed by hot water). Dissolve
residue in HCl; evaporate to dryness; add concentrated HCl
to the dry mass ; dilute with water and filter off residue, which
consists of Si02 and perhaps BaSO^, in case SO3 and BaO are
present in the water. Divide filtrate from Si02 into three
equal parts.
Treatment of first one-third part of solution for
PHOSPHORIC ACID.
Drive off excess of HCl from solution, and then remove it
entirely by boiling with concentrated HNO3 5 precipitate with
(NH4)2MoO^ and proceed as usual.
Treatment of second one-third part of solution for
IRON.
Precipitate the iron with NH^HO and NH^Cl, as usual ; filter,
wash, and re^lissolve the precipitate in HCl (or perhaps better
H2SO4); reduce with amalgamated zinc and Pt, determine
volumetrically with K2Mn208.
Treatment of third one-third part of solution for
BARYTA AND STRONTIA.
Dilute solution with water and add dilute H2SO4; boil
(enough acid should be added to precipitate a little lime, or
else some SrO may remain in solution). The precipitate, con-
sisting of (BaS04) SrS04, CaS04, should be treated with a
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408 THE CHEMISTS' MANUAL.
strong solution of (NH4)2C03, which converts the CaSO^ and
SrS04 into carbonates, while the BaSO^ is unaffected. The
carbonates are then dissolved away from the BaSO^i on the
filter with hot HCL The HCl solution, containing CaCl2 and
SrCla, is evaporated to drjTiess ; the chlorides converted into
nitrates; the calcic nitrate dissolved out by digesting with a
mixture of alcohol and ether. (See Fres.) The Sr(N03)2 is
dissolved in water and precipitated as SrSO^i with dilate
H2SO4.
All the precipitates should be examined in the spectroscope,
to ascertain if the operations have been perfect.
Treatment op the REsrouE, insoluble in hot water. In
case lithia be present in such quantity, or in such a form, as
not to be completely removed by boiling water, divide the
HCl solution into four equal parts, and take one part for the
determination of Kthia, using the other three as already stated.
Precipitate out with (NH4)2C03 and proceed according to
Fresenius, § 209, p. 564, in order to free the lithia from all
other bases precipitable by NaPOa-
Treatment of Water Solution resulting from the diges-
tion with hot water of the residue obtained by evaporation of
10 to 20 gallons. Evaporate to dryness, pulverize the residue,
and weigh ; divide into two portions, one for lithia, and one
for iodine and bromine.
DETERMINATION OF UTHIA.
Moisten the dry salt with HCl and evaporate on the water-
bath to dryness, in order to convert the lithia into the chloride.
Place the salt in a glass flask and agitate with absolute alco-
hol, decanting solution through a filter until the salt gives no
reaction for lithia in the spectroscope. Evaporate off the alco-
hol on a water-bath ; dissolve the residue in water. Treat the
solution thus obtained according to Fresenius (§ 101, p. 159),
in order to separate lithia.
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THE CHEMISTS' MANUAL.
409
DETERMINATION OF IODINE AND BROMINE.
Place the dry salt in a flask, boil on a water-bath repeatedly
with 70jg alcohol, until the salt gives no reaction for bromine
when treated with chlorine water and carbon disulphide.
Evaporate the alcoholic solution upon the water-bath ; dissolve
the residue in water. Add PdCla to a slight excess and heat ;
allow the whole to stand for some time, then filter out the
precipitated Pdlj, wash with warm water, dry and ignite.
Divide the filtrate from the Pdl into two equal portions.
Precipitate each with AgNOg. Filter off the AgCl + AgBr;
wash, dry, ignite one precipitate, and weigh. Place the other
precipitate of AgCl + AgBr in a beaker and digest in the heat
for 1 hour, with a solution of KBr(lKBr + 9H2O), whereby the
AgCl is completely converted into AgBr. From these data
estimate the amount of bromine in the first precipitate. About
as much KBr is required for the conversion as there is AgCl in
the precipitate. See "Wittstein Zeitschrift fiir Analytische
Chemie," 1863, S. 159.
CaCla + (NH^)HO MIXTURE.
60 grams CaCla in 250 c.c. HjO. Add 100 c.c. (NH^)HO,
boil, filter, add 100 c. c. (NH^)HO, dilute to 50Q c.c.
Note I. — In case H,S04 be present in a water, the residue insoluble in
HCl may contain BaSOf, and perhaps 81804. Treat residue with pure
NH4FI, to expel SiO,, weigh, and test the reeidae in the spectroscope.
GRAMS IN U. S. GALLON (231 cubic inches).
58318 1
116636 2
174»54 3
233272 4
291590 5
349908 6
408226 7
466t)44 8
524862 9
583180 10
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410
THE CHEMISTS' MANUAL.
METHOD OF CALCUUTING WATER ANALYSIS.
United States gallon contains 231 cu. inches = 58318 grains
of distilled H2O at 60° Fah.
Suppose an analysis of a litre of water gave the following.
Kequired the number of grains of each substance in a gallon.
1 Litre. Grains in a Ganon.
Na,0 0.031 1.807
CaO 0.173 10.089
CI 0.172 10.030
SiO, 0.250 14.579
Multiply each substance by 58318 and divide each by 1000.
TO CALCULATE HOW ACIDS AND BASES COMBINE.
ORDINARY DRINKING WATERS.
1 U. S. Gallon.
Na^O 0.336
K,0 0.097
CaO 0.988
MgO 0.524
CI 0.243
SO, 0.322
SiO, 0.621
Organic and volatile matter. 0.670
COj (calculated) 1.302
Total 5.093
Combfoed.
K,S04 179
NaCl 400
Na.SO^ 268
CaSO^ 156
CaCOj 1.650
MgCO, 1.100
SiO, 631
Org. and volatile matter. . .670
Total 5.039
Ist. Give SOg to K^O.
2d. " a " remainder K,0.
3d. " " " Na.
4th. " •' " Mg.
5th. " " « Ca.
6th. " SOa " Na,0.
5.093 — .054 (amount of oxygen in Na used to make NaCl) = 5.089.
7th. Give SOj to CaO.
8th. « " " MgO.
9th. " COj " Na.O.
10th. " " " CaO.
11th. " " " MgO.
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THE CHEMISTS' MANUAL. 411
ANALYSIS OF A MINERAL WATER.
HATHORN SPRING, SARATOGA SPRINGS.
By C. F. Chandler,
Sodic Chloride 509.9C8 grainB,
Potaasic Chloride 9.597 • '
Sodic Bromide 1.634 *•
Sodlc Iodide 198 "
Calcic Fluoride A trace.
Lathic Dicarbonate 11.447 "
Sodic Dicarbonate 4.288 "
Magnesic Dicarbonate 176.468 "
StroDtic Dicarbonate A trace.
Baric Dicarbonate 1.737 "
Ferrous Dicarbonate . . 1 .128 "
Potaasic Sulphate None.
Sodic Phoephate 006 "
Sodic Dilx>rate A trace.
Aluminic Oxide 131 "
Silicic Oxide 1.260 "
Organic Matter A trace.
Total Bolid contents. 888.403 grains.
Carbonic oxide (COg) in 1 gal., 375.747 inches ; density 1.009.
ANALYSIS OF THE ATLANTIC OCEAN
(By Von Bibba)
AND OF THE DEAD SEA
(By the Hebepathb).
Atlantic Ocean. Dead Sea.
Specific Gravity 1.0275 1.17205
SodicChloride 1671.34 6702.73
Potassic Chloride — 682.63
Ammonic Chloride — 8.35
Calcic Chloride — 1376.75
Magnesic Chloride 199.66 4457.23
Aluminic Chloride — 31.37
Ferruos Chloride Trace 1.50
Manganous Chloride — 8.35
SodicBromide 31.16 156.53
Carried forward 1903.18 13416.61
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412 THE CHEMISTS' MANUAL
Attantlc Ocean. Dead Sea.
Brought forward 1903.18 13416.61
Sodic Iodide Trace Trace.
Potaesic Sulphate 108.46 —
Magnesic Sulphate 34.99 —
Calcic Sulphate 93.80 88.07
Sodic Phosphate Trace —
Calcic Carbonate Trace Trace.
Silver Trace. , —
Copper Trace —
Lead Trace —
Arsenic Trace —
Silicic Oxide Trace Trace.
Organic Matter Trace 84.59
Bitumen — Trace.
Total in 1 U. S. gallon. . . . 2m93"gr 13489.17^
Per cent, by weight 3.669 19.733
Water..... 96.431 '. 80.267
Total mOOO 10000
Weight of 1 gallon. . .59922. grs 68352. gra
POTABLE WATER ANALYSIS.
(J] CJum, Society, London, vol. xxi, p. 771.)
I. TOTAL SOLIDS.
Evaporate \ litre to dryness rapidly at 100° C. to constant
weight.
II. ORGANIC CARBON.
To 2 litres in a stoppered bottle add 60 e.c. saturated solution
sulphurous acid ; J of this (1 litre) sulphurized water is boiled
for two or three minutes (unless it contains a considerable
amount of carbonates) ; then add 0.200 grams sodic sulphite to
secure saturation of SO3 formed during subsequent evapora-
tion. To secure expulsion of N, existing as nitrate, add 2 drops
FeCl2 or Fe2Cl5. Then evaporate boiled water to dryness in
glass capsule of 100 c.c. capacity, keeping capsule without a
lip, covered with paper stretched on a hoop to keep out dust ;
there should be no (NH4)H0 in the atmosphere ; when dry, a few
grams plumbic chromate, powdered, are added, and triturated
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THE CHEMISTS' MANUAL. 413
with contents in an agate mortar ; when the mixture is com-
plete the contents are transferred to a combustion tube six-
teen inches long sealed at one end, and the capsule rinsed with
PbCrO^, and the tube charged with CuO and about three
inches bright copper turnings. Then draw out open end and
connect with a Sprengel pump, letting the ends of glass tubes
touch inside of rubber tube, and plunge the joint under water.
The furnace is lighted around the forward end of combustion
tube and the pump worked for five or ten minutes. The de-
livery end of the pump dips into a mercury bath, and a tube
filled with mercury is placed over it. The combustion is con-
ducted as usual. When the organic matter begins to bum,
the operation proceeds slowly until the vacuum is impaired or
carbonic oxide will be formed. Combustion lasts forty-five
minutes to one horn*. Generally no gases will have passed
into the mercury tube unless the residue is very rich in organic
matter- The pump is now worked for ten minutes, when all
the gases will be transferred to the inverted tube. The gases
are COg, N, and NOg. (For separation and determination of
these, see J. Chem. Soc., vol. vi, p. 197.)
The weights of carbon and nitrogen are deducted from the
volumes of these gases, expressed in 100.000 parts of water.
The nitrogen may have been present as organic nitrogen or a
constituent of NH3. The latter is determined in the water
directly by Nessler's test. The nitrogen in this deducted
from total nitrogen = organic nitrogen.
Note. — CO^ is detennined by solution of K,0 of 1.8 specific gravity, and
oxygen by solation of pyrogallic acid (1 add to 6 water).
A correction is made by boiling distilled water for 24 hours
with alkaline potassic permanganate, and then distilling it;
refusing the distillate as long as it shows any reaction for
(NH4)H0 by Nessler's test, and then slightly acidulating it
with H2SO4., and rectifying it. A litre of this is acidified with
15 c.c. H2SO4, containing about 1.100 grams recently ignited
NaCl, and evaporated. The residue must now be burned in
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414
THE CHEMISTS' MANUAL.
Fig. 2.
PbCrO*.
IhiO made by oxidizing pure sheet copper
muffle — not from Cu2N0a.
PbCrO^ to be heated to redness for 2 hours,
1 transferred to stoppered bottle.
Mkboubt Tbough. '
vacuo, and the carbon and nitix)gen obtained deducted from
that obtained from the water analyzed.
N. B. — See J. Ch. Soc, London, vol. xxi, for apparatus for measuring
gases, also without absorbing same, and tables for calculating weight of
nitrogen, ete. See particularly Russell on Gr. Analysis, J. Chem. Soc,
London, vol. xxi, p. 128.
3. NITRATES AND NITRITES.
Tlie solid residue of ^ litre of water is treated with a small
quantity of distilled water — a very slight excess of AgjSO^
added, to convert chlorides into sulphates. The filtered liquid
concentrated in a small beaker to 2 or 3 c. c. This is trans-
ferred to a tube with a cup and stop-cock (see Fig. 2) filled
with mercury and standing in a mercury-trough — the beaker
being washed once or twice with a little recently-boiled dis-
tilled water, finally with pure H2SO4 in greater volume than
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THE CHEMISTS' MANUAL. 415
solution and rinsings. If air gets in, push tube down in mer-
cury and draw it out. Finally, close the tube firmly at the
bottom with the thumb, and shake ; resisting the flowing out
of the mercury between the acid liquid and the thumb. In 3
to 6 minutes the reaction is complete, when the gas is trans-
ferred to a measuring apparatus over mercury.
Half the volume of NO2 in tube = N ; the
weight calculated from the volume. Miller [1
proposes to estimate the nitrates by the v\
KaMnaOg solution, of which 1 c.c. = 0.00237
grams N2O3. He adopts Pugh's process for
nitrates. Or, J. Ch. Soc., vol. xii, p. 35.
MILLER'S METHOD OF KgMngOa.
lUj
1 c.c. =0.0001 gram oxygen requiring 0.395 gram to
1 litre water. Test it with a solution of oxalic acid containing
0.7875 gram to 1 litre water ; 100 c.c. of this, warmed with a
very dilute solution of H2SO4 should decolorize 100 c.c.
KgMngOe solution. 250 c. c. of the water to be tested is
placed in a flask with 3 c.c. dilute HjSO^ (1 acid -f 3 water).
Add the KaMngOs solution in successive portions of 0.5 c.c.
until the color disappears, and until after the last addition no
change takes place for one-half hour. After it is found that
no change takes place, the last 0.5 c.c. added is subtracted as
excess.
ORGANIC MATTER IN WATER.
(Permanganate Test)
Solution made is that 1 c.c. yields 0.0001 gram oxalic
acid, then 1 litre yields 0.100 gram oxalic acid.
H2C2O4 and 2H2O = 126 requires 1 At. 0 = 16.
16 : 126 : : 0.100 : .7875 = oxalic acid.
Then .7875 oxalic acid requires 0.100 oxygen.
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416 THE CHEMISTS' MANUAL.
Then .7875 oxalic acid dissolved in 1 litre HgO require for
each c.c. ^^^,j = .0001 oxygen. Permanganate is diluted until
1 c.c. oxidizes 1 c.c. oxalic acid solution; so 1 c.c. Kg.MnjOe
carries 0.0001 available oxygen.
AMMONIA.
If the (NH4)H0 be not alone one part in 10,000,000, which is
obtained by distillation alone or with NagCOs, use Iladow's
modification of Nessler's test. If it be alone this, Nessler's
test must be applied directly to the water. The water must
be colorless, free from carbonates of magnesia and lime. Any
tint in a column six or eight inches deep is fatal. In this case
add a few drops of concentrated solution of calcic chloride to
one-half litre water, and precipitate with slight excess NajCOs ;
filter after an hour ; use 100 c.c.
of the filtrate. To this volume
1 C.C. of the Nessler solution is
added, and the color observed.
See Miller on Potable Waters,
J. Ch. Soc, vol. xviii, p. 125.
Use a cylinder of such diameter
that 100 c.c. form a colunm seven
inches deep ; place it near a window.
AMMONIA.
(MnjiER's Method)
Into a capacious retort one litre water is introduced, and
the retort connected with a Liebig's condenser ; 25 c.c. of
baric hydrate is then added ; 250 c. c. water distilled over.
The residue in the retort is filtered and separated from salts
of baryta (carbonate and sulphate) and evaporated for deter-
mination of nitrates by Pugh's method. The distillate is
divided into two equal portions ; one for Nessler's test, as
practised by Hadow.
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THE CHEMISTS' MANUAL. 417
NESSLER^S SOLUTION.
Make a concentrated solution of 40 grams corrosive subli-
mate (HgCl2). Dissolve 62.5 grams Kl in 300 c.c. water, and
add to this the mercurial solution until the mercury iodide
ceases to be dissolved on agitation. Next dissolve 150 grams
KjO in its own weight of water and add it gradually to the
iodized mercurial solution, stirring while mixing ; then dilute
to one litre ; let it stand for a day or two until the brown
color disappears, and it becomes clear. Decant the cleai*
liquid.
About 3 c.c. of the above solution is added to the half of
the distillate, same as one-half litre. If (NH4)H0 be present,
a yellow color will appear; if the NHg be ^^nrirnnr P^^? make
a solution of NH^Cl 0.317 grams to one litre of water, which
is equal to 0.1 gram NH3 in one litre.
Place 3 C.C, of this solution in a beaker of same size used for
the distillate ; dilute with 150 c.c. water ; add 3 c.c. teat Uqiior.
If the colors coincide then, calculate the quantity of NH3.
When the NH3 exceeds 0.6000 milligram per litre, it must
be determined by neutralizing with a test acid solution. The
other one-half of the distillate is used. The solution contains
2.882 grams HaSO^ in one litre water; 1 c.c. = 0.001 NH3,
as usual with litmus solution.
NITRIC ACID.
(FuCH's Zeloehi AtioI. Chem,, vi, 175.)
Concentrate two litres water, adding KgMngOg to pink color.
Filter; concentrate fluid ; add pure HjSO^ and distil into a
flask containing BaC03 suspended in HjO until HjSO^ goes
over. Filter and determine the Ba existing as Ba(N03)2 and
BaCl2. Determine CI elsewhere and calculate the HNO3.
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418 THE CHEMISTS' MANUAL.
TOTAL RESIDUE.
(Wanklyn.)
Evaporate 100 c. c. in a small platinum dish holding about
125 C.C. The dish is heated, covered, to 130** C, cooled on a
thick piece of cold iron (still covered). Evaporate over steam
so as not to allow the dish to come in contact with the boiling
water. Use a can with a funnel in it, the dish standing in the
funnel. When dry, wipe, transfer to air-bath ; dry at 130° C,
at first with lid on, afterwards without it ; cool the dish, cov-
ered, as at first, on cold iron, and weigh. If the air-bath is at
a temperature of 130° when the dish is put in, the determina-
tion can be made in 1\ hours. Liability to error on account
of dust, destruction of organic matter on account of long diy-
ing, avoided.
SOAP TEST.
Dissolve marble in HCl; dry; fuse in a weighed crucible;
weigh. Difference = CaCla- Dissolve with water ; from
known! weight calculate water necessary to make solution so
that 1 litre = 1.110 grams CaCl2 ; each cubic centimetre =
0.001 = 1 c.c. CaCla = 1 c.c. CaCOa-
Take 2 parts lead plaster and 1 K2CO3 ; pound together a
little at a time. Extract with 90j? alcohol, 30 times as much
as the lead plaster ; allow to stand for some time ; filter ; dilute
with its own volume of water.
If this cannot be obtained, use good potash soap. Measure
accurately 10 c. c. of the soap solution, put it into a bottle
with 70 c.c. w^ater, and add CaCl2 solution until frothing stops.
Shaking up properly, from this calculate how much dilution is
necessary to make 17 c. c. of soap solution consume 16 c.c.
CaCla solution ; dilute accordingly with alcohol of 40^?, and
verify. [N. B. — 17 c. c. standard soap test should neutralize
16 c. c. of standard CaClg solution, in presence of 70 c. c. pure
water. Each c. c. of soap solution will then be equal to 1 mil-
ligram CaCOg, or its equivalent, or 0.010 grams per litre.]
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THE CHEMISTS' MANUAL. 419
Take 70 c. c. of the water, put it into a bottle, add soap
solution until it lathers ; each c. e. of soap = 1 gram in an
English gallon. To get it in litres, take 100 c.e. water ; each
C.C. soap = 10 milligrams CaCOg per litre. (This is not abso-
lutdy exact.)
K more than 17 c.c. of soap is required in 70 c.c, dilute
the water with its own volume of distilled water, and go on,
etc. Wanklyn claims that 70 c.c. distilled water have a soap-
destroying power = 1 milligram CaCOs.
NITRATES AND NITRITES.
100 c. c. water are introduced into a non-tubulated retort ;
50-70 c. c. solution of NaHO added (100 grams NagO to 1 litre
water).
Distil until not more than 100 c. c. remain, and until no
NH3 comes over. Now cool, and introduce a thin sheet of
aluminium.
Then incline neck upwards ; close it with a cork through
which passes the narrow end of a small tube 2 or 3 inches
long, filled with broken tobacco clay-pipe moistened with
dilute HCl, connected with a second tube holding pumice sat-
urated with H2SO4 ; allow to stand for some hours ; then wash
the contents of the pipe-clay tube back into the retort with a
little water and distil down one-half into 80 c.c. water. Make
the distillate up to 150 c.c. To 50 c.c. of this add Nessler's
solution.
If the color is not too strong, the estimation may be made
directly. If it is too strong, dilute the remainder, test, etc
TO DETERMINE NH3 BY TITRATION.
Use 1 litre evaporated to small bulk ; treat in same way as
above, receiving the distillate in stanchird acid mstead of
water. Soda may be purified from nitrates by dissolving
aluminum in cold solution, and boiling.
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420 THE CHEMISTS' MANUAL.
WITHOUT DISTILLATION.
Prepare soda by dissolving 100 grams solid soda, diluting to
1 litre ; dissolve a very little Al in it, to decompose nitrates.
1st. Then to 200 c. c. of this add 200 c. e. of the sample of
water and add a little more Al. This contains original amino-
nia and that from nitrates.
2d. Take 200 c.c. of the soda ley, dissolve in it a little Al as
before, then add 200 c.c. water, and allow to subside. This
will have the nitrates unreduced. Decant, and determine
NH3 by Nessler's solution.
Test in both 1st and 2d. Diflference = nitrates.
N.B. — To both samples of water, before mixing with soda
ley, add a little CaCl2 to get an appreciable precipitate.
ANALYSIS OF THE -CROTON WATER."
(Calculated for 100,000 parts water.)
CaH,C,0« (CiacJc Bicarbonate) 4.58
MgHjCjOe (Magneaic Bicarbonate) 855
SiO, 1.05
Fe,0, Trace.
A1,0, Trace.
CaSO^ 0.26
Na,S04 044
K,S04 0.30
Naa 0.68
Organic Matter 1 . 13
Total 11.64
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THE CHEMISTS' MANUAL.
421
PURITY OF CITY WATERS.*
Impurities contained in one wine gallon of 231 cubic inches expressed in
grains.
Crrr.
SOUBOK.
INOBOAKIO
Mattxb.
Oboahio
AND
YOLATILB
Mattxb.
Total
New York
Groton. 1869
4.11
88.95
8.87
4.68
2.98
2.80
2.40
8.47
6.09
46 88
5.60
12.18
12.02
474
5.62
1.77
15.55
90.38
7.88
14.45
64.55
0.67
4.59
0.59
2.86
0.55
1.20
071
2.81
1.84
2.88
0.96
1.80
1.28
1.58
1.06
1.84
0.88
9.59
1.00
2.18
4.88
478
Brooklyn
Jersey City
Trenton
Philadelphia
Boston
Well. 8th Ave
Ridgewood, 1869
Passaic River
48.54
8.92
7.44
Delaware River
Schuylkill River
Cochituate Lake
Hydrant
8.48
8.50
8.11
Albany
Troy
Schenectady
Utica
10.78
Hydrant
7.48
Well, State St
Hydrant
49.21
6.46
Syracuse
Rochester
Cleveland .......
New Reservoir
Genesee River
Lake Erie
18.98
18.26
6.27
Chicago
Dublin
Lake Michigan
Lough Valley
Thames River
Well, LeadenhaU St. . .
River Seine
a68
8.11
London
16.88
M
99.97
Paris
8.88
AmntArdRin .
River Vecht
16.58
If
Well
68.98
* Taken from Lee. on Mineralogy by T. Egleston, E. M.
COAL ANALYSIS.
In the ordinary analysis there is determined moisture;
volatile and combustible matter; fixed carbon (coke), and
sulphur.
(a.) Determination of moisture.* Pulverize the coal finely ;
heat one or two grains in a covered platinum or porcelain
crucible, fifteen minutes in an air-bath at 212° to 240° F.
Cool and weigh, repeat until weight is constant or begins to
rise. Loss = moisture.
(J.) Determination of volatile and combustible matter.
* See " Notes on Assaying," p. 95, by Ricketts, PIlD.
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423 THE CHEMISTS' MANUAL.
Heat the same crucible, with contents, to bright redness, over
a Bunsen burner or alcohol lamp, exactly three and one-half
minutes, and then three and one-half minutes over a blast-
lamp. Cool and weigh. Loss = volatile and combustible
matter. This includes one-half of sulphur of any sulphide of
iron contained in the coal.
(c.) Fixed carbon. Heat over the burner until the ash is
white and constant weight. Loss = fixed carbon and one-half
the sulphur from the sulphide of iron.
(d.) The sulphur may be determined as follows : "Weigh out
one to two grams of the finely pulverized coal and oxidize
with nitric acid and potassic chlorate in a fiask until action
ceafies ; then filter and wash. If the residue contain sulphur,
dry and weigh it ; then ignite and weigh. The difierence will
be the sulphur unoxidized ; add to this a little hydrochloric
acid, and then baric chloride in slight excess ; heat for a few
moments and allow the particles to settle. Pour oflp the
liquid through a filter and wash with dilute hydrochloric acid,
then with water. Dry and ignite the residue in a porcelain
crucible ; multiply the weight of the precipitate less that of
the filter-ash by xif.T I ^^^ product equals the sulphur in the
sample taken.
The following analyses are of different semi-bituminous
coals (by Pierre de Peyster Ricketts) :
Moisture 8.810 0.965
Volatile Combustible Matter 27.800 80.111
Fixed Carbon 61.965 61.088
Ash 7.425 7.829
Sulphur 8.863 1.847
27.300 minus -Mj^ and 30.111 mmus -^^ gives the cor-
rect amount of volatile matter. 61.965 minus -^^^ and
61.033 minus -^4j^, the correct amount of fixed carbon.
Phosphorus not determined.
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THE CHEMISTS' MANUAL. 428
CLAY ANALYSIS.
I. May contain AlgOg, 45102 + 6H2O, with variable quan-
tities of KjO, MgO, FeO, MnO, feldspar, sand, etc.
Dry a quantity of clay at 100° C, and weigh ; ignite and
weigh again. Loss = HjO. Treat then with H2SO4 (concen-
trated) ; heat ; evaporate off excess of acid ; dissolve in con-
centrated HCl, and filter off the SiOj (weigh). If the clay
contain an admixture of sand or feldspar, the silica is dissolved
in a boiling concentrated solution of sodic carbonate, which
leaves the sand and feldspar undissolved.
The hydrochloric acid solution is considerably diluted, and
gradually neutralized with sodic carbonate. Precipitate out
feme and aluminic oxide, then manganous, calcic, and mag-
nesic oxides remain in the solution as dicarbonates.
The Fe203 and AI2O3 are then separated, as also the man-
ganous, calcic, and magnesic oxides.
II. The clay is fused with three times its weight of potassic
and Bodic carbonate, the fused mass dissolved in dilute HCl,
the solution evaporated to dryness, the residue dissolved in
water containing HCl, and the solution filtered off. The sep-
aration of the other bases contained in the solution is then
effected as in I.
III. For the determination of the alkali a separate portion
of the clay is decomposed by ftision with baric hydrate or car-
bonate ; the baric oxide and the other bases are precipitated
fi"om the solution by a mixture of ammonic hydrate and car-
bonate ; after gently heating, the solution is filtered off, the
solution evaporated, and the residue ignited, when potassic and
sodic chloride are left, which may be separated if required. —
(From Wohler's Mineral Analysis.)
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424 THE CHEMISTS' MANUAL.
ANALYSIS OF CLAYS.
7%e hard, dark dap used for tite substance of the Mount Socage fireJrriek,
(John M Obdwat.)
S iUca «50.457
Al umina 86.904
Protoxide of Iron. 1.504
Oxide of Manganese Trace.
Lime 0.133
Magnesia. 0.018
Water and Organic Bifatter 12.744
Potash Inappreciable.
100.760
GUNPOWDER ANALYSIS-
I. For the estimation of moisture, 5 or 6 grams of powder
are dried over H2SO4, or in the air-bath at 100®.
II. A similar quantity of powder is moistened with water,
triturated in a mortar, rinsed into a filter, and thoroughly
washed. The solution of nitre thus obtained is evaporated to
dryness in a small weighed porcelain dish, the dry residue
heated for some time to 200°, or even until the nitre fuses,
and its weight determined.
III. In order to determine the sulphur 6 grams are inti-
mately mixed with 5 grams anhydrous NaaCOa, 5 grams of
nitre, and 20 grams of decrepitated NaCl, and the mixture
•heated to redness in a platinum crucible. When cool, the
mass is dissolved in water, the solution slightly acidified with
HNO3, ^^^ ^^® H2SO4 precipitated with BaClg.
The amount of carbon may be inferred by difference. In
order to determine its quality, and to ascertain whether it has
been completely or incompletely carbonized, the mixture of
sulphur may be separated with carbon disulphide, which dis-
solves the sulphur and leaves the carbon, which must be well
washed and dried.
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425
ANALYSIS OF GUNPOWDER.
GVKTOWDSBS.
Chabooax..
StTLPHUB.
NiTRB.
AUTHOBTPT.
Swedish war powder
Hessian artillery powder
musket "
French sporting *'
English " •'
Russian powder
Chinese "
9.0
10.7
10.7
13.5
13.7
17.7
23.1
16.0
15.1
15.6
9.6
10.1
11.7
15.4
75.0
74.2
73.7
76.9
76.2
70.6
01.5
Meyer.
Prechtl.
Ure.
Meyer.
Prechtl.
SCHEME FOR THE ANALYSIS OF GLASS.*
Two analyses are made, one by fusion with an alkaline
carbonate, for the determination of silicic acid ; the other by
decomposing the glass with hydroflaoric acid, in order to esti-
mate the alkali.
I. The very finely-powdered glass is fused with three times
its weight of potassic and sodic carbonate ; the mass is then
softened with water, dissolved in dilute hydrochloric acid,
evaporated to dryness, redissolved in water, acidulated with
hydrochloric acid, and the silica filtered ofl^ and washed.
From the solution, the small accidental impurities of ferric,
manganous, and aluminic oxides which are usually contained
even in white glass, are precipitated by ammonic hydrate, after
the solution has been mixed with some chlorine water to per-
oxidize the manganous oxide.
The lime is afterwards precipitated by oxalic acid, and the
solution filtered from the calcic oxalate is tested for magnesia,
which may, moreover, have been precipitated with the alu-
minic oxide.
If the glass contain plumbic oxide, that metal is precipitated
by sulphydric acid from the solution filtered from the silicic
acid.
* Mineral Analysis, W5hler, p. 209.
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THE CHEMISTS' MANUAL.
II. For the determination of the alkalies, a second quantity
of verj' finely-powdered glass is decomposed by hydrofluoric
acid, or by ignition with baric carbonate.
In the last case after fusion the mass is dissolved in water,
evaporated to dryness with a little hydrochloric acid, then dis-
solved again in water and the insoluble silica filtered off, when
a solution will be obtained from which may be determined the
alkalies, as also the other bases if necessary.
The following table contains the analysis of different speci-
mens of glass :
ANALYSIS OF GUSS.
Pale-green Glass used for Medical Bottles and Chemical Apparatus.*
Bottle Glam.
MBDICAL-BOTTLB Gl.Afl8.
K.O t
CaO
M^)
MnO
Fe-O,
ai
T.2
4.0
80
60.0
0.4
8.8
0.9
90.7
0.6
7.S
10.4
60.4
18.0
7.0
0.4
4.4
6.8
59.6
6.48
R74
6.9
10.6 lOJS 8.0
Z = 1 i«
10.0 16.« 18.0
- — 1 0.6
0.8 1.9 —
1.6 2.5 . 1.6
8.0 4.5 1 8.6
71.6 62.6 69.6
16.4
1&6
a7
ife?':::::::.::.:.:::::::
P,o\
6.01 14.0 !
58.66 466 !
"" 1 " 1
14
61.0
90.0 .100.0
99.4
100.00, 100.00
1 i
Vt,0
97.4 99.4 ) 99.8
The last four analjeeo are by Berthier.
ANALYSIS OF WINDOW GLASS.
a
b
C
d
e
1
if
Na.O
15.«
13.81
1.89
60.66
11.80
17.26
2.90
69.26
19.88
16.17
2.40
68.56
17.T0
9.66
4.00
68.66
18.7
7.8
10.0
68.6
m
14.8
76
68.0
11.1
Oa6
AUOa
SiOa
12.5
7.4
69.0
100.00
100.00
100.00
100.00
100.00
100.00
1
lOOJIO
^ to/ is French ; g^ English ; / and g^ the hardest and most
infusible ; J, the next ; d^ the softest and most easily fiised of
* Watt's Die. Cfaem., Article Glass.
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THE CHEMISTS' MANUAL^ > - ■ » .:^^4^'
the whole. In France, a mixture is used of 100 parts of quartz-
sand with between 30 and 40 parts of dry sodic carbonate (or
as much sulphate with charcoal) and 30 to 40 parts of calcic
carbonate (Dumas). Window -glass may be approximately
represented by the formula Na20.2Si02 + Ca0.2Si02.
CHLORIMETRY.
Chlorimetry has for its object the determination of the
available chlorine in the ^^ bleaching pow(fer^^ of commerce.
Bleaching powder is called " chloride of lime ; " it is a mix-
ture of calcic hypochlorite, calcic chloride, and calcic hydrate.
The following method of chlorimetry* is based upon the
conversion of arsenious acid into arsenic add ; the conversion
is effected in an alkaline solution. Potassic iodide starch-
paper is employed to ascertain the exact point when the re-
action is completed.
(a.) PREPARATION OF POTASSIC IODIDE STARCH-PAPER.
(Fre^enius, § 212.)
Stir 3 grams of potato starch in 250 c.c. of cold water, boil
with stirring, add a solution of 1 gram potassic iodide and
1 gram crystallized sodic carbonate, and dilute to 500 cc^
Moisten strips of Swedish paper with this fluid, and dry. Keep
in a closed bottle.
(&.) PREPARATION OP SOLUTION OF ARSENIOUS ACID.
Dissolve 4.436 grams of pure arsenious acid and 13 grani^
pure crystallized sodic carbonate in 600-700 c.c. of water,
with the aid of heat; let the solution cool, and then dilute to
one litre. Each c.c. of this solution contains 0.004436 grams
arsenious acid, which corresponds to 1 c.c. chlorine gas of O''
and 760 m.m. atmospheric pressure.
♦ By A. Penot, Dingler*8 Polytech. Jour, 127, 184
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428 THE CHEMISTS' MANUAL.
PREPARATION OF SOLUTION OF "CHLORIDE OF LIMR"
Weigh 10 grams of " chloride of lime," triturate finely with
a little water, add gradually more water, pour the liquid into
a litre flask, triturate the residue again with water, and rinse
the contents of the mortar carefully into the flask ; fill the
latter to the mark, shake the milky fluid and examine it at
once. 1 c.c. of this solution = 0.01 gram chloride of lime.
(c.) THE PROCESS.
Put 50 c,c. of solution of " chloride of lime" in a beaker,
and from a 50 c.c. burette add slowly, and at last drop by
drop, the solution of arsenious acid, with constant stirring,
until a drop of the mixture produces no longer a blue-colored
spot on the iodized paper. The number of ^ c.c used indi-
cates directly the number of chlorometric degrees. Suppose
40 C.C. of arsenious acid solution were used, the quantity of
'* chloride of lime" used in the experiment contains 40 c.c of
chlorine gas. Now the 50 c.c. of solution employed corresponds
to (1 C.C. = 0.01 gram) 0.5 gram of chloride of lime; therefore
0.5 gram of chloride of lime contains 40 c.c. chlorine gas;
therefore 1000 grams contain 8000 c.c. = 80 litres of chlorine
gas.
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ifflrjanic Snalgsis.
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THE ELEMENTARY OR ULTIMATE
ANALYSIS OF ORGANIC COMPOUNDS.
{From F0WNB8' Chsmistry, London, 1872.)
Organic componnds contain, for the most part, only a small
number of elements. Many consist only of carbon and hydro-
gen. A very large number, including most of those which
occur ready -formed in the bodies of plants and animals, consist
of carbon, hydrogen, and oxygen ; others consist of carbon,
hydrogen, and nitrogen. Others, again, including most of the
proximate principles of the animal organism, consist of four
elements, carbon, hydrogen, oxygen, and nitrogen. Some
contain sulphur, phosphorus, chlorine, and metallic elements ;
in fact, artificially prepared carbon compounds may contain
any elements whatever. Moreover, even those which contain
only a small number of elements often exhibit great complexity
of structure, in consequence of the accumulation of a large
number of carbon-atoms in the same molecule.
DETERMINATION OF CARBON AND HYDROGEN.
The quantities of these elements are determined by heating
a known weight of the body to be analyzed in contact with
some easily-reducible metallic oxide, black oxide of copper
being the substance generally used. The organic body then
undergoes complete combustion at the expense of the oxygen
of the cupric oxide, the carbon being completely converted
into carbonic oxide, and the hydrogen into water. These
products are collected and their weights determined, and from
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432 THE CHEMISTS' MANUAL.
the data thus obtained the quantities of carbon and hydrogen
present in the organic substance are calculated. When nothing
but carbon and hydrogen, or those bodies together with oxy-
gen, is present, one experiment suflBces; the carbon and
hydrogen are determined directly, and the oxygen by differ-
ence.
The substance to be analyzed, if solid, must be carefully
freed from moisture. If it will bear the application of a mod-
erate heat, this desiccation is very easily
Pig. 1. accomplished by a water or steam bath ; in
other cases, exposure at common tempera-
tures to the absorbent powers of a lai^
surface of oil of vitriol in the vacuum of an
air-pump must be substituted.
The dried powder is weighed in a narrow
open tube, about 2^ or 3 inches long ; the
tube and substance are weighed together,
and, when the latter has been removed, the
tube with any little adherent matter is re-weighed. This
weight, subtracted from the former, gives the weight of the
substance employed in the experiment. As only half a gram
(5 or 6 grains) is used, the weighings should not involve a
greater error than a milligram (or ^ J^ part of a grain).
The cupric oxide is best made from the nitrate by complete
ignition in an earthen crucible ; it is reduced to a powder and
reheated just before use, to expel hydroscopic moisture, which
it absorbs, even while warm, with avidity. The combustion
is performed in a tube of hard, white Bohemian glass, having
a diameter of 0.4 or 0.5 inch, and varying in length from 14
to 18 inches; this kind of glass bears a moderate red heat
without becoming soft enough to lose its shape. One end of
the tube is drawn out to a point, afl shown in the figure, and
closed; the other is simply heated, to fuse and soften the
sharp edges of the glass.
The tube is now two-thirds filled with the yet warm cupric
oxide, nearly the whole of which is transferred to a small por-
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THE CHEMISTS' MANUAL. 433
fiQ. 2.
SZZ)
celain or Wedgwood mortar, and very intimately mixed with
the organic subetance. Tlie mixture is then transferred to the
tube, and the mortar rinsed with a little fresh and hot oxide,
which is added to the rest ; the tube is lastly filled to within
an inch of the open end with oxide from the crucible. A few
gentle taps on the table suffice to shake together the contents,
so as to leave a free passage for the evolved gases from end to
end. The airangement of the mixture and the oxide in the
tube is represented in the above figure.
The tube is then ready to be placed in the fiimace or chauf-
fer ; this, when charcoal is the fuel employed, is constructed
of thin sheet-iron, and is furnished with a series of supports of
equal height, which seiTe to prevent flexure of the combustion-
tube when softened by heat. The chauffer is placed upon flat
bricks or a piece of stone, so that but little air can enter the
grating, unless the whole be purposely raised. A slight incli-
Fio. 3.
nation is also given towards the extremity occupied by the
mouth of the combustion-tube, which passes through a hole
provided for the purpose.
To collect the water produced in the experiment, a small
light tube of the form represented in Fig. 4, or a U-tube, as in
Fig. 7, filled with fragments of spongy calcic chloride, is
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434
THE CHEMISTS' MANUAL.
attached by a perforated cork, thoroughly dried, to the open
extremity of the combustion-tub^. The carbonic oxide is ab-
sorbed by a solution of potassic hydrate, of specific gravity 1.27,
which is contained in a small glass apparatus on the principle
of a Woulfe's bottle, shown in Fig. 5. The connection
Fig. 4.
Fio. 6.
between the latter and the calcic-chloride tube is completed
by a little tube of caoutchouc, secured with silk cord. The
whole is shown in Fig. 6, as arranged for use. Both the
calcic-chloride tube and the potash apparatus are weighed
with the utmost care before the experiment.
Pig. 6.
DBA WING OF THE WHOLB ABRANGEMEZVT.
The tightness of the junctions may be ascertained by sh'ghtly
rarefying the included air by sucking a few bubbles from tlie
interior through the liquid, using the dry lips, or, better, a
little bent tube with a perforated cork ; if the diflerence of
level in the liquid in the two limbs of the potash-apparatus be
preserved for several minutes, the joints are perfect. Ked-hot
charcoal is now placed around the anterior portion of the com-
bustion-tube, containing the pure cupric oxide; and when
this is red-hot, the fire is slowly extended towards the farther
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THE CHEMISTS' MANUAL. 4:35
extremity by shifting the movable screen represented in the
drawing. The experiment must be so conducted, that a uni-
form stream of carbonic oxide shall enter the potash-apparatus
by bubbles which may be easily counted ; when no nitrogen
is present, these bubbles are, towards the termination of the
experiment, almost completely absorbed by the alkaline liquid,
the little residue of air alone escaping. In the case of an
azotized body, on the contrary, bubbles of nitrogen gas pass
through the potash-solution during the whole process.
When the tube has been completely heated from end to end,
and no more gas is disengaged, but, on the other hand, absorp-
tion begins to be evident, the coals are removed from the
ferthest extremity of the combustion-tube, and the point of the
latter broken off. A little air is drawn through the whole
apparatus, by which the remaining carbonic oxide and watery
vapor are secured. The parts are, lastly, detached, and the
calcic-chloride tube and potash-apparatus re-weighed.
Pig.
The mode of heating the combustion-tube with red-hot char-
coal is the original process, and still extensively employed, the
construction of the furnace being most simple, and charcoal
everywhere accessible. But since the use of coal gas has been
universally adopted in laboratories, many contrivances have
been suggested, by means of which this convenient fuel may
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436 THE CHEMISTS' MANUAL.
Fig. 8. Fio. 9.
be employed also in organic analysis. An apparatus of this
kind * is the one represented in Fig. 7, in which the combus-
tion-tube is heated by a series of perforated clay burners.
These are fixed on pipes provided with stopcocks, so that the
gas may be lighted according to the requirements of the case.
The stopcocks being appropriately adjusted, the gas bunis on
tlie surface of the burners with a smokeless blue flame, which
renders them in a short time incandescent. The construction
of this furnace is readily intelligible by a glance at Figs. 8
and 9, which exhibit the different parts of the apparatus in
section. Fig. 8 representing furnace with five rows, and Fig.' 1^
a smaller furnace with three rows of clay burners.
The following account of a real experiment will serve to
illustrate the calculation of the result obtained in the combus-
tion of crystallized sugar :
Quantity of sugar employed 4.750 gnina.
Potasb-apparatus weighed after experiment. . 781 13 "
before " .. 77882
Carbon dioxide 7.81
Calcium-cbloride tube after experiment 226.05 *'
" before " 223.30
Water 2.75
* HofiEmann, Journal of Chemical Society, vol. xi, p. 80.
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THE CBEMISTS' MANUAL. 437
7.31 gr. carbon dioxide = 1.994 gr. carbon ; 2.75 gr. water = 0.8056 gr.
hydrogen ; or, in 100 parts sugar,*
Carbon , 41.98
Hydrogen 6.48
Oxygen by difference 51.59
100.00
When the organic substance cannot be mixed with cupric
oxide in the manner described, the process must be slightly
modified. If, for example, a volatile liquid is to be examined,
it is inclosed in a little glass bulb with a narrow stem, which is
weighed before and after the introduction of the liquid, the
point being hermetically sealed. The combustion-tube must
have, in this case, a much greater length ; and as the cupric
oxide cannot be introduced hot, it must be ignited and cooled
out of contact with the air, to prevent absorption of watery
vapor. This is most conveniently effected by transferring it,
in a heated state, to a large platinum crucible to which a
closely-fitting cover can be adapted. When quite cold, the
cover is removed, and instantly replaced by a dry glass funnel,
by the assistance of which the oxide may be directly poured
into the combustion-tube with merely momentary exposure to
the air. A little oxide is put in, then the bulb, with its stem
broken at a, a file-scratch having been previously made ; and
lastly, the tube is filled with the cold and dry cupric oxide.
It is arranged in the chauflfer, the calcic-chloride tube and
potash-apparatus adjusted, and then some six or eight inches
of oxide having been heated to redness, the liquid in the bulb
is, by the approximation of a hot coal, expelled, and slowly
converted into vapor, which, in passing over the hot oxide, is
completely burned. The experiment is then terminated in
the usual manner.
♦ The theoretical composition of sugar. Ci,H,,Oii, reckoned to 100
parts, gives :
Carbon 42.11
Hydrogen 6.43
Oxygen 51.46
100.00
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438 THE CHEMISTS' MANUAL.
Fig. 10.
Fusible fatty and wavy substances, and volatile concrete
bodies, as camphor, are placed in little boats of glass or plat-
inum.
Cupric oxide, which has been used, may be easily restored
by moistening with nitric acid and igniting to redness ; it be-
comes, in fact, rather improved than otherwise, as, after fre-
quent employment, its density is increased, and its troublesome
hygroscopic powers diminished.
For substances which are very diflScult of combustion, from
the large proportion of carbon which they contain, and for com-
pounds into which chlorine enters as a constituent, fused and
powdered lead chromate is very advantageously substituted for
the cupric oxide. Plumbic chromate freely gives up oxygen to
combustible matters, and even evolves, when strongly heated,
a little of that gas, which thus ensures the perfect combustion
of the organic body.
ANALYSIS OF AZOTIZED SUBSTANCES.
The presence of nitrogen in an organic compound is easily
ascertained by heating a small portion with solid potassic
hydrate in a test-tube ; the nitrogen, if present, is converted
into ammonia, which may be recognized by its odor and alka-
line reaction.
In determining the carbon and hydrogen in such bodies, by
combustion with cupric oxide, as above described, a longer
tube than usual must be employed, and four or five inches of
its anterior position filled with copper turnings rendered per-
fectly metallic by ignition in hydrogen.
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THE CHEMISTS' MANUAL. 439
This serves to decompose edj nitrogen oxides fonned in the
process of combustion, which, if suffered to pass off unde-
composed, would be absorbed by the potash, and vitiate the
determination of the carbon.
The nitrogen may be estimated either by converting it into
ammouia, by igniting the substance with an alkaline hydrate,
as above mentioned, or by evolving it in the free state and
measuring its volume.
1. By converaioii into ammonia: Will and Varrentrapp's
method. — An intimate mixture is made of 1 part sodic oxide
and 2 or 3 parts quicklime, by slaking lime of good qual-
ity with the proper proportion of strong sodic oxide, drying
the mixture in an iron vessel, and then heating it to redness
in an earthen crucible. The ignited mass is rubbed to powder
in a warm mortar, and carefully preserved from the air. The
lime is useful in many ways ; it diminishes the tendency of
the alkali to deliquesce, facilitates mixture with the organic
substance, and prevents fusion and liquefaction. A proper
quantity of the substance to be analyzed, namely, from 5 to 10
grains, is dried and accurately weighed out ; this is mixed in a
warm porcelain mortar with enough of the soda-lime to fill two-
thirds of an ordinary combustion-tube, the mortar being rinsed
with a little more of the alkaline mixture, and, lastly, with
a small quantity of powdered glass, which completely re-
moves everything adherent to its surface; the tube is then
filled to within an inch of the open end with the lime-mixture,
and arranged in a chauffer in the usual manner. The am-
monia is collected in a little apparatus of three bulbs (Fig. 11),
containing moderately strong hydrochloric acid, attached by a
cork to the combustion-tube. Matters being thus adjusted, fire
is applied to the tube commencing with the anterior extremity.
When it is ignited throughout its whole length, and when
no gas issues from the apparatus, the point of the tube is
broken, and a little air drawn through the whole. The acid
liquid is then emptied into a capsule, the bulbs rinsed into
the same, first with a little alcohol, and then repeatedly with
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440 THE CHEMISTS* MANUAL.
Fig. 11.
~^^^^
distilled water ; an excess of pnre platinic chloride is added ;
and the whole evaporated to dryness in a water-bath. The
dry mass, when cold, is treated with a mixture of alcohol and
ether, which dissolves out the superfluous platinic chloride,
but leaves untouched the yellow crystalline ammonic chloro-
platinate. The latter is collected upon a small weighed
filter, washed with the same mixture of alcohol and ether,
dried at 100°, and weighed ; 100 parts correspond to 6.272
parts of nitrogen. Or, the salt with its filter may be very
carefully ignited, the filter burned in a platinum crucible, and
the nitrogen reckoned from the weight of the spongy metal,
100 parts of that substance corresponding to 14.18 parts nitro-
gen. The former plan is to be preferred in most cases.
Bodies very rich in nitrogen, as urea, must be mixed with
about an equal quantity of pure sugar, to furnish inconden-
sable gas, and then diminish the violence of the absorption
which otherwise occurs; and the same precaution must be
taken, for a dififerent reason, with those which contain Uttle or
no hydrogen.
A modification of this process has been suggested by Peli-
got, which is very convenient if a large number of nitrogen-
determination is to be made. By this plan, the ammonia,
instead of being received in hydrochloric acid, is conducted
into a known volume (one-half to one cubic inch) of a standard
solution of sulphuric acid contained in the ordinary nitrogen-
bulbs. After the combustion is finished, the acid containing
the ammonia is poured out into a beaker, colored with a drop
of tincture of litmus, and then neutralized with a standard
solution of soda in water, or of lime in sugar-water, the point
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THE CHEMISTS' MANUAL. 441
of neutralization becoming perceptible by the sudden appear-
ance of a blue tint. The lime solution is conveniently poured
out from an alkalimeter. The volume of lime-solution neces-
sary to neutralize the same amount of acid that is used for
condensing the ammonia, having been ascertained by a pre-
liminary experiment, it is evident that the difference of the
quantities used in the two experiments gives the ammonia
collected in the acid during the combustion. The amount
of nitrogen may thus be calculated.
If, for instance, an acid be prepared containing 20 grams
of pure hydrogen sulphate (H2SO4) in 1000 grain-measures,
then 200 grain-measures of this acid, the quantity introduced
into the bulbs, will correspond to 1.38 grains of ammonia, or
1.14 grains of nitrogen. The alkaline solution is so graduated
that 1000 grain-measures will exactly neutralize the 200 grain-
measures of the standard acid. If we now find that the acid,
partly saturated with the ammonia disengaged during the com-
bustion of a nitrogenous substance, requires only YOO grain-
measures of the alkaline solution, it is evident that -^^^ 0^^^
= 60 grain-measures were saturated by the ammonia, and the
quantity of nitrogen is obtained by the proportion, 200 : 1.14
= 60 : a*, wherefore x = ^^ly^ = 0.342 grains of nitrogen.
2. By measure as free nitrogen. — When the nitrogen exists
in the organic substance in the form of an oxide, as in nitro-
benzine, C^H5(N02), ethyl ■ nitrate, C2H5(N0)0, etc., the pre-
ceding method cannot be employed, because these nitrogen
oxides are not completely converted into ammonia by heating
with alkaline hydrates : it fails also in the case of certain
organic bases. In such cases the nitrogen must be evolved in
the free state by heating the organic body with cupric oxide,
and its volume determined by collecting it over mercury in a
graduated jar. There are several ways of effecting this : the
one most frequently employed is that of Dumas, as simplified
by Melseus :
A tube of Bohemian glass, 28 inches long, is securely sealed
at one end ; into this enough dry hydrosodic carbonate is put
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442 THE CHEMISTS' MANUAL.
to occupy 6 inches. A little pure copper oxide is next intro-
duced, and afterwards the mLxture of oxide and organic sub-
stance ; the weight of the latter, between 4.5 and 9 grains, ia
a dry state, having been correctly determined. The remainder
of the tube, amounting to nearly one-half of its length, is
then filled up with pure cupric oxide and spongy metal, and
a round cork, perforated by a piece of narrow tube, is securely
Fig. 12.
adapted to its mouth. This tube is connected by means of a
caoutchouc joint with a bent delivery-tube, fir, and the com-
bustion-tube is arranged in the ftimace. A few coals are now
applied to the farther end of the tube, so as to decompose a
portion of tlie hydrosodic carbonate; the remainder of the
carbonate, as well as of the other part of the tube, being pro-
tected from the heat by a screen, n. The current of carbonic
oxide thus produced is intended to expel all the air from the
apparatus. In order to ascertain that this object, on which
the success of the whole operation depends, is accomplished,
the delivery-tube is depressed under the level of a mercurial
trough, and the gas which is evolved, collected in a test-tube
filled with concentrated potash-solution. If the gaa be per-
fectly absorbed, or, if after the introduction of a considerable
quantity only a minute bubble be left, the air may be con-
sidered as expelled. The next step is to fill a graduated glass
jar two-thirds with mercury and one-third with a strong solu-
tion of potash, and to invert it over the delivery-tube, aa
represented in Fig. 12-
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THE CHEMISTS' MANUAL. 443
This done, fire is applied to the tube, commencing at the
front end, and gradually proceeding to the closed extremity,
which still contains some undeeomposed hydrosodic car-
bonate. This, when the fire at length reaches it, yields up
carbonic oxide, which chases forward the nitrogen lingering
in the tube. The carbonic oxide generated during the com-
bustion is wholly absorbed by the potash in the jar, and nothing
is left but the nitrogen. When the operation is at an end,
the jar with its contents is transferred to a vessel of water,
and the volume of the nitrogen read off. This is properly cor-
rected for temperature, pressure, and aqueous vapor, and its
weight determined by calculation. When the operation has
been very successful, and all precautions minutely observed,
the result still leaves an error in excess, amounting to 0.3 or
0.5 per cent, due to the residual air of the apparatus, or that
condensed in the pores of the cupric oxide.
A modification of the process, by which this error is con-
siderably diminished, has been devised by Dr. Maxwell
Simpson.*
The method just described is applicable to the estimation
of nitrogen in the oxides and oxygen-acids of nitrogen, in
metallic nitrates and nitrites, and, in fact, to the analysis of
all nitrogenous bodies whatever.
ANALYSIS OF CHLORINATED COMPOUNDS.
The case of a volatile liquid containing chlorine is of very
frequent occurrence, and may be taken as an illustration of the
general plan of proceeding. The combustion with cupric
oxide must be very carefully conducted, and two or three
inches of the anterior portion of the tube kept cool enough
to prevent volatilization of the cupric chloride into the cal-
cic-chloride tube. Plumbic chromate is much better for the
purpose.
The chlorine is correctly determined by placing a small
* Quarterly Journal of the Chemical Society, vi, 299.
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444 THE CHEMISTS' MANUAL.
weighed bulb of liquid in a combustion-tube, which is after-
wards filled with fragments of pure quicklime. The lime k
brought to a red heat, and the vapor of the liquid driven over
it, when the chlorine displaces oxygen from the lime, and
gives rise to calcic chloride. When cold, the contents of
the tube are dissolved in dilute nitric acid, the liquid is fil-
tered, and the chlorine precipitated by silver nitrate.
Bromine and iodine are estimated in a similar manner.
ANALYSIS OF ORGANIC COMPOUNDS CONTAINING
SULPHUR.
When a body of this nature is burned with cupric oxide, a
small tube containing plumbic oxide may be interposed between
the calcic-chloride tube and the potash apparatus, to retain
any sulphurous acid that may be formed. It is better, how-
ever, to use plumbic chromate in such cases. The proportion of
sulphur is determined by oxidizing a known weight of the
substance with strong nitric acid, or by fusion in a silver ves-
sel with ten or twelve times its weight of pure potassic
hydrate and half as much nitre. The sulphur is thus eon-
verted into sulphuric acid, the quantity of which can be deter-
mined by dissolving the fused mass in water, acidulating with
nitric acid, and adding a barium salt. Phosphorus is, in like
manner, oxidized to phosphoric acid, the quantity of which i»
determined by precipitation as ammonic-dimagnesic phosphate,
or otherwise.
EMPIRICAL AND MOLECULAR FORMULC.
A chemical formula is termed empirical when it merely
gives the simplest possible expression of the composition of
the substance to which it refers. A molecular formula, on the
contrary, expresses the absolute number of atoms of each of its
elements supposed to be contained in the molecule, as well as
mere numerical relations existing between them. The em-
pirical formula is at once deduced from the analysis of the sub-
stance, reckoned to 100 parts.
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THE CHEMISTS' MANUAL. 445
The case of sugar already cited, may be taken as an ex-
ample.
This substance gives by analysis :
Carbon 41.98
Hydrogen 6.43
Oxygen 51.59
100.00
If each of these quantities be divided by the atomic weight
of the corresponding element, the quotient will express the
relations existing between the numbers of atoms of the three
elements ; these are afterwards reduced to their simplest ex-
pression.
This is the only part of the calculation attended with any dif-
ficulty. If the members were rigidly correct, it would only be
necessary to divide each by the greatest divisor common to the
whole ; but as they are only approximative, something is of
necessity left to the judgment of the experimenter.
In the case of sugar, we have
41-98 „,^ 6.43 ,,^ 51.59 ^ ,^
-j2~ = 3.50 ; -y- = 6.43 ; -^g- = 3.43,
or 350 atoms carbon, 643 atoms hydrogen, and 342 atoms
oxygen. Now it is evident, in the first place, that the hydrogen
and oxygen are present nearly in the proportion to form water,
or twice as many atoms of the former as of the latter. Again,
the atoms of carbon and hydrogen are nearly in the proportion
of 12 : 22, so that the formula C,2H22>0|| appears likely to
be correct. It is now easy to see how far this is admissible,
by reckoning it back to 100 parts, comparing the results with
the number given by the actual analysis, and obsersing
whether the difference falls fairly, in direction and amount,
within the limits of error of what may be termed a good ex-
periment, viz. : two or three tenths per cent, deficiency in the
carbon, and not more than one-tenth or two-tenths per cent,
excess in the hydrogen :
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44G THE CHEMISTS' MANUAL.
Carbon 12 x 12 = 144
Hydrogen 1 x 22 = 22
Oxygen 10 x 11 = 176
842 : 144 = 100 : 42.11
842 : 22 = 100 : 6.48
842 : 176 = 100 : 51.46
To determine the molecular formula, several considerationB
must be taken into account — ^namely, the combining or satu-
rating power of the compound ; if it is acid or basic, the num-
ber of atoms of any one of its elements (generally hydrogen)
which may be replaced by other elements ; the law of even
numbers, which requires that the sum of the numbers of atoms
of all the perissad elements (hydrogen, nitrogen, chlorine, etc.)
contained in the compound shall be divisible by 2 ; and the
vapor-density of the compound (if it be volatile without de-
composition) j which, in normally constituted compounds, is
always half the molecular weight.
The molecular formula may either coincide with the em-
pirical formula, or it may be a multiple of the latter. Thus,
the composition of acetic acid is expressed by the formula
CHjO, which exhibits the simplest relations of the three ele-
ments ; but if we want to express the quantities of these, in
atoms, required to make up a molecule of acetic acid, we have
to adopt the formula C2H4O2 ; for only one-fourth of the
hydrogen in this acid is replaceable by metals to form salts,
C2H3KO2, for example; and its vapor-density, compared with
hydrogen, is nearly 30, which is half the weight of the mole-
cule, C2H4O2 = 2 . 13 -I- 4: . H- 2 . 16. Again, the empirical
formula of benzine is CH ; but this contains an uneven num-
ber of hydrogen atoms ; moreover, if it expressed the weight
of the molecule of benzine, the vapor-density of that com-
12 4- 1
pound should be — ^ — = 6.5, whereas experiment shows that
it is six times as great, or equal to 39 ; hence the molecular
formula of benzine is C^H^.
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THE CHEMISTS* MANUAL. 447
Organic acids and salt-radicals have their molecular weights
most frequently determined by an analysis of their lead and
silver salts, by burning these latter with suitable precautions
in a thin porcelain capside, and noting the weight of the
lead oxide or metallic silver left behind. If the lead oxide be
mixed with globules of reduced metal, the quantity of the
latter must be ascertained by dissolving away the oxide with
acetic acid. Or the lead salt may be converted into sulphate,
and the silver compound into chloride, and both metals thus
estimated. An organic base, on the contrary, has its molec-
ular weight fixed by observation of the quantity of a mineral
acid or organic salt-radical, required to form with it in com-
pound having the characters of neutrality.
It is scarcely necessary to observe that the methods just de-
scribed for determining the empirical and molecular formula
of an organic compound from the results of its analysis, to-
gether with its physical properties and chemical reactions, are
equally applicable to inorganic compounds.
SCHEME FOR THE ANALYSIS OF BLOOD.
(Streck£R Hakdw. d. Chem., ii [2], 115.)
Wateb Determfnation. — Evaporate a weighed quantity;
dry the residue at 120°-130'' C, and weigh.
Fibrin E Determination, — The blood, as it runs from a
vein, is received in a tared vessel, and stirred from five to ten
minutes with a glass rod, the weight of which is included in
the tare, till the fibrine is completely separated. The blood,
together with the separated fibrine, is then weighed, strained
through linen, and the fibrine which remains thereon is placed
for some time in water, then dried, well boiled with alcohol
and ether, to free it from fat, and weighed after drying at
120® C. (Bacquerel and Rodier.)
Estimation op Albumen and other Matters CoAauLABLE
BY Heat, — A weighed quantity of blood, slightly acidulated
with acetic acid, is added by drops to boiling water, the liquid
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448 THE CHEMISTS' MANUAL.
is poured through a weighed filter, and the coagulum collected
thereon ; it is then washed on the filter with boiling water,
and dried, first at a gentle heat, afterwards at 120° to 130° C.
The residue may be freed from fat by treatment with boiling
ether. If the blood had not been previously freed from
fibrine, the weight of that substance, determined as above,
must be deducted from tlie total weight of the coagulum.
Estimation of the ExTRAcxrvE Matter. — The filtrate
obtained in the last detennination is evaporated on a water-
bath in a tared platinum basin, the residue dried at 120° C,
weighed, and burnt in a muflSo at as low a heat as possible.
The weight of the ash, deducted from that of the total dried
residue, gives approximately the amount of extractive matter.
Estimation of Fat. — A quantity of blood (which need not
be weighed) is dried at 100° C. ; the residue is pulverized and
dried at 120° C, and a weighed portion thereof is treated with
ether in a flask ; the ether is passed through a small filter into
a tared platinum capsule ; and the treatment of the residue
with ether is repeated several times. The collected ethereal
solution is carefully evaporated, and the residue dried at
100° C. As the weight of the solid constituents of the blood
have been previously determined, the quantity of blood from
which this fat has been obtained may be calculated from that
of the residue which was subjected to treatment with ether.
Estimation of Mineral CoNSTnuENTS. — A weighed quan-
tity of the blood is dried, mixed with ignited sodic carbonate,
then dried and incinerated in the muffle at the lowest possible
temperature, then treated according to scheme for the analysis
of ash.
Separate Estimation of the Serum and Coaoulum, wtth
their Constttuents. — ^Tlie fresh blood is collected in a tared
cylindrical vessel, having aground edge, and not too shallow;
it is covered with a glass plate and left to stand till the coagu-
lation is complete, after which the edge of the clot is detached
from the sides of the vessel by means of a needle. The blood
is then weighed, and after the clot has contracted as much as
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THE CHEMISTS' MANUAL. 449
possible, the serum is poured off, and the quantity of albumen,
etc., contained in it is determined as above described. The
clot and the inner surface of the vessel are then freed from
serum as completely as possible by wiping with bibulous
paper, and the clot is weighed on the vessel. This weight
deducted from the total weight of the blood, gives the propor-
Hon of serum.
The clot contains the blood-corpuscles, the fibrine, and a
certain quantity of serum ; the amount of water contained in
it may be determined by drying at 120® to 130° C. ; but there
is no known method of directly estimating the amount of the
blood-corpuscles. Prevost and Dumas estimated it approxi-
mately, on the assumption that the water contained in the clot
is all due to adhering serum, and accordingly deducted from
the weight of the dried clot an amount of serum-constituents
corresponding to the quantity of water in the clot, together
with the amount of fibrine separately determined. As, however,
the blood-corpuscles themselves contain water, this method
necessarily makes the quantity of dried corpuscles too small.
The separation of hematin from globulin cannot be effected ;
but if the quantity of iron in the dried coagulum be determined,
the amount of blood pigment may be calculated on the sup-
position that this pigment contains 6.64 per cent, of iron.
(See Analysis of Man.)
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450 THE CHEMISTS' MANUAL.
SCHEME FOR THE ANALYSIS OF URINE*
The following method is designed more particularly for the
analysis of the urine of herbivorous animals, but it may be
applied in the examination of that of carnivorous animals
and man also.
Specifio GRAvrrr. — Determine this by comparing the
weights of equal volumes of the urine and of water, or with
the urometer, a species of hydrometer constructed expressly
for this purpose ; when this instrument is used, all foam must
be carefully removed from the surface of the liquid by filter-
paper.
A difference of 4** C. in the temperature of the liquid usu-
ally makes a difference of about I'' in the reading of the
urometer.
The specific gravity of urine ranges between 1.01 and 1.04.
1. Total Amount of Dry Substance in Solution. — Deter-
mine this by evaporating a weighed quantity in a current of
dry hydrogen in such a manner as to estimate the ammonia
that is eicpelled at the same time. Take 4-6 cc. of the urine,
accurately weighed ; the evaporation to dryness is completed
in 4^5 hours.
In human urine, that has an acid reaction due to acid sodic
phosphate, the ammonia may be assumed to have been driven
from urea, and by multiplying the amount of it by 1.765 the
corresponding amount of urea will be obtained. But in the
urine of herbivorous animals, the ammonia resulting from t/i{j<
decomposition must be estimated by the difference between
the ammonia set free on evaporation to dryness and that found
in the urine by direct determination. Generally, however,
* Taken from Agric. Chem. Anal. Caldwell.
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THE CHEMISTS' MANUAL. 451
these quantities of ammonia are very small, and can be left out
of consideration.
2. The NON-VOLATILE MATTEB in this residue left on evap-
oration, is determined hy evaporating a fresh quantity of
100 c.c. of the urine in a platinum dish, and igniting the resi-
due ; determine carbonic acid in the ash.
3. Carbonic Acid (free and combined). — Detennine this in
two portions of 100 c.c. of the fresh urine. To one portion
add baric chloride containing amnionic hydrate in excess, and
to the other baric chloride alone ; heat both mixtures nearly
to boiling ; collect the precipitates on dried and weighed fil-
ters; wash, and dry them at 100°; weigh, and determine
carbonic acid in 1-2 grams of each precipitate ; the first pre-
cipitate contains the total carbonic acid, the second only the
combined.
4. NriROGEN. — ^The residue left from (1) may be used for
the determination of nitrogen, or another portion of 5-10 c.c.
of the urine may be acidified with oxalic acid, mixed with
ignited gypsum, and evaporated to dryness. In the former
case this second residue will contain only so much of the
nitrogen as was not expelled in the form of ammonia during
the desiccation ; in the latter, the oxalic acid will prevent the
escape of any nitrogen as ammonia. The dry substance may
be completely rinsed off the sides of the dish with some of
the soda-lime used in the combustion.
Or, this method of Voit may be used : Weigh out about
5 c.c. of the urine ; mix it in a shallow dish with a sufficient
quantity of fine quartz-sand to absorb it all ; put the dish
under the receiver of an air-pump, and exhaust the air ; the
whole becomes quite dry in a few hours and maybe pulverized
easily, and completely loosened from the sides of the dish and
mixed with the soda-lime.
The combustion may be performed in a short combustion-
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452 THE CHEMISTS' MANUAL.
tube, and very rapidly, without fear of losing any of the
ammonia.
5. Actual Ammonia. — Determine this by Schlossug's method
in 20 c.c. of the urine, after filtration to remove slimy or sedi-
mentary matters. In the fresh urine of horned cattle, the actual
ammonia does not amount to more than 0.009-0.01 per cent.,
but in human urine it ranges as high as 0.078-0.143 per cent.
6. Complete Analysis of the Ash. — Evaporate 200-500
grams of the urine to dryness ; incinerate the residue, and
examine the ash for its constituents in the usual manner. The
ash of the urine of herbivorous animals is poor in alkaline
earths, and 8-10 grams will be required for their determina-
tion. In the urine of ruminants, phosphoric acid is found in
hardly determinable quantity ; while in that of swine, and
often of calves, it is present in large quantity and should b©
estimated.
7. Chlobine Ain> Frea. — These are determined with the
aid of the standard solution of mercuric nitrate. The urine
must first be freed from phosphoric and hippuric acids. Acid-
ify 200 c.c. with nitric acid ; boil the mixture to expel the
carbonic acid ; neutralize the nitric acid with freshly ignited
magnesia, and cool the liquid to the temperature of the room,
by immersing the flask in cold water ; transfer the liquid to a
graduated cylinder, rinse the flask into the cylinder and bring
the volume of its contents to 220 c.c. ; add 30 c.c. of an aque-
ous solution of ferric nitrate of such a degree of concentration
that, with this quantity of the solution added, the salt will be
slightly in excess ; the excess may be recognized by a weak
reaction of the solution on a slip of filter-paper soaked in a
dilute solution of potassic ferrocyanide ; too large an excess of
the ferric salt will be indicated by a re-solution of the precipi-
tate that was formed at first on its addition ; filter the liquid
immediately through a large, dry, ribbed filter, and to 150 cc.
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THE CHEMISTS' MANUAL. 453
of the filtrate add 60 c.c. of a solution of baryta mixed with a
little calcined magnesia ; filter again, and for each determina-
tion of sodic chloride and urea take 16 c.c. of this filtrate,
corresponding to 9 c.c. of urine.
(a.) Chlorine (common salt). — Acidify exactly 15 c.c. of the
liquid with a drop of nitric acid, and allow the standard solu-
tion of mercuric nitrate to flow in from the burette, with
constant stirring, until a permanent turbidity appears. A
mere opalescent appearance of the liquid, which may be pre-
sented even in the beginning, is easily distinguished from the
cloudy turbidity which is the real indication of saturation.
Estimate the amount of sodic chloride, or of chlorine, on the
basis of the standard of the solution already detennined.
(6.) Urea, — In a second portion of 15 c.c. of the liquid,
proceed to determine urea with the same standard solution.
Subtract from the total amount of solution required, the
amount used in one ; and also make the correction required for
dilution of the solution.
8. HippuRio Acid. — ^Evaporate 200 c.c. of the urine down
to 50 c.c, and precipitate the acid with hydrochloric acid, etc.
It may be well to first digest the urine with animal charcoal
in the proportion of two grams of charcoal to 10 c.c. of the
liquid, in order to decolorize it.
There are usually only traces of uric acid in the urine of
herbivora, and it cannot be estimated ; but in the urine of
carnivora the proportion of uric acid generally exceeds that
of the hippnric.
According to the process of Meissner and Shepard, for
separating these two acids, evaporate the urine until it begins
to crystallize ; add so much absolute alcohol to the hot liquid
that a further addition causes no more precipitation ; let the
mixture cool, and filter it; the best absolute alcohol must be
used, and it must not be spared, else succinic acid may remain
in solution with the hippuric and cause trouble. Evaporate
the alcoholic solution, at first in a flask on the water-bath.
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454 THE CHEMISTS' MANUAL.
until all the alcohol and the water are expelled and only a
brown syrup remains, that solidifies to a crj^stalline mass on
cooling ; extract this mass, while yet warm and liquid, with
etiier and a few drops of hydrochloric acid added after the
ether; agitate the mixture violently, and repeat the process
two or three times with fresh portions of ether. If the alco-
hol and water were not carefully removed in the preceding
evaporation, some of the urea will pass into this ethereal
solution. Collect the ethereal extracts, distil off most of the
ether, and let the rest evaporate spontaneously in the air.
Ilippuric acid appears then in the form of handsome crystals.
If the crystals are not colorless, or they are not readily formed,
dilute the residue, left by the evaporation of the ether, with
water, boil the mixture with lime-water, filter, concentrate the
colorless filtrate, and precipitate the hippuric acid by hydro-
chloric acid in excess.
9. Phosphorio Acid. — (a.) This may be determined directly
in the urine, with the standard uranic solution. Filter the
urine, if necessary, add 5 c.c. of sodic acetate to 50 c.c. of the
filtrate, and titrate the mixture with uranic acetate.
(i.) To obtain a more accurate determination, add the mag-
nesia mixture to 50 c.c. of the clear urine, collect and wash
the precipitate in the usual manner, dissolve it, without dry-
ing, in acetic acid in not to great excess, dilute the solution to
50 c.c. with water, add 5 c.c. of the solution of sodic acetate,
and titrate as before with the uranic solution.
(<7.) To detemline the phosphoric acid that is combined with
alkaline earths only to 100-200 c.c. of the urine, according to
its strength, add ammonic hydrate until alkaline reaction
ensues, let the mixture stand twelve houi-s, and collect and
treat the precipitate in the manner described in (J). In
another precisely equal quantity of urine, the precipitate by
ammonic hydrate is ignited and weighed; the amount of
magnesic pyrophosphate in this mixture may be estimated by
multiplying the amount of phosphoric acid in it, as determined
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THE CHEMISTS' MANUAL. 455
above, by 2.1831, subtracting the sum of the phosphates from
this product, and multiplying the remainder by 2.5227. If it
is desired to determine lime and magnesia directly, dissolve
the mixture of the phosphates, obtained above by precipitating
with ammonic hydrate, without drying it, in as small a quan-
tity of acetic acid as possible ; precipitate the lime by ammonic
oxalate, and the magnesia as phosphate again by excess of
ammonic hydrate.
10. Sulphuric Acid. — ^Heat 50-100 c.c. of the urine, add
some nitric acid, and then baric chloride in slight excess.
11. Sulphur. — To determine the total sulphur, mix 50 c.c.
of the urine in a silver crucible with solid potassic oxide and
a little saltpetre ; evaporate the mixture cautiously to dryness,
ignite the residue strongly until it is quite white, exhaust it
with water, and determine sulphuric acid in the filtered solu-
tion, in the usual manner.
12. Carbon and Hydrogen. — Absorb 10 c.c. of the urine
by fine quartz-sand that has been previously boiled with acid,
washed and ignited, dry the mixture, and bum it with plumbic
chromate.
The following is an analysis of healthy urine, by Marchand :
Water 933.199
Urea 32.675
Uric acid 1.065
Lactic acid 1.521
Extractive matters 11.151
Mucus 0.288
Potassic sulphate 8 587
Sodic sulphate 3.213
Ammonic diphosphate 1.552
Sodic chloride 4.218
Ammonic chloride 1.652
Calcic and magnesic phosphate 1.210
Lactates 1.618
1000.000
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456
THE CHEMISTS' MANUAL.
The following analyses are by Vemois and Becquerel, show-
ing the comparative composition of male and female urine:
CosvrmjExm.
Mean Compositioh
OP THX
Urine of pottb
Hbaltht Men.
Mbam Coxpoerrioir
OF THE
UBINB OF FOUB
HBAI.THT WOMfEN.
Hban.
8fD6ci1lc artitilv
1.0189
968.815
31.185
18.888
0.891
9.261
7.695
1.01512
975.052
24.948
10.366
0.406
8.038
6.143
1.01701
Water
971.985
Solid confititaents
28066
Urea
12.102
Uric acid
Other organic matters
Fixed salts
ConsUting of--
Chlorine
0.898
8.647
6.919
0.502
Sulphuric acid
0.855
Phosnhoric acid
0.317
Potassic oxide
1.800
Sodic, calcic, and magnesic }
oxide
8.944
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THE CHEMISTS' J£ANUAL. 457
SCHEME FOR THE QUANTITATIVE ANALYSIS
OF MILK.
Evaporate to dryness at a gentle heat over a water-bath
5 grams of milk ; heat the same in an air-bath to 105° C,
until constant weight.
Loss IN Weight I Weight of Residue
will equal the Water. | will equal the MiLK-sOLmB.
TREATMENT OF THE MILK SOLIDS.
Moisten with alcohol and disintegrate the mass ; then boil
with ether two or three times to extract the fat.
Evaporate the eihev-extract over a water-bath at a moderate
heat to expel the ether ; transfer to the air-bath and increase
the heat to 105° C. to expel any traces of water or alcohol.
Weigh the residue, which will equal the fat. If the iirst
residue, after extracting the fat with ether, be heated to expel
any ether and alcohol it may contain, and weighed, the differ-
ence in weight of the milk-solids and this weight will equal
the/o^ extracted.
Heat the residue, after extracting the fat and evaporating
to expel ether, with alcohol (95 per cent.), then add 25 c.c. of
boiling water, and filter through a weighed fitter-paper ; filter
a little at a time, keeping the remainder hot over a water-bath.
When solution is all filtered, wash the casein on the filter-
paper with a little boiling water. Add to filtrate five to ten
drops of acetic acid, and evaporate to a small volume, by
which means all the casein remaining in the filtrate is coagu-
lated ; filter through the same filter-paper, and wash the casein
again on the filter-paper with hot water.
The filter-paper will then contain the casein and some in-
soluble salts. Heat in an air-bath until dry. The weight of
the same, minus the weight of the filter-paper, will equal the
casein and some insoluble salts ; ignite and subtract the weight
of ash. The remainder will equal the casein.
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468 THE CHEMISTS' MANUAL.
Evaporate the filtrate from the casein over a water-bath,
then heat in the air-bath to constant weight (note the weight).
Ignite the dry mass and weigh (note the weight) ; subtract the
last weight from the first, and the remaining weight will equal
the MILK-SUGAS.
To determine the inorganic salts evaporate to dryness and
ignite to constant weight about 5 grams of milk. The weight
obtained will equal the inorganic salts.
The following very convenient method for the analysis of
milk is adopted by Chandler :
W^ter is determined by evaporating a weighed portion of
milk in a flat platinum dish (about half an inch deep and one
and a half inches in diameter) at 212° F. The loss in weight
is the WATER. The salts are determined by carefully inciner-
ating the solid residue left after the evaporation of the water.
For the determination of the other constituents a platinum
dish is nearly filled with pure quartz-sand ; the whole weighed;
a small quantity of the milk is added, which is at once soaked
up by the sand, and the whole again weighed to find the weight
of milk taken. The whole is then dried at 212° F., the con-
tents of the dish extracted with anhydrous ether, and again
dried ; the loss in the weight of sand, etc., indicates the per-
centage of BUTTBR. The butter may be weighed directly by
evaporating the ethereal solution in a weighed beaker. The
residue, after removing the butter, is washed with wann
water, to the first of which a few drops of acetic acid is added
to remove the sugar. The diflference between the original
weight of the sand and of the sand and casein indicates the
percentage of casein. A correction must be made in the
weights of the sugar and casein on account of the salts, which
are washed out with the sugar. By evaporating and igniting
the sugar solution, the salts washed out will be determined;
they must be deducted from the percentage of sugar ; the re-
mainder of the salts (ash) must be deducted from the casein.
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THE CHEMISTS' MANUAL.
459
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460
THE CHEMISTS' MANUAL.
The following table contains the average composition of the
products obtained from milk in making butter (Alex. Muller) :
New
Milk.
SKimncD
Milk.
CRBAK. ®H!7?*-iBUTTBB.t
1 "'^- 1
BRonct
Fat
4.00
3.25
4.50
0.75
87.50
0.55
3.87
4.60
0.78
90.64
35.00 < 1.67 85 00
0.00
Albuminoids*
Milk-Sugar
Ash
Water
2.20
8.05
0.50
69.25
8.33
4.61
0.77
89.62
0.51
0.70
0.12
13.67
0.39
3.84
0.86
94.91
Total
100.00
100.00
100.00
100.00
100.00
100.00
* Casein and albamen. t Unsolted.
X Brine that separates on working after salting ; salt not included.
The following table contains analyses of cheese by E.
IIornig(1869):
A3
Ramadouz
Chbbsx.
IfJ
5*^0
PI
is
II
Water
Patty Matters
Casein
SalU
Loss
8?.ft3
20.14
6.17
0.13
G6.fX)
17.05
18.78
6.78
0.81
61.21
9.16
83.60
6.01
aoa
57.64
90.81
18.51
8.51
0.04
86.78
88.09
85.67
8.71
0.21
84.08
88.04
28.28
5.58
0.09
50.28
10.44
94.09
6.17
0.08
49.84
20.68
84.26
5.45
0.88
100.00
100.00
100.00
100.00
10000
100.00
100.00
100.00
The following analyses of cheese are given by Voelcker :
CONSTXTUINTS.
i
1
l|
||
K
Water
Butter
Caseine
Sugar of Milk. . . )
Lactic Acid f
Mineral Matter. ..
32.59
32.51
26.06
4.53
4.31
20 27
43.98
■ 33.55 }
2.20
3032
35.53
28.18
1.66
4.31
32.44
3017
31.75
1.22
4.42
28.10
83 68
30.31
8.72
419
27.29
8541
25.87
6J81
5J22
100.00
100.00
100.00
100.00
100.00
100.00
Nitrogen
Common Salt
4.17
1.59
8.89
0.29
4 51
1.55
5.12
1.42
4.85
1.12
4.14
1.97
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THE CHEMISTS' MANUAL. 461
The composition of whey is as follows (Voelcker) :
Water. 89.65
Butter 0.79
Casein 8.01
MUk-Sugar 5.72
Mineml Salts 0.88
100.00
The following analyses are by Dr. E. Waller (made in
January, 1875):
Amebic AN.
Baqlb.
Nbw Yobk.
Natiohal.
Fat
Casein.
So^ar
Salts
Water
16.29
17.20
10.64
2.77
58.04
14.36
15.07
11.64
2.10
56.83
14.28
13.96
13.90
2.00
55.86
13.97
14.02
10.44
2.33
59.24
100.00
100.00
100.00
100.00
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462
THE CHEMISTS' MA2JUAL.
SUGARS AND SOME ALLIED BODIES.
(Miller.)
VaKUBTY AMD
Origin oi* Suqab.
Sucrose, or
cane-sugar,
from sugar-
cane.
Principal PaopniTisa.
Crystallizes in four or six-sided rhomboidal i-risms,
is very soluble in water, less so in diluted alcohol,
sp. gr. 1.6, fuses at about 320" F. (160° C), is not preci-
pitated by Bubacetate of lead, but is so by an ammo-
niacal solution of acetate of lead, does not reduce an
alkaline solution of potassio cupric tartrate on boiling,
produces r^At-handed rotation = 7S°,S, undergoes aloo-
liolic fermentation with yeast, combines with alkalies,
yields dextrose and levulose when boiled with dilute
acids, with nitric acid yields saccharic and oxalic acids.
Inverted
cane-sugar,
C.H„0.;
from many
recent fruits.
Is not crytallizable, is soluble in dilute alcohol, is
not precipitated by subacetate of lead, reduces an alka-
line solution of potassio-cupric tartrate by boiling, pro-
duces left-hsinded rotation = — 26" at 59° F. (15* C).
undergoes alcoholic fermentation with yeast, turns
brown when treated with alkalies, is partially con-
verted into grape-sugar by boiling with dilute adds.
Dextrose,
or grape-sugar,
C.Hi.Oe.H^O;
from dried
fruits, or from
starch, altered
by acids.
Lactose, or
sugar of milk,
C,,H,,Oji,H,0;
from whey of
milk.
(Crystallizes in cubes or square tablss, is less soluble
in water than cane-sugar, but more soluble in alcohol,
yields a precipitate with ammoniacal acetate of lead,
reduces potassio-cupric tartrate and the salta of mer-
cury, silver and gold when boiled with them, ferments
readily with yeast, produces ri;^^-handed rotation =
57°. 4, becomes brown when treated with alkalies, with
nitric acid yields saccharic and oxalic acid.
Crystallizes in four-sided prisms, is less soluble in
water than grape-sugar. Is nearly insoluble in alcohol
and ether, is precipitated from its solutions by anuno-
niacal acetate of lead, reduces the salts of copper, sil-
ver, and mercury, when its alkaline solution is boiled
with them, produces n^A^-handed rotation = 56". 4, is
not directly susceptible of alcoholic fermentation, is
converted into galactose by boiling with dilute acids,
yields mucic and oxalic acids with nitric acid.
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THE CHEMISTS' MANUAL.
463
VAHraTT AKD
Orioih or SuoAB.
Trehalose, or
mycoee,
Ci,H„Oi,^H,0
(Berthelot) ;
Turkish manna,
product of
insect Larinus
nidifieans.
PBDICirAL PBOFKBTIU.
Crystallizes in brilliant rectangular octohedra or in
rhombic prisms, produces r^A^-handed rotation = 220°;
if heated quickly it fuses at 212% and at 266' (130° C.)
loses HgO and becomes solid ; may be heated without
decomposition to 410' (210' C), when it melts again ;
loses its water of crystallization, is very soluble in
water, and in hot alcohol, is sparingly soluble in cold
alcohol and ether, is precipitated by ammoniacal ace-
tate of lead, does not reduce potassioeupric tartrate,
■ferments slowly and imperfectly with yeast, yields
dextrose when heated with dilute acids, does not give
mucic with nitric acid, but when heated with it yields
saccharic and oxalic acids.
Melezitose,
CijHjjOu^gO
(Berthelot) ;
from
larch manna.
Crystallizes in short, hard, efflorescent rhombic
prisms, is very soluble in water, sparingly soluble in
alcohol, either hot or cold, insoluble in ether, has
a sweetness about that of glucose, fuses at 280"
(188° C), is precipitated by ammoniacal acetate of lead,
does not reduce the alkaline potassio^upric tartmte,
produces n^A^handed rotation = W**.!, ferments with
difficulty, yields dextrose when heated with dilute
acids, gives no mucic acid with nitric acid.
Melitose,
Ci.H„0»,.2H,0
(Berthelot);
from the
Eucalyptus.
Crystallizes in slender prisms, is freely soluble in
water, slightly soluble in alcohol, is feebly sweet,
melts and loses water at 260*' (127"* C), yields a precip-
itate with ammoniacal acetate of lead, does not reduce
an alkaline. solution of potassio-cupric tartrate, exerts
rl^/t^hande(l rotation = 102'', undergoes alcoholic fer-
mentation with yeast, at the same time half the sugar
is separate^ in an unfermontablo form as eucalin, fur-
nishes mucic add with nitric acid, is little affected by
alkalies.
Eucalin,
C,Hi,0,.H.O
(Berthelot);
from
fermentation of
melitose.
Is not cry stall izable, precipitates ammoniacal acetate
of lead, and reduces the alkaline potassio-cupric tar
trate when boiled with it, produces rigJU handed rota-
tion = about 50", is not susceptible of alcoholic fer-
mentation with yeast, becomes brown when treated
with alkalies, is not altered by boiling with dilute
acids.
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464
THE CHEMISTS' MANUAL.
Vabibtt and
OBIOm 0¥ SUOAB.
FBIMOIPAL PBOPEBTIB8.
Sorbin,
(Pelouze);
from berries of
service tree,
Sorhts
auevparia.
Ciystallizes in octohedra with a rectangular base, is
very soluble in water, nearly insoluble in alcohol,
sp. gr. 1.65, is fusible without loss of weight, gives a
white precipitate with ammoniacal acetate of lead, re-
duces the alkaline solution of potassio-cupric tartrate
on heating it with it, oocasioDS /^-handed rotation
= — 46". 9, is not fermentable with yeast, but with
cheese and chalk slowly yields lactic and butyric adds
and alcohol, becomes brown when treated with alka-
lies, yields a red solution with oil of vitriol, is con-
verted into oxalic and a little lacemic acid by nitric
acid.
Inosin,
C.H„0e,2H,0
(Scherer) ;
from muBCuhir
tissue.
Crystallizes in radiated tufts. Is soluble in water,
insoluble in absolute alcohol and ether, loses water by
heat, and fuses at 410'' (210** C), has no rotatory power
on polarized light, does not reduce the alkaline potas-
sio-cupric tartrate when boiled with it, is not suscepti-
ble of alcoholic fermentation, but with cheese and
chalk yields lactic and butyric acids, is not altered by
boiling with dilute acids or alkalies, forms a precipi-
tate with ammoniacal acetate of lead.
Mannite,
from the juice
of Fraxinus
ornu9.
Crystallizes in silky anhydrous four-sided prisms,
is soluble in water and alcohol, fuses at 320' (160' d.
gives a precipitate with ammoniacal acetate of lead,
reduces the salts of silver or gold by heat, does Dot
reduce the alkaline potassio-cupric tartrate when boiled
with it, exerts no rotary power on polarized light, is
not easily fermentable, with nitric acid yields saccharic
and oxalic acids, is soluble without coloration in oil
of vitriol, and in alkaline solutions.
Erytbrite,
C,H,oO,
(V. Luynes) ;
from Roccella
and other
lichens.
Crystallizes in broad, voluminous crystals of the
pyramidal system, is soluble in water and in aloohd,
fuses at 248° (120** C), has no rotatory power, gives do
precipitate with ammoniacal acetate of lead, does not
reduce the alkaline potassio-cupric tartrate, yields no
mucic acid with nitric acid, is not fermentable.
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THE CHEMISTS' MANUAL.
465
ORI6IN or SUAAB.
FBOtCtPJLL Pbofebtisb.
Duldte,
C.Hi40.
(Laurent) ;
origin
unknown.
CiyBtallizes in brilliant prismB, is soluble in water
and in alcohol, fuses at 856° (180** C), gives no precip-
itate with acetate or subacetate of lead, does not reduce
nitrate of silver or chloride of gold, produces no rota-
tion on polarized light, is not susceptible of fermenta-
tion with yeast, is not affected bj dilute alkalies, is
converted into mudc acid by nitric add.
Quercite,
from aooni0.
Crystallizes in transparent prisms, is soluble in water
and dUute alcohol, is fusible at 420*" (215^5 C), does
not reduce the alkaline potassio-cupric tartrate, is not
fermentable by yeast, is soluble without change of
color in oil of vitriol and in the alkalies, yields oxalic
acid with nitric add.
Finite,
C.H^.O,
(Berthelot);
from Pinna
lamberiiana.
Crystallizes slowly in hard, hemispherical radiated
masses, has a very sweet taste, is very soluble in
water, is sparingly soluble in alcohol, gives a precipi-
tate with ammoniacal acetate of lead, does not reduce
the alkaline potassio-cupric tartrate, sp. gr. 1.52, pro-
duces ri^/i«-handed rotation, is not fermentable, fuses
below 480" (249'* C), does not yield mudc with nitric
add.
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466 THE CHEMISTS' MANUAL.
CANE-SUGAR.
Cane-sugar, or sucrose, is the sugar of commerce, and is
prepared from the sugar-cane, Saccharum offidnarum* which
is a plant of the grass species ; its stalk is round, knotted,
and hollow, and the exterior of a greenish-yellow or blue with
sometimes violet streaks.
It grows from 2.6 to 6.6 metres (8.4 to 22.5 ft.) high, and
from 4 to 6 centimetres (1.6 to 2.4 inches) in thickness ; the
interior is cellular. The leaves grow to a length of 1.6 to
2 metres (5.2 — 6.6 feet), and are ribbed. The plant is grown
from seed, and also cultivated from cuttings.
A hectare (2.471 acres English) of land yields of new sugar:
By 15 Months' CnltiTaUon. In 1 Yeu.
From Martinique. . . .2,500 kUoe ( 5,510 Ibe. Av.). .2,000 kiloe ( 4,408 lbs. At.)
« Guadaloupe... 8,000 " (6,612" «).. 2,400 « (5,289" ")
•' Mauritius 6,000 " (11,020" ").. 4,000 - (8,816" ")
" Brazil 7,500 " (16,530 " " ). .6,000 " (13,224 " " )
The sugar-cane yields 90 per cent, of juice, containing, ac-
cording to P^got, 18 to 20 parts of crystallized sugar. The
following analyses are of the components of sugar-cane :
Composition of the OtaheUe Cane. by Payen :
Water 71 .04
Cane^ugar 18.00
Gellnlose, lignite, pectine, and pectic acid .- 0.56
Albumen and other nitrojifenouB principles 0.55
Geioeine, wax, fats, resins, coloring matter, essential oils, etc. 0.37
Soluble salts 0 16
Insoluble salts 0.12
Silica % 0 JM)
100.00
By PxuaoT. By Dufut. ^y Icbbt.
Martiniqae. Gnadalonpe. ManriUns.
Sugar 18.0 17.8 20.0
Water. 72.1 720 , 68.0
Cellulose 9.9 9-8 10.0
Salti — 0.4 ' 0.7-1J8
• See Johnson's Cycl., Article " Sugar," hy C. P. Chandler; also Wag-
ner's Tech., p. 864.
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THE CHEMISTS' MANUAL. 467
Oat of the 18 per cent, of the sngar found in the cane, as a
role not more than 8 per cent, of crystallized sugar can be
realized.
The loss may be accounted for thus : 90 per cent, juice is
expressed from the cane, from which only about 50 to 60 per
cent, can be clarified from the straw, etc. ; a fifth part is ex-
hausted by refining ; and finally, two-thirds of the sugar is
obtained by boiling, while the rest goes to the molasses. The
18 per cent, sugar may be realized in the following manner :
In the refuse sometimee remaiiiB 6 per cent.
By skimming 2.6 " "
In the molaases 8. " "
AsiawBogar. 6.5 '* '*
18 per cent.
Cane-juice from the Canade la tierra in Cuba, when evap-
orated in vacuo at the atmospheric temperature, yields in
100 parts, according to M. Casacca :
CiyBtalline i;?bite sugar 20.94
Water 78.80
Mineral substances 0.14
Organic matter, different from sngar 0.12
100.00
In 10 gallons of 231 cu. in. of cane-juice, making 8^° B.,
there are 5| ounces of salts, which consist of:
Potassic Bolpbate 17.840 grams.
Potassicsnlphate 16.028 "
Potassic chloride 8.855 '*
Potassic acetate 03.750 "
Calcic acetate 36.010 "
Gelatinous silica. 15.270 "
Total 157.253gr. = 5.57oz.Av.
Vameties op Sugar. — ^European and American commerce
deals with the following kinds of raw sugars :
1. West Indian. — Cuba, San Domingo or Hayti, Jamaica,
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468
THE CHEMISTS' MANUAL.
Porto-Eico, Martinique, Guadaloupe, St. Croix, St. Thoinas,
Havana.
2. American. — ^Rio Janeiro, Bahia, Surinam, Pemambuco.
3. East Indian. — Java, Manila, Bengal, Mauritius, Bour-
bon, Cochin-China, Siam, Canton.
Of late there has been a distinction between sugar culti-
vated by slave and that by free labor ; the latter comes from
Jamaica, Barbadoes, Demerara, Antigua, Trinidad, Dominica;
the former from Cuba, Havana, Brazil, St. Croix, and Porto-
Rico.
Besides the above-named sugar, American commerce deals
with New Orleans, Mexico, Honolulu, and sometimes with
Egyptian sugars.
According to method of preparation, raw sugars have re-
ceived, besides the above, the following names : Melado, clay,
muscovado, molasses, centrifugal, drone, and potted sugars.
The raw sugars come into market packed in hogsheads,
tierces, barrels, bags, mats, baskets, and cheeroons.
In the French and English colonies sugar is exported in
chests covered with fire-clay under the name of chest or tub
sugar.
The mode of manufacture depends on the foreign constituents
of sugar, all of which must be destroyed before the sugar t^an
be refined. According to Mulder, we have in the foUowing
sugars from —
Java.
10 Samplee.
Havana.
6 Samples
Surinam.
4 Sample*.
Cane Sugar
Glucose
Extractive matter, gum, etc.
Asli
98.6-83.1
5.5— 0.3
8.5- 0.5
1.9— 0.9
6.3— 0.8
97.0-«7.3
8.7- 0.9
4.5— 0.4
1.1- 0.0
3.8— 0.9
92.3-85.4
4.4- 1.6
2.1 - 1.1
1.4— a8
Water
6.9- 4.0
Molasses is produced by the long-continued heating of the
cane-juice. It is used principally in the colonies for the
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THE CHEMISTS' MANUAJL 469
manu&ctore of mm ; it is soon converted to spirit, and then
quickly becomes acetated.
West India molasses, according to Dr. Wallace, has the
following composition :
Cane-sugar 47.0
Qlucoae 20.4
Extractive and coloring matter, etc 27
Salts (aah) 2.6
Water 27.3
100.0
Specific gravity 1.36
SnGAB FROM Beets. — Marggraf, in the year 1747, was the
discoverer of sugar in beets, and suggested the manufacture of
sugar from this source. The following are the principal sugar
beets:
Quendlinhurg heei is a slender, rose-colored root, and very
Bweet ; it is matured fourteen days before any other kind.
Silesian heel is a pearnshaped root, white in the body and
light-green on top; it does not yield as much sugar as the
former, but as more beets can be grown on the same amount
of ground, it produces more sugar. It is much cultivated in
France and Germany.
Sihe7*ian beet is known as the white-ribbed beet; it is pear-
shaped, with very light green ribbed leaves. Percentage of
sugar in this beet is less than Silesian beet, although of
greater weight.
The French or Belgian beet has small leaves and a slender
and spiral root, yielding sugar.
The Imperial beet is slender, pear-shaped, very white, rich
in sugar, but does not yield as well as Silesian beet.
The King beet is a biennial ; in the first year the root is
merely developed ; in the second it bears seed.
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470
THE CHEMISTS' MANUAL.
ANALYSES OF SUGAR BEET&*
Naio.
1
1
1
fi;
1^
1
m
OB
<
Ahaltr.
Hobenhelm
MoBckem
81.6
84.1
81.7
79.5
80.0
80.0
79.0
88.7
81.8
8S.1
885
84.4
88.7
84.1
0.87
0.83
0.84
0.90
0.70
0.68
0.66
0.96
1.16
1.14
1.05
1.14
148
1.80
11.90
9.10
11.81
18.07
18.90
18.87
18.88
18.84
10.15
9.86
8.46
9.80
11.67
9.88
8.47
8.90
1.88
1.05
0.89
0.99
0.94
OM
0.70
0.74
0.00
0.79
1.18
1.15
0.98
0.09
0.63
0.77
Wolff.
Ritthaasen.
" 9 lbs
S.86 1.86
5.09 IJSSt
5.00 1.80
u
" 1 "
i.
Blckendorf. li lbs
Groaven.
Slaadstadt. 3 lbs
5.81
6.58
8.94
6.77
6.86
7.07
896
8.68
4.04
StOckbardt
Lockwita, 1\ '»
Tharand H *' manured
1*" " :;::::
Silesia, maniired
u
(I
Bretscbnieder.
'' *' with ftodic nitrate
** calcic pbos.
»i
Aveiage
81.5
0.96
11.5
8.7 1 1^
0.86
• From " How Crope Grow "— (Johnson).
The following analysis is more elaborate than the above,
and is considered a fair average analysis of the sugar beet.*
Water.
Percent
82.60
(1.) InsolvbU Constituents.
CellnloBe
Pectose, pectase, pectic, and pectosic acide
Metarabic acid
Fatty, waxy, and resinous bodies
Albuminoids
Pectates, parapectates, metapectates, pectosates, oxalates,
and phosphates of magnesium, caldnm, iron, and man-
ganese
Silica
0.80
0.dO
Cane-sugar .
Glucose . . . .
(2.) Soluble ConetUuentB.
11.80
1.50
Albumen, casein, etc ,
Asparagine (C4HgNjO,) —
Betaine(C5HiiN0a) 0.10
Carried forward 96.00
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THE CHEMISTS' MANUAL.
471
Brought forward
Pectine, parapectin, metapectin, and pectase.
ftumxny bodies
Cromogene
A yellow extractive body
Parapectic, metapectic, aspartic, citric, and malic adds
Pectates, parapectates, metapectates, citrates, malatea, ox-
alates, aspartates, sulphates, phosphates, nitrates, and
chlorides of potassium, sodium, rubidium, and ammo-
nium
Citrates, malates, asparates, sulphates, nitrates, and chlo-
rides of magnesium, calcium, iron, and manganese
SiMca.
96.60
a40
100.00
Near Magdeburg, where the beet is extensively cultivated,
the general results give :
The greatest sugar productions, as 18.8 per cent.
That from inferior beets. 9.2 " "
The average beet yielding 11,8 " '*
12J cwts. of beet yield on an average 1 cwt. of raw sugar.
THE ANALYSIS OF CANE-SUGAR.
OOOTTITU a UTS.
Oxygen . . .
Carbon. . . .
Hydrogen .
Li
56.63
42.47
6.90
49.856
43.265
6.875
Pbout.
53.35
6.66
XJVM.
50.83
43.88
FownM.
51.59
41.98
6.43
51.46
42.11
6.43
Formula for Sugar (sucrose), Ci,H,|Oii.
SACCHARIMETRY.
There are several methods for determining the amount of
saccharine matter contained in the various crude sugar pro-
ductions ; the following may be employed :
1. Mechanical,
2. Chekical, or
8. Physical Method.
* Taken from article on Sugar by C. F. Chandler— (Johnson's Cyd.).
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*72 THE CHEMISTS* MANUAL.
The Mechanical Method is applicable for determiniDg
the sugar in beets :
" The* middle part of the beet is cut in thin slices to the
weight of 25 to 30 grams each and dried. From the differ-
ence in weight before and after drying, the quantity of water
contained in the root is ascertained. The dry residue is pul-
verized, and then treated with boiling dilute alcohol of a
specific gravity of 0.83. By this means the sugar is dissolved
and the weight ascertained. The insoluble residue gives, after
drying, the weight of the cellulose, proteine bodies and min-
eral constituents. If the alcoholic solution be placed in a
vacuum over caustic lime, it gradually becomes more and more
concentrated until, after standing about a day, the sugar,
owing to its insolubility in absolute alcohol, may be collected
in small colorless crystals, only absolute alcohol remaining.
Good sugar-beets give 20 per cent, dry residue, the water
amounting to 80 per cent. Of the 20 per cent., 13 per cent,
is usually sugar, and the remaining 7 per cent, pectine,
cellulose, proteine, and mineral substances. The higher the
specific w^eight of the juice of the beet, the more sugar it con-
tains. The juice of a good beet properly cultivated marks
8° and sometimes 9° B."
"Chemical Method. — The chemical method is based on
the following facts :
a. The known proportional solubility of calcic hydrate in
cane-sugar.
J. The capability of a cane-sugar solution to reduce the
hydroxides of copper to protoxides, the quantity reduced
affording an estimate ; and the conversion by acids of cane-
sugar into inverted sugar (a mixture of levulose with dextrose
or glucose).
c. The fermentation of sugar, giving rise to the formation
of alcohol and carbonic acid, the amount of which can be
ascertained, 4CO2 corresponding to one molecule of cane-sugar
C12H22H1 !•
* Wagner's Technology.
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THE CHEMISTS' MANUAL. 473
The first of these methods is that of determining the solu-
bility of calcic hydrate in a cane-sugar solution. The fluid
coutaining sugar is stirred with calcic hydrate, the quantity
of which dissolved, estimated by titration with sulphuric acid^
determines the quantity of sugar.
The second method is grounded on the researches of M.
Trominer, who found —
(1.) That cane-sugar in an alkaline fluid does not reduce
cupric oxide ; but it becomes reduced if the sugar has pre-
viously been boiled with sulphuric or hydrochloric acid, the
acid converting the cane into inverted sugar.
(2.) The quantity of the reduced protoxide is proportional
to the quantity of sugar. Barreswil and Fehling give a test
based on this law. An alkaline solution of cupric oxide is made
by dissolving 40 grams of cupric sulphate in 160 grams of
water, and adding a solution of 160 grams of neutral potassic
tartrate in a httle water, with 600 to 700 grams of sodic
hydrate of a specific gravity 1.12. The mixture sliould be
diluted to 1154.4 c.c. at 15**. A litre of this copper solu-
tion contains 34.65 grams of cupric sulphate, and requires
for its reduction 5 grams of dextrose or levulose ; or 10
atoms cupric sulphate (1247.5) are reduced by means of one
atom of dextrose or levulose (180) to protoxide (34.65 : 5
= 1274.5 : 180 or 6.93 : 1), 10 c.c. of the copper solution
corresponding also to 0.050 grams of dry dextrose or levulose.
Mulder prefere a solution in which 1 part of cupric oxide
corresponds to 0.552 parts of dextrose or levulose of the
formula CgHjgOg + HaO; by the use of this test-liquor, the
amount of sugar can be ascertained with great accuracy. By
another method 10 c.c. of this copper solution are heated with
40 c.c. of water, and placed in a sugar solution tiU all the
cupric oxide is reduced. When this point is nearly reached,
the precipitate becomes redder and forms more rapidly. Test-
ing the filtrate with potassic ferrocyanide, will throw down a
yellow precipitate if there be sugar in excess. The copper
salts are instantaneously reduced by the sugar in correspond-
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474 THE CHEMISTS' MANUAL.
ing quantities ; long boiling is not necessary ; 100 parts of
dextrose or levulose correspond to 95 parts of canensugar."
Febment Test. — " The third method, the ferment test, as it
is generally termed, is grounded on the fact that a solution of
sugar may be preserved for an indefinite period in an open or
close vessel ; but that if decomposing, azotized matter be acci-
dentally or intentionally added, the sugar is converted first into
dextrose or levulose, which, suffering vinous fermentation, is
converted into alcohol with the evolution of carbonic acid :
1 moL of cane-sugar ) yields by j 4 mols. of carbonic acid = 176,
(CjtHjaOi, =842) ) fermentation i 4 mols. of alcohol = 188.
The estimation of the quantity of carbonic acid is easily
performed by means of the alkalimetric apparatus of Fresenins
and Will. The fermentation being complete, the air is sucked
out of the apparatus and the amount of carbonic acid estimated
from its loss, which —
multiplied by ^ = 1.04d2 gives the quantity of cane-sugar ;
" Vji = 2.04646 gives the quantity of dextrose."
IV. A mixture of one-third volume ether with two-thirds
volume absolute alcohol. This is neither charged with acid
nor saturated with sugar.
SCHEIBLER'S METHOD.
This method is founded on the principle of treating samples
of sugar with saturated solution of sugar in alcohol ; this solu-
tion dissolves and eliminates the impurities of the sample
without in the least acting upon the crystallized portion. The
necessary reagents for analysis are :
I. Alcohol of 85-86"* mixed with acetic acid (50 c.c. to each
litre of alcohol), and saturated with sugar. For this a good
refined sugar is taken, which is powdered and introduced into
the bottle; the above-mentioned solution is poured in, it is
hermetically closed, and shaken frequently during several days.
II. Alcohol of about 92°.
III. Alcohol of about 96°. Alcohols II and III have no
addition of acetic acid, but are saturated with sugar, as was
the case with the first solution.
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THE CHEMISTS' MANUAL. 475
The apparatus required is shown in the figure.
It consists of a 50 c.c. flask ; the neck of the flask is some-
i^hat enlarged, as shown in the figure A. Through a rubber
stopper K is inserted the glass filtering-tube OS. At tlie
lower end of this tube is fastened a somewhat larger tube, and
to this is fitted a felt-filter. There is also a flask B, in which
a vacuum can be formed by means of suction. This flask is
attached to A by means of the rubber tube P.
The operation is as follows : A normal quantity of sugar is
weighed (26.048 grams if the Ventzke's polariscope is used,
or 16.35 grams if the Duboscq) in the flask A. The stopper
with the filter-tube is inserted in the fiask.
Solution IV is now introduced into the flask and allowed to
remain for fifteen or twenty minutes, during which time the
water of the sugar, as also the small quantities of foreign sub-
stances, such as fatty bodies, alkaline salts, alkaline salts of
fatty acids (butyric, valerianic, etc.), are dissolved, and the
sugar is precipitated. The alcohol and ether is then with-
drawn into the flask B by means of suction applied at m.
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476
THE CHEMISTS' MANUAL.
After this solution No. I is introduced, and then No. II,
about 10 c. c. of each. This washing separates the absolute
alcohol adhering to the sugar, which is finally saturated with
solution II. After this latter has been drawn oft' by suction,
solution No. I is introduced. The solution is left for fifteen
to twenty minutes, suflBcient time for the solution of all im-
purities of the raw sugar, the molasses, during which time the
mass of sugar diminishes in volume and settles ; the solution
is then removed by suction the same as the others into the
flask B. The filter-tube is now withdrawn, and any adhering
sugar is washed into the flask ; tri-plumbic acetate is added,
then water, until the 50 c.c. mark is reached. The solution
is then polarized. By this improved method it is claimed
that great exactness can be obtained, much time spared, and
less liability to loss than in the first method proposed by
Scheibler. The operation occupies about two hours, and sev-
eral analyses can be carried on at the same time.*
Physical Method. — M. Soleil has constructed an apparatus
based upon the rotatory power of liquids, for analyzing sac-
charine substances, to which the name aaccharornetei* is applied.
The following table shows the efiect of sugars on polarized
Ught :
SUGABS.
Cane-sugar (sucrose)
Melezitose (from Larch manna)
Mycose (from Turkish manna, product )
of an insect) \
MeUtose (from eucalyptus)
Dextrose (grape-sugar)
Malt-sagar (maltose)
Fruit sugar (laevulose)
Eacalin (from fermentation of melttoee). .
Sorbin (from berries of the service tree). .
Milk-suflfar (Uictose)
Galactose
Inverted sucrose (from honey and manna )
and some fruits) f
FoBxnuE.
c: h!:o:
C. H,,0,
C, H„0.
Effect on PoLABxm)
Light.
Right, 73'.8.
94M.
" 198\0.
" 103°.0.
57M
« 172°.0.
Left,106^atl8'5C.
Right, 50 .0.
Left. 46=.9.
Right. 56%4.
" 83".8.
Left, ^S"* at 1412* C.
* For details for preserving solutions, etc., see Am. Chem., March 187S
and September 1878.
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THE CHEMISTS' MANUAL. 4:77
The above table, according to Berthelot, are the rotary
powers of the diflTerent varieties of sugar, if equal weights of
each are dissolved in an equal bulk of water ; the quantity of
each sugar is calculated for the formulse annexed.
SOLEIL-DUBOSCQ SACCHARO METER.
* ^otEEEEEH^fifeS^ ■*
KK'
H, — Is a ray of light (Argand burner, gas-light is generally
used).
P, — ^Is the polarizer, formed by two prisms, one of crown
glass, the other of calc spar. The ordinary and extraordinary
rays are polarized at right angles, the ordinary ray alone meets
the eye. The principal division of the spar is in a vertical
plane with the axis of the instrument
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478 THE CHEMISTS' MANUAL.
R, — Two quartz plates of opposite rotating power cut per-
pendicular to axis (c and d) of instrument, having a thickness
of 3.75 millimetres (or 7.50 m.m.), equal to a rotation of 90°,
and giYes a violet tint called the "tint of passage," or
" transition tint.*'
T. — This is the tube made of copper or brass, which is
sometimes tinned inside, with two glass plates for each end to
close the tube withy so that it can hold the liquid to be
analyzed.
Q. — This is a quartz plate 5.5 millimetres thick, having the
property of right-handed rotation.
KK'. — This is a wedge of left-handed quartz ; it is made by
cutting a quartz plate with two parallel sides, obliquely, so
that they will have the same angle. The scale of the instru-
ment is attached to these parts : ab = cd = 4 millimetres.
A, — Is the analyzer. Formed in three parts : the first is a
very small flint-glass prism, the second is a crown-glass prism^
the third is a prism of calc spar.
C, — Is a plate of quartz.
LL'j — Is a Galil6e Telescope.
N, — Is a nickel prism, which with C (quartz plate) produces
the sensible tints.
S, — Is the eye of observer.
NoTB. — ^The Daboeoq inBtnunent, in oompariaon to the Ventzke, is best
adapted for the examination of raw sugars, for the reason that only 1S.85
grams are taken for analysis, whilst ^.048 grama are required for the
Ventzke instrument Some raw sugars are very dark-oolored, and are diffi-
cult to decolorize ; therefore, the least amount of sugar taken in a girea
quantity of water (100 cc.), the easier wiU it be to decolorise the i
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THE CHEMISTS' MANUAL.
479
THE ANALYSIS OF SUGAR BY MEANS OF THE
OPTICAL SACCHAROMETER.
The analysis of sugar solutions by means of the optical saccha-
lometer usually gives rise to one of the following problems :
(1.) " To determine* the quantity of pure sugar in the solu-
tion such as it is ; or,
(2.) To determine the quantity of pure sugar in the solu-
tion, irrespective of the quantity of water in it ; t. e,y the
quantity of pure sugar in the substance as it would be if
deprived of its water, or, more briefly, the quantity of sugar
in the dry substance.'*
In the first case we must treat it as we would any other
saccharine substance, as for example —
RAW SUGARa
The raw sugar to be analyzed is first weighed : 16.35 grams
are taJken if a Soleil-Duboscq saccharometer is to be used, or
26.048 grams if a Yeutzke-Soleil instrument is used. The
sugar weighed is dissolved in a small beaker,f in about 60 c.c,
of water, and then transferred to a small flask of 100 c.c.
capacity, being careful to dissolve every particle of the sugar
and transfer the same to the flaskj where it is diluted to
90 C.C., after which 4 c.c. of a solution of common salt is
added, and then 6 c.c. of tri-plumbic acetate, making in all
10 c.c. The flask is then agitated for a few moments, when
the contents are flltered. If the filtered solution has a reddish
color, J it may be filtered through weU-dried bone-black, when
the red color will disappear. If bone-black is not at hand, to
50 c.c. of the filtrate add 50 c.c. of water and filter if neces-
sary, when a solution will be obtained which can be examined
in the saccharometer.
• Amer. Chem., Oct., 1S73. Article by P. Casamajor.
f It is only in cases of very dark sugars that the filtrate may sometimefl
be red ; when red it cannot be nsed in the instrument.
X Nickel-plated copper-beakers wiU be found to be veiy useful, espedaUy
In the case of centrifugal sugars, which are difficult to dissolve.
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480 THE CHEMISTS* MANUAL.
The filtrate of a white or yellow color is now to be exam-
ined in the saccharometer. The tube of the inBtrament of
20 C.C. capacity, and 20 centimetres in length, is thoroughly
washed out with the filtrate and then filled to overflowing, when
the open end is covered by a round piece of glass, and the cap
is put on. The tube is then put in the instrument and the
solution examined. It is necessary to see that the zero (0)
point on the scale of the instrument is correct ; this is accom-
plished by means of a tube filled with pure water.
The color of the field best adapted to examine the solution
depends on the sensitiveness of the eye. Experience has
shown, though, that a yellow field is the most sensitive.
When once the tints of the two halves of the plate are
exactly alike, the division of the scale corresponding to the
vernier is read ofi^, and the corresponding number gives the
strength of the solution.
In the second case, that is,
TO DETERMINE THE QUANTITY OF PURE SUGAR IN A
SOLUTION, IRRESPECTIVE OF THE QUANTITY OF
WATER IN IT.
The following is the process of P. Casaraajor : * Two cases
may present themselves : either the solution is light-colored
enough to be placed in the saccharometer, or it is dark and
needs to be decolorized. Suppose a solution which, after dilu-
tion, its density falls between 5° and 15° Balling, is light-col-
ored enough to go into the saccharometer. First place the
areometer in the solution; suppose that it indicates 14:°.3;
next place in the solution a thermometer which will indicate
say 27 J ° C, and note that the excess of 27^° over 17 J° C. is 10^
[Note. — The indications of the areometer are true : for the temperature of
17^" C. and for any other temperature, either higher or lower, we must con-
sult the table for " correction of temperature," which is given on p. 482.]
It is necessary to turn now to the Table for Correction of
Temperatures, and find the quantity to be added to the degrees
Balling as 27^° > 17J° = -f 10. Opposite 10 in the table is
♦ Amer. Chem., Nov. 1873. p. 161.
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THE CHEMISTS' MANUAL. 481
0.545, whicjh we add to 14°.3 Balling = (14^3 + 0.545 =
14°.845) 14°.84 comes nearest to 14.8 of the table marked
Duboseq, and opposite to 14.8 is 1.043, and in the table
marked Ventzke, 1.659.
Suppose a Yentzke instrament is used, and the solution
indicates 43 per cent. ; by multiplying 43^ by 1.659 = 71.33^
gives the quantity of pure sugar in the dry substance of the
solution.
If the solution is too dark to be used in the saccharometer,
it must be decolorized. The first step to be taken is to test
the solution with the areometer and thermometer, and obtain
the rectified degree Balling corresponding to 17J° C. Op-^
posite to this degree Balling we find in the table the corre-
sponding factor, which is written down for future use.
The solution is next clarified by adding the " sodic chloride
solution " and tri-plumbic acetate. The total addition will be
10 per cent, of the volume of the sugar solution. K the solu-
tion is light, 5 per cent, will do. As this addition of liquid
weakens the saccharimetric strength of the solution by 5 or
10 per cent., according to the quantity of decolorizer added,
it must be compensated for by adding 5 or 10 per cent, to the
factor written down. The solution, after being filtered, is
finally placed in the tube of the saccharometer, and the indica-
tion of the instrument is multiplied by the factor obtained by
adding 5 or 10 per cent, to the factor of the table.
NciTERTCAL EXAMPLE. — Supposo we have a dark solution. After being
dilated with water, it \s tested by the areometer and thermometer, showing
IV A BalUng, the temperature being 25|° C. The excess of 26^ oyer 17^^
= 8. Opposite 8 in Table for Ck>rrection of Temperatures we find 0.486,
which is added to 11*.4 Balhng (ir.4 + 0.436 = 11.886). Suppose we have
a Ventzke instrament, we find in the table marked Ventzke, opposite 11.8
(nearest 11.886), 2.107, which we write down. The solution being dark, we
add 10 per cent, of clarifying solution, say 8 or 4 per cent, of sodic chlo-
ride, and the balance tri-plumbic acetate As this weakens the solution, we
compensate for it by adding to the factor 2.107, 10 per cent, of its value =
0.2107, which ^ves 2.317. The solution, after being clarified by filtration
is placed in the saccharometer, and then shows say 22} per cent. By multi-
plying 2.317 by 22|, we obtain 52.1, which is the percentage of pure sugar
in the dry substance of the solution.
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482
THE CHEMISTS' MANUAL.
TABLES FOR THE CORRECTION OF TEMPERATURES.
.Difference between
the temperatare ob-
served and 17^" C.
1
2.
8.
4
5.
6 .
7,
8 .
9
10
11 ,
12
18
14,
15
Quantity to be added
or aabtracted from
degree Balling.
0.054
0.109
.. .. 0.168
0.218
.. 0.272
0.327
0.381
0.436
0.490
0.545
0.600
0.664
0.708
0.762
0.817
VENTZKE.
Table of factors, corresponding to degrees Balling, to be muUipUed hn the
indication of the saccha/rometer.
W
11
^ !
11
^
HO
h
I Si
III
Il3.
i
6.
5.107
7.
8.618
9.
2.792
11.
2.267
1.902
5.1
5.013 I
7.1
a668;
9.1
2.762
11.1
2.246
, 18.1
1.887
6.2
4.920 1
7.2
8.519 1
9.2
2.781
11.2
2JJ25
18.2
1.878
58
4.820 1
7.8
8.470 !
9.8
2.700
11.3
2.204
' 13.8
\m
5.4
4.733 1
7.4
8.430'
9.4
2.670
11.4
2.184
1 18.4
1.844
5.5
4.639 1
7.5
8.871 1
9.5
2.640
11.5
2.163
18.5
1.829
6.6
4.559
7.6
8.323.
9.6
2.612
11.6
2.144
, 18.6
1.815
6.7
4.479 '
7.7
3284
9.7
2.585
11.7
2.125
1 18.7
1.801
58
4.399'
7.8
3.240
9,b
2.558
11.8
2.107
1 18.8
1.787
5.9
4.319 ,
7.9
3.197
9.9
2.580
119
2.088
1 18.9
1.773
6.
4.239
8.
3.15.4
10.
2.508
12.
2.069
14.
1.759
6.1
4.171 1
8.1
3.116
101
2.478
12.1
2.052
141
1.746
62
4.103 '
8.2
8.078
10.2
2.453
i 12.2
2.034
' 14.2
1.733
6.3
4.035
8.3
3.089
10.8
2.428
12.8
2.016
' 14.8
1.721
6.4
3.968
8.4
8.001
10.4
2.408
12.4
2.000
' 14.4
1.70B
6.5
3.909
8.5
2.963
10.5
2.878
i 12.5
1.982
14.5
1.695
6.6
8.844
8.6
2929
10.6
2.856
i 126
1.966
146
1.688
6.7
8.787
8.7
2.895
10.7
2.884
12.7
1.950
147
1.671
6.8
8.730 1
8.8
2.860
10.8
2.311
12.8
1.984
, 148
1.659
6.9
3.674 1
8.9
2.826
10.9
2.289
12.9
1.918
! 149
1648
1
1
1
15.
I
1.638
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THE CHEMISTS' MANUAL.
483
DUBOSCQ.
Table of faetors, correspondi/if/ to degrees Balling, to he muUipiied hy the
indiecUion of the eaceharometer.
6.
6.1
5.3
68
6.4
5.5
6.6
5.7
5.8
5.9
6.
6.1
6.2
6.8
6.4
6.5
6.6
6.7
6.8
6.9
3.206
8.151
8.097
8.042
2.988
2.988
2.879
2.824
2.770
2715
2.661
2.622
2.588
2.544
2.505
2.466
2.427
2.888
2.349
2.810
7.
7.1
7.2
7.8
7.4
7.5
7.6
7.7
7.8
7.9
8.
8.1
8.2
8.8
8.4
8.5
8.6
8.7
8.8
8.9
2.271
2.240
2.207
2.176
2.147
2.116
2.088
2.061
2.084
2.007
1.980
1.955
1.981
1.906
1.882
1.860
1.839
1.817
1.796
1.774
9.
9.1
9.2
9.8
9.4
9.5
9.6
9.7
9.8
9.9
10.
lO.l
10.2
, 10.8
I 10.4
, 10.5
! 10.6
I 10.7
, 10.8
I 10.9
1.763
1.784
1.714
1.695
1.676
1.657
1.640
1.622
1.605
1.588
1.571
1.555
1.540
1.524
1.508
1.493
1.479
1.465
1.451
1.437
11.
11.1
11.2
11.8
11.4
11.5
11.6
11.7
11^
11.9
12.
12.1
122
12.8
12.4
12.6
12.6
12.7
12.8
12.9
1.423
1.410
1.397
1.884
1.871
1.358
1846
1.834
1.823
1.311
1.299
1.288
1.277
1.266
1.255
1.244
1.234
1.224
1.214
1.2(^
18.
18.1
13.2
13.3
13.4
18.5
18.6
13.7
13.8
13.9
14.
14.1
14.2
14.8
14.4
14.5
14.6
14.7
14.8
14.9
15.
1.194
1.185
1.176
1.166
1.157
1.148
1.139
1.130
1.122
1.113
1.104
1.096
1.088
1.080
1.072
1.064
1.056
1.049
1.048
1.084
1.027
DETERMINATION OF THE WATER IN SUGAR.
There are two methods which can be employed :
(1.) By drying the sugar near the point of caramelization ;
i. ^., 120° to 130°, the loss in weight will equal the water.
The operation requires about two hours.
(2.) By means of the " water areometer." The following is
a description of the process of P. Casamajor :
To determine the amount of water in sugar : Take 16.35
grams of the sugar to be tested, which dissolve, so that the
solution shall occupy 100 c.c. without adding tri-plumbic ace-
tate or any other decolorizing agent.
After shaking up thoroughly, so as to have a uniform liquid,
pour some of it into a glass cylinder ; put an areometer into
t^e solution and note the division to which it sinks ; also note
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484
THE CHEMISTS' MANUAL.
the temperature of the solution. The indications of the
areometer show the quantity (provisional) of water in the sugar
tested, if the temperature is 17J° C. If the temperature is
not 17^° C, corrections are to be made by means of the fol-
lowing table :
Degrees Cel»lnB,
above or below
17*0.
Qnantlty to add
when below and to
subtract when
above 17ft C.
Suppose 70a have the indication
of your areometer 2.60 and that of
the thermometer 2^'' C. Then
23J - 17i = 6^ Opposite 6** you
find 2.16. The amount of water is
1
0.36
2
8
4
6
0.71
1.07
1.44
1.80
2.60
-2.16
Provisional, 0.86 per cent
6
2.16
If the areometer indicates 2.50
7
2.50
and the thermometer 14° C; the
8
9
10
2.87
8.12
8.48
difference 17^ - 14** = Sy, to
which correspond 1.25, average of
11
8.84
1.07
12
4.20
1.44
13
14
16
16
4.65
4.81
5.16
6.52
2)2.51
1.26
2.60 + 1.25 = 3.75 per cent (pro-
visional).
There is another correction to be made which relates to the
salts contained in the sugar. Suppose we have a sugar giving
in the saccharometer 85 per cent. ; the water areometer, after
correction for temperature, giving 4 per cent. The sugar may
be provisionally put down :
Saccharimetric ... 86 per cent )
Water 4 " > ProviaionaL
Impurities 11 " )
Casamajor found, by comparing a large number of tests in
which he determined the ashes, that ^ of the impurities in
cane-sugar and ^ in beet-sugar should be added to the water
as found above, to correct the error due to salts.
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THE CHEMISTS' MANUAL. 486
Thus, in the above example, J^ = 0.55, whidi, when added
to 4, makes 4.55 per cent. ; therefore, we have —
Saccharimetric 85 per cent.
Water 465 "
Impurities 10.46
100.00
By the above process the amount of water may be deter-
mined very rapidly.
If it is desirous to determine the quantity of sugar, using
the same solution, add to it 5 or 10 per cent, of decolorizing
material, and to the result of the saecharometer add 5 or 10
. per cent, to counteract for the dilution.
DETERMINATION OF THE SCALE OF THE WATER
AREOMETER.
The 0 point is obtained by dissolving 16.35 grams of pure,
dry sugar in water, so that the solution will occupy 100 c.c.
at 17^*" 0. The next point to be determined is 10 per cent.,
which is easily obtained by taking 90 c.c. of the above solu-
tion and diluting with pure water up to 100 c.c. This second
solution at 17J° C. corresponds to a sugar having 10 per cent,
of water. Having obtained the 0 point, as also the 10 per cent.
on the instrument, the space may be divided equally between
these two points for the percentages. The points obtained
thereby are not strictly correct, but the error committed is
only a theoretical one, and is not appreciable on such an
instrument.
The different points give the true percentage of water in a
sample of sugar at 17J° C, after allowing for the correction
due to salts mentioned above. At any other temperature, cor-
rection must be made as above.
DETERMINATION OF THE ASH IN SUGARS.
Weigh out 9 grams of the sugar, to be examined in a
platinum-dish, and add four drops of sulphuric acid, diluted
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486 THE CHEMISTS' MANUAL.
in about 2 centimeters of water. The platinum-dish is gentlj
heated at first to prevent bubbling over, and finally heated
strongly to incinerate the carbon. The result is the same as
taking 10 grams and deducting a tenth.*
• The reason for deducting one-tentli is to counterbalance the additional
weight due to the conversion of the sugar-salts into sulphate ; it is entirely
a conventional matter.
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I
ssagtng.
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ASSAY OF IRON ORES.
DIRECTIONS FOR SELECTING SAMPLES FOR ANALYSIS.
Several fragments should be selected from diflferent parts of
the vein or bed, amounting in the aggregate to fifty or sixty
pounds. Or when the ore has been mined and is lying in
heaps, several shovels-full of ore, coarse and fine, should be
obtained, so as to procure a fair average of the whole ; it is
also better to select from difierent parts of the pile— a keg-fuU
in all is sufficient. A few ounces, or even less, is all that is
actually required for the analysis, but it is better to pulverize
a large quantity together, and the portion analyzed is a much
better representation of the mine than a single fragment can be.
PREPARING THE SAMPLE FOR ANALYSIS.
" Break up in an iron mortar forty or fifty pounds of the
ore, into pieces that will pass through a tin sieve with half-
inch holes. Thoroughly mix the fine and the coarse. Now
break up about ten pounds of average quality, so that it will
pass through a sieve made of tin with quarter-inch holes.
Mix welly take one pound of this, and pulverize in iron mor-
tar, until it will pass through a sieve of 60 meshes to the linear
inch. Mix weU, take out about 50 grams, pulverize in agate
mortar, pass through muslin bolting-cloth, and put into a
small bottle, tightly corked, for analysis and special determi-
nations. Any portion of this taken for Assay or for Quali-
tative or QuANTTTATivE ANALYSIS, must bo pulverfzed to an
impalpable powder in an agate mortar."
In the assay of moN ores it is necessary to slag off from
the iron all the impurities, so that the iron will be set free in
a pure state. The formula for the slag must be = K^Oa-SiOa
+ 2(3K0.Si02).
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490
THE CHEMISTS' MANUAL.
Its approximate percentage eompositioii is :
Silica 88 1 r 2J parte.
RgOg (Alumina) 15 >- or aboat •< 1 part.
EO (CaO, MgO, etc.) 47 ) (Sparta.
CHARGES FOR ORES OF UNKNOWN COMPOSITION.
1. 8. 8.
Silica 2.5 1 4.0 grama.
Lome 2.5 4 1.5 "
Ore 10 10 10.
It is necessary to make two assays of the ore, using first
charge 1, then charge 2, etc.
TO CALCULATE THE CHARGE WHEN THE COMPOSITION
OF THE ORE IS KNOWN.
The ore contains—
Percent
10 tframB
orore
coDtaln—
Required to
form Blag.
Difference to
be added.
Silica
Alumina
CaO.MirO. etc
1.05
1.04
441
0.165
0.194
0.451
2.50
1.00
8.00
2.885
0.806
2.548
Kaolin is used a« a means to furnish alumina, and kaolin is
(AI2O3 J . SIO2 i). Now, since 0.806 alumina must be added to
charge to form the proper slag, twice as much kaolin must be
used, as only one-half of the kaolin is alumina. Therefore,
.806 X 2 = 1.612 grams of kaolin to be added. But in add-
ing 1.612 grams of kaolin, 0.806 gram of Si02 is added
because half of the kaolin is Si02. Therefore 0.806 grams
must be subtracted from the amount of Si02 to be added.
2.335 grams — 0.806 grams = 1.529 grams SiOg to be added.
The charge is therefore :
Ore 10. grams.
Silica 1.529 grama
KaoUn 1.612 **
Lime 2.549 "
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THE CHEMISTS' MANUAL.
491
The above example was where the ore did not contain suffi-
cient Si02 to form the required slag. The following is an
example of an ore containing too much Si02 :
The ore contatne—
Percent
30 fframs
ofore
contain—
Beqnlred
To be
added.
Silica
Alumina.
CaO, MgO, etc
25.96
6.92
7.59
2.596
0.692
0.759
2.50
1.00
3.00
0.096
0.308
. 2.241
To add 0.308 of AlgOg, twice 0.308 or 0.616 of kaolin must
be added. In adding 0.616 kaolin, 0.308 SiOj is added.
Therefore, since there is already 0.096 Si02 too much, there
will be 0.096 + 0.308 or 0.404 SiOg too much, and this amount
must be treated so that it will form a slag.
Constitaenta.
EzceBB.
Reqoired.
Difference to be
added.
Silica
0.404
3.50
1.00
8.00
2.096
Alumina
CaO MffO. etc
1.000
3.000
Now in adding 1.000 gram of AI2O3 two grams of kaolin
must be added, and in adding two grams of kaolin one gram
of Si02 is added ; therefore this amount of SiOj must be sub-
tracted from the amount of SiOa necessary to add, which is
2.096 ; /. 2.096 - 1.000 = 1.096.
The charge is therefore :
Ore 10 grams.
Silica 1.096 grams.
Kaolin 0.616 -f- 2.000 = 2.616 grams.
Lime 2.241 + 3.000 = 5.241 **
To add Si02, ground quartz is used. Ores containing
titanium require the addition of fluor-spar, 0.5 to 10 grams,
according to the amount of titanium that is present.
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492 THE CHEMISTS' MANUAL.
PREPARING THE CRUCIBLE.
The crucible used is a Hessian crucible. They are filled
with hrasque. Brasque in this case is four parts of pulverized
charcoal to one part of molasses. This is thoroughly kneaded
until a ball of it, made in the hands, resists to a sensible
degree an attempt to pull it apart.
The crucibles are packed full by driving the brasque in with
a mallet; a conical-shaped cavity of sufficient size for the
charge is cut out of the brasque with a knife, and the cavity
on the inside polished with a strong glasa tube. The crucible
is then dried by a fire (must not be heated too high).
PREPARING CHARGE.
The charge is weighed out and thoroughly mixed on glazed
paper, then put into the crucible. The top of the conical cavity
is then covered with a piece of charcoal, and then the whole
top of the crucible is covered with a coating of fire-clay (fire-
clay with one-fourth to one-half part of fine sand and a little
hair, thoroughly kneaded). The outside of the crucible is also
covered with fire-clay (very thin coating), and then the cruci-
ble is luted on a fire-brick and thoroughly dried before putting
it into the furnace. The fire should be kept up in the furnace
between four and 5 hours, with anthra^jite coal.
Duplicate assays should not vary more than 0.3-0.4 of one
per cent.
The button should be gray or grayish-white, the grain fine,
or tolerably so. PnosPHORrs in the ore makes the button cold'
short — ^hard, brittle, and a white metal. Sulphub makes the
button strong reticulated — ^mottled structure, and red-shorL
Manganese gives a button with a smooth surfece, hard and
non-graphitic; it presents a white crystalline fracture. The
slag obtained has an amethyst color, or yellow, green, and
brown when manganese is present in excess.
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THE CHEMISTS' MANUAL. 493
Chbomiuh gives a smooth button, " well fused, with a brilliant
crystalline fracture, and tin-white color ; at other times it is
white and only half-fused, or it may even form a spongy mass
of a clear gray color, according to the quantity of chromium
contained in the iron. The slag is dark and resinous, sur-
rounded with a tliin metallic coating."
" TrrANiUM gives a button with a smooth surface ; has a deep
gray fracture, dull and crystalline, and adheres strongly to the
slag. The button is sometimes covered with the nitro-cyanide
of titanium with its characteristic copper color. The slag is
resinous, black, and scoriaceous, curiously wrinkled on the out-
side, and covered with metallic pellicles of nitro-cyanide of
titanium with its characteristic copper color; sometimes the
slag is vitreous and of a bluish tint."
The following is a comparison between the results obtained
by analysis and fire-assay, by Ricketts :*
Ore. Iron by Analysis. Qy Fire Assay.
Magnetite 68.86 per cent 69.6 71.2 71.3 percent.
Hematite 44.50 " " 44.6 46.0 48.6 " «
Umonite 44.30 " " 448 44.6 45.2 " "
• " Notes on Afleaying," Ricketts, p. 89.
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494 THE CHEMISTS* MANUAL.
ASSAY OF GOLD AND SILVER.*
The assay of gold and silver will comprise : I. Assay of
Ores; IL Assay of Alloys.
I. ASSAY OF ORES.
PREPARATION OF THE SAMPLE.
It is essential, in the first place, to obtain a fair average
sample of the ore, otherwise the results of the assay may be
commercially worthless. Selection must be left to the judg-
ment of the assayer. The sample must be dried, if necessary ;
care being taken not to roast it. It must then be pounded in
an iron mortar, and passed through a sieve of eighty meshes
to the linear inch. If any native metal, in the form of scales
or filaments, remain upon the sieve, take the weight, separately,
of what has passed through and of what is left upon the sieve.
The latter must be assayed according to " Assay of Alloys,"
and the result referred to the whole amount of ore. It is essen-
tial that the whole of the sampUy except the malleable portion,
be passed through the sieve. Mix thoroughly the sifted ore.
The collection of the gold and silver in a button of metallic
lead is effected in a crucible, or in a scorifier, whence arise two
methods of assay : I. Crucible Assay ; II. Scoeification Assay.
The crucible assay is applicable to all ores ; the latter is limit-
ed, practically, by the small size of scorifiers, to the richer ores.
I. CRUCIBLE ASSAY.
An ore of gold and silver is composed of precious metal,
gangue, and oxides, sulphides, etc., of foreign metals.
To collect the precious metals in a button of lead, the ore is
mixed with litharge, suitable fluxes, an oxidizing or a reducing
agent, and fused in a Hessian crucible. Lithai^ is reduced
to metallic lead; the latter seizes upon the previous metals
and collects in a button at the bottom of the crucible, while
the foreign materials form, with the fluxes, a fusible slag above
the lead button.
* See Amer. Cbem., 1870— Articles by T. M. Bloeeom, E.M.
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THE CHEMISTS* MANUAL. 495
The crucible is broken when cold, and the malleable button
detached from the slag by hammering on an anvil. The fol-
lowing are the necessary reagents :
REAGENTS.
Litharge, Carbonate of Soda or of Potash,
Nitre, Argol (crude bitartrate of potash),
Charcoal, Borax Glass,
Silica, Common Salt.
Carbonate of Ammonia,
The reagents must be finely pulverized and dried, and kept
in closed vessels.
Borax should be fused to a glass and pulverized.
PRELIMINARY ASSAYS OF REAGENTS.
Ordinary commercial litharge always contains silver ; so it
becomes necessary to determine in each new lot the amount
of silver contained, for deduction from the silver found in the
regular assay of an ore.
There must also be determined, beforehand, the reducing
powers of argol and charcoal, and the oxidizing power of nitre.
This necessity arises from the impurity of the reagents. By
reducing power is meant the amount of metallic lead that one
gram of the reagent will reduce from litharge ; and by oxidizing
power, the amount of metallic lead that one gram of nitre will
oxidize. The following are the charges for the preliminary
assay:
I. REDUCING POWER.
Argol. CHABCOAii.
Argol 2 grams. Charcoal 1 gram.
Litharge .2 A.T.* Litharge 2 A.T.
Carb. Soda 1 A.T. Carb. Soda i A.T.
Salt to Cover. Salt Cover.
* A.T. means Assay Ton. It is obtained as follows :
1 Av. lb. contains 7000 grains = 16 Av. ob. 1 oz. = 437J grains.
1 Troy lb. contains 6700 grains = 12 oz. Troy. 1 Troy oz. contains
480 grains.
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496 THE CHEMISTS' MANUAL.
OxTDjZTNQ Power. Silver in Litharge.
Nitre 8 grams. Litharge 4 A.T.
Charcoal 1 gram. Carb. Soda 2 A. T.
Litharge 2 A.T. Charcoal 1 gram.
Carb. Soda J A.T. Salt Cover.
Salt Cover.
It is necessary to know the reducing power of the ore to be
assayed ; therefore a Pbeliminaby Assay is made.
CHARGE.
Ore 2 grams.
Litharge 25 "
Carb. Soda 10 "
Salt Cover.
The reducing power of an ore is due to the presence of
sulphur, arsenic, antimony, zinc, etc., but generally sulpbur
contained in the pyrites, etc. It is necessary, if possible, to
determine from the mineralogical composition of the ore to be
assayed, if it is rich or poor. K rich, ^ A.T., or J, ^, ^ A.T., is
taken. If the ore is poor, 1 A.T. or 2 A.T. is taken.
From the preliminary assay of reagents we have fonnd:
One gram of nitre will oxidize 5.4 grams of lead (about).
One gram of charcoal will reduce 24 grams of lead (about).
And from the preliminary assay of the ore we found that
2 grams of ore gave a button of lead weighing 3 grams.
METHOD OF CALCULATING CHARGES.
Example. — Ore pretty rich.
J A.T. will be taken of the ore.
Reducing power found 2 grams of ore = 3 grams of lead.
2 grams = 3 grams Pb.
1 gram = 1.5 grams Pb.
1 ton contains 2000 lbs. (2240). 2000 lbs. x 7000 gr. = 1400QpOO gnina in
one ton.
14000000 -4- 480 = 291661 Troy ounces in a ton of 2000 lbs.
0.001 gram = 1 milligram = 1 Asm}/ Ounce.
29166t -»- 1000 = 29.166} grams = 1 Assay Ton = 1 A.T.
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THE CHEMISTS' MANUAL. 497
1 A.T. is taken as 30 grams for convenience. J A.T. of ore
30 -^ 2 = 15 ; 15 x 1.5 = 22.5 grams.
A cupel should not be made to hold a button weighing
more than 18 grams ; and this button, 22.5 grams, is too large ;
it mast be reduced by oxidation.
22.5 — 18 = 4.5 grams too large.
Oxidizing power of nitre = 5.4.
.'. 4.5 grams H- 5.4 grams = .83 grams nitre required.
The charge is therefore :
Ore iA.T.
Litharge 1 "
Carb.Soda. i "
Nitre 83 grams.
Salt Cover.
In the above charge we see that 1 A.T. of litharge and J A.T.
were taken. The rule is to take twice as much litharge as ore,
and the same amount of carbonate of soda as ore. The salt
cover is used, as its name implies, to cover the charge in the
crucible. It also serves to wash down the sides of the crucible,
if the charge boils up.
The above charge is put into a Hessian crucible, and the latter
put into the fiirnace, covered over, on top of a brick laid on
the bottom. The crucible is left in the furnace equal times to
and from fusion. That is, if it takes ten minutes to promote
fusion of the charge (the knowledge of which may be obtained
by lifting the cover off the crucible and looking in), the cruci-
ble is left in the ftirnace ten minutes longer.
The above ore treated was a rich ore ; the following will be
a poor ore :
Example. — Ore is poor. 1 A.T. must be taken. Reducing
power of ore, 2 grams of ore = .35 gram of lead.
2 = .35 ; /. 1 = .175.
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498 THE CHEMISTS' MANUAL.
1 A.T. = 30 grams. .•. 30 x .175 = 5.25 grams.
Button wanted must weigh 18 grams.
18 — 5.25 = 12.75 grams too small.
1 gram charcoal = 24 grams Pb.
24 -=- 12.75 = I gram (about) of charcoal must
be added to charge.
The chaise, then, is :
Ore 1A,T.
Litharge 2 "
Carb. Soda 1 «
Charcoal ^ gram.
Salt Cover.
ORES TO BE ROASTED.
Ores containing a large amount of sulphur or arsenic, anti-
mony or zinc, should always be roasted.
ROASTING THE ORE.
The ore may be roasted in a cast-iron pan, a common spider,
over the crucible furnace. There ought to be a hood over the
furnace to carry off the fumes. The pan should be covered
with chalk on the inside ; an even coating may be made with
chalk paste, then dried over the fire. The coating prevents a
loss of ore.
The weighed sample of ore must be spread over the pan and
stirred, while heated with a bent wire until all fumes are
driven off.
Ores roasted have no reducing power ; then enough charcoal
must be added to reduce from the lead a button weighing
18 grams. 1 gram charcoal = 24 grams lead. For 18 grams^
therefore, .555 gram of charcoal must be added.
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THE CHEMISTS' MANUAL. 499
II. SCORIFICATION ASSAY.
The reagents necessary for a scorification assay are test^ead
and horax glass. The ore is mixed with these, put into a
scorifier, and Aised in a muffle.
The following table exhibits the proportions found by expe-
rience to be best adapted to the dilFerent gangues. The pro-
portions are referred to one part of ore :
Chancter of Qangiie. Fftrts Test-lead. Plaits Borax.
Qnartsose 8 —
Bmic (Fe,0„ A1,0„ CaO, eta) 8 0J85— 1.00
Galena 6—6 0.15
Aiscnical 16 0.10—0.60
Antimonial 16 0.10—1.00
Fahlerz 12—16 0.10—0.16
Iionpyritee. : 10-15 0.10—0.20
Blende 10—15 0.10—0.20
No preliminary roasting of ore is required. The scorifier is
gently heated at first, and then highly heated, until the button
of lead on the surface of the charge has disappeared, when it
is taken out of the muffle.
Charge of ore is generally |, J, or -j^jy of an assay ton.
CALCUUTING CHARGE.
Example. — Suppose the ore is rich (take J AT.) and gangue
antimonial. 1 A.T. = 30 ; | A.T. = 10.
We see by table, for ores having antimonial gangue, use
16 parts of test-lead and 0.10-1.00 of borax = .5 (average).
Therefore, 16 x 10 = 160 Pb, and .5 x 10 = 5 of borax.
Charge is therefore :
Ore JA.T.
Test-lead 160 grams.
Borax. 6 "
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500 THE CHEMISTS' MANUAL.
GALENA— SPECIAL METHOD.
It is best and most convenient always to make a scorification
assay of galena. If, however, it be desirable for any reason to
make a crucible assay, a Chabge of nitre, 20 grams per assay
ton of ore used, and the same weight of carbonate of soda as of
ore used.
CUPELLATION.
The lead button to be cupelled must be malleable, and the
proper size for the cupel, aboilt 12 to 15 grams. The cupel is
made of bone-ash, and weighs 18 grams ; it absorbs the scoriae,
leaving a pure bead of precious metal. The cupel must be
carefully dried before use, and must be free from cracks, which
would cause a loss of precious metal. The bottom of the
muffle should be covered with sand, to prevent injury to it by
upsetting a cupel.
Before introducing the button to be cupelled, the muffle, as
also the cupel, should be at a reddish-white heat. The button
melts, and gradually diminishes in size by oxidation and
absorption. When the bead becomes dull, then bright, resem-
bling precious metal, the cupel must be withdrawn, but very
gradually, to the front of the muffle, where it must be covered
over with an inverted cupel, and then the whole is withdrawn
and placed one side to cool. The beads of gold and silver,
when cold, is removed from the cupel, washed and weighed.
(The balance used for weighing must weigh down to one-tenth
of a milligram.)
INQUARTATION AND PARTING.
The separation of gold from silver is called parting. To
dissolve the bead in nitric acid, the silver must be 2.5-3 times
the amount of gold.
N.B.— The assayermust judge from the color of the bead if there is
enough silver present ; if not, he must add some to it by fuflion with *
blowpipe. This addition of silver is best done on charcoal.
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THE CHEMISTS' MANUAL. 601
The inquartated bead is flattened on the anvil, and treated
in a porcelain capsule with nitric acid, 1.16 sp. gr. (21° B.).
It is heated a little, until all the silver is dissolved from the
button, when, if gold is present, it will be left as a brown
powder, undissolved. (Acid must be free from all traces of
chlorine.) The gold residue is thoroughly washed with dis-
tilled water, detached by the knife, transferred to a cornet of
lead, and cupelled. The gold bead obtained is weighed, and
the ASSAY IS COMPLETED. It remains only to calculate the
results.
CALCUUTION OF RESULTS.*
Every milligram of precious metal obtained per assay ton
of ore corresponds to ounces in the ton of 2000 lbs. Av.
Example. — Suppose that the sample presented for assay
gave, on being pulverized and passed through the sieve of
80 meshes to linear inch, the following weights :
A. Sifted ore 1458.32 grams.
B. Scales of metol 40.75 "
- C. Total 1499.07 '*
It being known from the mineralogical composition of the
sample that it was a rich ore, ^ AT. was taken for an assay of
the sifted portion (A). The residue of metallic scales, etc. (B),
was scorified with test-lead, and yielded a button weighing
60.35 grams. This button was rolled out, and two average
samples of 10 grams each were cupelled.
The following results were obtained from the complete
assays:
A.-SIFTED ORE— CRUCIBLE ASSAY.
One-third assay ton, 9.722 grams yielded :
1. 8. AToragp.
Au + Ag. 0.19355 0.19275 0.19315
Au (by parting) 0.00025 0.00025 ^.00025
Ag 0.19330 0.19250 0.19290
♦ See Amer. Chem., 1870— Article by Blossom.
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602 THE CHEMISTS' MANUAL.
1. %. Ayenge.
Ag 0.19330 0.19250 0.19290
Ag in litharge* 0.00067 0.00067 0.00067
Aginore 0.19263 0.19188 0.:
B.— METALLIC SCALES.
10 gramfl of the scorified button yielded :
1. %. Avenge.
Au + Ag 5.0625 5.0620 5.0622
Au (by parting) 0.0020 0.0020 ft0020
Ag 5.0605 5.0600 5.0603
Ag in test-lead None None None.
A. Sifted ore (In all).... 1458.82 x -;J^ = 28.819 Ag.
9.722
B. Metallic scales (in all) 40.75 = ^^—^ x 60.35 = 30.538 Ag.
Total ore 1499.07 59.357, Total Ag.
1A.T. = 29.166666. 29166.66 = milligrams in 1 A.T.
29166.66 X -^^f- = 115471 oz. per 2000 lb.
A. Sifted ore 1468.82x5^^ =0.0876 Au.
B. Metallic scales 40.75 = ^^ x 60.35 = 0.0121 Au.
C. Total 1499.07 0.0496 Tl An.
29166.66 X j^^ = 0.97 oz. per 2000 lbs.
Bbsult per 2000 lbs. Obb.
saver 115471 oz. @ $ 1.29 $1,480J»
Gold 0.97 oz. @ $20.67 f 2a04
Total bullion. . . . 1155.97 oz $1,509.62
* The litharge yielded one milligram of silver per assay ton, and two-
thirds assay ton of it was employed.
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THE CHEMISTS' MANUAL. 603
ASSAY OF ALLOYS.
I. SILVER COIN AND BULLION.
The form of assay used for silver coin and bullion is that
known as Gay-Lussac's Wet Method, which consists in deter-
mining the fineness of the alloy by the quantity of a standard
solution of common salt necessary to precipitate, fully and ex-
actly, the silver contained in a known weight of aUoy.
Process embraces two steps :
A, Preliminary Assay, and B, Assay Proper. The latter
requires for its conduction the preparation of three solutions,
called Normal SaU^ Decime Salty and Decime Silver.
Normal Salt Solution. — This is a solution of common salt
of such a strength that 100 c. c. will exactly precipitate one
gram of silver. It is prepared as follows: Make a concen-
trated solution of salt in water ; take 10 c.c. and evaporate to
dryness in a weighed porcelain capsule, and weigh ; the in-
crease of weight will equal the amount of salt in 10 c.c. ; mul-
tiply this result by 10, and it will equal the amount of salt in
100 C.C. of solution. Suppose that 100 c.c. of the concentrated
salt solution contains 35 grams of salt. Suppose 45 litres of
the normal salt solution is required. If the salt were pure :
At. Wt Ag. At. Wt. T7aCL
108 : 58.5 : : 45 x 10 : x = 243.75 grams =
weight of pure salt required. But on evaporation of 100 c.c.
of solution, only 35 grams of salt were obtained ; therefore,
pure salt (243.75 -4- 35) x 100 = 696.29 = number of cubic
cent, salt solution required for 45 litres of water. Since in
adding the salt solution we also add 696.29 c.c. of water, there-
fore, 45 litres — 696.29 cc, or 44 litres 304 c.c. of water must
be added.
Decime Salt Solution. — This is a solution of common salt
only one-tenth the strength of the former ; i.e., 100 c. c. will
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504 THE CHEMISTS' MANUAL.
exactly precipitate 0.1 gram, 1 c.c. will precipitate 1 milligram
of silver. The solution is made by diluting the normal saU
solution with 8 parts of pure water.
Decime Silver Solution. — Dissolve 1 gram of pure silver in
nitric acid, and dilute to a litre ; 1 c.c. of the solution will con-
tain 1 milligram of pure silver.
The decime silver solution is equivalent to the decime salt
solution ; Le.^ if mixed in equal quantities, they wiU mutually
suffer complete decomposition.
The normal salt solution^ after being prepared, is tested and
accurately standardized. In three bottles of 250 c.c. capacity
(8 oz.), 1 gram of silver is dissolved (in each) in nitric acid,
and the whole largely diluted with water; then 100 c.c. of
normal salt solution is allowed to pass into the bottle, when
chloride of silver is precipitated ; the bottle, being closed by
a well-fitting glass-stopper, is shaken for quite a while ; if the
solution is clear on standing, the normal solution is of the right
strength, unless, by adding some of the decime salt solution, a
precipitate is produced; add 2 thousandths of the decime salt
solution^ agitate as before, and when solution becomes clear,
add again 2 thousandths decime salt, and repeat the operation
until a precipitate fails to appear. Suppose there have been
added 16 thousandths. The last two produced no precipitate
and are not counted. The two preceding thousandths were
only needed in part, so that the acting thousandths were above
12 and below 14 = 13 in number. Thus, 1013 parts of normal
solution are required to precipitate 1 gram of silver, while only
1000 parts or 100 c.c. should be required. The solution is too
weak, and the quantity of salt solution to be added may be
found by considering that 696.29 c.c. have produced a standard
of only 1000-13 or 987 thousandths. It remains to provide
for the 13 thousandths. The additional quantity of salt solu-
tion required is found as follows :
987 : 696.29 : ; 13 : a? = 9.2 c.c. of concentrated solution to
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505
be added. After this is added, the solution is tested the same
as before.
A.— PRELIMINARY ASSAY.
Weigh out one gram of the alloy and wrap it in a sheet of
lead (one sheet of lead about two inches square, weighing
■^^ ounces, or 5.287 grams), and cupel in the ordinary manner.
Suppose a button of silver is obtained weighing 0.8695 grams;
then —
Gram.
1 : 0.8695
1000 : X = 869.5 = approximate fineness.
This must be corrected for the unavoidable losses of a fire-
assay (Table from Mitchell). The corrections are given in
thousandths, and are in all cases to be added to the standards
of cupellation.
TABLE OF CORRECTIONS FOR LOSS IN CUPELLATION.
Stahbabd.
CoBsaoTioir.
Standabd.
COBBBCTIOH.
Stasdabd.
COBBKCnOlf.
M8.97
1.03
645.29
4.71
297.40
2.60
»73.24
1.76
620.30
4.70
272.42
2.58
947.50
2.50
595.32
4.68
247.44
2.56
921.75
8.25
570.32
4.68
222.45
255
896.00
4.00
545.32
4.68
197.47
2.55
870.98
4.07
520.32
468
173.88
2.12
845.85
4.13
495.32
4.68
148.30
1.70
820.78
4J32
470.50
4.50
123.71
1.29
795.70
480
445.69
4.31
99.12
088
770.59
4.41
1 420.87
4.13
74.34
0.66
745.38
4.52
1 396.05
3.95
49.56
0.44
720.36
4.64
371.39
3.61
27.78
0.22
695.25
4.76
1 346.73
3.27
670.27
4.78
' 822.06
1
2.94
The number in the column of standards next nearest to
869.5 is 870.93, and the corresponding correction is 4.07 ; add-
ing this to 869.5 we obtain 873.57 for the true approximate
fineness.
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506 THE CHEMISTS' MANUAL.
B.— ASSAY PROPER.
Take such a weight of the alloy as will contain one gram
of pure silver. This is found from the approximate fineness
by the following proportions :
873.57 : 1000 :: 1 : x = 1.145 grams.
Put this amount in an 8 oz. stoppered bottle and dissolve it
in nitric acid. Add 100 c.c. of no7*maZ salt solution , and pro-
ceed the same as in testing normal salt solution until the
decime salt fails to give a precipitate. Suppose six thousandth
of the decime salt solution were added ; the last gave no pre-
cipitate, so that more than 4 and less than 5 or 4.5 thousandths
are required. Add 1,5 thousandths of dechne silver solution ;
this will decompose 1.5 thousandths of the decime salt, which
was added in excess ; it is known that 4 thousandths decime
salt were wholly required ; the fifth gave a precipitate, but
was only required in part ; the 1.5 thousandth decime silver
added will decompose 1.5 thousandths decime salt; add now
0.5 thousandths decime silver; if a precipitate is produced,
between 4 and 4.5 or 4.25 thousandths decime salts were
required. If no precipitate was found on the addition of the
0.5 decime silver solution, 4.5 would thus be proved correct.
Suppose, however, that a precipitate had been obtained, the
number of thousandth normal salt solution would be 1000
<100 C.C.)* + 4.25 decime = 1004.25 ; I e., the weight of alloy
taken contained exactly 1004.25 milligrams, equal to 1.00425
grams of fine silver. The fineness is given by the following
proportion :
1.145 : 1.00425 : : 1000 : x = 877.07 (fineness).
The pieces of apparatus peculiar and most essential to the
assay of silver coin and bullion are the reservoir for contain-
* For sake of oonTenience the pipette of 100 c.c was diyided into 1000
parts.
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THE CHEMISTS' MANUAL. 507
ing, and the pipette with its connectionB for meaeuring the
normal solution.
A common glass carboy is a very suitable vessel for a reser-
voir, and is easily obtained and adapted to its purpose. The
following figure will show the method of arranging and con-
necting it with a simple measuring-apparatus. The carboy
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508 THE CHEMISTS' BiANUAL.
will hold about 60 litres, or 15-16 gallons. It has a paper
scale aflSxed to it, which is graduated by adding, successively,
a known number of litres of water until the carboy is filled,
and marking, after each addition, the height of the liquid.
B and V are parts of an hydraulic valve. B is a bell, or
cover of glass, through which the tubes pass, being fitted by
means of a cork. V is the neck of sheet-iron, about four
inches deep. The valve is closed with mercury, which should
fill the neck to about one-third of its height. An enlarged
section of the valve and tubes is shown at Y. The tube T
and the siphon S reach nearly to the bottom of the carboy ;
the former admits air to the carboy, and as no air can pass out
by the tube, evaporation is effectually prevented. The siphon
is jointed with rubber-tubing at " a," and has a stop-cock at
" b." It is furnished, at the lower end, with a piece of rubber-
tubing of sufficient length for connecting it with the lower end
of the pipette P ; the latter is supported by the brackets "cc,"
which are themselves affixed to the wall of the room, or to an
upright standard. The upper extremity of the pipette passes
through a vessel, " d," designed to catch the liquid running
over from the former.
The method of using the apparatus is, to attach the tube to
the pipette, as shown in the figure ; open the pinch-cock " e,'^
and allow the normal solution to fiow upwards into the pipette
until the latter overflows. Stow the flow and close the
pipette with the finger, as shown ; upon removing the rubber-
tube, and wiping off with a sponge any of the solution adher-
ing to the outside of the pipette below, the latter is ready to
deliver exactly 100 c.c. of liquid into the bottle placed to
receive it. The method of measuring the normal solution is
employed at the United States Assay Office in Ifew York; it
certainly has the merit of being simple and expeditious. We
have shown at Z the form of apparatus in use for the same
purpose at the School of Mines, New York. By this arrange-
ment the pipette is filled from above. EE are two sockets,
separated by a stop-cock, F. The upper one, which is screwed
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THE CHEMISTS' MANUAL.
509
inside, is connected by means of a cork '^ g," with the siphon
S, which condacts the normal solution. The lower socket is
cemented to the pipette, and is furnished with a conical air-
tap, G. Below the air-tap 6, and soldered to the socket, is a
very narrow silver tube H, conducting the solution into the
pipette, and allowing the escape of displaced air by the air-
tap. The cock F is provided with a thumb-screw "h," by
means of which it is adjusted on its seat; "cc" are brackets
for the support of the pipette and tube. To use the apparatus :
open the air-tap 6, and close the lower orifice of the pipette
with the finger ; open the cock F, and allow the solution to
fill the pipette above the 100 c.c. mark, then close the cock
and air-tap. The finger may now be removed, and the solu-
tion lowered to the 100 c.c. mark by allowing air to enter
slowly through the tap G. "When the liquid reaches the
proper level, close the tap and remove with a sponge any of
the solution adhering to the outside of the pipette, which is
now ready, on opening the air-tap, to deliver exactly 100 c.c.
of the normal solution. To facilitate the last part of the
■operation we employ the following contrivance :
0 is a cylinder of tin plate to receive the assay bottle, m is
s, sponge enveloped in linen and forced into a tube of tin plate,
terminated above by a cup, open below, so that the liquid
may run into the vessel B, on which the tube is soldered. The
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510 THE CHEMISTS^ MANUAL.
whole of this apparatus is affixed to a sheet of tin plate, mova-
ble in two slots, R R. The extent of this movement is deter-
mined by two stops, 1 1, BO placed that when the base of the
apparatus abuts against one of them, the pipette will be in
contact with the sponge, and that, when it strikes the other,
the orifice of the pipette will be directly over the centre of the
neck of the bottle. The sponge is placed in contact with the
pipette immediately after removing the finger.
The precipitated chloride of silver must be exposed to the
light as little as possible. Sunlight converts the chloride into
a subchloride, liberating chlorine, and thus vitiates the results.
This is avoided by placing the bottle in a cylinder of tin plate
when about to agitate the solution, and by keeping it, at other
times, in some receptacle which will shut out the light. We
employ for this purpose a table with a double top ; the upper
is pierced with holes, along its length, for the reception of the
bottles, which, when resting on the lower, hardly project above
the top. The table is also provided at the back with a black-
board and means for draining the bottles. On the blackboard
are recorded the additions of salt and of silver solution ; the
former are designated by a + sign, and the latter by a — sign.
The action of sunlight may be prevented by windows of
yellow glass, which exclude the chemical rays.
In the foregoing description it has been assumed that the
temperature of the normal solution remains the same as that
at which it was standardized. Such is not the case in practice,
for the temperature varies constantly. At a higher tempera-
ture the pipette will contain less salt, and at a lower tempera-
ture more salt ; consequently the standard of the bullion would
be fixed too high in the former and too low in the latter case.
It is convenient to standardize the normal solution for a tem-
perature of 20° C. A simple calculation will give the follow-
ing table of corrections to be made in the estimated standard
of bullion, when the temperature of the normal solution is
other than that at which it was standardized, or 20^ C. The
correction is given in milligrams or thousandths, and when
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THE CHEMISTS' MANUAL.
511
positive is added to, and when negative subtracted from, the
estimated standard.
CORRECTIONS
VOB E8TDCATED STANDABD OF BULLION CX>RRE8F02n}INO TO DIFFKRBNT
TEMFERA.TT7BB8 OF THE MORICAL SALT SOLUTION.
CXHT. DbQ.
OOBBBCTION.
Cknt. Dig.
CoRBacnox.
Cknt. Dm.
COBBECTXON.
10
+ 0.8
15
+ 0.6
20
0.0
11
+ 0.8
16
+ 0.5
21
-0.2
12
+ 0.8
17
+ 0.4
22
-0.4
18
+ 0.7
18
+ 0.3
23
-0.6
14
+0.7
19
+ 0.1
24
-0.8
It is not necessaiy for the normal solution to have a temper-
ature of 20° C. when it is standardized. Suppose it be 15® C. ;
from the above table, +0.6 is the correction for 16° C. ; i. e.y
100 cc. of a solution standardized at 20° C. will precipitate, at
15° C, 1000.6 milligrams of pure silver. The solution is there-
fore made of the latter strength, and corrected for a tempera-
ture of 20° C.
GOLD COIN AND BULLION.
The assay of gold coin and bullion comprises two determina-
tions: (a), of copper or base metal, and (5), of gold. The
difference between the sum of these two and the total weight
of bullion represents the amount of silver.
A.--BASE METAL DETERMINATION.
If the alloy contain no more than 20 thousandths of copper,
weigh out 0.600 grams, and cupel with half a sheet of lead.
If it contain more than 20 thousandths of copper, cupel
0.250 grams of the alloy with a whole sheet of lead.
K a large amount of silver be present, cupel 0.500 grams
with a whole sheet of lead. The copper is scorified and carried
into the cupel, leaving a button of gold (and silver, if there is
any). A check assay is made with every set of assays. A
proof alloy containing 850 parts of gold, 12 parts copper, and
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612 THE CHEMISTS' MANUAL.
38 parte Bilver, may be employed. This ought to lose by
cupellation just the 12 parts of copper. It may lose more or
less, and, according to the difference one way or the other, we
correct the regular assays which have been made under the
same conditions. Suppose the check assay yielded 11.8 thou-
sandths copper ; 0.2 thousandths have been retained, and the
proportion of copper in each of the regular assays must be
increased by that amount.
If the check assay had yielded 12.2 thousandths as the pro-
portion of copper, it would be known that 00.2 thousandths
of silver were lost, and the proportion of copper obtained in
each of the regular assays would be diminished to this extent
B.— GOLD PARTING.
Add to 0.5 gram of alloy enough pure silver so that the
silver will be twice as much as the gold in its composition.
The assayer can tell by the touchstone about how much
silver was originally present. Wrap the alloy .5 gram and
silver in a sheet of lead and cupel. If the alloy be above 950
fine, add say 0.005 grams of rolled copper, to toughen the
cornet. This addition should be made in the fine gold proof.
The button fi-om cupellation is flattened by the hammer on
an anvil. It is then heated to redness in a clay annealing cup
placed in the muffle, when it is removed. When cold, it is
passed between the rolls of a small flatting-mill. When rolled
sufficiently thin, the ribbon is again annealed and wound into
a comet or spiral round a small glass rod.
PARTING.
The comet is next subjected to the action of nitric acid in a
glass matrass of about three ounces capacity. Pure acid, abso-
lutely free from chlorine, is added at different intervals and
heat applied. Acids of two different degrees of strength are
employed.
The first has a specific gravity 1.16 (21° Baum^ ; the sec-
ond a specific gravity of 1.26 (32° Baume). First pour on
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THE CHEMISTS' MANUAL.
518
acid, 21** B. and heat for ten minutes ; replace this by acid
32° B. and boil ten minutes ; decant and make a second boil-
ing with acid of the same strength, 32** B. Finally, the comet
18 washed with distilled water, the flask is tilled completely
with water, a porcelain capsule is placed over the neck, and
the whole inverted. The comet falls gently through the
water into the capsule, the flask is removed, the water de-
canted and the cornet dried, and annealed in the muffle.
The weight of this comet gives the total amount of gold in
the sample assayed.
The gold, copper, and silver are reported in thousandths as
in the assay of silver bullion.
NATIVE METAL AND ALLOYS.
Eough metal in scales, etc., is lefl on the sieve during pul-
verization of ores. The assay of the above material consists,
ordinarily, of scorification, cupellation, and parting. The
quantity of test lead for scorification would vary in every case ;
but an appreciation of what has been said already concerning
scorification will enable the assay er to judge of the proper
quantity.*
FINENESS OF ALL GOLD AND SILVER COINED
IN THE UNITED STATES.
GOLD.
Datbof
Imitb.
$».
$10.
$5*
$8.
$S.60.
♦1.
PiNBWESS IN
TBOU8Ain>TH8.
17»2
_^
270
185
^_
67.5
_
916}
1834
—
258
129
-~
64,5
—
899-9-40
1837
—
258
129
-^
645
...
900
1849
616
258
129
64.5
26.8
900
1853
516
258
129
77.4
64.5
25.8
900
1878
516
258
129
77.4
64.5
25.8
900
^ See Author's Preface.
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514
THE CHEMISTS' MANUAL.
SILVER.
Date of
Issue.
Half-
Doll AB.
QUAB.
TKB.
DniB.
Half-
DniR.
Thkkk-
CBNT
PiBCE,
THOUSAXimB.
1792
1837
1851
1853
1873
416
412}
412}
412}
420 tt
208
206}
206}
192
192-9-10
104
1034
lOSj
96
t 962-5
416.10
41}
41
882-5
t 383-6
208-10
19-1-5
tl93-10
•12J
11.52
892-4-10
900
900
900
900
* The three-cent piece of 1861 was to be only 750 flue.
t Twelve and a half grams.
t Nearly.
ASSAY OF LEAD ORES.
The ore is first properly ground, when 10 grams of it are
taken for one assay ; this is mixed with 25 grams of black flux
or its substitute (10 grams of NajCOa *^ ^ grams of flour) on
a piece of glazed paper ; this is put into a Hessian crucible.
Three wire loops, after being sandpapered, are put in so that
they cross each other on top, and the charge is covered with
salt. It is then introduced into the fire and covered, where it
is left equal times to and from fusion. That is, if it takes
twenty-six minutes to fuse the charge, leave it in six minutes
longer ; then remove it from the fire, and set it aside to cool.
When perfectly cool, the crucible is broken, the button is ham-
mered on an anvil into a cube and weighed. The weight will
equal, when multiplied by 10 (^^^), the percentage of lead in
the ore. Tliree assays of each ore ought to be made, and the
average will equal the true percentage if the results of all
are about the same. The above method, I have found, gives
better results than any other yet known.
ASSAY OF TIN ORES.
Ten grams of the pulverized ore is mixed thoroughly on
glazed paper with 10 grams of cyanide of potassium (KCy).
This is introduced into a crucible (Hessian crucible) lined with
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THE CHEMISTS* MANUAL. 515
chalk and covered with salt. The crucible is then introduced
into a very hot fire and covered over. If it takes ten minutes
to fusion, leave the crucible in ten minutes longer ; then take
out and set one side to cool. When cold, crack crucible and
weigh button, its weight multiplied by 10 will equal the per-
centage of tin in the ore. Three assays of each ore ought to
be made, and the average will equal the true percentage, if
the results are about alike in each.
The crucible may be lined by a paste of chalk ; then dried.
ASSAY OF ANTIMONY.
Ten grams of the pulverized ore is mixed thoroughly on a
sheet of glazed paper with 30 grams of potassium cyanide
(KCy), and introduced into a (Hessian) crucible and covered
with salt. The crucible is then introduced into a very quick
fire, covered over and left in for eight minutes, when it is
taken out and put one side to cool. When cold, the crucible
is cracked and the button taken out and weighed. It is better
to do duplicate assays. The weight of the button multiplied
by 10 will equal the percentage.
PLATINUM.
The assay of platinum may be performed as follows :
Fusion with leadJ^ — Weigh and pulverize the sample as
finely as possible, and sift ; the metalh'c residue will contain
most of the metal sought for. Weigh the residue and sittings
separately.
1. SiFTiKGS. — Charge 20 grams in a small crucible with
Litharge 60 grams.
Borax glass 15
Soda 80 *•
Charcoal 1
* Taken from " Notes on Assaying." (Ricketts.)
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616 THE CHEMISTS' MANUAL.
Part of the soda should be mixed with the chai^, and part
used as cover. The proportion of fluxes may be varied to
suit the gangue, so as to render the slag as fusible as possible.
The litharge is reduced by the charcoal, and alloys with the
platinum and foreign metals, save osm-iridium, which will be
found principally under the lead-button. The lead-button ia
then broken out, scorified with a little borax glass, if too lai^,
and cupelled at as high a temperature as possible iu an ordi-
nary bone-ash cupel until it solidifies. The residue will be
platinum, with a little silver, gold, etc. It may be purified
by fusing in a crucible of cut lime, which is heated by coal-
gas^ the combustion being supported by a current of oxygen.
The lead retained in the unpurified button is about one-
eighth to one-quarter of its weight.
2. REsrouE. — ^Fuse directly in a scorifier with pure lead and
borax glass, cupelling the whole or a weighed portion of the
resulting button if it be too large, as in 1.
RsiCAiiKS. —In place of the method ased for the siftings, pure galena and
iron wire might be employed, as in the assay for lead ; other flaxes being
added to suit.
In the charge given for siftiugs, twenty to thirty grams of granulated
lead in addition to the litharge can be used with advantage. Instead of
cupelling the lead-button containing the platinum alone, add five or six
times the weight of the platinum in silver. This gives a result free from
lead. The sUver can afterwards be deducted in the calculation of the
platinum.
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|lie«ti^tr8 of §[m.
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ANALYSIS OF A MAN.
(Bt Pbof. Miller.)
A man 5 feet 8 inches high, weighing 154 pounds.
IbK.
Oxygen Ill
Hydrogen 14
Carbon
Nitrogen ,
Inoiganic elements in tbe aeh :
Phosphorus
Calcium
Sulphur
Chlorine
1 ounce = 4S7 grains.
Sodium
Iron.
Potassium
Magnesium
Silica
Total
21
3
1
2
0
0
0
0
0
0
_0
154
0
0
0
10
2
0
0
2
2
0
0
0
_0
0
gre.
0
0
0
0
88
0
219
47
116
100
290
12
The quantity of the substances found in a human body
weighing 154 lbs. :
lbs.
0£.
gTB
Water.
.... Ill ...
0 ..
.. 0
Gelatin
.... 15 ...
0 ..
.. 0
Albumen
4 ...
8 ..
0
Fibrine
4 ...
4 ..
.. 0
Fat
.... 12 ...
0 ..
0
Ashes
7 ...
9 ..
0
Total
.... 154 ...
0 ..
.. 0
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520 THE CHEMISTS* MANUAL.
THE BLOOD.
The blood is one of the principal fluids of the body which is
intended for its nutrition, and exists in two states :
_ ( Arteria] blood — bright-red or Bcarlet.
Blood \
( Vein blood — dark-red or purple.
Blood has a clammy feel, salt to the taste, slightly alkaline,
and has a specific gravity of about 1.055 ; is viscid, drying
rapidly.
When blood is allowed to coagulate, the fibrine entangles
the globules, and forms a clot and a fluid :
_ ( Plasma or Liquor Sanguinis.
Blood ] ^
i Serum. .
The plasma consists of:
j Fibrine.
( Blood -cells or corpuscles.
The serum :
C Albumen.
Serum ■< Water.
(Salts.
The fibrine only becomes solid on allowing the blood to
coagulate, as it is held in solution in the blood.
ANALYSIS OF BLOOD.
(By M. Gobbtjf Besanez.)
let spec 9d spec
Water .. 796.»8 783.63
Solidmatters ^^^1 216.37
Fibrine 1.95 1.56
Corpuscles 108.28 115.13
Albumen 70.75 62.7i
Extractive matter and salts.... 27.14 36.94
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^ V t;
IT
THE CHEMISTS* MANUA^i^.*^ ^ *• J^J;^
COMPARISON OF THE ARTERIAL AND VENOUS BLOOD.
(Bt mm. Poooiale and Mabchal.)
Mah.
Arterial Blood In
1000 parti!.
Water. 822,46
SoUd matter 177.54
Fibrine 6.17
Albumen 66.08
Fatty matter. 1.10
Globules ©7.46
Sodic chloride 8.15
Soluble salts 2.10
Calcic phosphate 0.79
Ferric oxide 0.63
0.11
Total 1000.00
Mah.
Venous Blood In
1000 parts.
818.80
181.59
6.08
61.87
1.20
106.05
8.29
2.19
0.76
0.58
0.09
1000.00
MEAN COMPOSITION
OF MALE AND FEMALE VENOUS
BLOOD.
(By BAcquEREL axd Rodier.)
Male.
Density of defibrinated blood 1060.00
Density of serum 1028.00
Water 779.00
Rbrine 2.20
Fatty matters 1.60
Serolin 0.02
Fhosphorized fat 0.49
Cholesterin 0.09
Saponified fat 1.00
Albumen 69.40
Blood-corpuscles 141.10
Extractire matters and salts 6.80
Sodic Chloride 8.10
Other soluble salts 2.50
Earthy phosphates 0.38
lion 0.57
Female.
1017.50
1027.40
791.10
2.20
1.62
0.02
0.46
0.09
1.04
70.50
127.20
7.40
8.90
2.90
0.85
0.54
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622 THE CHEMISTS' MANUAL.
COMPOSITION OF THE ASH OF HUMAN BLOOD.
(By ESndeblin.)
Triflodic phosphate 22.100
Sodic chloride 54. 769
Potassic chloride 4.416
Potaasic sulphate 2.461 .
Calcic phosphate 8.686
Magnesic phosphate 0.769
Ferroos oxide and ferrous phosphate 10.770 .
83.746 i ^^^^^^
( Sa]t&
i Salts.
98.921
BLOOD GLOBULES.
BLooD-GLOBrLES are often called Uood-corpusdea or blood-
disks. There are two kinds : red and white. The red glob-
ules are round, having a concave center, raised on the edge ;
their diameter varies between -^^ and ^^^ of an inch ; aver-
age, about g^*^ of an inch. There are from three to four hun-
dred times as many red globules as white (Harley.) Fifty
times as many (Todd and Bowman). The white globules are
much larger than the red globules, and they have a granular
surface. Their diameter is about -^^ of an inch.
DIAMETER OF RED GLOBULES.
(By Mr. Gulliver.)
In the Ape ^^ of an inch. In the Cat -^^ of an inch-
Horse T<W "
Ox TiiW"
Gbat ,nrW"
" Fox :nJ^«
" Wolf. ,Vinr"
" Elephant... Tn\nj "
« Red-deer. . . ^lAnF "
" Musk-deer. .-nrJvo "
The amoimt of blood in proportion to the entire weight of
a body is as 1 : 8. So that a man weighing 145 lbs. contains
on the average 18 lbs. of blood.
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THE CHEMISTS' MANUAL, 623
ANALYSIS OF BLOOD-CORPUSCLES AND OF LIQUOR
SANGUINIS OR PLASMA.
(By Lehman.)
Blood Ck>rpaBCle8. Llqnor SaDgninlB.
Water eSS.OO 902.90
Solid constituents. 312.00 97.10
Specific gravity 1 .0885 1.021
Httmatin 16.75 Fibrin. 4.05
Haemato crystallin 241.07 Albumen. 78.84
Cell membranes 41.16 —
Fat 2.81 1.72
Extractive matter 2.60 8.94
Mineral substances (exclasive of iron). 8.12 8.55
Chlorine 1 . 686 8. 644
Acid sulphuric 0.066 0.115
Add phosphoric 1.184 0.191
Potassium 8.828 0.323
Sodium 1.052 8.841
Oxy^n 0.667 0.408
Calcic phosphate 0.114 0.311
Magnesic phosphate 0.078 0.222
DETECTiON OF HUMAN BLOOD BY THE MICROSCOPE,
The crystals which form in blood under certain circum-
stances, and when treated by certain reagents, affords a means
of detecting human blood from other blood.
rma:
1 ••
' may form Hsematin crystals.
Blood -j " *' Hsematoidin crystals.
Hflemln **
'* ILehatik cbystals found in normal blood, particularly in the spleen,
may be obtained by agitating the blood with water or ether, so that the
blood corpuscles are ruptured and their contents crystaUized." (See draw-
ing below.)
" H^£MATOiDiN CRYBTAL8 are found in old clots." (See below.)
^'HiEMiN CBT8TAL8 may be made by mixing dried blood with equal
quantity of common salt, and boiling it with a few drops of glacial acetic
acid till the whole has dissolved. A drop of the mixture on the slide will
show the crystals on cooling."
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824 THE CHEMISTS' MANUAL.
12 8 4 5 6
Hffure 1 represents the crystals firom blood of a gainea-pig (trihedral).
" 8 " " " ** " "" squirrel (peno^onal).
** 8 " " " " *' "** rat and mouse (octahednl).
" 4 '* '• " " haman blood (hsmatin ciystals).
" 6 " " " " " " (h«matoidin crystals).
" 6 " " " " " " (hiemin crystals).
*^ 7 a represents red corpuaelea, and 6 represents while eorpusdet.
MUCUS.
Mucus is prepared in the follicles or glandnlsB with which
nearly all the mucous membranes are provided.
^^ Mucus is a clear colorless fluid which is poured out in
large or small quantity on the sur&ce of the mucous mem-
branes. It is distinguished from other secretions bj its vis-
cidity, which is its most marked physical property, and which
depends on the presence of a peculiar animal matter, known
under the name of mucosine. When mixed with other ani-
mal fluids, this viscidity is so great that the mucus has nearly
a semi-solid or gelatinous consistency."
Mucus is very smooth and slippery (slimy) to the tonch, and
this property enables it to protect the mucous membrane trom
injury, and facilitates the passage of foreign substances.
The following is an analysis of the pulmonary mucus, that
is, the fluid secreted by the follicles of the trachea and bron-
chial tubes :
(By Nabsbl)
Water 955.630
Solid constitnentB 44.480
Mudn, with a little albumen 23.754
Water extract 8.006
Alcohol extract 1.810
Fat 2.887
Sodic chloride 5.825
" Bulphate 0.400
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THE CHEMISTS' MANUAL. 525
Sodie carbonate 0.198
" phoephate 0.080
Potasaic phosphate, with trace of iron. . . 0.974
carbonate 0.291
Silica, and potassic sulphate 0.255
Mucus, when viewed under the microscope (200 diameters),
is seen to consist of granular oval corpuscles and epithelial
scales, and a watery fluid. This fluid, if examined under a
more powerful magnifier, is seen to consist of minute molecu-
lar particles, which have not been studied as yet. The aver-
age diameter of the mucous-corpuscles is about ^^^ of an inch ;
they vary considerably.
SEBACEOUS MATTER.
Sebaceous matter is produced in the hmnan subject in three
forms : first, by the sebaceous glands of the skin ; second, by
the ceruminous glands of the external auditory meatus ; and
third, by the meibomian glands of the eyelid.
Sebaceous matter is characteristic by containing a very large
proportion of fatty or oily ingredients.
COMPOSITION OF THE SEBACEOUS MATTER OFTHE SKIN.
(Bt Esbnbeck.)
Animal aabstances 858
Fatty matters 868
Calcic phosphate 200
" carbonate 21
Magnesic carbonate 16
Sodic chloride, acetate, etc 87
looo
PERSPIRATION.
Perspiration is a clear-colored watery liquid, with a dis-
tinctly acid reaction, and a specific gravity of 1.003 or 1.004.
Lavoisier and Seguin found that in 24 hours about 13.500 gr.,
or nearly two pounds avoirdupois of perspiration was given
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THE CHEMISTS' MANUAL.
out of a healthy person. It appears that the lungs exhale
during the same time over 8000 grains ; so that from the lungs
and skin combined the watery exhalations amount on the
average to rather more than three pounds per day. The
amount of perspiration discharged during violent exercise has
been known to rise as high as 5000 or 6000 grains per hour.
Southwood Smith found that the laborers employed in heated
gasworks lost by both cutaneous and pulmonary exhalation as
much as 3 J pounds weight in less than an hour.
COMPOSITION OF PERSPIRATION.*
Water 996.50
Sodic chloride 2.23
Potassic chloride 0.24
Sodic and potassic sulphate 0.01
Sodiam and potassium united to organic adds. ... 2.02
1000.00
TEARS.
This secretion is a clear, alkaline, watery fluid, containing
an organic substance similar to albimien, and saline matters
consisting for the most part of sodic chloride. The following
is its composition :
COMPOSITION OF TEARS.
{Taken from Robin, Le^on 9ur les Humeurs.)
Water 982.0
Albuminous matter 5.0
Sodic chloride 13.0
Other mineral salts .3
1000.3
MILK.
The fluid secreted by the mammary glands of women (as in
the case of all animals), near the end of utero-gestation during
• This analysis and the above remarks are taken from different parts of
an article on Perspiration, in Dalton's Physiology.
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THE CHEMISTS' MANUAL.
527
a period which vanes considerably and has not been accurately
determined, as also the fluid secreted for a few days after
delivery, is called colontrum,
Flint describes the colostrum secreted before delivery as a
thiekish, stringy fluid, which bears little resemblance to
perfectly-formed milk.
The colostrum after delivery the author has always found
to be a light yellowish, opaque, alkaline fluid, having, as Flint
says, " a mucilaginous consistence."
The following table contains an analysis of the colostrum of
a white and colored woman :
COLOSTRUX
WUITB WollATV
Average. (Tidy
".)
COLOSTRDU
Colored Woxan.
(MOTT.)
Water
84.077
15.923
100.000
■
85.01
SoUds.
14.09
100.00
Fat
6.781
8.228
6.513
0.385
15.023
4.31
Casein
Albumen
Milk-sumr
:::::!
8.22
.88
6.05
Mineral salt
0.53
14.99
From observations, microscopical and otherwise, the author
has come to the conclusion that on the eighth or tenth day after
delivery all the characters of the colostrum disappear, and the
secretion becomes normal, that is to say, healthy milk. In
some very rare cases, though, a few colostrum corpuscles and
masses of agglutinated milk-globules may be discovered after
the tenth day, but such cases are very rare.
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S28
THE CHEMISTS* MANUAL.
The following table contains analyses of pure healthy
woman's milk :
WAU Woman's
Milk.
Afferage, 89 Anal.
(Vehnois and
Becquerel).
T^Ue Womah*t
Milk.
Averags, ih Anal.
qTidt).
Colored Woman'*9
Milk.
Afferage.liAHaL
(ftoTT).
Water
88.908
11.093
87.806
12.193
86.34
Milk solids
13.66
100.000
100.000
100.00
Fat
2.666
3.924
4.364
0.138
4.021
3.528
4.265
0.285
4.03
Caseiii
3.S2
Milk-sugar
5.71
InnrfriiTiiP. nalts
0.60
11.092
12.193
13.66
Human milk is white, bluish-white, and more rarely
yellowish-white opaque fluid, having a slight odor, sweetish
taste, and possessing an alkaline reaction. Its specific gravity
varies between 1.02561 — 1.04648 (Vernois and Becqnerel).
Its average specific gravity, according to Simon, is 1.032.
The average specific gravity of colored woman's milk is
1.0223.
If a drop of milk be examined under the microscope,
myriads of beautifully formed globules of various sizes will
be seen suspended in a clear liquid. These globules are
known as milk-globules, are of a slight yellow color, dark
around the edges, and exhibit a pearly gloss. The diameter
of the human milk-globule is not larger than ^tjVtt ^^ *^
inch, and most of them are about YJjhru ^^ ^^ inch. The
colostrum-corpuscles spoken of above are somewhat larger;
their diameter varies between if-^ to -5^ of an inch ; th^e
corpuscles always make their appearance in the milk, when it
is in an unhealthy condition. It is to the envelopes which
surround the milk-globules that the opaque and white appear-
ance of milk is due. These envelopes are translucent, and
(but to no great extent) refract light.
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THE CHEMISTS' MANUAL. 529
When the milk is allowed to stand for some time, most of
the milk-globules, owing to their low specific gravity, rise to
the surface and form a thick, fatty, yellowish-white stratum, to
wliidi the name cream has been given. The fluid below the
layer of cream has necessarily become poorer in fat ; it has a
more bluish-white color, and its specific gravity is increased.
If this fluid be allowed to stand still longer, the casein which
it contains is precipitated, or curdled, that is to say rendered
insoluble ; at the same time the fluid becomes acid or sour.
The acidity is due to the luetic acid which has been formed ;
the lactose or milk-sugar merely having undergone a molecular
change. This natural coagulation of milk is due to the growth
and development of fungus plants ; the lactic acid is not neces-
sary for its progress ; the casein undergoes a change similar
to the change from soluble silica to insoluble silica.
SALIVA.
" Human saliva, as it is obtained directly from the buccal
cavity, is a colorless, slightly viscid and alkaline fluid, with a
specific gravity of 1.005. When first discharged it is frothy
and opaline, holding in suspension minute whitish flocculi.'^
— (Dalton's Human Physiology.)
COMPOSITION OF SALIVA.
(By Biddeb and Schmidt.)
Water 9©5.16
Organic matter 1.34
Potaseic sulphocyanide 0.06
Magneaic, Bodic and calcic phoapliate .08
Sodic and potassic chlorides .84
Mixture of epitlieliam 1.62
1000.00
The sediment that deposits from human saliva consists of
buccal and glandular epithelium, with granular matter and
oil-globules.
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530 THE CHEMISTS' MANUAL^
COMPOSITION OF HUMAN PAROTID SALIVA.
(By Pkop. Maukice Perkins.)
Water 983.808
Organic matter precipitated by alcohol 7.852
SubstanceB destructible by beat, but not predpitated by alcohol
or adds 4.810
Sodlc Bolphocyanide 0.830
Caldc phosphate 0.240
Potassic chloride 0.900
Sodic chloride and sodlc carbonate 3.060
1000.000
Saliva required for mastication of 19* ounces of bread = 4572 graina.
16* •' meat = 3360 "
Secreted in intervals of meals = 122S3 "
Total quantity in 24 hours = 90164 "
Or rather less than three pounds additional (Dalton).
GASTRIC JUICE.
The gastric juice should be drawn about fifteen minutes
after feeding, separated by filtration from accidental iinpimties.
Its specific gravity is 1.010. Becomes opalescent on boiling,
owing to the coagulation of its organic ingredients.
The following is the composition of gastric juice of the dog,
based on a comparison of various analyses by Lehmsnn,
Bidder and Schmidt, and other observers.— (Dalton's Physiol-
ogy, p. 126.)
* AUowance for a man in full health.
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THE CHEMISTS' MANUAL. 531
COMPOSITION OF GASTRIC JUICE.
Water 975.00
Organic matter 15.00
Lacticacid^ 4.78
Sodic chloride 1 . 70
Potassic chloride 1.08
Calcic chloride 0.20
Ammonic chloride 0.65
Calcic phosphate 1.48
Magnesic phosphate 0.06
Iron 0.05
1000.00
PANCREATIC JUICE
Pancreatic juice is a clear, colorless, somewhat viscid fluid,
having a specific gravity of 1.008 to 1.010, and a distinctly
alkaline reaction.
COMPOSITION OF PANCREATIC JUICE.
(By Bidder ai7D Schmidt.)
Water 900.76
Organic matter (pancreatine) 00.88
Sodic chloride 7.36
Soda, free 0.82
Sodic phosphate 0.45
" sulphate 0.10
Potassic sulphate 0.02
r Calcic oxide 0.54
Combinations of •< Magnesic oxide 0.05
( Ferrous oxide 0.02
looo.oo
* Lehmann finds lactic and hydrochloric acid ; more of the former than
of the latter. Bidder and Schmidt find, in place of lactic acid, in most of
their analyses hydrochloric. Fownee states that " hydrochloric, lactic,
butyric, propionic, and acetic acids are present," and gives the sp. gr. 1.002.
" It contains two albuminous substances, one insoluble in water and absolute
alcohol, the other soluble in water but precipitated by alcohol, tannin, mer-
curic chloride and lead salts. This is pepsin. In the ^stric juice of man it
exists to the amount of 0.310 per cent. When the gastric juice has the
greatest solvent power, 100 parts of fluid are saturated by 1.25 parts of
potash. The gastric juice dissolves the albuminous substances taken as
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532 THE CHEMISTS' MANUAL.
** The albuminous substance resembles ptyalin, together with
leucine, guanine, xanthine, and inosite. The pancreatic juice
has three distinct actions — firet, on starch ; secondly, on fat ;
and thirdly, on albuminous matter.
" Starch is converted into sugar more energetically by the
pancreatic fluid than by the saliva. Fat is changed into fatty
acids and glycerine at a temperature of 35° C. ; and boiled
albumen and fibrin are quickly dissolved at the same tempera-
ture, while the alkalescence distinctly remains."
INTESTINAL JUICE.
The intestinal juice is "colorless and glassy in appearance,
viscid and mucous in consistency, and has a distinct alkaline
reaction. It has the property, when pure, as well as when
mixed with other secretions, of rapidly converting starch into
sugar at the temperature of the living body." — (Dalton's
Physiology.) Frerichs found from 2.2 to 2.6 of solid constit-
uents in the intestinal juice, in which the parts soluble in water
amounted to 0.87^, the fat 0.195j^;, and the ash 0M%. Leh-
mann only found 2.156^ of solid constituents.
BILE.
The bile is very readily obtained from the gall-bladder. It
is a " somewhat viscid and glutinous fluid, varying in color
and specific gravity according to the species of animals from
which it is obtained. Human bile is of a dark golden-brown
color, ox bile of a greenish yellow, pig's bile of a nearly clear
yellow, and dog's bile of a deep brown. Specific gravity of
human bile, 1.018; that of ox bile, 1.024; that of pig's* bile,
1.030 to 1.036." The bile is distinctly alkaline, and miscible
in water in all proportions.
The following is an analysis of the bile of an ox, based on
the calculations of Berzelius, Frerichs, and Lehmann (Dal-
ton's Physiology, p. 162) :
food, and sliglitly changes their reaction. Thus, albumen, fibrin, casein,
legumin, glaten, and chondrin, give rise to as many different peptones.**
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13.43
15.24
THE CHEMISTS* MANUAL. 533
COMPOSITION OF OX BILE.
Water 880.00
Sodic glyk(M;holate ) 90 00
" tauro-cholate )
Biliverdin
Fats
Sodic and potaseic oleates, palmitate, and stearato .
Cholesterin
Sodic chloride
•* phosphate
Calcic phosphate
Magnesic phosphate
Sodic and potassic carbonate
Mucos of the gall-bladder 1.34
1000.00
COMPOSITION OF HUMAN BILE.
(By Gorup-Besaitet.)
Water 828—908
Solid matter 177— 92
Bile-acids with alkali 106— 56
Fat and cholesterin 47— 40
Mucos and coloring matter 24 — 15
Ash 11— 6
The bile is formed or prepared by the liver from venous
instead of arterial blood. The most important constituent in
the bile is sodic glyko-cholate and tauro-cholate, which sub-
stances were discovered in ox bile by Streeker, in 1848. Both
these salts are freely soluble in water, and if plumbic acetate
be added to the solution, plumbic glyko-cholate is precipitated,
which may be filtered oft*; then if plumbic subacetate be
added, a precipitate of plumbic tauro-cholate is produced, which
may also be filtered off. The above-named salts, sodic glyko-
cholate (NaCaeNOg) and sodic tauro-cholate (NaaCjaHjoNj
S2O , 5), only exist in ox bile ; the similar compounds in human
bile, when in a water solution, are precipitated by plumbic
acetate and plumbic subacetate, but, aller adding the first of
the above reagents, if to the filtrate plumbic subacetate be
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534 THE CHEMISTS' MANUAL.
added, no precipitate is produced. The entire biliary ingre-
dients of human bile are therefore precipitated by both or
either of the salts of lead.
" The principal coloring matter of the bile is called BiliruUn
or ChoUpyrrhin, When dry it is reddish-brown and uncrys-
tallizable, insoluble in water, more soluble in alcohol, which
it colors yellow, and most soluble in caustic alkali. On the
addition of nitric acid to the yellow alkaline solution, a change
ensues. The color passes through green, blue, violet, and red ;
after some time, the liquid again turns yellow, probably in
consequence of a gradual process of oxidation.
" Another coloring matter of bile is called Biliverdin, It
is dark-green, amorphous, without taste or smell, insoluble in
water, slightly soluble in alcohol, but soluble in ether."
PETTENKOFER'S TEST.
Add to the watery solution of the bile or of the biliary
substances, one drop of a solution of sugar in water (1 pt. of
sugar to 4 pts. of water) ; then add sulphuric acid, drop by
drop ; a white precipitate forms (which is abundant in case of
an ox, less in a dog), which dissolves in excess of acid. The
acid is added until the solution assumes a somewhat syrupy
consistency and an opalescent look, owing to the development
of minute bubbles of air. A red color begins to show itself
at the bottom of the mixture, and afterwards spreads until the
whole fluid is a clear, bright cherry red. This color gradually
changes to a lake, and finally to a deep, rich opaque purple.
Add now three or four volumes of water to the mixture ; a
copious precipitate forms, and falls down ; the color is destroyed.
The red color obtained cannot be relied upon as proof of
the presence of biliary matter, but if the put'pU cci^r is ob-
tained, the presence of biliary matter may be considered
proved.
If the biliary matter is present in only small quantities in
the solution to be tested, the red color will not show itself for
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THE CHEMISTS' MANUAL. 536
seven or eight minutes, nor the purple under twenty or
twenty-five minutes.
In delicate reactions '^ evaporate the suspected fluid to dry-
ness, extract the dry residue with absolute alcohol, precipitate
this solution with ether, and dissolve the ether precipitate in
water before applying the test. In this manner, all foreign
snbstances which might do harm will be eliminated, and the
test will succeed without difficulty.
Draper states that if the average results obtained by Bidder
and Schmidt from the cat and dog be applied to the human
subject, in an adult man weighing 140 pounds, the daily
quantity of the bile will be certainly not less than 16.94:0
grains, or very nearly 2^ pounds avoirdupois.
The bile is not an active agent in digestion ; it might be
supposed it was, as it pours into the intestines in the greatest
abundance immediately after a hearty meal ; this is because
the intestinal fluids are themselves present at that time in
greatest abundance, and therefore can act upon and decom-
pose the greatest quantity of bile.
CHYLE.
This is an opaque, milky, and feebly alkaline fluid, which
varies considerably.
"It is nothing more than the lymph which is constantly
absorbed by the lymphatic system everywhere, with the addi-
tion of more or less fatty ingredients taken up from the intes-
tines during the digestion of food."
ANALYSIS OF THE CHYLE OF AN ASS.
(By Dr. Rees.)
Water 902.87
Albumen 85.16
Fibrin 8.70
Spirit extract 8.82
Water extract 12.88
Pat 36.01
Saline matter 7.11
1000.00
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636 THE CHEMISTS' MANUAL.
ANALYSIS OF THE CHYLE OF A HORSE.
(FOWNBS* Chemibtry.)
Water C1.00 to 96.00 per cent
Fixed constituents 9.00 400
Nuclei and cells Variable.
Fibrin 0.19 0.7
Albumen 1.98 4.84
Fat 1.89 0.68
Extractive matter free from salts 7.27 8.84
Solublesalts 7.49 6.78
Insoluble about 2.00
The chyle approximates in composition and properties to
the blood.
LYMPH.
The lymph is an " opalescent or nearly transparent alkaline
fluid, usually of a light amber color and having a specific
gravity of 1.022. Its analysis shows a remarkable similarity in
constitution between it and the plasma of the blood."
ANALYSIS OF LYMPH.
(Bt Lassaigne.)
Water 9640
Fibrin 000.9
Albumen 28.2
Pat 0.4
Sodic chloride 6.0
Sodic carbonate ^
" phosphate V 1.2
" sulphate ;
Calcic phosphate 0.5
998.22
ANALYSIS OF THE LYMPH OF AN ASS.
(By Dr. Rees.)
Water 965.86
Albumen 12.00
Fibrin 1.20
Spirit^xtract 2.40
Water-extract 18.19
Fat Trace.
Saline matter 5.85
1000.00
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THE CHEMISTS' MANUAL. 537
The following table gives the quantity of fluids secreted and
reabsorbed during twenty-four hours, calculated for a man
weighing 140 pounds :
(Drafeb's Physiology, p. 325.)
Seliva 20.164 grains, or 2.880 pounds.
Gastric juice 98.000 " *' 14.000 "
Bile 16.940 " ** 2.420 "
Pancreatic juice 13.104 " " 1.872 "
Lymph 27.048 " " 8.864 "
25.086 pounds.
" A little over twenty-five pounds of the animal fluids tran-
sude through the internal membranes, and are restored to
the blood by reabsorption in the course of a single day. It is
by this process that the natural constitution of the parts,
though constantly changing, is still maintained in its normal
condition by the movement of the circulating fluids, and the
incessant renovation of their nutritious materials."
BONES.
" At the age of twenty-one years the weight of the skeleton
is to that of the whole body as 10.6 to 100 in man, and as
8.5 to 100 in woman, the weight of the body being about 125
or 130 pounds. Bones are construoted of organic matter
called Ossein^ which yields gelatin on boiling, and is made
stiff by insoluble earthy salts, of which calcic phosphate [Cag
(^04)2] ^9 ^h® most abundant. The proportion of earthy and
animal matter vary very much with the h'nd of bone and
with the age of the individual, as will be seen in the follow-
ing table, in which the corresponding bones of an adult and
of a still-bom child are compared.'' — (Fownes' Chemistry.)
Adult. Stiil-bobh.
BOHBS. iDorsanic Organic iDoif^nlc Oi^nic
Matter. Matter. Matter. Matter.
Femur 62.49 87.51 67.51 42.49
Humerus 63.02 86.98 58.08 41.92
Radius 60.51 89.49 56.90 44.10
Ostempofum 68.50 86.50 55.90 4410
Costa 57.49 42.61 63.75 46.26
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538 THE CHEMISTS' MANUAL.
" The bones of the adult are constantly richer in earthy salts
than those of the infant."
The following complete comparative analysis of human and
ox bones is due to Berzelius :
Bnman Bones. Ox Bases.
Animal matter soluble by boiling 32.17)
Vascular substance 1.18 J^
Calcic phosphate with a little calcic fluoride 53.04 57.35
Calcic carbonate 11.80 8.85
Magnesic phosphate 1.16 2.05
Soda and sodic chloride 1.20 8.45
100.00 100.00
The following is another analysis of bones by Berzelius :
Oiganic matter : Gelatin and blood-vessels 83.80
^Calcic phosphate 51.04
" carbonate 11.80
" fluoride 200
Magnesic phosphate ■ . . 1.16
LSoda and sodic chloride 1.20
Inorganic
and
Earthy matter.
100.00
Some chemists add to this about one per cent, of fat.
TEETH
Have a very similar composition, but contain less organic
matter ; their texture }b much more solid and compact. The
enamel does not contain more than 2 to 3.5 per cent, of ani-
mal matter, but contains about 81 to 88 per cent, of calcic
phosphate, with about 7 to 8 per cent, calcic carbonate and
more calcic fluoride than the bones contain.
ANALYSIS OF THE GRAY AND WHITE MATTER OF THE
BRAIN.
(By Labsaione.)
Gray. White.
Wate r 85. 9 73. 0
Albuminoas matter 7.5 9.9
Colorlessfat 1.0 13.9
Redfat 8.7 0.9
Osmazoroe and Lactates 1.4 1.0
Phosphates 1.9 1.3
106.0 lOOO
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THE CHEMISTS' MANUAL. 539
^^ It appears from this analysis that the cerebral substance
consists of albumen dissolved in water, combined with fatty
matters and salts. The fetty matter, according to Fremy,
consists of cerebrie acid, which is most abundant, cholesterin,
oleophosphoric acid, and olein, margarin,* and traces of their
acids. The same analyst states that the fat contained in the
brain is confined almost exclusively to the white substance,
and that its color becomes lost when the fatty matters are
removed. According to Vauquelin, the cord contains a larger
proportion of fat than the brain ; and according to L'Heritier,
tl)e nerves contain more albumen and more soft fat than the
brain." — (Gray's Anatomy, p. 60, 1870.)
PUS.
There is a number of different substances that are included
under the name of pus. The normal secretion is known as
tru€ or genuine pusy the other substances as spurious or false
pus. True pus is the natural secretion of a wounded or other-
wise injured surface. It is a creamy, white, or yellowish
opaque liquid, having a specific gravity of 1.030 or 1.033.
When viewed under the microscope, it is seen to consist of
minute granular corpuscles similar to those in mucus, and
serum surrounding them. The diameter of the corpuscles vary
considerably, but are about -^-^ of an inch in diameter. Pus
is neutral to test*paper, although in some rare cases it is either
acid or alkaline.
Blue pus sometimes forms on the bandages on which the
pus has been discharged. If this be treated with water and
agitated with chloroform, a blue crystalline coloring matter
(pyocyanin) may be obtained (Fordos).
* Margaiin is compoeed of pAlmitin and BtearixL
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540
THE CHEMISTS* MANUAL.
COMPOSITION OF PUS.
(By De. Wright.)
Pas ft-om a
Vomica.
Water 894.4 .
Fatty matter 17.5 )
Cholesterin 5.4 J'
Mucus 11.2 .
Albumen. 68.5 .
Sodic, potassic, and calcic lactates, car-
bonates, and phosphates 9.7
Iron A trace. .
Loss 3^ .
1000.0 .
Pas from a
Pbom
At>sce«8.
. 885.2 .
28.8 .
. 61 .
. 63.7 .
. 18.5 .
. 2^ .
. 1000.0 .
Pub from a
Abeoa«.
879.4
2G.5
88.6
&9
1.6
1000.0
URINE.
The urine is a clear, aml>er-colored, watery fluid, possesang
when wann an aromatic odor, whi^h disappears upon cooling.
The specific gravity of urine varies. Urina potus has a
specific gravity varying from 1.003 to 1.009 ; this urine is
light-yellow in color, and is passed after drinking much water.
Urina chyli has a specific gravity about 1.030; this is passed
after the digestion of a full meal. Urina sanguinis possesses
the average specific gravity 1.015-1.025 ; this is passed imme-
diately after a night's rest. The average density of the whole
urine passed by a man in 24 hours (which varies between 20
and 50 fluid-ounces) is usually from 1.015 to 1.020.
The urine is usually acid to test-paper, but the urine passed
shortly after eating is often neutral, or even alkaline, becom-
ing again gradually more and more acid up to the time the
next meal is taken (according to Dr. Bence Jones). The
acidity of urine Is due mostly to mono-sodic orthophosphate
(NaHaPO^). If the urine is to be examined chemically, it is
best to take a sample of all the urine passed in twenty-four
hours.*
The following analysis of urine is by Lehmann :
* See Scheme for the Analysis of Urine.
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THE CHEMISTS' MANUAL.
541
COMPOSITION OF THE URINE.
Water 037.682
Urea 81.450
Uric add 1 .031
Lactic acid 1.496
Water and alcohol extractives 10.680
Lactates 1.897
Sodic and amnionic chlorides 8.646
Alkaline phosphates 7.814
Sodic phosphate 8.765
Magnesic and calcic phosphate 1.133
Mucus 0.112
1000.195
62.318
BoUd matter.
HELLER'S ANALYSIS OF URINE.
PHYSICAL PROPERTIES.
Color.
Odor.
Reaction.
Litmus. Turmeric
Sp. Gr.
Urinometer.
Sediment.
NORMAL CONSTITUENTS.
Uroph^in.
Ur. gtt. 10 + H,SO* oz. BS.
Brown color.
Uroxanthin.
Ur. gtt. 30 + HCl oz. ss.
Amethyst color.
Urea.
Ur. gtt. + HNO, gtt.
Nit. Urea Crystals.
Uric Acid.
Ur. + iHCl + 24 hrs.
Ppt. U. Crystals
Chlorides.
Ur. + HNO3 + (AgN0a + 8Aq.)
Clumpy white ppt
Sulphates.
Ur. + (Sat. Sol. BaCl, + iHCV).
Ppt. within hour.
Earthy Pnoe.
Ur. + NH4(0H) in excess.
U ti If
Ale. Phos.
Ur. — Earthy Phos. ppt. by
NH4{0H) ; filt. and add (Sat.
Sol. MgS04 +HC1) made Alk.
by NH4(0H).
Precipitate.
ABNORMAL CONSTITUENTS.
Albumen.
Heat or HNOj.
Coagulates.
Bile.
Ur. spread on plate + HNOj gtt.
Prismatic rings.
BlAX>D CORFUHCLE&
By microscope.
Pus CORPUBCLEB.
<t 4«
Iodine.
Ur. + HNO;, + Starch.
Blue color.
Sugar.
Ur. + i Liquor Potass®.
Urerythren.
Boil and let cool.
Ur. + A + PbA.
Brown color.
Fawn ppt.
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542
THE CHEMISTS' MA1?UAL.
HUMAN EXCREMENT.
The following are the constituents of human excrement:
Excretm* (C^gHi 5^0,8).
Excretolic acid.
Peculiar red coloring matter.
Calcic palmitate and stearate.
Magnesic "
Butyric add.
Taurin.
Calcic phosphate.
Magneeic and ammonic phosphate.
Potassic phosphate.
Insoluble and undigested matters derived from the food.
SUBSTANCE ABSORBED AND DISCHARGED.
The following table gives approximately what is absorbed
and discharged during 24 hrs. by a healthy adult human subject.
ABSORBED DUBINO 24 HOUBS.t
DIBCHABOED DTTEOrO 24 HOUBL
Oxygen 1.470 lbs.
Water 4.535 "
Albuminous matter 805 "
Starch 660 "
Fat 220 "
Carbonic acid
.. 1.630 lbs.
Aqueous vapor
Perspiration
Water of the urine ...
Urea and salts
.. 1,155 -
.. 1.930 -
.. 2.080 "
.. .137 "
Salts 040 "
Feces
.. .358 *•
7.230 •'
7.280 ••
" Rather more than seven pounds, therefore, are absorbed
and discharged daily by the healthy adult human subject;
and for a man having the average weight of 140 pounds, a
quantity of material equal to the weight of the entire body
* Dr. Marcet estimates the average amount of excretin in each encua-
tion at about 2.8 grams. In the fieoes of an infant, cholesterin was foujid,
but no excretin. The f feces of a man with a diseased pancreas contained a
large proportion of sodic bistearate. — (Bowman's Med Chem., p. 168.)
Stercobike was found to be an ingredient of the human fjBces by Pk>^
A. Flint, Jr. (Am. Jour. Med. Science, Oct. 1862), and was obtained by liim
in proportions varjnng from .0007 to .008 of the .whole mass of the f«cea.
f Dalton's Human Physiology, p. 870.
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THE CHEMISTS' MANUAL. 543
thus passes through the system in the course of twenty
days."
ANALYSIS OF HUMAN SEMEN.
(By VAU<i0BLm.)
Water 90 parts.
Mucus : 6 "
Calcic phosphate 3
Sodic phosphate 1 '*
100 «
" To examine the semen* in a pure state, it must be taken
from the vasa efferentia of an animal recently dead, and whose
death has been produced from intention or accident, but not
from disease.
" The seminal fluid, or semen, which it is the function of
the testicles to secrete, is always, when evacuated, mixed with
the secretions of the vesicute seminales and prostate gland,
and mucus of the urethra ; floating in it are also to be found
a greater or less number of epithelial scales.
" The secretions, however, which enter into the composition
of the ejaculated fluid, have a relative proportion to each
other ; that of the vesicute seminales amounting to about
four-sevenths; that of the testicles and vasa deferentia to
about one-seventh; while the remaining portion consists of
the products of the prostate gland, mucus of the urethra, etc.
"Thef semen is a tliick, whitish fluid, having a peculiar
odor. It consists of a fluid portion called the liquor seminis,
and solid particles termed seminal granules and spermatozoa.
"The seminal granules are round corpuscles, measuring
^-j^th of an inch in diameter.
" The spermotozoa are the essential agents of impregnation,
or rather the elements which mix with the elements of the
egg or ovum, by which process fecundation is effected. They
* Dr. H. J. Jordan. Lecture on the Generative Organs.
t Sexual Physiology by R. T. Trail, p. 23.
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644: THE CHEMISTS' MANUAL.
are minute, elongated particles, with an oval extremity or
body, and a long, slender lilament. They move in an undu-
latory manner, and are supposed by many physiologists to be
animalctdes.
" The ovum is exceedingly minute, measuring from ^^i^th
to 120th of an inch in diameter, consisting externally of a
transparent envelope, the zona peUucida or vitelline mem-
brane, and internally of the yelk or vitellus^ a small vesicular
body ; imbedded in the substance of the yelk, is the germinal
vesicle, and this contains a minute substance called the (jer-
minal spot. The germinal vesicle is a fine, transparent
membrane, about y^th of an inch in thickness ; the germinal
spot is opaque, of a yellow color, and measures j^'^th to
5^>5^th of an inch.
" The ovisacs contain the ova, and are termed graafrein
vesicles. They vary in number from ten to twenty ; in size
they vary from that of a pin's head to that of a pea."
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i.«lh,.... S,,a,l«...
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CLASSIFICATION OF THE ELEMENTS.*
(By Mbndelejeff.)
The relations between the atomic weights of the elementary
bodies and their physical and chemical characters, have been
further developed by Mendelejeff in an elaborate paper (Ann.
Ch. Pharm. SuppL, viii, 133-229).
Mendelejeff points out that when the elements are arranged
according to the order of their atomic weights, from H = 1 to
U = 240, the relations between their properties and their
atomic weights exhibit the form of a periodic function. If, for
example, the fourteen elements whose atomic weights lie
between 7 and 36 be thus arranged :
Li = 7; G = 94; B = 11 ; C = 12; N = 14; O = 16; F = 19.
Na = 28; Mg = 24; Al = 27.8; Si = 28; P = 81; S=»2; Q = 85.5,
it is seen at once that the characters of these elements vary
gradually and regularly as their atomic weights increase, and
that this variation is periodical, ?. ^., varies in the two series in
the same manner, so that the corresponding members of these
series are analogous to one another; Na and LI; Mg and G;
Al and B ; Si and C ; S and 0, etc., forming similarly consti-
tuted compounds, or, in other words, possessing equal atom-
icity or combining capacity. Moreover, the combining capacity
of the elements in each series increases regularly with the
atomic weight, the first members forming monochlorides, the
second dichlprides, the third trichlorides, etc., or corresponding
oxides or oxychlorides.
* From Watt's Die. Chem., 2 SuppL
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548 THE CHEMISTS' MANUAL.
The physical characters of tlie elements and their correspond-
ing compounds likewise exhibit remarkable regularity when
thus arranged, as may be seen with regard to the specific
gravities and atomic volumes of the elements in the second
series above given :
Ka Mg Al 81 P 8 CI
Sp.gr 0.97 1.75 2.67 2.49 1.84 2.08 1.33
At. volume. 24 14 10 11 16 16 27
Na,0 MgO, Al.O, 810, P.O, 8.0, Cl.O,
Sp.gr 2.8 8.7 4.0 2.6 2.7 1.9 (?)
At. volume. 22 22 25 45 55 82 (?)
Most of the other elements may likewise be arranged in
groups of seven, the members of which eidiibit similar rela-
tions, €. gr. :
A«
Cd
In
8n
Sb
Te
I
At. weight..
108
112
118
118
122
125(?)
127
Sp.gr
10.5
8.6
7.4
7.2
6.7
6.2
4.9
Such a group of seven elements is called by Mendelejeff, a
sniull period or aeries.
The elements which can be thus seriated are contamed in
the first seven columns of the table on page 547, those in tlie
same colunm having equal combining capacity, and therefore
forming oxides of corresponding composition.
On comparing the several series in this table, it will be
observed that the corresponding members of an even, and of
the following uneven series (the fourth and fifth, for example)
difler from one another in character much more than the cor-
responding members of two even or two uneven series \e. y.,
the fourth and sixth, or the fifth and seventh) ; thus, calcium
resembles strontium much more than it resembles zinc. The
members of the even series are not so distinctly raetalloidal
as those of the uneven series ; and the last members of the
even series resemble in many respects (in their lower oxides,
etc.) the first members of _the nneven series. Thus, chromium
and manganese in their basic oxides are analogous to copper
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THE CHEMISTS' MANUAL.
549
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550 THE CHEMISTS' MANUAL.
and zinc. On the other hand, strongly marked differences
exist between the last members of the uneven series (haloids)
and the first members of the following even series (alkali-
metals). Now, between the last members of the even series
and the first members of the uneven series there occur, accord-
ing to the order of the atomic weights, all those elements
which cannot be included in the small periods. Thus, between
Cr and Mn on the one hand, and Cu and Zn on the other, there
come the elements Fe, Co, Ni, forming the foDowing transition
series :
Cr = 52; Mn = 65; Fe = 66 ; Co = 69; Ni = 69; Cu = 63; Zn = 65.
In like manner, after the sixth series follow the metals Ru, Rh,
Pd ; and after the tenth, O3, Ir, Pt. These two series of seven
terms each, together with the three intervening members, fonn
a long period of seventeen members.
As these intermediate members are not included in either
of the seven groups of short period, they form a group of
themselves (the eighth), some of the members of which, viz.,
Os and Ru, are capable of forming oxides of the form RO4 or
RjOe. Tliis group contains nine metals, viz. :
Fe = 66 ;
Ni = 69;
Co = 59.
Ru = 104;
Rh= 104;
Pd = 106.
Ob = 198;(?)
Ir = 195;(f)
Pt = 197.
These metals resemble one another in many respects:
(1.) They are all of gray color and diflScult of ftision ; the
fusibility increases from Fe to Co and Ni, just as in the follow-
ing series Ru, Rh, Pd, and Os, Ir, Pt (2.) They possess in a
high degree the power of condensing and giving passage to
gases, as seen especially in nickel, palladium, iron, and plati-
num. (3.) Their highest oxides are bases, or acids of little
energy, w^hich are easily reduced to lower oxides of more
decided basic character. (4.) They form stable double cyanides
with the alkali-metals. Fe, Ru, and Os form analogous com-
pounds K4RCy^; Co, Rh, Ir form salts having the general
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THE CHEMISTS* MANUAL.
561
formula KgRCy^ ; Ni, Pd, Pt form salts having the composition
K2RCy4. (5.) All these metals form stable metallammonium
salts, resembling one another in many of their characters.
Thus, rhodium and iridium ibrm salts analogous in composi-
tion to the roseocobaltic salts RX3.5NH3. (6.) Some of the
compounds of these metals, especially those of the higher
degrees of combination, are distinguished by characteristic
colors.
The metals Cu, Ag, Au are also, on account of analogous
behavior, included in the eighth group ; although, according
to the constitution of their lower oxides, they may also be
included in the first group
The arrangement of the elements in the order of their
atomic weights, and the composition of the short and long
periods, is more clearly seen in Table II, in which the periods
form vertical columns :
K =89
Rb = 86
08 = 188
Ca = 40
Sr = 87
Ba=137
—
—
?Yt = 88?
?D1 = 188?
Br = 178?
—
Tt =48?
Zr = 90
Ce = 140?
?La = 180?
Th = 981
V =51
Nb = 94
—
Ta= 18i
—
Cr=M
Mo = 90
—
W = 184
U =940
Mn=55
^
—
—
_
Fe = M
Bo =104
—
08 = 196?
—
TmcAL Blimbhtb.
Co = 60
Rh =104
—
Ir =197
—
Na =28
Ni = B9
Cu = 68
Pd =106
Ag =106
—
Pt = 198?
Aa=190?
^
H = l
Ll= 7
—
Q = 9.4
Mg =94
Zn = 65
Od =119
- j Hg= 900
—
B =11
Al =97JI
—
In = 118
- i Tl =904
—
C =1«
Si =98
—
So =118
—
Pb = 907
—
N =14
P =81
Ab = 75
Sb = la
—
Bi =906
_
0 =18
8 =83
8e =78
Te =196?
—
-
—
F =19
01 =8K.6
Br = 80
J =197
—
—
—
In the members of the even series (Table I), the metallic or
basic character predominates, whereas the corresponding mem-
bers of the uneven series rather exhibit acid properties. Thus
there is a decided difference between V, Nb, Ta, from the even
series of the fifth group, and P, As, Sb, Bi, from the uneven
series whose highest oxides have a similar constitution R2O5,
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653 THE CHEMISTS' MANUAL.
the former yielding less powerful acids than the latter. The
members of the even series do not, so far as is known, yield
volatile compounds with hydrogen or the alcohol-radicles, like
the corresponding members of the uneven series; thus all
attempts to prepare the compound Ti(C2H5)4 from TiC^ have
been unsuccessful, in spite of the great resemblance between
TiCl4, SiCl4, and SnCl4.
The position of the second series seems at first sight to be
inconsistent with the general division of the elements into
even and uneven series ; for most of the members of this series
possess acid properties, form compounds with hydrogen and
the alcohol-radicles, and some of them are gaseous — ^in all
which characters tliey rather resemble the elements of the
uneven series. It must, however, be observed, with regard to
this series : (1) That it does not include an eighth group, like
the other uneven series ; (2) That the atomic weights of the
elements included in it differ from those of the corresponding
elements of the following series by only 16, whereas in all the
other series this difference ranges from 24 to 28. The differ-
ence between the atomic weights of successive even series is
generally about 46, but in the elements of the second and
fourth series it is only 32-36.
Li G B C N 0 P Na Mg Al Si P 8 C
K Ca — Ti V Cr Mn Cu Zn — ~ Ab 8e Br
DiflE. 83 81 — 86 87 86 86 40 41 — — 44 46 45
These peculiarities explain the apparent anomalies above
mentioned, and, moreover, afford additional evidence of the
dependence of the properties of the elements on their atomic
weights. To make the elements of the second series analogous
in character to those of the fourth, their atomic weights should
indeed be smaller than they actually are. Similar anomalies
may also be observed in comparison of Na with Ca, and of Mg
with Zn, but they disappear in cases of P and As, S and Se,
CI and Br, where the diiOferences in the atomic weights conform
to the general rule.
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THE CHEMISTS' MANUAL. 653
In consequence of the peculiar properties of the elements of
the second series, Mendelejeff designates them as typical
eleinentSy to which category, also, belong hydrogen, and like-
wise sodium and magnesium, for the reason just stated. These
typical elements may indeed be regarded as analogous to the
lowest members of homologous series (HjO and CH4O, for
example), which, as is well known, do not exhibit all the prop-
erties of the higher homologues.
The preceding considerations likewise explain the isolated
position of hydrogen, the element possessing the lowest atomic
weight. According to the form of its salifiable oxide HgO, and
of the salts HX, it belongs to the first group ; its nearest
analogue is Na, which likewise belongs to an uneven series of
the first group. More remote analogues of hydrogen are Cu,
Ag, and Au.
Mendelejeff also develops several applications of the law of
periodicity, viz. : (1.) To the classification of the elements.
(2.) To the determination of the atomic weights of elements
whose properties are but little known. (3.) To the determinar
tion of the properties of hitherto unknown elements ; those,
namely, which might be expected to occupy the blank spaces
in the preceding tables. (4.) To the correction of the values
of atomic weights. (5.) To the completion of our knowledge
of the combination-forms of chemical compotmds.
For the details of these applications, we must refer to the
original paper.
KoTB.— Mendelejeff places the new element GalUiim between Alumi-
num and Indium, Group III (see Table I). GaUium was discovered by
M. Lecog Boisbaudran in 1875. Gallium forms an oxide Ga,0,. See p. 5.
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554
THE CHEMISTS' MAKUAL.
CHRONOLOGICAL TABLE
OF DEFUNCT ELEMENTS, WITH REFERENCE TO ORIGINAL
PAPERS.
(By H. Cabbhtoton Bolton, Ph.D.*)
NoTS.— Artlde« leferrlDg to the decease of the element are marked by an aaterisk.
Datb.
Element.
DiSCOYEBEB.
BXTBBEHCE.
ITH..
Edelerde
Bergmann...
Meyer
1780..
Hydrosldernm
Schriil, Geo. Nat. Pr. Berlin, 11, 884 ; 111, 880.
1784
Rstumnin
Mouuet
Joam. de Phye., xxvlll.
BeschWt, Ges. Nat. Fr. Berlin, viii, St. 4.
1788..
DiamaDtspatherde...
Elaproth ....
1790
AnfftrfiHa
Wedgwood..
Femandes...
Seherer's Allg. Journal, 1790.
Bcherer^s Allg. J.
1790..
Nameless earth
1800..
Agasterlde
Trommsdorff
J Scherer'B Allg. J., Iv. BIS.
1 ♦Qehlen's N. J., 1, 445, and v.
1801..
Pnenm^Ikali
Hahnemaim .
Scherer's Allg. J., v.
1801..
j Erythromlnm 1
I Panchrominm. )
DelRis
(Annalesdes Mines (l),lv.
-l •Ann. Chem. Phys. (2), llli, 8(8.
( 'Pogg. Ann., xxi, 49.
1806
Sllenlum
Proust
j Joum. de Phys., Iv, SOT and 457.
1 •Gilbert Ann., xlii, IST.
1805..
NicrolAPum r
Richtcr
WlDterl. . .
Gilbert Ann., zlz, 877.
1806..
JAndronla 1
iThellke f
J Gchlen's J^ iv. Gilbert Ann., xx, 480.
1 •Gehleu's J. (3), iii, 886.
1810..
Jnnonlam
Thompson ..
J Phil. Mag. (1), xxrvl, 278. GUbert Ann.,
1 xUi,116. Gilbert Ann., xliv, 118.
1816
Thorinm
Berzelios.. ..
Schwelgg. J., xxl, 16. •Pogg. Ann., iv, 146.
J Glib. Ann., lix, 96 and 887. •Trommsdn Jm
iii, 1,393. *Gi]b.Ann.,lxii,80.
1818..
Vertlmn orSlrium..
Von Vest...
1818.
Wodanimn
Glib. Ann., Ix, 99. •Gilb. Ann.,lxiv,838.
1890
Crodonlun* , - - r
Trommsdorff
Brngnatelli..
Osann
Glib. Ann., Ixv, 206. •Gilb. Ann., Ixvl, S90.
1831
Adtto
Gilb. Ann , Ixvii, 885.
1838..
Knthcninm
Pogg.. xlii, XiT.
1828..
Flnraniam.
Osaun
Pogg., xill, 891.
1828..
Pollninm
Osann
Pogg., xlv, 863.
• Am. Chem., July, 1870, p. 1.
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ized by Google
THE CHEMISTS' MANUAL. 555
Chronological Table of Depunct Elesients — (Continued).
Date.
1886.
1838
1848.
1M6.
1846.
1348.
16S0.
1861.
1854.
1857.
1860.
1861.
1803.
1863.
1864.
1864.
18S9.
1800.
TCt-wmkiit-
Donium. ..
Treeninin .
Terbiam . .
Norinin . . .
Polopium. .
Ilmeninm .
Aridlnm..
Donariam.
ThAUiam.
\ KameleBB metal of }
1 platinum group. )
( Nami-lefta earth in I
I zircons. f
DUOOYKBEB.
Salpharinm .
Diannm
j Nameless earth of {
\ caldom group, f
Wat>iam.
j Nameless metal of (
{ platinum groap. )
j NamelesH earth in )
( aircons. f
( Nameless earth in )
I limestones. s
Jargoniam
Nameless earth. .
Richardson..
Boase
Mosander . . .
Ivanberg....
H. Rose
nerrmann..
Ullgren
Beigcmann,.
Owen
Genth
Sjogren
Jones
Yon Eobell..
Dapr6
Bahr
Chandler
Nylander. . . .
BiBchoff
Sorby
Loew
SxnBSNOB>
j Ann. Chem. Pharm., six, 164.
1 *AmL Chem. Pharm., zxiii. 889.
J Thompson's Records General Science, iv, 90.
1 Chem. Centr., 1886, 616.
J Ann. Chem. Pharm. , xlvill , 290. •Ann. Chem.
1 Pliarm., cxzxi, l'^^, and cxzzvii, 1.
J Berzelian, Jahresb., zxr. 149.
( *Joam. pr. Chem., mi, 146 ; and xcvii, SSL
Pogg. Ann., Ixlx, 115. *Pogg. Ann., xc, 4B6.
j Jonm. pr. Chem., xxxrlil, 109 ; and xl, 497.
(*Pogg., Ann.,lxxiii,449.
^Jonm j;>r. Chem., lii, 443.
Ann. Chem. Pharm., Ixxvi, 989.
*Ann. Chem. Pharm., Ixxxviii, 961
j Ann. Chem. Pharm., Ixzx, 267.
1 *Ann. Chem. Pharm., Ixxxiv, 987.
j Am. J. Sci. (9). xiii, «K>.
1 'Am. J. Sci. (9), xvi, 96 ; xvll, 180.
Am. J. Sci. (9), XT, 946.
j Joum. pr. Chem., Iv. 906.
1 *Joam. pr. Chem., Irii, 146.
j Mining Joum., July 14, 1867.
1*Chem. News, ▼U,9(».
Ann. Chem. Pharm., cxxzri, 909.
j PhU. Mag. (4), xxi, 86.
1 Chem. News, iU, 199.
j Poge. Ann., cxix, OT9. *Jomrn. pr. Chem.,
) xci, 316. *Compte*s Rendns, Jm
Am. J. Sci. (9), xzziii, 861.
Acta Universit. Londensis, 1861
Pogg. Ann., cxxii, 646.
I Chem. News (Am. Repr.\ iv, 281.
I *Chem. News (Am. Repr.). Apr., 18T0.
Annals N. Y. Lye. Nat. Hist, ix, 911.
Digiti
ized by Google
i i
556
THE CHEMISTS' MANUAL.
PRICE OF METALS.*
{Arranged hy H. C. Boltok, PH.D.)f
Mjstai.
State.
Valus nr
Gold per
IS. AYom.
Puce or
Gold pes
GaAX.
AmVOXITT.
Vanadium
Cryst. fused
Wire
$4792.40
8261.60
2446.20
2446.20
2446.20
2228.76
2985.44
1671.57
1680.06
1576.44
1522.06
1804.64
1250.28
1082.84
924.12
788.39
652.32
498.80
466.59
434.88
299.72
289.80
196.20
196.20
122.31
108.72
54.84
4530
22.65
18.60
16.80
12.68
8.80
8.26
8.26
1.95
1.00
.86
J85
.22
.15
.10
.06
.014
$10.80
7.20
5.40
5.40
5.40
4.92
6.48
8.96
3.60
348
8.86
2.88
2.76
2.28
2.04
1.63
1.44
1.10
1.08
.96
.52
.43
.43
.27
.12
.10
.06
.086
.028
.008
.007
.007
.0043
Prices t
recent (
8.
Bubidium
8.
Calcium
Tantalum
Electpolvtic
Pure...'.
Fused globules .
Globules
Wire
S.
S.
Cerium
a
Lithium
s.
Lithium
8.
Erbium
Fused
B.
Didvmium
<«
a
Strontium
Electrolytic
Pure
a
lT>di"n», .... T - - r - - - ^
T.
Ruthenium
CnliimhiiiTTi
Fn«u»d
T.
8.
Rhodium
1 1 1 1 1 ill
T.
Barium*
a
Thallium
T.
Osmium
T.
Palladium
T.
Iridium
T.
Uranium
Gold
T.
Titanium
^^
Tellurium
M
Chromium
«(
Platinum
(«
Manganese
«
T.
Molybdenum
Magnesium
Wire and tape. .
Globules
Bar
T.
T.
Potassium
T.
Silver.
Aluminium r . . » ....
a
Cobalt
Cubes
a
Nickel
T.
Cadmium
Cruda
T.
Sodium
T.
Bismuth. ... ....
a
Mercury
Antimonv
T.
Tin '.
CoDDer
Arsenic
akenfrom
Zinc
luotatioxi&
I>ad
Iron
* S. and T. annexed to the price per gram stands for Schuchaidt and
Trommsdorff, respectively, and indicates the source of the data,
f Am. Chem., June, 1875.
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ized by Google
TABLE !.♦
COMFOBmON OF THB ABH OF AgRICULTUBAL PLAZTTO AND PRODUCTS
giTing the Average of all trufitworthy Analyses pabliahed up to August,
1865, by Professor Emil Wolff, of the Royal Academy of Agriculture,
at Hohenheim, Wirtembeig.f
SxmnAMcm,
P
s
L— MEADOW HAY AND GRASSES.
1 Meadow hay
SYoDnggnsa
8 Dead ripe hay
4 Rve gnw in (lower
5 Timothy
6 Other sweet gRweee
7 Oats, headiiif? oat
8 " In flower
9 Barley, heading out
10 ** in flower
11 , Winter wheat, headinff out .
13 " " in flower....
13| Winter rye. headins: oat. . . .
14 Green cereals, light
** *" heavy
Han^rian millet, green ....
fferm.).
18
7.TO
25.6
7.0
4.9
11.6
6.2
6.1
29.6
1
9.aJ
56.2
1.8
2.8
10.7
10.5
4.0
10.8
1
7.73
7.6
2.9
8.4
12.9
4.4
0.7
68.1
4
7.10
24.9
4.2
2.1
7.6
7.8
8.8
39.6
8
7.01
29.8
2.7
8.7
9.4
10.8
8.9
86.6
39
7.27
83.0
1.8
2.6
6.5
7.8
4.4
876
6 , 9.46
41.7
4.4
8.6
7.0
8.8
8.4
27.9
7 . 7.28
88.0
8.8
8.2
6.7
8.8
2.7
88.2
6 ■ 8.98
88.5
1.7
2.9
7.0
10.1
2.9
81.2
6 i 7.04
26.2
0.6
8.1
6.0
9.8
2.9
48.0
8 , 9.73
84.7
1.9
1.6
4.9
7.4
2.8
41.9
8
6.90
25.7
0.5
2.2
8.1
7.3
1.9
66.8
1
6.42
88.6
0.8
8.1
7.4
14.7
1.6
82.0
5
7.20
20.6
1.6
8.9
6.6
9.1
4.1
41.4
6
9.21
85.6
&4
4.7
8.8
8.1
4.8
80.0
S
7.28
87.4
ao
10.8
6.4
8.6
29.1
8.0
S.0
6.7
6.4
6.0
4.1
4.4
4.0
6.6
8J5
6.8
2.8
4.'8
6.6
6.4
n.— CLOVER AND FODDER PLANTS.
17[BeddoTer
a. 16-26 per cent potash
A. 25-86 '*
c. 86-60 " **
18 White clover.
19 Locem
iO Esparsctte
21 Swedish clover
S2 AfUhyUis vvineraria.. . .
88 Green vetches
84 Green pea, in flower. . . .
25 Green rape, yonng
66
6.T8
84.6
1.6
12.2! 84 0
9.9
8.0
2.7
16
6.011 20.8
^1.9 18.2i 89.7
9.4
8.8
1.2
23
6.74< 298
*1.6 11.8' 86.6
10.6
8.0
2.7
18
7.19 4ti.8
1.4 7.8 27.8
9.2
2.2
2.5
2
7.16
17.6
7.8 10.0 82.2
14.1
8.8
4.5
7
7.14
25.8
1.1 68 48.0
8.5
6.1
2.r)
2
6.89
89.4
1.7 6.8 82.2
10.4
8.8
4.0
2
6.63 838
1.5 16.8 81.9. 10.1
4.0
12
1
6.60
10.8
4.5
4.6 68.9 7.0
1.6
2.9
8
8.74
42.1
2.9
6.8 26.3! 12.8
8.7
1.8
1
7.40
40.8
0.2
8.2 28.71 18.2
8.5
2.6
5
8.97
82.8
8.8
4.61 28.1
8.7
16.8
8.2
8.7
6.4
2.9
8.2
8.8
1.9
8.0
8.8
0.8
8.1
1.8
7.6
• The following eleven tablcn have been taken fW>m "How Crops Grow,*' by Johnpon.
t From Professor WolflTs Mlttlere Zusammensetzung der Attcne^ aUer land- ynd font-
wirthKhc^fUichen wichiigen Stofe, Stuttgart. 1865. The above table, being more complete,
and in most pnrttcnlars more exact, than the anthorV meanf* of reference enable him to
construct, and being moreover likely to be the ba»iR of calcalations by agricaltarol chem-
ists abroad for some years to come, has been reproduced here literally. The references
and important explanations accompanying the original, want of space precludes quoting.
In the table, oxide of iron, an ingredient normally present to the extent of less tnan one
per cent., is omitted. Chlorine is often omitted, not because absent from the plant, bat
fK>m uncertainty as to its amount. Carbonic acid is also excluded in all cases for the sake
of aniformity and flicility of comparison.
Digiti
ized by Google
558
THE CHEMISTS' MANUAL.
Composition of the Ash of Agricultitral Plain's Aia> Products.
SUBSTAITCB.
ft •
I <
I
in.— ROOT CROPS.
96|Potatoefl....
97 Artichokes. ,
88*Beete
S9 Sngar-beeto,
80" •
81
89
88
84
86
Tnrnlpt). .
Turnips*
Rnta-bagas
Carrots
Chiccory
Sugar beet-heads t .
81
8.74
80.8
1.6
4.5
2.8
19.1
6.6| 2^1
1
&.16
65.4
2.71 8.5
16.0
8J8! ...
15
6.86
58.1
14.8
5.1 4.6
9.6
8.3 8.S
44
4.35
49.4
9.6
8.9
6.8
14.8
47| 8.5
15
8.28
89.3
11.4
8.9
10.4
18.8
14.3 2.4
2
7.20
50.6
3.8
2.1
13.4
174
6.0 1.1
2
7.68
61.2
6.7
2.0
9.7
15.8
8.4 0.5
10
6.27
86.7
22.1
5.8
10.7
12.5
6.4I 20
7
5.21
40.4
7.7
6.8
8.7
14.5
9.2; 6.1
1
4.08
29.0
24.4
11.0
9.1
12.6
7.61 2.01
9J
14
6u6
10
4.1
6.4
5.1
8J
17
0.5
IV.— LEAVES AND STEMS OF ROOT CROPS.
86 Potatoes, Angnst .
87 ** October.
88 Beets
Sugar-beets
Turnips
Kohl-rabi ,
Carrots
Chiccory
Cabbage ,
Cabbage-stalk
8
8.92
14.5
2.7
16.8
39.0
6.1
5.6
1 1 5.12
6.3
OS, 22.6
46.2
6.5
6.5
6 115.96
29.1
21.0 9.7
11.4
6.1
7.4
7 i 17.49
22.1
16.8| 18.3
19.7
7.4
8.0
16 13.68
22.9
7.8, 4.5
32.4
8.9
9.9
1 16.87
14.4
8.9
4.0
83.3
10.4
11.7
7
13.57
14.1
23.1
4.6
33.0
4.7
7.9
1
12.46
60.0
0.7
a2
14.3
9.0
9.0
2
10.81
48.6
3.9
88
15.3
15.8
8.5
1
6.46
4a9
6.5
4.1
11.3
20.9
11.8
8.0i 4.6
4J»' 10
4.8 11.8
11; 17
3.8l II
10.5 19
5.6 7.1
1.0 1.7
1.2 15
1.1, U
v.— REFUSE AND MANUFACTURED PRODUCTS.
Sugar-beet cake
a. Common cake
Residue of maceration
e. Residue from centrifugal ma-
chine
Beet molasses
Molasses slumps
64
4B Raw beet sugar.
Potato slump^.
Potato fibers
Potato juice I . . . .
Potato skins 5
Fine wheat flour.
65 Rye flour.
66-^ • -
67
68
89
60
61
82
63
64
65
66
67
68
Barley flour
Bailey dust**...
Maize meal
Millet meal
Buckwheat grits.
Wheat bran
Rye bran
Brewer's grains
Malt
Malt sprouts.
Wine grounds .
Orape skins. .
Beer.
8.15
8.03
8.53
8.11
11.28
19.02
1.43
11.10
0.99
23.45;
969
0.47
1.97
2.33
5.62
1.35
0.72
6.43
8.22
5.17
2.78
6.«i
4.60
4.04 i
86.6
8.4
25.0
12.7
86.8
9.4
45.6
9.8
711
10.5
80
8
83.3
28.0
46.3
6.6
15.6
60.5
72.0
07
36.0
09
38.4
1.8
28.8
2.6
18.9
1.4
28.8
a6
19.7
2.8
25.4
5.9
W.O
0.6
27.0
1.8
4.2
0.8
17.3
34.9
58.4
0.5
49.4
2.2
37.5
7.8
5.6
I'l'S
0.4
0
as
7.6
8.5
a7
8.2
8.0
13.5
7.7
14.9
25.8
12.9
16.8
15.8
10.1
8.4
1.4
8.2
6.1
4.91
26.81 1021 8.9i 6.S
27.2| 12.91 18
27.3 6.0 2.3
13.0 6.5
25.8
6.0 0.5
9 0.1
8.5
6.2! 20.0
47.8 23.91
1.0 16.8
9.61 8.4
2.8, 52.0
1.0 48.8
2.8l 47 8
2.5 28.9
6.8
2.8
4.7
3.5
11.6
8.8
1.5
15.5
13.0
45.0
47.8
48.1
61.8
47.9
88.0
86.5
21.0
15.5
.-._ 20.8
2.2I 82.7
0.7
2.1
1.7
22.9! a9
7.8| 14
... 11
8.6 0.1
0.4 17
8.1
90.0
11
4.8
110
OS
10.1
16
18
11
1.8
7.4
11
U
OS 812
...I 812,
6.31 20.5
7.8' ....
4.4 15' OJ
...i 10.2;
0.5
♦ While turnips in the original, but apparently no special kind.
t Probably the crowns of the roots, removed in sugar-making.
iThe residue after fermenting and distUling oflT the spirit.
Reftise of starch manuflicture.
Undiluted.
^ Prom boiled potatoes.
** Reftise lu making barley grits.
Digiti
ized by Google
THE CHEMISTS' MANUAL.
559
CoMFOsmoN OF THs AsH OF Agbicultubal Plaivts ahd Pboducts.
SxmnAMcm.
u
il
v.— REFUSE AND MANUFACTURED PRODUCTS.
09;Orapemiut...
TOftepe cake.. .
~ LiDseedcake..
Poppy cake.
Waloat cake
Cotton-eeed cake. .
68.8
0.9
6.6
4.9
17.7
6.5
1.8
6.60
S48
0.1
11.6
10.9
86.9
8.8
M
0.94
23.8
1.4
16.9
8.6
86.2
8.4
6.6
10.60
ao.8
4.6
4.8
88.1
87.8
2.0
4.8
6.86
88.1
1».«
6.7
48.8
1.2
1.6
6.tt6
86.4
4.8
4.6
48.8
1.1
4.0
0.6
OJI
0.6
0.9
VL— STRAW.
TSi Winter wheat.,
78 WlDter rye. . .
77 Winter ppelt...
78 Summer rye...
79 Barley
80OaU
81 Maize
88 Peas
83 Field bean
84 Garden bean..
86 Buckwheat . . . .
86 Rape
87.Poppy
12
4.96' 11.6
2.9
2.6
6Ji
6.4
2.9
668
4.81 18.7
8.8
ai
7.7
4.7,
1.9
68.1
5.56, 11.2
0.4
0.9
4.8
6.8|
1.8
71.4
5.65, 28.4
, .
2.8
8.9
6.5
2.6
559
17
5.10 21.6
4.5
2.4
7.6
4.8|
8.7
68.8
5.12 22.0
5.8
4.0
8.2
4.2
8.5
4a7
5.49 85.8
1.2
5.5
10.5
&]
5.2
88.0
21
5.74 21.8
5.8
7.7 87.9
7.8
5.6
5.7
4
7.12, 444
8.8
7.8 28.1
7.0
0.2
5.4
6
6.06' 87.1
6.0
5.2 27.4
7.8
8.6
4.7
6
6.15 46.6
2.2
8.6| 18.4
11.9'
5.8
5.5
12
4.58 25.6
10.8
5.7; 26.5
7.0,
7.1
6.7
1
7.86i 88.0
1.3
6.5
80Ji
8.51
5.1
11.4
6.1
18.8
6Jl
7.7
12.4
2.6
881 Wheat
808pelt
90' Barley
Ol.Oate
92;MaijEe cobs . . . .
OslFtaa-eeed holla .
VII.— CHAFF, Etc.
10.78
9.1
1.8 1.8
1.9
4.8' ...1 81.8
9.60
9.6
0.8 2.6
8.4
7.8 8.81 74Ji
14.28
7.7
0 9 1.8
10.4
2.0 8.0. 70.8
9.22
18.1
4.8 2.6
8.9
0.8 2.5! 69.9
0.56
47.1
1.2, 4.1
8.4
4.4| 1.91 26.4
6.6S
31.1
4.8> 2.8
29.6
2.81 4.81 17.2
6.1
Vm.— TEXTILE PLANTS, Etc.
94|FIax fitraw. 8
95 1 Rotted flax stems 8
98Flaxllber 8
97 Entire flax plant 2
98 Entire hemp plant ' 2
99 Entire hop plant I 1
100 HoM I 12
101 Tobacco I 7
8.71
86.9
6.1
7.1
28.8 11.6
5.8
6.C
2.40
9.0
4.8
6.4
51.4 5.9
8.1
13.8
0.67
3.3
8.2
5.4
68.6 10.8
2.7
6.2
4.30
34.2
4.8
9.0
15.5; 28.0
4.9
2.6
4.60
18.8
8.21 9.6
48.4 11.6
2.8
7.6
9.87
26.2
8.8 5.8, 16.01 12.1
5.4
21.5
6.80
37.8
8.2 5.5, 16.91 15.1
2.6
15.4
24.06
27.4
a7
10.5
87.01 8.6
8.9
9.6
4.0
0.4
5.9
8.5
4.0
8.4
IX.— LITTER.
lOSIHeath
108: Broom (Spartium)
104 Fern (^«pkWMm)
105 Hconrin^r mf»h {Equisetum)
106 Sea-weed {Fucus)
107'Beech leaves in aatnmn
106 Oak '• " "
109 Fl r ** ( FinvJt tylveHrU) . . .
110> Rod pine leaves (Hnw ploea) . . .
11 l\Tleed (Arundn phrcKj )
112 Down f2^«i> (Psamma arearia)..
118 Sedge ( Ciirer)
114 Rn»n (Junau)
115iBiilnuh (iSScif^iM) I 8
8
4.61
2
3.25
5
7.01
2
•23.77
8
14.39
6
6.75
4.90
1.40
5.82
4.69
il
8.08
5.30
8.66
13.2' 6.3'
36.5 8.5
42.8 4.5
13.2| 0.5
14.5 24.01
5.2 0.61
3.5 0.6
10.1 ....I
1.5 ....'
8.6 02|
2«.8 4.0
33.2 7.8
36.6, 66i
9.7l 10.3:
8.41 18.
124 17.
7.7, 14.
2.8, 12.
9.5 13.
6.0 44.
4.0 48.
9.9 41.
2.3 15.
1.2i 5.
8.8 16.
4.2 5
6.4> 9.
8.0i 7.
.8
6.1
4.4 86.8
.1
a6
8.5 10.3
0
9.7
5.1 . 6.1
.51
8.0
6.8, 68.8
9!
8.1
24.01 1.7
.91
4.2
8.7 88.9
.6
ai
4.4 80.9
.4>
16.4
4.4 18.1
.2
8.2
2.8, 70.1
.9
2.0
2.8- 71.5
.5,
7.2
8.6 18.5
.3'
6.7
8.8 81.5
.5:
6.4
8.7i 10.9
.81
6.5
5.61 48.8
2.1
2.7
10.8
5.7
10.1
0.4
4.4
6.6
14.8
Digiti
ized by Google
660
THE CHEMISTS' MANUAL.
CoMFOsmoK OF THE AsH OF Agbicultubal Plaitts Ain> Products
SUB8TANCS.
I O
|W
X.— GRAINS AND SEEDS OF AGRICULTURAL PLANTS.
116 Wheat
117 Rye
llSBarley
1190Bt«
190 Spelt with bask
ISlMalse
133 Rice witbhufiik
1«8 " huftked
IM Millet with bask
183 " hnakod
liMSora-hani
l«7Bnckwheat
188 Rape seed
189Flax '"
180; Hemp "
131Poppy "
13«Madia "
188'Mn»tard"
134Beet "
135Tuniip ♦*
135Carrot " .
137 Peas
188Vetche8
139 Field beans
110 Garden beans
141 Lentils
142 LnpineH
143 dorer eeed
144' Espanette seed
78
9.07
81.1
8.5
19.2
8.1
14
8.08
80.9
1.8
109
9.7
84
9.66
91.9
9.8
8.8
96
90
8.07
15.9
&8
7.8
8.8
8
4L90
17.8
1.8
5.8
2.6
8
1.49
87.0
1.5
14.6
9.7
7.84
18.4
4.5
8.6
6.1
0.80
98.8
4.8
18.4
2.9
4.49
11.9
1.0
K.4
1.0
1.49
18.9
5.8
1&6
1.86
10.8
8.8
14.8
1.8
1.07
S8.1
6.9
18.4
8.8
15
4.94
98.5
1.1
18.2
18.8
8.65
89.9
1.8
18.8
8.4
6.48
90.1
0.8
6.6
98.5
6.18
18.0
1.0
9.6
85.4
. ...
9.6
11.9
15.4
7.7
4.80
15.9
5.8
10.8
18.8
6.66
18.7
17.8
18.9
15.6
8.96
91.9
1.8
8.7
17.4
8.60
19.1
4.8
6.7
8R.8
80
9.81
40.4
8.7
8.0
4.8
9.40
8C.6
10.6
8.5
4.8
8.46
40.6
IJK
6.7
6Jt
8.06
44.1
9.9
7.5
7.7
9.06
87.8
9.9
9.0
5.1
83.5
17.8
6.8
7.8
4.11
87.3
0.6
18l2
6.8
4.47
98.6
2.8
6.6
81.6
46.9
2.4
1.71
.....
47.5
2.8
1.5
88.8
9.3
97.8
907
1.6
46.4
.....
20.O
8.6
44.C
44.7
1.1
8.1
47.8
0.6
06
61.0
0,6
8.0
98.4
OJt
S9.I
68.6
lA
60.9
7.5
48.0
2.1
1.7
48.9
8.6
1.1
OJ
40.4
1.1
1.1
e.i
86.3
09
11.8
OJ
81.4
1.9
8.8
4.4
650
89.0
4.7
8.4
a4
16.6
4.9
8.1
9.4
40.9
7.1
0.7
15.8
5.6
&«
18
86.8
&6
09
U
88.1
4.1
8.0
1.1
89.9
6.1
IJ
19
80.4
8.8
0.8
0.9
99.1
1.1
as
85.5
as
a9
L8
88.6
4.7
2.4
u
98.9
S.9
asl
u
XL— FRUITS AND SEEDS OP TREES, Etc.
145 Grape seeds
146 Alder
147 White pino. ..
l48Redpiue
149 Beech nats
160 Acorns
151 Horse-chestnut
158 ^' ffreen hask. .
158 Apple, entire (hiit
154 Pear, '' '" ...
156 Cherry, " "
156 Plum, " "
9.81
6.14
.
8.80
9.36
4.88
28.6
87.6
91.8
98.4
82.8
64.5
68.9
76.4
86.7
54.7
61.9
60.9
ao
88.9
24.0 2.51
16
8.0
80.7
18.0 3.4I
7.1
16.8
lA
89.7 :
1.8
15.1
1.9
46.0'....
10.0
11.6
94.5
90.8t 9.9'
0.7
5.4
7.0
16.81 9.8
0.5
11.6
99.4! 1.4
....
1.0
10.0
68 1.4
96.1
8.8
4.1
13.6 6.1 >
8.5
5.9
8.0
15.3 6.71
9.8
6.5
7.6, 16.0, 5.11
OJi
5.6
10.0
16.11 831
1.1
8.8
11.7
10.4
1.9
1.1
0.8
0.6
4.3
1.5
9.0
9l4
0.1
06
17
6.4
6J
U
XII.— LEAVES OF TREES.
157 Mulbenr
156 Horse-cnestnnt, spring...
159 ** autumn .
160 Walnut, sprlnsf
161 ** autumn
16:2 Beech, summer
163 " autumn
l'>i Oak, summer
165| •' autumn
166, Fir, autumn
1671 Red pine, autumn
8.58
19.6
6.4
96.7
7.17
88.8
8.9
91.8
7.58
19.6
7.8
406
7.72
49.7
4.6
26.9
7.01
86.6
..
9.6
68.7
4.83
18.5
1.8
8.6; 86.5
6.75
6.8
0.6 6.01 44.9
4.60
88.1
18.5! 96.1
4.90
8.51 0.6
4.0' 48.6
1.40
10.1
0.9 41.4
5.88
IJb
9.8
15.2
lOJ
28.4
a2
91.1
4.0
7.8
4.9
19.9
8.1
16.4
83
0.5
6.0
1.7
2.6
97
8.1
8.7
9.7
4.4
4.4
2.8
88JH ai
9.9 8j8
13.9 4.1
1.8,' OJi
8.d 0.8
16.8 IJ
83.9' &4
4.41 ai
3a9{
U.1I 4.4
TWl
Digiti
ized by Google
THE CHEMISTS' MANUAL.
561
Composition op the Ash op Agricultural Plants and Products.
SUSSTAHCX.
00
90
xin.— WOOD.
IflB'Grape
vn Mulberry
ITOBircta
171 Beech, body-wood
173 '" emul wood
ITS " brush
174lOak, bodT-wood
ITS' ** enuu] brancbee with bark. . . .
176 Horse-chestnut twigs, autumn...
177l Wahint twipr», autumn
178 Poplar, young twigs
ITBWtoow. '• "
ISOElm. " "
181 Elm, body-wood
182 Linden
188 Apple tree
184iRedpine
185 White pine
186 Fir
ISTLarch.
S.75
89.8
6.7
&8i 97.8
18,9
8.7
0.8
1.60
6.5
14.8
5.7 673
8.8 10.8
8.6
0.31
11.6
6.8
8.9 60.0
8.6 0.8
4.8
0.66
16.1
8.4
10.8 66.4
6.9
1.0
4.7
1.05
16.8
2.1
16.81 45.8
11.6
0.7
6.7
1.45
14.1
8.8
10 8 4ao
18.8
1.2
9.8
lao
8.6
4,8! 73,5
6A
1.4
1.1
19.8
7.5, 54.0
9.8
1.6
8.1
8.81
19.4
5.9 51.0
21.7
0.7
2.99
15.8
.*.
8.1 65.9
12.2
8Jd
8.9
14rO
0.4
7.5 68.4
18.1
1.5
8.0
......
114
6.6
10.1 50.8
16.4
8.1
a7
94.1
8.1
10.0, 87.9
9.6
5.4
6JI
81.9
18.7
7.7' 47.8
8.3
1.3
8.1
85.8
6.0
4.8 99.9
4.9 5.8' 5.8
1.90
18.0
1.6
5.7" 71.0
4.6' 29! 1.8
0.85
5.8
96.8
6.9 47.9
5.1 8.0 2.0
0.38
15.8
9.9
5.9 50.1
6.5' 8.0
6.0
0.81
ll.fi
4.6
9.1 60.1
6.8 2.8
15.0
0.82
15.8
7.7
84.6, 97.1
8.61
1.7
8.6
0.8
4.8
0.6
0.1
0.1
0.1
OJ
1.4
0.8
0.1
0.6
6.7
i*.6
0.9
4.0
0.8
0.4
0.6
XIV.— BARK.
189,
190
191|
1»9
1981
194
196
198,
Birch
Horve-chestnuti young, autumn'.
Walnut " "
Linden
Red ptne...,
White pine .
Flp. ........
1.88
6.OT
6.40
2.81
3.30
8.01
8.81 5.4
14.7 0.4
84.S|
11.61
8.9| 10.1
16.1 1 5.7
5.3, 4.9
8.0 8.9
8.0 1.0
8.9
4S.6
7JJ
1.8
0.8
67.9
0.4
1.8
4.0
61.8
7.0
1.1
10.6
70.1
5.9
0.8
8.8
72.7
1.6
0.6
8.0
60.8
4.0
0.8
4.7
63.4
8.6
1.0
8.0
60.8
8.5
1.6
1.4
48.7
&8
as
80.1
IJ
18.0
1.1
1.9
0.7
0.4
ao
83
1.8
16.7
OJ
8.4
1.0
81.1
0.1
Digiti
ized by Google
562
THE CHEMISTS' MANUAL.
T A BLE I I.
COMPOfllTION OF FbEBH OB AlR-DRT AgrICTLTCBAL PHO0OCTB, giving
the average quantity of Water, Sulphur, Ash, and Ash-iDgiedients, in
1,000 parts of substance, by Prof. WoLPP.
STTBaTAHOS.
I.— HAT.
Meadow hay. . . .
Dead ripe hay. . ,
Bed clover
White clover
Rwedish clover. .
Lucem
Esparfiette
Green vetches. . .
Green oats
144
66.6
17.1
4.7
8.8
7.7
4.1
8.4
19.7
144
66.2
6.0
1.9
2.8
&6 1 2.9
0.6
41.8
160
66.6
19.5
0.9
6.9
19.2 1 6.6
1.7
1.6
leo
60.8
10.6
4.7
6.0
19.4 , 8,6
5.8
2.7
leo
46.6
16.7
0.7
7.1
14.8
4.7
1.9
0.6
160
60.0
15.2
0.7
8.6
2R.8
6.1
8.7
1.2
160
45.8
179
0.8
2.6
14.6
4.7
1.6
1.8
160
T8.4
80.9
2.1
6.0
19.8
9.4
2.7 1.8 1
146
61.8
24.1
2.0
2.0
4.1
&1
1.7
20.6 1
6.8 I 1.7
88 2.7
2.1 12.1
i.9 ! 2.7
1.8'....
1.1 2.6
1.4
2.8 j 1.5
II.— GREEN FODDER
Meadow graas, In bloseom.
Toan^graea
Byegrasit
Timothy
Other gni»Bes
Oats, MglnDing to head
** In blo<«POTn
Barley, beglnDing to head. .
" in DlosMnn
Wheat, beglnring to head. .
" iiiDloB«om
Bye fodder
BLangnrlan mUleU
Bed clover
Whitedover
Swedish clover
Lacem ,
Esparfiette
AfUhyUis fndneraria
Green vetches
** peas
•* rapeJ
700
28.8
6.0
1.6
1.1
2.7
IJJ
1.2
800
20.7
U.6
0.4
0.6
2.2
2.2
0.8
700
21.8
6.8
0.9
OJi
1.6
1.7
0.8
700
21.0
6.1
0.6
0.8
2.0
2.8
0.8
700
21.8
7.2
0.4
0.6
1.2
1.7
1.0
8W
17.0
7.1
0.8
0.6
1.2
14
0.6
770
16.6
6.6
0.6
0.6
1.1
1.4
0.6
760
22.8
8.6
0.4
0.7
1.6
2.8
0.7
680
%t6
6.9
0.1
0.7
1.4
2.2
0.7
770
22.4
7.8
0.4
0.8
1.1
1.7
0.4
090
21.7
5.6
0.1
0.6
0.7
1.6
0.4
700
16.8
6.8
0.1
0.6
12
2.4
0.2
680
28.1
8.6
1.9
2.6
1.8
Oi)
800
184
4.6
0.2
1.6
4.6
1.8
0.4
810
18.6
2.4
1.1
1.4
4.4
2.0
1.2
816
10.2
8.5
0.2
1.6
8.2
1.0
0.4
758
17.6
4.6
OJB
1.0
8.6
1.6
1.1
786
11.6
4.6
0.2
0.7
8.7
IJi
0.4
780
12.8
18
0.5
0.6
a6
0.9
0.2
820
15.7
6.6
0.6
1.1
4.1
2.0
0.6
815
18.7
6.6
1.1
8.9
1.8
0.6
880
18.6
4.4
0.6
0.6 1
8.1
1.2
UJt
6.9
1.9
0.6
2.1
a4
0.4
6.4
1.1
a7
7.6
1.1
0.8
8.2
0.9
0.7
4.7
0.8
0.8
66
0.7
0.4
7.0
1.2
OJi
10.8
08
0.7
9.4
IJ
0.8
12.8
0.6
M
6.2
....
..••
6.7
1.5
....
0.4
0.6
0.5
0.6
0.4
0.6
0.1
0.8
0.4
0.3
0.8
0.6
0.8
0.4
....
08
0.5
OJ
0.4
0.2
0.4
1.0
OjS
III.— ROOT CROPS.
Potato
Artichoke
Beet
Bagar-beet
Tomip
White tnmlp* .
Kohl-rabi
Carrot
Sagar-beet headst.
750
800
a«
816
909
915
8T7
860
840
ChTccory .' 1800
9.4
6.6
0.1
0.4
0.2
1.8
0.6
0.2
as
10.8
6.7
0.8
0.4
1.6
0.8
. . . ..
0.2
8.0
4.8
1.2
0.4
0.4
0.8
0.8
0.2
0.6
8.0
4.0
0.8
0.7
06
1.1
0.4
0.8
02
7.5
8.0
0.8
0.8
0.8
1.0
1.1
0.2
0.3
6.1
8.1
0.2
0.1
0.8
1.1
0.4
0.1
0.4
9.5
4.9
0.6
0.2
09
1.4
0.8
0.1
Oii
8.8
8.2
1.9
0.5
0.9
1.1
0.0 i OJS
0.8
6.5
1.9
1.6
0.7
0.6
0.8
0.5 0.1
0.1
10.4
4.2
0.8
0.7
0.9
IJS
1.0
0.6
a4
OJI
0.1
0.4
(U
• No special variety?
t Crowns of sagar-beet roots.
Digiti
ized by Google
THE CHEMISTS' MANUAL.
563
CoHPOBinoN OF Frbsh OB AnuDBT Agricultubal Pbodcctb.
SvBnAxam,
IV.— LEAVES AND STEMS OP ROOT CROPa
Potato top0, end of Angiut > 885
'* " flntofOctober T70
Beet tops. 907
Sugar-beet tops ; 807
Tomlptope ; 898
Kohlrabi tops | 850
Carrot top«. 808
Chiccory tops 850
Cabbage heads | 886
** stems l8iK)
15.6
2.8
0.4
2.6
51
1.0
0.9
1.2
0.7
11.8
14.8
0.7
0.1
2.7
6.5
0.6
0.6
0.5
0.4
4.8
8.1
1.4
1.7
0.8
1.1
0.7
1.7
18.0
4.0
8.0
8.8
8.6
1.8
1.4
0.6
1.0
14.0
8.2
1.1
0.6
4.5
1.8
1.4
0.5
1.2
S5.8
8.6
1.0
1.0
8.4
2.6
8.0
2.6
1.0
S8.1
8.7
6.0
1.2
8.6
1.2
2.1
1.6
1.9
18.7
11.2
0.1
0.6
2.7
1.7
1.7
0.2
0.8
12.4
0.0
a5
a4
1.9
2.0
1.1
0.1
as
11.6
6.1
0.6
OJi
1.8
2.4
0.9
OJi
0.1
0.6
0.6
0.6
a6
i'.4
0.6
v.— MANUFACTURED PRODUCTS AND REFUSE.
Bngar-beet cake
a. Common cake
A. Beeldae from centrif. machine
c. Besldae of maceration
Beet molasses
Hola9ses slump*
RaW'beet sngar
Pouto slump*
Potitoflbret
Potato sklust
Fine wheat flour
Bye flour.
Barley our
Barley dust |
Maixe meal
MilletmeaL
Bnckwheat grits
Wheat bran
Bye bran
Bre wer^B grains
Malt :
Driedmalt
Malt sprouts
Winc-gr unds
Grape skins
Beer
Wine.
Bapecaks
Linseed cake
Poppy cake
Walnut cake
Cottoo-eeedcake
692
9.7
692
9.8
820
6.6
885
4.1
175
98.1
907
177
48
18.7
947
5.9
806
1.9
800
67.1
188
4.1
142
16.9
140
20.0
118
49.8
140
9.5
140
11.6
140
6.2
185
66.6
131
71.4
768
12.0
476
14.6
42
86.6
92
69.6
660
16.1
600
16.2
900
89
866
2.8
150
66.0
115
G5.2
100
05.4
186
46.4
116
61.5
8.6 I 0.8
28
2.6
1.5
66.2
15 9
4.6
2,7
0.8
4&8
1.5
6.5
5.8
9.4
2.7
2.8
1.6
13.8
19.3
0.5
2.5
4.6
20.8
8.6
0.1
0.5
0.5
0.1
4.6
0.8
1.4
2.7
88
1.4
8.0
0.8
9.4
11.8
1.2
1.2
8.0 I 0.4
1.5 0.8
1.8'...
18.6 0.1
12.9 , 0.8
19.8 ' 4.8
15.4 1....
21.8 1....
2.6
2.6
1.4
1.1
5.6
I
1.2
0.4
0.9
6.4
0.1
OJI
0.6
IJi
0.6
0.1
2.6
2.6
1.4
0.6
2.2 I 1.0
0.8 I 0.9
0.5 I 2.5
1.0 I
> 0.2;
I 0.2'
6.4 1
8.8 I
4.1 26.8
6.7 I 8.1
2.6 1 2.8
1.2
0.6
2.8
2.1
8.5
9.5
14.4
4.8
6.6
8.0
28.8
84.2
4.6
5.8
0.7
12.5
2.5
8.4
1.8
0.5
20.7
19.4
86.1
20.8
29.6
0.4
0,6
0.6
0.6
1.2
0.4
...
. ••
0.1
, ,
0.1
...
2.0
0.6
9.4
0.8
0.8
8.1
0.1
0.8
0.4
0.2
0.1
0.1
....
0.8
1.8
1.4
0.6
9.9
0.8
— t
....
0.1
"6.6
0.1
....
0.1
8.9....
4.81....
, ,
8.8
....
8.8
17.7
IJK
0.1
0.7
6.6* 0.1
0.1
0.4, 0.1
0.1
0.1 ....
1.0
4.9| 0.1
....
1.9
8-6
0.8
1.9
4.6
0.5
0.7
0.1
0.7
2.6
....
VI.— STRAW.
Winter wheat.
Winter rye....
Winter spelt..
Summer rye...
Barley
Oats.
Peas
Field beau . . .
Garden bean.
141
42.6
4.9
1.2
1.1
2.6
2.8
1.2
154
40.7
7.6
18
1.8
8.1
1.9
0.8
143
47.7
5.8
0.2
0.4
2.8
8.0
0.9
148
47.6
11.1
1.8
4.4
8.1
1.2
140
48.9
9.8
2.0
1.1
8.3
1.9
1.6
141
44.0
97
28
1.8
8.6
1.8
1.5
140
47.2
16.6
0.5
2.6
5.0
8.8
2.5
143
49.2
10.7
2.6
8.8
18.6
8.8
2.8
180
58.4 26.9
2.2
4.6
18.5
4.1
0.1
160
61.5
19.1
8.1
2.7
14.1
4.1
1.8
2a2'....
1.6
23.7 ....
0.9
84.1i....
26.61....
28.61....
1.8
21.2 ....
1.7
17.9 ....
8.9
2.8 8.0
0.7
8.1 8.1
2.2
2.41 2.7
2.1
* Besidue from spirit manulkcture.
t Beftue of starch mannikcture.
t From boiled potatoes.
I BelUso from making barley grita.
Digit!
ized by Google
564
THE CHEMISTS' MANUAL.
Composition of Frebh or Aib-dbt Agricultcral Pboductb.
SUBSTAKCS.
IN
VI.— STRAW.
Backwheat
R^pe
roppy
liaO 61.7
34.1
1.1
1.9 ■ 9.5
6.1 a.7
2.8
4.0
170 38.0
9.7
8.9
2.1 10.1
97 2.7
«.«
4.7
160 06.0 115.1
00
4.8 19.9
2.8 8.4
7.6
1.7
1.4
Vn.— CHAFF.
Wheat
Spelt
Barley
OatB
Maize cob»
Flax-seed halls
188
92.6
&4
1.7
1.2
1.9 1 4.0
180
88.7
7.9
0.2 1 2.1
2.0 : 6.0
1.9
140
122.4
9.4
1.1 1.6
12.7 2.4
8.7
143
79.0
10.4
8.8
2.1
7.0 0 2
2.0
115
5.0
2.4
0.1
0.2
0 2 0.2
0.1
120
68.8
lai
2.5
1.6
17.2 1 6
2.8
75.1'....
0.8
61.4,....
86.7'....
47.8 ....
1.31 0.2
IJ
1C.0| 3.6
1.8
VIIL—TEXTILE PLANTS, ETC.
Flax straw ! 140
Rotted flax stems ! 100
FlQx fiber I 100
Entire flax plant 250
Entire hemp plant .
Entire hop plant.. .
Hops
Tobacco
81.9 11.8 I 1.6
21.6 1.9 I 1.0
6.0 0.2 0.2
82 8 11.8
28.2 ; 6.2
74.0 !l9.4
59.8 122.8
180 ,mj& |64!l
7.8 20.7
8.8
11.1
8.8
6.0
12.2
11.8
10.1
T8.1
2.2
8.0
0.8
0.8
2.1
16.9
9.2
19.0
1.5! 1.4
...I OJi
2.0
41
Heath
Broom {Spartium) ,
Fern (Aspidium). ,
Scouring raf>b {£!qui»etum'). . .
Sea-weed {Fucus)
Beech leaves
Oak leaves ,
Fir leaves (Pinus ndwatriti) . .
Red pine leaves (Anw picea)
'Rffed{Arundo phrag.)
Sedge ( Carex)
RnFb («/fincr/«)
Balnisb (/$dr/w«)
IX.— LITTER
200
160
160
140
ISO
150
irjO
1(K)
160
180
140
140
140
86.1
4.8 1 1.9
8.0
6.8
1.8
18.9
6.9 0.5
2.8 1 8.2
1.6
58.9
25.2 2.7
4.5 ' 8.8
6.7
2(M.4
27.0 1.0
4.7 26.6
4.1
118.0
17.1 28.8
11.2 16.4
8.7
57.4
8.0 > 0.3
a4 25.8
2.4
41.7
1.5 0.2
1.7 20.2
8.4
11.8
1.2 ....
1.1 1 4.9
1.9
48.9
0.7
1.1
7.4
4.0
.38.5
8.3 0.1
0.6
2.8
0.8
69.5
23.1 5.1
2.9
8.7
4.7
46.6
16.7 3.0
2.9
4.8
2.9
74.4
7.2 , 7.7
%st
6.4
4.8
1.6
12.7
0.8
0.7
1.9 0.6
8.0
8.6 6.0
12.9
110.0 11.7
28.8
2.0,11.9
2.1
19.5. 0.2
1.8
12.9 ...
0.5
1.5 0.6
1.4
84.8
1.1
275
2.8
21.8
8."9
4.0
6.0
6.5
4.2
82.2
8.0
X.— GRAINS AND SEEDS OF AGRICULTURAL PLANTS.
Wheat 148
Rye ....
Barley
Oats.
Spelt, with husk.
Maize
Rice, with bask..
husked
Millet, with bask,
hui^ked ...
Sorffbara
Buckwheat
Rape seed
Flax seed
Hemp t>eed
149
145 [
140
148
136
120
I 130
130
181
140
141
120
118
122
Poppy seed i 147 i
17.7
&6
0.6
2.2
0.6 i 8.2
a4
a8'....
1.5
17.8
5.4
0.3 1.9
0.6 ' 8.2
0.4 1 0.81....
1.7
21.8
48
0.6 ' 1.8
0.5 7.2
0.6 j 6.9....
1.4
26.4
4.2
1.0 , 1.8
1.0 6.5
0.4 1 12.8 ...
1,7
85.8
6.2
0.6 2.1
0.9 7.2
0.6 16.8i....
12.3
a3
a2
1.8 0.3 6.6
0.1
0.3 ....
U
69.0 12.7
8.1
6.9
8.6 82.6
0.4
0.4l..,.
8.4
0.8
0.2
0.6
ai 1.7i....
0.1 ....
39.1
4.7
0.4 3.8
0.4 9.1 , 0.1
20.6...
1.8
12.3
2.8
0.7 2 8
....; 6.6 0.2
16.0
4.2
U.6 2.4
0.2' 8.1 i....
i.2....
...
9.2
2.1
aO i 1.2 0.8 1 4.4 0.2
0.2
37.3
8.8
0.4
4.6 6.2 16.4 i 1.8 , 0.4 0.1
a2
82.2 10.4
0.6
4.2 2.7 13.0 0.4 0.4... .
1.7
48.1 ; 9.7
0.4
2.7 11.8 17.5 0.1 I 6 7 0.1
1 SO
7.1
0J»
(U)
[18.6 (16.4
1 1.0
1.71 «^ .
....
Digiti
ized by Google
THE CHEMISTS' MANUAL.
565
Composition of Fresh ok Aib-dbt Agricultural Products.
SUBSTAXCa.
X.— GRAINS AND SEEDS OF AGRICULTURAL PLANTS.
MDBtardaeed.. .
BeetBeed ,
Tnmip eeed
Carrot 8eed
Peas
Vetches
Field beans
Garden beans...
Lentils
Lupines
Clover seed
Eapaniette seed .
190
87.8
6.0
9.2 1 8.9
7.1
14.7
1.8
0.9
0.2
140
48.7 9.1
8.4 , 9.2 . 7.6 1 7.6
2.0
1.0
4.6
im
86.0 i 7.7
0.8
8.0
6.1 14.1
2.5
0.2
m
74.8
148 8.6
5.0
20.0 ll.K
4.2
4.0
2.6
188
»4.d
9.8 , 0.U
1.9
1.2 8.8
0.8
0.2
0.6
1%
W.7
6.8 1 2.a
1.8
0.6
7.9
0.9
0.4
0.2
14t
SW6
12.0 1 0.4 2.0
1.6
11.6
1.5
0.4
0.8
148
».l
11.6 ' 0.8 2.0
2.0
79
1.0
0.2
0.8
184
17.8
7.7 1.8
0.4
0.9
62
0.2
06
138
84.0
11.4 1 6.0
2.1 ; 2.7
8.7
2.3
08
0.6
150
86.9 18.8 1 0.2
4.5 1 2.8 12.4
1.7
0.9
05
IfiO
87.0
10.8
1.1
2.5
11.9 I 9.0
1J»
as
0.4
10.1
0.8
7.8
2.7
2.4
"2.8
2.5
2.8
XL— FRUITS AND SEEDS OF TREES, ETC.
Qmpe seeds
Alder *»
Beech nuts
Acorns, tresh
'* dried
Uorse-chestnats, ttoeh
** f^'een bosk
Apple, entire fhiU
Pear, ** ''
Cherry, " "
Plnm, " "
120 \
140
180 I
5ti0
158
492'
818
*«)
800
780
820
24.7 1 7 1
2.1
8.4
6.9
06
0.8
0.1
44 2 16.6
0.7
85
18.6
57
1.5
14
27.1 6.2
2.7
81
6.7
6.6
0.6
0.5
0.1
9.6 6.2
01
0.5
0.7
1.6
0.2
0.2
0.1
188 11.8
0.1
1.0
1J&
8.8 0.6
04
0.8
120 ; 71
0.1
14
2.7 1 0.2
0.8
&0
61
01
0.8
0.6 0.1
01
0.4
27
1.0
a7
0.2
01
0.4 ; 0.2
0.1
4.1
22
0.4
02
08
06 0.2
0.1
48
2.2 1 0 1
0.2
0.8
0.7 0.2
0.4
0 1
4.0
2.4
0.2
0.4
06
0.2
ai
XII.— LEAVES OF TREES.
Mulberry
Horse-chestnnt, spring. .
autumn
Walnut, spring
'* autumn
Beech, summer
" autumn
Oak, summer
" autumn
Fir, autumn
Bed pine, autumn
m
117
2.8
....'
0.6
8.0
12
0.1
4.1
TW
21.5
8.8;....
08
4.6
6.0
1.3
0.6
0.8
600
80.1
6.9
24
12.2
2.6
0.6
4J
1,2
700
28.2
9.9
....
1.1
6.2
4.9
0.6
0.8
0,1
600
2J.4
7.6
2.8
15.8
1.1
OS
0.6
0.2
750
12.1
2.2
0.2
1.1
4.4
0.9
0.4
18
0.1
550
805
1.6
0.2
1.8
18 7
141
1.1
108
0.1
700
13UJ
4.6
. ...
1.'.) 3.6
1.7
0.4
0.6
600
19 6 1 0 7 1 0.1
0.8 , 9.5
1.6
0.9
6.1
560
6.8; 0.6 ....
0.6 1 2.6
1.8
0.8
0.8
0.8
560
262
0.4
....
0.6
4.0
2.1
0.7
ia4
XIII.— Wood. (Air.dry.)
Grape 180
Mulberry 150
Birch 150
Beech, body-wood 150
small wood 150
" brush 150
Oak, body-wood 150
'* small branches with bark .... 150
Horse-chestnut, young wood In f . ^»|
autumn fi *^
Walnut 150
Apple tree I 160
Red pine 150
White pine I V:Q
Fir 150
Larch 1160
28.4 1
18.7
2.6
5.5 I
8.9!
12.8 1
5.1 I
10.2 1
7.0 I 1.6 ! 1.6
0.9 , 2.0 ; 0.8
0.3 0.2 0.2
0.9 0 2 0.6
1.4 0.2
1.7 0.8
0.6 0.2
2.0
28.1 5.6
25.5
11.0
2.1
2.4.
26:
2.7 I
0.6
8.0
1.8 0.2
0.1 a6 I 0.1
0.4 ' 0 2 I 0.1
0.3 0.1 0.2
0.4 . a2 . 0.7
1.6 14.8
2.0 14.2
0.1
1.0 j 0.1
1.5 01
0.2 ' 0.2
06 I 0.6
0.1 ....
08 ....
ao ....
12 ....
01 ....
0L8
0.2
0.8' 07
0.8 0.2
ai ;
02 I
a4
ai I
Digiti
ized by Google
566
THE CHEMISTS' MANUAL.
Ck)MP08ITI0N OF FBESH OB AlBrDBY AgBICULTTTBAL PbODUCTB.
SUBSTAVOB.
S.
Birch
HorM'Cheatnut, joang In aatumn .
Waloat, youD^ in aatamn
Bed plDe
White pine
Fir.....
XIV.— BARK.
IBO
118
0.4
0.6
09
6.9
0.8
0.9
9.8
M
150
669
18-6
9.2
348
89
0-6
M
0.7
150
64-4
68
6.8
88.1
8.9
0.1
04
a9
160
98-9
18
10
11
149
06
a9
8.8
0-1
160
98.1
9.8
0.9
08
196
0.7
06
9.3
0.8
160
171
0.6
09
0.2
7.6
1.4
ai
6.8
TABLE III.
PBOXIMATB COMPOflmOK OF AGBICULTTTBAL PlAWTB ASJ> PRODUCTS,
giving the average quantities of Water, Organic Matter, Ash, Albumi-
noidfl, Carbohydrates, etc., Crude Fiber, Pat, etc, by ProfeasorB Wolpf
and Knop.*
SUBSTAKCB.
a. IS-!-^ ^
Mendo^ hay, iRedinm Quality
HAT.
14.8 79.6 1 8.9 1 R^ t 41JI
80.0 U
Aft^mmth '.
14.8
16.7
16.7
16.7
16.7
16.7
167
79.9 6 JS 9.6 ' 46.7
77.1 6.9 ia4 99.9
77.7 5.6 9.4 90.8
74.8 8.6 14.9 84.8
76.0 8.8 16.8 '89.9
78.8 1 &0 ia9 98.1
74.6 8.7 t 19.7 . 89.9
94.0 94
Bed doTor, fhll blottBom
•* ** ripe
86.8 Si
48-0. to
White clorer, ftiU bloBsom
86.6 8.5
Swedish or Alii>ike clover (TiifoUwn
" clover, ripe
hyMdam)
80.5 a.8
46.0 IS
Lncero. Toansr.... .... . .. --.rr.,
910 8.3
• LandwMhMShqtmOur JCaleruUr, 1807, throng Knop's AffHckitur-ChmMle, 186B.
pp. 715-790. This Table is, as regards water and ash, a repetition of Table II. bat hadndes
the newer analyses of 1865-7. Therefore the averages of water and ash do not in all ca«e4
agree with those of the former Tables. It gives, besides, the proportions of nitrogeDooc
and non-nitrogenoas compounds, i. «., albnminoids and carbohydrate«, etc It also statei
the avera^s of cmde fibre and of fkt, etc. The discossion of the daU of this Table bek»gt
to the subjects of food and cattle-feeding. They are, however, inserted here, as it b be-
lieved they are not to be fonnd elsewhere in the Bnglish language.
t Organic matUr here signifies the combustible part of the plant
t OarixfhtfdraUs, etc, include &t, starch, sugar, pectin, etc, all in Ihct of orffaiOe mai-
tety except albuminoids and crude fibre.
S OiMftfJI&rtf is impure cellulose.
1 FcA. «te.y is the ether extract, and contains, beaides flit, wax, cfaloroph^ and in sane
resins.
Digitized by Google 1
THE CHEMISTS' MANUAL. 667
PbOXIMATE COMPOSmOK OP AOBICULTUBAL PLANTS AOT) PrODUCTB.
BUBSTAVOB.
II
HAY.
Laoem, in bloasom
Sand Incern. early bloesom (MitHeago kUermedia).
&*pareette, in bloeeom
iDcmmate clover, in bloseom (TYlfolUtm incarruiium)
Yellow " •* " iMadicago lyptUina)
YetdieB, inbloaaom
PtoM, " '*
Field vpiiny, in blossom (Sperffvia ixrvenHs)
** •* after blossom.
Bemdella, '* '' {OmUhopus tativus).
before "
ItmHan rye sraiM (LoAum UoMcum)
Timothy {mieum pralmue)
Xarly meedow grass (A>a ofMiMi)
Created dog''»-tai\ iOipumirut crifUUus)
Boft brome grass (.BtwntM fnotfi«)
Ordkard grass iDactyiis fflomaxUa)
Barley grass (Hordeum pratense)
Meadow foxtail (Alcpecurw pratmtii)
Oat grass, French rye grass {ArrMnathtrvm
otfenacsttm)
EDglleh rre grass (Lottum perenns)
Barter SchwlDgel {Fegtucaf)
Sweet-scented vernal grass (AfUhoxcaUAum
(fdcratvfri}
Yelyet grass (Holeus lanatvs)
Spear grass, Kentncky Blue grass (Boa pro-
iffigjtf)
Rough meadow grass (Pm trivUtiU)
Yellow oat grass (Avenajktveeoerui)
Qnaklng grass (Brixa media)
Areiage of aUtbe grasses
16.7
ie.7
16.7
16.7
16.7
16.7
16.7
16.7
16.7
16.7
16l7
14.8
148
14.8
14.3
14.3
I 14.8
. 143
B,143
d 14.8
2, 14.8
a 14.8
" 14.8
14 8
14.8
14.8
14.8
14.8
76.9 6.4
77.a 6.1
77.1 6.8
76.1 . 7.2
TT.8 I 6.0
75.0 I 8.8
76.8 7.0
73.8 I 9.6
73.6 7.8
77.7 6.6
75.8 7.5
77.9 7.8
81.9 I 4.5
88.8 ' S 4
80.9 I 6.5
80.7 ' 5.0
81.1 ; 4.6
80.4 5.8
79.0 . 6.7
75.8 9.9
T9.9 ' 6.6
81.0 I 4.7
80.8 6.4
80.3 5.6
80.6
78.6
6.1
7.1
79.8 5.9
78.8 I 7.4
79.9 I 5.8
STRAW
Winterwheat ! 14.8 ' 80.9
** rye ' 14.8 89.6
" spelt 114.8 79.7
" barley 114.3 80.9
Summer barley
Oat
Vetch fodder .
Pea
Bean
Lentil
Lupine
Maize
with clover .
14.3 I 78.7
14.3 77.7
14.8 ' H).7
14.8 79.7
14.8 81.7
17 3 I T7.7
14.3 79.9
14.9 81.4
14.0 I 89.0
CHAFF AND HULLS.
Wheat
Spelt
Rye
Barley
Oat
Vetch.
Pea
Bean
Lupine . . . .
Rape
Maize cobs .
14.8 ' 78.7 :19.0
14.8 77.9 a5
14.8 78.9 I 7.5
14.8 i 72.7 ;i3.0
14.8 67.7 ,18.0
15.0 I 77.0 8.0
14.8 179.7 6.0
16.0 77.0 8.0
14.8; 89.9 2.8
10.3I77JS 8.6
10.8|88Ji 9.8
14.4
99.6
16.'9 1 96.9
18.8 ; 86.7
19.9 80.1
146 ! 86.5
14.2 ; 85.8
14.8 1 86.8
12.0 1 89.8
7.8 1 41.7
14.6 90.2
15.8 87.9
8.7
51.4
9.7
48.8
10.1
47.2
9.5
48.0
14.9 1 85.0
11.6 1 40.7
9.6 42.0
10.6
80.5
11.1
85.3
10.9 1 88.9 j
10.4
87.5
8.9
40.9
9.9
86.7
8.9
89.1
8.4
87.6
6.4
42.6
59
42.8
9.6
41.7
9.0
1.6
9.0
2.0
8.0
60
9.6
7.5
6.5
10.9
14.0
4.9
8.0
4.6
2.9
8.5
8.0
4.0
8.5
8.1
10.5
2.5
8.5
1.4
80.9 1
27.0 '
27.7
29.8
82.7
84.7
88.9
28.9
35.9
38.5
27.2
84.7
89.01
88.2
82.8
28.2
38.7
29.7
39.5
86.6
29.5
47.2
40.0
44.0
40.0
9JI
85.1
8.0
27.1
2.6
88.8
8.0
96.2
8.8
25.6
2w5
86.2
2.6
28.0
8J
96.0
9.5
88.9
1.5
96.1
1.9
16.9
2.8
89.7
8.0
25.9
2.9
22.6
%M
81.0
1.8
98.9
9.7
27.2
9.0
20.0
2.5
29.4
9.7
30.2
2.7
33.2
2.9
81.2
9.9
83.6
8.1
89.6
9.8
82.6
8.9
808
9.9
80.3
9.6
28.7
9.6
48.0
1.5
540
1.8
50.5
1.4
48.4
1.4
48.0
1.4
87.5
1.7
40.0
2.0
44.0
2.0
40.0
2.0
84.0
1.0
80.6
2.0
41.8
1.5
4ao
1.1
86.0
1.4
41.6
1.8
46.5
1.9
80.0
1.5
34.0
1.5
86.0
2.0
85.0
2.0
87.0
2.0
8ao
2.5
34.0
1.6
87.8
lA
Digiti
ized by Google
568
THE CHEMISTS' MANUAL.
Proximatb CoicFOBiTiON OP Agricxtltuhal Plants and Pboductb.
BUBSTAKOB.
GREEN FODDER,
Ora^s, before blossom
after '*
Red clover, before biossom. ..
ftUI
White clover, lUll
SwediBh clover, early blossom
" fall "
Lacem, very yoaog
" in blossom
Sand lucem, early blossom. . . . .
Esparsette, m '^
Incarnate clover, in
Yellow clover, in
Serradella, '*
Vetches, **
Peae, *♦
Oats, early blossom
( TtifoUum incamatum).
(MedieasfO lupulina)
(OmUhopus gcUivus)
Rye.
Maize, Inte end Aninist.
" early '* " .
Hnnffarian miUet, in blossom {Panieum gennanieum)
aorgkum 9aech€aratum . .
Sorghum vulgare
Field 8pnrry, in blossom
Cabbage ,
'* stumps
Field-beet leaves
Carrot leaves
Poplar and elm leaves . . .
Artichoke stem
Rape leaves
75.0 I 9S.9
W.O 89.0
88.0 { 15.6
78.0 S0.3
80i5 17.5
85.0 13.5
8S.0 16.2
81.0 I 17.8
74.0 i 94.0
78.0 ' 90.1
80.9 I 18.5
81.5 I 16.9
80.0 18.5
80.0
89.0
81.5
81.0
79.9
84.8
89.9
85.6
74.0
77.8
80.0
80.0
82.0
90.5
18.7
16.9
17.0
17.6
95.5
14.6
16.7
89.0
95.1
91.6
18.0
9.8
16.1
6.7
82.3 ' 14.2
70.0 I 98.0
80.0 ! 17.8
dry 75.6
91
9.0
1.5
1.7
9.0
1.5
1.8
1.7
90
1.9
1.6
1.6
1.5
1.8
1.8
1.6
1.4
1.6
1.1
1.1
9.4
0.9
1.1
9.0
IJt
L9
1.8
8.6
9.0
9.7
945
8.0 I 199
96 l&O
8.3 I
8.7
8.5 I
8.3
8.3 i
4.5,
4.6
4.0
, 8.9
I 2.7,
I 8.5
&6
701
8.1 76
8.S a2
9.8 8.8
8.3 ' 14.9
0.9
R7
1.1
10.9
6.9
160
9.6
16J
9,9
11.9
9.8
]a4
1.6
68
11
199
1.9
4.6
8.9
80
6.0
15.5
8.3
106
90.0
47.6
7i)
1L5
45
80
60
45
66
60
19.5
95
65
7.5
60
81
55
66
65
78
CO
68
67
0.7
0.8
0.8
66
66
68
67
68
0.6
66
0.8
64
0.6
66
66
69
65
4.7 66
115 1.5
78, 1.4
67 I !
68 67
90 I 64
9.8 I 68
1.8 66
80 10
65 1.6
&4,0J»
aO 10
ROOTS AND TUBERS.
Potato [96.0
Jerufialem artichoke I 80.0
Turnip chervil ? (Kocrbelrflbe). .
Kohl-rabi
Field beets (about 3 Ilb. weight).
Sasw beets (1-9 lbs.)
Rota-bagas (about 8 lbs.)
Carrot (about y^ lb.)
Giant carrot (1-9 lbs.)
Turnips (Stoppelrflbc)
Turnips (TuniipsrUbe)
Parsnip
Pumpkin
78.0
88.0
88.0
81.5
87.0
85.0
87.0
91.5
99.0
88.3
94^
94.1
0.9
9.0
91.0
1.1
18.9
1.1
9.0
16.6
1.8
93.1
0.9
8.9
17.0
1.0
10.8
1.9
9.8
7J
1.2
11.1
0.9
1.1
9.1
a9
17.7
a8
1.0
16.4
1.8
19.0
1.0
1.6
9.3
1.1
14.0
1.0
1.6
lOi)
1.7
19.2
0.8
1.9
9.8
IJ
7.7
0.8
0.8
6.9
IX)
7.9
0.8
1.1
6.1
1.0
11.0
a7
1.6
8.4
1.0
4.6
lU)
1.8
9^
IJ)
OJ
OS
66
0.9
61
61
61
61
69
61
61
OJ
61
GRAINS AND SEEDS.
Rice
Winter wheat...
Wheat flour
Spelt
Winter rye . . . .
Rye flour
Winter barley ..
Summer barley .
Oats
Maice
14.6
14.4
12.6
14.8
84.9
88.6
86.7
81.8
1401 ; W.7
14.0 I 84.4
14 8 83.4
14.3 , 88.1
14.3 89.7
14.4 I 88.5
OJJ
7.5 763
69
9.0
18.0 07.6
80
0.7
11.8 74.1
67
8.9
10.0 54.8
166
9.0
11.0 00.9
8.5
1.6
10.5 ; 79J5
1.5
9.8
9.0 86.9
86
16
9.6 66.6
7.0
8.0
19.0 ec.9
168
9.1
laO 08.0
6.6
Digiti
ized by Google
THE CHEMISTS' MANUAL.
569
PbOXIMATE COMPOSmOK OF AORICULTURAIi PlAIITS AKD PRODUCTS.
SUBSTAHCB.
III"
n
H -
GRAINS AND SEEDS.
Minet
Backwheftt
Vetches
Peaa
Beand (field)
Lentils
Lapines
Aeoms withoat shell, dry
" with '* fre»h . . .
Chestnuts withoat Bhell, frei^h
HtdUseed
Flaxseed
Kape seed
Hemp seed
Poppy seed
Horse chestnut
14.0
14.0
14.8
14.8
14.5
14.5
14.6
ao.o
56.0
4dJK
8.4
12.8
11.0
1S.9
14.7
800)
188.0 1
88.6
88.4 I
88.8,
,88.0 1
188.5
83.0'
78.4'
48.0
49.0
,86.9'
82.7 1
'85.1 I
88.6,
178.8
flB.8
8.0 I 14.6
2.4 9.0
2.8 ' 27.5
2.6 . 22.4
8.6 25.5
8.0 I 23.8
SJH ! 81.5
1.6' 5.0
1.0 1 8.0
1.8 8.0
4.7 28,9
20.5
19.4
16.8
17.5
10^
68.1
6.4
8.0
60.6
16.0 ' 2.5
49.2
6.7 i 2.7
02.8
9.2 ; 2.6
45.6
11.6 , 8.0
82.0
6.9
2.6
88.0
14.6
6.0
68.8
4.6
4.8
86.5
4.5 1 2.8
45J2
0.8 2.5
46.0
18.0 41.0
65.0
7.2 37.0
65.4
10.8 40.0
66.2
12.1 88.6
54.7
6.1 41.0
6&8
4.0 .8.80
REFUSE.
Icake
^' residae from centrifhgal machine. . .
" " ♦* •* " maceration
Potato shimp
Rveslomp
Maise slunp
Molasseis damp
Brewer^s grains
Halt sprouts
Fresh malt with sproats
Dry malt withoat eproqts
Wheat bran
Rye bran
Bapecake
Linseed cake
Oold of pleaenre cake
Poppy cake
Hemp cake
Beectmot cake
»* '* withoat shells
Beet molasses
Potato fibre
T0.O
26.6
a4
1.81
82.0
16.8
1.2 1 1.0
92.6
6.6
0.8 1 0.8
94.8
4.6
0.6
1.0
89.0
10.5
05
8.1
89.0 10.5
0.5
2.0
92.0 1 6.8
1.7
1.2
76.6 22.2
1.2
4.9
aO 85.2
6.8
28.0
47.5 50.8
1.7
6.5
4.2 981
2.7
as
13.1 81.8
5.1
14.0
12.5 ,83 0
4.5 14.5
15.0 77.6
7.4 aaa
11.5 '80.6
7.9 28.3
15.0 i7ai
6.9 28.5
10.0 ,81.6
8.4 , 82.5
10.5 85.5
4.0 27.0
10.0 ,84.8
6,2
24.0
12.5 79.8
7.7
87.8
16.7 T2.6
10.8
8.0
82.6
17.1
0.8
0.8
ia6
12.2
4.4
ao
6.8
7.2
5.1
11.1
44.7
89.5
78.8
60.0
58.5
8.5
41.8
87.1
87.7
86.5,
81.8
86.9
64.5
16.0
6.8
a6
1.4
0.6
1.6
1.8
ai
17.5
4.8
ao
17.8
0.2
0.1
0.1
0.1
0.4
IJSt
i!6
2.5
1.5
2.5
a8
15.0 I a6
16.8
11.0
12.5
11.4
22.0
20.6
6.5
9.0
10.0
8.6
ai
6.2
7.6
7.6
1.8 0.1
COFFEE, TEA-
Cfittee bean
Chocolate bean . .
Black China tea .
Qreen ** **
13.0
11.0
15.0
15.0
93 0 1 7.0 I 10.0 I 49.0 I 84.0
86.0 4.0 , 20.0 ! 52.0 18.0
79.0 6.0 I ao 82.0 I 40.0
79.0 ao 6.0 I 27.0 , 45.0
12.6
44.0
ao
ao
Digiti
ized by Google
570
THE CHEMISTS' MANUAL.
TABLE IV.
DETAILED ANALYSES OF BREAD GRAINS.
i
P .
I*
Ajtaltbt.
From Eleaee
*' Saxony
** America
" Flanders
'* Odesea ,
**• Tansanrock .
** Poland
" Haiig;nry
" Egypt
14.6
11.8
10.9
10.7
14.8
18.6
81.6
18.4
S0.6
69.7
64.4
68.4
61.0
fiO.6
67.9
68.4
62.3
66.4
WHEAT.
7.2| 1.3
1.4 3.6
8.8
9.8
6.8
7.9
6.8
5.4
6.0
1.7
86
8.8
1.8
1.7
3.8
1.7
1.7
1.8
1.6
1.6
1.6
1.7
1.4
1.6
1.9
1.7
1.6
14.0 Bonppingault
16.6 Wunder.
10.8 Puleon.
14.6 Peligot.
16.8
14.8
18.9
14.6
14.8
From Heesia —
" France ....
** Saxony
RYE.
18.0! 60.6
8.9
0.9
10.1 ; 1.8
11.6 66.8
10.2
1.9
8.5 ' 8.8
9.1 64.9
0.4
8.8
8.6 ; 1.4
9.6 66.7
6.4
3.1
8.6 8.8
16.0 Freeenias.
14.1 Payen.
18.8 A.lflUler.
16.6jWolff.
From Salcmnnde, Prassia..
BARLEY.
10.5] 60.8| 6.5| 8.01 18.6
18.8 68.7 4.8 8.6 11.6
9.8 60.41 l.al sol 0.7
8.8! 16.7 WoMr.
3.8 18.0PolBon.
3.41 16.0iGrooven.
8.8|
16.7
10.81
66.4|
88.3
OATS.
8.61 6.4| 9.6 ;
!!!:;r6".iri6!6'
S.7| 14.6A.Mmier.
4.1 IS.OKrocker.
8.71 13.6:Ander8on.
Husked, from Vienna —
ki i4 ii
Unhtuked...'.
BUCKWHEAT.
3.6
8.6
13.1
8.6
9.1
78.9
76.7
8.8
4.8
0.9
1.8
8.9
1.0 ....
1.8 ....
8.5 3.6
8.0
87.8
46.0
7.1
0.4
38.0 8.4
12.7jBibm.
18.7 **
IS.OlBoneiMnffanlt.
14 . 2 j Horsford & Krocker.
14.0!Zenneck.
From Saxony
" America ,
" Galacz
" Switzerland
8.8
8.8
9.1
MAIZE.
68.01
64.4!
49.6
51.8
4.0
16.8
30.4
18.6
8.31 10.6 HellriegeL
1.71 13.0, Poison.
1.8 11.8 "
... lO.olBibra.
From Plemont
** Patna
" Plemont
'* East Indies
7.5
7.3
7.8
6.9
79.9
78.9
S.8
RICE
0.6
0.1
0.3
0.9
0.9
0.6
8.4
8.0
14.6|Boii8eingaii]t
9.8 Poleou.
18.7|Pellgot
14.0.Bibra.
Bunked, Hagenan
** Nuremberg..
80.01
10.8
MILLET.
8.01
8.0|
57.0 11.01
3.4
3.0
8 SI 14.0|BonBsin£aiilt
....| 13.8|Blbra.
Digiti
ized by Google
THE CHEMISTS' MANUAL.
571
TABLE V.
DETAILED ANALYSES OF POTATOES, by Grouven.
{AgricnUur-Chemie, He Avf,, p.p. 495 and 855.)
White Potatokb, mswlt duo.
Varioub Sobts.
avebaoe of
19 Analtsbb.
MAinTBED.
Water
Albamen
Ca^ffin ... ... .....
74.95
0.471
0.04
0.29
181
= 2.11
ra.oi
0.891
0.25 • = *•**
2.02 J
1.56
1.60
0.06
13.40
1.24
1.06
76.00
OUadin and Mncldin (?)
2.80
Veeetable Fibrin
Gum and pectin
0.76
S.0O
0.07
17.88
i.go
0.88
181
Oiganlc acids
080
Starch
15.94
OeUnlose
1 01
Aah
096
lOO.
100.
Digiti
ized by Google
572
THE CHEMISTS' MAJ^UAL.
s
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Digiti
ized by Google
THE CHEMISTS' MANUAL.
578
m §§ gs '-
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88S SS 88 i
i 8 838 88g 88
es g?
SjQo Sao
§§ 8S ': : §
§1 §1
t'eiHaioaHoin ^S§
>B8V snaaioiisi I odd
s!
f : : : : I III lli Si If
g, OOO S©S, 03,
SI
0^ do
'asojbasj
-1X0 <i^^ SKixs
'saxa^
ddo 00
§ §i§ ill
t4 doo i-icid
I
odd
^|§
II -
-- IS
1
PS
tneoM
naiiiog itju>x
III
8^S : S
dio'd
§1 Si
«d T^'co
'siKaiaaHOKi
-H8V maiog
ill
ddd
ig
'KOLLVNiairoo
HI 9aioy I
aiHTOHO "K^O '
■ggiaog-Kixoad I
l§8
^dM
'soioKxiKasiY
iSi i§
0.000
0.886
0.000
0.666
ill
!i
do
§22:
5'
1
•9
Md
§8
00?
"!i
S5§
odd
dd
dd
^sis; iH
88^ SS8S lea^ S5ti
Digiti
ized by Google
674
THE CHEMISTS' MANUAL.
oS
ft
I
§§ § i 88 88 888 § §
8S 8 8 ^8 88 888 8 8
Si § § S8 3S ^SSo I § '
t'flUOUOMHDHI
-Hsy STKaiosKX
'nojuNu
'flons
9^ S S aK 88 :|SS S S I
m5<o «* Ok died «6«i a*<^e« *^ "* 3
8^ e ^ :^ ^^
Iff
^ s *
^ e
21
13
de'
i!
-2 ^^
§ i
|1
-8HXJ.ATH
'■xjcsacnuoin
•H«y noniog
'KOIlTJHXaXOO
Mjsaioy
OIHTOHO 'KIIO
'floioiziKaHnv
s
II]
•s§
ss
1
liJ
8 2
ii
I'dlOV EIHJ
»*sT6as
dd d d
88 S3 6^9
11
»9 e&$ s?8 § i
dd dt- K^«fd t^ t^
ii a i Ii ii Hi i i
Hi e
h
is I
is n
I i
*l
I' I
8^
I I'
9 4
Digiti
ized by Google
THE CHEMISTS' MANUAL.
675
TABLE VII.
FRUITS ARRANGED IN THE ORDER OP THEIR CONTENT OP
SUGAR (Average). —(Frbsknius.)
FBB CEKT.
Peaches 1.6
Apricots 1.8
Pliims 2.1
Reinedaades 8.1
MinbeUefl 8.6
Raspberries 4.0
Blackberries 4.4
Strawberries 6.7
Whortleberries 6.8
FIB CUTT.
Carrants 6. 1
Prunes 6.8
Gooseberries 7.2
Red pears 7.6
Apples 8.4
Soar cherries 8.8
Mulberries 9.3
Sweet cherries 10.8
Qrapes 14.9
TABLE VIII.
FRUITS ARRANGED IN THE ORDER OP THEIR CONTENT OP
FREE ACID EXPRESSED AS HYDRATE OP MALIC ACID
(Average).— (Fresenius.)
Redpears 0.1
Mlrsbelles 0.6
Sweet cherries 0.6
Peaches 0.7
Grapes 0.7
Apples 0.8
Prones 0.9
Beioeclandes 0.9
ApricoU 1.1
FSB CBHT.
Blackberries 1.2
Sour cherries 1.8
Plums 1.8
Whortleberries 1.8
Strawberries 1.8
Gooseberries 1.6
Raspberries 1.6
Mulberries 1.9
Currants 3.0
TABLE IX.
FRUITS ARRANGED ACCORDING TO THE PROPORTIONS BE-
TWEEN ACID, SUGAR, PECTIN AND GUM, ETC. (Averages).
— (Fresenius.)
pRtJlTS.
Acid.
SUOAB.
Pbctin, Gum, etc.
Plums
Apricots
1.6
1.7
3.8
2.7
8.0
8.4
8.7
4.8
4.4
4.9
4.9
6.2
6.9
7.0
11.3
17.8
20.2
94.0
3.1
0.4
Peaches
Raspberries
11.9
1.0
Currants
01
Reineclaudes
11.8
Blackberries
Whortleberries
1.2
04
Strawberries
01
Gooseberries
0.8
Mulberries
1 1
Mlrabelles
09
Sour cherries
1 4
Prunes
44
Apples
Sweet cherries .....
6.6
2.8
20
Grapes
Redpears
44.4
Digiti
ized by Google
576
THE CHEMISTS' MANUAL.
TABLE X.
FRUITS ARRANGED ACCORDING TO THE PROPORTIONS BE-
TWEEN WATER, SOLUBLE MATTERS, AND INSOLUBLE
MATTERS (Averages).— (FRESENirs.)
Fbuitb.
Watkb.
SOLUBLI
Mattbbs.
IlTBOLUBUi
Mattbbs.
Baspberries
100
100
100
100
ino
100
100
100
100
100
100
100
100
100
100
100
100
100
9.1
9.8
9.4
9.7
11.0
18.1
12.8
18.0
18.8
14.8
14.6
15.3
16.5
16.6
16.9
18.5
18.6
2S.8
6.9
BUwiberriets
Strawberries
6.5
5.9
Plnms
Cnrranto
Whortleberries
Gooseberries
Mirabelles
Apricots
Red pears
Peaches
0.9
6.6
16.9
8.6
1.5
S.1
6.5
S.1
Prunes
8onr cherries
Mulberries
Apple?
8Ji
1.8
1.5
8.6
RenieclaudcB
l.f
Cherries
Grapes
1.6
6.8
TABLE XL
PROPORTION OF OIL IN VARIOUS AIR-DRY SEEDa
(Acooiding to Berjot.)
(Knop'8 AgrmUturChemie, p. 725.)
(The air dry seeds contain 10-12 per cent, of hygroscopic water.)
Ck>]n. common 40-46
" Schirmrapi 44
" red lodU 40
" white 40
Flax 84
P«>PPy , 40-50
Sesame !.. .... 63
Mnstard, white 80
black 89
Hemp 28
Feanat 88
Gold of Pleasare. 85
Watermelon.... 86
Charlock l6-4t
Oran«e 40
Ctolocynth 16
Cheny 48
Almond 40
Potato 16
Buckthorn 16
Currant 96
Beechnat 84
Digiti
ized by Google
THE CHEMISTS* MANUAL.
577
TABLE XIL
ARTIFICIAL FRUIT ESSENCES.
The following table shows the number of parts of each ingredient to be
added to 100 parts of alcohol (all chemicallj pure).
(DiNOLEB's Polytechnic Jaumal.)
SUBSTAHCS.
Glycerine
duorofonn
Nitric ether
Aldehyde
Acetate of ethyl
FonnlAte of ethyl
Batyxmte of ethyl
Valerianate of ethel
Bensoate of elhel
OBnaothylate of ethel
8ebacic acid
Salicykite of methyl
Acetate of amyl
Batyrate of amyl
Valerianate of amyl
Efuience of orange
Alcoholic ^Tartaric acid.
eolntioufk I Oxalic acid. . .
•ataratedln [Succinic acid,
the cold of I Benzoic acid.
1 !•
|i|
5 I 10
5 > 6
1 , S
1'! 2
6 10
1
1 ...
8 1...
10 6
10
1 ;
1 ...
10 ;...
10
1
10 1
6 I 6
"aVi"
... 1
10
10
Digiti
ized by Google
678
THE CHEMISTS' MANUAL.
GLYCERINE AS A SOLVENT.
Klever has estimated the solubilities of a number of sub-
stances in glycerine. The following are his results.
At the ordinary temperature, 100 parts of glycerine dissolve:
08 parts of Sodic carbonate.
16 parts of Ferrous lactate.
60 '
' Sodic borate.
16
Oxalic acid.
60 '
* Potaasic arseniate.
10
Cupric acetate.
60 '
' Sodic arseniate.
10
Benzoic acid.
60 '
' Zincic chloride.
10
Boradcacid.
60 '
* Tannin.
10
Baric chloride.
60 '
Urea.
8
Sodic dicarbonate.
40 *
* Alum.
8
Ferrous tartrate.
40 *
Potassic iodide.
7.5
Mercuric chloride.
40 '
' Zincic iodide.
6.7
Cinchoninic sulphate.
86 '
' Zincic sulphate.
5.5
Tartar emetic.
88 *
* Potassic cyanide.
5
Calcic polysttlphnret
80 '
* Cupric sulphate.
4
Strychnic nitrate.
27 '
' Mercuric cyanide.
3.5
Potassic chlorate.
26 *
* Potassic bromide.
8
Atropin.
26 '
' Ferrous sulphate.
2.25
Brucin.
22.5 '
* Strychnic sulphate.
1.90
Iodine.
20 *
* Morphlnic acetate.
1
Veratrin.
20 '
* Plumbic acetate.
0.50
Cinchonin.
20 '
* Arsenious acid.
0.50
Quinin.
20 '
* Arsenic acid.
0.45
Morphin.
20 '
* Ammonic carbonate.
0.26
Quininic tannate.
20 *
' Sodic chlorate.
0.25
Strjxhnin.
20 '
' Hydroammonic chlorate.
0.20
Phosphorus.
20 '
* Hydromorphinic chlorate.
0.10
Sulphur.
FORMUUE
OF FREQUENTLY OCCURRING SUBSTANCES.
Acrolein C3H4O.
Alcohol CaHgO (Ethylie).
Alizarin C,oH503,2H20 (Strecker)
Aniline C^jH^jHaN.
Antichlor NajSjOg (H;vT)08nlphite).
Anthracene or paranapthalin Cj^H ,0 (Anderson).
Argols KHC4H40g (Bitrartrate).
Digiti
ized by Google
THE CHEMISTS' MANUAL. 579
Asparagin ■ C4H8N203,H20.
Atropia CiyHaaNOg (Planta).
Ball Boda, Ist product in making. . . Na2C03.
Barilla NajCOg (crude).
Bleaching powder or Javelle water . CaCla + CaCl202.
Benzol C^Hg.
Caftein or thein CgH ,oN402,H20 (Strecker).
Calamine ZnCOa.
Calomel HgCl.
Camphor C,oH,gO.
Cellulin or cellulose CjsHaoOis.
Chalk CaCOg.
Chloral or triehoraldehyd C2CI3HO.
Chloraniline (CgH4Cl)H2N.
Cldoroform CHCI3.
Cinchonia C20H24N2O.
Cinnabar HgS.
Codeia C,8H2|N03.
Copperas or green vitriol FeS04,
Corrosive sublimate HgClg.
Cream of tartar KHC4H40g.
Creasote or kreasote C,2H ,g02?(^orup.Besanez)
Dextrin C^HjoOs.
Dextrose or grape sugar CgH ,205,H20.
( (C3H5)'" )
DiBtearin 4 (CisHajO) > O3.
( H )
Elayl or olefiant gas C2H4.
Epsom salts MgS04,7H20.
Green vitriol FeS04.
Fire damp or light carburet ted ) pj.
. hydrogen *.. ) *'
Fruit sugar or Isevulose C^H , 20^,
Fusel oil or amylic alcohol C5H,20.
Glycerin C3H8O3.
Glauber salts Na2S04,10H20.
Digiti
ized by Google
580 THE CHEMISTS' MANUAL.
Grape sugar dextrose C^H ,205,H20.
Gun-cotton or pyroxylin C,8H2i,9N02,0,5 (Hadow)
Haematein C,gH,20g.
Javelle water, or bleaching powder . CaCla + CaCl202.
Kreasote \?A^^'''V
I (Gorup-Besanez).
Lactose, or sugar of milk C,2H240 ,2-
LflBvulose, or fruit-sugar C^H ,20^.
Leucine C^H 1 3NO2.
Malt sugar C^H ,20^.
Marsh gas CH^.
Meerschaum 2MgO,3Si02.4:H20.
Morphia CjyHjjNOa.
Naphthalin CjoHg.
Narcotin C22H23NO7.
Nitroglycerin C3H5(N02)303.
Nitre KNO3.
Nux vomica, or strychnia C21H22N2O2.
Olefiant gas C2H4.
Palmatin C5, HjgOg (Berthelot).
Paraffin xlcH^).
Pearlaah (crude potassic carbonate) . K2CO3.
Prussianblue i Fe,Cy.e,18H20=
I Fe4Fcy3,18H20.
« " (basic) \ f'®7Cy,8,»^e203,a?H20 =
( Fe4Fcy3,Fe203,arH20.
Tumbull's blue, or ferrous) Fe5Cy,2.ajH20=
ferricyanide ! Fe3Fdcy2,xH20-
Williamson's blue, or ferro- 1 Fe2KCy5,arH20=
potassic ferricyanide ) FeK,Fdcy,a:H20.
T> 1 x» . i Sn"Au2Sn20g4H20.
Purple of cassms < ,^. . v
^ I (Figuier.)
Pyroxylin, or gun-cotton C,8H2i,9N0250,5 (Hadow).
Quick-lime CaO.
Quinia C2oH24N202,3H20.
Rochelle salts KNaC4H40fi,4H20.
Digiti
ized by Google
THE CHEMISTS' MANUAL. 681
Rosaniline •*C2oH|9N3,H20.
Salalembroth eH^NCljHgCla.HaO.
Salammoniac H4NCI.
Salenixam, or bisulphate of potash. KHSO4.
Salgem, or rock salt NaCl.
Salprunella, or fused nitre KNO3.
Salt cake Na2S04.
Salt of sorrel H2C204,2H20.
Saltpetre KNO3.
Scheele's green CuHAsOa-
Schweinfurt green 3CuAs04,Cu2C2H302.
Spelter, or zinc Zn.
Soapstone, or French chalk Mg05Si02.2MgO,8Si02.
Steatite, or soapstone MgO,Si02.2MgO,3Si02.
Stearin C57H, ,oOg (Berthelot).
Strychnia C21 H22N2O2.
Sucrose, or cane-sugar C,2H220, ,.
Tartar emetic 2[C4H4K(SbO)Og].H20.
Toluol CyHg.
Triolein C57H ,040^.
Tripalmatin CgiH^gO^.
Tristearin C57H , ,oOg.
Zylol CsHjo.
FORMUUE
OF THE FREQUENTLY OCCURRINa ACTOS.
Acid Acetic HC2H3O2.
'' Acrylic HC3H3O2.
" Antimonic HgSbOg.
Antimonous HSb02.
Apocrenic ^2^24^ 12O13 ? (Mulder).
Arsenic H3ASO4,
Arsenous H3ASO3.
Aspartic HC4HgN04.
Basic (stearic) ^^te^ssO^-
Digiti
ized by Google ^
582 THE CHEMISTS' MANUAL.
Acid Benzoic HC7H5O2.
" Bismuthic HBiOg.
" Boric H3BO3.
" Bromic HBrOg.
" Butic C20H40O2 (Heintz).
" Butyric HC4H7O2.
" Camphoric HjCjoH ,404.
" Capric (rutic) HC,oH,902.
" Caproic HCgH, ,02-
" Caprylic HC8H,502.
« CarboUc (phenic) HCcHjO.
" Carbazotic (picric-trinitro- ) ur u /rvin \ n
pnenic) )
" Carbonic H2CO3.
" Carminic C,4H,408.
« Citric HaCfiHsOyjHjO (Liebig).
« Chloric C102(0H).
" Chlorous .C10(0H).
" Chromic H2Cr04.
" Diphosphoric H4P2O7.
« Gallic H3C7H305,H20.
« Glycolic HC2H3O3.
" Hippuric HC9H8NO3.
" Hydrobromic HBr.
«< Hydrochloric HCl.
" Hydrocobalticyanic HgCoCyg
" Hydroferricyanic H3FeCyg.
" Hydroferrocyanic H4FeCy5.
« Hydrofluoric HF.
« Hydriodic HI.
" Hydrosulphocyanic HCyS.
" Hydrosulphuric H2S.
" Hypobromous HBrO.
« Hypochlorous C1(0H).
" Hypoiodous HIO.
" HyposulphurouB H2SO2.
Digiti
ized by Google
THE CHEMISTS' MANUAL. 583
Acid Iodic HIO3,
" Kresylic HC7 H ^0.
" Lactic HC3H5O3.
" Malic H2C4H^05.
" Meta-gallic C^H^Oa.
" Meta-phoBphoric H PO3.
" Meta-Btannic H2Sn03.
" Meta-Bilicic H2Si03.
« Meta-tartaric HaC^H^O^.
" Myristic HC.^HayOa.
" Nitric HNO3.
« Nitrous HNO2.
" Oleic HC,8H3302.
« Palmitic HC.gHaiOa.
" Pentathionic HaSgOg,
" Perchloric C103(0H).
" Perchromic H2Cr208.
" Periodic HIO4.
" Permanganic H2Mn208.
« Phenic (carbolic) HCcHjjO.
" Phosphoric H3PO4.
" Picric (carbazotic) H,CgH2(N02)30.
" Pyrocitric H2C5H4O4.
« Pyrogallic CeHg03.
" Pyroligneous HC2H3O2.
" Pyrotartaric H2C4H40fi,H20.
" Eacemic H2C4H40e,H20.
" Saccharic HjCgHgOg.
Silicic (ortho) H4Si04.
Stannic (ortho) H4Sn04.
Stearic HCieHgsOj.
Succinic H2C4H4O4.
Sulphantimonic H3SbS4.
Sulphocarbonic H2CS3.
Sulphosulphuric H2S2O3.
Sulphuric H2SO4.
Digiti
ized by Google
584 THE CHEMISTS' MANUAL.
Acid Sulphurous H2SO3, 14 aq.
" Tetrathionic H2S40g.
" Trithionic HaSgO^.
" Tannic CayHaaOiy (Strecker>
" Tartaric HqCa^aPs-
" Uric or lithic H2C5H2N4O3.
" Valeric or valerianic HC5H9O2.
ARTIFICIAL FORMATION OF ORGANIC BODIES.
1828. Urea. (Wohler.)
1831. Formic acid. (Pelouze.)
1846. Marsh gas. (Melsens.)
1847. Acetic acid. (Dumas, Malaguti, and Le Blanc.)
1857. Cinnamic acid. (Bertagnini.)
1857. « " (Hamitz Hamitzky.)
1858. Formic acid, ethylene, marsh gas, and acetylene.
(Berthelot.)
1858. Acetic and propionic acids. (Wanklyn.)
1859. Glycols. (Wurtz.)
1860. Malic and tartaiic acid. (Eekul^, Perkin and Dappa.)
1861. Gallic acid. (Lauteman.)
1861. Sugar and formic acid. (Boutherow.)
1861. Formic acid. (Kolbe.)
1862. Alcohol. (Wurtz.)
1862. Amylene. (Wurtz.)
1862. Amine from lower cyanides. (Mendius.)
1863. Lactic acid. (Wislecenius.)
1863. Diatomic acids. (Lippeman.)
1863. Leucic " (Frankland.)
1863. Malonic « (Kolbe and Muhler.)
1863. Carballylic " (Maxwell Simpson.)
1863. Isomer of Rutylic alcohol. (Boutherow.)
1864. Secondary biitylic alcohol. (Lieben.)
1864 and 1865. Fatty and aromatic series of acids. (H.
Hainitzky.)
Digiti
ized by Google
N
THE CHEMISTS' MANUAL. ^ 586
1864 and 1865. Toluene and Xylene. ' (Fittig and ToUens.)
1865. Aceconitic acid. (Beeyer.)
1865. Butyric and Caproic acid. (Frankland.)
1865. Isomer of tartaric acid. (Scbogen.)
1866. Toluicacid. (K6kule.)
1867. Oxalic and malonic acids. (Berthelot.)
1868. Neurine. (Wurtz.)
1869. PicoHn. (Schiff.)
1870. Oil of Rue. (Gorup-Besanez.)
1870. Alizarine. (Graebe, Linderman, etc.)
ALCOHOLS.
MONATOMIC ALCOHOLS.
First series, CteHfa+s+SOc (fatty ffroup).
Methylic alcohol, or wood spirit, hjdrate of methjl (Taylor,
1812; Dumas and Peligot, 1885) ^. C, H4 O,
Vinous alcohol, or ordinary alcohol, hydrate of ethyl C4 Hg 0«
Propylic alcohol, or hydrate of trityle (Chancel, 1853) Cg Eg O,
Butylic alcohol, or hydrate of tetiyle (Wurtz, 1852) C, H, qO,
Amylic alcohol, or hydrate of pentyle (Scheele, 1785 ; Cahours
and Balard, 1880) ; C, qH , ,0,
Caproic alcohol, or hydrate of hexyle (Faget, 1852). C , jH , ^O,
(Enanthylic alcohol, or hydrate of heptyle (Faget, 1862) Cj 4H , gO,
Caprylic alcohol, or hydrate of octyle (Bouis, 1851) CigH, gOj
Rutic or capric alcohol, or hydrate of decyle C, 0H2 2O2
Cetylic alcohol, or hydrate of cetyl (Chevreul, 1823 ; Dumas
and PeUgot, 1886) C3SH34OJ
Cerotic alcohol, or eerie, or hydrate of ceryle (Brodie, 1848). . . C54H06OS
Melissic, or myricic alcohol, or hydrate of myridle (Brodie,
1848) CgoHg.O,
Second series, CjnHgnOs.
Acetylenic, or vinylic alcohol (Berthelot, 1860) C4 H4 O,
Allylic alcohol, or hydrate of allyle (Cahours and Hoffinann,
ia56) Cg He O.
Menthic alcohol CcoHgQOf
Third series, CjnHjtt-sOs.
Campholic alcohol, or Borneo camphor (Pelouze, 1840) C, qH, gOf
Digiti
ized by Google
586 THE CHEMISTS' MANUAL.
I^rth eerieSf CsnHin-eOs {aromaUe aeries).
Benzyl alcohol, or hjdiate of benzyl (Cannizaro, 1858) Ci 4Hg O,
Toluic, or tolly lie alcohol (Cannizaro, 1853) C , gHi oOf
Cumylic alcohol, or hydrate of cumyl (Kraut, 1854) CfoHi 40,
Syroceric alcohol, or hydrate of syroceryle (Warren de la Rue,
Muller, 1859) CagH^oO,
Fifth series, C^Uin-bOf.
Cinnamic alcohol, or styrone, hydrate of cinnamyle (Simon,
1839) CsH.uO,
Cholesteric alcohol, or cholchesterine (Conradl, 1775) CjxH^ 4O2
DIATOMIC ALCOHOLS, OR GLYCOLS.
Ethylic glycol, or hydrate of the oxide of ethylene (Wurtz,
1856) C4 Hg O4
Propylic glycol, or hydrate of the oxide of propylene (Wurtz,
1856) Ce Hg O4
Butyl glycol, or hydrate of the oxide of butylene (Wurtz,
1856) Cs H,o04
Amyl glycol, or hydrate of the oxide of amylene (Wurtz,
1856) C , oH , ,04
Hexylglycol, or hydrate of oxide of hexylene (Wurtz, 1854).. . C, jH, 4O4
Capryl glycol, or hydrate of the oxide of octylene (De Cler-
mont, 1865) C 1 eH , 6O4
Saligenine (Piria, 1845) C,4Hg O4
Anise alcohol (Cannizaro and Bertagnini) C^ gH, 0O4
TRIATOMIC ALCOHOLS.
Glycerin (Scheele, 1779 ; Berthelot, 1860) Cg Hg Og
Amylglycerin (Bauer, 1863) CoHjoOg
TETRATOMIC ALCOHOLS
Propylphydte (Carius, 1866) Cg Hg O*
Erythrite (De Luynes, 1862) Cg H.oO,
HEXATOMIC ALCOHOLS.
Mannite (Proust, 1806} C, ^H , 4O, ,
Glucose (Lowitz, 1790; Proust, 1802) C,,H,,0,,
Inoeite (Scheerer, 1850) C,,H,,0,,
PinXte (Berthelot, 1858) C,jH,40,,
Quercite (Braconnot, 1849) Cj (H, 40|t
Digiti
ized by Google
THE CHEMISTS' MANUAL.
687
ALLOYS AND COMPOSITIONa
(Bt Habweix.)
SUBflTAHCB.
55
60
8.7
84.8
75
79.8
98.2
80
88.8
74.3
GO
88.9
90
10
67
66
87*
86
67.8
80
90
98
98
91.4
65.1
404
80
69
73
87.5
88.3
40.4
40.5
81.6
77
80
87 5
77.4
60"
66"
66
50
66.6
88.4
7.4-
69.8
78
84
8.5
6'.%
85
6.4
ao"
11.3
33.3
81
8.8
80"
88
84
13
11.1
31.8
19 8
85.4
6.6
^A
25.4
24
r
40
45"
%T
7.4
85.8
18.8]
i
6
1
81
40
19*
iT
31.6
31.6
84
sia...
monia
i
<
i
0
1
<
Argffntan
s75
89
10.5
14^8
7.8
Ta
8^8
10
10
26
To
1.6
20
10
7
7
1.4
8^6
10.1
81
86.5
18,5
18^4
83
80
18.5
15.6
86"
80
23"
29
88.4
66.6
88^4
4.4
Magne
Sal^m
AiKcntirerotu*
8.5i -
- 7.8
1
- 2.5
Babbitt^B metal
Brass, common
—
*' bard
^* mathematical Instrnments
** Dinchbcck
-
-
-
" redtombac
- rolled
" tntenag
—
** verv ttiDAcloas •
** wheels, valves
35
85
85
** white
-
1.5
8.5
•' wire
" yellow, line
BritauDia metal
'' " whoD Ihsed, add
Bronze, red
»» red
-
" yellow
" cymbals
** gun metal, large
•» *♦ small
medals
" stAttiary. ..............
r7 -
-
Chinese silver
3.48 18
Chinese white copper
T.9
76
30
80
60
•
Chorch bells
(k u
-
-
aock bells
Clocks, musical bells
German silver
—
Oong* . . . . r , ......
16.7 ^8
— —
House bells
Lathe basboff ....,,
Machinerr bearinin
.
" ^"*^hard :::.:..
Metal that expands in cooling..
Montz metal
— —
-
_
Pewter, best
Printing characters
Sheathing metal
Speculum "
Telescopic mirrors
Temper
Typo and stereotype plates ....
White metal
14
80
15 5
ur Q
15.5
-
-
18
** " hard
"
Oreide
.4.4
ca.5
Crei
Qui
imo
cklio
ftart
ae .
[ir6..
.. 1.3
Ifm
izes.
Digiti
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588 THE CHEMISTS' MANUAL.
ALLOYS FOR SOLDERS.
Newton'8 fusible 8Bi+6Pb+8Sn 212°.
Rose's " 2Bl + lPb+lSii 20V.
Amore " 5Bi + 3Pb + 2Sn 199^
Stillmore " 12Sn + 25Pb+50Bi + 13Cd 155°.
For tin solder, coarse 18n + 8Pb 500.
" ordinary 2Sn + lPb 360%
For brass, soft spelter ICu + lZn 550°.
Hard, for iron 2Cu + IZn TOO*.
For steel 19Sn + 3Ca + lZn —
For fine brass work lSn + 8Cu + 8Zn.
Pewter soft solder lBi+lPb + 2Sn.
Goldsolder 24Au+2Sn + lCu.
Silver solder, hard 4Sn + ICu.
soft 2Sn + l brass (wire).
For lead 16Sn+83Pb.
FLUXES FOR SOLDERING OR WELDING.
Iron Borax.
Tinned iron Resin.
Copper and brass SaLammoniac
Zinc Cliloride of sine
Lead Tallow or resin.
Lead and tin pipes Resin and sweet oil.
AMALGAMS.
Gold. — One weight of mercury amalgamates with two weights of gold.
SiLYEB. — 10 silver to 19 mercury.
7 " " 20
Tin. — 1 tin to 3 mercury, for looking-glasses.
1 tin, 1 lead, 2 bismuth, 10 mercury, for glass^lobes.
1 tin, 1 zinc, 3 mercury, for rubbers in electric machines.
Digiti
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THE CHEMISTS* MANUAL.
589
T ABL E.
(By H. jSfrbingicl, Ph,D.)
Showing the total amount of oxygen, and the oxygen available for com-
bustion, in a few oxygen compounds.
Naxx.
Formula.
Total O
IM 100.
Ayail-
ablbOin
100.
Peroxide of hydrogen. .
Water
Nitric acid
Nitric anhydride
Carbonic add
Peroxide of lithium? . . .
Oxalic add
Nitric peroxide
Tetranitromethane
Sulphuric add ,
Perchloric acid
Trinitroglycerin
Nitrate of ammonia
Gun-cotton
Nitrate of sodium ,
TrinitroacetouitriJ
Peroxide of acetyl . . , .
Acetic acid ,
Glycerin
Silica ,
Nitrate of urea ,
Cellulose
Picric acid
Nitrate of potassium . . .
Chlorate of potassium. .
Cyanic add
Cyanuric add
Cyamelide
Fulminuric add
Peroxide of manganese
Nitrate of diazobenzine
Nitrobenzine
Iodic add
Phenol
Fulminating mercury. .
Charcoal
H,0,
H,0
HNO,
N.O.
CO,
LigO,
H.C.O^
NO,
C(N0,)4
HjSO^
HCIO,
C.H,(NO,\0,
NH.NO,
C.H,(lS0,),0.
NaNO,
C,(NO,),N
C,H,0^
C.HgO,
SiO,
H4N,C0,HN0,
C,H,oO.
KaNO,
KaClO.
CNHO T
CaNjHnOn f
CeH^^HNO,
C.H.(NO,)
lA
C-H-O
C,Hg(lfO,)N
CmHaOp
941
88.8
76.2
74.0
72.7
71.1
71.1
69.5
65.3
65.8
63.6
63.4
60.0
50.3
56.4
54.5
54.2
58.8
52.2
51.9
51.4
49.4
48.9
475
89.2
87.2
86.7
28.7
26.2
28.9
17.1
11.2
10.0
47.0
63.5
74.0
£5.5
69.6
65.3
?
55.7
42.3?
50.0?
82.8?
47.0
54.5
18.5?
?
?
82.5
?
41.9
89.6
89.2
18.8
28.9
26.2
28.9
?
11.2
?
Digiti
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590 THE CHEMISTS* MAJfUAL.
THE OLD NAMES FOR A FEW SALTS.
Salt (AMM0i7iACAii, fixed). Calcic chloride.
" (AMMONIACAL, BECRET) of Glauber. Ammonic snlpbate.
(arsenical, neutral) of Macquer. Potassic hjdric aisenata
" (bitter cathartic). Magnesium sulphate.
(COMMON). Sodic chloride.
*' (DIGESTIVE) of Sylvius, Potassic acetate.
" (EPSOM). Ma^esic sulphate.
" (febrifuge) of Sylvius. Potassic chloride.
" (fusible). Ammonic phosphata
*' (fusible) of Urine. Ammonio-sodic phosphate.
" (green). In the mines of Wieliczka the workmen give this name
to the upper stratum of native salt, which is rendered impure bj
a mixture of clay.
" (marine). Sodic chloride.
" (MARINE, argillaceous). Aluminic chloride.
" (microcosmic). Ammonio-sodic phosphate.
" (NITROUS ammonical). Ammonic nitrate.
** OF Amber. Succinic acid.
" OF Benzoin. Benzoic acid.
" OF Canal. Magnesic sulphate.
" OF CoLCOTHAR. Perrous sulphate.
** OF Egra. Magnesic sulphate.
** OF Lemons (essential). Potassic hydric oxalate.
" OF Saturn. Plumbic acetate.
" OF Sbdlitz. Magnesic sulphate.
** OF Seionette. Potassio-Bodic tartrate.
" OF Soda. Sodic carbonate.
" OF Sorrel. Potassic hydric oxalate.
" of Tartar. Potassic carbonate.
« OF Vitriol. Purified zinc sulphate.
" OF Wisdom. Ammonio-mercuric chloride.
•' (perlate). Disodic orthophosphate.
" (polychrbst) of Glaser. Potassic sulphate.
" (sedative). Boracic add.
" (SPIRIT OF). Hydrochloric acid was formerly called by this i
which it still retains in commerce.
" (SULPHUREOUS) of Stahl. Potassic sulphite.
" (wonderful). Sodic sulphate.
" (wonderful, perlate). Diflodic orthophosphate.
Digiti
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THE CHEMISTS' MANUAL.
591
TABLE
SHOWING THE INDEX OF REFRACTION OP A FEW SUBSTANCES.
(FOWNES.) Index of
Substance. Refbaction.
Tabasheer* 1.10
Ice 1.30
Water 1.84
Fluor-spar 1.40
Plate glass 1.50
Rock crystal 1.60
Chrysolite 1.09
Carbon disulphide 1.70
Garnet 1.80
Glass (with much plumbic oxide) 1.90
Phosphorus 2.20
Diamond 2.50
Plumbic chromate 8.00
Cinnabar 8.20
ELECTRICITY.
(Nybtrom.)
ELECTRO-CHEMICAL ORDER OF SIMPLE SUBSTANCES.
Lead.
Boron.
Tungsten.
ORDER OF COM-
POUNDS.
PotaHvinm.
Tin.
Molybdenum.
Sodlom.
Blemath.
Vanadium.
Elbctbo-positiyv.
LIthlam.
C6pper.
Chromium.
Pur.
Barium.
SUver.
Arsenicum.
Smooth glass.
Strontinm.
Mercury.
Phoepbonis.
Woolen cloth.
Calclnm.
Palladium.
Iodine.
Feathers.
Hftgneeinm.
Platinum.
Bromhie.
Wood.
Alnminiom.
Gold.
Chlorine.
Paper.
UraDianL
Hydrogen.
Fluorine.
SUk.
Manganese.
Silicon.
Nitrogen.
Lac.
Zinc.
Titanium.
Selenium.
Rough glass.
Iron.
Tellurium.
Sulphur.
Sulphur.
Nickel.
Antimony.
Oxygen.
Cotton.
Cobalt
Carbon.
ELBCTBO-meATIVB.
EUECTBO-NEOATITV.
In chemical formulas the electro-positive substance is placed first, and the negative last
Oxygen^ befn:; the substance most electro-negative, combines with the most electro-
positive substance In the couple, and the force liberated by the oxidation, or that which
kept the oxidated substance solid, forms the electricity. No electricity can be formed
without the consumption of some force or substance.
The substances are arranged in their order of positive and negative electricity. The
substance is positive to either one below it, and negative to any one above. The exciting
fluid to be diluted sulphuric acid. Other fluids cause some difference in the order, depend-
ing upon the different chemical afllnity between the flaid and the sabstances in the gal^
▼anic couple.
« A ailicioiis deposit in the Joints of the bamboo.
Digiti
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592
THE CHEMISTS' MANUAL.
ORDER OF CONDUCTING POWER FOR ELECTRICITY.
Metals, best conduc-
Living aninuds.
Phosphonis.
Dyed silk.
tor*.
Steam.
Lime.
Bleached silk.
Well-bornt charcooL
Salta soluble in wa-
Dry chalk.
Baw silk.
Flumbago.
ter.
Caoatchoac.
Diamond.
Concentrated acids.
Barefled air.
Camphor.
Mica.
Powdered charcoaL
Vapor of aloohoL
SilicioQs stones.
AU vitriilcatiaiiB.
DUated acids.
Moist earth and
Dry marble.
Qlass.
Saline solutions.
stones.
Porcelain.
Jet
Metallic ores.
Powdered glass.
Baked wood.
Wax.
Animal flaids.
Flower of ^alphnr.
Dry gases and air.
Sulphur.
Sea water.
Dry metallic oxides.
Leather.
Besine.
Spring water.
Oils, the heaviest
Parchment
Amber.
Rain water.
the best
Dry paper.
Shellac.
Ice above 18^ Fahr.
Ashes.
Feathers.
Gntta-perchft, (hs
Snow.
Transparent crystals.
Hair.
tponl eondveter
Living vegetables.
Ice below 18*> Fahr.
WooL
qfalL
VdocUy f^eUetrieUy through the beet eondnctors Is equal to that of light throngfa plane-
tary space— about 200,000 miles per second. When the conductor is insulated with a solid
non-conducting substance, hke gutta-perclia, and immert>ed in water as a submarine cable,
the velocity may be reduced to only 10,000 miles per second, or less.
The substances are set up in their order of conducting power for electricity. The con-
ducting power of substances for heat appears to be in the same proportion as that tor elec-
tricity. The poor conductors for electricity are called insulatort^ and employed between
good conductors to stop the flow or passage of the electric fluid.
POISONS AND THEIR ANTIDOTES.*
As poisoning may and does often occur from accident or
design, it is well for every person to make himself familiar, if
not with the proper antidote (for every poison has its antidote),
with some necessary preliminary treatment before the doctor
arrives. Much suifering and even death may then, in the
majority of cases, be prevented.
** When known that poison has been taken into the stomach,
the first thing is to evacuate it by means of the stomach-pump
or an emetic, unless vomiting takes place spontaneously.
" As an emetic, ground viuatard mixed in warm water is
always safe. Take one tablespoonful to one pint of warm
water. Give the patient one-half in the first instance, and the
remainder in fifteen minutes, if vomiting has not commenced.
In the interval drink copious draughts of warm water. Irri-
tate the throat with a feather or finger, to induce vomiting.
* The following table has been carefully compUed from Wood's Lexicon,
Cutter's Anatomy, and Jahr's (Hull) Symptoms.
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THE CHEMISTS' MANUAL,
598
After vomiting lias begun give mucilaginous drinks, such as
flax-seed tea, gum-arabic water, or slippery elm.
" If the patient is drowsy, give a strong infusion of cold
coffee, keep him walking, slap smartly on the back ; use elec-
tricity ; it may be well to dash cold water on the head, to
keep the patient awake.
" After the poison is evacuated from the stomach to sustain
vital action, give warm water and wine or brandy. If the
limbs are cold, apply warmth and friction.
** In all cases of poisoning, call immediately a physician, as
the after treatment is of great importance."
PomoK.
{Large Otmt.)
Antidotb,
(SbnuBopathicaUY-mnaa
Ooees.)
Chalk, whiting, magnesia, eoap
or oil. Alkaline bicarbonates, milk,
white of eggf or almost any demul-
cent.
China, nux vomi-
ca, coif ea, arsenicum,
belladona.
Acid
Htdboctakic,
or
Pbussic Aero ;
BrTTBB
At.moni>b
(oUof):
Laxjbbl Water.
Drink at once one teaspoonf al of
ammonic hydrate (spirits of harts-
horn) in one pint of water. Inhale
odor of ammonia. Clilorine, either
in vapor, or taken internally. Cold
infusions, artificial respiration,
stimulating injections. Sulphate
of iron.
Same.
Acid
Htdbochloric,
Muriatic, or
Marine Acid.
Neutralize the add by chalk or
calcined magnesia, or a dilute solu-
tion of an alkaline carbonate, milk,
white of egg, strong soapsuds and
lime. Large draughts of tepid
water or mucUage should follow
the antidote.
Large doses : mag-
nesia calcinata, sapo,
medicus. Of small
doses : bryonia (?),
camphor.
Acm Sulphuric
or
OiLOFVrrRiOL.
Same as hydrochloric acid — ^mu-
riatic add.
Pulsatilla.
Acid Oxalic.
Powdered chalk; magnesia, or
its carbonate, suspended in water
or milk. An emetic, if free vomit-
ing is not induced by the above
means.
Same.
Digiti
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^
594 THE CHEMISTS' MANUAL,
PoiBOKs AI7D THEiB AirnT>OTESr-{Continuedi,
POUOK.
{Large cbWM.)
AHTXDOn.
Acid
Phosphoric.
Magnesia, emetics, and emollient
drinks.
Camphor and cof-
fea.
Acid Nitric
or
Aquafortis.
Same as hydrochloric acid.
Calcarea carbontte.
Camphor. Caniom
maculatum. Hepar.
sulph uris-cakaream.
Mercurius. Petro-
leum. Phoephonia
Phosphorus acid.
Sulphur.
Alcohol.
The stomach-pump. Cold affu-
sions. Ammonic hydrate (spirits
of hartshorn).
Same.
Chloroform
and
Ether.
Cold affusions on the head and
neck, ammonia to the nostrils, arti-
ficial respiration, electridtj, open-
ing the trachea.
Same.
Ammonio
Htdratb
(Ammonia, or
Spirits of Harto-
Iiom),
Potash or Soda.
Weak acids, as vinegar and water,
followed hj acidulated demulcent
drinks. Lemon juice, olive oil in
large quantities, large draughts of
cream or milk. Use no emetic
In poisoning by the vapor of
ammonia, the inhidation of the var
por of acetic acid or of dilute hy-
drochloric acid.
Same.
loDims
and Iodide op
Potassium
(Potassic Iodide).
Take a mustard emetic. Drink
a mixture of starch, gruel, or arrow-
root beat in water.
Same.
Mad Doo Bite,
or
Htdrophobia.
Cauterization of the wound with
argentic nitrate (nitrate of silver,
lunar caustic).
The following is said to be suc-
cessful :
Slice or bruise the green or dry
root of elecampane, put into a pint
of fresh milk, and boil down to half
a pint, strain when cold ; drink,
fasting, at least six hours afterward.
The next morning, fasting, repeat
Same.
Digiti
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THE CHEMISTS* MANUAL. 695
PoifiOKS AND THBiB AwtiDCTBa^ConHnued),
Fonov.
Htdbofhobia.
(Continued,)
AjXTtDQTM AHD B>MSDD0.
{Large dote$.)
the dose, using two ounces of the
root Repeat this the third mom-
ing, and it will be sufficient.
According to Dr. Grzyvala, of
England, and Prof. Guber, of Paris,
tanthium 9pino9um possesses anti-
rabic properties. Of the dried
leaves, powdered, the dose for an
adult is nine grains, thrice daily.
For children under that a^e, half
that dose. Sure cure for hydropho-
bia, both in man and animals.
" Gases treated with the actual
cautery and the daily use of genista
tinetoria, died with hydrophobia,
when with the above plant {ean-
thium spin<mtm), similar cases were
all mastered." (British Med. Jour.)
Antedotb.
(HomacpatMcaU^-'amaU
Toadstools
(non^dible
mushrooms).
Prof. Maurice Schiif , of Florence,
has demonstrated that the non-
edible mushrooms contain a common
poison, muecariny and that its ef-
fects are counteracted by atropin or
dantrin.
Same.
Absbnic;
Cobalt
(fly powder) ;
Kino's Yellow;
Ratsbaite ;
scheklb's
Gbsbk.
An emetic, stomach-pump, zincic
sulphate, cupric sulphate ; or mus-
tard mav be used as an emetic, or
salt and water ; or vomiting may
be produced by tickling the throat
witn a feather. The vomiting
should be assisted by demulcent
drinks. After free vomiting, give
large quantities of calcined magne-
sia. The antidote for arsenic is
hyd rated sescmioxide of iron, fresh-
ly predpitated.
if the poison has passed into the
bowels, castor-oil.
Camphor, china,
chin-sulph., ferrum,
hep. iod,, ipee., ntuc. v.,
BBanh,,tabae, verat.
Aktimont
(Wine of);
TabtabEicetic.
Vomiting should be produced
by tepid water ; any astringent in-
fusion, such as tea, oak, bark,
tannin (ground nutgall) ; afterward
opiates (pareeoric). warm bath, and
mustard poultices.
Hepar - sulphuris-
calcareum. Mercu-
rius. Pulsatilla (?).
Babtta Salts.
Stomach-pump or emetics ; mag-
nesic sulphate or soda.
Same.
Digiti
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696 THE CHEMISTS' MANUAL.
PoiBOKs Ain> THsm XsTiDorrE&^ChnUnued).
PoiBoa.
{Large dotu.)
Aimoon.
dOMS.
Ck>PFER;
Vebdigbis ;
Blue Vitriol.
Demulcent fluids to induce vom-
iting, stomach-pump, albumen in
large excess, mUk, cooking soda,
iron filings, manna, preparations of
sulphur.
Belladona, calcarea
carb., china, coc.
dulc. (?), hep. sulph.,
ipec., mer. oorr.. nux
v., rhus, sulphur.
iBOir.
drinks.
Arnica, anenicum,
beUadona, china,
hep. 8., ipec, mere,
puis., verat.
T4RAi> ;
ACBTATE OF
LsAD (Sugar of
White Lead;
LiTHABGB.
Emetic— mustard. Follow with
zincic sulphate (Epsom or Glauber
salts). Antidote is weak sulphuric
acid. Take laige draughts of milk
contunmg white of eggs.
Alum, add. sulph.
in the shape of a
lemonade, belladona,
hyoe., mere, nux v.,
op., plat, Pulsatilla,
sabad., sec. c, stram.,
stiychnine.
Iodine.
Starch or wheat flour beat in wa-
ter, taken in large quantities. Take
a mustard emetic ; tepid baths.
(Mercurius, arseni-
cum), antimony, cam-
phor, arsenicum,
china, chin-sulph.,
coffea, hep. s., op.,
etc
Mbbcuky ;
CORROSIYB
Sublimate
(bug poison) ;
WmTB Pbbgif-
itate;
Red Prucifi-
TATE
(Vennilion).
Beat the whites of ax eagt (albu-
men) in one quart of cold water ;
give a cupful every two minutes.
Induce vomiting. A substitute for
eggs is soap-suds slightly thickened
with wheat flour. Tne white of one
egg neutralizes four grains of the
poison.
Emetics should not be given.
Acid, nitric. mM.
phos., am. c, am.,
are., asaf., aoer.,
aurum m., bell.,
camphor, carb. v.,
china, con., cupr.,
dulc, elec, ferr. iod.,
opium, phosphorus,
staph., sulphate of
zinc, etc ; white of
an egg.
NiTBATBOF Pot-
ash (Saltpetre) ;
Nitrate OF
Soda (Chili
Saltpetre).
Take at once 9, mustard emetic;
drink copious draughts of warm
water; followed with oil or cream.
Same.
Pearl-ash Let
(f m wood aehes);
Salts of
Tartar.
Drink freely of vinegar and wa-
ter; followed with a mucilage, as
flaxseed tea.
Same.
Digiti
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THE CHEMISTS' MANUAL. 697
POISONB AND THEIB AJXTIDOTEA^Contiwud).
Ponov.
AXTIDOTB AlTD BbMKDXBI.
(Largt doBe$.)
dO&6S.
I'hosfhosus
Matches; Rat
EXTEBIflNATOB.
Give two tablespoonfuls of cal-
cined magnena; followed by muci-
laginous drinks.
Camphor, nuz v.,
ooffea, vinum.
Carbomio Acid
Qas (charcoal
fumes);
Chlorinb Oas ;
Nitrous Oxidb
Oas ; or Ordi-
nary Gas ;
BuRNUCG Fluid.
Fresh air and artificial respinu
tlon; may inhale ammonia, ether,
or the vapor of warm water.
Same.
Aconite
or ACONITIN
(Monkshood).
Thorough evacuation of the
stomach, either by an emetic (mus-
tard) or the stomach-pump ; ammo-
nia and brandy, and t le use of stim-
finely-powdered animal charcoal ;
vegetable infusion containing tar-
taric acid. Tincture of nuz vomica.
Iodine and potassic iodide. Keep
patient active. Emetics — ^mustard,
zincic sulphate, or ipecac Wine,
vegetable acids (vinegar acid fruits).
Camphor, nux v.,
par.(?j.guacco(?)
Atropih;
Belladonna
(Deadly Night-
shade).
An emetic and use of stomach-
pump, as with aconite. Morphine
administered by the mouth or sub-
cutaneous ii^ection. Drink black
coffee.
Black coffee, cam-
phor, hepar sulph.,
opium, puis., vinum,
zinc.
Daturin.
Same as above.
Same.
Hellebore;
Helleb Niger.
Emesis and subsequent stimula-
tion. Opium has been used*
Camphor, china.
Nicotin.
Same as above.
Same.
Ofiuh.
Any portion of the unabsorbed
poison should be removed quickly
from the stomach. Use the stom-
ach-pump, or an emetic of gr. xz or
gr. XXX zincic sulphate, or about
gr. X cupric sulphat<». Or powdered
mustard or salt. Keep patient in
Large doses of
black coffee, also by
injection ; camphor,
ether, am. c, natr,,
ipec.. asaf.
Of small doses:
bell., camph., coff..
Digiti
ized by Google
698 THE CHEMISTS' MANUAL.
POISOKS AND THEIR AlVTIDOTEB— (Obn^i'ntMd).
POIBOV.
ASTIDOTB AND HnfEDEM.
{Large dotet.)
Aktidote.
iHomaapalMcaUy-^amaU
domg.
Opium
(Continued),
motion. Apply cold water to head
and chest. Belladonna is recom-
mended as an antidote.
hyos., ipec, mere,
strychnine, nux. v.,
plumb., stram., vi<
num.
Strychnine,
or
Nux Vomica.
An emetic, or use of the stomach-
pump; internal use of chloroform
by iiQialation ; tannic acid, 25 parts
of tannin to one of strychnine ; so-
lution of potassic iodide, iodine,
chlorine, camphor, animal charcoal,
lard or fat, nicotin.
Of large doses :
wine, coffee, camph,,
opium.
Of small doses :
alcohol, bel. , camph.,
cham., cocc., ooff.,
op., puis., stram.
As a rule, *' for tegetdbie poisons give an emetic of mustard ; drink freely
of warm water ; irritate the throat with a feather to induce vomiting. Keep
the patient awake until a physician arrives."
Sting op Insects. — Ammonia; or cooking soda, moistened with water,
applied in the form of a paste. The wound may be sucked, followed by
application of water. Pennyroyal. Ledum palustri.
For buRNS. —Apply immediately hot alcohol or turpentine ; never cold
water. May be bathed afterwards with a mixture of lime-water and sweet
on.
THERMOMETERS.
There are three differently graduated thermometers in use,
namely, Fahrenlieit^ Centigrade^ and Reaumur.
No. 1 = Fahrenheit.
No. 2 = Centigrade.
No. 8 = Reaumur.
To convert the scale of one ther-
mometer into either of the others :
n'^C. = tn'*R = |n*'-i-82'F.
n'R. = }n*'C. = }n'*-i-82°F.
n° F. = 1(11''- 82°)C. = }(n''-82°)R
Digiti
ized by Google
THE CHEMISTS' MANUAL.
599
COMPARISON OF FAHRENHEIT AND CENTIGRADE
THERMOMETERS.
-Wkr.
Omt.
JbAr.
Cnu.
Fahr.
Oent.
rahr.
Cent,
Fafir.
Omt.
—16
-86.11
49
9.44
118
46.00
177
80.55
941
116.11
—14
—95.66
60
10.00
114
46.65
178
81.11
949
116.66
18
-96.00
61
10.56
115
46.11
179
81.66
943
117.99
IS
91.44
69
11.11
116
46.66
180
88.22
944
117.77
11
98.89
68
11.66
117
47.99
181
89.77
945
1184»
10
98.88
64
12.99
118
47.77
182
88.83
946
118.88
9S.78
66
19.77
119
48.38
168
88.88
947
119.44
99.92
56
18.88
190
48.88
184
84.44
948
120.00
91.ff7
67
13.88
191
49.44
186
85.00
949
120.66
91.11
66
14.44
199
saoo
186
85..15
950
121.11
90.65
69
15.00
198
60.55
187
86.11
961
121.06
90.00
60
16.55
194
61.11
188
86.66
9G8
122.29
19.44
61
16.11
195
51.66
189
87.22
958
129.77
18.89
69
16.06
196
52.22
190
87.77
954
198.88
18.88
68
17.93
127
62.77
191
88.88
256
198.88
17.78
64
17.77
198
58.38
193
88.88
966
194.44
+1
-17.9i
65
18.88
129
63.88
198
89.44
967
195.00
■fS
-16.86
61
18^
180
54.44
194
90.00
258
195.66
—18-11
67
19.44
131
55.00
196
90.65
260
126.11
16.56
68
80.00
189
55.56
186
91.11
960
126.66
16.00
69
90.65
183
56.11
197
91.66
961
127.29
14.44
TO
91.11
184
56.66
198
92 29
909
127.77
18.88
71
91.66
185
67.29
199
92.77
963
128.88
18.88
79
93.98
186
57.77
200
96.88
964
128.88
19.T7
78
93.77
IW
66.38
901
96.88
966
129.44
10
18.93
74
98.38
188
56.88
202
94.44
966
180.00
11
11.66
75
93.83
189
60.44
903
96.00
967
180.66
19
11.11
76
94.44
140
60.00
294
96.66
968
181.11
18
10.66
77
95.00
141
60.56
905
96.11
960
181.66
14
10.00
78
95.55
149
61.11
206
96.66
270
182.29
16
0.44
79
96.11
148
61.66
907
97.22
271
132.77
16
8.88
80
96.66
144
62.22
906
97.77
279
138.38
17
8.83
81
97.29
145
62.77
2*19
98.38
978
183.88
18
—7.77
89
37.77
146
68.38
210
98.88
274
184.44
19
-7.99
88
98.83
147
68.88
911
99.44
976
186.00
»
-6.66
84
98.88
148
64.44
919
100 00
976
186.66
U
6.11
86
29.44
149
65.00
218
100.56
277
186.11
»
6.56
86
86.00
150
65.55
914
101.11
278
186.66
i8
6.00
87
80.56
161
66.11
915
101.66
279
187.99
M
4.44
88
81.11
159
66.66
916
102.99
280
187.77
16
8.88
89
81.66
158
07.29
917
1C2.77
281
138.38
»
8.88
90
82.93
IM
67.77
918
103.38
S83
188.88
Tt
9.77
91
82.77
156
68.88
919
108.88
288
189.44
88
9.99
93
83.83
166
68.88
920
104.44
384
140.00
80
1.66
03
88.88
167
69.44
921
105.00
286
140.56
80
1.11
94
84.44 I
158
70.00
939
106 55
296
141.11
81
.66
96
85.00 !
159
70.55
998
106.11
287
141.66
88
.0
96
85.55 ;
160
71.11
994
106.66
288
142.29
88
+0.66
97
86.11 i
161
71.66
295
107.29
280
142.77
+84
+ 1.11
98
86.66
163
78.28
996
107.77
290
143.38
86
1.66
99
87.93
163
72.77
927
108.88
291
148.88
86
9.99
100
87.T7
164
73.83
938
108.8R
292
144.44
87
9.77
101
88.88
166
73.88
229
109.44
298
145.00
88
8.88
108
88.88
166
74.44
930
110.00
294
145.56
80
8.88
106
89.44
167
75.00
9:)1
110.65
996
146.11
40
4.44
104
40.00
168
75.55
232
111.11
296
146.66
41
6.00
106
40.56
169
76.11
933
111.66
297
147 ja
48
6.56
106
41.11
170
76.66
934
112.22
29S
147.77
48
6.11
107
41.66
171
T7.22 t
285
113 77
999
148.88
44
6.66
106
42.98
173
77.T7
986
113.33
800
148.86
46
7.9J
109
42.77
178
78.83 ,
287
113.88
400
904.44
46
7.T7
110
48.88
174
78.88
288
114.44
600
815.56
47
8.88
HI
48.88
175
79.44
239
115.00
800
438.88
48
8.88
119
44.44
176
80.00
940
116.66
1000
687.77
Digiti
ized by Google
600
THE CHEMISTS' MANUAL.
COMPARISON OF CENTIGRADE AND FAHRENHEIT
THERMOMETERS.
Ceni,
Fahr,
Cfmt.
Fahr.
CeiU,
Fahr.
Omt,
Fahr.
Cent.
F^ikr.
978
461
—49
-669
19
86.9
490
788
1100
8018
-880
—486
-48
-64.4
90
88.0
480
806
1110
8080
-«»
—418
—47
—69.6
91
80.8
440
894
1190
8048
—940
—400
-46
-^.8
98
71.6
460
849
1180
800B
-980
-«a
—45
—49.0
98
78.4
460
880
1140
8064
^a90
-864
-44
—47.9
94
75.9
470
878
1160
8109
-910
-846
—48
—46.4
95
77.0
480
806
1160
9180
—900
—828
-49
-48.6
96
78.8
490
914
UTO
8188
-190
-810
—41
^41.8
97
80.6
600
989
1180
8156
-180
-998
-40
-40.0
98
89.4
510
960
1190
8174
—170
-974
-80
-88.9
99
84.9
680
968
1900
8188
-160
-966
-88
-86.4
80
86.0
680
966
1910
8810
-IBO
-988
-87
-34.6
81
W.8
540
1004
1990
8898
-140
-990
-36
-89.8
88
89.6
550
1089
1880
8946
-180
-909
-«
-81.0
88
914
660
1040
1940
9864
-190
-184
-84
-99.9
84
98.9
570
1058
1860
-110
-186
-88
-97.4
85
95.0
680
1076
1960
8800
-100
-148.0
-«9
-95.6
86
96.8
690
1004
1970
8818
— 99
-146J
-ai
-98.8
87
98.6
600
1119
1880
8886
-98
--144.4
-80
-99.0
88
100.4
610
1180
1990
8854
-97
-149,6
—99
-90.9
89
108.9
890
1148
1800
8878
— 98
-140.8
-98
-18.4
40
104.0
680
1186
1810
8B80
- 95
-189.0
-97
—16.6
41
105.8
640
1184
1890
8406
— 94
-137.9
-96
-14.8
49
107.6
650
1908
1880
9486
— 98
—135.4
-95
-18.0
48
109.4
680
1980
1840
9444
— 99
-138.6
-94
-11.9
44
111.9
670
1888
1850
8488
— 91
-181.8
—98
-9.4
45
118.0
680
1956
1800
8480
-90
-180.0
-99
— 7.6
46
114.8
690
1974
1870
8408
-80
—198.9
—91
— 6.8
47
116 6
700
1909
1880
8516
— 88
-196.4
-90
— 4.0
48
118.4
710
1810
1890
8584
-87
-194.6
-19
-9.9
49
190.9
790
1898
1400
96BI
-88
-199.8
-18
— 0.4
60
199.0
730
1346
1410
8!no
— 86
—191.0
—17
+ 1.4
80
140
740
1864
1480
9SBB
-84
—119.9
-16
&9
70
158
780
1889
1480
8806
-88
-117.4
—15
5.0
80
176
780
1400
1440
8884
— 89
—116.6
—14
68
90
194
770
1418
1460
8648
-81
-118.8
—18
8.6
100
919
780
1486
1460
8800
— 80
—119.0
IS .
10.4
110
980
790
1454
1470
8878
— 79
-110.9
.—11
19.9
190
948
800
1479
1480
8896
— 78
-108.4
—10
14.0
180
906
810
1480
1490
9714
-77
—106.6
15.8
140
984
890
1508
1500
9788
— 76
—104.8
— 8
17.6
160
809
880
1696
1510
87B0
-76
-108.0
— 7
19.4
100
890
840
1544
1590
8798
-74
-101.9
— 6
91,9
170
388
880
1569
1680
8786
— 78
-99.4
— 5
98.0
180
866
800
1680
1540
8804
— 79
— 97.6
._ 4
94.8
190
874
870
1698
1650
— 71
-96.8
— 8
9B.6
900
899
880
1616
1560
' 8840
-70
-94.0
— 9
98.4
910
410
890
1684
1570
9868
-89
-99.9
^^ 1
80.9
990
498
900
18fia
1580
9876
-88
-90.4
Zero.
•1-89.
980
446
910
1670
1600
9894
-67
-88.6
+1
+8&8
940
464
990
1888
1600
9918
-86
— 86^
86.6
960
489
980
1706
1610
-65
-85.0
87.4
980
500
940
1794
1690
9048
-64
-889
80.9
970
518
960
1748
1880
9866
-68
-81.4
41.0
980
686
960
1760
1640
9964
-89
— 79.6
49.8
990
554
970
1T»
1660
8008
— 61
— 77.8
44.6
800
679
980
1796
1660
8080
— 60
-76.0
46.4
810
600
990
1814
1870
8008
— 60
— 74.9
48.9
890
606
1000
1839
1680
8066
-68
-79.4
50.0
880
696
1010
1850
1600
8074
— 67
— 70.6
51.8
840
644
1090
1868
1700
8008
-66
-68.8
58.6
860
669
1080
1886
1710
8110
— 65
— (W.O
55.5
860
880
1040
1904
1780
8198
— 54
-65.9
57.9
870
698
1060
1989
17»
8146
- 58
— 68.4
69.0
880
716
1080
1940
1740
8164
— 69
-61.6
80.8
890
734
1070
19B8
17S0
aitt
— 61
— 69.8
69.6
400
759
1060
1976
1700
880O
-60
— 68.0
18
64.4
410
770
1090
1904
1770
8818
Digiti
ized by Google
THE CHEMISTS' MANUAL.
601
Omt.
Fahr.
OmL
F^r.
Omi.
Fakr.
Cent.
Fahr.
Cent.
Fa^.
M80
8286
18TO
8896
1960
8649
9080
8886
2110
8880
1790
8864
1880
8416
1960
8560
9040
8704
2190
8848
1800
8S7S
1800
6484
1970
8578
9050
8792
2180
4166
1810
asm
1900
8458
1960
8606
9060
8740
2140
4184
18S0
8806
1010
8470
1990
8614
9070
8756
9160
4162
1880
8886
19»
8488
8000
8682
2060
8776
9160
4180
1840
8344
' 1900
8606
9010
8660
9000
8794
2180
4216
1860
88S8
1940
8fid4
9090
8668
2100
8812
2200
4262
1860
8880
!
NUMBER OF DEGREES CENTIGRADE = NUMBER OF
DEGREES FAHRENHEIT.
Ill
.1
Tenths or ▲
Dtobxh— CniTieBADB Scale.
.0
.2
.3
.4
.6
.0
.7
.8
.0
Fahr.
Fahr.
Fahr.
Fahr.
Fahr.
Fahr.
Fahr.
Fahr.
Fahr.
Fahr.
0.00
0.18
0.86
0.M
0.79
0.90
1.06
1.26
1.44
1.69
1^
1.96
2.16
2.84
8.65
2.70
2.88
8.06
a94
8.42
860
8.78
8.96
4.14
4.89
4.60
4.68
4.86
6.04
5.22
6.40
6.68
6.76
5.94
6.18
6.80
6.48
6.66
6.84
7.08
7.20
7.88
7.66
7.74
7.98
8.10
888
8.46
a64
8.88
9.00
9.18
986
9.64
9.718
9.90
10.06
10.86
10.44
10.68
10.80
10.06
11.16
11.84
11.68
11.70
11.88
12.06
19.94
13.48
18.60
18.78
19.96
18.14
18.82
18.60
18.66
13.86
14.04
14.82
14.40
14.66
14.76
14.94
15.18
16.80
16.46
15.66
16.84
16.02
16J»
16.36
16.66
16.74
16.92
17.10
17.28
17.46
17.64
17.82
NUMBER OF DEGREES FAHRENHEIT = NUMBER OF
DEGREES CENTIGRADE.
<5(S
Tbmths of a
Degree— FAHBBNnxiT
Scale.
.0
.1
.2
.3
A
.6
.6
.7
.8
.9
Cent.
Cent
Cent.
Cent.
Cent.
Cent.
Cent.
Cent
Cent.
Cent.
0.00
0.06
0.11
0.17
0.28
0.28
0.88
0.88
0.44
0.50
0.66
0.61
0.67
0.78
0.78
0.88
0.80
0.94
1.00
1.06
1.11
1.17
1.28
1.88
1.38
1.89
1.44
1.60
1.66
1.6
1,67
1.78
1.78
1.88
1.80
1.04
2.00
8.06
8.11
2.17
2.82
8.88
8.88
8.80
2.44
2.50
2.66
8.61
8.67
8.72
9.78
8.88
8.89
8.94
8.00
8.06
8.11
8.17
8.83
8.88
8.88
84»
8.44
8.60
8.66
8.61
8.6T
8.78
8.78
8.80
8.89
8.94
4.00
4.06
4.11
4.17
428
4.88
4.38
4.39
4.44
4.60
4.66
4.61
4.67
4.72
4.78
4.88
4.89
4.94
5.00
6.06
5.11
6.17
5.82
5.88
5.88
6.89
6.44
6.50
Digiti
ized by Google
602
THE CHEMISTS' MANUAL.
EXPANSION OR DILATATION OF SOUDS.
(Faradat.)
At 212%^ the length of the bar at 82°= 1.
Bismath 1.0013908
BrasB 1.0019002
Cast-ilwii 1 .0011112
Cement 1.001436
Copper 1.001745
Fire-brick 1.0004928
Glaae 1.000a545
Gold 1.001495
Granite 1.0007894
Lead 1.0028426
Platinum 1.0009642
Sandstone 1.001748
Silver. 1.00201
Slate. 1.0011436
Steel 1.0011899
Stock-brick 1.0005502
Tin 1.002
Wrought-iron 1.0012575
Zinc 1.002»42
DIFFERENT REMARKABLE TEMPERATURES.
CBmaBABB.
Gbbatebt artificial cold produced bj a bath of carbon
bisulphide and liquid nitroiis acid
Greatest cold produced by ether and liquid carbonic
anhydride
Greatest neutral cold recorded in arctic expeditions. .
Mercury freezes
Sodic phosphate 9 parts by weight )
Acid nitric (dilute) 4 " " " J
Ammonic nitrate 5 parts by weight \
Acid nitric (dilute) 4 " *' " t
Sodic sulphate 6 " " '* )
Sodic sulphate 8 parts by weight )
Add nitric (dilute) 2 « " " )
Pounded ice or snow 2 parts by weight )
Sodic chloride 1 " " " )
Sodic sulphate 8 parts by weight )
Add hydrochloric 5 " " " >
Ammonic nitrate 1 part by weight )
Water 1 " " " )
Sodic phosphate 0 parts by weight ^
Ammonic nitrate 6 '* " " >•
Add nitric (dilute) 4 « « « )
Snow 2 parts by weight ) __
Caa, 8 " " " :..)
Snow 2 parts by weight
Add sulphuric 10 " '* "
-140**
-110*
-49"
-39'
+ 10°
to-29''
+w
to-2(r
■hW
to -19'
+ 10''
to -18'
+ 10*^
to -17'
10^ to
-13'.88
lO^'to
-29'.44
26Mlto-55*'J5
I -55'.65 to -or .T7
Digiti
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THE CHEMISTS' MANUAL.
603
Snow 8 parts by weight.
Potash fuaed 4 " "
Sodic sulphate 8 parts by weight.
Add nitrous (dilute) 2 " " " .
Sodic phosphate 9 parts by weight.
Add nitrous (dilute) 4 •' " " .
Ammonia (liquid) freezes
Blood (human), heat of.
** " freezes
Brandy freezes
Charcoal bams
Ice melts
Greatest density of water
Blood heat
Water boUs.
Mercury boils
Hed-heat (just visible^Daniel)
SUver melts
Cast-iron melts
Highest heat of wind ftimace
Point of absolute cold deprived of all heat ,
Lard melts.
Milk freezes
Nitrous oxide freezes
Nitric acid (Sp. Or. 1.434) freezes.
Sea-water freezes ,
Snow and salt (equal parts)
Sulphuric add (Sp. Gr. 1.641) freezes
Acetous fermentation begins
ends
Vinous fermentation
Ckxtiobadb.
0* to -46M1
lO'to-19%44
10" to -24^44
■-48°.88
36^67
3^89
-21^67
438^88
0"
+ 4'
86^6
lOO'.OO
850^00
526'
1002"
1580*
1804*
-275'
85'.00
-IMl
-lOlMl
-42'.77
2'.22
17'.78
-42'.7
25°.65
81M1
15'.55 to 26'.00
TABLE OF BOILING POINTS OF SATURATED SOLUTIONS.
(Watt's Dict. Chbm.— Lbgkand.)
Salt.
WnoHT OF Salt
DI880LTKD IN
100 PARTS OF HaO.
PotAfmic AT-^'tftte , r
798.2
862.2
205.0
200.0
224.8
lOO"" C
Calcic nitrate
isr
Potasfiic carbonate
135"
Sodic acetate
124".4
Sodic nitrate
121"
Digiti
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604 THE CHEMISTS' MANUAL.
Boiling Pointb op Saturated SGLvnovB-^CorUinued.)
Salt.
Wbioht of Bait
DXBflOLTSD IN
lOOpABTLorH.O.
BoELDTo Ponrr.
Potaasic nitrate
Ammonlc rhloride.
836.1
88.0
296.2
61.5
41.2
112.6
117.6
48.6
60.1
116°.9
114^3
114^7
104^2
108*.4
106^6
117».8
104^6
104^4
Potassic tartrate
Potamic chlorate . .
Sodic chloride
Sodic phosphate (dried)
Strontic ch ioride
Sodic carbonate. .....•• • •
Baric chloride,
BOILING POINTS CORRESPONDING TO ALTITUDES OF
THE BAROMETER.
Baboutbb.
BonjKe
POIHT.
Baboxstkb.
BoiLXRe
PoniT.
Bomve
Pdixt.
15 inches.
81.66'' C.
21 inches.
90.22^ C.
27.02 in.
97.05' C.
16.06
8888
22.04
91.50
28.00
98.05
17
84.77
28.02
92.66
29.08
99.05
18
86.22
24.08
98.88
80
100.00
19
87.61
25.08
94.94
81.01
100.94
20
88.94
26.01
96.99
TABLE OF THE CORRESPONDING HEIGHTS OF THE
BAROMETER IN MILLIMETRES AND ENGLISH INCHES.
(Fbok MnxEB's OBOAino Chemibtbt.)
MlLU-
Bnolmh
Mhjj-
BVOLISH
Muxi-
£hqush
■ITBB8
niOHES.
XBTBBB.
orcHss.
MKTBBS.
mcms.
720
—
28.847
789
==
29.095
758
=:
29.848
721
=
28.886
740
:=
29.184
759
=r
29.882
722
=
28.425
741
=
29.174
760
rs
29.922
728
=
28.465
742
=
29.218
761
^z
29.961
724
^
28.504
748
=
29.252
762
=r
80.000
725
—
28 548
744
—
29.292
768
=
80.039
726
=
28.588
745
=
29.881
764
=
80.079
727
—
28.622
746
=
29.870
765
=:
80.118
728
r=
28.662
747
r=
29.410
766
=
80.158
729
—
28.701
748
=
29.449
767
=
80.197
730
=
28.740
749
=
29.488
768
=r
80J»6
731
=
28.780
750
=
29.528
769
=
80.276
782
—
28.819
751
=r
29.567
770
=r
80.816
788
rr
28.858
752
=r
29.606
771
=
80.856
784
z=
28.898
758
=
29.645
772
=r
80.894
785
=
28.987
754
=r
29.685
778
=
80.438
786
=
28.976
755
n:
29.724
774
=
80.478
787
=
29.016
756
=r
29.764
775
rr
80.612
788
r=
29.055
767
=
29.808
Digiti
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THE CHEMISTS' MANUAL.
605
WEIGHTS AND MEASURES.
FRENCH MEASURES OF LENGTH.
(According to United States Standard,)
MiUimetre*. . jX^ metres.
Centimetref . . yj^
Decimetre '^
MetreJ 1
Decametre. ..10
Hectometre . . 100
Kilometre.... 1000
Myriametre. . .10,000
n.S.Iir.
8.03685
30.8685
^93.685
Bead \
measure 1
U. S. Ft.
.008281
.082807
.828071
828071
82.8071
828.071
8280.71
828D7.1
U. S. Ysfl.
.109357
1.09857
10.9357
109.357
1093.67
10935.7
U.S. Mi.
.0621347
.6213466
6.213466
MEASURE OF LENGTH.
Mnjn.
PnsLones.
BoDB.
Yabwi.
Prar.
1
8
80
820
1760
5280
63860
0.125
1
10
40
220
660
7920
0.0125
0.1
1
4
22
66
792
0.003125
0.025
0.25
1
5.5
16.5
198
0.00056818
0.0045454
0.045454
0.181818
1
. 8
36
0.00018939
0.00151515
0.01515151
0.0606060
0.38888
1
12
0.000015783
0.000126262
0.001262626
0.00505050
0.0277777
0.083883
1§
* Nearly the ^ part of an inch. f Fall } inch.
X Very nearly 8 ft. 8} in., which is too long by only one part in (
The metre, at the time its length was fixed by the French government,
was supposed to be a ten-millionth part of a quadrant of a meridian circle
of the earth passing through Dnnkirk and Barcelona.
Subsequent more extended geodetic measurements have shown that it
differs from this by about ^^^ of its length. A platinum rod is therefore
nsed as the standard, which measures at 82' (Fahr.)— O** (C.) 39.3685 U. S.
inches = one metre.
linch
Ifoot
1 yard
Irod
Ifurlong 201.1643 "
Imile 1609.3149 "
§ The Standard Measure of Length in the United States is a brass rod =
1 yard at the temperature of 82'' Fah. The length of a pendulum vibrating
seconds in vacuo at Philadelphia is 1.08614 yards, at + 82' Fahrenheit.
2.54 centimetres.
0.8048 metres.
0.9144 "
6.0297 "
Digiti
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606
THE CHEMISTS' MANUAL.
The inch is sometimes divided into 3 barleyeorru, or 12 Une$.
1 point = ^ inch.
6 points = 1 line = ^ indL
12 lines = 1 inch.
FRENCH SQUARE MEASURE.
{According to U. S. Standard,)
Kamxb.
U. S. 8<|. In.
U. 8. Sq. Fmt.
U.S.SQ.TD8.
U. S. ACIOEB.
Sq. Millimetre
.001549
.154988
10.4988
1549.88
154988
Sq. MiLm.
.8860716
88.60716
.00001076
.00107681
.10763058
10.763058
1076.3058
10768.058
107680.68
10763058
.0000012
.0001196
.0119589
1.195895
119.5895
1196.895
11958.95
1195895
Sq. Centimetre
Sq. Decimetre
Sq. Metre, or Centiarb.
Sq. Decametre, or Are. .
Dbcare (not used)
Hbctabb
.000247
.024709
.247086
2.47086
Sq. Kilometre
247.086
Sq. Myriametr*;^. , t .
24706.6
square inch . . 6.40 square centimetres.
« foot 0.0929 " metres.
'• yard 0.8360 '*
" rod 25.292
« rood 10.1168 ares.
*' acre 404671 "
" mile 258.9894 hectares.
MEASURE OF SURFACE.
Sq. Milbb.
ACBB8.
Sq. Chains.
Sq. Bods.
Sq.ft.
8q. fir.
0.001669
O.0O01669
0.000009764
0.000000898
0.0000000868
0.00000000096
640
1
0.1
0.00695
0.0009006
0.000009896
0.000000143
0400
10
1
0.0696
0009066
0.00009990
0.00000148
109400
100
16
1
0.0880
0.00867
0.00009669
809TB00
4840
484
80.96
1
0.1111111
0.0007716
97878400
48660
4856
979.96
9
1
0.006044
4014489600
096960
fl96W
88904
1996
144
1
Digiti
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1
THE CHEMISTS' MANUAL.
607
MEASURES OF CAPACITY.
{According to U. 8. Standard.)
Naxb.
Litem.
Mlllllltre, or Cubic I ,^
Centimetre f""*
Centilitra t^o
DecUitre. ][ A
Litra.
Decalitre, or Centi-
Btere
Hectolitre, or Deci-
stere
Kilolitre, or Stere
M jriolltre,or Beca-
fltere
10
[lOO
1000
1 10000
Cubic
llBAsna.
1 ca. cent
10 " "
100 ** "
1000 " •*
10 " dec.
A " met.
10 " »*
Dbt Mxasubb.
.001816 di7 pint
.01816 " ••
.1816 " *
.1186 Dk.
= .908 dry qt.
=1.816 dry pt i
.988rr4iba. '
=1.185 pk.
=9.08 dry qt
9.88749 Im.
98.8748 "
988.749 "
Liquid
MXAflUBB.
.0084685 gin.
.064585 '*
f .8495 " t
l=jm81pt )
j 1.06606 qt)
1=2.1181 ptr
(9.64141 U.S.)
1 Uq. galloo. f
[ 86.4141 U.S.
I llq. gallon.
> 964r.l41 U. S. ^
' llq. gallon.
; 9641.41 U. S.
I liq. gallon. !
Cubic
Inchbs.
.0610166
.610166
6.10166
61.0165
610.165, or
.868105ca.ft.
Cubic Fbbt.
8.68106
85.8105, or
1.8078 ca. yd.
868.105, or
18.078 en. yd.
DRY MEASURE.*
1 pint 0.65067 litres,
Iquart 1.10185 "
Ipeck 8.8108 "
Ibuflliel* 85.3482 «
LIQUID MEASURE.t
1 minim 0.0000616 litres.
Ifluiddrachm 0.008697 "
1 fluid ounce 0.039578 "
1 pint 0.47826
Iquart 0.9465
Igallonf 8.786
Ibarrel 129.349
Ihogshead 268.498
* The basis of this measure is the old British Winchester struck bushel
of 2150.42 cubic inches, or 77.627418 pounds Avoirdupois of pure water at
its maximum density. Its dimensions by law are 18^ inches inner diameter,
19 1 inches outer diameter, and 8 inches deep.
f The basis of this measure in the United States is the old British wine
gallon of 231 cubic inches *, or 8.88888 lbs. Avoirdupois of pure water, at its
maximum density (89°.2 Fah., 4** C), the barometer at 80 inches. A cylin-
der 7 inches in diameter and 6 inches high contains 280.904 cubic inches, or
almost precisely a gallon.
Digiti
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608 THE CHEMISTS' MANUAL.
UNITED STATES MEASURE OF LIQUIDS.
Gallok.
QVABTS.
PDm.
Cu. Ik.
Wt. or Lbs. At.
1
0.25
0.125
0.08125
0.004829
4
1
0.5
0.125
0.017815
8
2
1
0.25
0.08468
82
8
4
1
0.18858
231
57.75
28.875
7.2175
1
8.88888
2.15019
1.04269
0.08609
CUBIC MEASURE IN CUBIC METRES.
1 cubic yard 76450 cubic metres.
1 cubic foot 28.81486 *• dedmetres.
Icubicinch 16.88591 " centimetres.
MEASURE OF CAPACITY.
Cu. Yd.
Babbbu.
BV8HXL8.
C?u. Ft.
Gaux>ns.
Cu. iB.
1
0.17R8
0.08961
O.O87067
0.009008
0.004861
0.00008148
6.6108
1
0.8883
0.807B
0.06666
0.08777
0.0001808
86.8467
4L6
1
0.804
a86
0.185
0.000466
87
4 8186
1JM88
1
0.86788
0.18860
0.0006787
100.987
8.78809
1
0.6
0.0081645
801.974
86
8
7.47619
8
1
0.004889
40666
8816
8160.48
1788
4tt
881
1
To convert parts per 100,000 into grains per gallon, multiply by 0.7.
** " . grains per gallon into parts per 100,000, divide by 0.7.
" " grams per litre into grains per gallon, multiply by 70.
BRITISH IMPERIAL MEASURE, BOTH LIQUID AND DRY.
(Oreat Britain only.)
The basis of this system is the imperial gallon of 277.274
cubic inches, or 10 pounds Avoirdupois of pure water at the
temperature of 62° F., when the barometer is at 30 inches.
AvomDUPon
Pounds of
Watbb.
CUBIO
Inchbs.
Cubic
Febt.
Bdob or ▲
CUBB OF
BQUAL CAFA*
CITTIHCBB&
4 gills 1 pint.
2 pints 1 quart.
2 quarts 1 pottle.
2 pottles 1 ffallon.
2 gallons 1 peck.
4 pecks 1 bushel.
4 bushels 1 coomb.
2 coombs 1 quarter.
1.25
2.60
6.
10.
80 1 "^
820 r
640 ^
84.6692
69.8186
188.687
277.274
664.648
2218.192
8872.768
17746636
8.2606
4.1079
6.1756
6.6206
8.2157
1.2837
6.1847
10.2694
13.0417
Digiti
ized by Google
\.
THE CHEMISTS' MANUAL.
To reduce imperial liqtiid measure to IT. S. ones of the same name,
multiply by 1.20082 ; or add one-fifth part. To reduce imperial measure to
U. S. ones, multiply by 1.081515.
SURVEYOR'S MEASURE.
IirOBBS.
LIHK.
VOIM.
CHAor.
FuBLcnre.
MiLB.
'«
1
25
1
792
100
4
1
7920
1000
40
10
1
08860
8000
820
80
8
1
GEOGRAPHICAL AND NAUTICAL MILES.
1 statute mile = 5280 ft. = 0.86875 nautical mile.
1 nautical mile = 6087.424 = 1.150 statute mile.
1 cable length
1 fathom
ROPES AND CABLES
= 120 fathoms
r= 6 feet
720 feet
SURVEYOR'S MEASURE.
Vn.nK.
A0BB8.
Roods.
Pkbches.
Sq. Lxsxs.
1
640
1
2560
4
1
6400.0
100
25
1.0
102.400
160
40
16
1
64.000.000
100.000
25.000
10.000
625
1 9quare mile = 6400 square chains = 640 acres.
1 i»»te = 8 fur. = 820 rods = 1760 yards = 5280 feet = 68.860 inches.
1 sq. acre = 160 sq. rods = 4840 sq. yaids = 48560 sq. feet
208.7108 feet square, or 69.5701 yards square, or 220 feet x 108 feet :
1 acre.
Digiti
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610
THE CHEMISTS' MANUAL.
FRENCH MEASURE OF WEIGHTS.
TSfAME,
MUHgram
Oeot%ram
Docifpram <
Onm
Decagram
HecUH^m ,
Kilogrem
Myriogram ,
Qaintal
ToDnean ; MiUier or Toime
No. OF
Gbaixs.
TWO
10
100
1000
10000
100000
lOOOOOO
Wr. OF Watbb.
i^DAllTY AT
lea. m.m
10 ca. ni.m.
^ en. centimetre.
1 ca. centimetre.
10 ca. cent
Idecalitra
llltre
lOlUree
1 hectolitre
t cubic metre....
Oralni.
.01548816
.1648816
1.648816
15.48816
Fnmdtoo.
.09804787
.8904787
8JW4787
88.04787
S90.4787
S804.787
(hmcm.
86JR8B
TuiqfnUOOti
The gram is the basis of French weights, and is the weight of a cable
centimetre of distilled water at its Tnaximnm density, at sea level, in latJiode
of Paris ; barometer, 29.922 indies.
AVOIRDUPOIS.
1 dram 1.77168 grams.
lounce 28^704 "
1 pound 453;»264 "
1 hundred weight (100 lbs.) 45355J364
1 ton (2000 lbs) 907.10528 kilognms.
lton(2240) 1015.0579
AVOIRDUPOIS.
TOK.
OWT.
OuMun.
Dam.
1
0.05
0.00044642
0.00002790
0.00000174
20
1
0.0089285
0.000558
0.0000848
2240
112
1
0.0625
0.0016
86840
1792
16
1
0.0625
578440
28672
256
16
1
Digiti
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THE CHEMISTS' MANUAL.
611
TROY WEIGHT.
Igndn* 0.004795 grams.
1 pennjweight 1.555008 "
1 ounce 81.10186 "
Ipound 878.2223
TROY.
FOUSJMI.
OUMOES.
PWT.
Obadto.
POUKD AtODL
1
0.088838
0.004166
0.0001786
1.215275
12
1
0.05000
0.00208383
14.58838
240
20
1
0.0416666
219.6666
5760
480
24
1
7000
0.822861
0.068671
0.0084285
0.00020571
1
1 Troy pound = .822857 Avoirdupois pound.
1 Avoirdupois pound = 1.215278 Troy
1 lb. Av. = 7000 gr. Tr. = 1 lb, 2 ob. 11 pwt. 16 gr. Tr,
1 lb. Tr. or Ap. = 5760 *' = 18 ob. 2H* dr. Av.
loB. Tr. orAp. = 480
loi.Av. = 487i
Idr. Ap. = 60
1 dr. Av. = 27H
1 pwt. Tr. =24
1 sc Ap. =20
1 gr. Tr. or Ap. = 1
= 13 OB. 2Ht dr. Av.
= 1 09S. 1^ dr. Av.
= 18 pwt. ii gr. Tr.
= 2^ dr. Av.
= 1 pwt. 3H gr. Tr.
= HI dr. Av.
= mdr.Av.
= AlVdr.Av.
Note. — To change a quantity from one weight to its equivalent in
another weight, reduce the giom quaniUy to Trap grains, and then find
their wtlue in denominations qfthe weight required.
APOTHECARIES WEIGHT.
1 grain 0.064795 grams.
1 scruple 1 . 29591
Idram 8.88773
lounce 81.10186
Ipound 378.2223
* Grain (Lat. grtmum, a seed), the smallest measure of weight in use ; it
is obtained from wheat ; it is taken from the middle ear and well dried.
5760 grains equal 1 Troy pound, and 7000 grains equal 1 Avoirdupois pound.
Digiti
ized by Google
612
THE CHEMISTS' MANUAL.
EQUIVALENT OF METRIC MEASURES OF CAPACITY IN
U. S. APOTHECARIES MEASURE.
Hectolitre
Decalitre.
Litre
Decilitre..
Centilitre.
Gal.
26
Fdtt.
Fluid
OUHOB.
•Fluid
Drax.
20
20
82
8
42
APOTHECARIES FLUID MEASURE.
Mnmn.
Dbaxs.
OUITCEB.
PmTs.
QlIXOMS.
61240
1024
128
8
1
7680
128
16
1
480
8
1
60
1
APOTHECARIES'.*
FOUMM.
OVHOBB.
I>RAX8.
SoBunxs.
Gbaixs.
1
0.08888
0.01041666
0.0084722
0.00017861
12
1
0.125
0.0416666
0.020888
06
8
1
0.8888
0.16666
288
24
8
1
0.05
5760
480
60
20
1
DIAMOND WEIGHT.
CASAT.f
GBAnr.
Pabti.
Gbaixs (Tbot).
1.
0.25
0.015625
0.8125
4.
1.
0.0625
12.5
64
16
1
20
8.2
0.8
0.06
1.
* The pound, ounce, and grain are the same as in Troy weight,
t 1 carat in United Statee = 8.2 grs.; in London, 8.17 gra.; in Paris,
8.18 gn.
Digiti
ized by Google
THE CHEMISTS' MANUAL.
613
GOLD ASSAY WEIGHT.
POUHD.
Ouircx.
Cabat.*
Qbjjx.
<iUA]iTEB.t
1
12
288
1152
'4608
1
24
96
884
1
4
1
16
4
Perfectly pare gold is worth $20.67183 per ounce Troy; or $ia84151 Avoir.
" diver " $ 1.86166 ** " ; or $ 1.24110 "
Standard gold " $18.60465 " " ; or $16.95786 "
silver " $1.22549 ** « ; or $1.11698 "
In the United States the standard for coin is 9 parts by weight of gold or
silver to 1 part of alloy.
SUver,
$15 = 1 lb. Troy ; or $18J^8 = 1 lb. Avoirdupois.
857.08 grains pure silver = $1 ; 28.22 grains pure gold = $1.
T A BLE
SHOWING DIFFERENCE OF TIME AT 12 O'CLOCK (noon) AT NEW
YORK.
(Dick's Enctclop^sdia.)
New Yobk. 12.00 m.
Buffalo 11.40 a.m.
ancinnati 11.18 "
Chicago 11.07 "
St. Louis 10.55 "
San Francisco 8.45 "
NewOrleans 10.56 "
Washington 11.48 *•
Charleston. 11.86 "
Havana 11.26 "
Boston 12.12 p.m.
Quebec 12.12 "
Portland, 12.15 "
London 4.55 •*
Paris 5.05 "
Rome 5.45 "
Constantinoflb 6.41 •*
Vienna 6.00 "
St. Petersburg 6.57 "
Pekin (night) 12.40 a,m.
* The carat is an Abyssinian weight
t The assay quarter-grain equals 1} grains Troy.
Digiti
ized by Google
614
THE CHEMISTS' MANUAL.
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Digiti
ized by Google
INDEX.
Acedc add, 581, ^84.
antluote for, 593.
detection, 153.
Acld,aoecofimc, 585.
mciylic, «8i.
antimonic, 581.
antimonoos, 581.
•pocreDic, 581.
•isenic, 581.
Iwsic, 581.
benzoic, 58a.
bismutluc, 58a.
boracic, 151.
boric, 58a.
bromlc, 147, 58a.
butic, sJBa.
butyric, 583, 585.
camphonc, 58a.
capnc, 58a.
caproic, 58a, 585.
caprylic, 583.
carballylic, 584.
carb«xotic,58a.
carbolic, 58a.
carbonic, 58a.
carminic, 58a.
chloric, 583. X50.
chlorous, 58a.
chromic, 58a, 153.
citric, 58a.
** detection of, 153-3.
" " 'loric, 58a.
rfc, em.
hydriodic, «8ia.
hydrobromic, 147-583.
hydrochloric, 147-149,
58a.
hydrocobaldcyanic,58a.
hydroferricyanic, 147,
58a.
hydrofierrocyanlc, 147,
583.
hydrofluoric, 58a.
hydrosulphocyanic, 58a.
hydrosulphuric, 583.
hypobromous, 58a.
hypochloroua, 58a.
hyposulphuric, 58a.
hyposulphurous, 58a.
kresylic. J583.
lactic, 583, 584.
in*Uc, 583, 584, 153.
meta-galDc, 583.
meta-phoApboric, 583.
meta-silicic, 583.
meta-atannic, 583.
meta-tartaric, 583.
Acid, myristic, 583.
nitric, 150. 583.
nitrous, 583.
oleic, 583.
osallc^ 15Z.
palmitic, 583.
pentathionic, 583.
perchloric, 583.
periodic, 583.
permanganic, 583.
phenk, ^3.
phosphoric, Z50, 583.
picric. 583
p3nnocitric, 583.
pyrogallic, 583.
pyrongneous, 583.
pyrotartaric, 583.
racemic, 583.
charic, 583.
suicic, 153, 583.
stannic, 583.
stearic 583-
succinic, 583.
sulphantimonic, 583.
sulphocarbonic, 583.
sulphosulphuric, 583.
sulphuric, 147, 583.
. sulphurous, <B4.
tannic, 531, 584.
tartaric, 153, 584.
tetrathi nic, 584.
trithronic, 5JB4.
uric, 584.
▼alenc, 584.
Aconltln, 173. 174.
antidote for, 597.
Actinollte, 303.
Asricultund products, 557.
Aud>andite, 390.
Albite, 304.
Alcohol, antidote for, 594.
sp. gr. of, 310^18.
table of, 319.
Alizarin, 585.
Alkaloids, new reac for, 174.
scheme for, zra.
detection ana sep-
aration of, X74.
Alkfaiite,348.
Alloys and compositions, 585.
and solders, 586.
assay of, 503.
Almandite, 390, 303.
Alumlnite, 343.
Aluminium, atomic weight of,
before ^e blow-
charmctensdc re-
actions, 76.
deportment with
reag'nts,73,i54.
Alwminhim, detection, 1x3.
discover^ by, 3.
discovered in, 3.
melting-point, 4.
metallK, 73.
minerals, 343.
oxides, 7s.
salts, X94.
spec, ffravlty, 4.
specific heat, 7.
Alunete, 349.
Alunogen, 341.
Amal^un, 331. «88.
* antidote for, M4.
before the blow-
Ammonia, antidote for.
pipe, Z98.
characteristic re-
action, Z36.
deportment with
reaffenta. 133.
detecdon ot, 137.
specific gravity ol^
337.
table of, f 35.
Amphibole, 303.
Analclte, 305.
Analysis of &tty oils, 178.
of man, 5x7.
of sugars, 479-
qualitative, X38.
Analytical chem., table of,
An£iluale, 305.
Anglesite, 3&1.
Anorthite, 304.
Antimony, aasay of, 5x5.
atomic weight, x,
before the blow-
pipe, X96,aoo. 55,
303.
characteristic re-
action, 55, 71.
deportment with
reagents, 50, 53,
X58.
discovery by, x.
discovery In, x.
film, 198.
melting-point, 4.
metallic, 5X.
minerals, 344.
native, 344.
oxides, so.
price oC 556.
specific gravity, 4*
specific neat, 7.
wine of, antidote
for, S97<
Anhydrite. 350.
Annabeigite, 395.
Digiti
ized by Google
616
INDEX.
beK>r<
Apatite. 950, 997.
ApopbyUite, 905.
Aqtui fortis, antidote for,
594*
An^nite, 350.
Arg^entan, 587.
Aii^entic ozld^ 13.
Argentiferous atfoy, 587.
Argentite, jai, 339.
Afgentous oxide, 14.
Axwnk, antidote for, 595.
atomic weight of, i,
re tiie blowpipe,
Z97400.
duLfacterisdc reac-
tions, 48, 71,
deportment witli le-
agents, 43, 48,
detection, 113.
discovered by, z.
discovered in, z.
film, Z98-900.
meltine-point, 4.
metallk:, 44.
minerals, a 16.
native, 346.
oiides, 43.
price of, 556.
8pedfi<; gravity, 4.
specific neat, 7.
Aisenopyrite, 073.
Araeniolnderite, 973.
Artiads, 3, 3, 4, 5, 6.
Ash of fitter-paper, 370.
Ansylng, 487.
Atropln. Z73, 174, 175.
Atacamtte, 953.
Atlantic ocean, 4zz.
Atomic weights, z, a, 3, 4, 5, 6.
Atoms, zz,
Azotized substances, anaL of,
43^-
Azurite, 363, 969.
Babbitt metal, 40a, 587.
Ball soda, 579.
Barilla, sk'
Barium, atomic weight, s, 4,
»re the blowpipe,
Z97.
chsLzacteristic reac-
tions, zx8.
deportment wHh re-
agents, ZZ4, Z54.
detection, Z37.
discovery by, 9.
discovery In, 3.
melting-point, 4.
oxides, X14.
price of, 556.
salts. xz6.
specific mvity, 4«
specific beat, 7.
Baric, analyses of ash, 56Z,
566.
Barley, 5S9xS&>. , ^
anal3rsis of ash, stow
dust, 558-
flour, 558.
heading out, 555.
in flower, 555.
Barometer, boU.-polnts, 604.
• heights, 604.
Baryta salts, antidote for, <9s.
Batune, sp. gr. heavier than
water, 9Z4.
m. gr. lighter, azd.
Bean, field, 559, 560.
» w J[*«*«» S59» 560-
Bebeenn, Z74.
Beech leaves in autumn, 559,
66a
leaves in summer, 56a
nuts, 560.
Beer. 558.
Beet seed, 560.
sugar,47o.
» -^ V ■naly«te of, 47a.
Beets, ash, 558.
moksses, 558.
raw sugar, 558.
8Ugar,558.
sugar heads, «8.
Bells, composition oi, 585.
" 579.
B, 174.
ente, 961.
' Fetteiucofer's test, 534.
Biotite, 304.
Bismuth, at weight, z, 4< 549.
before the blow-
pipe, 41, Z96, 300,
903.
characteristic reac-
tions, 41.
deportment with xe>
sgents, 38, z69.
detection, 49, 70, 7Z.
discovered by, z.
discovered in, 4.
film, Z98.
minerals, 948.
native, 348.
oxides, jd.
price 0C556.
speci^mvity,4.
specific heat, 4.
Bismuthinlte, 348, 9^9.
Bitter-almonds, antidote for.
Bleaching powders, 579.
Blood, analysis of, 447, sao.
arterial, 591.
coq>uscles, 533.
aystal8,534.
detection of, 533.
diameter, 533.
globules, 533.
plasma, 533.
venous, 53Z.
Blowpipe scheme, aoa
tests, 106, 107.
»1, antidote for, »6.
Boiling-points corres. to altl-
Blue vitriol, antidote f
tudesofbarom
eter, 604.
ofdi£sol.,6o3.
Bones, 537, 538.
Boracic, 15Z.
Boracite. 387.
Borates, before the blowpipe,
Z97.
BoriddSf*!
Bomite, 363, s66.
Boron, atomic weight, z, 4.
discovered By, z.
discovered in, z.
melting-point, 4.
specific gravity, 4.
specific heat, 7.
Bowmonite, 384.
Brass, composition of, 587.
Braunite, 390.
Brewen* grains, 558.
Brine, 460.
Britannia metal, 40s, 587.
Brochantite, 363.
Bromine, atomic weight, i.
Ml 549>
before the blow-
^ J>lpc, «9;vaoo.
dacoveied by, z.
discovered in, z.
specific gravity, 4.
specific heat, 7.
Bromyrite, 33Z.
Bronze, composition o^ 587.
Broom, 559.
Brudn, Z73, Z74.
Brucite, 387.
Buclcwheat, 550, 560, 570.
Bulrush, 559.
Bums, remedy for, 598.
Butter, 460.
Buttermilk, 460.
C.
Ctdmlum, at. wt, x, 4, «J9.
before the Slow-.
action, 38, 7Z.
deportment with
reafents,3s,i6a.
deteraon, 43.
discovered by, a.
discovered In, a.
film, X98.
melting-point, 4.
metaUK, 36.IL
price of; 556.
oxides, 35.
saltSja, 36, Z04.
specific gravis, 4.
specific heat, 7.
Caesliim, at weight, i, 4« 549^
deportment with r»>
agents, z.
discovered by, z.
discovered in, z.
melting-point i.
specific gravity, &
specific heat, 7.
Calfcfa, Z74, 579.
Calamine, 305, 579.
Calaverite, 37a
Calcite, 350, 35Z.
Calcium, atomic weight, a, 4,
b^Nre the blowpipe,
X97. ^ ^
characteristic leao*
tion, za4.
deportment witii re*
agents, zsz, zs4.
detection, za7.
Digiti
ized by Google
^
INDEX.
617
Calcium dlsoorered by, a.
discovered in, a.
melting-point, 4.
metallic, zaa.
minerals, ajo.
oxides, zai.
price of, 556.
■alts. xaa.
specific navity, 4.
specific beat, 7.
Calculations, 353.
Callainlte, 397.
Calomel, 394, 579.
Camphor, 579.
Cane-sugar, 466, 471, 476.
rotatory power,
Carbon, at weight, j, 4, 549-
discovered by, 3.
minerals of, aso.
specific gravi^, 4.
specific heat, 7.
Carbonates before the blow-
pipe, 197.
Cari>onic judd, detection of,
aoo.
Carrot'-seed, 560.
Carrots. 558.
Casamaiors scheme, 196.
Cassitente, 330, 331.
Cast-iron, analyses of, 387.
analysis, 384.
Castor-oO, 176, 178.
Celestite, 3a8.
Cellulin, 579.
Cellulose, 579.
Centigrade mto Fahren., 600.
Cerargyrite, 331. 335.
Cereals, green, light, 557.
heavy, 557.
Cerium, atomic weight, a, 4.
before the blowpipe,
196.
deportment with re-
discovered by, a.
discovered in, a.
melting-point, 4.
price of, 556.
spsdfic gravity, 4.
Cerruslte, 384, aBs.
Chabazite, 306.
Chaif, 559.
anal3rsisofash, 564.
Chalcanthite, 363.
Clialcocite, 363, a6s.
Chalcopyrite, 363, 367.
Chalk, 579.
Cheese, 460.
Chemical calculations, 353.
Cherries, 573.
Cherry, entire fruit, 560.
Chiccory, 1:58.
Chinese suver, composition
of, 587»
Chloral, i;79.
Chloraniune, 579.
Chlorastrolite, 305.
Chloric acid, 150.
Chlorimetry, 437.
Chlorinated compounds, 443.
Chlorine, at weight, x, 549.
before the blow-
pipe, 196, aoob
detection c^, aoo*
discovered by, 1.
discovered in, x.
Chlorine, specific gravity, 4.
specific heat, 7.
Chloroform, 570.
antidote for, 594.
Chocolate, anaL of ash, 569.
Chromic acid, xsa.
iron anal3r8e8 of, 369.
iron analysis, 388.
Chromite, a6o, 373.
Chromium, at. wt., 1, 4. C49.
before tne blow-
pipe, xod, 83.
chazactenstic re-
actions, 83.
deportment with
reagents, 76, X58.
detection of ttj.
discovered by, 3.
discovered in, 3.
metallic, 80.
minends, a6o.
oxides of, 76.
price of, 556.
salts, 8z, Z9^.
Chroiidrodlte,304.
Chrysoberyl, a4a.
Chrysocolla, 305.
ChrysoIite.303-
Church-l>ellB, comp. of, 587.
Chyle, 535, 536.
Cmchonia, 579.
CinnatMr, 394, 579.
Citric acii,iia.
City waters, purity of; 431.
Clausthalite, 384.
Clay, analyses of, 434.
analysis, 433.
Clays, chemical, 3x8.
ordinary, 3x7.
Cloclc-bells, comp. of, 587.
Clover, red, 557.
Swedish, 557«
white, 557.
Clover-seed, 560.
Coal, 336.
analysis, 4ax.
analysis of ash, 341.
and wood, composition
anthradte, 340.
bituminous, 340.
Brier Hill, 336.
brown, 340.
cannel, 34 x.
districts, 34X.
evap. power of, 347.
measure, 336.
non-calcing, 340.
series, 336.
343-
Cobalt, at wt. of, ^ 4* 549-
before the olowpipe,
X96, zox.
characteristic reac-
tions, zox.
deportment with re-
agents, 96, x6a.
detection, XX3.
discovered by, 3.
discovered in, 3.
melting-point, 4.
metallic, 98.
Cobalt, muwrals of, a6i.
oxides of, 96.
price oi; 556.
«It«,^, 194.
specific gravity, 4,
K>ecific beat, 7.
Cobaltite, a6x, a6a.
Codeia,579.
Codein, 174, X75.
Cod-liver oil, X76.
ColTee, analyses of ash, 569.
Coins, standard, 6x4.
Colchicin, X7a, X75.
Columblte, 373.
Columbium, atomic weight,
a, 4, 549- ^ __.,^
deportment with
reagents, X58.
discovered by, a.
discovered in, a,
melting-point, 4. ^
price of, 556. \ j
specif, gravity, 4.
specific heat, 4.
Compounds, reduc. of, 363.
specific heats o£^
8,9,10.
various sp. gr.
of, 335.
Condensed milk, 46X.
Conin, X73, 174, X75.
Copiapite, 373.
Copper, analysis of, 394.
antidote for, 596.
atomic weight, x, 4.
before the blowpipe,
Z96.
characteristic reao-
tk>n, 35, 7x.
deportment with re-
agents, 30, z6a.
detection, ^.
meltiiMf-point, 4.
metallic, 3a
minerals of, 363.
native, 363, 364.
ore analy8is,393.
oxides, 3X.
price of, 549, 55«- ,
P3rrites, analyses ol,
specific gravity, 4.
specific heat, 7.
Copperas, 57?. ^
iblimate, ^79.
antidote for, 596.
Corrosive sublimate, ^79.
Corundum, 343.
Cotton-seed calce, 559.
Cream, 460.
of tartar, 579.
Creasote, 579.
Crocoite, 384.
Croton water, 430.
Cryolite, 34a, 343.
Cryptolite, 397.
Cuprite, 363. 364.
Currants, analysis of, 579.
Cyanite, 305.
DatoUte, 305.
Daturin, antidote for, 597.
Dead Sea. 4XX.
Defunct elements, 554.
Delpliin, X7a.
Digiti
ized by Google
618
INDEX.
Depoitmenl of metals with
reagenta, 13.
of salts, with re-
agents, 13.
Determination of ap. gr., 907.
Dextrin, 579.
Dextrose, 463, 579.
Diamonds, 256, a^j.
wt of the largest,
Dtaspore, 042.
Didymium, atomic weight, 3,
. 4, 549- _, ^
deporttnent with
reagents, 154.
discovered by, a.
discovered in, a.
price of, 556.
specific gravity, 4.
Digitalin, 173.
Dictation of solids, 60a.
Dioptase, 305.
Distearin, 579.
Dolomite, 250, 255.
analyses of, 400.
analysis. 399.
-_jf oils, 180.
site, 465.
Earthy cobalt, 361.
Electricity, 591.
Elements, atomic weight of,
^ »«»«3i4i5.A549.
by Menuelejefi,547.
defunct, 5^.
discovered by, 1-3.
discovered in, 1-3.
dyads, a.
ele
/
iectro-chem. or-
der, 59 1,
equiv. of atoms, i,
hexkds, 3.
monads, i, a.
pentads, a.
price of, 556.
specific heat of, 7.
symbols of, i, s, 3.
table of 549.
table of, I, I, a, 3.
V table of, II, 4, 5, 6.
tetrads, 3.
triads."^,
volatile, 198.
Embolite, 331.
Emetin, 175.
Epidote, 304.
Epsom salts, 590.
Epaomite, 387.
Erbium, atomic weight, 9, 4.
deportment with re-
agents, 1*4.
discovered by, a.
discovered In, 3.
melting-point, 4.
price of, 556.
specific gravity, 4.
Erythrite, 261. 464.
Esparsette, 557.
seed. 560.
Essences, artificial. 579.
Essential oils, i8a.
optical prop, of, xSa.
Essential oils, sp. gr. of, tSa.
Ether, antidote Tor, 594.
specific gravity of, aa6.
Ettcalin, 463, 476.
Eudase, 305,
seed, 569.
Excrement, 542.
Expansion of solids, 60a.
Fahrenheit into Cenitgnde,
Fat oils, i8a
reactions of, 176.
Fatty oil, scheme for, 179.
Feldspar, analyses of, 399.
analysis, 398.
Fern. 559.
Fertilizers, analysis, 403.
Fibrolite, 305.
Filter-paper ash, 370.
Fineness of g^old, 513.
of silver, 5x4.
Fir leaves, 559.
autumn, 560.
Fire-damp, 570.
Flax, entire plant, 559.
fibre, 559.
roUed stems, 559.
seed. 560.
seed hulls, 559.
»Ttiw, 559.
Flour, barley, 558.
rye, 558.
wheat, fine, 558.
Fluorine, at. weight, 5, 549*
before the blow-
pipe, 196.
cnaracteristic reac-
tion, 8.
discovered by, 7.
discovered in, x.
specific gravity, 5.
Fluorite, 350.
Fluxes for soldering. 588.
Fodder, green, aiulyses of
ash, 569, 568.
Franklinite^ 973, 976.
Freezing mixtures, tea.
French nut, 176.
Fruit essences, 575.
sugar, 579.
Fruits, 57«i 5.73i 574i 577* 57«'
acid m, 575.
composition of, 573,
573..S74-
sugar in, 575.
Fruits and seeds ottrees, 560,
565. ,
plants, 565.
Fuels, heating power of, 347.
Fusel oil, 579.
Galactose rotatory power,476.
Galena, special method assay,
Galen'it
jite, 384.
GaUipoU oU, X76.
Gallium discovered by, 553.
discovered in, 593.
melting-point. 5.
specific gravity, 5.
Garnet, 393, 313.
Gases, sp. gr. of, 909.
Gastric juice, 530^ 531.
German sdver, compositkm
of, 587.
Glass, analyses of, 496.
analysis, 495.
Glauber salts, 579.
Glauberite, 395, 396.
Gludnum, atomic weight, a,
S« 549*
deportment with
reag^ents, 154.
letection. sra.
1 by, 9.
dct©
discovered'!
discovered in, 9.
equiv. of atoms, a.
melting-point, 5.
q>ecific £ravity, 5.
specific heat, 7.
Glycerine, 939, 578, 579.
as a solvent, 576.
id amalgam, 970.
at. weight, X, 5, 549.,
before the blo^
«97,
•wpipe.
duumcteristic reaction,
69, 7x.
deportment with re-
agents, 65, xs8.
detection, oo.
discovered by, x.
discovered in, x.
fineness of, 5x3.
minerals of, 970W
native, 970, 97X.
oxides, 65.
parting, 5x9.
price of, 556.
salts, 66.
* spedfic gravity, 5.
specific heat, 7.
Gold and silver, 506W
crucible assay,
scormoation as*
I bullion, 5XX.
Gold coin and I
Golthite, 973.
Gongs, composition of, 587.
Gooseberries, anal, of, 579,
Goslante, 332.
Grains andaeeds of agricul-
tural plants, 560, 564, 5^
568,569.
Grams in U. S. gallon, 409.
Grape must, 559.
seed, s6ck.
skins, 558.
sugar, ^
Grapes, 573.
Graphite, 959.
Grass, down, 5*9.
' 'flof
rye, in i
8^««t, 557.
young, 557:
ifodde
• 557*
Green rodder, analysis of ash,
.560, 5<«.
vitriol, 579.
Grossularite, 303.
Group I, X3*t49.
n, 4a-«43.
Ill, 7a-«44.
V, xa8-X45.
Digiti
ized by Google
INDEX.
619
Gummlte, 997.
Gun-cotton, 58a
Gunpowder, analyses of, 435.
analysis, 434.
Gypsum, 350.
H.
Hsematein, 580.
Halite, 325, jfl6.
Hardness of substances, 350.
scale of, 3SO.
Harmotome, 306.
Hathorn Spring, 4x1.
Hausmanite, 290*
Hauynite, 304.
Hay, analysis of ash, sda, 566,
dead ripe, 557.
meadow, 557.
timothy, 557.
HeMh,559.
Hedenbergite, 303.
Hellebore, antidote for, 597.
Hematite, 973, 377.
analjrsis of, 383.
Hemp, entire plant, 559.
Hemp-seed, 5(0.
oil, 176, X78.
Henlandite, 306.
Hop, entire plant, 559.
Hornblende, 303.
Horsechestnut, 560.
autumn, 56a
spring, 560.
greenbusk,56o.
House bells, composition of,
587.
Hydrobrpmine, 147.
Hydrocarbons from essential
oils, Z83.
optical prop.
of, 183.
sp. gr. of, X83.
Hydrochloric add, 147, 149.
antidote for,
593.
sp. grav. of,
3x9.
Hydrocyanic add, antidote
for, 593.
Hydroferricyanic, 147.
Hydroferrocyanic, 147.
Hydrogen, at weight, x, 549.
discovered by, x.
discovered in, i .
specific eravity ,5.
specific neat, 7.
Hydrometer, Baum6, sp. gr.,
ai4, 915.
Hydrophobia, antidote for,
Hycffozincite, 339.
I.
Ilmenite, analjrses of, 397.
analysis, 397.
India nut oil, 176.
Indium, atomic weight of, 3,
lent with re-
apents,5.
discovered by, 3.
discovered in, 3.
melthig-point, 5.
Indium, price of, 556.
salts of, 91, 94.
specific tntvity, 5.
specific heat, 7.
Inosin. 464.
Insoluble substances, qualW
tative scheme for, 146.
Intestinal juice, 539.
Inverted sugar, 4^1.
rotatory power of,
476.
Iodine, antidote for, 594, 596.
atomicwcieht,i,549.
before the blowpipe,
X96, 900.
discovered by, x.
discovered in, x.
melting-point, 5.
specific heat^ 7.
spedfic gravity, 5.
lodyrite, 3ax.
lohte, 304.
Iridosmine, 979.
Iron, analyses of, 383.
antidote for, 596.
at. weight, 3, 5 549
before the blowpipe,
95, X96, aoo.
cast, analyses of, 386.
cast, analysis, 384.
characteristic reactions,
"3-
chromic, axuil3rsis, 388.
deportment with re-
agents, 87, x69.
detection, X13.
discovered by, 3.
discovered in, 3.
film. 198.
malleable, anftl. of, 386.
melting-point of, 5.
metallic, 90.
minerals of, 973.
native, 973, 974.
ore, appendix to, 381.
ore, quant anal., 373.
ore, assay of, 489.
ore, assavs of, 493.
oxides of, 8. Z 1
pic, anal>-ses of, 384.
price of, 556.
salts, 194. . • /
spedfic graviCv of, 5.
specific neat of, 7.
volumetric determina-
tion of, 379.
Iridium, atomic weight, ^g,
deportment wtth re-
agents, X58.
discovered Dy 3-5.
discovered in, 3-5.
minerals of, 979.
native, 979.
price of, 556.
specific gravity, 5.
JaveUe water, 580.
K.
Kalinite, 249.
Kaolin, 3x6.
KermesUe, 344.
King's yellow, ant for, 595.
Kreasote, 580b
Labradorite,
LADraoome, 304.
Lactose, 4(9, 476, 580.
Lsevuiose, 476, 580.
Lanthanium, atomic weight,
_. a» S» 549- . ^
deportment with
reagents, X58.
discovered by, 9.
discovered in, a.
melting-point, 5.
minerus of, 980.
r I . 1. *P*^- P^vity, 5.
Lapis lazuli, 304, 3x4.
Lard oil, 176.
Lathe busnes, comp. of, 587.
Laumonite, 305.
Laurel water, antidote for.
Lead, antidote for, 596.
assays. 5x4.
at weight, 1, 4, S49.
before the blowpipe,
X96, 900, SOX, 903.
characteristic reaci'ns,
99.
deportment in the re-
agents, 17, 169.
detections of, 37, 43, 7X.
film, X98.
limit of reaction, 99.
meltijw-point, 5, X7.
metallic, xo.
minerals of, 984.
native, 984.
oxides, x8.
pig, analyses of, 39a.
pig, analysis, 390.
price of, 556.
salts. 18, 194.
specific gravity, 5, 17.
specific neat, 7, 17.
Leaves and stems of root
crops, analysis of
ash, 563.
oftrees, 560, 565.
Lentils, 560.
Lepidolite, 386, 304.
Leucine, 580.
Leucite, 304.
Leucopyrite, 973.
Libethenite, 963.
Lignite. 340.
Lime, before the blowpipe,
. »97.
deportment of, 154.
Limonite, 973, 979.
Linnaeite, 961.
Linseed (kke, 559.
oil, X76, X78, X79.
Liquids, official spec, gravity,
93a.
Liroconite, 963.
Litharge, antidote for, 596.
Lithiainlca, 986.
Lithium, at weight, z, ^49.
deportment with r^
agents, X54.
discovered by, 5.
discovered in, 5.
mdting-point, 5.
price of, 556.
specific gravity, 5.
specific neat, 5.
Litter, 559- _, , ^
analysis of ash, 564.
Digiti
ized by Google
INDEX.
Lucerne, S57.
Lupines, 560.
Lymph, 536.
Madkinery betrings, oompo-
«itlooof,587.
Mad doff bite, anu for, 594.
a ou, 178.
— d, 5(So.
Magnesite, 387.
Mafpietic iron ore, 383.
Magnetite, 973, 275.
MagnoriHin, atomic weight,
boore the blow-
nipe, 197.
charactenstic re-
actions, 127.
deportment with
reagents, 124,
16a.
detection, 127.
discovered by, a.
discovered in, a.
melting-point, 5.
minerals, 287.
oxides, 134.
price of, 556.
salts, 125.
spec, gravity, 5.
spec, heat, 7.
Maize, 559, sfci 570.
cobs, 659.
meal, 558.
Malachite, 363-966.
Malaoolite, 30a.
Malleable iron, 386.
cobs, 558.
sprouts, 558.
Malt-sugar, 476, 580.
rotatory power,
476.
Man, analysis of, 5x9.
Manganese, at. wt, 1, 5, 09.
before the blow-
pipe, xia, 196,
a o.
characteristic re-
actions, xxa.
deportment with
reagents, xo6,
detection* 1x3.
determ. of, 379.
discovered by, 3.
discovered in, 3.
melting-point, 5.
metallic, 108.
minerals of. 990.
ore.anal. or, ^5.
oziaes of, lod.
price of, 556.
salts, 109, 194.
spec, gnvity, 5.
Manganlte, S90, aga,
Mannite, 464.
Manufactured product and
refuse, 56}.
Marble, analysis of, 399.
Marcasite. 273.
Marine acid, antidote for, 593.
Marsh gas, 580, 584.
Matches, antidote for, 597.
Measures, French and Amer-
ican, 607.
Meeracliaum, 580.
Melantcrite, 973.
Melexitose, 463.
Melitose, 463, 476.
rotaL power, 476.
Melting-points, tab. of, 4, 5, 6.
Menaccanite, 973.
Mercury, antidote for, 596.
atomic weight, x, 5,
before the blow-
pipe, 96, 30, 197,
900.
characteristic reao-
tions, a6» 30.
deportmen. with re-
agents, 93,38,158.
detection of. 97, da,
discovered by, x.
discovered in, x.
film, X98.
melting-point, 5.
metallic, ar, 95.
minerals of, 994.
Bad ve, 994.
oxides, 99.
price of, 556.
specific gravity, 5.
Metal that expanos on cool-
ing. 585-
analysis of, ^.
Metallic oxides, influence of
fixed organic
substances on
precip., X93.
precip. of, X9^.
Metals, deportment of, with
reagents. 13.
price of, 1:56.
Metalthal expands on cool-
ing, analyns of, 40a.
Meteorites, 973.
Metric sjTstem, 605.
MiUc, analyses of, 459.
analysis,4X7.
camel, 459-
canine, 450.
condensed, 461.
col. woman, 459, 597.
colostrum, ^97.
cow, 459, 4&>.
ewe, 459.
feat, 459.
ippopotamus, 459.
mare, 459.
sow, 459.
white woman, 459, 537.
Milk-sugar, rotatory power,
Mitferite, 99^
Miller's method, ixj.
Millet, analysis of ash, 570.
Hungarian, green, 557.
husked, 560.
meaL, 558.
with husk, cfo.
Mineralogy. 939.
Minretite, 984.
Mirabilite, 3a<.
Molasses, snaJyais of^ 469.
slump, 558.
Molecules, ix.
Molybdenum, atomic weight,
before the blow-
pipe, X96.
deportment with
reagentsu x66.
discovered by, 3.
discovered in, 3.
melting-point, 5.
spec, gravity, 5.
Mon^ standard, 6x4.
Morphia, 580.
Morphin, X73, 174.
Mucus, ^.
Mulbemcs,s73.
Mulberry, 560.
price of, 556.
Muntz metal, comp. of, 587.
Muriatic acid, antidote lor,
Muscovite, 394.
Mustard seed, 560.
Mycose,463.
rotatory power, 476.
N.
Napfath^,^ow
Marcotin, 173, X74, jSa
antidote for, 597.
Native metal and alloys, as-
say of, 513.
Natrolite, 303.
analyses of, 398.
__ ^ analysis, 397.
Natron, 3S5.
Neat's-footoU, X76.
Nephelite, 304.
Nessler's solution, 4x7.
Neurine, 585.
NicooUte, 995, 896, 3CM.
analyses or, 393.
Nickd, atomic weight of, 3, 5,
before <
the blowpipe,
X05, X96.800.
characteristic reac-
tion, 106.
deportment with re-
agents, xoa, x6a.
detection, 1x3.
discovered by, 3.
discovered in, 3.
metallic, un.
mhierals 0^395.
ore, analyses of, 39a.
ore, analysis, 393.
oxides, xoa.
price of, 556.
salts, 103, X94.
specific gravity of, ^
specific Beat o^ 7.
Nlcotin, X73.
antidote for. 597.
Nitrates before the blowpipe,
X97.
Nitre, 30a, 580.
Nitric add, 130.
antidote for, 397.
detection of, aoou
sp. gr. of; aao.
Nitrogen, atomic weight, x.
discovered by, x.
discovered in, x.
specific gravity, ^
specific heat, 7.
Digiti
ized by Google
INDEX.
621
Nitrofflyoerin, 58a
Noo-oryiog otls, i8a
Niu yomioi, 580.
antidote for, 598.
Oak leaves in autumn, 5591
autumn, 560.
summer, 560.
Oats, «59»J^. 570.
neacung out, 557.
in flower, 557.
Official liquids, spec, gravity
of, 333.
Oil, castor, 176.
ood-Uver, 176.
fresh nut, 176.
Gallipoll, X76.
hemp-seed, 176.
neats^oot, 176.
of almonds, 178.
of French (nut), 176.
of lead, Z76.
of olives. 176, X78.
of rue, 585.
of vltru>( antidote
p& rape seed, 176.
poppy, 176.
sesame, 176.
seal, X76b
sperm, 176.
for,
OOsC
train, 179.
tdryinpf),
:8senDal, z8a.
gf;
180.
hydrocarbons of,
183.
optical prop.
of, 183.
sp. rntv* of,
optica] properties
of, i8a.
sp. grav. of, 183.
X x8o.
of, 197.
name ofplant, x8o.
(non-drying), 180.
solidifying point, i80b
specific gravity of^ z8o.
Olefiant gas, 580.
Olevenite, 963.
Oligodase, 304, 31$.
Olive oil, Z76, Z78.
Opal, 30s, 30Q.
Opium, anSdote for, 597.
Oreide, composition or, 587.
Organic analysis, 43Z«
Orpiment, 346, 347.
Orthodase, 304. 3X5<
analy^s, 398.
Osmium, at wt. of, 3, s, 549.
deportment with re-
sgents, z66.
detection, z66.
discovered by, 3.
discovered in, 3.
melting-point, 5.
price of, 556.
specific gravity, 5.
Otaheite cane, 466.
Ouvarovite, 303.
Oxalic acid, zsx.
antidote for, S93*
Oxide, oompositioa of, 585.
Oxygen, atomic weighty a, 5,
avSLble, 589.
discovered by, a.
discovered in, a.
specific gravity, 5.
specific neat, 5.
P.
Pslladium, 870.
wL 3, St 54^ ^
deportment with
reagents, z66.
discovered by, 3.
discovered in, 3.
meltlne-point, 5.
price of, 5<6.
^_^ \iake, 53*.
Psraffin, 580.
Pea, green, hi flower, 557.
Peaches, 574.
Pear, entire Ihdt, 560.
Pearl ash, 580.
Pears, 574. ^
PectoUte, 305.
Peperin, Z75.
Perspiration, 535.
Petalite, 303.
Petroleum, 348.
di8tllUtran'of,349.
strata, 348.
Pettenkoffer's test, 534.
Petzlte, 870.
Pewter, analysis of, 403.
composition of, 587.
PharmaooIHe. 350.
PharmaoopoBial prep., X85.
*' tests of,
Z85.
Phaimaooelderite, S73.
Phenacite, 303.
Phosphates before the blow-
pipe, Z97.
Phoq>horgummite, 397.
Phoephoffic add, zco.
antidote for,
594.
detennination
of, 378,
sp. gr. of, 333.
Phosphorus, ant for, 597.
at weight I, 5.
discovered by, z.
discovered m, z.
melt-point 5.
minerals of, 997.
specinc beat, 5.
Phrenlte, 305.
Picolin, «8s.
Plcrotoun, zts.
Pig iron, analyses of, 386.
analjrsis, 384.
Pig lead, analyses of, 398.
amOysIs, 390.
nne, red, 560.
red autumn, 560.
red leaves, 559.
white, 560.
Pinlte, 465.
Plperin, Z7S.
Plants textile. 564.
Platinum, 556.
Msay, 515.
bef. the olowpipe,
197.
characteristic reac-
tions, 64,71-
deport, with re-
agents, 69, Z58.
detection, 70.
discovered by, 3.
discovered in, 3.
melting-point, 5.
metallic, 63.
minerals, 30a
native, 300.
oxides, 03.
price of, 556.
salts. 63.
specific gravity, 5*
specific heat, 7.
Plum, entire Iruit, 560.
Plums, 573.
Poisons and their antidotes,
Poiybasite, 33Z.
distiU.*oL 349.
strata, 348.
Poppyf5^
ott, 1^76, Z78.
seed, 560.
Porpesite, 370.
PoUble water, analysis of;
4x3.
Potash, antidote for, 590.
Potassa before the blowpipe,
X97.
Potassic hydrate, sp. gr., 330.
Potassium, at. weight, x. 549.
before the blow-
chanctortotic re»
action, X3a
deport With re-
agents, 138, X54.
detection, X37.
discovered oy, i.
discovered in, z.
melting-point, 5.
minerus, wx.
oxides, xa8.
price of, 556.
salts, X39-ZJ4-
specific heat, 7.
anidyses of, 571.
fibre, 557.
Juice. 557.
ridns,557.
Powders, determhiation of
sp. gr., 807.
Printing characters, 587.
anal, of, 40s.
Prochlorite, 306.
Prottstite, 33X.
Prunes, 573.
Prussian blue, 58a
Prussic add, antidote for, 593.
Pseudomalachite, 397.
PsIiomeUne, 390.
Purple of cassius, 580.
Digiti
ized by Google
622
INDEX.
Pus. S39»54o-
Pyrargyrite, 031,383.
Pyrite, 973, 380.
Pyrolusite, 390, 391.
analyses of, 396.
analysis of, 395.
Pyromorphite, 384, 097, 399.
Pyrrhotite, 373,
I^roxene, 303.
Pyroxylin, 580.
QualitatiTe analysis, 13.
for insol. sub.
146.
scheme of, 138,
deter, or substances
by the blowpipe,
•00.
ntitative analysis, 371.
rtx, 303, 306.
uercite, 465.
uickllme, 580.
uinla, 580.
uinidin, 174.
dnin, 174, 175.
R.
Rape, 550.
cake, 557.
green, voung, 557.
seed, 560.
Rape«eeed oil, 176, 178.
Raspberries, 573.
Ratsbane, antidote for, 595.
Raw^ttgar analysis, 479.
Realgar, 346, 347.
Red precipitate, antidote for,
Reduction of compounds, 363.
Reed, 5*9.
Refraction, «89.
Refuse, anaijrsis of ash, 569.
Remingtonite, 361.
Rhodium, at wt, 3, 5, M9.
deport, with re-
agents, z66.
discovered by, 3.
discovered in, 3.
melting-point, 5.
price M, 556.
specific gravity, 5.
Rhodhxm gold, 370.
Rhodochrosite, 390.
Rhodomite, 303.
Rice, analysis of ash, 570.
husked, «6o.
with husk« 560.
Rochelle salts, «£».
Root crops, anal, of ash, 560.
leaves and stems
of, 560.
Roots and tubers, 568.
RosaniUne, 580.
Rotatory power of sugars,
476.
Rubidium, at. wt., x, 5, 549.
deportment with
reagents, 154.
detection, x.
discovered by, x.
discovered in, x.
melting-point, 55.
Rnbidlum, price of, 556.
aptdBc gravity, 5.
specific heal, 5.
Rttdi, S59-
scouring, 559.
Ruta-bagas, 558.
Ruthenium, at. wt., 3, 5, 549*
deportment with
reagents. X54.
discovered in, 3.
discovered by, 3.
melting-point, 5.
price of, 5^.
spec, sravity, 5,
^wcinc heat, 7.
Rye, sfio.
analysis of ash, 570W
flour, 558.
summer, 559.
whiter, 559.
S.
Saccharimetry, 47X.
chemical method,
47"*
mechan. method,
47">
physical method,
Sclieib!
ieibler*8 meth^*
S««harometerr!;7r
Sahlite,jo3.
Salalembroth, 58X.
Salammoniac, 581.
Salenixum, 581.
Sakrem, 583.
Saliva, 529. 530.
Saltpetre, 581.
Salprunella, 581.
Salt cake, 5^1.
of sorrel, 58X.
Salts, deportment o^ widi re-
agents, X3.
old name for, 590.
Scale of hardness, 350.
Scheele's green, 58X.
antidote for,
595*
Scheibler's method, 474.
Scheme for Group 1, 13.
tU» ^'
in, "3.
IV, 137.
V, X37,
for anal, of blood, 447.
for anal of clay. 433.
for anal, of coal, 43X.
for anal, of copper ore,
393*
for anal, of dolomite,
399*
for anal, of fertilisers,
403.
for anal, of glass, 435.
for anal, of gnnpow*
der, 434.
for anal, of llmenlte,
for anal, of Iron ore,
373-
for anal, of milk, m,
for anal, of natrollte,
397*
for anaL of nickel ore,
Scheme for anal, of oithodaae,
for anaL of pyrolusite,
for anaL of silver com,
408.
for anal, of slag, 373.
for anal, of type OMtil,
40X.
for anaL of urine. 450.
for anal, of white kid,
for aioal. of xfaic ore,
394.
for qualitative saaL,
X38, X70.
for blowpipe analyria,
300.
for detection ibrslki-
folds, Z73.
Sdureibersite. 397.
Schweinfiixt green, 58X.
Scorodite, ayx.
Scouring rush, 559.
Seal od, X76W
Sea-weed, 559-
Sebaceous matter, 535.
Seeo, various, oil in, 57^
Seeds and fruits of trees, ^
grains of agnaiW
tuial plants, 56a
Selenium, at wt, 3, 6, «i9L
before the Uow-
diflcovered by. a.
discovered in, s.
films, X98.
meltmg-pohit, 6.
specific aravlty, &
specific neat, 7.
1,543.
Senarmonite, 344.
SepioUte, 306.
Serpentine, 306.
Sesame oil, 176, 178.
Sheathing mctd, oompostloB
of. 587.
Sheelite, asow
Siderite, 373, 383.
Silica bet the blowpipe, 197.
SiUdc acid, 153.
""' - iicwel
atomic weight, 3, &
detection at sooh
discovered by, 3.
discovered in, 3.
minerals, 30a.
specific gravity, 3.
specific Beat 7.
Snvcr, X3.
before the blowpqKi
X7, X96, 197, 3oa
chaiacterist readkaii
deportment with rs"
ageiits, x3. X58.
detection of, 37.
meltiiiff-point, 6, x>
metallic, 14.
oxides of, 13.
minerals oC 3ax.
native, J81.
price oC 556.
spedfic gravity, 6, i>
specific hsat, 7*
Digiti
ized by Google
INDEX.
SQver and gold assay, 494.
assay proper,
cnidble assay,
494*
metb.ofcalcuUt-
ting cbaiiges,
Silver and gold scorlfication
assay, 499.
Slver coin, analyses of, 403.
analysis of, 40a.
Skimmed milk, 460.
Slag, analysis of, 373, 387.
Smaltite, 961.
Smithsonite, 33a, 334.
Soap test, 4x8.
Soapstone, 581.
Soda, antidote for, 596.
nitre, 325.
Sodic hydrate, sp. gravity of,
Solders,388.
U Dubc
i477.
SoleU
I, at. weight, I, 549.
before the blowpipe,
X97.
characteristic reac-
tion, 133.
dsportment with re-
agents, 131, 154.
detection, 137.
discovered by, x.
discovered in, x.
melting-point, 6.
minerals of, 335.
oxides, x3x.
price of, 556.
salts, 13a.
specific sravity, 6.
specific neat, 6b
Solanin, 175.
Soldering, fluxes for, 588.
« .. _ -^
iboscq 8Bocharoi»-
SoUds,' expansion of, 60a.
determination of sp.
gr., ao7, ao8.
dilatation of. 60a.
Solnbillties, table of, 360.
of, notes, 36a,
Solutions, boiling-points, 603.
Soighum, 560.
Sorbin, 464.
rotstory power, 476.
Specific gravity detennina-
tion,ao7.
acetic acid, 331.
ammonic hy-
dnUe, aa7.
Baum^, 3x4,8x5.
ether, aa6.
gases, ao9.
glycerine, 333.
nydrochl. acid,
3x9.
nitric add, a
official Uquid,
phosphor, add,
aa3.
potastic hy<
drate, aa9.
powders, ao7.
iodic hydrate,
930.
•mall solids,
S07.
Specific gr. of solids heavier
than water,
ao8.
sulphuric add,
aas.
Twaddle, 3x5.
vapors, aoo.
Specific heats of compounds,
8. 9, xo.
table of, 7,8,9,
xo.
gravities, Uble of, 4,
5*6.
Speculum, 587.
Spelt, 5SD.
winter, 5<
withhv '
Spelter, jdBi.
Sperm oil, 176.
Spessartite, 303.
Sphalerite, 3^, 333.
Spinel, 887, a88.
Spirits of hartshorn, a&tidoto
for, 596.
Spodamene, 303.
Stennite,j3o.
Stas-otto^ scheme, 179.
Staurolite, 305.
Stearin, 58X.
Steatite, 582.
Stelbite,3o6.
Stephanito, 391, 334.
Stibnite, 344, 345.
Stoichiometry, 353.
Stolzite, 384.
anal. ofash,j63,564,567.
flax, 559>
Stimwberries, anaL of, 57a.
Strontianite, 308, 3^
Strontittm, at. weignt, x, 6.
before the blow-
pipe, 197.
characteristic r^
actions, lax.
deport, with re-
agents, xx8, X54.
detection, 137.
discovered by, x.
discovered in, x.
meltinff-point, 6.
minerus, taB.
price of, 556.
salts, 1x9.
specific gravity, 6.
specific heat, 7.
Strychnia, sfix.
Strychnfaie, X73, 175. ^
antidote for, 598.
Substances absorbed, etc,
543.
Sucrose, 469, 466, 581.
Sugar, 463, 586.
beets, aiuil. of, 47a
Guadaloupe, anal, of,
466.
in fruits, 577.
Martinique, anal, of,
466.
Mauritius, anal, o^ 466.
molasses, anal, of, 469.
ultimate anal, of, 43X
Sugar-cane, 466, 47X.
Sugars, ash determ., 465.
elTect on polarized
liglit, 476.
Sugars, raw, anal, of 479^ 4S0.
rotatory power of,
476.
water determination.
Sulphur, at. wt, a, 6, 5^9.
before the blow-
pipe, X97, aoo.
Sulphur, detection oL X47.
melting-point, 6.
native, 330.
specific gravity, 6.
spedficl
Sulphuric add, X47.
itid<
Sylvanite, sto*
antidote for,
595. ,
sp. gr. of, 395.
T,
Table of ammonia, 135.
, analytical chenL,
X54-169.
city waters, 4ax.
detiinct elements,
554.
cor. in cupellation,
505.
cor. of temperature
in sugars, 48a.
for Duboacq sao-
charometer, 483.
for Ventzke sac-
charometer, 483.
hydrocarbons from
essential oils, 183.
hydrocarl>ons, op-
tical properties
of, X83.
hydrocarbons, sp.
JT, of; X83.
official tests, for
impur. in phar-
macopceial prep-
arations, 185.
oils, x8o.
optical prop, of e»-
sential oils, x8a.
showing the con-
stituents sought.
lofuiu
solubilities, 360.
sp. gr. and weights,
935.
sp. gr. of acetic
add, 93X.
ap. gr. of alcohol,
9x6, 9x7, 9X8.
sp. gr. of ammonia,
937.
sp. gr. of Battm4,
sp. gr. of ether, 8a6.
sp.gr. of glycerine,
339.
sp. gr. of hydro-
chloric add, 3x9.
sp. gr. of nitric
add, 990.
ip.gr. of oils, 189.
sp. gr. of phos-
phoric acid, 993.
sp. gr. of potaasic
hydrate, 990.
sp. gr. of sodk hy-
drate, 930^
Digiti
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INDEX.
b^oi
Table of sp. gr. of sulphuric
acid, »<.
sp. gr. of Twaddle,
9x5.
time at diC places,
613.
volatile elements
that can be re-
duced as films,
X98.
™c, 205,319.
TantaUum, atomic weijjrht,
a, 6.
discovered by, a.
discovered in, a.
melUns-poiat, 6.
price (»', 556.
spec ffraVity, 6.
specific heat, 6.
Tartar emetic, 581.
antidote for, 597.
Tartaric acid, 153.
Tea, analysis ot ash, 569.
Tears, 596.
Teeth, 538.
Telescope minors, 587.
Tellurium, atomic weight, a,
»re the blow-
pipe, Z96.
depoRment with
reagents, x66.
discovered by, a.
discovered in, s.
films, 198.
melting-point, 6.
price or, 556.
specific gravity, 6.
specific heat, 7.
Temper, comp. of, 587.
Temperatures, remarlcable,
60a.
Tennantite, 063.
Tetradymite, 348.
Tetrahedrite, 263.
Textile plants, «59, 564.
Tludlium, atomic weight, i, 6,
549*
deportment with re-
agents, x66.
discovered by x.
discovered In, z.
melting-poiot, 6.
price <«; 556. ^
spadfio gravity, 6.
Thenardite, 385.
Thermometers, 598.
Thorium, atomic weight, 3, 6.
deport, with re-
agents, x<4<
discovered oy 3.
discovered in, 3.
melting-point, 6.
specific gravity, 6.
Time at different places, 013.
Timothy hay, 557.
Tin, assay of, 5«v ,
atomic weight of, 3, 6,
before the blowpipe, 60,
X97, sac.
characteristic reactions,
60.
deport with reagents,
^ 56, 6x, 158.
detection, 7X.
discovered by, 3.
disoovered in, 3.
Thi, equivalent of atoms, 3.
film, Z98.
-point, 6.
minerals, 330.
oxides, 57.
salts, «9, 6x.
spedfic gravity, 6.
specific heat, 7.
Titanic acid, det. of, 377.
Titanite, 305.
Titanium, atomic weight of,
b(»ore the blow-
pipe. X96.
deportment with
reagenta, x66.
discovered by, 3.
discovered in, 3.
melting-point, 6.
ore, amu. of, 397.
price of, 556.
specific gravity, 6.
Toadstools, antidote for, 595.
Tobacco, 5S9.
Toluol, 58Z.
Topaz, ops, 3x8.
Tnurmaline, 304.
Train oil, xtIb.
Trautwhie*8 tables of sp. gr.,
Trehalose, 463.
Tremolite,303.
Triolein, 58X.
Trlpllte. 990^
Tristeailn. 58X.
Tubers, 56B.
pipe, Z96.
deportment with
reagents, x66.
discovered in 3.
disoovered by, x.
melting-point, 0,
specific gravity, 6.
Tumbull*s blue, 580.
Turnip-seed, 5^
Turnips, ^58.
Type and stereotype plates,
587.
metal, analyses of, 40a.
analysis, 40X.
Turquois, 842.
Twaddle, sp. gravity, SZ5.
U.
Ulmanite, 99^.
Ultimate analysis, 431.
Uranium, atomic weight, 3,
before the blow-
pipe, X96.
deportment with
reagents^ x66.
disoovered by, 3.
discovered in, 3.
melting-point, 6.
price w, 556.
Valentinite, 944.
Vanadium, at. wL, 9, 6, S^h.
deportment Whlk
reagents, 158.
isoovered by, 9*
8alta,x94.
specific g
.. gravity, 6.
Urea, 584.
Urine, 540.
•M}^ of, 455* 456.
UeUerVaaalysiit, S4x.
disoovered in, 9.
melting-point, 6^
price of, 5«6.
spMMpa vlty, <w
spednc heat, 7.
Vapors, sp. gravity of; aio.
Veratrin, 179, 175.
Verdigris, antidote for, 596.
Vermilion, antidote for, 596.
Versuvlanlte, 393.
Vetches, 557, 560.
Vivianite.973.
Voktile oements, X9S.
Wad, 990, 993.
Wallastonite, 308.
Walnut, autumn, s6ow
Water aoalyas,' 404!
detection ot, aoow
mineral anal, ct, 4x1.
baiyteftstra»-
ilatai.407.
calculating m-
lodine and btt^
mine in, 409.
iron in, 407.
lithia in, 408,
plioqthoncacid
in, 407.
potable, anal, of, 430,
42X.
potable analysis, Ata.
pot anal., ammooia In,
4x6, 4x9.
nitrates and nl»
ofganic caxboB,
otganlci
soap test, 4xt.
Waterilte, 949.
Weights and measures, 605.
W^ei'nerite, 31H*
Wheat, 359-
analysis of ssh, 590.
bran, M&.
flour, nne, 558.
winter, M9.
winter, heading out,
wmter, in flower, 537.
WUte lead analysis, 400.
metal, 40a, 583.
precipitate, antidoto
for, 596.
Whortlebernes, 573*
Willemite, 303.
Wniiamson^s Dine, 58a.
Wine grounds, 538.
Wood and coal, f ~
oi;33«.
Digiti
ized by Google
INDEX.
625
Wood, analyses of ash, 561,
change of, 339.
darabUity of, 343.
Wolfenite, 384.
Wolframite, 373.
Yyttrium, atomic weight, 3,
.6,549-
deportment with
reagents, 154.
detection, 1^4.
discovered by, 3.
discovered in, s.
melting-point, 6.
specific gravi^, 6.
Zarratite, 395.
Zettnows scheme, 170.
Zinc, analyses of, 395.
at. weight, 3, 6. 549.
before the bion pipe,
87, X97, 300.
blende, anal, of, 305.
char, reactions, xoo.
deportment witn re-
agents, 84, 163.
detection, 1x3.
discovered by, 2.
discovered in, 3.
film, 198.
melting-point, 6.
metallic, 84.
Zinc, minerals, ^.
ore analysis, 394.
oxides, 84.
price of, 556.
salts, 86. 194.
specific gravity, 6.
specific heat of, 7.
Zincite, 333.
Zircon^ 303, 335.
Zirconium, at. weight, 3, 549.
deportment wiu
discovered by, 3.
discovered in, 3.
melting-point, 6.
miner^, 335.
Zylol, 58X.
(({ -
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