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ir.
i
i
i
1
Book of Reactions,
USE OF THE STUDENTS
Chemical Laboratory of Brown University;
JOHN H. APPLETON. A. M.,
Newport-Rogers Professor of Chemistry in Brown University,
Providenu, R. I.
PROVIDENCE :
PRINTED FOR THE AUTHOR BY J. A. * R. A, REID.
1S7&
HAKVARD C0LLE6E llVMAillt
BY EXCHANIIE
FEB 12 1932
Xntered Moordlng to Mt of Congrem, in fhe yew 187(^ by
1 JOHN H. APPLETON,
In the office of fhelilmMrian of OongreM at Wftddngton.
I
i
i
CONTENTS.
-♦-
BOOK I.
CHAP. I. — ^The non-metallic Monads 1
Hydrogen : 1
Chlorine 2
Bromine • 8
Iodine 8
Fluorine. 8
CHAP. II.— The non-metallic Dyads 4
Oxygen 4
Compounds of Oxygen with Hydrogen 4
** " withChlorine 6
Sulphur 6
Compounds of Sulphur with Hydrogen 7
with Oxygen. .1 7
it ((
CHAP. III.— The non-metallic Triads :.. 8
Nitrogen 9
Compounds of Nitrogen with Hydrogen 9
" " with Oxygen 9
Phosphorus 9
Compounds of Phosphorus with Hydrogen 10
" with Oxygen. 10
CHAP. IV.— The non-metallic Tetrads 10
Carbon 10
Compounds of Carbon with Hydrogen 11
" " with Oxygen 11
" " with Sulphur ...12
" '" with Nitrogen 12
Complex Carbon compounds 12
Silicon 15
IV.
BOOK II.
Qualitative Analysis 16
First Group of Metals 16
Their compounds. • . •*. 17
Second Group of Metals 19
Their compounds 21
Third Group of Metals 22
Their compounds 24
Fourth Group of Metals.... ^.26
Their compounds 27
Fifth Group of Metals 27
Their compounds 28
Treatment of metals and alloys 28
The Inorsranic Acids 29
First Group; the Deflagrating acids 29
Second Group; the Efifervescing acids.. 30
Third Group ; the Silver group 31
Fourth Group ; the Barium group 31
Fifth Group; the Mineral acids 33
The Organic Acids 33
Exceptional Oxalates^ Phosphates and Borates 35
Substances insoluble in water and acids. 35
BOOK III.
Quantitative Analysis 37
f Notes on Weights and Measures 37
Notes on the Examples for Practice 38
Aluminum • 38
Ammonium 38
Antimony 39
Arsenic 39
Barium 39
Bismuth 40
Boron 40
Bromine 40
V.
Cadmium • 40
Calcium 40
Carbon 41
Cyanogen 41
Chlorin e 41
Chromium 42
Cobalt ' 42
Copper. 43
Gold 43
Iodine 44
Iron. 44
Lead 44
Magnesium 44
Sulphur 45
Zinc 46
BOOK I. Chapter I.
THE NON-METALLIC MONADS.
Hydrogfen
H
1
(a)
Fluorine
Fl
19
(b)
Chlorine
CI
35.46
Bromine
Br
80
Iodine
I
127
ta
HYDROGEN.
1. Preparation.
2H2O + Nag = 2NaOH + Hg
SHaO + 6Fe = 2Fe304 + SHjj
FeiTOso-fenic oxide
H,SOi + Zn = ZnSOi + H,
2K0H + Mg = K,0,Mg + H,
Potassio-magnesic oxide
2, Properties of Hydrogen.
1 Litre (about 1 quart) of Hydrogen weighs, at 0*^0 and
760 m. m. pressure, .0896 Gm. This weight is called 1 Grith.
1
1 cubic inch of Hydrogen contains the number of molecules
represented by the 23d power of 10 or 10*^, or one hundred
sextillions (100, 000, 000, 000, 000, 000, 000, 000 molecules.)
The mean velocity of the Hydrogen molecule in diffusion, is
6,097 feet per second.
The heat of combustion of Hydrogen is 34,462. One gramme
of Hydrogen, burned in a sufficient quantity of pure Oxygen,
affords heat enough to raise 34,462 grammes of water from
o^ctorc.
CHLORINE.
. 3* Preparation.
Pt CI4 (heated) = Pt 01, + 01,
Plfttlmc chloride Platinous chloride
MnO,+4H01=Cl3+Mn01a+2HgO
ManganouB chloride
MnOj, + 2NaCl + 2H2SO4 = CI, + MnSO, + Na^SO^ + 2H,6
ManganouB sulphate
4« Properties of Chlorine.
Solution of Ohlorine in water yields, when cooled to 0® 0, a
crystalline hydrate, [Ol, + IOH2O]
The heat of Oombustion of Ohlorine in Hydrogen is 23,783
units. • ..
1 Litre of Ohlorine gas under normal conditions weighs
85.46 criths.
SbjSb, + 1001, = 4SbOl6
Antimonic chloride
V'
i
5- Preparation and use of Bleaching-powder, (Calcic hypo-
chlorite and Calcic chloride).
CaO + HgO = CaOgHjj
Quicklime Calcic hydrate or slaked lime
2Ca02Ha + 201, = [CaO^ag -f- CaO J + 2H80
Bleaching powder
LCaO,C3, + CaCas] + 2H,S0. = 2CaS04 + 2H,0 + 2C1,
6. Chlorohydric Acid.
Hg + Clg = 2HC1
A mixture of the gases, explodes when exposed to the sunlight.
NaCl + H3SO, = HCl + HNaSO*
Hydro-sodic sulphate
The molecular weight of HCl is 36.46. The density of the
gas is 18.23. One Litre weighs 18.23 criths.
BROMINE.
7. The liquid boils at 66° C.
The Sp. Gr. of the liquid is 3.1 at 0° C.
IODINE.
8. The Sp. Gr. of solid Iodine is 4.95.
FLUORINE.
9. CaFla + H2SO, = 2HF1 + CaSO*
Fluor spar
SiOa + 4HF1 = SiFl^ + 2H2O
Silicic anhydride Silicic fluoride
(a gas)
BOOK I. Chapter II.
I NON-METALLIC 1
•
DYAl
(a) Oxygen
16
(b) Sulphur S
Selenium Se
Tellurium Te
32
79.4
128
OXYGEN.
10. Preparation of Oxygen.
2HgO (heated) = Hg^ + Og
Mercuric oxide
2KCIO3 (heated) = 2KC1 + 308
Potassic chlorate Pota»sic chloride
2CaO + 2CI2 = 02+ 2CaCl2
The density of Oxygen is 16 ; one Litre weighs 16 criths^
11. Preparation of Ozone, O3.
SKgMn A + 9H2SO4 =
PotasBic per-manganate
3K2SO4 + eMnSOi + 9H2O + 5O3
12. Liberation of Iodine by Ozone, for Schonbein's test^
6KI + O3 + 3H2O = 6K0H + 3I2
Starch (used in this test) is CgHioOs
The density of Ozone is 24 ; one Litre weighs 24 criths^
13* Formation of Water.
H2 + CuO (heated) = Cu + H2O
Cupric oxide
14* Hydrogen peroxide.
Its formula is H2O2 or H — O — O — H
— \
15* Compounds of Oxygen with Chlorine.
ClaO Hypochlorous anhydride
CI2O3 Chlorous anhydride
CI2O4 Chlorine tetroxide
ClgOs Chloric anhydride
ClgOy Perchloric anhydride
16. The Formation and Structure of Acids and Salts Illus*
trated.
CI2O + H2O = 2 (HCIO) Hypochlorous acid
ClgOs + H2O = 2 (HCIO2) Chlorous acid.
ClgOfi + HgO = 2 (HCIO3) Chloric acid.
CI2O7 + H2O = 2 (HCIO4) Per chloric acid.
General formula of a ternary acid, H — D — R (except Haloid
« acids, which are binaries).
+
General formula of a ternary salt, R — D — R (except Haloid
salts, which are binaries).
Example of normal salt, KoSO^ K — O — ) ark
K-0— I ^^«
Example of acid salt, HK SO4 H — O ] csrk
K~0 [ ^^«
Example of basic salt. Plumbic nitro-hydrate, Pb (NOsHO)
(named from analogy of the term base, formerly applied to
hydrates as Pb02H2)
Plumbic nitrate, Pb (NOs) « or Pb"^^;^^"
Plumbic hydrate, Pb02H2 or Pb q -^
Plumbic nitro-hydrate, Pb (NOsHO) or Pb~Q~g^«
Example of Sulphur salts.
K3A8S4, Potassic sulpho-arsenato K — S — )
K— S— f. AsS
K— S— )
(formed after the analogy of
HsAsOa, Arsenic acid
and E3ASO4, Potassic arsenate
6
SULPHUR, SELENIUM AND TELLURIUM.
17* Corresponding Compounds of these Elements.
HgS Sulphuretted hydrogen
HgSe Selenuretted hydrogen
HgTe Telluretted hydrogen
SOg Sulphurous anhydride
Se02 Selenious "
TeO« Tellurous
SO3 Sulphuric anhydride
TeOa Selenic
TeOs Telluric
HgSOs Sulphurous acid
HgSeOs Selenious
HgTeOs Tellurous
((
t*
H2SO4 Sulphuric acid
HgSeO* Selenic ''
H2Te04 Telluric "
K2SO3 Potassic sulphite
KgSeOs *' selenite
K2Te08 " tellurite
K2SO4 Potassic sulphate
K2Se04 '* selenate
KsTeO^ " teUurate
SULPHUR.
18. Its Mineral Forms.
Iron pyrites, FeS2, Fe <
Copper pyrites, FeCuSg
— S
-I
Galena, PbS
Zinc blende, (called Black-jack) ZnS
Silver glance, AggS
19* Preparation of Sulphydric Acid (H^S)
FeS + H2SO4 = H2S -r FeSO^
Ferrous sulphide Ferrous sulphate
SbgSs + 6HC1 = 3H2S + 2Sb2Cl3
Antimonious sulphide
HjSg is Hydrogen persulphide, H — S — S — H
20. Sulphurous and Sulphuric Oxides.
S + Og = SO2 Sulphurous anhydride.
Cu + 2H2SO4 = SO2 + CuSOi + 2H2O
Hg + 2H2SO4 = SO2 + HgSOi + 2H2O
C + 2H2SO, = 2SO2 + CO2 + 2H2O
502 + H2O = H2SO3
Sulphurous acid
503 + 2K0H = K2SO3 + H2O
Potassic sulphite
SO3 + H2O = H2SO4
21. List of the Oxygen Acids of Sulphur.
[Hyposulphurous anhy-
dride SO] ;
(hypothetical)
Sulphurous anhydride SO2;
Sulphuric anhydride SO3 ;
[Sulpho-sulphuric anhy-
dride SO2S];
(hypothetical)
Hyposulphurous acid H^SOg
(also called Hydroaulphurous acid)
Sulphurous acid HgSOj
Sulphuric acid HgSO*
~0 } ®^»
H—
H
Sulpho-sulphuric acid H2SO3S
(also called Hyposulphurous acid)
H—
H
s}so.
8
Nordhausen eulphuric add
(H,SO« + SO,)
Diibionic acid H2S2OS
Trithionic acid HgSsOj
Tetrathionic acid HgS^Oft
Pentathionic acid HsSsO^
BOOK I. Chapter III.
THE NON-METALLIC TRIADS.
22. (a) Nitrogen
N
(b) Phosphorus P
Arsenic As
Antimony Sb
14
31
75
122
23. Corresponding Compounds of these Elements.
HsN Ammonia gas
HjP Phosphoretted hydrogen
HsAs Arseniuretted hydrogen
HjSb 4JitiD^oniuretted hydrogen
NjOs Nitrous anhydride
PjOs Phosphorous**
AsjOs Arsenious "
SbgOs Antimonious"
HNO2 Nitrous acid
HjPOs Phosphorous "
HsAsOs Arsenious "
HSbOs Antimonious "
NgOs Nitric anhydride
PgOfi Phosphoric
AsgOs Arsenic
SbsOs Antimonic
((
t(
t€
HNOa Nitric acid
H3PO4 Phosphoric
HsAsOa Arsenic
HSbOs Antimonic
tt
(C
C(
9
NITROGEN.
24* Preparation of Nitrogen.
8NH3 + 3CI2 = GNH,C1 + N2
(there is danger of forming the explosive NCI3)
25* Compounds of Nitrogen with Hydrogen.
NH2, Amidogen (hypothetical)
NHs, Ammonia gas
NH4, Ammonium (hypothetical)
Phenyl, (CeHg) forms Phenyl-amine (CeHg)— N = Hg
Acetyl, (C2H8O) forms Acet-amide (C2H3O) — N = H2
NH3 (gas) + HCl (gas) = NH^Cl (solid)
Na^Hg, + r (NH.Cl) = (NH,)rHg, + rNaCl
Sodium amalgam Ammonium amalgam
26. Compounds *of Nitrogen with Oxygen.
NgO Nitrogen protoxide (laughing gas)
NO or N2O2 Nitrogen dioxide
N2O3 Nitrous anhydride
NO2 or N3O4 Nitrogen tetroxide (brown fumes)
N2O6 Nitric anhydride.
27* Aqua regia.
(Typical reaction) 2HNO3 + 2HC1 = CI2 + N2O4 + 2H2O
PHOSPHORUS.
28. Preparation of Phosphorus.
First Stage, Cag (P0,)2 + 2H2SO4 = H^Ca (PO^g + 2CaS04
Bone ash Hydro-calcic phosphate
Second Stage, H^Ca (PO^g heated = Ca (P03)2 + 2H2O
Third Stage, 3[Ca(P08)2] + 10 C = P* +Ca3 (P0,)2 + 10 CO
10
29« Preparation and Combustion of Phosphoretted Hydrog^en.
P* + 3NaOH + 3H,0 = H,P + 3 (H,NaPO,)
Hydro-sodic hypophoephite
H3P + 20, = H3PO4
30. Compound of Phosphorus with Oxygen.
PjOs, Phosphorous anhydride
PA, Phosphoric ''
(€
(C
HsPOg Hypophosphorous acid
H3PO3 Phosphorous
H3PO4 Phosphoric
HPO3 Metaphosphoric acid
H4P2O7 Pyrophosphoric "
BOOK I. Chapter IV.
NON-METALLIC TETRADS,
31. (a), Carbon
(b), Silicon
Titanium
Tiu
c
12
Si
28
Ti
60
Sn
118
32. Corresponding Compounds of these Elements.
CO2 Carbonic anhydride
SiOa Silicic
TiOg Titanic "
SnOg Stannic
H2CO3 Carbonic acid
H2Si03 Silicic
H2Ti03 Titanic
H2Sn03 Stannic
11
33* Compounds of Carbon
with Hydrog^en.
1st Series, The Paraffines,
Cntl2n+2-
Marsh gas CH^
2d Series, The Olefines,
CnHan-
Ethylene CjH^
3d Series, The Acetylenes,
Cntl2n_2'
Acetylene CgHg
4th Series, The Terpenes,
CnH2n_4.
Turpentine CioUis
6th Series, The Benzenes,
CnHgn-*-
Benzene CcH^
6th Series, PhenyJene, *
CnH2n_8.
Phenylene CeH^
T^Vk Cf^-M'^^n
Cnlign— 10-
8th Series, Naphthalene,
^n^ia—lZ'
Naphthalene CioHg
Ofh ^nri rn
CnHgn-u-
Di-phenyl CigHio
10th Series, Stilbene,
^vPia-W
Stilbene CuHu
11th Series, Anthracene,
^n^Zn-lS'
Anthracene CuTTio
12th Series, Wanting,
13th Series, Pyrene,
^n-"8n— 28*
Pyrene C„Hio
14th Series, Chrysene,
CnHgn— 84-
Chrysene Ci^Hia
34* Preparation of Carbonous Oxide, GO.
By heating Formic acid with concentrated HgSO^, the former
Isplits up as follows :
H0(CH0)=C0 + H20
By heating Oxalic acid with concentrated H^SO^, the former
splits up as follows :
HjOjCCaOa) = CO + COgHjO
K^CeNeFe + GHaSO* + 6H2O
PotoBrioferro cyanide = 6C0 + 2K2SO4 + 3 (NHOjjSO* + FeSO^
35- Preparation of Carbonic Oxide, COg
. c + o,= co,
CaCO, (heated) =COs + CaO
CaCO, + 2HC1 = CO, + CaCl,
CO, + CaO = CaCO,
12
3^* Reactions of Carbon with Sulphur.
C (heated) + S^ (vapor) = CS^
Carbonic disulphide
CS, + (NHOaS = (NH,),CS,
Amnionic sulpho-carbonate
(NH4)2CS3 + 2HC1 = 2NH,C1 + H^CSg
Sulpho carbonic acid
CSg + SOg = CO2 + 2SO2
37* Reactions of Compounds of Carbon with Nitrogen.
HgCya (heated) = Hg + Cy^
Mercuric cyanide Cyanogen
/// ///
Cyanogen Cyg = CN— CN
Cy3 + K, = 2KCy
HgCy, + H,S = HgS + 2HGy
Cyanohydric add
HOCy, Cyanic acid
KOCy, Potassic cyanate
KSCy, Potassic sulphocyanate
38- Complex Carbon Compounds.
+
B, represents one molecule of an electro-positive radicle. It
may be either simple or compound. When compound, it is
usually made up of Carbon and Hydrogen.
R, represents one molecule of an electro-negative radicle. It
may be either simple or compound. When compound, it is
usually made up of Carbon, Hydrogen and Oxygen.
D, represents one atom of a linking dyad. It is usually
Oxygen.
M, represents one atom of a monad metal.
13
ist Type, H— H. The Hydrogen-gas Type.
± ±
The general formula is R — K.
Examples.
R— R Positive radicle CHs— CHj Methyl,
,R R Negative radicle CaHsO—CgHsO Acetyl,
R— H Hydride
R— H Aldehyd
f+
R— CI Haloid ether
W—Ci Acidhalide
CHs— H Methyl hydride (marsh-
CgHsO—H Acetic Aldehyd,
C2H5— CI Ethyl-Chlorhydric-ether
or Ethyl-chloride '^
CsHsO— CI Acetyl-chloride.
2d Type, H»0, or H— O— H, The Water Type.
± ±
The general formula is B — ^D — K.
Examples.
R— O— R Simple ether CgHg— O— CgHs Ethylic ether.
' I
<
•-t
Mixed ether
CHs— O— CjHg Methyl-ethyl ether
5— O— R Anhydride C2HSO— O— CgHst) Acetic anhydride,
R— O— R Compound ether CgHg— O— CjHsO Ethyl-acetic ether,
^-O— H Alcohol C2H5— O— H Ethyl alcohol,
R—S— H Mercaptan QJH5— S— H Ethyl sulpho-hydrate,
,— Se— H Seleno-mercaptan CaHs— Se— H Ethyl seleno-hydrate,
H— O— R Acid • H— O— CjHsO Acetic acid,
M— 0— R Salt Na— O— CgHsO Sodlc acetate.
it
14
3d Type, H^N, The Ammonia-gas Type.
R— As
Hs Amine,
=H8 Arsine,
Ha Stibine,
Ha Phosphine,
B— ]Sr=Ha Amide
B— N
^Alkalamide,
-H
Examples.
CgHs— N=H2 Ethyl-amine,
(CH3)3A8 Tri-methyl-arsine,
(C2H6)sSb Tri-ethyl-stibene,
CjHs— P=H8 Ethyl-phosphine,
CaHsO— N=H8 Acet>-amide,
CaHg— NZ^^'^ Ethyl-acet-amide,
„_0-H
_jr Amicacid, (C4H402)"_jx_g Succin-amic acid
4th, Type, H^C, The Marsh-gas Type.
Example.
0=C=ER Ketone, 0=C==(CH8)2 Ordinary acetone (methyl-acetyl)
5th Type, NH4CI, Ammonium-chloride Type.
Examples.
51=p— (
Cl Ammonium subs, comps. (CzEU)4=N — 01 Ethyl-ammo-
nium chloride,
•01 Phosphonium subs.comp8.(OH8)4=P— 01 Tetrarmethyl
phosphonium chloride.
E^As— 01 Arsonium substitution compounds.
Bi=Sb—
01 Stibonium substitution compounds.
6th, Type, Organo-metallic Bodies.
5i=Zn
ii^Sn
Examples.
(02H5)8Zn
(OgBt)* Sn
Zinc ethide
Stannic tetr-ethide.
15
SILICON.
SiH^, Silicic hydride
SiPl^ " fluoride
SiCl* " chloride
SiBr^ ** bromide
Sii; " iodide
BOOK II.
QUALITATIVE ANALYSIS.
FIRST GROUP OF METALS.
Lead, Silver and Mercury in the Mercnrous form.
39. AgNO, ) AgCn
Pb(NO,), f- + 5HC1 = PbCl, [ + 5HN0,
Hg,(NO,),) Hg.C!l,)
40. PbCl, + H;iS04 = PbSO« + 2Ha
2PbCl, + K,Cr,0, + H,0 = 2PbCr04 + 2Ka + 2HC31
PbCl, + (NH^)^ = PbS + 2NH4CI
PbS + K,CO, + C = Pb + K^ + CO, + CX)'
41. Aga l+NH40H=[Aga.+ NH«0H]
Hg,Cl, ) -j- 2(NH.0H = (NH,Hg,)Cl + NH*C1 + 2H,0
Amido-mercurous chloride
H—
17
H—
H—
(NH^,)a — Hg— i-N— a
U
42. [ AgOl + NH4OH] + HNO, = AgCl + NH4NO, + H,0
2Aga + K8C084- C = AgaH- 2KC1 + CO, + CO
43. 2HNOs + 2Ha = Cl, + NA + 2H,0
2[NH,Hg,Cl] + IOHNO5 + 6HC1 =
4HgCl, + 10H,O + 5NA + N,
8Cu + SHNOs = 3Cu(NOs)8 + NA + 4H,0
N20, + 0, = NA
CuCu + HgClg == CuHg + CuCl,
COMPOUNDS OF FIRST GROUP METALS.
44. SILVER.
There are three compounds with oxygen.
Argentous oxide Ag^O
Argentic oxide Ag20
Argentic peroxide AgA
45- LEAD.
Litharge, Plumbic oxide PbO
(\
Plattnerite, Plumbic dioxide PbO,, Pb~Q
2*
18
Red lead, Di-plumbic trioxide PbjOj, Pb_o_P''=0
<(
U
Tri-plumbic tetroxide PbsO^, p^~q'~ I Pb
Tetra-plumbic pentoxide Pb^Og, Pb — — '
I
o
^Pb
Pb— O—
Pb=0,=
White lead, Tri-plambic di-hydric carbonate
Pb,H,(CO
Pb
*^» Pb=0,= I C
l-o )
=0,= ^
-0 j
Pb=0.==5.C
H-
Galena, Plumbic sulphide PbS
Sugar of Lead, Plumbic acetate, PbOgA^
( = 0.
f_0_CJ — c =
|_-0— C ( — c =
1 =
46. MERCURY.
Calomel, Mercurous chloride HgaClg
Corrosive sublimafe, Mercuric chloride HgClg
Black precipitate, Amido-mercurous chloride (NH2Hg2)Cl
White precipitate, Amido-mercuric chloride (NH2Hg)Cl
Cinnabar also Vermilion, Mercuric sulphide HgS
19
SECOND GROUP OF METALS.
47. The effect of diluting the solution with water.
SbCl, + H,0 + Aq = SbOCl + 2HC1 + Aq
BiCl, + H,0 + Aq = BiOCl + 2HC1 + Aq
48. Preparation etc. of the Sulph.Tdric gas.
FeS + HjSO^ = H,S + FeSO,
H,S + 2HN0j = S + NA + 2H,0
49. Precipitation of the whole Group.
2A8C1, )
2SbClj y + 7HS = Sb,S, )■ + 14HC1
SnCa, )
Cn(NO,), "1 CuS 1
2BiOCl I I fiTT o _ Bi A
Hg(NO,), f-|-*'^^-HgS
Cd^NO,), J CdS
+6HN0, + 2HC1 + 2H,0
50. Treatment of the members of the First Division.
Ab,S, ) 2[(NH4),A8SJ
Sb,S, [ + 7(NH,)A = 2|.(NH0,SbSJ + S,
SnS ) (NH4),SnSs
2[(NH,),A8SJ ) As,S,
2[(NH.'isSbS4] } + 14HC1 = Sb^
(NH,),SnS, ) SnS,
+7H,S + l^NH^a
51. A8.S. + (NH.),CO, = [As,S, + (NH0,CO,]
[As A + (NHOsCO,] + 2HC1 = Ae A + CO, + 2NH4CI + H,0
20
Sb + 4HN0, = HSbO, + NA + NA + H,0
HSbOs + [H4O4T] =
H, SbO _
L H,
+ h;,o + o
53. Sn + 2HC1 = SnCl, + H,
SnCl, + 2HgCl, = HgjCl, + SnCl^
(Na,BA + lOHjO) heated = Na,BA + 10H,O
Crystallized borax Borax glass Steam
NagB A + CuSO* = l^a^CuB A + SO,
2(Na8CuBA) + Sn = SnO + CugO + 2(Na8BA)
54. Treatment of the members of the Third Division.
Cus 1 Cucij ^
g«| I + 12HC1 + 12HN0, = ^JgJ^ I + 6S+6NA + 1^W>
CdS J CdCla J
The test for Mercury.
HgClg + CuCu = CuHg + CuClg
CuClgl +2NH,0H Cii(NH3)2Cla + 2H,0
2BiCl-
CdCl
2 J
6NH,0H=:BiA+ 6NH4CI + 3BJ0
HgClI f + 2NH4OH NHgHgCl + NH4CI +'2H20
+ 3NH,0H = [CdOgHg + NH^OH] +2NH4a
which dissolves 4
(in excess of Ammonia)
The test for Bismuth.
Bi A + 6HC1 = 2BiCl8 + SBfi
BiCls + H2O + Aq = BiOCl + 2HC1 + Aq
2BiOCl + K2CO3 + 20 = 2Bi + 2KC1 + 200^ + CO
I
21
[CdOaHj + NH^OH] ) + ^^^ ~ ^ ^^^® solution is decolorized)
The test for Copper.
Chi(NH3),Clg + 2H0l = CuCle + 2(NH40A)
2CuCl2 + K^FeCy. = CuaFeCy, + 4KC1
COMPOUNDS OF SECOND GROUP METALS.
55, ARSENIC.
Wliite Arsenic, Arsenious anhydride, Asfi^
^' Orpiment, Arsenious sulphide, As^Ss
Sclieele's Green, Hydro-cupric arsenite, HCuAsO,
Arsenate of Soda, Sodic arsenate, NasAsO^ -{- 12H20
or Hydro di-sodic arsenate, HNagAsO^ -|- I2H2O
56. ANTIMONY.
K SbO >
Tartar-emetic, Potassioantimonylic tartrate, ' ^ ^©^(CiHjOj)
57- TIN.
Tin Crystals, Stannous chloride SnClg + 2H2O
Stannate of Soda, Sodic stanuate NasSnOs
58. COPPER.
Red oxide of Copper, Cuprous oxide Cu^O
Black oxide of Copper, Cupric oxide CuO
Copper glance, ' Cuprous sulphide CujS
Blue vitriol, Cupric sulphate, CuSO^ + 5H,0
59- BISMUTH.
Nitrate of Biamuth, Bismathoos nitrate Bi(NOs),
Baaic nitrate of Biamntli, BiBmntli^I nitrate (BiO)KO(
Bismatliyl carboDate (2BiO)CO,
Pearl white, Bismutbf 1 ehloride (BiO)Cl
60. MERCURY.
See oomponude of First Group metals.
61. CADMIUM.
Iodide of Cadmiam.
OdI,
62. THIRD GROUP OF METALS.
Co(NO,),
Ni(NO,),
Fe.(NO.),
2M11SO,
Cr^O.).
Zii(NO,),
A1,(N0,),
NiO,H, ; ''iiSiJ
Fe,O.H, +i!4NH,N0,
+ 28NH,OH = 2MeO,H, [
Cr,0,H. +2(NH0,BO,
ZdO^,
AI,0,H, J
A1,0,H, J
CoS 1
NiS
2Fe3 I
+ 8(NH,),S= 2M11S |-+16HH,0H+S
Cr,0,H,
ZqS
A1,0A
23
CoS 1
NiS
■jT-a y unchanged
2FeS
2FeCl8 ")
2Mna
• + 22HC1 = 2MnCl, + 5H^ + 12H,0
CrAH,
CrjCl,
►
ZnS
ZnCl»
AlAH, J
A],C1. J
63. Treatment of Cobalt and Nickel.
CoS + Na,BA + O, = Na,CoB A + SO,
NiS + NaJBA + O, = Na,NiBA + SOj
2NiS } + ^^^^ + ®^^^» = kS } + ^ + 8H,0 + 4NA
I
The yellow Cobalt precipitate, CoA(NA) + 6KNO5
NiClg + 2NaOH = NiO^H^ + 2NaCl
64. Treatment of the Second and Third Divisions of this
group.
2FeCl2
2MnCls
Oracle
ZnClg
2Fe02H2
2Mn02Hg
y + 22NaOH = Cr AHe 5^ +22Naa
ZnOsjHg I
AlAHe J
The same, after boiling with excess of NaOH and free access
of air.
2FeOaH8
2Mn08Ha
CrAH,
ZnOgHj,
Ai,oja.
Fe,0,H,
Mn,0,H,
+ 4NaOH + O, = CrAH, + 4H,0
Na^ZnO,
NMJ«0*
24
65. Treatment of the Second Division (Iron, Manganese
and Chrominm).
2K,FeOt ) +9H,0 +
+ 6KN0, + 4K,C0, = 2K,Mn04 }■ SCO, + 3N,0,
2K,CrO, ) +K.CO,
Bj boiling the solid products of the foregoing, in water
( 2K,Fe04 + 2H2O = Fe A + 4K0H + 30
^ 3K,Mn04 + 2Hj50 = KgMn A + MnOg + 4K0H
( 2K8Cr04 + Aq = 2X8010* + Aq (unchanged)
The tests for Iron.
FcgOs + 6HC1 = FegOle + SH^O
FejOle + 6KS0y = Fe,S,Oje + 6K01
2(Fe,Cl«) + 3K,(FeOj,) = Fe,(FeO je)8 + 12K01
The tests for Ohromium.
KjCOa + 2(H008H30) = OOg + 2(K0A) + H^O
Acetio acid
KjCrO* + PbOjA, = PbCi O4 + 2(K0A)
Plumbic acetate
66. Treatment of the Third Divisioti (Zinc and Aluminum).
(NajAl A + NajS) + lOHCl = AlgOl. + 4NaCl + HgS+fflgO
Na,ZnOs
Na.
COMPOUNDS OF THIRD GROUP METALS.
67. COBALT.
Nitrate of Cobalt. Oobaltous nitrate Co(NOs)8 -{- BUfi
25
68. NICKEL.
Kupfer-nickel, Nickel arsenide NijiAs,
Double Sulphate of ] Ammonio-nick- C (NH4)8S04,NiS04 + '
Nickel and ammonia ) eioas sulphate ( 6HsO
69. IRON.
Iron pyrites, Iron sulphide, FeS,
Copperas or green vitriol. Ferrous sulphate, FeSO^-f-THnO
70. MANGANESE.
Pyrolusite, Manganese di-oxide, MnOg
Permang^anate of Potash, Potassic permanganate, K^Mnfi^
Bi-chrome,
Chrome-yellow,
71. CHROMIUM.
Potassic di-chromate
i^lumbic chromate
K,CrA
PbCrO^
White vitriol,
Zinc white,
72. ZINC.
Zinc sulphate
Zinc oxide
ZnS04+ 7H,0
ZnO
73. ALUMINUM.
Alum, Ammonio-aluminic sulphate (NH4)2S0^A1,(S04)«
+24H,0
Concentrated Alnm, Aluminic sulphate, A1,(S04)8 + 18HsO
Red Liquor,
3
Aluminic acetate, Alfi^A^
26
FOURTH GROUP OF METALS.
74. [MgCl, + NH,C1= (NH,)MgCl,]
Ba(NO,),) BaCO, )
Sr(NO,), [ + 3(NH.),C0, = SrCO, }■ + 6NH4NO,
Ca(NO,), ) CaCO, )
75. BaCO, ) BaCl,
SrCO, } + 6HC1 = Si CI, + SCO, +3H,0
CaCO, ) CaCl,
The Test for Barium.
76. BaCl, + CaSO, = BaSO^ + CaCl,
CaCl, ) CaSO* )
SrCl, y + 3H,S04 = SrSO, [ + 6HC1
[BaCy ) [BaSOJ )
77. CaSOi ) CaCO,
SrSO* }■ +2Na,CO,+K,S04 = SrC0H-2Na,S0.+K,S0«
[BaSOJ) . [BaS0«]
ggg;} +4Ha = gg + 2CO. + 2H.O
78. First portion ; the test for Strontium.
SrCl, + CaSO* = SrSO* (the precipitate)
CaCl, 2CaCl8
Second portion ;
79. The test for Calcium.
CaSO/+(NH^,CA = CaCA + (NH«),SO,
27
COMPOUNDS OF FOURTH GROUP METALS.
Witherite,
Heavy spar,
Muriate of baryta,
80. BARIUM.
Baric peroxide,
Baric carbonate,
Baric sulphate.
Baric chloride,
81. STRONTIUM.
Strontic peroxide,
Strontic carbonate,
Strontic sulphate.
Strontianite,
Celestine,
Muriate of strontia, Strontic chloride,
Quicklime,
82. CALCIUM.
Calcic oxide.
Calcic peroxide.
Chalk, marble, lime-l ^^^^^^ carbonate
stone, etc., )
Gypsum, Calcic sulphate.
Bone, largely Calcic phosphate, Csiz(^0^\
nunnhif^rr r.r.r„A^. I ^^^^^^ hypochlorite CuClA +
Bleaching powder, | with Calcic chloride, CaCl,
BaOa
BaCOs
BaSO^
BaClg +2H80
SrO,
SrCOs
SrSO*
SiCla
CaO
CaOa
CaCOg
CaS04 + 2H80
THE FIFTH GROUP OF METALS.
83. The tests for Ammonium.
NH,C1 + NaOH = NH, + NaCl + H^O
NH3 + HCl = NH,C1
NH4CI + PtCla = (NBy^PtCl.
84. The test for Magnesium.
(NH4)MgCl8+ NH4OH + HNagPO, =
(NHOMgPO^ + 2NaCl + NH,C1 + HgO
85. The test for Potassium.
2KC1 + PtCl^ = KjjPtCl^
28
COMPOUNDS OF FIFTH GROUP METALS.
86. AMMONIUM.
Sal-ammoniac, Ammonic chloride, NH^Cl
Ammonia, Ammonic hydrate, (NR^)0'H.
87. MAGNESIUM.
Magnesia, Magnesic hydrate and carbonatejM^OaH^-f-MgCOs
Epsom salts, Magnesic sulphate, MgSO^
88. POTASSIUM.
Caustic potash, Pbtassic hydrate, KOH
Pearl ash or Sal tartar* Potassic carbonate, E«COs
Cream ofvtartar, Hydro-potassic tartrate, (HKH,)04(C4H,0,)
Saltpeter, Potassic nitrate, KNO,
89. SODIUM.
Common salt, Sodic chloride, NaCl
Caustic soda or Soda by lime, Sodic hydrate, NaOH
Soda ash, Sodic carbonate, NagCOs
Soda or Sal soda) Sodic carbonate, crystallized, Na,C08 +
or Soda Crystals, ) • lOH^O
Glauber's salt, Sodic sulphate, NagSO^
Chili saltpeter, Sodic nitrate, NaNOs
THE TREATMENT OF METALS AND
ALLOYS.
Class First.
90. 4Zn+10HNO8+Aq=4Zn(NOs)8+N,O+5H8O+Aq
3Cu + SHNOs + Aq = SCaCNOs), + N A + ^H,0 + Aq
29
Class Second.
5Sn + 20HNOs = Hi,Sd,0„ + 10NA+ 5F,0
Sb + 4HN0, = HSbO, + N ,0, + N A + H,0
^'' ^fbof"* } + 25HC1 = It^^^ } + 18H,0
Class Third.
J^ } + 8HC1 + 8HNOs = JJ^^J^ } + CI + 4N,0, + 8H«0
92. SnCla + FegCle = SnC]* + 2FeC^2
Fen io chloride Ferrous chloride
PtCl* -h 2NH4CI = (N HOsPtCJ.
THE INORGANIC ACIDS.
FIRST GROUP OF ACIDS— The Deflagrating
Acids.
Nitric acid HNOs
93. 2KNO3 + C (heated) = K2CO3 + N A
TFeSO^ + 3H2SO4 + 2HNO3 = FeSO^NA + SFcgCSOOs +
* Ferrous-nitro-Biilphftte 4-T? Q
CHjNO + 0= CH^O,
Indigo-blue Isatin
Picric acid is Tri-nitro phenyl-alcohol, C«H6(N02)3 — O — ^H
CHLORIC ACID, HCIO3
94. 2KCIO3 + 3C (heated) = 2KC1 + SCOg
KClOs (heated) = KCl + O,
KCl + AgNOs = AgCl + KNO3
3*
30
SECOND GROUP OF ACIDS— The Effervesdna:
Acids.
95. (a) K,CO, + 2HNO,=-CO, + 2KNO,+H,0
(b) (in dilate solutions)
K^ + 2HN0, + Aq = H^ + 2KN0, + i^O + Aq
(in concentrated solutions)
K;S + 4HN0, =! S 4- 2KN0, + NA + 2H,0
(c) (in dilate solutions)
K,SO, + 2HN0, + Aq = 2KN0, + SO, + H,0 + Aq
(in concentrated solutions)
K,SO, + 2HN0, = K|SO« + N A + H,0
(d) 2KI + 4HNO, = I,+ 2KNO, + NA + 2H,0
(e) Na,SiO, + 2HN0, = H,SiO, + 2NaN0,
KSbO, + HNO, = HSbO, + KNO,
96. CARBONIC ACID, H,CO(
CO, + CaO,H, = CaCO, + H,0
97. SULPHYDRIC ACID, H,S
PeS + H,SO, = H^S + FeSO«
PbO,A, + 2NaOH = PbO A + 2NaOA
PbOA + H,S = PbS + 2H,0
98. SULPHUROUS ACID, QiSO,
ZZa+ 4H,S0«+Na,S0, =H,^4-Na,SO«+3ZnSO,+3H,0
K,SO, + 2HN0, = K,SO« + N,04 + H,0
K,SO« + BaCa, = BaSO» + 2KC1 '
31
THIRD GROUP OF ACIDS— The Silver Group.
90. Ka ) AgCl .
KI ^+3AgN0, = AgI +3KN0,
KCN ) AgCaSf
2AgCN (heated) = Ag + CN + (AgCN)
P*racyanide of silver
AgCl+Zn + H^0« = Ag + HCl + H + ZnSO«
HCa + AgNO, = AgCl + HNO,
100. 18K0y. + 3FeCn, + 2Fe,Cl, = 2Fe,(FeOy,), + 18KCa
Ferric ferro-oyaiiide
PeO, + Fe,Cl, + 8NaOH = FeHA + Fe.O.H. + SNaa
FeHA + Fe,H,0, + 8HC1 = FeC3, + Pe,a, + 8H,0
FOURTH GROUP OF ACIDS— The Barium Group.
100. 1— Na,SO* + BaCl, =BaS0,+ 2NaCl
2— Na^^O, + BaCl, = BaSO, + 2NaCl
Na,CO, + BaCla = BaCO, + 2Naa
3— NagCaO* + BaCl, = BaC A + SNaQ
2(Na3PO,) + 3BaCa, = Bas(P0,)2 + 6NaCl
Na,CrO, + BaCl, = BaCrO* + 2NaCl
Na,BA + BaCl, = Baric borate (^TJSSS?")
Potaasio tartrate *
H } 0« I C.H,0, + BaCl, = Baric citrate CSSSSaD
Potaasio citrate
32
lOI. OXALIC ACID, HA(CA) or HjCgO*
(NHO AO4 + CaCla + = CaCA + 2NH4CI
CaCA (heated) = CaCO, + CO
CaCOs + 2HC1 = CO, + CaC), + H,0
102. PHOSPHORIC ACID, H5PO4
2(HNa,PO0 + Fe,C1e + Aq = Fe^CPO,), + 4Naa +
2HC1 + Aq
NH4OH + HOA = NH,OT+ H,0
Ammonic molybdate is (NH4)2Mo04
103. Phosphoric anhydride, PA ; Phosphoric acid, HjPO^
Meta-phosphoric acid, HPOs
Pyro-phosphoric acid, H^PjOy
Phosphorous anhydride, PgOs ; Phosphorous acid, HsPOj
Hypo-phosphorous acid, H^O^
104. CHROMIC ACID, HsCiOa
KgCr A + 2Pba + HgO = 2PbCr04 + 2KC1 + 2Ha
I05, BORACIC ACID, HsBOj
Na,B A + HjSO* + SHgO = 4HiBOs + Na^SO^
Borax
33
FIFTH GROUP OF ACIDS— The Mineral Acids.
I06. SILICIC ACID, HgSiOs
SiO, + KsCOs = K^SiOs + COj,
KjSiOs + 2HCl = H8Si08 + 2KC1
HgSiOs (heated) = SiOa + HgO
SiOj + 2NaOH = Na^SiOs + 2Hfi
107* (Preparation and use of Sodic aluminate).
l8t Stage, (NH;)S0^ + A]^{SO^)s + 8NaOH = AlAH^ +
Alum
2NH8 + 4Na8S()4 + 2H80
2d Stagey AlaOjHe + 2NaOH = Na,Al A + ^HgO
Sodic aluminate
BNa^SiOs + NagAl A + ^H^O = Al«(Si08)8 + 8NaOH
Aluminic silicate
107. FLUOHYDRIC ACID, HFl
CaFla +H8S0, = 2HF1 + CaSO,
Fluor-spar
SiO, + 4HF1 = SiFl, + 2H,0
of the glass gaseous
108. THE ORGANIC ACIDS.
The salts of an organic acid char, when heated.
2[KH,H8,04,C4HAJ heated = KgCOj + SH^O + 4C0 + 30
Cream of tartar
But Oxalates are exceptions to this law.
thus [CaO AO2] heated = CaCOa + CO
Calcic oxalate
34
109. ACETIC ACID, HOCCgHjO)
Ethyl alcohol, ^«^^ I O
Acetic ether, C,Hg ) p.
C.H,0 1 "
Ethyl ether, CjHj ) ^
Acetic add,
no. CITRIC ACID, HsH.O^CQHA)
This acid is tetratomic, bat tri-basic. It forms salts of the
following types : (M represents a monad metal, but it is
understood that dyad or triad metals may be substituted for
the proper numbers of monad atoms).
M8H,04Ci HM8H,0,cr H2MH,04Ci
2(Na8HACi) + 3CaCl, = CasHAcTj, + 6NaCl
HI. OXALIC ACID, Bfi^iCfii)
See p. 32.
1X2. GALLIC ACID, C7HA or H^O^fCyHjO)
TANNIN, also called TANNIC ACID, CgyHjgOig
1x3. TARTARIC ACID, HiO^CC^HgOg)
K,Hs,0[t + CaCU= CaHg,©^ + 2Ka
36
EXCEPTIONAL OXALATES, PHOSPHATES
AND BORATES.
ZX4. OXALATES.
CaOjjCA (heated) = CaCO, + CO
CaCOs + 2HC1 = CaClg + COj + UJO
11$. PHOSPHATES.
NH4OH + HOA = NH.G'A + HjO
Ha + NH,OT = NH4CI + HOA
BasCPO*), + Fegd^ = Fe^CPOOs + SBaCl,
1x6. BORATES.
Sr3(B0,), + 3H,S04 = SSrSO, + 2H3BO,
SrSOs is fused with E2COS like an insoluble substance, (see
below,) or it is boiled in a solution of NsaCOs and E^SO^ (see
p. 26, par. 77.)
xxy. SUBSTANCES INSOLUBLE IN WATER
AND ACIDS.
Sand, Quartz, Silicic anhydride, SiO,
(See Silicic acid, p. 33.)
Feldspar, Potassio-aluminio silicate.
5}o.{si.o.
K,Al»(^(Si,0:) + 5K,C0, = 6K,SiO, + 5C0, + A1,0,
Glass, orown glass, Sodio-calcic silicate,
flint glass, Potassio- or sodio-plumbio silicate.
36
Heayy-spar, Bacdc snlpbate. ;
BaSO* + KjCOs = BaCOs + K^SO*
Anglesite, Plambic sulphate.
PbSO^ + KjCOs + (fused on charcoal) = Pb + KgSO* +
CO, + CO
or, by more prolonged fusion on charcoal
PbSO, + K^COj + 40 = Pb + KjbS + 3C0, + CO
BOOK III.
QUANTITATIVE ANALYSIS.
NOTES ON WEIGHTS AND MEASURES.
118. The English system of measures is defined by the
length of a pendulum vibrating seconds of mean time, in a
vacuum at the level of the sea, the latitude of London, the
temperature being 62° F. The length of such a pendulum is
about 39.1393 inches.
1 19. The Metric system is based on the length of the earth's
quadrant. The metre is theoretically the one ten-millionth of
the quadrant. The metre actually used as a standard, has been
found to be about one ten-thousandth too short.
120. The Metric system has certain advantages :
(a) In the employment of a decimal system of division.
(b) In the employment of simple and suggestive names.
(c) In the possession of measures of weight and measures
of volume, which bear simple relations to each
other.
(d) These features have already led to its use by chemists
of all nations.
121. A FEW FUNDAMENTAL DATA.
Of Length.
One Metre = 39.37 inches.
One Kilometre = | of a mile (nearly.)
Of Volume.
One English or Imperial gallon equals 277.274 cubic inches.
4
38
One American or Wine gallon equals 231. cubic inches.
One Litre is one cubic decimetre or 1,000 cubic centimetres.
One Litre is about equal to one Quart.
Of Weight.
One English or Lnperial gallon of water weighs 10 lbs. At.,
or 70,000 grains.
One American gallon of water weighs 8.33 lbs. At., or
58,372.2 grains.
One Litre of water weighs one Kilogramme or 1,000'grammes.
One cubic centimetre of water weighs one gramme.
Z22. The English grain has an absolute weight of 64.8 milli-
grammes. The weight of the girain is the same in Troy,
Apothecaries' and Avoirdupois weight.
One Kilogramme equals about 2^ lbs. Av.
Oi\e gramme equals about 15^1^ grains.
NOTES ON THE EXAMPLES FOR PRACTICE.
123. ALUMINUM, Al, 27.5.
Ordinary or Ammonia Alum when crystallized is,
(NH,),SO, + Al,(SO08 + 24H,0
<NH4)^0, + Al,(SO08 + 6NH4OH = Al^OeHe + 4(NH0j»SO4
AlAHe (heated) = Al^O, + 3H,0
Z24. AMMONIUM, NH4, 18.
It is weighed as NH4CI,
or as Ammonio-platinic chloride (NH4)8PtGle
By distDlation with Ca02Hs, NHs is eyolved.
2NH4a + CaOjH^ = 2NHs + CaCl, + 2H,0
39
I2S. ANTIMONY, Sb, 122.
2SbCl, + 3H|S = SbgS, + 6HC1
Tartar emetic is Potassio-antimonylio tartrate,
(K, SbOH,)0,(C.HA)
SbjS, + 8HN0, = Sb A + 3S + 4H,0 + 4NA
or Sb,S, + 26HNO, = SbA + 3S0, + 13H,0 + 13NA
SbfO^ is called Antimony tetroxide.
126. ARSENIC, As, 76.
AsjO, + 4KaO, + 14HC1 = 2AsCIs + 4KC1 + 7H,0
+ 2C1.0*
The process of construction of the above reaction, illus-
trated :
As,Os is to be changed into 2ASGI5
As^OsH- 6HC1 =2AsCl8 + SHgO [1]
now 2AsCls is to be changed into 2ASCI5; hence 2C1 are needed
2KC10s+ 2Ha = 2KC1 + HgO + Cifi, + [2]
butO + 2HCl = Ca8 + H,0. [3]
by combining [2] and [3] we have
2KCIO3 + 4HC1 = Cla + 2KC1 + 2H80 + CIA M
but since 2C\% are needed we must double the amounts in [4]
thus : 4KCIO3 + 8HC1 = 201, + 4KC1 + 4:Bifi + 201 A- • • [6]
now combining [1] and [5] we have the reaction given at the
beginning.
AsCle + 8NH,0H = (NH^sA^sO, + SNH^Cl + 4HaO
(NH4)sAs04 + MgSO^ = NH4,Mg,AsO, + (NH^^SO^
Ammonio-magnesic arsenate
127. BARIUM, Ba, 137.
Weighed as BaSO^. The salt tested is BaCI, + 2H80
BaSO, + CeHioOj (heated) = BaS + 5H,0 + 4C0 + 20
Filter-paper
BaS + HaSO* = BaSO* + H,S
40
Z28. BISMUTH, Bi, 208.
2BiCl3 + 3H^ = BiA + 6HC1
BijSs + eHNOs = 2Bi(N08)s + 3H,S
2Bi(N08), + 3(NH,),COs = Bi^CCO,), + GNH^NO,
Bi^CCOs), (heated) =Bi A + 3CO2
Z29. EORON, B, 11.
4H3BO8 + NajCOs = Na,B A + CO^ + GH^O
Boracic acid is best weighed as Potassio-boric fluoride,
KBFl,
130. BROMINE, Br, 80.
KBr + AgNO, = AgBr + KNO,
131. CADMIUM, Cd, 112.
Cdia + Na,COs = CdCOs + 2NaI
CdCOj (heated) = CdO + COa
132. CALCIUM, Ca, 40.
CaCO, + 2HC1 = CaClj + CO2 + HgO
CaCl, + (NHOjOjCCA) = CaOg (CA) + 2 NH,a
Ammonie oxalate
CaO,(CA) (heated) = CaCO, + CO
CaCOs (heated) = CaO + CO,
41
133. CARBON, 0, 12.
Composition of good Bone-coal.
Carbon (together with Nitrogen and
a little organic matter) 10.0 per cent.
Calcic phosphate, Ca8(P04)8 ....... .81.0
Calcic carbonate, CaCOs 8.0
Alkaline salts, 4
Silica, SiOg 3
Calcic sulphate, CaSO^ • 2
Ferrous oxide, FeO 1
100.0
X34. CYANOGEN, CN or Cy, 26.
KCj + AgNOs = AgCy + KNO,
AgCN heated = Ag + C + N
C + O, = CO,
135. CHLORINE, CI, 107.97.
NaCl + AgNOs = AgCl + NaNOg
2AgCl + CeHioOg = 2 Ag + 2HC1 + 4HaO + C 0+ 50
(Filter-paper)
60 + 50, = 500,
6 Ag + 8HN08 = 6 AgNOs + N A + 4HgO
AgNOs + Ha = AgCl + HNOs
Compounds of Chlorine and Oxygen (see page 5).
Preparation of Chlorine and of Bleaching-powder (see pp.
2 and 3).
Z36. Reactions in testing Bleaching-powder.
(1st) Stannous chloride method.
[CaOaClj + CaClJ + 4HC1 + 2SnCl8 =
Bleachiog-powder 2CaCl8 + 2H«0 + 2SnCl4
4*
42
SSnCl, + KjCr A + 14Ha = SSnCl* + 2KCI + CraCl« +
7H,0
K,CrA + 14HC1 + 6KI = 61 + CrjCa. + 8KC1 + 7H,0
(2d) The Sodic arsenite method.
As,Os + SNajCO, = 2Na8As03 +3C0,
NasAsO, + HgO + CI, = Na5As04 + 2HC1
NasAsOs + HjO + I« = NajAsO* + 2HI
2kl + Cla = 2KCr+ I,
[CaO,Cl, + CaCla + CaOgHJ + 2Na8AsOs = '
Bleaching-powder
CbsCAsOOs + 4NaCl + 2NaOH
X37. CHROMIUM, Cr, 52,48.
K^Cr A + H,0 + 2Ha = 2H,Cr04 + 2KC1
Beducing the Chromic acid.
2H8CrO,+3H2S +6HC1 = CrgCl, +8H80 + 3S
2H8CrO,+3SO, = Cr^CSOOs +3H,0
2HaCr04+3(C2H50H+6HCl = CrjCl* +81^0 + dC^US)
Ethyi-Alcohol Aldehyd
Cr,Cl« + 6NH4OH = CrAH« + 6NH4CI
Cr AH« heated = Cr A + 3H80
138. COBALT, Co, 59.
CoCNOs), + HjS = CoS + 2HN08
2CoS + [6HC1 + 6HNO3] = Co,Cl« + 3NA + BHgO + 23
Aqua Begia
Co,Clc + 2H3SO4 = 2C0SO4 + 4HC1 + a.
43
139. COPPER, Cu, 63.4
CuSO* + 2NaOH = CuOgHa + Na^SO^
3CaO,Hs = (after boHing) CusHjO* + 2H,0
CU3H A (heated) ;=;3Cu O + H,0
140. The precipitation of Copper by Iron.
CUSO4 + 2Fe + 2HC1 = Cu + FeSO^ + PeCl, + H,
The dissolving of Copper ore&
(Ca^,FeA) + 6HC1 + 22HNO, =
Copper pyrites Aqua regU
2CUSO4 + 'Fefik + 2S + UNA + 1^0
GOLD, Au, 196.
141. Precipitation from solution.
2Aua3 + 6Fe(SO0 = 2Au + 2Fe,(S04)8 + Pe,Cle
142. The action of the fluxes in the fire-assay.
(a) The Argols.
2[HKH2, O4, C^HaOJ heated = IS^COs + SHjO + 200, + 6C
(b) The Litharge.
2PbO + C = 2Pb + COg
PbO + SiOa = PbSiOs
(c) The Sodic carbonate.
Na^COs + SiOg = Na^SiOs + COj
(d) The Borax.
[NajBA + lOHjiO] heated = Na^BA + lOHgO
NaaBA + CuO = NagCuBA
Sodio-cupric borate
44
Z43. IODINE, I, 127.
2Na,S0,S + 1, = 2NaI + NaAO,
Sodio iulpho-sulpbate Sodio tetn^thionate
IRON, Fe, 56.
Z44. The gravimetric test.
6[(NH4)8S04+FeSOJ + 6HC1 + 6HN0, =
6(NH0,SO4 + 2 [Fe^SOO,] + Fe,Cl, + 3NA + 6H,0
Fe,(SO0, + I'e.Cl, + 12NH,0H = 2Fe,0.He+ 3(NH4),SO,+
6NH4CI
Fe,OeH« (heated) = FeA + 3H,0
Z45. The Permanganate test
K,Mn A + 3(H^O0 = K,SO, + 2MnS04 + 3H,0 + 50
lOFeSO* + 50 + 5H,S04 = 5[Fej^SO0s] + 5H,0
• >
146. The Stannous chloride test.
FejCl, + SnCl, = 2FeCl, + SnCi«
SnCl, 4- 2HC1 + 1, = SnCl, + 2HI
147. LEAD, Pb, 207.
Pb(NO,), + B^Ot = PbSO* -f 2HN0,
8PbS + 16HN0, = PbSO. + 2[Pb(N0,) J + 2S + 6NA +
8H,0
148. MAGNESIUM, Mg, 24
MgS04+ (NH0OH+HNa,PO,= (NH^MgPO^-f Na,SO»+H,0
2[NH4MgPOJ heated = Mg,P,0, + 2NHs + H,0
45
149. SULPHUR, S, 32.
H,S + If=2HI + S
150. ZINC, Zn, 65.06.
KaSO^ + Z11SO4 + N%COs = ZnCOj + K, SO* + NagSO*
INDEX.
Acid, Acetic, 34.
Boracic. 32.
Carbonic, 30.
Chloric. 29.
Chlorohydric, 3, 31.
Chromic, 32.
Citric, 31, 34.
Cyanohvdric, 31.
Fiuohydric, 33.
Gallic, 34.
Hypo-phosphorous. 10.
Hypo-sulphurous, 7.
lodohydric, 31.
Meta-phosphoric, 10.
Nitric, 6, 8, 29.
Nitrous, 8.
Oxalic, 32, 33.
Phosphoric, 10, 32.
Phosphorous, 10.
Picric, 29.
Pyro-phosphoric, 10.
Silicic, 33.
Sulpho-sulphuric, 7.
Sulphuric, 7, 31.
Sulphurous, 7, 30.
Sulphydric, 7, 30.
Tannic, 34.
Tartaric, 31, 34.
Acids, deflagrating, 29.
— : — eflFervescing, 30.
organic, 33.
structure of, 5.
tests for, 29.
the Barium group of, 31.
the Mineral group of, 33.
the Silver group of, 31.
Alloys, 28.
Aluminum, 22, 25, 38,
Amidogen, 9.
Ammonium. 8, 9, 27, 28, 38.
Antimony, 8, 19, 21, 39.
Aqua regia, 9.
Arsenic, 8, 19, 21, 39.
Barium, 26, 27, 39.
Bismuth, 19, 22, 40.
Bleaching-powder, 3, 41,
Borates, exceptional, 35.
Boron, 40.
Bromine, 1, 3, 40.
Cadmium, 19, 22, 40.
Calcium, 26, 27, 40.
Carbon, 10, 41.
complex compounds of, 12.
compounds of, 11, 12.
Chlorine, 1, 2, 41.
Chromium, 22, 25, 42.
Cobalt, 22, 24, 42.
Copper, 19, 21, 43.
Crith, 1.
Cyanogen, 12, 41.
English system of weights and
measures, 37.
Fifth group of metals, 27.
First group of metals, 16.
Fourtb group of metals, 26.
Fluorine, 1,3.
Gold, 29, 43.
Hydrogen, 1.
Insoluble substances, (in water
and acids,) 35.
Iodine, 1, 3, 44.
Iron, 22, 25, 44.
Lead, 16, 17, 44.
Magnesium, 27, 28, 44.
Manganese, 22, 25.
Measures, (and weights) Notes
on, 37.
47
Mercury, (Mercurous form) 16,
18.
— (Mercuric form) 19.
Metals and alloys, 28.
Metric system, 37.
Nickel, 22, 25.
Nltrop^en, 8, 9.
Oxygen, 4.
Ozone, 4.
Phosphates, exceptional, 35.
Phosphorus, 8, 9.
Platinum, 29.
Potassium, 27, 28.
Qualitative analysis, 16.
Quantitative analysis, 37.
Second group of metals, 19.
Selenium, 4, 6.
Silicon, 10, 15.
Silver, 16, 17.
Sodium, 28.
Strontium, 26, 27.
Sulphur, 4, 6, 45.
Tannin, 34.
Tellurium, 4, 6.
Third group of metals, 22.
Tin, 10, 19, 21.
Titanium, 10.
Weights and measures, 37.
Zinc, 22, 25, 45.
Thb End.
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