George Willard Benton.
A laboratory guide for a twenty weeks course in general chemistry : containing detailed illustrations for the successful performance of over 150 experiments in general inorganic chemistry and useful tables of reference for pupil and teacher online
. (page 5 of 6)
Online Library → George Willard Benton → A laboratory guide for a twenty weeks course in general chemistry : containing detailed illustrations for the successful performance of over 150 experiments in general inorganic chemistry and useful tables of reference for pupil and teacher → online text (page 5 of 6)
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Now treat a solution of ferric chloride, Fe 2 Cl 6 , with
the three reagents, omitting the use of HNO 3 . Com-
pare with tjae preceding results. (?)
What effect does HNO 3 have on an " ous " salt of
iron?
Devise a table for record of results so that a compari-
son will be easy. The equations are difficult.
Experiment 139. Chromium. The Bead Test. Dip the
hot borax-bead into a solution of potassium chromate,
K 2 CrO 4 , or of potassium bichromate, K 2 Cr 2 O 7 , and heat
in the oxidizing flame before the blowpipe. Chromium
colors the bead green. (?)
Experiment 140. Chromium. Tests for Chromium in the
Wet Way. Divide the solution into three parts.
Through the first pass H 2 S. (?) To the second add
Pb(C 2 H 3 O 2 ) 2 . (?) To the third, AgNO 3 . ( ? )
The products should be in order, a green solution, a
yellow precipitate, and a red precipitate. The two
precipitates are PbCrO 4 and Ag 2 CrO 4 , lead and silver
chromates.
Write reactions for these on the supposition that the
chromium was present as potassium chromate.
138 LABORATORY GUIDE IN CHEMISTRY.
Experiment 141. Test for Aluminum in Solution. Take
5 CC of the solution to be tested. Add one drop of
HC1. ( ? ) Now pass H 2 S for a moment. ( ? )
Should any change be produced up to this time it is
caused by the presence of metals of the first and second
groups, which must be thoroughly precipitated and fil-
tered off before proceeding.
Boil to expel the excess of H 2 S. (The tube should
no longer smell of the gas.) In case first and second
groups are known to be absent, the preceding steps
may be omitted.
Add 1 c c to 2 c c of a solution of ammonium chloride,
NH 4 C1, and then add ammonia, NH 4 OH, a drop at a
time, until on shaking the solution smells of ammonia.
The appearance of a white, gelatinous precipitate of
aluminum hydroxide, A1 2 (OH) 6 is proof of the presence
of aluminum.
Experiment 142. To Separate and Identify Iron, Chro-
mium, and Aluminum in the same Solution. Take 10 c c of
the solution, add two drops of HC1. Pass H 2 S. Fil-
ter if necessary to remove Groups I. and II.
Boil until the solution no longer smells of H 2 S. Add
two drops of cone. HNO 3 and boil for a moment. (?)
Compare Exp. 138. (?)
Add NH 4 OH until the solution is alkaline. Now
add l cc of NH 4 C1. (?) The precipitate contains
Fe a (OH) 6 , Cr a (OH) 6 and A1 2 (OH) 6 .
Colors red, green, and white. Filter and wash.
Make a hole in the bottom of the filter, and wash the
precipitate through into a clean tube. Decant to 5 CC .
Add 1 c c of KOH and boil for some minutes. The
A1 2 (OH) 6 dissolves. Filter.
140 LABORATORY GUIDE IN CHEMISTRY.
Treat the filtrate with HC1 to acid reaction, then add
NH 4 OH and NH 4 C1 as before. Aluminum hydroxide is
precipitated. Compare Exp. 141.
The precipitate of iron and chromium hydroxides
obtained above is now treated for iron and chro-
mium as follows : One-half the paper with its precipitate
is washed with dilute HC1. The precipitate dissolves.
Test this for iron as in Exp. 138. (?)
The remainder of the precipitate with the accompany-
ing paper is put on a piece of platinum foil, covered
with a mixture of equal parts of KNO 3 and Na 2 CO 3 and
fused in the Bunsen flame.
On cooling it is found to be tinged yellow, caused by
the oxidation of the chromium to the form of a chromate.
Remove the mass and dissolve in o cc of H 2 O. Acid-
ulate with acetic acid, and add one drop of lead acetate
solution. (?) Compare Exp. 140. (?)
Experiment 143. Nickel. The Bead Test. Dip the hot
borax-bead into the solution, which will in most cases be
greenish in color, and heat in the oxidizing flame before
the blowpipe. The bead becomes brownish-red while
hot, yellow when cold. (?)
This test is obscured by the presence of cobalt. See
Exp. 145. The reducing flame produces a grayish color,
owing to the reduction to metallic nickel. (?)
Experiment 144. Nickel. Tests in the Wet Way. Take
5 CC of the solution to be tested; add two drops of
NH 4 OH. (?) The apple-green precipitate is Ni (OH) 2 .
Now add an excess of NH 4 OH. (?) Compare the
test for copper, Exp. 137. ( ? ) Now add KOH. ( ? )
To a second portion of the original solution add
KOH. (?) Compare the reactions with NH 4 OH. (?)
142 LABORATORY GUIDE IN CHEMISTRY.
Experiment 145. Cobalt. The Bead Test. Dip the hot
borax bead into the solution to be tested, and heat in
the oxidizing flame. (?)
All cobalt salts produce blue beads. Compare Exp.
39. (?)
Experiment 146. Cobalt. " Sympathetic Ink." Write
on a piece of glazed paper with a solution of cobaltous
nitrate, Co(NO 3 ) 2 . (?) Allow to dry and then
warm. (?)
Hydrated cobalt salts are pink in color; anhydrous
salts are violet. Account for the changes noted.
Experiment 147. Zinc. The Blowpipe Test. Powder
the solid to be tested, mix with sodium carbonate, Na 2 CO 3 ,
and heat in the oxidizing flame before the blowpipe on
charcoal. A coating of oxide will be formed around
the assay, yelloiv while hot, white when cold. (?)
Touch the coating with a rod moistened with a solu-
tion of cobaltous nitrate, Co(NO 3 ) 2 . Heat again in the
oxidizing flame. (?)
The product is a pigment (?) and its production
here is proof of the presence of zinc.
GROUP IV.
Barium, Strontium, and Calcium.
Experiment 148. Barium. Flame and Spectrum Tests.
Moisten a clean platinum wire with a strong solution of
a barium salt and put into the non-luminous flame. (?)
The predominating color of the barium flame is green.
Examine the flame with the spectroscope. (?) The
sifting of the rays of different tinge reveals the presence
of the other colors.
144 LABORATORY GUIDE IN CHEMISTRY.
The bright yellow indicative of sodium is generally
present in all spectrum tests.
Name and locate, with the assistance of the luminous
scale, the bright lines of the barium spectrum.
Experiment 149, Barium. Tests in the Wet Way. A
soluble barium salt may be tested for as follows :
(a) To one portion of the solution add K 2 Cr 2 O 7 and
NH 4 OH. (?) Barium chromate, BaCrO 4 is yellow.
(?) Compare tests for lead, Exp. 123. (?) This
precipitate should be insoluble in HC 2 H 3 O 2 . (?)
() To a second portion, add H 2 SO 4 . (?) Try
its solubility in acids. (?) Barium sulphate is white.
Compare test for a sulphate, Exp. 117.
Try to filter it. (?) Barium sulphate is difficult to
filter, owing to the exceeding fineness of the particles.
(e) To a third portion add one drop of a clear solu-
tion of CaSO 4 . (?) Compare the precipitate with
that obtained in b. (?) It should be the^ame.
Experiment 150. Strontium. Flame and Spectrum Tests.
Treat a strontium salt solution precisely as in Exp.
148. (?)
Name and locate the bright lines.
Experiment 151. Green and Ked Fire. Mix intimately
one part powdered barium nitrate, Ba(NO 3 ) 2 , one part
powdered potassium chlorate, KC1O 3 , and J part flowers
of sulphur. Ignite with a match. (?)
Repeat the experiment, using instead of the Ba(NO 3 ) 2 ,
an equal quantity of powdered Sr(NO 3 ) 2 . (?)
To what are the colors due? Why are the KC1O 3
and sulphur used. (?)
NOTE, Powdered shellac may be substituted for sulphur in Exp. 151.
146 LABORATORY GUIDE IN CHEMISTRY.
Experiment 152. Calcium. Flame and Spectrum Tests.
Treat a calcium salt solution as in Exps. 148 and
150. (?)
Name and locate the lines.
GROUP V.
Potassium and Sodium.
Experiment 153. Potassium. Its Affinity for Water.
Carefully, by means of nippers, drop a piece of metallic
potassium in water in a dish. (?) Look at the flame
through a blue glass. (?)
All potassium salts and the metal itself color the
flame violet. Try the water with litmus paper. (?)
Never handle potassium and sodium with the fingers.
Why? Complete the equation H 2 O + K = KOH + ?
Compare Exp. 49.
The color of the flame is caused by the heat of the
reaction igniting the evolved hydrogen, which in turn
vaporizes some of the potassium which burns with the
characteristic color, forming an oxide, K 2 O.
Experiment 154. Potassium. Flame and Spectrum Tests.
Try a potassium salt solution as before with the flame
and spectroscope. (?)
Name and locate the bright lines.
NOTE. The violet line is difficult to get.
Experiment 155. Sodium. Comparison with Potassium.
Drop a piece of metallic sodium into a dish of water.
(?) Compare Exp. 153. (?)
Repeat the experiment, using hot water. (?) Is
potassium more or less active than sodium ? Explain.
148 LABORATORY GUIDE IN CHEMISTRY.
Try the water with litmus paper. (?)
Why do sodium and potassium float on water ? Com-
pare properties of sodium and potassium.
Experiment 156. Sodium. Flame and Spectrum Tests.
Examine the sodium salt solution as before.
Name and locate the bright lines.
APPENDIX
TABLE OF BEFEBENCES.
REFERENCE BOOKS. ABBREVIATION.
Shepard's Chemistry . . . . ... . . . Shep.
Att field's Chemistry Att.
Fresenius's Qualitative Fre.
Fresenius's Quantitative Fre. Q.
Remsen's Briefer Course Rem.
Richter's Chemistry . . . . . Rich.
Wagner's Technology Wag.
Gage's Elements of Physics ....... Gage.
Dana's Text-Book of Geology Da.
References by Experiments.
EXP.
EXP.
EXP.
EXP.
EXP.
11.
EXP. 7
EXP. 8-
317.
EXP. 9
EXP. 10
EXP. 11
EXP. 12
EXP. 13
EXP. 14
EXP. 15
149.
EXP. 16
EXP. 17
EXP. 18
Fre. Q. P. 30.
Gage P. 9.
Att. P. 91.
Da. P. 27 and 31.
Gage P. 9 ; also Exp.
Att. P. 36.
Att. P. 115 ; Shep. P.
Att. P. 84.
Rich. P. 9*0 ; Fre. P. 4.
Fre. P. 15.
Fre. P. 5.
Fre. P. 8.
- Att. P. 106 ; Fre. P. 9.
-Fre. P. 11 ; also Exp.
- Shep. P. 9.
-Shep. P. 10.
- Shep. P. 172.
EXP. 19 Shep. P. 11.
EXP. 20 Shep. P. 325.
EXP. 21 Att. P. 143.
EXP. 22 Shep. P. 23.
EXP. 23 Shep. P. 23 ; Rem. P.
41.
EXP. 24 Att. P. 17 ; Rem. P.
10.
EXP. 25 Explanation of the
action of MnO 2 : It either
remains unchanged or under-
goes a double change acting
as a carrier in freeing the
KClO 3 of its oxygen. Such
action has been called " ca-
talysis."
EXPS. 26, 27, and 28-Shep. P. 25.
EXP. 29 Shep. P. 317.
EXP. 30 Shep. P. 27; Att. P.
23.
EXP. 31 Shep. P. 27.
EXP. 32 Shep. P. 27.
153
154
APPENDIX.
EXP. 33 Wag. P. 618; Att. P.
30.
EXP. 34 Rem. P. 51-3.
EXP. 35 Gage, P. 145.
EXP. 37 Shep. P. 28; Rich. P.
293; Rem. P. 199.
EXP. 38 Shep. P. 29; Rem. P.
198.
EXP. 39 Rem. P. 201 ; Shep.
P. 282.
EXP. 40 Rem. P. 52.
EXP. 41 Rem. P. 196; Att. P.
23.
EXP. 42 Rem. P. 196; Att. P. 23.
EXP. 44 Rem. P. 53; Att. P.
155, Note 1.
EXP. 45 Shep. P. 31 ; Rem. P.
91.
EXP. 46 Shep. P. 31.
EXP. 47 Att. P. 86.
EXP. 49 Shep. P. 35; Att. P.
94; Rem. P. 59.
EXP. 50 Rem. P. 65 ; Shep. P.
37; Att. P. 20.
EXP. 51 Att. P. 21.
EXP. 54 Rem. P. 77.
EXP. 55 Wag. P. 646.
EXP. 56 Rem. P. 77; Shep. P.
40.
EXP. 57 Shep. P. 35.
EXP. 58 Rem. P. 72.
EXP. 59 Rem. P. 127; Shep.
P. 50.
EXP. 60 Shep. P. 51 ; Rem. P.
131.
EXP. 61 Rem. P. 139; Shep.
P. 52.
EXP. 62 Shep. P. 52.
EXP. 63 Shep. P. 55.
EXP. 64 Shep. P. 58.
EXP. 65 Att. P. 94; Rem. P.
117.
EXP. 66 Shep. P. 59; Rem. P.
157.
EXP. 67 Shep. P. 60; Rem. P.
158.
EXP. 68 Shep. P. 61 ; Rem. P.
158.
EXP. 69 Shep. P. 63.
EXP. 70 Shep. P. 64.
EXP. 71 Shep. P. 67; Rem. P.
148.
EXP. 72 Shep. P. 68; Rem. P.
152.
EXP. 73 Shep. P. 69; Rem. P.
310; Wag. P. 148.
EXP. 74 Shep. P. 69.
EXP. 75 Shep. P. 69.
EXP. 76 Wag. P. 160.
EXP. 77 Shep. P. 70; Att. P.
285.
EXP. 78 Shep. P. 70; Att. P.
286.
EXP. 79 Shep. P. 92; Att. P.
29; Rem. P. 98.
EXP. 80 Shep. P. 93 and 95:
Rem. P. 101.
EXP. 81 Shep. P. 96.
EXP. 82 Shep. P. 97; Hem. P.
103.
EXP. 83 Shep. P. 99.
EXP. 84 Shep. P. 109; Rem.
P. 237.
EXPS. 85 and 86 Shep. P. 110.
EXP. 87 Shep. P. 110; Att. P.
268.
EXP. 88 Att. P. 268.
EXP. 89 Shep. P. 116; Rem.
P. 240.
EXP. 90 Shep. P. 117; Att. P.
271.
EXP. 91 Shep. P. 118.
EXP. 92 Shep. P. 119; Att. P.
271.
EXP. 93 Att. P. 271.
APPENDIX.
155
EXP. 94
273.
EXP. 95
P. 243.
EXP. 96
EXP. 97
EXP. 98-
EXP. 99
P. 645.
EXPS. 101
135.
EXP. 103 -
EXP. 104-
EXP. 105 -
EXP. 106 -
EXP. 107-
P. 181.
EXP. 108-
EXP. 109 -
P. 205.
EXP. 110
P. 248.
EXP. 111-
EXP. 112 -
P. 252.
EXP. 113
P. 252.
EXP. 114 -
EXP. 115-
P. 257.
EXP. 116-
EXP. 117 -
EXP. 118-
P. 267.
EXP. 119-
EXP. 120-
P. 192.
EXP. 121
Shep. P. 119 ; Att. P.
Shep. P. 122; Rem.
Shep. P. 130.
Shep. P. 132.
Shep. P. 133.
Shep. P. 135; Wag.
and 102 Shep. P.
Shep. P. 136.
Shep. P. 140.
Shep. P. 140 and 142.
Shep. P. 138.
Shep. P. 138; Rem.
Da. P. 36-7.
Shep. P. 146; Rem.
Shep. P. 158; Rem.
Rem. P. 249.
Shep. P. 158; Rem.
Shep. P. 160; Rem.
Shep. P. 163.
Shep. P. 164; Rem.
Shep. P. 166.
Shep. P. 173.
Shep. P. 197; Rem.
-Shep. P. 204-206.
-Shep. P. 211; Att.
Shep. P. 225.
EXP. 122 Shep. P. 225 ; Rem.
P. 365.
EXP. 123 Shep. P. 228.
EXP. 124 Shep. P. 229; Rem.
P. 341.
EXP. 125 Shep. P. 229.
EXP. 126 Shep. P. 233.
EXP. 127 Shep. P. 234.
EXP. 128 Shep. P. 235.
EXP. 129 Shep. P. 239.
EXP. 130 Shep. P. 242.
EXP. 131 Shep. P. 246; Rem.
P. 271.
EXP. 132 Shep. P. 252.
EXP. 133 Shep. P. 253.
EXP. 134 Shep. P. 259.
EXP. 135 Shep. P. 261; Rem.
P. 335.
EXPS. 136 and 137 Shep. P. 261.
EXP. 138 Shep. P. 281.
EXP. 139 Shep. P. 285.
EXP. 140 Shep. P. 285.
EXP. 141 Shep. P. 288.
EXP. 142 Shep. P. 289.
EXPS. 143 and 144 Shep. P.
292.
EXPS. 145 and 146 Shep. P.
294; Att. P. 231.
EXP. 147 Shep. P. 300.
EXP. 148 Shep. P. 312.
EXP. 149 Shep. P. 311.
EXP. 150 Shep. P. 313.
EXP. 152 Shep. P. 316.
EXP. 153 Shep. P. 321.
EXP. 154 Shep. P. 326.
EXP. 155 Shep. P. 328.
EXP. 156 Shep. P. 333.
156
APPENDIX.
TABLE OF WEIGHTS AND MEASURES.
ENGLISH WEIGHTS.
Avoirdupois Weight.
POUND.
OUNCES.
DRACHMS.
GRAINS
1
. . 16 . . ,
, . . 256 . .
7000
1
16
. . .437.5
1 . .
. 27.3495
1
GRAMMES.
453.5926
28.3495
1.7718
.0648
Troy Weight.
POUND.
1 .
OUNCES.
. . 12 .
PENNYWEIGHT.
. . . 240 . .
GRAINS.
. 5760 .
GRAMMES.
. . 373.2419
1
20
. 480 .
. . 31.1035
1
24 .
. . 1.5552
1 .
.0648
METRIC MEASURES.
Measures of Weight.
1 milligram (mg)
1 centigram (cg)
1 decigram (dg)
0.001 gram
0.010 gram
about -fa of grain.
gram
(g)
= 0.100 gram.
= 1.000 gram = 15.4323 grains.
1 liter ^
1 quart
1 meter (m)
1 inch
Equivalents.
= 1.0567 quarts.
= .9463 liters.
= 39.3708 inches.
= 2.54 centimeters (cm) .
APPENDIX.
157
A TABLE OF THE PRINCIPAL ELEMENTS.
ELEMENTS.
AT.
WT.
SYM.
VAL.
SP. G.
CONDITION.
g f Oxygen
16
O
2
1.105
Gas.
Jttj
Nitrogen
14
N
1,3,5
0.971
Gas.
t *-
Chlorine
35.5
Cl
1
2.45
Gas.
*
Bromine
79.8
Br
1
3.187
Liquid.
3
Iodine
126.6
I
1
4.948
Solid.
i
Fluorine
19
F
1
1.313
Gas.
o|
Carbon
12
C
4
3.S-.6
Solid.
i Jj
Sulphur
32
S
2,4
2.05
Solid.
"S.2
Phosphorous
31
p
3,5
1.83
Solid.
11
Arsenic
75
As
3,5
5.73
Solid.
* [_ Chromium
52.4
Cr
4,6
6.5
Solid.
Hydrogen
1
H
1
.069
Gas.
f Manganese
54
Mn
2,4,6
8.03
Solid.
fee
Boron
11
Bo
3
2.5?
Solid.
Lead
206.5
Pb
2,4
11.37
Solid.
5
Silver
107.7
Ag
1
10.53
Solid.
I
Mercury
200
Hg
1,2
13.55
Liquid.
S3
Magnesium
24
Mg
2
1.74
Solid.
X!
to
Tin
117.7
Sn
2,4
7.29
Solid.
1
Copper
63
Cu
1,2
8.95
Solid.
1
Iron
56
Fe
2,4
7.86
Solid.
I 1
Aluminum
27
Al
4
2.6
Solid.
1
Nickel
58
Ni
2,4
8.9
Solid.
o
Cobalt
59
Co
2,4
S.5-.7
Solid.
a
Zinc
65
Zn
2
7.15
Solid.
S
Barium
136.8
Ba
2
3.75
Solid.
"S
Strontium
87.4
Sr
2
2.54
Solid.
.2
Calcium
40
Ca
2
1.57
Solid.
1
"S
Potassium
39
K
1
.87
Solid.
s
Platinum
194.4
Pt
4
21.50
Solid.
^ Sodium
23
Na
1
.978
Solid.
158 APPENDIX.
LIST OF CHEMICALS AND APPARATUS
FOR THE COURSE.
Preparation of Reagents.
Aniline A few particles in H 2 to required color.
AgN0 3 1 g. of the crystal salt to 40 cc distilled
H 2 0.
Alcohol Use 95 %.
A1 2 K 2 (S0 4 ) 4 . .....1 g. to!0 cc .
BaCl 2 1 g. to!0 cc .
Ba(N0 3 ) 2 1 g. to!0 cc .
Ca(OH) 2 Digest slaked lime in H 2 0, and filter.
Co(]Sr03) 2 1 g. to 15 cc . Use the crys. salt.
Chlorine water .... Saturated solution of chlorine in H 2 0.
Protect from light.
Chloral Hydrate . . . 1 g. to 20 cc .
Cr 2 K 2 (S0 4 ) 4 Ig. to!0 cc .
CuS0 4 Ig. to!0 cc .
CoCl 2 Ig. to!0 cc .
C 2 H 4 2 30%. >
CaCl 2 1 g. to!0 cc .
CaS0 4 Saturated solution in H 2 0.
FeS0 4 Make up as needed with distilled H 2 O.
Fe 2 Cl 6 . 1 g. to 10 cc . Use crys. salt.
HC1, dil Beagent strength 1 to 4 by vol. Equiv.
to 8.5 % HC1.
HN0 3 dil 1 to 3 by vol. Equiv. to 20 % HN0 3 .
APPENDIX. 159
H 2 S0 4 , dil 1 to 5 by vol. Equiv. to 25 % H 2 S0 4 .
Pour the acid into the water care-
fully.
HgCl 2 Saturated Solution.
HgN0 3 1 g. to20 cc .
H 2 S Prepare as needed, using Kipp gene-
rator or equiv. with FeS and com-
mercial HC1 dil. 1 to 1 by vol.
H 3 As0 4 1 g. to50 cc .
KMn0 4 Strong sol. 1 g. to 10 cc ; or, better, a sat-
urated solution.
KMn0 4 , dil l cc of strong sol. to 200 cc H 2 0.
KI 1 g. to20 cc .
KOH Ig. to!0 cc .
KCy 1 g. to 10 c c . Use cold water. Does not
keep well.
KBr Ig. to20 cc .
K 2 O 2 7 1 g. to 10 cc . Use warm H 2 0.
K 4 FeCy c 1 g. to 15 CC .
KCyS 1 g. to!5 cc .
K 3 FeCy 6 Make up as needed, 1 g. to 15 c c . Does
not keep.
K 2 Cr0 4 Ig. to20 cc .
NaOH 1 g. to 10 c c . Allow to settle, and decant.
NH 4 OH Dilute cone. 1 to 3 by vol. Equiv. to
10% NH 3 .
NH 4 C1 Ig. to!0 cc .
Nad Ig. to!0 cc .
(NH 4 ) 2 C0 3 ........ 200 g. (NH 4 ) 2 C0 3 , 800 cc H 2 0, and
209 CC NH 4 OH.
(NH 4 ) 2 S Saturate KH 4 OH with H 2 S. Add
NH 4 OH to alkaline reaction.
(N"H 4 ) 2 S 2 Add a little flowers of sulphur to
(NH 4 ) 2 S.
160 APPENDIX.
......... lg. to20 cc .
MC1 2 ............ 1 g. to!0 cc .
Pb(C 2 H 3 2 ) 2 ...... lg. to20 cc .
Starch ........... Digest 1 spoonful in 300 c c cold water,
and boil.
SnCl 2 ............ Dissolve in least amount of hot cone.
Hl. Dilute with H 2 0, l cc to
20 c c , and keep in a bottle with a
piece of metallic tin.
SnCl 4 ............ Dissolve tin in aqua regia. Evaporate
to dryness. Make up 1 g. to 20 cc
or more dilute if desired.
SrCl 2 ............ 1 g. to!0 cc .
Sr(N0 3 ) 2 ......... lg. to!0 cc .
Touch Paper, made by dipping filter paper in strong solution
KN0 3 and drying.
ZnS0 4 ........... Saturated solution.
ZnCl 2 ............ 1 g- to 10 CC .
APPENDIX.
161
PURCHASING LIST.
Alcohol . . . ".
Ammonium Carbonate
Ammonium Hydrate, cone.
AS 2 3 . . . ; .
Borax .
Carbon Disulphide . ' .
Copper clippings
CuS0 4 . . . .
CaCl 2 '. . : .
CaO ...~ ...
CaF 2 .'. . '}. . ,
Cotton, common
Cotton, gun
Charcoal, powdered - ; .
Charcoal, sticks for blowpipe
Coal, bituminous . .
Ether ....
FeS0 4 .....
FeS, fused ....
HgO . . ' . . .
Hydrochloric Acid, C.P. Sp. G.
Hydrochloric Acid, com. Sp. G.
Iodine, sublimed
Iron Filings, very fine .
KNO,. . ...
KBr . . ; . . .
KI . \".
KC!0 3
1.20
1.20
Fou 20 PUPILS.
1 quart,
i pound.
4 pounds.
1 ounce.
pound,
i pound.
1 pound.
1 pound.
^ pound.
I pound.
1 pound.
2 ounces.
1 ounce.
\ ounce.
1 pound.
20.
^ pound.
1 pound.
^ pound.
1 pound.
pound.
6 pounds.
2 pounds.
ounce.
J pound.
pound.
2 ounces.
2 ounces.
2 pounds.
162
APPENDIX.
K 4 FeCy 6
Lead, metallic ......
Litmus Paper, red and blue
Mercury, metallic .....
Mn0 2
Magnesium Ribbon .....
Marble, White . . . . ;
Nad ; ." , ..' . . . .'-
NH 4 1TO 3 , anhydrous . . . .'
NH 4 C1. . '
NaC 2 H 3 2 .
Na 2 C0 3 . . - . . . ?. . - .
NaOH . . . ... .' . .
Nitric Acid, Sp. G. 1.42 . . .
Plaster of Paris . . .
Pb(NO,) a . . . V . . ;'.
PbS, powdered . . . . . .
Pbo . ;-. . . .
Phosphorus . . . . .
Potassium, metallic
Potassium Hydroxide, sticks
Platinum Wire, for blowpiping .
Platinum Foil . . . - t ' . . .
Starch . . . . . .
Sr(X0 3 ) 2
Sodium, metallic
Sulphur, roll . . .
Sulphur, flowers . .
Sulphuric Acid, Sp. G. 1.84 .
Sugar, granulated
Zinc, sheet
Zinc, granulated, made by pouring melted
lumps into H 2
ZnS, powdered .
^ pound,
i pound.
1 'sheet each.
1 pound.
pound.
^ ounce.
2 pounds.
1 pound.
2 pounds.
1 pound.
2 ounces.
1 pound.
pound.
3 pounds.
1 pound.
2 ounces.
1 ounce.
1 ounce.
1 ounce,
i ounce.
1 pound.
5 grams.
5 grams.
L pound.
% pound.
ounce.
J pound.
1 pound.
9 pounds.
1 pound.
1 pound.
2 pounds.
1 ounce.
Order Chemicals not otherwise specified in 1 ounce packages. Use
C. P. Chemicals and distilled water for solutions wherever possible.
APPENDIX. 163
Apparatus required for each Pupil.
1 Metric and English rule. 1 foot.
6 Test-tubes, g-"x6".
1 Rubber delivery tube.
1 Glass delivery tube.
1 Piece of window glass 2" square.
1 Piece of blue glass 2" square.
1 Evaporating dish.
1 Pair nippers.
1 Watch crystal, diameter 2",
1 Small microscope.
10 Filters, 5".
1 Funnel, 2f .
1 Glass rod.
1 Small magnet.
1 Tin-box cover.
1 Pneumatic trough.
4 Wide-mouth 4 oz. bottles.
Wide-mouth 1 oz. bottle.
Narrow-mouth 4 oz. bottle.
Foot No. 18 iron wire.
Foot fine iron wire.
Combustion spoon.
2 Pieces white cardboard, 2" square.
4 Pieces glass tubing, 4" diameter, ?>" long.
1 Glass tumbler.
1 Paraffin candle.
1 Lamp chimney, Argand.
1 Strip zinc, 4"xl".
1 Blowpipe.
1 Piece of wire gauze, 4" square, iron.
1 Tripod or ring stand.
1 Test-tube holder.
1 Wash bottle.
Assorted rubber stoppers and corks to fit bottles and test tubes.
YB 36031
SCIENCE.
Chemistry : An Introduction to the Study of the Compounds of Carbon.
By IRA REMSEN, Professor of Chemistry, Johns Hopkins University,- Baltimore.
374 pages. Cloth. Price by mail, $1-30; Introduction price, #1.20.
The Elements of Inorganic Chemistry : Descriptive and Qualitative.
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399 pages. Cloth. Price by mail, $1.25 ; Introduction price, $1.12.
The Elements Of Chemistry .' Descriptive W Qualitative. Briefer Course.
By JAMES H. SHBPAKD, Professor of Chemistry in So. Dakota Agricultural Col leg*,
48 pages. Price by mail, 90 cts.; Introduction price, 80 cts.
Practical
Or Guide for the Physical Laboratory.
By H. N. CHUTE, Instructor in Physics, Ann Arbor High School, Mich. Cloth.
407 pages. Price by mail, $1.25 ; Introduction price, #1.12.
The Laboratory Note- Book. For Students using any Chemistry.
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Cloth back. 192 pages. Price by mail, 40 cts. ; Introduction price, 35 cts.
The Elements of Chemical Arithmetic : with a short system O f EI~
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Chemical Problems, Adapted to High Schools and Colleges.
By JOSEPH P. GRABFIBLD and T. S. BURNS, Instructors in General Chemistry in the
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196 pages. Price by mail, 85 cts. ; Introduction price, 80 cts.
First Book of Geology.
By N. S. SHALER, Professor of Palaeontology, Harvard University. 272 pages, with 130
/iguresin the text. Price by mail, $1.10 ; Introduction price, $1.00.
The Teaching of Geology.
By N. S. SHALER, author of First Book in Geology. Paper. 74 pages. Price, 25 cents.
Petrography. AH Account of the Application of the Microscope to the
Study of Geology . By GEORGE HUNTINOTON WILLIAMS, of the Johns Hopkins University
Paper. 35 pages. Price, 25 cents.
Astronomical Lantern and How to Find the Stars.
By REV. JAMES FREEMAN CLARKE. Intended to familiarize students with the constel-
lations. by comparing them with fac-similes on the lantern face. Price of the Lantern, kt
the three reagents, omitting the use of HNO 3 . Com-
pare with tjae preceding results. (?)
What effect does HNO 3 have on an " ous " salt of
iron?
Devise a table for record of results so that a compari-
son will be easy. The equations are difficult.
Experiment 139. Chromium. The Bead Test. Dip the
hot borax-bead into a solution of potassium chromate,
K 2 CrO 4 , or of potassium bichromate, K 2 Cr 2 O 7 , and heat
in the oxidizing flame before the blowpipe. Chromium
colors the bead green. (?)
Experiment 140. Chromium. Tests for Chromium in the
Wet Way. Divide the solution into three parts.
Through the first pass H 2 S. (?) To the second add
Pb(C 2 H 3 O 2 ) 2 . (?) To the third, AgNO 3 . ( ? )
The products should be in order, a green solution, a
yellow precipitate, and a red precipitate. The two
precipitates are PbCrO 4 and Ag 2 CrO 4 , lead and silver
chromates.
Write reactions for these on the supposition that the
chromium was present as potassium chromate.
138 LABORATORY GUIDE IN CHEMISTRY.
Experiment 141. Test for Aluminum in Solution. Take
5 CC of the solution to be tested. Add one drop of
HC1. ( ? ) Now pass H 2 S for a moment. ( ? )
Should any change be produced up to this time it is
caused by the presence of metals of the first and second
groups, which must be thoroughly precipitated and fil-
tered off before proceeding.
Boil to expel the excess of H 2 S. (The tube should
no longer smell of the gas.) In case first and second
groups are known to be absent, the preceding steps
may be omitted.
Add 1 c c to 2 c c of a solution of ammonium chloride,
NH 4 C1, and then add ammonia, NH 4 OH, a drop at a
time, until on shaking the solution smells of ammonia.
The appearance of a white, gelatinous precipitate of
aluminum hydroxide, A1 2 (OH) 6 is proof of the presence
of aluminum.
Experiment 142. To Separate and Identify Iron, Chro-
mium, and Aluminum in the same Solution. Take 10 c c of
the solution, add two drops of HC1. Pass H 2 S. Fil-
ter if necessary to remove Groups I. and II.
Boil until the solution no longer smells of H 2 S. Add
two drops of cone. HNO 3 and boil for a moment. (?)
Compare Exp. 138. (?)
Add NH 4 OH until the solution is alkaline. Now
add l cc of NH 4 C1. (?) The precipitate contains
Fe a (OH) 6 , Cr a (OH) 6 and A1 2 (OH) 6 .
Colors red, green, and white. Filter and wash.
Make a hole in the bottom of the filter, and wash the
precipitate through into a clean tube. Decant to 5 CC .
Add 1 c c of KOH and boil for some minutes. The
A1 2 (OH) 6 dissolves. Filter.
140 LABORATORY GUIDE IN CHEMISTRY.
Treat the filtrate with HC1 to acid reaction, then add
NH 4 OH and NH 4 C1 as before. Aluminum hydroxide is
precipitated. Compare Exp. 141.
The precipitate of iron and chromium hydroxides
obtained above is now treated for iron and chro-
mium as follows : One-half the paper with its precipitate
is washed with dilute HC1. The precipitate dissolves.
Test this for iron as in Exp. 138. (?)
The remainder of the precipitate with the accompany-
ing paper is put on a piece of platinum foil, covered
with a mixture of equal parts of KNO 3 and Na 2 CO 3 and
fused in the Bunsen flame.
On cooling it is found to be tinged yellow, caused by
the oxidation of the chromium to the form of a chromate.
Remove the mass and dissolve in o cc of H 2 O. Acid-
ulate with acetic acid, and add one drop of lead acetate
solution. (?) Compare Exp. 140. (?)
Experiment 143. Nickel. The Bead Test. Dip the hot
borax-bead into the solution, which will in most cases be
greenish in color, and heat in the oxidizing flame before
the blowpipe. The bead becomes brownish-red while
hot, yellow when cold. (?)
This test is obscured by the presence of cobalt. See
Exp. 145. The reducing flame produces a grayish color,
owing to the reduction to metallic nickel. (?)
Experiment 144. Nickel. Tests in the Wet Way. Take
5 CC of the solution to be tested; add two drops of
NH 4 OH. (?) The apple-green precipitate is Ni (OH) 2 .
Now add an excess of NH 4 OH. (?) Compare the
test for copper, Exp. 137. ( ? ) Now add KOH. ( ? )
To a second portion of the original solution add
KOH. (?) Compare the reactions with NH 4 OH. (?)
142 LABORATORY GUIDE IN CHEMISTRY.
Experiment 145. Cobalt. The Bead Test. Dip the hot
borax bead into the solution to be tested, and heat in
the oxidizing flame. (?)
All cobalt salts produce blue beads. Compare Exp.
39. (?)
Experiment 146. Cobalt. " Sympathetic Ink." Write
on a piece of glazed paper with a solution of cobaltous
nitrate, Co(NO 3 ) 2 . (?) Allow to dry and then
warm. (?)
Hydrated cobalt salts are pink in color; anhydrous
salts are violet. Account for the changes noted.
Experiment 147. Zinc. The Blowpipe Test. Powder
the solid to be tested, mix with sodium carbonate, Na 2 CO 3 ,
and heat in the oxidizing flame before the blowpipe on
charcoal. A coating of oxide will be formed around
the assay, yelloiv while hot, white when cold. (?)
Touch the coating with a rod moistened with a solu-
tion of cobaltous nitrate, Co(NO 3 ) 2 . Heat again in the
oxidizing flame. (?)
The product is a pigment (?) and its production
here is proof of the presence of zinc.
GROUP IV.
Barium, Strontium, and Calcium.
Experiment 148. Barium. Flame and Spectrum Tests.
Moisten a clean platinum wire with a strong solution of
a barium salt and put into the non-luminous flame. (?)
The predominating color of the barium flame is green.
Examine the flame with the spectroscope. (?) The
sifting of the rays of different tinge reveals the presence
of the other colors.
144 LABORATORY GUIDE IN CHEMISTRY.
The bright yellow indicative of sodium is generally
present in all spectrum tests.
Name and locate, with the assistance of the luminous
scale, the bright lines of the barium spectrum.
Experiment 149, Barium. Tests in the Wet Way. A
soluble barium salt may be tested for as follows :
(a) To one portion of the solution add K 2 Cr 2 O 7 and
NH 4 OH. (?) Barium chromate, BaCrO 4 is yellow.
(?) Compare tests for lead, Exp. 123. (?) This
precipitate should be insoluble in HC 2 H 3 O 2 . (?)
() To a second portion, add H 2 SO 4 . (?) Try
its solubility in acids. (?) Barium sulphate is white.
Compare test for a sulphate, Exp. 117.
Try to filter it. (?) Barium sulphate is difficult to
filter, owing to the exceeding fineness of the particles.
(e) To a third portion add one drop of a clear solu-
tion of CaSO 4 . (?) Compare the precipitate with
that obtained in b. (?) It should be the^ame.
Experiment 150. Strontium. Flame and Spectrum Tests.
Treat a strontium salt solution precisely as in Exp.
148. (?)
Name and locate the bright lines.
Experiment 151. Green and Ked Fire. Mix intimately
one part powdered barium nitrate, Ba(NO 3 ) 2 , one part
powdered potassium chlorate, KC1O 3 , and J part flowers
of sulphur. Ignite with a match. (?)
Repeat the experiment, using instead of the Ba(NO 3 ) 2 ,
an equal quantity of powdered Sr(NO 3 ) 2 . (?)
To what are the colors due? Why are the KC1O 3
and sulphur used. (?)
NOTE, Powdered shellac may be substituted for sulphur in Exp. 151.
146 LABORATORY GUIDE IN CHEMISTRY.
Experiment 152. Calcium. Flame and Spectrum Tests.
Treat a calcium salt solution as in Exps. 148 and
150. (?)
Name and locate the lines.
GROUP V.
Potassium and Sodium.
Experiment 153. Potassium. Its Affinity for Water.
Carefully, by means of nippers, drop a piece of metallic
potassium in water in a dish. (?) Look at the flame
through a blue glass. (?)
All potassium salts and the metal itself color the
flame violet. Try the water with litmus paper. (?)
Never handle potassium and sodium with the fingers.
Why? Complete the equation H 2 O + K = KOH + ?
Compare Exp. 49.
The color of the flame is caused by the heat of the
reaction igniting the evolved hydrogen, which in turn
vaporizes some of the potassium which burns with the
characteristic color, forming an oxide, K 2 O.
Experiment 154. Potassium. Flame and Spectrum Tests.
Try a potassium salt solution as before with the flame
and spectroscope. (?)
Name and locate the bright lines.
NOTE. The violet line is difficult to get.
Experiment 155. Sodium. Comparison with Potassium.
Drop a piece of metallic sodium into a dish of water.
(?) Compare Exp. 153. (?)
Repeat the experiment, using hot water. (?) Is
potassium more or less active than sodium ? Explain.
148 LABORATORY GUIDE IN CHEMISTRY.
Try the water with litmus paper. (?)
Why do sodium and potassium float on water ? Com-
pare properties of sodium and potassium.
Experiment 156. Sodium. Flame and Spectrum Tests.
Examine the sodium salt solution as before.
Name and locate the bright lines.
APPENDIX
TABLE OF BEFEBENCES.
REFERENCE BOOKS. ABBREVIATION.
Shepard's Chemistry . . . . ... . . . Shep.
Att field's Chemistry Att.
Fresenius's Qualitative Fre.
Fresenius's Quantitative Fre. Q.
Remsen's Briefer Course Rem.
Richter's Chemistry . . . . . Rich.
Wagner's Technology Wag.
Gage's Elements of Physics ....... Gage.
Dana's Text-Book of Geology Da.
References by Experiments.
EXP.
EXP.
EXP.
EXP.
EXP.
11.
EXP. 7
EXP. 8-
317.
EXP. 9
EXP. 10
EXP. 11
EXP. 12
EXP. 13
EXP. 14
EXP. 15
149.
EXP. 16
EXP. 17
EXP. 18
Fre. Q. P. 30.
Gage P. 9.
Att. P. 91.
Da. P. 27 and 31.
Gage P. 9 ; also Exp.
Att. P. 36.
Att. P. 115 ; Shep. P.
Att. P. 84.
Rich. P. 9*0 ; Fre. P. 4.
Fre. P. 15.
Fre. P. 5.
Fre. P. 8.
- Att. P. 106 ; Fre. P. 9.
-Fre. P. 11 ; also Exp.
- Shep. P. 9.
-Shep. P. 10.
- Shep. P. 172.
EXP. 19 Shep. P. 11.
EXP. 20 Shep. P. 325.
EXP. 21 Att. P. 143.
EXP. 22 Shep. P. 23.
EXP. 23 Shep. P. 23 ; Rem. P.
41.
EXP. 24 Att. P. 17 ; Rem. P.
10.
EXP. 25 Explanation of the
action of MnO 2 : It either
remains unchanged or under-
goes a double change acting
as a carrier in freeing the
KClO 3 of its oxygen. Such
action has been called " ca-
talysis."
EXPS. 26, 27, and 28-Shep. P. 25.
EXP. 29 Shep. P. 317.
EXP. 30 Shep. P. 27; Att. P.
23.
EXP. 31 Shep. P. 27.
EXP. 32 Shep. P. 27.
153
154
APPENDIX.
EXP. 33 Wag. P. 618; Att. P.
30.
EXP. 34 Rem. P. 51-3.
EXP. 35 Gage, P. 145.
EXP. 37 Shep. P. 28; Rich. P.
293; Rem. P. 199.
EXP. 38 Shep. P. 29; Rem. P.
198.
EXP. 39 Rem. P. 201 ; Shep.
P. 282.
EXP. 40 Rem. P. 52.
EXP. 41 Rem. P. 196; Att. P.
23.
EXP. 42 Rem. P. 196; Att. P. 23.
EXP. 44 Rem. P. 53; Att. P.
155, Note 1.
EXP. 45 Shep. P. 31 ; Rem. P.
91.
EXP. 46 Shep. P. 31.
EXP. 47 Att. P. 86.
EXP. 49 Shep. P. 35; Att. P.
94; Rem. P. 59.
EXP. 50 Rem. P. 65 ; Shep. P.
37; Att. P. 20.
EXP. 51 Att. P. 21.
EXP. 54 Rem. P. 77.
EXP. 55 Wag. P. 646.
EXP. 56 Rem. P. 77; Shep. P.
40.
EXP. 57 Shep. P. 35.
EXP. 58 Rem. P. 72.
EXP. 59 Rem. P. 127; Shep.
P. 50.
EXP. 60 Shep. P. 51 ; Rem. P.
131.
EXP. 61 Rem. P. 139; Shep.
P. 52.
EXP. 62 Shep. P. 52.
EXP. 63 Shep. P. 55.
EXP. 64 Shep. P. 58.
EXP. 65 Att. P. 94; Rem. P.
117.
EXP. 66 Shep. P. 59; Rem. P.
157.
EXP. 67 Shep. P. 60; Rem. P.
158.
EXP. 68 Shep. P. 61 ; Rem. P.
158.
EXP. 69 Shep. P. 63.
EXP. 70 Shep. P. 64.
EXP. 71 Shep. P. 67; Rem. P.
148.
EXP. 72 Shep. P. 68; Rem. P.
152.
EXP. 73 Shep. P. 69; Rem. P.
310; Wag. P. 148.
EXP. 74 Shep. P. 69.
EXP. 75 Shep. P. 69.
EXP. 76 Wag. P. 160.
EXP. 77 Shep. P. 70; Att. P.
285.
EXP. 78 Shep. P. 70; Att. P.
286.
EXP. 79 Shep. P. 92; Att. P.
29; Rem. P. 98.
EXP. 80 Shep. P. 93 and 95:
Rem. P. 101.
EXP. 81 Shep. P. 96.
EXP. 82 Shep. P. 97; Hem. P.
103.
EXP. 83 Shep. P. 99.
EXP. 84 Shep. P. 109; Rem.
P. 237.
EXPS. 85 and 86 Shep. P. 110.
EXP. 87 Shep. P. 110; Att. P.
268.
EXP. 88 Att. P. 268.
EXP. 89 Shep. P. 116; Rem.
P. 240.
EXP. 90 Shep. P. 117; Att. P.
271.
EXP. 91 Shep. P. 118.
EXP. 92 Shep. P. 119; Att. P.
271.
EXP. 93 Att. P. 271.
APPENDIX.
155
EXP. 94
273.
EXP. 95
P. 243.
EXP. 96
EXP. 97
EXP. 98-
EXP. 99
P. 645.
EXPS. 101
135.
EXP. 103 -
EXP. 104-
EXP. 105 -
EXP. 106 -
EXP. 107-
P. 181.
EXP. 108-
EXP. 109 -
P. 205.
EXP. 110
P. 248.
EXP. 111-
EXP. 112 -
P. 252.
EXP. 113
P. 252.
EXP. 114 -
EXP. 115-
P. 257.
EXP. 116-
EXP. 117 -
EXP. 118-
P. 267.
EXP. 119-
EXP. 120-
P. 192.
EXP. 121
Shep. P. 119 ; Att. P.
Shep. P. 122; Rem.
Shep. P. 130.
Shep. P. 132.
Shep. P. 133.
Shep. P. 135; Wag.
and 102 Shep. P.
Shep. P. 136.
Shep. P. 140.
Shep. P. 140 and 142.
Shep. P. 138.
Shep. P. 138; Rem.
Da. P. 36-7.
Shep. P. 146; Rem.
Shep. P. 158; Rem.
Rem. P. 249.
Shep. P. 158; Rem.
Shep. P. 160; Rem.
Shep. P. 163.
Shep. P. 164; Rem.
Shep. P. 166.
Shep. P. 173.
Shep. P. 197; Rem.
-Shep. P. 204-206.
-Shep. P. 211; Att.
Shep. P. 225.
EXP. 122 Shep. P. 225 ; Rem.
P. 365.
EXP. 123 Shep. P. 228.
EXP. 124 Shep. P. 229; Rem.
P. 341.
EXP. 125 Shep. P. 229.
EXP. 126 Shep. P. 233.
EXP. 127 Shep. P. 234.
EXP. 128 Shep. P. 235.
EXP. 129 Shep. P. 239.
EXP. 130 Shep. P. 242.
EXP. 131 Shep. P. 246; Rem.
P. 271.
EXP. 132 Shep. P. 252.
EXP. 133 Shep. P. 253.
EXP. 134 Shep. P. 259.
EXP. 135 Shep. P. 261; Rem.
P. 335.
EXPS. 136 and 137 Shep. P. 261.
EXP. 138 Shep. P. 281.
EXP. 139 Shep. P. 285.
EXP. 140 Shep. P. 285.
EXP. 141 Shep. P. 288.
EXP. 142 Shep. P. 289.
EXPS. 143 and 144 Shep. P.
292.
EXPS. 145 and 146 Shep. P.
294; Att. P. 231.
EXP. 147 Shep. P. 300.
EXP. 148 Shep. P. 312.
EXP. 149 Shep. P. 311.
EXP. 150 Shep. P. 313.
EXP. 152 Shep. P. 316.
EXP. 153 Shep. P. 321.
EXP. 154 Shep. P. 326.
EXP. 155 Shep. P. 328.
EXP. 156 Shep. P. 333.
156
APPENDIX.
TABLE OF WEIGHTS AND MEASURES.
ENGLISH WEIGHTS.
Avoirdupois Weight.
POUND.
OUNCES.
DRACHMS.
GRAINS
1
. . 16 . . ,
, . . 256 . .
7000
1
16
. . .437.5
1 . .
. 27.3495
1
GRAMMES.
453.5926
28.3495
1.7718
.0648
Troy Weight.
POUND.
1 .
OUNCES.
. . 12 .
PENNYWEIGHT.
. . . 240 . .
GRAINS.
. 5760 .
GRAMMES.
. . 373.2419
1
20
. 480 .
. . 31.1035
1
24 .
. . 1.5552
1 .
.0648
METRIC MEASURES.
Measures of Weight.
1 milligram (mg)
1 centigram (cg)
1 decigram (dg)
0.001 gram
0.010 gram
about -fa of grain.
gram
(g)
= 0.100 gram.
= 1.000 gram = 15.4323 grains.
1 liter ^
1 quart
1 meter (m)
1 inch
Equivalents.
= 1.0567 quarts.
= .9463 liters.
= 39.3708 inches.
= 2.54 centimeters (cm) .
APPENDIX.
157
A TABLE OF THE PRINCIPAL ELEMENTS.
ELEMENTS.
AT.
WT.
SYM.
VAL.
SP. G.
CONDITION.
g f Oxygen
16
O
2
1.105
Gas.
Jttj
Nitrogen
14
N
1,3,5
0.971
Gas.
t *-
Chlorine
35.5
Cl
1
2.45
Gas.
*
Bromine
79.8
Br
1
3.187
Liquid.
3
Iodine
126.6
I
1
4.948
Solid.
i
Fluorine
19
F
1
1.313
Gas.
o|
Carbon
12
C
4
3.S-.6
Solid.
i Jj
Sulphur
32
S
2,4
2.05
Solid.
"S.2
Phosphorous
31
p
3,5
1.83
Solid.
11
Arsenic
75
As
3,5
5.73
Solid.
* [_ Chromium
52.4
Cr
4,6
6.5
Solid.
Hydrogen
1
H
1
.069
Gas.
f Manganese
54
Mn
2,4,6
8.03
Solid.
fee
Boron
11
Bo
3
2.5?
Solid.
Lead
206.5
Pb
2,4
11.37
Solid.
5
Silver
107.7
Ag
1
10.53
Solid.
I
Mercury
200
Hg
1,2
13.55
Liquid.
S3
Magnesium
24
Mg
2
1.74
Solid.
X!
to
Tin
117.7
Sn
2,4
7.29
Solid.
1
Copper
63
Cu
1,2
8.95
Solid.
1
Iron
56
Fe
2,4
7.86
Solid.
I 1
Aluminum
27
Al
4
2.6
Solid.
1
Nickel
58
Ni
2,4
8.9
Solid.
o
Cobalt
59
Co
2,4
S.5-.7
Solid.
a
Zinc
65
Zn
2
7.15
Solid.
S
Barium
136.8
Ba
2
3.75
Solid.
"S
Strontium
87.4
Sr
2
2.54
Solid.
.2
Calcium
40
Ca
2
1.57
Solid.
1
"S
Potassium
39
K
1
.87
Solid.
s
Platinum
194.4
Pt
4
21.50
Solid.
^ Sodium
23
Na
1
.978
Solid.
158 APPENDIX.
LIST OF CHEMICALS AND APPARATUS
FOR THE COURSE.
Preparation of Reagents.
Aniline A few particles in H 2 to required color.
AgN0 3 1 g. of the crystal salt to 40 cc distilled
H 2 0.
Alcohol Use 95 %.
A1 2 K 2 (S0 4 ) 4 . .....1 g. to!0 cc .
BaCl 2 1 g. to!0 cc .
Ba(N0 3 ) 2 1 g. to!0 cc .
Ca(OH) 2 Digest slaked lime in H 2 0, and filter.
Co(]Sr03) 2 1 g. to 15 cc . Use the crys. salt.
Chlorine water .... Saturated solution of chlorine in H 2 0.
Protect from light.
Chloral Hydrate . . . 1 g. to 20 cc .
Cr 2 K 2 (S0 4 ) 4 Ig. to!0 cc .
CuS0 4 Ig. to!0 cc .
CoCl 2 Ig. to!0 cc .
C 2 H 4 2 30%. >
CaCl 2 1 g. to!0 cc .
CaS0 4 Saturated solution in H 2 0.
FeS0 4 Make up as needed with distilled H 2 O.
Fe 2 Cl 6 . 1 g. to 10 cc . Use crys. salt.
HC1, dil Beagent strength 1 to 4 by vol. Equiv.
to 8.5 % HC1.
HN0 3 dil 1 to 3 by vol. Equiv. to 20 % HN0 3 .
APPENDIX. 159
H 2 S0 4 , dil 1 to 5 by vol. Equiv. to 25 % H 2 S0 4 .
Pour the acid into the water care-
fully.
HgCl 2 Saturated Solution.
HgN0 3 1 g. to20 cc .
H 2 S Prepare as needed, using Kipp gene-
rator or equiv. with FeS and com-
mercial HC1 dil. 1 to 1 by vol.
H 3 As0 4 1 g. to50 cc .
KMn0 4 Strong sol. 1 g. to 10 cc ; or, better, a sat-
urated solution.
KMn0 4 , dil l cc of strong sol. to 200 cc H 2 0.
KI 1 g. to20 cc .
KOH Ig. to!0 cc .
KCy 1 g. to 10 c c . Use cold water. Does not
keep well.
KBr Ig. to20 cc .
K 2 O 2 7 1 g. to 10 cc . Use warm H 2 0.
K 4 FeCy c 1 g. to 15 CC .
KCyS 1 g. to!5 cc .
K 3 FeCy 6 Make up as needed, 1 g. to 15 c c . Does
not keep.
K 2 Cr0 4 Ig. to20 cc .
NaOH 1 g. to 10 c c . Allow to settle, and decant.
NH 4 OH Dilute cone. 1 to 3 by vol. Equiv. to
10% NH 3 .
NH 4 C1 Ig. to!0 cc .
Nad Ig. to!0 cc .
(NH 4 ) 2 C0 3 ........ 200 g. (NH 4 ) 2 C0 3 , 800 cc H 2 0, and
209 CC NH 4 OH.
(NH 4 ) 2 S Saturate KH 4 OH with H 2 S. Add
NH 4 OH to alkaline reaction.
(N"H 4 ) 2 S 2 Add a little flowers of sulphur to
(NH 4 ) 2 S.
160 APPENDIX.
......... lg. to20 cc .
MC1 2 ............ 1 g. to!0 cc .
Pb(C 2 H 3 2 ) 2 ...... lg. to20 cc .
Starch ........... Digest 1 spoonful in 300 c c cold water,
and boil.
SnCl 2 ............ Dissolve in least amount of hot cone.
Hl. Dilute with H 2 0, l cc to
20 c c , and keep in a bottle with a
piece of metallic tin.
SnCl 4 ............ Dissolve tin in aqua regia. Evaporate
to dryness. Make up 1 g. to 20 cc
or more dilute if desired.
SrCl 2 ............ 1 g. to!0 cc .
Sr(N0 3 ) 2 ......... lg. to!0 cc .
Touch Paper, made by dipping filter paper in strong solution
KN0 3 and drying.
ZnS0 4 ........... Saturated solution.
ZnCl 2 ............ 1 g- to 10 CC .
APPENDIX.
161
PURCHASING LIST.
Alcohol . . . ".
Ammonium Carbonate
Ammonium Hydrate, cone.
AS 2 3 . . . ; .
Borax .
Carbon Disulphide . ' .
Copper clippings
CuS0 4 . . . .
CaCl 2 '. . : .
CaO ...~ ...
CaF 2 .'. . '}. . ,
Cotton, common
Cotton, gun
Charcoal, powdered - ; .
Charcoal, sticks for blowpipe
Coal, bituminous . .
Ether ....
FeS0 4 .....
FeS, fused ....
HgO . . ' . . .
Hydrochloric Acid, C.P. Sp. G.
Hydrochloric Acid, com. Sp. G.
Iodine, sublimed
Iron Filings, very fine .
KNO,. . ...
KBr . . ; . . .
KI . \".
KC!0 3
1.20
1.20
Fou 20 PUPILS.
1 quart,
i pound.
4 pounds.
1 ounce.
pound,
i pound.
1 pound.
1 pound.
^ pound.
I pound.
1 pound.
2 ounces.
1 ounce.
\ ounce.
1 pound.
20.
^ pound.
1 pound.
^ pound.
1 pound.
pound.
6 pounds.
2 pounds.
ounce.
J pound.
pound.
2 ounces.
2 ounces.
2 pounds.
162
APPENDIX.
K 4 FeCy 6
Lead, metallic ......
Litmus Paper, red and blue
Mercury, metallic .....
Mn0 2
Magnesium Ribbon .....
Marble, White . . . . ;
Nad ; ." , ..' . . . .'-
NH 4 1TO 3 , anhydrous . . . .'
NH 4 C1. . '
NaC 2 H 3 2 .
Na 2 C0 3 . . - . . . ?. . - .
NaOH . . . ... .' . .
Nitric Acid, Sp. G. 1.42 . . .
Plaster of Paris . . .
Pb(NO,) a . . . V . . ;'.
PbS, powdered . . . . . .
Pbo . ;-. . . .
Phosphorus . . . . .
Potassium, metallic
Potassium Hydroxide, sticks
Platinum Wire, for blowpiping .
Platinum Foil . . . - t ' . . .
Starch . . . . . .
Sr(X0 3 ) 2
Sodium, metallic
Sulphur, roll . . .
Sulphur, flowers . .
Sulphuric Acid, Sp. G. 1.84 .
Sugar, granulated
Zinc, sheet
Zinc, granulated, made by pouring melted
lumps into H 2
ZnS, powdered .
^ pound,
i pound.
1 'sheet each.
1 pound.
pound.
^ ounce.
2 pounds.
1 pound.
2 pounds.
1 pound.
2 ounces.
1 pound.
pound.
3 pounds.
1 pound.
2 ounces.
1 ounce.
1 ounce.
1 ounce,
i ounce.
1 pound.
5 grams.
5 grams.
L pound.
% pound.
ounce.
J pound.
1 pound.
9 pounds.
1 pound.
1 pound.
2 pounds.
1 ounce.
Order Chemicals not otherwise specified in 1 ounce packages. Use
C. P. Chemicals and distilled water for solutions wherever possible.
APPENDIX. 163
Apparatus required for each Pupil.
1 Metric and English rule. 1 foot.
6 Test-tubes, g-"x6".
1 Rubber delivery tube.
1 Glass delivery tube.
1 Piece of window glass 2" square.
1 Piece of blue glass 2" square.
1 Evaporating dish.
1 Pair nippers.
1 Watch crystal, diameter 2",
1 Small microscope.
10 Filters, 5".
1 Funnel, 2f .
1 Glass rod.
1 Small magnet.
1 Tin-box cover.
1 Pneumatic trough.
4 Wide-mouth 4 oz. bottles.
Wide-mouth 1 oz. bottle.
Narrow-mouth 4 oz. bottle.
Foot No. 18 iron wire.
Foot fine iron wire.
Combustion spoon.
2 Pieces white cardboard, 2" square.
4 Pieces glass tubing, 4" diameter, ?>" long.
1 Glass tumbler.
1 Paraffin candle.
1 Lamp chimney, Argand.
1 Strip zinc, 4"xl".
1 Blowpipe.
1 Piece of wire gauze, 4" square, iron.
1 Tripod or ring stand.
1 Test-tube holder.
1 Wash bottle.
Assorted rubber stoppers and corks to fit bottles and test tubes.
YB 36031
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