flinnsci.com SAFETY REFERENCE PREPARATION OF SIMPLE INORGANIC SALT SOLUTIONS
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Preparation of Simple Inorganic Salt Solutions
Name / Formula / F.W. Concentration g/L
Aluminum chloride 0.2 M 48.3 g
AlCl3 • 6H2O 0.05 M 12.1 g
241.43
Aluminum nitrate 0.1 M 37.5 g
Al(NO3)3 • 9H2O
375.13
Aluminum sulfate 0.1 M 66.6 g
Al2(SO4)3 • 18H2O
666.42
Ammonium acetate 1.0 M 77.1 g
NH4C2H3O2 0.1 M 7.7 g
77.08
Ammonium chloride 1.0 M 53.5 g
NH4Cl 0.5 M 26.7 g
53.49
Ammonium nitrate 1.0 M 80.0 g
NH4NO3 0.5 M 40.0 g
80.04 0.1 M 8.0 g
Ammonium sulfate 0.1 M 13.2 g
(NH4)2SO4
132.1
Barium chloride 0.1 M 24.4 g
BaCl2 • 2H2O
244.28
Barium hydroxide 0.1 M 31.5 g
Ba(OH)2 • 8H2O
315.50
Barium nitrate 0.5 M 130.7 g
Ba(NO3)2 0.1 M 26.1 g
261.35
Bismuth nitrate 0.1 M 48.5 g in
Bi(NO3)3 • 5H2O 500 mL 6M
485.1 HNO3*
Name / Formula / F.W. Concentration g/L
Bismuth trichloride 0.2 M 63.1 g in
BiCl3 500 mL 3M
315.34 HCl*
Cadmium chloride 0.1 M 22.8 g
CdCl2 • 21⁄2H2O
228.34
Cadmium nitrate 0.1 M 30.8 g
Cd(NO3)2 • 4H2O
308.49
Calcium acetate 0.5 M 88.1 g
Ca(C2H3O2)2 • H2O 0.1 M 17.6 g
176.19
Calcium chloride 1.0 M 147.0 g
CaCl2 • 2H2O 0.1 M 14.7 g
147.02
Calcium hydroxide saturated 2 g†
Ca(OH)2
74.10
Calcium nitrate 0.5 M 118.1 g
Ca(NO3)2 • 4H2O 0.1 M 23.6 g
236.16
Chromium(III) chloride 0.1 M 26.6 g
CrCl3 • 6H2O
266.48
Chromium(III) nitrate 0.1 M 40.0 g
Cr(NO3)3 • 9H2O
400.18
Cobalt(II) chloride 0.1 M 23.8 g
CoCl2 • 6H2O
237.95
Cobalt(II) nitrate 0.1 M 29.1 g
Co(NO3)2 • 6H2O
291.05
Copper(II) chloride 0.5 M 85.2 g
CuCl2 • 2H2O 0.1 M 17.0 g
170.49
Copper(II) nitrate 0.5 M 120.8 g
Cu(NO3)2 • 3H2O 0.1 M 24.2 g
241.6
Copper(II) sulfate 1.0 M 249.7 g
CuSO4 • 5H2O 0.5 M 124.8 g
249.69
Iron(II) sulfate 0.01 M 2.8 g and
FeSO4 • 7H2O 1 mL conc.
278.03 H2SO4*
Iron(III) chloride 1.0 M 270.3 g
FeCl3 • 6H2O 0.1 M 27.0 g
270.32
Iron(III) nitrate 0.1 M 40.4 g
Fe(NO3)3 • 9H2O
404.00
* Add solid to acid solution, stir, then add to water. Dilute to 1 L. Remember, always add
acid to water.
† Approximate amount for 1 L of saturated solution. Keep adding solute until it no longer
dissolves; stir for 1 hour, then filter.
PREPARATION OF SIMPLE INORGANIC SALT SOLUTIONS
continued on next page.
Normality: A concentration unit (N); defined as the number of equivalents of
solute per liter of solution (e.g., 1 M H2SO4 = 2 N H2SO4).
Saturated Solution: A solution that contains the maximum
amount of a particular
solute that will dissolve at that temperature.
Solute: The substance that is dissolved or has gone into solution (typically
a solid).
Solution: A uniform homogeneous mixture of two or more substances. The
individual substances may be present in varying amounts.
Solvent: The substance which does the dissolving (typically a liquid, such as
water or alcohol). Must be greater than 50% of the solution.
Standard Solution: A very precise solution, usually to 3–4 significant figures,
used in quantitative analysis or an analytical procedure.
Supersaturated Solution: A solution that contains more solute than
equilibrium conditions allow; it is unstable and the solute may precipitate
upon slight agitation or addition of a single crystal.
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