flinnsci.com SAFETY REFERENCE PREPARATION OF SIMPLE INORGANIC SALT SOLUTIONS
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Preparation of Simple Inorganic Salt Solutions, continued
Name / Formula / F.W. Concentration g/L
Potassium chromate 1.0 M 194.2 g
K2CrO4 0.5 M 97.1 g
194.21 0.1 M 19.4 g
Potassium dichromate 0.1 M 29.4 g
K2Cr2O7
294.22
Potassium ferricyanide 0.5 M 164.6 g
K3Fe(CN)6 0.1 M 32.9 g
329.26
Potassium ferrocyanide 0.1 M 42.2 g
K4Fe(CN)6 • 3H2O
422.41
Potassium hydrogen 0.1 M 20.4 g
phthalate
KHC8H4O4
204.23
Potassium hydroxide see page 1212
Potassium iodate saturated 214.0 g†
KIO3 0.2 M 42.8 g
214.01 0.1 M 21.4 g
Potassium iodide 1 M 166.0 g
Kl 0.5 M 83.0 g
166.01 0.2 M 33.2 g
Potassium nitrate 0.5 M 50.6 g
KNO3 0.1 M 10.1 g
101.11
Potassium permanganate 0.2 M 31.6 g
KMnO4 0.1 M 15.8 g
158.04 0.01 M 1.6 g
Potassium phosphate, 0.1 M 13.6 g
monobasic
KH2PO4
136.09
Potassium phosphate, 0.1 M 17.4 g
dibasic
K2HPO4
174.18
Name / Formula / F.W. Concentration g/L
Potassium phosphate, 0.1 M 21.2 g
tribasic
K3PO4
212.27
Potassium sulfate 0.5 M 87.1 g
K2SO4 0.1 M 17.4 g
174.27
Potassium thiocyanate 1.0 M 97.2 g
KSCN 0.5 M 48.6 g
97.18 0.1 M 9.7 g
Silver nitrate 0.5 M 84.9 g
AgNO3 0.1 M 17.0 g
169.87
Sodium acetate 1 M 136.1 g
NaC2H3O2 • 3H2O 0.5 M 68.0 g
136.08
Sodium bicarbonate 0.5 M 42.0 g
NaHCO3 0.1 M 8.4 g
84.01
Sodium borate 4 % 40.0 g
Na2B4O7 • 10H2O
381.42
Sodium bromide 1.0 M 102.9 g
NaBr 0.1 M 10.3 g
102.90
Sodium carbonate saturated 214.0 g†
Na2CO3 1.0 M 106.0 g
105.99 0.1 M 10.6 g
Sodium carbonate 1.0 M 124.0 g
Na2CO3 • H2O 0.1 M 12.4 g
124.00
* 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.
Nitrates (NO3
General Solubility Rules for Inorganic Compounds
–): All nitrates are soluble.
Acetates (C2H3O2
–): All acetates are soluble; silver acetate is moderately
soluble.
Bromides (Br–), Chlorides (Cl–) and Iodides (I–): Most are soluble except for
salts containing silver, lead and mercury.
Sulfates (SO42–): All sulfates are soluble except barium and lead. Silver,
mercury(I) and calcium are slightly soluble.
Hydrogen sulfates (HSO4
–): The hydrogen sulfates (aka bisulfates) are more
soluble than the sulfates.
Carbonates (CO32–), phosphates (PO43–), chromates (CrO42–) and silicates
(SiO42–): All carbonates, phosphates, chromates and silicates are insoluble,
except those of sodium, potassium and ammonium. An exception is MgCrO4,
which is soluble.
Hydroxides (OH–): All hydroxides (except lithium, sodium, potassium, cesium,
rubidium and ammonium) are insoluble; Ba(OH)2, Ca(OH)2 and Sr(OH)2 are
slightly soluble.
Sulfides (S2–): All sulfides (except sodium, potassium, ammonium, magnesium,
calcium and barium) are insoluble. Aluminum and chromium sulfides are
hydrolyzed and precipitate as hydroxides.
Sodium (Na+), potassium (K+) and ammonium (NH4
+): All sodium, potassium,
and ammonium salts are soluble (except some transition metal compounds).
Silver (Ag+): All silver salts are insoluble. Exceptions are AgNO3 and AgClO4.
AgC2H3O2 and Ag2SO4 are moderately soluble.
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