Additional Solubility Practice Problems
Write the solubility product constant expression for the following:
Mg(OH)2
Ca3(AsO4)2
SrCO3
Calculate the solubility product constant for copper (II) iodate, Cu(IO3)2. The solubility of copper
(II) iodate at room temperature in water is 0.13g/100mL. Answer: 1.2x10-7
3. One liter of water is able to dissolve 2.15x10-3 mol of PbF2. What is the Ksp for PbF2?
Answer: Ksp = 3.98x10-8
1.
a.
b.
c.
2.
4. What is the molar solubility of PbBr2 in water? The Ksp for lead (II) bromide is 6.3x10-6?
Answer: 0.0116M
5. 0.23M sodium sulfate solution is added to strontium sulfate solution. The Ksp for strontium
sulfate is 2.5x10-7.
a. What is the common ion in this example?
b. What is the molar concentration of the strontium ion before the addition of sodium
sulfate?Answer: 5x10-4 M
c. What is the molar concentration of the strontium ion after the addition of sodium sulfate?
Answer: 1.17x10-6 M
d. What would the concentration of strontium sulfate be in grams per liter after the addition
of sodium sulfate? Answer: 2.0x10-4g/L
6. From each of the following ion concentrations in a solution, predict whether a precipitate will
for in the solution:
a. Ba2+ = 0.02M, F- = 0.0015M; Ksp = 1.0x10-6 Answer: yes, ion of products = 4.5x10-6 > Ksp
value
b. Pb2+ = 0.025M, Cl- = 0.050 M; Ksp = 1.6x10-5 Answer: yes, ion of products = 6.25x10-5 > Ksp
value.
7. Will a precipitate of PbSO4 form if 100mL of 1.0x10-3 M Pb(NO3)2 solution is added to 100mL of
2.0x10-3 M MgSO4 solution? Ksp = 6.3x10-7. Answer: ion products = 5x10-7 < Ksp value, so no
precipitate.