Unit 8 – Equilibrium
Section 2 – Solubility Product Equilibrium
1. Write the expression for the solubility product constant for each of the following ionic
compounds:
a. Mn(CO3)
b. Hg(OH)2
c.
Cu3(PO4)2
2. What is the concentration of a saturated silver (I) acetate solution? Ksp(AgC2H3O2) = 1.94 x 10-3.
3. What is the concentration of a saturated lead chloride solution? Ksp(PbCl2) = 1.17 x 10-5.
4. I have discovered a new chemical compound with the formula A 2B. If a saturated solution of A2B has a
concentration of 4.35 x 10-4 M, what is the solubility product constant for A2B?
5. Solubility product constants are usually specified for 25 ºC. Why does the Ksp value for a chemical compound
depend on the temperature?
6. Calculate the Ksp for each of the salts whose solubility is listed below.
a. CaSO4 = 5.0 x 10-3 mol/L
c. AgC2H3O2 = 1.02 g/100 mL
b. MgF2 = 2.7 x 10-3 mol/L
7. Calculate the solubility in moles/L of each
a. AgCN Ksp = 2.0 x 10-12
b. BaSO4 Ksp = 1.5 x 10-9
d. SrF2 = 12.2 mg/100 mL
c.
Ag2S Ksp = 1.6 x 10-49
d. CaF2 Ksp = 4.9 x 10-11
8. This is a question from an actual AP test. Answer the following questions that realte to solubility of salts of
lead and barium.
a. A saturated solution is prepared by adding excess PbI2(s) to distilled water to form 1.0 L of solution at
25°C. The concentration of Pb2+(aq) in the saturated solution is found to be 1.3 × 10 −3 M. The chemical
equation for the dissolution of PbI2(s) in water is shown below.
PbI2(s) ←→ Pb2+(aq) + 2 I−(aq)
i.
Write the equilibrium-constant expression for the equation.
ii.
Calculate the molar concentration of I−(aq) in the solution.
iii.
Calculate the value of the equilibrium constant, Ksp.