Solubility Equilibrium: Worksheet #3
1. Ksp for AgBr is 1.0 x 10-13. How many moles of AgBr will dissolve in 1.0 L of 0.020 M KBr solution?
2. Ksp for AgCl is 1.6 x 10-10. How many moles of AgCl will dissolve in 5.0 L of 0.010 M NaCl solution?
3. Ksp = 1.1 x 10-8 for PbSO4. If 5.0 x 10-6 mol of PbSO4 can dissolve in 1.0 L of a K2SO4 solution, what is the
molar concentration of the K2SO4 solution?
4. Ksp = 1.4 x 10-7 for Cu(IO3)2. If 2.0 x 10-5 mol of Cu(IO3)2 can dissolve in 2.0 L of a NaIO3 solution, what is
the molar concentration of the NaIO3 solution?
5. Powdered AgOH is slowly added to 2.0 L of a 0.020 M solution of NaOH until no more AgOH will dissolve.
If Ksp = 1.4 x 10-8 for AgOH:
a. what is [Ag+] in the saturated solution?
b. what mass of AgOH had to be added to the solution to produce this concentration of Ag+?
6. When excess Ag2CO3 is shaken with 1.00 L of 0.0100 M K2CO3, 6.84 x 10-3 g of Ag2CO3 dissolve. Calculate
the solubility product constant (Ksp) of Ag2CO3.
7. Ksp for BaSO4 is 1.5 x 10-9. If BaSO4 is added to a solution of K2SO4, the solubility of the BaSO4 is
2.0 x 10-7 M. What is the concentration of the K2SO4 solution?
8. A solution contains 0.020 mol of (NH4)2S. How many grams of MnS must be added to 1.0 L of the solution
to just start forming a precipitate of MnS? Ksp = 1.4 x 10-15 for MnS.
9. Silver oxide dissolves according to the reaction:
Ag2O + H2O
2 Ag+ + 2 OHIf Ksp = [Ag+][OH-] = 2.0 x 10-8 for AgOH, how many moles of Ag2O will dissolve in 2.0 L of a solution having
[OH-] = 1.0 x 10-3 M?
10. Ksp = 3.7 x 10-15 for Al(OH)3. A precipitate just began to form when 50.0 mL of 2.0 x 10-6 M Al(OH)3 was
mixed with 50.0 mL of NaOH solution. What was the concentration of the NaOH solution?
11. What is the solubility (expressed in grams per litre) of Mg(OH)2 in 0.050 M MgSO4. Ksp for Mg(OH)2 is
1.2 x 10-12.
Challenge:
12. Ksp = 1.08 x 10-10 for BaSO4 and Ksp = 1.73 x 10-6 for BaF2. Ba2+ ions are added to a solution which is
0.0100 M in Na2SO4 and 0.0100 M in NaF until 50% of the F- has been precipitated. What is [SO42-] after
the addition of the Ba2+?
13. A 1.00 L solution contained a small amount of FeC2O4 and Fe(OH)2 such that no undissolved solid was
present. The concentration of OH- in the solution was one-half that of the C2O42-. The addition of
Fe(ClO4)2(s) to the solution caused FeC2O4 and Fe(OH)2 to precipitate simultaneously. What was the
concentration of the FeC2O4 in the original solution? Ksp = 2.10 x 10-7 for FeC2O4; Ksp = 1.64 x 10-14 for
Fe(OH)2.