Solubility Unit Problems Worksheet 1. Calculate the Ksp for each of the salts whose solubility is listed below. a) CaSO4 = 5.0 x 10-3 mol/L b) MgF2 = 2.7 x 10-3 mol/L c) AgC2H3O2 = 1.02 g/100 mL d) SrF2 = 12.2 mg/100 mL 2. Calculate a) the solubility in moles/L of each of three salts and  b) the concentration of the cations in mg/mL in each of the saturated solutions. i) AgCN Ksp = 2.0 x 10-12 ii) BaSO4 Ksp = 1.5 x 10-9 iii) FeS Ksp = 3.7 x 10-19 iv) Mg(OH)2 Ksp = 9.0 x 10-12 v) Ag2S Ksp = 1.6 x 10-49 vi) CaF2 Ksp = 4.9 x 10-11 3. Consider these slightly soluble salts: i) PbS Ksp = 8.4 x 10-28 ii) PbSO4 Ksp = 1.8 x 10-8 iii) Pb(IO3)2 Ksp = 2.6 x 10-13 a) Which is the most soluble? b) Calculate the solubility in moles/L for PbSO4. c) How many grams of PbSO4 dissolve in 1 L of solution? d) How can you decrease the concentration of Pb2+(aq) in a saturated solution of PbSO4 solution? e) What is the concentration in moles/L of PbS in a saturated solution of the salt? 4. For each of these substances, calculate the milligrams of metallic ion that can remain at equilibrium in a solution having a [OH-] = 1.0 x 10-4 mol/L. a) Cu(OH)2 Ksp = 1.6 x 10-9 b) Fe(OH)3 Ksp = 6.0 x 10-38 c) Mg(OH)2 Ksp = 6.0 x 10-12