Solubility Product Practice Problems

  1. A saturated solution of calcium fluoride CaF2 in water on analysis was found to contain at 298 K 1.7 x 10-3 g per 100 cm3. Calculate the solubility product.
  1. The solubility of silver chromate Ag2CrO4 is 8.0 x 10-5 mol L-1. Calculate the solubility product.
  1. Complete the statement. If solubility of Al2(SO4)3 is x its solubility product would be
  1. Calculate the solubility product of AgCl, if the solubility of the salt in saturated solution at 298 K is 0.00198 gL-1.
  1. Differentiate between solubility product and solubility
  1. What is the difference between ion product and solubility product?
  1. What are the conditions for the precipitation of a salt from its aqueous solution?
  1. What are some of the conditions for the dissolution of an electrolyte in aqueous solution?
  1. What is a sparingly soluble salt?
  1. Differentiate between strong and weak electrolytes?
  1. What is “Common ion” effect? Give some of its applications.
  1. Write Ksp expressions for the following sparingly soluble salts BaCrO4, Mg(OH)2, PbCl2, Ag2CrO4 etc.
  1. The solubility product of AgCl is 1.5 x 10-10. Predict whether there will be any precipitation by mixing 50 ml of 0.01M NaCl and 0.01 M AgNO3 solution.
  1. Equal volumes of 25.0 ml of 5.0 x 10-2 M Ba(NO3)2 M NaF solution are mixed. Predict, whether precipitation of BaF2 will be formed or not Ksp for BaF2 is 1.7 x 10-6 at 298 K