Solubility Equilibrium

1. The K_sp of Ba(IO₃)₂ at 25 ^oC is 6.0x10^-10 . What is the molar solubility of Barium iodate in pure water? What are the concentrations of Ba⁺² and IO₃^-?

 ([IO₃^-1]= 1.06 x10^-3 M)

2. What is the molar solubility of AgI (K_sp = 8.3x10^-17 ) in .05 M NaI? At equilibrium what is the molar concentration of all ions in solution?

3. The molar solubility of CaF₂( K_sp = 3.9 x 10^-11 ) in pure water would be _______M.

answer 2x10^-4

4. What is the solubility of CaF₂ in 0.1 M NaF? (K_sp = 3.9 x10^-11 ).

answer to b s= 3.9x10^-9 M

5. It is desired to calculate the molar solubility of silver acetate (K_sp=2.3x10^-3 ) in a 0.9 M solution of sodium acetate. a) What is the reaction that takes place when silver acetate dissolves? b) What is the equilibrium expression for this reaction? c) If s is the molar solubility of silver acetate, what are the concentrations of silver ions and acetate ions in terms of s? d) Calculate the value of s? (acetate = AcO^-)