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At 25 0C the solubility product constant, Ksp, for strontium sulfate, SrSO4, is 7.6 x 10-7....

At 25 0C the solubility product constant, Ksp, for strontium sulfate, SrSO4, is 7.6 x 10-7. The solubility product constant for strontium fluoride, SrF2, is 7.9 x 10-10.

(a) What is the molar solubility of SrSO4 in pure water at 25 0C?

(b) What is the molar solubility of SrF2 in pure water at 25 0C?

(c) An aqueous solution of Sr(NO3)2 is added slowly to 1.0 litre of a well-stirred solution containing 0.020 mole F- and 0.10 mole SO42- at 25 0C. (You may assume that the added Sr(NO3)2 solution does not materially affect the total volume of the system.)

  1. Which salt precipitates first?
  2. What is the concentration of strontium ion, Sr2+, in the solution when the first precipitate begins to form?

(d) As more Sr(NO3)2 is added to the mixture in (c) a second precipitate begins to form. At that stage, what percent of the anion of the first precipitate remains in solution?

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