Any help would be greatly appreciated, not quite sure how to workout this proble

Question

Any help would be greatly appreciated, not quite sure how to workout this problem....does anyone mind walking me through it? Lifesaver of course. Thank you!!

A solution contains Ca2+ and Pb2+ ions, bothat a concentration of 0.010 M. The two ions can be separated byprecipitating one but not the other usingNa2SO4 as the precipitating agent. What isthe concentration that remains of the first ion that precipitatesjust before the second, more soluble ion begins to precipitate?Ksp(CaSO4) = 9.1 x 10-6 andKsp(PbSO4) = 1.6 x 10-8

Explanation / Answer

This is a trick question                                 Here, we use the result :                Ksp(CaSO4) =[Ca+2][SO4-2]                      Ksp(PbSO4) =[Pb+2][SO4-2]                         Since Ksp(PbSO4) is lower , it precipitatesfirst.                             Thus, till that point is reached all the [Ca+2] remainsin solution .                     Therefore, concentration of first ion, Ca+2 = 0.01 M

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