A solution contains 1.0 x 10^-4 M Cu2+ and 2.0x10^-3 Pb2+ (Ksp (PbI2) = 1.4x10^-8, Ksp(CuI)=5.3x10^-12...?
A solution contains 1.0 x 10^-4 M Cu2+ and 2.0x10^-3 Pb2+ (Ksp (PbI2) = 1.4x10^-8, Ksp(CuI)=5.3x10^-12. If solid NaI is slowly added to this solution
A)Will PbI2 (s) or CuI(s) precipitate first?
If solid NaI (s) is added...do I need to find what the Qsp and Ksp of I are?
B)At what [I-] will Pb2+ begin to precipitate?
A precipitate forms when Qsp = Ksp, so do I solve for [I-]? How does it look?
C)At what [I-] will Cu+ begin to precipitate?
D)When PbI2 just begins to precipitate from solution, what concentration of Cu+ remains in solution?
I don't get this one >.<
How do I do these problems? Any direction will be appreciated