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