An aqueous solution contains 0010 M Br and 0010 M I If Ag is

An aqueous solution contains 0.010 M Br and 0.010 M I-. If Ag+ is added until AgBr(s) just begins to precipitate, what are the concentrations of Ag+ and I-? (Ksp of AgBr = 5.4x10^-13, Ksp of AgI= 8.5x10^-17)

I have the answer already, I just want to know the steps to solve the problem. Thank you.

Solution

Ag+ + Br- ------> AgBr

Ksp1 = [Ag+][Br-] = 5.4*10^-13

[Ag+] = 5.1*10^-11 M...................ans

Ag+ + I- ------> AgI

Ksp2 = [Ag+][I-]= 8.5*10^-17

[I-] = 1.57*10^-6 M..................................ans