[QT_PI]

Please help me with another problem. Your input will be greatly appreciated

A solution containin .10 M Cl^- and .10 M PO₄^3- is to be traken through the process of fractional precipitaion by the addition of the Ag⁺ ion.
The Ksp of AgCl = 1.6x10^-10 and Ksp of Ag₃PO₄ = 1.8x10^-18

a) Calculate the [Ag⁺] required to initiate the precipitation of AgCl
b) Calculate the [Ag⁺] required to initiate the precipitation of Ag₃PO₄
c) Calculate the % Cl^- ion left in solution at the highest concentration of Ag+ ion that wont bring on the precipiation of Ag₃PO₄
d) Calculate the molar solubility of both compounds using the given Ksp values.

[Mitch]

You have to show some work, why don't you start by writing the balanced chemical equation.