Calculate Solubility of Ions given Ksp

Question

The Ksp of PbCl₂ is 4.18⋅10^−13 M. Calculate the solubility of each ion in a saturated solution: (Pb^2+ and Cl^-)

I'm so confused on how to do this problem. Any help is appreciated.

Answer 1

PbCl₂(s) <==> Pb²⁺(aq) + 2Cl^-(aq)

Ksp = [Pb²⁺][Cl^-]²

4.18x10^-13 = (x)(2x)²

4x³ = 4.18x10^-13

x³ = 1.05x10^-13

x = 4.72x10^-5 M = solubility of PbCl₂