Concentrations of Pb2+ and Cl2 at equilibrium

[magma_saber]

Homework Statement

A solution is prepared by mixing 50.0 mL of 0.36 M Pb(NO3)2 with 50.0 mL of 1.7 M KCl. Calculate the concentrations of Pb2+ and Cl2 at equilibrium. Ksp for PbCl2(s) is 1.6 x 10-5.

Homework Equations

I think its Ksp = [Pb(NO₃)2][KCl]²

Pb(NO₃)2 = 0.018 mol
KCl = 0.085 mol

Is this right? what do i solve for?

 

[Borek]

Your Ksp is wrong. It should be made of ions concentrations.

Otherwise it is limiting reagent question. Once everything precipitates out, you will be left with the excess of one of the ions involved. Use this concentration to calculate concentration of the other using (correct) Ksp formula.