Calculate the [Cl-] required to form each precipitate?

okay so the entire equation is:
AgNO3 + Pb(NO3)2 + 3 NaCl -- AgCl + PbCl2 + 3 NaNO3

The entire net is:
Ag+ + Pb2+ + 3 Cl- -- AgCl + PbCl2

I have 0.10M AgNO3, 0.20M Pb(NO3)2.
Ksp AgCl = 1.8 E-10
Ksp PbCl2 = 1.6 E-5

Question

Calculate the [Cl-] required to form each precipitate?

okay so the entire equation is:
AgNO3 + Pb(NO3)2 + 3 NaCl    -->    AgCl + PbCl2 + 3 NaNO3

The entire net is:
Ag+ + Pb2+ + 3 Cl-    -->    AgCl + PbCl2

I have 0.10M AgNO3, 0.20M Pb(NO3)2.
Ksp AgCl = 1.8 E-10
Ksp PbCl2 = 1.6 E-5

anonymous · Answer

I think I need an ICE chart?

thomaster · Answer

I had this kinda stuff at reaction kinetics last year. I hated it so i didn't remember a lot XD I would need to read all stuff from last year again and i don't have time for that now Maybe this will help: http://chemwiki.ucdavis.edu/Physical_Chemistry/Chemical_Equilibrium/Le_Chatelier's_Principle/Ice_Tables

anonymous · Answer

thanks xD

anonymous · Answer

So how did you end up doing it?