CHEMISTRY RAAAAAAGE

If anybody could help me out with this... that'd be awesome.

Using the Ksp (1.8 x 10^-10) for PbCl2, calculate the molar solubility of PbCl2 in 1.0 M NaCl @ 25 C. Compare with the molar solubility of AgCl in 1.0 M NaCl. Which precipitates at a lower concentration of Cl-.

I'm assuming the latter part would Be AgCl, since it forms in a 1:1 ratio, rather then a 2:1 ratio. For the solubility of PbCl2, I get some bullshit 1.9652E-14. That can't be right...

This part should read:

Which precipitates at a lower concentration of Cl-?

Ur a dumbass lol
1st part
[Pb2+][Cl-]^2 = x(1M)^2 = Ksp of PbCl2,
so [Pb2+]=Ksp of PbCl2

which from examining Wikipedia for 5 seconds shows that it's not 1.8E-10 at all:
http://en.wikipedia.org/wiki/Solubility_equilibrium#Solubility_constants

2nd part, you need to know Ksp of AgCl, which apparently is closer to 1.8E-10.  But since it's again in 1M Cl- solution, the solubility of AgCl will just be Ksp of AgCl