# Chemistry

posted by
**Ash** on
.

A 25.00 mL sample of a clear saturated solution of PbI2 requires 14.3 mL of a certain AgNO3(aq) for its titration.

I^-(from satd PbI2)+ Ag^+(from AgNO3)= AgI(s)

So, this is where I am.

using the Ksp equation for PbI2:

7.1*10^-9=4x^3

solving for x gives me 0.00121

Giving the concentration for I = 0.00242mol/L

Times this by 25ml gives me moles...

This is where I'm stuck