Question

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
Sorry the question is What is the molarity of this AgNO3(aq)?
Never mind I got it, just divide by the other ml amount :)

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