So the question goes
"What are the equilibrium concentrations of Pb2+ and F- in a saturated solution of lead fluoride if the Ksp of PbF2 is 3.2*10^-8"
So I used the formula
(x)(2x)^2 = 3.2 *10^-8
4x^3 = 3.2 *10^-8
I solved for .002. Which IS the correct conc. for Pb2+.
However I am unable to find the conc. for F-. Help?
If 0.002 mole/L of PbF2 dissolves, the concentration of Pb^+2 will be 0.002 mole/L and the concentration of F^-1 must be 0.004 mole/L (2 x 0.002 = 0.004)