What is the solubility product of CaF2 if 0.1 M Ca2+ and 0.02 M F- are in solution just before precipitation occurs?


4.0 × 10^-5

The solubility product cannot be determined.

1.6 × 10^-4

2.0 × 10^-3

2 answers

.....................CaF2 ==> Ca^2+ + 2F^-

Write the Ksp expression for CaF2, the problem gives you the value for Ca^2+ and for F^-, cubstitute those values and solve for Kp. NOTE: The problem tells you that the (F^-) is 0.02M. Do NOT mutiply that by 2.
It's 4.0 × 10^-5