Question

Calculate the molar solubility of MgF2 in 0.08M MgCl2 at 25 degrees C.
MgF2 ==> Mg^+2 + 2F^-

Ksp = (Mg^+2)(F^-)^2
Substitute 0.08 M for (Mg^+2) and solve for (F^-).
do I use the Ksp of MfF2 and plug it in the equation?
Yes.
from the equation:

Ksp=(.08M)(F^-)^2

there are two unknown how do we solve it

you have to find the Ksp in the back of your chemistry book.
the value 3.0x10^-5 was wrong for me?

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