MgF2 ==> Mg^+2 + 2F^-
Ksp = (Mg^+2)(F^-)^2
Substitute 0.08 M for (Mg^+2) and solve for (F^-).
Calculate the molar solubility of MgF2 in 0.08M MgCl2 at 25 degrees C.
6 answers
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
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?
1 answer