Ksp = (Ba^2+)(F^-)^2
You know (F^-) = 1.5E-2 M
You know (Ba^2+) = 1/2 the F^-
Plug those into Ksp expression and solve for Ksp.
Suppose a saturated solution of barium fluoride contains 1.5 x 10 ^ -2 M of F-. What is the Ksp of BaF2.
I know that the balanced equation of this reaction is:
BaF2 (s) --> Ba2+ (aq) + 2F- (aq)
There is a 1:1 ratio between BaF2 and Ba2+ and there is a 1:2 ration between BaF2 and 2F-. I am unsure of how to work through this.
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