Question

The Ksp for a certain metal hydroxide, M(OH)2 (molar mass = 127) is 3.5 × 10-19. What is the pH for a saturated solution of this hydroxide?

Confused on how to set up this problem...

Answer 1

M(OH)2 ==> M^+2 + 2OH^-
Set up an ICE chart and substitute
Ksp = (M^+2)(OH^-)^2
Ksp = (x)(2x)^2 = 3.5E-19
Solve for x. 2x = (OH^-) then convert to pOH, finally to pH. I get something like 7.6 or so.

Answer 2

Thanks a lot man!