At 22 °C an excess amount of a generic metal hydroxide M(OH)2, is mixed with pure water. The resulting equilibrium solution has a pH of 10.56. What is the Ksp of the compound at 22 °C?

I have found my [OH-] concentration (3.63x10^-4) but I'm not sure I'm setting up my ICE table or my Ksp expression right:

M(OH)2 ---> M^2+ + 2OH^-
excess 0 2(3.63x10^-4)
+x +x
less x (7.26x10^-4)x

Ksp = [M][OH^-]^2

=(x)(7.26x10^-4x +x)

Not real sure where to go from here...
Thank you for any guidance!

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  1. Your 3.63E-4 = (OH^-) is correct but your ICE table needs some work.
    ..........M(OH)2 ==> M^2+ + 2OH^-
    [note: If the pH is 10.58 and OH^- = 3.63E-4, then that's what OH IS. It isn't 2 times that. So
    Ksp =- (M^2+)(OH^-)^2
    (M^2+) = 1/2 x 3.63E-4 = 1.82E-4
    (OH^-) = 3.63E-4
    Substitute into Ksp expression and solve for Ksp.

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  2. Oh geez, thank you SO much! And so quick!

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  3. How did you find the concentration of [OH-]

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  4. 14-pH = pOH

    From the pOH, you can calculate [OH-] raising 10 to the opposite pOH power.


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  5. why is OH/2 of M^2+

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