Calculating Ksp for Iron(II) Hydroxide

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SUMMARY

The calculation of the solubility product constant (Ksp) for iron(II) hydroxide (Fe(OH)2) is based on its molar solubility of 3.65 x 10^-6 M. The correct formula for Ksp is Ksp = [Fe^2+][OH^-]^2. The accurate calculation involves substituting the molar solubility into the equation as Ksp = [3.65 x 10^-6 M] * (2*[3.65 x 10^-6 M])^2, which accounts for the stoichiometry of the dissociation reaction. The professor's assertion that the hydroxide concentration is equal to the iron concentration is incorrect.

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Homework Statement



A saturated solution of iron(II) hydroxide has a molar solubility of 3.65 x 10^-6 M. Calculate the Ksp for Fe(OH)2.

Homework Equations



Ksp = [A]^a^b

The Attempt at a Solution



Fe(OH)2 --> Fe^2+ + 2OH-

Ksp = [3.65 x 10^-6 M] * (2*[3.65 x 10^-6 M])^2

This, however, doesn't yield an answer. The professor's answer is equivalent to

[3.65 x 10^-6 M] * ([3.65 x 10^-6 M])^2

I'm assuming this is an error on his part because the concentration of hydroxide ions should be twice the concentration of iron ions, not the same.
 
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Your approach is the correct one.
 

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