Calculating Ksp for Iron(II) Hydroxide

In summary, the formula for calculating Ksp of Fe(OH)2 is [Fe2+][OH-]^2, where [Fe2+] is the molar concentration of Fe2+ ions and [OH-] is the molar concentration of hydroxide ions. The molar concentration of Fe2+ ions can be found by dividing the number of moles of Fe2+ ions by the volume of the solution in liters. Similarly, the molar concentration of hydroxide ions can be found by dividing the number of moles of hydroxide ions by the volume of the solution in liters. The solubility product constant (Ksp) is a measure of the maximum amount of a compound that can dissolve in
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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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  • #2
Your approach is the correct one.
 

FAQ: Calculating Ksp for Iron(II) Hydroxide

What is the formula for calculating Ksp of Fe(OH)2?

The formula for calculating Ksp of Fe(OH)2 is [Fe2+][OH-]^2, where [Fe2+] is the molar concentration of Fe2+ ions and [OH-] is the molar concentration of hydroxide ions.

How do you find the molar concentration of Fe2+ ions?

The molar concentration of Fe2+ ions can be found by dividing the number of moles of Fe2+ ions by the volume of the solution in liters.

How do you determine the molar concentration of hydroxide ions?

The molar concentration of hydroxide ions can be found by dividing the number of moles of hydroxide ions by the volume of the solution in liters.

What is the significance of Ksp in relation to Fe(OH)2?

Ksp, or the solubility product constant, is a measure of the maximum amount of a compound that can dissolve in a solution. In the case of Fe(OH)2, Ksp represents the equilibrium constant for the dissociation of Fe(OH)2 into Fe2+ and OH- ions.

How does temperature affect the calculation of Ksp for Fe(OH)2?

The value of Ksp for Fe(OH)2 is dependent on temperature. As the temperature increases, the solubility of Fe(OH)2 increases, leading to a higher value for Ksp. Therefore, when calculating Ksp for Fe(OH)2, it is important to take into account the temperature of the solution.

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