How Much Metallic Ion Can Remain at Equilibrium in Fe(OH)3 Solution?

Thread starter haber101
Start date Apr 5, 2010
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Equilibrium Ion

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To determine the milligrams of metallic ion (Fe3+) that can remain at equilibrium in a solution of Fe(OH)3 with a hydroxide ion concentration of [OH-] = 1.0 x 10^-4 mol/L and a solubility product constant (Ksp) of 6.0 x 10^-38, it is essential to first calculate the concentration of Fe3+ ions. The Ksp expression for Fe(OH)3 is given by Ksp = [Fe3+][OH-]^3. By substituting the known [OH-] value into this equation, the concentration of Fe3+ can be derived. However, without the volume of the solution, it is not possible to convert this concentration into a mass measurement in milligrams. Thus, while the concentration of Fe3+ can be calculated, the lack of volume information prevents the calculation of the total mass of Fe3+ present in the solution.

Apr 5, 2010

haber101

Calculate the milligrams of metallic ion that can remain at equilibrium in a solution of Fe(OH)3 having a [OH-] = 1.0 x 10-4 mol/L and Ksp = 6.0 x 10-38.

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Apr 5, 2010

PhaseShifter

You're missing some important information, like the volume of solution.

It's possible to calculate the concentration of Fe³⁺ from that information, but not the mass.

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