Chemistry College

Calculate the molar solubility of iron(II) hydroxide, Fe(OH)2, in a solution buffered at a pH of
13.15. The Ksp of Fe(OH)2 is 1.6 × 10−14.

Answers

Answer 1

The solubility of solute in a solution can be find out from the solubility constant Ksp and molar concentrations. The solubility of iron hydroxide in the solution is 3.19 ×10 ⁻¹⁶ M.

What is solubility?

Solubility of substance is the fraction of its concentration which dissolves in a solvent at a specific temperature. The solubility constant Ksp is the product of molar concentrations of the ions in the solute.

It is given that the pH of the solution is 13.15. Thus, pOH = 14 -13.15 = 0.85.

[OH-] = Antilog (pOH) = antilog (0.85)

         = 7.07 M.

The solute Fe(OH)₂ dissociates into Fe²⁺ ion and 2 OH- ions. Let s be the solubility of one mole of ion. Thus [Fe²⁺] = s. Then, the Ksp can be written as follows:

Ksp = [Fe²⁺] [OH-]²

 1.6 × 10⁻¹⁴  = s  × [7.07 M]²

   s =   1.6 × 10⁻¹⁴/[7.07 M]²

      =  3.19 ×10 ⁻¹⁶ M.

Therefore, the molar solubility of iron(II) hydroxide in the given solution is  3.19 ×10 ⁻¹⁶ M.

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