The hydroxide ion concentration of a saturated solution of Fe(OH)₂ is $1.16 \times 10 ^ { - 5 }$ M. What is the solubility product constant for Fe(OH)₂?

Question

Quizplus · Accepted Answer

The solubility product constant $K_{sp}$ for Fe(OH)$_2$ is calculated using the formula $K_{sp} = [Fe^{2+}][OH^-]^2$. Given $[OH^-] = 1.16 \times 10^{-5}$ M, $[Fe^{2+}] = \frac{1.16 \times 10^{-5}}{2}$ M. Thus, $K_{sp} = \left(\frac{1.16 \times 10^{-5}}{2}\right)(1.16 \times 10^{-5})^2 = 7.9 \times 10^{-16}$.

The Hydroxide Ion Concentration of a Saturated Solution of Fe(OH)2 1.16×10−51.16 \times 10 ^ { - 5 }1.16×10−5

The Hydroxide Ion Concentration of a Saturated Solution of Fe(OH)₂ $1.16 \times 10 ^ { - 5 }$