Determine the molar solubility of Fe(OH)₂in pure water. K_sp for Fe(OH)₂ = 4.87 × 10^-17. A) 2.44 × 10^-17 mol L^-1 B) 1.62× 10^-17 mol L^-1 C) 4.03 × 10^-9 mol L^-1 D) 3.65 × 10^-6 mol L^-1 E) 2.30 × 10^-6 mol L^-1

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The molar solubility of Fe(OH)₂ can be calculated using the K_sp expression:K_sp = [Fe²⁺][OH^-]² = 4.87 × 10^-17Since Fe(OH)₂ dissociates into one Fe²⁺ ion and two OH^- ions, the molar solubility (s) can be expressed as:s = [Fe²⁺] = [OH^-]/2Substituting this into the K_sp expression, we get:K_sp = s(2s)² = 4s³Solving for s, we get:s = (K_sp/4)^1/3 = (4.87 × 10^-17/4)^1/3 = 2.30 × 10^-6 mol L^-1

Determine the Molar Solubility of Fe(OH)2 in Pure Water

Determine the Molar Solubility of Fe(OH)₂in Pure Water