A solution contains 1 molar each of M²⁺ and X³⁺ ions. NaOH is added gradually to this solution. Which of the following statements is correct about precipitation of M(OH)₂ and X(OH)₃?
[Given: Ksp [M(OH)₂] = 4 × 10-10 ; Ksp [X(OH)₃] = 2.7 × 10-14]
M(OH)₂ will precipitate first as it requires 3 × 10-5 M OH- ion concentration for saturation.
X(OH)₃ will precipitate first as it requires 2 × 10-5 M OH- ion concentration for saturation.
X(OH)₃ will precipitate first as it requires 3 × 10-5 M OH- ion concentration for saturation.
M(OH)₂ will precipitate first as it requires 2 × 10-5 M OH- ion concentration for saturation.
For precipitation of M(OH)₂ → M(OH)₂ ⇌ M²⁺ + 2OH⁻
Ksp = [M²⁺][OH⁻]² = 4 × 10⁻¹⁰
[OH⁻] = 2 × 10⁻⁵ M
For precipitation of X(OH)₃ → X(OH)₃ ⇌ X³⁺ + 3OH⁻
Ksp = [X³⁺][OH⁻]³ = 2.7 × 10⁻¹⁴
[OH⁻] = 3 × 10⁻⁵ M M(OH)₂ will precipitate first as it requires less concentration of OH⁻ ion
Consider the following two statements for the given equilibrium Fe³⁺(aq) + SCN⁻(
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