The molar solubility of CaF₂ is 2.15 × 10^-4 M in pure water.Calculate the K_sp for CaF₂. A) 1.63 × 10^-12 B) 8.05 × 10^-9 C) 3.97 × 10^-11 D) 4.47 × 10^-12 E) 5.31 × 10^-10

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Quizplus · Accepted Answer

The dissolution of CaF2 in water is represented by the equation: CaF2 ⇌ Ca²⁺ + 2F⁻. The molar solubility of CaF2 is 2.15 × 10⁻⁴ M, so [Ca²⁺] = 2.15 × 10⁻⁴ M and [F⁻] = 2 × 2.15 × 10⁻⁴ M = 4.30 × 10⁻⁴ M. The Ksp is calculated as [Ca²⁺][F⁻]² = (2.15 × 10⁻⁴)(4.30 × 10⁻⁴)² = 3.97 × 10⁻¹¹.

The Molar Solubility of CaF2 Is 2

The Molar Solubility of CaF₂ Is 2