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What is the solubility product of caf2 if 0.1 m ca2+ and 0.02 m f- are in solution just before precipitation occurs?
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What is the solubility product of caf2 if 0.1 m ca2+ and 0.02 m f- are in solution just before precipitation occurs?

User William Dan Terry
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1 Answer

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CaF₂ ↔ Ca²⁺ + 2 F⁻
Solubility product Ksp is the product of ions forming a sparingly soluble salt each ion raised to power equal its stoichiometric factor in balanaced equation.
So:
Ksp CaF₂ = [Ca²⁺] [F⁻]²
= (0.1) (0.02)² = 4.0 x 10⁻⁵
User Ophelie
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