Practice question
Question
For BaF₂(s) <=> Ba²⁺(aq) + 2F-(aq) , Ksp = 1.7 × 10⁻⁶ . In a 0.01 M NaF solution, what is [Ba²⁺] in a saturated solution?
Explanation
Ksp = [Ba²⁺][F-]² = 1.7 × 10⁻⁶ . [F-] = 0.01 + 2[Ba²⁺] ≈ 0.01 M (since [Ba²⁺ is small). [Ba²⁺] (0.01)² = 1.7 × 10⁻⁶ , [Ba²⁺] = (1.7 × 10⁻⁶/0.0001) = 1.7 × 10⁻² M .
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