Calculate the molar solubility of () in a solution of . — Ionic Equilibrium Chemistry Question
Question
Calculate the molar solubility of $CaF_2$ ($K_{sp} = 5.3 \times 10^{-11}$) in a $0.1 \text{ M }$ solution of $NaF$.
Answer: A
💡 Solution & Explanation
In $0.1 \text{ M } NaF$, $[F^-] \approx 0.1 \text{ M}$. $K_{sp} = [Ca^{2+}][F^-]^2 = S \times (0.1)^2 = 5.3 \times 10^{-11}$. $S = 5.3 \times 10^{-11} / 0.01 = 5.3 \times 10^{-9} \text{ M}$.
💬Ask on WhatsApp →
Still have doubts about this question?
Send it to our AI chemistry tutor on WhatsApp — gets answered in minutes