When of () is added to of a saturated solution of (), what is the resultant concentration of in the — Ionic Equilibrium Chemistry Question
Question
When $0.1 \text{ mol}$ of $CuCl$ ($K_{sp} = 1.0 \times 10^{-6}$) is added to $1 \text{ L}$ of a saturated solution of $AgCl$ ($K_{sp} = 1.6 \times 10^{-10}$), what is the resultant concentration of $Ag^+$ in the solution?
Answer: B
💡 Solution & Explanation
$CuCl$ provides $[Cl^-] = \sqrt{10^{-6}} = 10^{-3} \text{ M}$. Since $K_{sp}(CuCl) \gg K_{sp}(AgCl)$, it acts as a strong common ion source. For $AgCl$, $K_{sp} = [Ag^+][Cl^-] \implies 1.6 \times 10^{-10} = [Ag^+](10^{-3}) \implies [Ag^+] = 1.6 \times 10^{-7} \text{ M}$.
💬Ask on WhatsApp →
Still have doubts about this question?
Send it to our AI chemistry tutor on WhatsApp — gets answered in minutes