AP Chemistry
7.12 Common-Ion Effect
7.11 Introduction to Solubility Equilibria
7.3 Reaction Quotient and Equilibrium Constant
A student adds excess solid \(\text{AgCl(s)}\) to separate beakers containing pure water and \(0.10\text{ M }\text{NaCl(aq)}\) at \(25^\circ\text{C}\). After equilibrium is established, undissolved solid remains in both beakers. Assume that no silver-containing complex ions form.
\[\text{AgCl(s)}\rightleftharpoons\text{Ag}^+\text{(aq)}+\text{Cl}^-\text{(aq)}\qquad K_{sp}=1.8\times10^{-10}\]
Which statement best compares the molar solubility of \(\text{AgCl(s)}\) in the two beakers and explains the difference?
\[\text{AgCl(s)}\rightleftharpoons\text{Ag}^+\text{(aq)}+\text{Cl}^-\text{(aq)}\qquad K_{sp}=1.8\times10^{-10}\]
Which statement best compares the molar solubility of \(\text{AgCl(s)}\) in the two beakers and explains the difference?
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