AP Chemistry
7.12 Common-Ion Effect
7.11 Introduction to Solubility Equilibria
A student models the recovery of lead(II) iodide from a pigment-waste stream using the dissolution equilibrium
\(\text{PbI}_2\text{(s)} \rightleftharpoons \text{Pb}^{2+}\text{(aq)} + 2\text{I}^-\text{(aq)}\)
At the temperature of the experiment, \(K_{sp}=4.0\times10^{-9}\). Excess \(\text{PbI}_2\text{(s)}\) is added to a \(0.020\text{ M}\) solution of \(\text{NaI(aq)}\), which dissociates completely. Assume that the iodide ions produced by dissolution of \(\text{PbI}_2\text{(s)}\) make a negligible contribution to the total iodide concentration. What is the approximate molar solubility of \(\text{PbI}_2\text{(s)}\) in the solution?
\(\text{PbI}_2\text{(s)} \rightleftharpoons \text{Pb}^{2+}\text{(aq)} + 2\text{I}^-\text{(aq)}\)
At the temperature of the experiment, \(K_{sp}=4.0\times10^{-9}\). Excess \(\text{PbI}_2\text{(s)}\) is added to a \(0.020\text{ M}\) solution of \(\text{NaI(aq)}\), which dissociates completely. Assume that the iodide ions produced by dissolution of \(\text{PbI}_2\text{(s)}\) make a negligible contribution to the total iodide concentration. What is the approximate molar solubility of \(\text{PbI}_2\text{(s)}\) in the solution?
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