Lead bromide, \(\mathrm{PbBr}_{2}\), is moderately soluble, with
\(K_{\mathrm{rp}}\) cqual to \(1.86 \times 10^{-5}\)
a. Predict the solubility of lead bromide in pure water, based on this
\(K_{\mathrm{rg}}\) value. (How many moles of solid \(\mathrm{PbBr}_{2}\) could be
completely dissolved in one liter of solution?) Ignore the effect of any other
equilibria that may impact the solubility (for example, interactions between
\(P b^{2+}\) and \(O H^{-}\) ). Your result will not match literature values for
the actual solubility of \(P b B r_{2}\)
______ moles/L
b. What would the predicted solubility of \(\mathrm{PbBr}_{2}\) be in \(0.10
\mathrm{M}\) NaBr? (How many moles of solid \(\mathrm{PbBr}_{2}\) could be
completely dissolved in 1 L of solution?) Again, ignore all other equilibria;
assume that the
\(\mathbf{K}_{p}\) expression for \(P b B r_{2}\) completely describes the
situation.
________ moles/L
c. The difference in the results obtained in \(3(a)\) and \(3(b)\) is caused by
what is known as the common ion effect. State in words what the common ion
effect predicts.
