91Ó°ÊÓ

The solubility product constant of magnesium hydroxide is \(8.9 \times 10^{-12}\), calculate its solubility in (a) water and (b) \(.05 \mathrm{M}\) \(\mathrm{NaOH}\)

A chemist dissolves \(\mathrm{BaSO}_{4}\), in pure water at \(25^{\circ} \mathrm{C}\). If its \(\mathrm{K}_{\mathrm{sp}}=1 \times 10^{-10}\), what is the solubility of the barium sulfate in the water?

Determine the approximate solubility of \(\mathrm{AgCl}\) in \(0.10 \mathrm{M} \mathrm{NaCl}\) solution. \(\mathrm{K}_{\mathrm{sp}}\) for \(\mathrm{AgCl}=1.1 \times 10^{-10}\).

A saturated solution of \(\mathrm{CaF}_{2}\) contains \(.00168 \mathrm{~g}\) of \(\mathrm{CaF}_{2}\) per \(100 \mathrm{~g}\) of water. Determine the \(\mathrm{K}_{\mathrm{sp}}\).

Calculate the solubility of carbon dioxide in water at \(25^{\circ} \mathrm{C}\), where the partial pressure of \(\mathrm{CO}_{2}\) over the solution is 760 torr., using Henry's law constant, \(\mathrm{K}_{\mathrm{CO}(2)}\) at \(25^{\circ} \mathrm{C}=1.25 \times 10^{6}\). Assume that a liter of solution contains 1000 grams of water.

The solubility of iodine in pure water is \(0.0279 \mathrm{~g}\) per \(100 \mathrm{~g}\) of water. In a solution that is originally \(0.10 \mathrm{M} \mathrm{KI}\), it is possible to dissolve, at the maximum, \(1.14 \mathrm{~g}\) of iodine per \(100 \mathrm{~g}\) of solution. What is \(\mathrm{K}\) for the reaction \(\mathrm{I}_{2}+\mathrm{I}^{-} \rightleftharpoons \mathrm{I}^{-}_{3} ?\)