Problem 41
When \(250 \mathrm{mg}\) of \(\mathrm{SrF}_{2},\) strontium fluoride, is added to \(1.00 \mathrm{L}\) of water, the salt dissolves to a very small extent. $$\mathrm{SrF}_{2}(\mathrm{s}) \rightleftarrows \mathrm{Sr}^{2+}(\mathrm{aq})+2 \mathrm{F}^{-}(\mathrm{aq})$$ At equilibrium, the concentration of \(\mathrm{Sr}^{2+}\) is found to be \(1.0 \times 10^{-3} \mathrm{M} .\) What is the value of \(K_{\mathrm{sp}}\) for \(\mathrm{SrF}_{2} ?\)
Problem 42
Calcium hydroxide, \(\mathrm{Ca}(\mathrm{OH})_{2},\) dissolves in water to the extent of \(1.3 \mathrm{g}\) per liter. What is the value of \(K_{\mathrm{sp}}\) for \(\mathrm{Ca}(\mathrm{OH})_{2} ?\) $$\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{s}) \rightleftarrows \mathrm{Ca}^{2+}(\mathrm{aq})+2 \mathrm{OH}^{-}(\mathrm{aq})$$
Problem 43
You add \(0.979 \mathrm{g}\) of \(\mathrm{Pb}(\mathrm{OH})_{2}\) to \(1.00 \mathrm{L}\) of pure water at \(25^{\circ} \mathrm{C} .\) The \(\mathrm{pH}\) is \(9.15 .\) Estimate the value of \(K_{\mathrm{sp}}\) for \(\mathrm{Pb}(\mathrm{OH})_{2}.\)
Problem 44
You place \(1.234 \mathrm{g}\) of solid \(\mathrm{Ca}(\mathrm{OH})_{2}\) in \(1.00 \mathrm{L}\) of pure water at \(25^{\circ} \mathrm{C}\). The \(\mathrm{pH}\) of the solution is found to be 12.68 Estimate the value of \(K_{\mathrm{rp}}\) for \(\mathrm{Ca}(\mathrm{OH})_{2}.\)
Problem 49
The \(K_{\mathrm{sp}}\) value for radium sulfate, \(\mathrm{RaSO}_{4},\) is \(4.2 \times 10^{-11} .\) If \(25 \mathrm{mg}\) of radium sulfate is placed in \(1.00 \times 10^{2} \mathrm{mL}\) of water, does all of it dissolve? If not, how much dissolves?
Problem 57
Which insoluble compound in each pair should be more soluble in nitric acid than in pure water? (a) \(\mathrm{PbCl}_{2}\) or \(\mathrm{PbS}\) (b) \(\mathrm{Ag}_{2} \mathrm{CO}_{3}\) or \(\mathrm{AgI}\) (c) \(\mathrm{Al}(\mathrm{OH})_{3}\) or \(\mathrm{AgCl}\)
Problem 59
You have a solution that has a lead(II) concentration of \(0.0012 \mathrm{M}\) \begin{equation}\mathrm{PbCl}_{2}(\mathrm{s}) \rightleftarrows \mathrm{Pb}^{2+}(\mathrm{aq})+2 \mathrm{Cl}^{-}(\mathrm{aq})\end{equation} If enough soluble chloride-containing salt is added so that the \(\mathrm{Cl}^{-}\) concentration is \(0.010 \mathrm{M},\) will \(\mathrm{PbCl}_{2}\) precipitate?
Problem 62
You have 95 mL of a solution that has a lead(II) concentration of \(0.0012 \mathrm{M}\). Will \(\mathrm{PbCl}_{2}\) precipitate when \(1.20 \mathrm{g}\) of solid NaCl is added?
Problem 64
Will a precipitate of \(\mathrm{Mg}(\mathrm{OH})_{2}\) form when \(25.0 \mathrm{mL}\) of \(0.010 \mathrm{M} \mathrm{NaOH}\) is combined with \(75.0 \mathrm{mL}\) of a \(0.10 \mathrm{M}\) solution of magnesium chloride?
Problem 66
Solid silver iodide, AgI, can be dissolved by adding aqueous sodium cyanide to it. $$\mathrm{AgI}(\mathrm{s})+2 \mathrm{CN}^{-}(\mathrm{aq}) \rightleftarrows\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}(\mathrm{aq})+\mathrm{I}^{-}(\mathrm{aq})$$ Show that this equation is the sum of two other equations, one for dissolving AgI to give its ions and the other for the formation of the \(\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}\) ion from \(\mathrm{Ag}^{+}\) and \(\mathrm{CN}^{-}\). Calculate \(K_{\text {net }}\) for the overall reaction.
