Problem 77
Magnesium hydroxide, \(\mathrm{Mg}(\mathrm{OH})_{2},\) found in milk of magnesia, has a solubility of \(7.05 \times 10^{-3} \mathrm{~g} \mathrm{~L}^{-1}\) at \(25^{\circ} \mathrm{C}\). Calculate \(K_{\mathrm{sp}}\) for \(\mathrm{Mg}(\mathrm{OH})_{2}\)
Problem 99
Write the chemical equilibria and equilibrium laws that correspond to \(K_{\text {form }}\) for the following complexes: (a) \(\mathrm{CuCl}_{4}^{2-}\), (b) \(\mathrm{AgI}_{2}^{-}\), (c) \(\mathrm{Cr}\left(\mathrm{NH}_{3}\right)_{6}^{3+}\).
Problem 100
Write the chemical equilibria and equilibrium laws that correspond to \(K_{\text {form }}\) for the following complexes: (a) \(\mathrm{Ag}\left(\mathrm{S}_{2} \mathrm{O}_{3}\right)_{2}^{3-},\) (b) \(\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}^{2+}\) (c) \(\mathrm{SnS}_{3}^{2-}\).
Problem 101
Write equilibria that correspond to \(K_{\text {form }}\) for each of the following complex ions and write the equations for \(K_{\text {form }}:\) (a) \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}^{3+}\) (b) \(\mathrm{HgI}_{4}^{2-}\), (c) \(\mathrm{Fe}(\mathrm{CN})_{6}^{4-}\).
Problem 102
Write the equilibria that are associated with the equations for \(K_{\text {form }}\) for each of the following complex ions. Write also the equations for the \(K_{\text {form }}\) of each: (a) \(\mathrm{Hg}\left(\mathrm{NH}_{3}\right)_{4}^{2+},\) (b) \(\mathrm{SnF}_{6}^{2-}\), (c) \(\mathrm{Fe}(\mathrm{CN})_{6}^{3-}\).
Problem 103
Write equilibria that correspond to \(K_{\text {inst }}\) for each of the following complex ions and write the equations for \(K_{\text {inst }}:\) (a) \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}^{3+},\) (b) \(\mathrm{HgI}_{4}^{2-}\) (c) \(\mathrm{Fe}(\mathrm{CN})_{6}^{4-}\).
Problem 104
Write the equilibria that are associated with the equations for \(K_{\text {inst }}\) for each of the following complex ions. Write also the equations for the \(K_{\text {inst }}\) of each: (a) \(\mathrm{Hg}\left(\mathrm{NH}_{3}\right)_{4}^{2+},\) (b) \(\mathrm{SnF}_{6}^{2-}\), (c) \(\mathrm{Fe}(\mathrm{CN})_{6}^{3-}\).
Problem 106
The overall formation constant for \(\mathrm{Ag}(\mathrm{CN})_{2}^{-}\) equals \(5.3 \times 10^{18}\), and the \(K_{\text {sp }}\) for \(\mathrm{AgCN}\) equals \(6.0 \times 10^{-17}\) Calculate \(K_{\mathrm{c}}\) for the following reaction: \(\mathrm{AgCN}(s)+\) \(\mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{Ag}(\mathrm{CN})_{2}^{-}(a q)\).
Problem 112
Suppose that some dipositive cation, \(M^{2+},\) is able to form a complex ion with a ligand, \(L\), by the following balanced equation: \(M^{2+}+2 L \rightleftharpoons M(\mathrm{~L})_{2}^{2+} .\) The cation also forms a sparingly soluble salt, \(M \mathrm{Cl}_{2}\). In which of the following circumstances would a given quantity of ligand be more able to bring larger quantities of the salt into solution? Explain and justify the calculation involved: (a) \(K_{\text {form }}=1 \times 10^{2}\) and \(K_{\text {sp }}=1 \times 10^{-15}\), (b) \(K_{\text {form }}=1 \times 10^{10}\) and \(K_{\mathrm{sp}}=1 \times 10^{-20}\).
Problem 117
Suppose that \(50.0 \mathrm{~mL}\) of \(0.12 \mathrm{M} \mathrm{AgNO}_{3}\) is added to \(50.0 \mathrm{~mL}\) of \(0.048 \mathrm{M} \mathrm{NaCl}\) solution. (a) What mass of \(\mathrm{AgCl}\) will form? (b) Calculate the final concentrations of all of the ions in the solution that is in contact with the precipitate. (c) What percentage of the \(\mathrm{Ag}^{+}\) ions have precipitated?
