The solubility of copper(II) hydroxide in water can be increased by adding either the base \(\mathrm{NH}_{3}\) or the acid \(\mathrm{HNO}_{3}\) . Explain. Would added \(\mathrm{NH}_{3}\) or \(\mathrm{HNO}_{3}\) have the same effect on the solubility of silver acetate or silver chloride? Explain.

Copper(II) hydroxide (\(\mathrm{Cu(OH)_{2}}\)) is only slightly soluble in water and the equilibrium can be represented as: \[\mathrm{Cu(OH)_{2}(s) \rightleftharpoons Cu^{2+}(aq) + 2\,OH^{-}(aq)}\] When we add \(\mathrm{NH}_{3}\) (ammonia, a base) to the solution, it reacts with \(\mathrm{Cu^{2+}}\) ions to form the soluble copper-ammonia complex ion, \(\mathrm{[Cu(NH_{3})_{4}]^{2+}}\). The reaction is: \[\mathrm{Cu^{2+}(aq) + 4\,NH_{3}(aq) \rightleftharpoons [Cu(NH_{3})_{4}]^{2+}(aq)}\] This reaction reduces the concentration of \(\mathrm{Cu^{2+}}\) ions in the solution, causing the equilibrium of \(\mathrm{Cu(OH)_{2}}\) dissolution to shift to the right, and making it more soluble. Now, when we add \(\mathrm{HNO}_{3}\) (nitric acid) to the solution, it reacts with the \(\mathrm{OH^{-}}\) ions as follows: \[\mathrm{H^{+}(aq) + OH^{-}(aq) \rightleftharpoons H_{2}O(l)}\] In this case, the addition of acid neutralizes the \(\mathrm{OH^{-}}\) ions and decreases their concentration, causing the \(\mathrm{Cu(OH)_{2}}\) solubility equilibrium to shift to the right.

Now, let's consider the solubility of silver acetate (\(\mathrm{AgC_{2}H_{3}O_{2}}\)) and silver chloride (\(\mathrm{AgCl}\)) in water, represented by the following equilibria: \[\mathrm{AgC_{2}H_{3}O_{2}(s) \rightleftharpoons Ag^{+}(aq) + C_{2}H_{3}O_{2}^{-}(aq)}\] \[\mathrm{AgCl(s) \rightleftharpoons Ag^{+}(aq) + Cl^{-}(aq)}\] When we add ammonia to these equilibria, \(\mathrm{Ag^{+}}\) ions form soluble complexes – \(\mathrm{[Ag(NH_{3})_{2}]^{+}}\) – similar to the copper case, increasing the solubility of both silver acetate and silver chloride. \[\mathrm{Ag^{+}(aq) + 2\,NH_{3}(aq) \rightleftharpoons [Ag(NH_{3})_{2}]^{+}(aq)}\] However, if we add an acid like \(\mathrm{HNO}_{3}\) to these solutions, there will be no significant reaction with the anions of silver acetate (\(\mathrm{C_{2}H_{3}O_{2}^{-}}\)) and silver chloride (\(\mathrm{Cl^{-}}\)), as they are not basic anions. Hence, the solubility of silver acetate and silver chloride will not change significantly when an acid is added. In conclusion, adding ammonia increases the solubility of all three compounds, while adding nitric acid only has a significant effect on the solubility of copper(II) hydroxide in water and not on the solubility of silver acetate or silver chloride.