Because the oxide ion is basic, metal oxides react readily with acids. (a) Write the net ionic equation for the following reaction: \(\mathrm{FeO}(s)+2 \mathrm{HClO}_{4}(a q) \longrightarrow \mathrm{Fe}\left(\mathrm{ClO}_{4}\right)_{2}(a q)+\mathrm{H}_{2} \mathrm{O}(l)\) (b) Based on the equation in part (a), write the net ionic equation for the reaction that occurs between \(\mathrm{NiO}(s)\) and an aqueous solution of nitric acid.

First, we need to write the balanced chemical equation, which is already given as: \[\mathrm{FeO(s)} + 2 \mathrm{HClO_4(aq)} \longrightarrow \mathrm{Fe(ClO_4)_2(aq)} + \mathrm{H_2O(l)}\] Next, we'll break this balanced chemical equation into the corresponding ionic equation. In order to do this, we must identify the correct ionic forms of the compounds that are dissolved in the aqueous solution: \[\mathrm{FeO(s)} + 2\mathrm{H^+(aq)} + 2\mathrm{ClO_4^-(aq)} \longrightarrow \mathrm{Fe^{2+}(aq)} + 2\mathrm{ClO_4^-(aq)} + \mathrm{H_2O(l)}\] Now, let's write the net ionic equation by canceling out the spectator ions (the ions that remain unchanged during the course of the reaction). In this case, the spectator ions are the \(\mathrm{ClO_4^-}\) ions: \[\mathrm{FeO(s)} + 2\mathrm{H^+(aq)} \longrightarrow \mathrm{Fe^{2+}(aq)} + \mathrm{H_2O(l)}\] Thus, the net ionic equation for the reaction between \(\mathrm{FeO}\) and \(\mathrm{HClO_4}\) is: \[\mathrm{FeO(s)} + 2\mathrm{H^+(aq)} \longrightarrow \mathrm{Fe^{2+}(aq)} + \mathrm{H_2O(l)}\]

Based on the reaction in part (a), we can write the net ionic equation for the reaction between \(\mathrm{NiO(s)}\) and an aqueous solution of nitric acid (\(\mathrm{HNO_3}\)). The overall reaction is: \[\mathrm{NiO(s) + 2 HNO_3(aq) \longrightarrow Ni(NO_3)_2(aq) + H_2 O(l)}\] Breaking the equation into the ionic equation, we get: \[\mathrm{NiO(s)} + 2\mathrm{H^+(aq)} + 2\mathrm{NO_3^-(aq)} \longrightarrow \mathrm{Ni^{2+}(aq)} + 2\mathrm{NO_3^-(aq)} + \mathrm{H_2O(l)}\] Now, let's write the net ionic equation by canceling out the spectator ions (the ions that remain unchanged during the reaction). In this case, the spectator ions are the \(\mathrm{NO_3^-}\) ions: \[\mathrm{NiO(s)} + 2\mathrm{H^+(aq)} \longrightarrow \mathrm{Ni^{2+}(aq)} + \mathrm{H_2O(l)}\] Thus, the net ionic equation for the reaction between \(\mathrm{NiO}\) and an aqueous solution of nitric acid (\(\mathrm{HNO_3}\)) is: \[\mathrm{NiO(s)} + 2\mathrm{H^+(aq)} \longrightarrow \mathrm{Ni^{2+}(aq)} + \mathrm{H_2O(l)}\]