Write the expression for the solubility-product constant for each of the following ionic compounds: AgI, SrSO \(_{4}, \mathrm{Fe}(\mathrm{OH})_{2},\) and \(\mathrm{Hg}_{2} \mathrm{Br}_{2}\) .

Let's write the dissolution equations for each ionic compound: 1. For AgI: \(AgI \rightleftharpoons Ag^+ + I^-\) 2. For SrSO4: \(SrSO_4 \rightleftharpoons Sr^{2+} + SO_4^{2-}\) 3. For Fe(OH)2: \(Fe(OH)_2 \rightleftharpoons Fe^{2+} + 2OH^-\) 4. For Hg2Br2: \(Hg_2Br_2 \rightleftharpoons 2Hg^{2+} + 2Br^-\)

Now, let's write the expressions for the solubility product constants (Ksp) for each compound, using their dissolution equations: 1. For AgI: Dissolution equation: \(AgI \rightleftharpoons Ag^+ + I^-\) Ksp expression: \(K_{sp} = [Ag^+][I^-]\) 2. For SrSO4: Dissolution equation: \(SrSO_4 \rightleftharpoons Sr^{2+} + SO_4^{2-}\) Ksp expression: \(K_{sp} = [Sr^{2+}][SO_4^{2-}]\) 3. For Fe(OH)2: Dissolution equation: \(Fe(OH)_2 \rightleftharpoons Fe^{2+} + 2OH^-\) Ksp expression: \(K_{sp} = [Fe^{2+}][OH^-]^2\) 4. For Hg2Br2: Dissolution equation: \(Hg_2Br_2 \rightleftharpoons 2Hg^{2+} + 2Br^-\) Ksp expression: \(K_{sp} = [Hg^{2+}]^2[Br^-]^2\) So, the expressions for the solubility product constants for the given ionic compounds are: - AgI: \(K_{sp} = [Ag^+][I^-]\) - SrSO4: \(K_{sp} = [Sr^{2+}][SO_4^{2-}]\) - Fe(OH)2: \(K_{sp} = [Fe^{2+}][OH^-]^2\) - Hg2Br2: \(K_{sp} = [Hg^{2+}]^2[Br^-]^2\)