Using the general solubility rules given in Table 4.1, name three reagents that would form precipitates with each of the following ions in aqueous solution. Write the net ionic equation for each of your suggestions. a. chloride ion \(\quad\) d. sulfate ion b. calcium ion \(\quad\) e. mercury \((1)\) ion, \(\mathrm{Hg}_{2}^{2+}\) c. iron(M) ion \(\quad\) f. silver ion

a. Chloride ion: 1. \(Ag^+ + Cl^- \rightarrow AgCl(s)\) 2. \(Pb^{2+} + 2Cl^- \rightarrow PbCl_2(s)\) 3. \(Hg^{2+} + 2Cl^- \rightarrow HgCl_2(s)\) b. Calcium ion: 1. \(Ca^{2+} + CO_3^{2-} \rightarrow CaCO_3(s)\) 2. \(Ca^{2+} + SO_4^{2-} \rightarrow CaSO_4(s)\) 3. \(Ca^{2+} + C_2O_4^{2-} \rightarrow CaC_2O_4(s)\) c. Iron(II) ion: 1. \(Fe^{2+} + 2OH^- \rightarrow Fe(OH)_2(s)\) 2. \(Fe^{2+} + CO_3^{2-} \rightarrow FeCO_3(s)\) 3. \(Fe^{2+} + SCN^- \rightarrow FeSCN(s)\) d. Sulfate ion: 1. \(Ba^{2+} + SO_4^{2-} \rightarrow BaSO_4(s)\) 2. \(Pb^{2+} + SO_4^{2-} \rightarrow PbSO_4(s)\) 3. \(Ca^{2+} + SO_4^{2-} \rightarrow CaSO_4(s)\) e. Mercury(I) ion, \(\mathrm{Hg}_{2}^{2+}\): 1. \[\mathrm{Hg}_{2}^{2+} + 2Cl^- \rightarrow \mathrm{Hg}_2Cl_2(s)\] 2. \[\mathrm{Hg}_{2}^{2+} + 2I^- \rightarrow \mathrm{Hg}_2I_2(s)\] 3. \[\mathrm{Hg}_{2}^{2+} + S^{2-} \rightarrow \mathrm{Hg}_2S(s)\] f. Silver ion: 1. \(Ag^+ + Cl^- \rightarrow AgCl(s)\) 2. \(Ag^+ + Br^- \rightarrow AgBr(s)\) 3. \(Ag^+ + I^- \rightarrow AgI(s)\)