Using the general solubility rules given in Table \(6-1,\) 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 d. sulfate ion b. calcium ion e. mercury(I) ion, \(\mathrm{Hg}_{2}^{2+}\) c. iron(III) ion f. silver ion

For chloride ions, precipitates can form with silver nitrate, lead nitrate, and mercury(II) nitrate. The net ionic equations are: 1. \(Ag^+ + Cl^- \rightarrow AgCl\) 2. \(Pb^{2+} + 2Cl^- \rightarrow PbCl_2\) 3. \(Hg^{2+} + 2Cl^- \rightarrow HgCl_2\) For sulfate ions, precipitates can form with barium chloride, lead nitrate, and calcium chloride. The net ionic equations are: 1. \(Ba^{2+} + SO_4^{2-} \rightarrow BaSO_4\) 2. \(Pb^{2+} + SO_4^{2-} \rightarrow PbSO_4\) 3. \(Ca^{2+} + SO_4^{2-} \rightarrow CaSO_4\) For calcium ions, precipitates can form with sulfate ion, phosphate ion, and oxalate ion. The net ionic equations are: 1. \(Ca^{2+} + SO_4^{2-} \rightarrow CaSO_4\) 2. \(3Ca^{2+} + 2PO_4^{3-} \rightarrow Ca_3(PO_4)_2\) 3. \(Ca^{2+} + C_2O_4^{2-} \rightarrow CaC_2O_4\) For mercury(I) ions, precipitates can form with chloride ion, bromide ion, and iodide ion. The net ionic equations are: 1. \(Hg_2^{2+} + 2Cl^- \rightarrow Hg_2Cl_2\) 2. \(Hg_2^{2+} + 2Br^- \rightarrow Hg_2Br_2\) 3. \(Hg_2^{2+} + 2I^- \rightarrow Hg_2I_2\) For iron(III) ions, precipitates can form with hydroxide ion, phosphate ion, and sulfide ion. The net ionic equations are: 1. \(Fe^{3+} + 3OH^- \rightarrow Fe(OH)_3\) 2. \(Fe^{3+} + PO_4^{3-} \rightarrow FePO_4\) 3. \(2Fe^{3+} + 3S^{2-} \rightarrow Fe_2S_3\) For silver ions, precipitates can form with chloride ion, bromide ion, and iodide ion. The net ionic equations are: 1. \(Ag^+ + Cl^- \rightarrow AgCl\) 2. \(Ag^+ + Br^- \rightarrow AgBr\) 3. \(Ag^+ + I^- \rightarrow AgI\)