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 b. calcium ion c. iron(III) ion d. sulfate ion e. mercury(I) ion, \(\mathrm{Hg}_{2}{ }^{2+}\) f. silver ion

a. Chloride ion: Ag⁺, Pb²⁺, Hg₂²⁺ Net ionic equations: \( Ag^+ + Cl^- \rightarrow AgCl↓ \) \( Pb^{2+} + 2Cl^- \rightarrow PbCl_2↓ \) \( Hg_2^{2+} + 2Cl^- \rightarrow Hg_2Cl_2↓\) b. Calcium ion: CO₃²⁻, PO₄³⁻, C₂O₄²⁻ Net ionic equations: \( Ca^{2+} + CO_3^{2-} \rightarrow CaCO_3↓ \) \( 3Ca^{2+} + 2PO_4^{3-} \rightarrow Ca_3(PO_4)_2↓ \) \( Ca^{2+} + C_2O_4^{2-} \rightarrow CaC_2O_4↓\) c. Iron(III) ion: OH⁻, PO₄³⁻, S²⁻ Net ionic equations: \( Fe^{3+} + 3OH^- \rightarrow Fe(OH)_3↓ \) \( 2Fe^{3+} + 3PO_4^{3-} \rightarrow Fe_2(PO_4)_3↓ \) \( Fe^{3+} + 3S^{2-} \rightarrow Fe_2S_3↓\) d. Sulfate ion: Ba²⁺, Pb²⁺, Ca²⁺ Net ionic equations: \( Ba^{2+} + SO_4^{2-} \rightarrow BaSO_4↓ \) \( Pb^{2+} + SO_4^{2-} \rightarrow PbSO_4↓ \) \( Ca^{2+} + SO_4^{2-} \rightarrow CaSO_4↓\) e. Mercury(I) ion, Hg₂²⁺: Cl⁻, Br⁻, I⁻ Net ionic equations: \( Hg_2^{2+} + 2Cl^- \rightarrow Hg_2Cl_2↓ \) \( Hg_2^{2+} + 2Br^- \rightarrow Hg_2Br_2↓ \) \( Hg_2^{2+} + 2I^- \rightarrow Hg_2I_2↓\) f. Silver ion: Cl⁻, Br⁻, I⁻ Net ionic equations: \( Ag^+ + Cl^- \rightarrow AgCl↓ \) \( Ag^+ + Br^- \rightarrow AgBr↓ \) \( Ag^+ + I^- \rightarrow AgI↓\)