For the following chemical reactions, determine the precipitate produced when the two reactants listed below are mixed together. Indicate “none” if no precipitate will form $\mathrm{Sr}\left(\mathrm{NO}_{3}\right)_{2}(a q)+\mathrm{K}_{3} \mathrm{PO}_{4}(a q) \longrightarrow$__________________(s) $\mathrm{K}_{2} \mathrm{CO}_{3}(a q)+\mathrm{AgNO}_{3}(a q) \longrightarrow$__________________(s) $\mathrm{NaCl}(a q)+\mathrm{KNO}_{3}(a q) \longrightarrow$__________________(s) $\mathrm{KCl}(a q)+\mathrm{AgNO}_{3}(a q) \longrightarrow$__________________(s) $\mathrm{FeCl}_{3}(a q)+\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(a q) \longrightarrow$__________________(s)

To predict precipitation, we need to know the solubility rules. Some general solubility rules are: - Most nitrate (\(NO_3^-\)), acetate (\(CH_3COO^-\)), and perchlorate (\(ClO_4^-\)) salts are soluble. - Most alkali metal (group 1A) salts and ammonium \((NH_4^+)\) salts are soluble. - Most chloride, bromide, and iodide salts are soluble, except for those with silver (\(Ag^+\)), lead (\(Pb^{2+}\)), and mercury (\(Hg_2^{2+}\)) cations. - Most sulfate (\(SO_4^{2-}\)) salts are soluble, except for those with calcium (\(Ca^{2+}\)), strontium (\(Sr^{2+}\)), barium (\(Ba^{2+}\)), mercury (\(Hg_{2}^{2+}\)), and lead (\(Pb^{2+}\)) cations. - Most hydroxide salts are slightly soluble or insoluble, except those with alkali metals and calcium, which are soluble. - Most sulfide, carbonate (\(CO_3^{2-}\)), chromate (\(CrO_4^{2-}\)), and phosphate (\(PO_4^{3-}\)) salts are insoluble, except for those with alkali metals and ammonium.

Based on the reactants, determine the possible products by exchanging ions between various reactants. 1. \(Sr(NO_3)_2 (aq) + K_3PO_4 (aq) \longrightarrow Sr_3(PO_4)_2 (s) + 6KNO_3 (aq)\) 2. \(K_2CO_3 (aq) + AgNO_3 (aq) \longrightarrow 2Ag_2CO_3 (s) + 2KNO_3 (aq)\) 3. \(NaCl (aq) + KNO_3 (aq) \longrightarrow NaNO_3 (aq) + KCl (aq)\) 4. \(KCl (aq) + AgNO_3 (aq) \longrightarrow AgCl (s) + KNO_3 (aq)\) 5. \(FeCl_3 (aq) + Pb(NO_3)_2 (aq) \longrightarrow 3PbCl_2 (s) + 2Fe(NO_3)_3 (aq)\)

Use solubility rules to determine which of the possible products will form a precipitate. 1. \(Sr(NO_3)_2 (aq) + K_3PO_4 (aq) \longrightarrow Sr_3(PO_4)_2 (s) + 6KNO_3 (aq)\) - Soluble: \(KNO_3\) - Insoluble: \(Sr_3(PO_4)_2\) - Precipitate: \(Sr_3(PO_4)_2\) 2. \(K_2CO_3 (aq) + AgNO_3 (aq) \longrightarrow 2Ag_2CO_3 (s) + 2KNO_3 (aq)\) - Soluble: \(KNO_3\) - Insoluble: \(Ag_2CO_3\) - Precipitate: \(Ag_2CO_3\) 3. \(NaCl (aq) + KNO_3 (aq) \longrightarrow NaNO_3 (aq) + KCl (aq)\) - Soluble: \(NaNO_3, KCl\) - No precipitate. 4. \(KCl (aq) + AgNO_3 (aq) \longrightarrow AgCl (s) + KNO_3 (aq)\) - Soluble: \(KNO_3\) - Insoluble: \(AgCl\) - Precipitate: \(AgCl\) 5. \(FeCl_3 (aq) + Pb(NO_3)_2 (aq) \longrightarrow 3PbCl_2 (s) + 2Fe(NO_3)_3 (aq)\) - Soluble: \(Fe(NO_3)_3\) - Insoluble: \(PbCl_2\) - Precipitate: \(PbCl_2\)