A solution contains one or more of the following ions: Ag+, Ca2+, and Cu2+. When sodium chloride is added to the solution, no precipitate forms. When sodium sulfate is added to the solution, a white precipitate forms. The precipitate is filtered off and sodium carbonate is added to the remaining solution, producing a precipitate. Write net ionic equations for the formation of each of the precipitates observed.

SO₄⁻² (aq) + Ca⁺₂ (aq) → CaSO₄ (s)

CO₃⁻² (aq) + Cu⁺² (aq) → CuCO₃ (s)

Explanation:

When sodium chloride (NaCl) is added to the solution, it dissociates and forms the ions Na + and Cl-. The anion can be form salts with the other cations presented in the solution. According to the solubility table of the salts, AgCl is a nonsoluble salt, and so, it was expected to form a precipitate. Perhaps, the concentration was not higher enough to do this.

When sodium sulfate (Na2SO4) is added, it dissociates and forms Na + and SO₄⁻², the sulfate ion can react with the other cations. According to the solubility table, the salt CaSO4 (Ca is from group 2) is nonsoluble, so it will be formed. The net ionic equation represents the ions in solution that reacts:

Na⁺ (aq) + SO₄⁻² (aq) + Ca⁺₂ (aq) → Na⁺ (aq) + CaSO₄ (s)

SO₄⁻² (aq) + Ca⁺₂ (aq) → CaSO₄ (s)

When sodium carbonate (Na2CO3) is added, it dissociates and forms Na + and CO₃⁻². According to the solubility table, the salt CuCO₃ is nonsoluble and will form a precipitate:

Na⁺ (aq) + CO₃⁻² (aq) + Cu⁺² (aq) → Na⁺ (aq) + CuCO₃ (s)

CO₃⁻² (aq) + Cu⁺² (aq) → CuCO₃ (s)