Asolution contains one or more of the following ions: ag+, ca2+, and co2+. lithium bromide is added to the solution and no precipitate forms. an excess of lithium sulfate is then added to the solution and a precipitate forms. the precipitate is filtered off and lithium phosphate is added to the remaining solution, producing a precipitate. a. which ions are present in the original solution? ca2+ag+co2+b. write a net ionic equation for the formation of the precipitate observed after the addition of lithium sulfate. include physical states. c. write a net ionic equation for the formation of the precipitate observed after the addition of lithium phosphate. include physical states.

#1. Ca²⁺

# 2. Ca²⁺(aq) + SO₃²⁻(aq) → CaSO₄(s)

#3. 3Ag⁺(aq) + PO₄³⁻(aq) → Ag₃PO₄(s)

Explanation:

The question above concerns solubility of salts or ions in water.

The solution given contains Ag+, Ca2+, and Co2+ ions.

In the first case, when Lithium bromide is added to the solution, there is no white precipitate formed.In the second case, the addition of Lithium sulfate results in the formation of a precipitate because of the Ca²⁺ in the solution combined with the SO₃²⁻ from lithium sulfate to form an insoluble CaSO₄. The net ionic equation for the reaction is;

Ca²⁺(aq) + SO₃²⁻(aq) → CaSO₄(s)

From the solubility rules, all sulfates are soluble except BaSO₄, CaSO₄, and PbSO₄.In the third case, the addition of Lithium phosphate results in the formation of a precipitate because Ag⁺ ions in the solution combine with phosphate ions ( PO₄³⁻) from lithium phosphate to form an insoluble salt, Ag₃PO₄.The net ionic equation for the reaction is;

3Ag⁺(aq) + PO₄³⁻(aq) → Ag₃PO₄(s)

According to solubility rules, all phosphates are insoluble in water except Na₃PO₄, K₃PO₄, and (NH₄)₃PO₄.