Asolution 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.

Cl⁻ + Ag⁺ → ClAg ↓

CO₃⁻² + Ca²⁺  →  CaCO₃ ↓

CO₃⁻² + Cu²⁺  →  CuCO₃ ↓

Explanation:

The cations in solution are Ag⁺, Ca²⁺, and Cu²⁺

When sodium chloride is added to the solution, no precipitate forms.

FALSE

NaCl → Na⁺ + Cl⁻

Cl⁻ + Ag⁺ → ClAg ↓

When sodium sulfate is added to the solution, a white precipitate forms.

FALSE - No precipitate formed

The precipitate is filtered off and sodium carbonate is added to the remaining solution, producing a precipitate.

When you filtered off the precipitate (we mean AgCl), in solution there's still remain Ca²⁺ and Cu²⁺

Na₂CO₃ → 2Na⁺  +  CO₃⁻²

CO₃⁻² + Ca²⁺  →  CaCO₃ ↓

CO₃⁻² + Cu²⁺  →  CuCO₃ ↓

i believe the answer is 5,000