A student is given 50.0mL of a solution of Na2CO3 of unknown concentration. To determine the concentration of the solution, the student mixes the solution with excess 1.0MCa (NO3) 2 (aq), causing a precipitate to form. The balanced equation for the reaction is shown below.

Na2CO3 (aq) + Ca (NO3) 2 (aq) →2NaNO3 (aq) + CaCO3 (s)

a) Write the net ionic equation for the reaction that occurs when the solutions of Na2CO3 and Ca (NO3) 2 are mixed.

Question

Chemistry

Shiloh

22 March, 03:40

A student is given 50.0mL of a solution of Na2CO3 of unknown concentration. To determine the concentration of the solution, the student mixes the solution with excess 1.0MCa (NO3) 2 (aq), causing a precipitate to form. The balanced equation for the reaction is shown below.

Na2CO3 (aq) + Ca (NO3) 2 (aq) →2NaNO3 (aq) + CaCO3 (s)

a) Write the net ionic equation for the reaction that occurs when the solutions of Na2CO3 and Ca (NO3) 2 are mixed.

+2

Answers (1)

Know the Answer?

Morgan Blackburn · Answer 1

CO₃²⁻ + Ca²⁺ → CaCO₃ (s)

Explanation:

In a net ionic equation there are listed just the ions that are involved in the reaction.

For the reaction:

Na₂CO₃ (aq) + Ca (NO₃) ₂ (aq) → 2NaNO₃ (aq) + CaCO₃ (s)

Ions are:

2 Na⁺ + CO₃²⁻ + Ca²⁺ + 2 NO₃⁻ → 2 Na⁺ + 2 NO₃⁻ + CaCO₃ (s)

Thus, ions that react are just CO₃²⁻ and Ca²⁺ and net ionic equation is:

CO₃²⁻ + Ca²⁺ → CaCO₃ (s)