Question

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.

Answer 1

Answer:

Ca(aq)⁺²  + CO₃⁻²(aq) → CaCO₃(s)

Explanation:

Breaking down the equation into ionic form gives:

2Na⁺(aq) + CO₃⁻²(aq) + Ca⁺²(aq) + 2NO₃⁻¹ (aq)  →  2Na⁺(aq) + 2NO₃⁻¹(aq)  + CaCO₃(s)

Eliminating all the same ionic states on both sides of the equation gives following final equation

Ca(aq)⁺²  + CO₃⁻²(aq) → CaCO₃(s)