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.

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)

answer; the numbers of valence electrons in the acetic acid molecule (ch3co2h) is 24;