Chemistry Help work

Question

Enter the net ionic equation, including phases, for the reaction of  and  Refer to the  as needed.

Answer 1

It's easier if you first write the complete molecular equation.

AgNO₃(aq) + KCl(aq) ==> AgCl(s) + KNO₃(aq) ... you can refer to your solubility rules for the phases

Since AgCl(s) is a precipitate, only the Ag⁺ and Cl^- will appear in the net ionic equation.

Net ionic: Ag⁺(aq) + Cl^-(aq) ==> AgCl(s)

If you want to see how this is obtained from the total ionic equation, see below:

Total ionic: Ag⁺(aq) + NO₃^-(aq) + K⁺(aq) + Cl^-(aq) ==> AgCl(s) + K⁺(aq) + Cl^-(aq)

K⁺(aq) and NO₃^-(aq) are spectator ions and cancel leaving you with the net ionic as shown above.