Which one of the following equations represents the net ionic equation for the reaction between aqueous potassium chloride and aqueous silver nitrate? A. Cl - (aq) + Ag + (aq) AgCl (s) B. K + (aq) + Cl - (aq) + Ag + (aq) + NO3 - (aq) AgCl (s) + K + (aq) + NO3 - (aq) C. KCl (aq) + AgNO3 (aq) AgCl (s) + KNO3 (aq) D. K + (aq) + NO3 - (aq) KNO3 (aq)

Ag⁺ (aq) + Cl⁻ (aq) → AgCl (s)

Explanation:

The questions requires we write the net ionic equation for the reaction between aqueous potassium chloride and aqueous silver nitrate.

Step 1: Writing a balanced equation for the reaction. The balanced equation for the reaction between aqueous potassium chloride and aqueous silver nitrate will be given by;

KCl (aq) + AgNO₃ (aq) → KNO₃ (aq) + AgCl (s)

AgCl is the precipitate formed by the reaction. Step 2: Write the complete ionic equation. The complete ionic equation for the reaction is given by showing all the ions involved in the reaction.

K⁺ (aq) Cl⁻ (aq) + Ag⁺ (aq) NO₃⁻ (aq) → K⁺ (aq) NO₃⁻ (aq) + AgCl (s)

Only ionic compounds are split into ions. Step 3: Write the net ionic equation for the reaction. The net ionic equation for a reactions only the ions that fully participated in the reaction and omits the ions that did not participate in the reaction. The ions that are not involved directly in the reaction are known as spectator ions and are not included while writing net ionic equation.

Ag⁺ (aq) + Cl⁻ (aq) → AgCl (s)