Which of the following is the correct net ionic equation for the precipitation reaction that occurs when aqueous solutions of AgNO_3 and NaCl are mixed?

• A. AgCl (aq) → Ag^+ (aq) + Cl^- (aq)
• B. Ag^+ (aq) + Cl^- (aq) → AgCl (s)
• C. AgNO_3 (aq) + NaCl (aq) → AgCl (s) + NaNO_3 (aq)
• D. Ag^+ (aq) + NO_3^- (aq) + Na^+ (aq) + Cl^- (aq) → Ag^+ (aq) + NO_3^- (aq) + Na^+ (aq) + Cl^- (aq)

Answer: (B)

Verified step by step guidance

1. Identify the reactants and products in the given reaction: aqueous solutions of AgNO_3 and NaCl are mixed, resulting in the formation of AgCl as a precipitate and NaNO_3 remaining in solution.
2. Write the full molecular equation for the reaction: \(\mathrm{AgNO_3 (aq) + NaCl (aq) \rightarrow AgCl (s) + NaNO_3 (aq)}\).
3. Dissociate all strong electrolytes (soluble ionic compounds) into their ions to write the complete ionic equation: \(\mathrm{Ag^+ (aq) + NO_3^- (aq) + Na^+ (aq) + Cl^- (aq) \rightarrow AgCl (s) + Na^+ (aq) + NO_3^- (aq)}\).
4. Identify the spectator ions, which are ions that appear unchanged on both sides of the equation. In this case, \(\mathrm{Na^+}\) and \(\mathrm{NO_3^-}\) are spectator ions.
5. Remove the spectator ions to write the net ionic equation, which shows only the species involved in the formation of the precipitate: \(\mathrm{Ag^+ (aq) + Cl^- (aq) \rightarrow AgCl (s)}\).