Which of the following is the balanced net ionic equation for the formation of the precipitate when solutions of AgNO_3 and NaCl are mixed?

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

Answer: (A)

Verified step by step guidance

1. Identify the ions present in the solutions before mixing: AgNO_3 dissociates into Ag^+ and NO_3^- ions, and NaCl dissociates into Na^+ and Cl^- ions.
2. Write the full molecular equation showing the reactants and products: AgNO_3 (aq) + NaCl (aq) → AgCl (s) + NaNO_3 (aq).
3. Write the complete ionic equation by breaking all strong electrolytes into their ions: Ag^+ (aq) + NO_3^- (aq) + Na^+ (aq) + Cl^- (aq) → AgCl (s) + Na^+ (aq) + NO_3^- (aq).
4. Identify the spectator ions, which are ions that appear unchanged on both sides of the equation (Na^+ and NO_3^- in this case).
5. Remove the spectator ions to write the net ionic equation, which shows only the ions and compounds directly involved in forming the precipitate: Ag^+ (aq) + Cl^- (aq) → AgCl (s).