Given the reaction between aqueous solutions of NaCl and AgNO3, which is the net ionic equation?

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

Answer: (D)

Verified step by step guidance

1. Identify all the species present in the reaction and write the full molecular equation: \(\text{NaCl (aq)} + \text{AgNO}_3 \text{(aq)} \rightarrow \text{AgCl (s)} + \text{NaNO}_3 \text{(aq)}\).
2. Write the complete ionic equation by dissociating all strong electrolytes (soluble salts) into their ions: \(\text{Na}^+ (aq) + \text{Cl}^- (aq) + \text{Ag}^+ (aq) + \text{NO}_3^- (aq) \rightarrow \text{AgCl (s)} + \text{Na}^+ (aq) + \text{NO}_3^- (aq)\).
3. Identify the spectator ions, which are ions that appear unchanged on both sides of the equation. Here, \(\text{Na}^+\) and \(\text{NO}_3^-\) are spectator ions.
4. Remove the spectator ions from the complete ionic equation to write the net ionic equation, which includes only the species that participate in forming the precipitate.
5. Write the net ionic equation as \(\text{Ag}^+ (aq) + \text{Cl}^- (aq) \rightarrow \text{AgCl (s)}\), showing the formation of the solid precipitate.