Consider the chemical equation below:AgNO_3(aq) + NaCl(aq) → AgCl(s) + NaNO_3(aq)Which is the net ionic equation for this reaction?

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

Answer: (B)

Verified step by step guidance

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