Which of the following represents the total ionic equation for the reaction between HNO3 and NaOH in aqueous solution?

• A. HNO3 (aq) + NaOH (aq) → NaNO3 (aq) + H2O (l)
• B. H^+ (aq) + NO3^- (aq) + Na^+ (aq) + OH^- (aq) → Na^+ (aq) + NO3^- (aq) + H2O (l)
• C. H^+ (aq) + OH^- (aq) → H2O (l)
• D. HNO3 (aq) + OH^- (aq) → NO3^- (aq) + H2O (l)

Answer: (B)

Verified step by step guidance

1. Identify the reactants and products in the given reaction: HNO3 (aq) + NaOH (aq) → NaNO3 (aq) + H2O (l). Both HNO3 and NaOH are strong electrolytes and will dissociate completely in aqueous solution.
2. Write the dissociation of each strong electrolyte into its ions: HNO3 (aq) dissociates into H^+ (aq) and NO3^- (aq), and NaOH (aq) dissociates into Na^+ (aq) and OH^- (aq). Similarly, NaNO3 (aq) dissociates into Na^+ (aq) and NO3^- (aq).
3. Express the total ionic equation by replacing all strong electrolytes with their respective ions, while keeping water as a molecular species since it is a liquid and does not dissociate: H^+ (aq) + NO3^- (aq) + Na^+ (aq) + OH^- (aq) → Na^+ (aq) + NO3^- (aq) + H2O (l).
4. Recognize that spectator ions (ions that appear unchanged on both sides of the equation) can be identified. In this case, Na^+ (aq) and NO3^- (aq) are spectator ions.
5. Confirm that the total ionic equation includes all ions present in the reaction mixture before and after the reaction, showing the actual species in solution.