Which one of the following represents the net ionic equation for the reaction of AgNO3 and LiBr in aqueous solution?

• A. AgBr (s) → Ag+ (aq) + Br- (aq)
• B. Ag+ (aq) + NO3- (aq) + Li+ (aq) + Br- (aq) → AgBr (s) + Li+ (aq) + NO3- (aq)
• C. AgNO3 (aq) + LiBr (aq) → AgBr (s) + LiNO3 (aq)
• D. Ag+ (aq) + Br- (aq) → AgBr (s)

Answer: (D)

Verified step by step guidance

1. Identify the reactants and products in the given reaction: AgNO\_3 (aq) reacts with LiBr (aq) to form AgBr (s) and LiNO\_3 (aq).
2. Write the full ionic equation by dissociating all strong electrolytes (soluble salts) into their ions: AgNO\_3 (aq) dissociates into Ag\^+ (aq) and NO\_3\^- (aq), LiBr (aq) dissociates into Li\^+ (aq) and Br\^- (aq), and LiNO\_3 (aq) dissociates into Li\^+ (aq) and NO\_3\^- (aq).
3. Identify the spectator ions, which are ions that appear unchanged on both sides of the equation. In this case, Li\^+ (aq) and NO\_3\^- (aq) are spectator ions.
4. Remove the spectator ions from the full ionic equation to write the net ionic equation, which includes only the species that undergo a chemical change.
5. Express the net ionic equation showing the formation of the solid precipitate AgBr (s) from its ions: Ag\^+ (aq) + Br\^- (aq) → AgBr (s).