Which of the following is the net ionic equation for the reaction between KBr(aq) and NaCl(aq)?

• A. There is no net ionic equation because no reaction occurs.
• B. K^+(aq) + Cl^-(aq) → KCl(s)
• C. Na^+(aq) + Br^-(aq) → NaBr(s)
• D. K^+(aq) + Br^-(aq) → KBr(s)

Answer: (A)

Verified step by step guidance

1. Identify the species present in the solutions: KBr(aq) dissociates into K\^+(aq) and Br\^-(aq), and NaCl(aq) dissociates into Na\^+(aq) and Cl\^-(aq).
2. Write the possible combinations of ions that could form precipitates or new compounds: K\^+ with Cl\^-, Na\^+ with Br\^-, and K\^+ with Br\^- (original compound).
3. Check the solubility rules to determine if any of these combinations form an insoluble solid (precipitate). Both KCl and NaBr are soluble in water, and KBr is already dissolved, so no precipitate forms.
4. Since no precipitate, gas, or weak electrolyte is formed, no chemical reaction occurs between these ions in solution.
5. Conclude that the net ionic equation does not exist because all ions remain as aqueous ions and no net change occurs.