Which of the following represents the right side of the complete ionic equation for dissolving Al(NO3)3 in water?

• A. Al(NO_3)_3(s)
• B. Al^{3+}(aq) + NO_3^{-}(s)
• C. Al^{3+}(aq) + 3 NO_3^{-}(aq)
• D. Al^{3+}(s) + 3 NO_3^{-}(aq)

Answer: (C)

Verified step by step guidance

1. Step 1: Understand that when an ionic compound like aluminum nitrate, \(\text{Al(NO}_3)_3\), dissolves in water, it dissociates into its constituent ions completely because it is a strong electrolyte.
2. Step 2: Write the formula of aluminum nitrate and identify the ions it produces upon dissociation. Aluminum nitrate consists of one aluminum ion, \(\text{Al}^{3+}\), and three nitrate ions, \(\text{NO}_3^{-}\).
3. Step 3: Write the dissociation equation showing the solid aluminum nitrate dissociating into aqueous ions: \(\text{Al(NO}_3)_3(s) \rightarrow \text{Al}^{3+}(aq) + 3\ \text{NO}_3^{-}(aq)\).
4. Step 4: Recognize that in the complete ionic equation, all strong electrolytes are shown as ions with their correct charges and states. The aluminum ion is \(\text{Al}^{3+}(aq)\) and nitrate ions are \(\text{NO}_3^{-}(aq)\), both aqueous.
5. Step 5: Confirm that the correct representation of the right side of the complete ionic equation is \(\text{Al}^{3+}(aq) + 3\ \text{NO}_3^{-}(aq)\), indicating full dissociation into ions in aqueous solution.