To write the second net ionic equation for the addition of aqueous ammonia \((\text{NH}_3)\) to aluminum nitrate \((\text{Al(NO}_3\text{)}_3)\), we need to first understand the reaction that occurs when ammonia is added to aluminum nitrate in aqueous solution.
First Net Ionic Equation (NIE)
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Dissociation of Reactants: \[ \text{Al(NO}_3\text{)}_3 (aq) \rightarrow \text{Al}^{3+} (aq) + 3\text{NO}_3^{-} (aq) \] \[ \text{NH}_3 (aq) + \text{H}_2\text{O} (l) \rightleftharpoons \text{NH}_4^{+} (aq) + \text{OH}^{-} (aq) \]
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Overall Reaction: The overall reaction combines the dissociated ions: \[ \text{Al}^{3+} (aq) + 3\text{NO}_3^{-} (aq) + \text{NH}_3 (aq) + \text{H}_2\text{O} (l) \rightleftharpoons \text{Al(OH)}_3 (s) + 3\text{NO}_3^{-} (aq) + \text{NH}_4^{+} (aq) \]
Net Ionic Equation (NIE) 1
The first net ionic equation, indicating the formation of a precipitate \( \text{Al(OH)}_3 \), is: \[ \text{Al}^{3+} (aq) + 3\text{OH}^{-} (aq) \rightarrow \text{Al(OH)}_3 (s) \]
Second Net Ionic Equation (NIE)
In the second net ionic equation, we focus on the ammonium ion formation from ammonia in the presence of water: \[ \text{NH}_3 (aq) + \text{H}_2\text{O} (l) \rightleftharpoons \text{NH}_4^{+} (aq) + \text{OH}^{-} (aq) \]
Summary of Net Ionic Equations
Putting both net ionic equations together in the appropriate order: 1. \[ \text{Al}^{3+} (aq) + 3\text{OH}^{-} (aq) \rightarrow \text{Al(OH)}_3 (s) \] 2. \[ \text{NH}_3 (aq) + \text{H}_2\text{O} (l) \rightleftharpoons \text{NH}_4^{+} (aq) + \text{OH}^{-} (aq) \]
These equations represent the essential chemical interactions when aqueous ammonia is added to aluminum nitrate.