Identify the species that acts as an acid.
This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Step 1: Identify the species that acts as an acid.
According to the Brønsted-Lowry theory, an acid is a proton ($\text{H}^+$) donor. In the given reaction, $\text{NH}_4^+$ loses a proton to become $\text{NH}_3$.
$$ \text{NH}_4^+ \text{(aq)} \longrightarrow \text{NH}_3 \text{(aq)} + \text{H}^+ $$
Step 2: Identify the species that acts as a base.
A base is a proton ($\text{H}^+$) acceptor. In the reaction, $\text{OH}^-$ accepts a proton to become $\text{H}_2\text{O}$.
$$ \text{OH}^- \text{(aq)} + \text{H}^+ \longrightarrow \text{H}_2\text{O (l)} $$
Step 3: State the acid and the reason.
The acid in the reaction is $\text{NH}_4^+$. It acts as an acid because it donates a proton ($\text{H}^+$) to $\text{OH}^-$.
The acid is $\boxed{\text{NH}_4^+}$.
Reason: $\text{NH}_4^+$ donates a proton ($\text{H}^+$) to $\text{OH}^-$ to form $\text{NH}_3$ and $\text{H}_2\text{O}$.
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