Question:
The conjugate base of \(NH_4^+\) is:
The conjugate base of \(NH_4^+\) is:
Show Hint
A conjugate base is formed when an acid loses one proton \((H^+)\), whereas a conjugate acid is formed when a base gains one proton \((H^+)\).
\[
NH_4^+ \rightleftharpoons NH_3 + H^+
\]
Hence, \(NH_3\) is the conjugate base of \(NH_4^+\).
Updated On: Jun 26, 2026
- \(NH^{2-}\)
- \(NH_3\)
- \(NH_2^{-}\)
- \(NH_4OH\)
Show Solution
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The Correct Option is B
Solution and Explanation
Step 1: Recall the definition of a conjugate base.
According to the Brønsted-Lowry concept, a conjugate base is formed when an acid donates a proton \((H^+)\).
Thus, \[ \text{Conjugate Base}=\text{Acid}-H^+ \]
Step 2: Remove one proton from \(NH_4^+\).
The ammonium ion is \[ NH_4^+ \] When it loses one proton, \[ NH_4^+ \rightarrow NH_3 + H^+ \] Therefore, the species formed is \[ NH_3 \]
Step 3: Verify the conjugate acid-base pair.
The pair is \[ NH_4^+/NH_3 \] where \[ NH_4^+ \] acts as the acid and \[ NH_3 \] acts as its conjugate base.
Step 4: Analyze the other options.
\[ NH^{2-} \] and \[ NH_2^- \] are not obtained by removing only one proton from \(NH_4^+\).
\[ NH_4OH \] is ammonium hydroxide and is not the conjugate base of \(NH_4^+\).
Step 5: Final conclusion.
Hence, the conjugate base of \[ NH_4^+ \] is \[ \boxed{NH_3} \] Therefore, the correct option is \[ \boxed{(2)} \]
According to the Brønsted-Lowry concept, a conjugate base is formed when an acid donates a proton \((H^+)\).
Thus, \[ \text{Conjugate Base}=\text{Acid}-H^+ \]
Step 2: Remove one proton from \(NH_4^+\).
The ammonium ion is \[ NH_4^+ \] When it loses one proton, \[ NH_4^+ \rightarrow NH_3 + H^+ \] Therefore, the species formed is \[ NH_3 \]
Step 3: Verify the conjugate acid-base pair.
The pair is \[ NH_4^+/NH_3 \] where \[ NH_4^+ \] acts as the acid and \[ NH_3 \] acts as its conjugate base.
Step 4: Analyze the other options.
\[ NH^{2-} \] and \[ NH_2^- \] are not obtained by removing only one proton from \(NH_4^+\).
\[ NH_4OH \] is ammonium hydroxide and is not the conjugate base of \(NH_4^+\).
Step 5: Final conclusion.
Hence, the conjugate base of \[ NH_4^+ \] is \[ \boxed{NH_3} \] Therefore, the correct option is \[ \boxed{(2)} \]
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