Question

The conjugate base of \(NH_4^+\) is:

• A. \(NH^{2-}\)
• B. \(NH_3\)
• C. \(NH_2^{-}\)
• D. \(NH_4OH\)

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 \(NH_4^+\).

Answer 1

The Correct Option is B

Step 1: Apply Bronsted-Lowry definition.
Conjugate base = acid minus one proton (H\(^+\)).

Step 2: Remove H\(^+\) from NH\(_4^+\).
NH\(_4^+\) - H\(^+\) = NH\(_3\). So NH\(_3\) is the conjugate base of NH\(_4^+\). \[ oxed{NH_3} \]