The ammonium ion (NH_4^+) acts as: | vedclass

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(A) According to the Bronsted-Lowry theory,an acid is a proton $(H^+)$ donor and a base is a proton acceptor.$NH_4^+$ can donate a proton to form $NH_

Vedclass · Accepted Answer

Conjugate acid

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(A) According to the Bronsted-Lowry theory,an acid is a proton $(H^+)$ donor and a base is a proton acceptor.$NH_4^+$ can donate a proton to form $NH_3$ $(NH_4^+ \rightarrow NH_3 + H^+)$,therefore it acts as a conjugate acid of the base $NH_3$.It cannot accept a proton to form $NH_5^{2+}$,so it does not act as a base in this context.Thus,$NH_4^+$ acts as a conjugate acid.

The ammonium ion $(NH_4^+)$ acts as:

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