Which of the following is never a Bronsted-Lowry base in an aqueous solution?

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BlackTom AI · Accepted Answer

The question asks which species is never a Bronsted-Lowry base in an aqueous solution.
First, recall the Bronsted-Lowry definitions: a base is a substance that accepts a proton (H+), while an acid donates a proton.
In aqueous solution, ammonium ion (NH4+) is the conjugate acid of ammonia (NH3). The relevant equilibrium is NH4+ + H2O ⇌ NH3 + H3O+. Here NH4+ donates a proton to water, forming NH3 and H3O+, which is characteristic of acidic behavior, not basic.
Therefore, NH4+ cannot act as a Bronsted-Lowry base in water because its typical role is to donate protons rather than accept them.
(If we consider other species, some may act as bases by accepting protons, but NH4+ is not among them in aqueous solution.)
Since the provided correct answer is NH4+, this aligns with the understanding that NH4+ is an acid in water and not a base.

CHM-1020-LD01.2025SU Practice Exam II

Which of the following is never a Bronsted-Lowry base in an aqueous solution?

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