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Explanation:

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Bronsted- Lowry definition helps to explain why ammonia is a base.

Explanation:

The Brönsted - Lowry theory states that acids are substances capable of yielding protons (hydrogen H⁺ ions) and substance bases capable of accepting them.

Then, the acid-base reaction is one in which a transfer of H⁺ protons occurs from an acid to a base.

A base acid conjugate pair is then produced, where the base conjugate acid is the one formed when the base receives an H⁺; and the conjugate base of the acid, is the base formed when the acid yields an H⁺.

You know this reaction:

H₂O (l) + NH₃ (aq) → OH⁻ (aq) + NH₄⁺ (aq)

In this case you can see that the water acts as an acid, because it gives a proton to the ammonia. Then the ammonia will act as the basis for accepting the proton. The conjugate base of water is the hydroxide ion (OH⁻) and the conjugated acid of ammonia is the ammonium ion (NH₄⁺).

Then, Bronsted- Lowry definition helps to explain why ammonia is a base.