Here's how it works:
* Brønsted-Lowry Definition: This definition defines an acid as a proton donor and a base as a proton acceptor.
* Ammonia's Reaction: When ammonia reacts with water, it accepts a proton from a water molecule, forming the ammonium ion (NH₄⁺) and hydroxide ion (OH⁻):
```
NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq)
```
* Proton Acceptance: As ammonia gains a proton (H⁺) in this reaction, it acts as a base.
Key Points:
* Ammonia's lone pair of electrons on the nitrogen atom allows it to readily accept a proton.
* The formation of hydroxide ions (OH⁻) in the reaction is also characteristic of a base.
Therefore, based on its ability to accept a proton, ammonia is classified as a base according to the Brønsted-Lowry definition.
