In liquid ammonia, the reaction of hydroxide ion (OH⁻) with ammonia (NH₃) demonstrates its basic nature. Here's the chemical equation:

OH⁻ (l) + NH₃ (l) ⇌ NH₂⁻ (l) + H₂O (l)

Explanation:

* OH⁻ (l): Hydroxide ion in liquid ammonia.

* NH₃ (l): Liquid ammonia, acting as a solvent and a weak acid.

* NH₂⁻ (l): Amide ion, the conjugate base of ammonia, formed by the removal of a proton (H⁺).

* H₂O (l): Water, formed by the combination of the proton removed from ammonia and the hydroxide ion.

Mechanism:

Hydroxide ion, being a strong base in liquid ammonia, readily accepts a proton from ammonia. This results in the formation of the amide ion (NH₂⁻), a stronger base than ammonia, and water. This reaction highlights the Brønsted-Lowry definition of acids and bases, where a base accepts a proton.

Note: This reaction lies heavily to the right, indicating that the hydroxide ion is a strong base in liquid ammonia and readily reacts to form the amide ion.