Final answer:
In the reaction between NH₂⁻ and H₃O⁺, NH₂⁻ acts as a Brønsted-Lowry base by accepting a proton to become NH₃, while H₃O⁺ donates a proton to become H₂O, acting as a Brønsted-Lowry acid.
Step-by-step explanation:
If H₃O⁺ is a Brønsted-Lowry acid, we can write a reaction equation where it donates a proton to NH₂⁻, which will act as a Brønsted-Lowry base. The correct balanced reaction would be:
NH₂⁻ + H₃O⁺ → NH₃ + H₂O
In this reaction, NH₂⁻ accepts a proton to become NH₃, and the hydronium ion H₃O⁺ donates a proton to become water (H₂O). Thus, NH₂⁻ is the Brønsted-Lowry base, and H₃O⁺ is the Brønsted-Lowry acid.