Final answer:
In the reaction HNO₃⁺ + H₂O ↔ H₃O⁺ + NO₃⁻, HNO₃⁺ is the acid and H₂O is the base. The products H₃O⁺ and NO₃⁻ are the conjugate acid and base, respectively. The equilibrium lies predominantly to the right since the reaction favors the formation of the weaker acid and base.
Step-by-step explanation:
According to the Brønsted-Lowry definition, an acid is a proton donor and a base is a proton acceptor. In the reaction HNO₃⁺ + H₂O ↔ H₃O⁺ + NO₃⁻, the acid is HNO₃⁺ because it donates a proton to water, and the water (H₂O) acts as a base because it accepts a proton. The products of this reaction are H₃O⁺ (the conjugate acid of water) and NO₃⁻ (the conjugate base of HNO₃⁺).
To predict where the equilibrium lies, we consider the relative strengths of the acids and bases on both sides of the reaction. Since HNO₃ is a strong acid, its conjugate base, NO₃⁻, will be a weak base. Similarly, water is a much weaker acid compared to HNO₃. Thus, the equilibrium of the reaction favors the formation of the weaker acid (H₃O⁺) and the weaker base (NO₃⁻), meaning it will lie predominantly to the right.