Identify the Brønsted–Lowry acid–base pairs in each of the following equations: b. NH4⁺(aq) + H₂O(l)⇄NH₃(aq) + H₃O⁺(aq)

Verified step by step guidance

1. Identify the species that donates a proton (H⁺) in the reaction. This species is the Brønsted–Lowry acid.
2. Identify the species that accepts a proton (H⁺) in the reaction. This species is the Brønsted–Lowry base.
3. In the given equation, NH₄⁺ donates a proton to form NH₃. Therefore, NH₄⁺ is the acid, and NH₃ is its conjugate base.
4. H₂O accepts a proton to form H₃O⁺. Therefore, H₂O is the base, and H₃O⁺ is its conjugate acid.
5. The Brønsted–Lowry acid–base pairs are: (NH₄⁺, NH₃) and (H₂O, H₃O⁺).

Key Concepts

Brønsted–Lowry Theory

The Brønsted–Lowry theory defines acids as proton donors and bases as proton acceptors. This framework allows for a broader understanding of acid-base reactions beyond just the presence of hydroxide ions or hydronium ions. In this theory, the transfer of protons (H⁺ ions) between species is the central focus, making it essential for analyzing chemical equations involving acids and bases.

Acid-Base Pairs

An acid-base pair consists of two species that differ by the presence or absence of a proton. In the context of the Brønsted–Lowry theory, when an acid donates a proton, it transforms into its conjugate base, while the base that accepts the proton becomes its conjugate acid. Identifying these pairs in a reaction helps in understanding the dynamics of proton transfer and the equilibrium established in the reaction.

Equilibrium in Acid-Base Reactions

Acid-base reactions often reach a state of equilibrium, where the rates of the forward and reverse reactions are equal. This means that the concentrations of reactants and products remain constant over time. Understanding this concept is crucial for analyzing the given equation, as it allows for the identification of the predominant species and the direction of the reaction based on the strength of the acids and bases involved.