In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. b. CH₃NH₂(aq) + H₂O(l) ⇌ CH₃NH₃⁺(aq) + OH^–(aq)

Key Concepts

Brønsted–Lowry Acid-Base Theory

The Brønsted–Lowry theory defines acids as proton donors and bases as proton acceptors. In this framework, an acid-base reaction involves the transfer of protons (H+) from the acid to the base. This theory expands the understanding of acid-base reactions beyond just the presence of hydroxide ions, allowing for a broader range of substances to be classified as acids or bases.

Conjugate Acid and Conjugate Base

In the context of Brønsted–Lowry theory, a conjugate acid is formed when a base accepts a proton, while a conjugate base is formed when an acid donates a proton. These pairs are related; for every acid, there is a corresponding conjugate base, and for every base, there is a corresponding conjugate acid. Understanding these relationships is crucial for analyzing acid-base reactions.

Identifying Species in Reactions

To analyze acid-base reactions, it is essential to identify the reactants and products involved. In the given reaction, CH3NH2 acts as a base by accepting a proton from water (H2O), which acts as an acid. The products, CH3NH3+ and OH-, represent the conjugate acid and conjugate base, respectively. Recognizing these roles is key to understanding the dynamics of the reaction.