Identify the Brønsted–Lowry acid and the Brønsted– Lowry base on the left side of each equation, and also identify the conjugate acid and conjugate base of each on the right side. (a) HBrO1aq2 + H2O1l2ΔH3O+1aq2 + BrO-1aq2

Key Concepts

Brønsted–Lowry Acid-Base Theory

The Brønsted–Lowry theory defines acids as proton donors and bases as proton acceptors. This framework emphasizes the transfer of protons (H⁺ ions) during chemical reactions, allowing for a broader understanding of acid-base behavior beyond just the presence of hydroxide or hydronium ions.

Conjugate Acid-Base Pairs

In the Brønsted–Lowry theory, a conjugate acid is formed when a base gains a proton, while a conjugate base is what remains after an acid donates a proton. This relationship highlights the reversible nature of acid-base reactions, where the products can act as acids or bases in subsequent reactions.

Identifying Species in Reactions

To analyze acid-base reactions, it is essential to identify the reactants and products correctly. In the given equation, recognizing which species donate or accept protons allows for the determination of the Brønsted–Lowry acid and base, as well as their corresponding conjugate pairs, facilitating a deeper understanding of the reaction dynamics.