In each reaction, identify the Brønsted–Lowry acid, the Brønsted–Lowry base, the conjugate acid, and the conjugate base. a. H₂CO₃(aq) + H₂O(l) ⇌ H₃O⁺(aq) + HCO₃^–(aq) c. HNO₃(aq) + H₂O(l) → H₃O⁺(aq) + NO₃^–(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 releases a hydrogen ion (H+) in a reaction, while a base accepts that ion. This theory expands the understanding of acid-base reactions beyond just the presence of hydroxide ions, allowing for a broader range of chemical interactions.

Conjugate Acid and Base

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

Identifying Species in Reactions

To analyze acid-base reactions, it is essential to identify the roles of each species involved. In the given reaction, H2CO3 acts as the Brønsted–Lowry acid by donating a proton to H2O, which acts as the Brønsted–Lowry base. The resulting H3O+ is the conjugate acid of water, while HCO3- is the conjugate base of carbonic acid, illustrating the dynamic nature of these chemical species.