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)

Verified step by step guidance

1. Identify the Brønsted–Lowry acid: Look for the species that donates a proton (H+). In this reaction, H2CO3 donates a proton to H2O.
2. Identify the Brønsted–Lowry base: Look for the species that accepts a proton. In this reaction, H2O accepts a proton from H2CO3.
3. Determine the conjugate acid: This is the species formed when the base gains a proton. Here, H3O+ is the conjugate acid formed from H2O.
4. Determine the conjugate base: This is the species formed when the acid loses a proton. Here, HCO3- is the conjugate base formed from H2CO3.
5. Summarize the roles: H2CO3 is the Brønsted–Lowry acid, H2O is the Brønsted–Lowry base, H3O+ is the conjugate acid, and HCO3- is the conjugate base.

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.