H2SO4(aq) + H2O(l) ⟶ H3O+(aq) + HSO4–(aq) (Stage I)

Identify the Brønsted-Lowry acid and base in the reaction.

In the reaction H2SO4(aq) + H2O(l) ⟶ H3O+(aq) + HSO4–(aq) (Stage I), the Brønsted-Lowry acid is H2SO4 and the Brønsted-Lowry base is H2O.

To identify the Brønsted-Lowry acid and base in the given reaction, we need to understand the concept of acids and bases according to the Brønsted-Lowry theory.

According to the Brønsted-Lowry theory, an acid is a substance that donates a proton (H+) and a base is a substance that accepts a proton (H+). In this reaction, the H2SO4(aq) donates a proton, so it acts as an acid, and H2O(l) accepts a proton, so it acts as a base.

Therefore, in the given reaction:
- The Brønsted-Lowry acid is H2SO4(aq) because it donates a proton (H+).
- The Brønsted-Lowry base is H2O(l) because it accepts a proton (H+).

Note: H3O+ and HSO4– are the resulting species formed after the acid-base reaction.

acid that donates a proton is H2SO4

base that accepts proton is H2O