Identify the Bronsted-Lowry acid in the following reaction.
H2O (l) + HCO31- (aq) → H3O+ (aq) + CO32- (aq)
In the given reaction, the Bronsted-Lowry acid is H2O (water).
To identify the Bronsted-Lowry acid in this reaction, we need to understand the concept of Bronsted-Lowry acids and bases.
According to the Bronsted-Lowry theory, an acid is a substance that donates a proton (H+ ion), while a base is a substance that accepts a proton. In this reaction, we need to identify which species donates a proton.
In the given reaction: H2O (l) + HCO31- (aq) → H3O+ (aq) + CO32- (aq)
H2O is a molecule of water, and HCO31- is the bicarbonate ion. H3O+ is the hydronium ion, and CO32- is the carbonate ion.
H2O donates a proton (H+) to form H3O+, so H2O is acting as an acid in this reaction and can be identified as the Bronsted-Lowry acid.