According to the Bronsted-Lowry definition of acids and bases, is water an acid or base? Provide examples to support.
According to the Bronsted-Lowry definition, an acid is a substance that donates a proton (H+) in a chemical reaction, while a base is a substance that accepts a proton. Water (H2O) can act both as an acid and a base, depending on the context.
When water donates a proton (H+), it behaves as an acid. For example, in the reaction with ammonia (NH3), water donates a proton to ammonia:
H2O + NH3 -> NH4+ + OH-
In this reaction, water is acting as an acid by donating a proton (H+) to ammonia.
On the other hand, when water accepts a proton (H+), it acts as a base. For instance, in the reaction with hydrochloric acid (HCl), water accepts a proton from hydrochloric acid:
H2O + HCl -> H3O+ + Cl-
In this reaction, water is acting as a base by accepting a proton (H+) from hydrochloric acid.
So, according to the Bronsted-Lowry definition, water can function as both an acid and a base, depending on the reaction it participates in.