Brønsted-Lowry

Encyclopedia : B : BR : BRN : Brønsted-Lowry

In chemistry, Brønsted-Lowry refers to a theory which defines acids and bases. This acid-base theory was independently proposed by Johannes Nicolaus Brønsted and Thomas Martin Lowry in 1923. In this system, a Brønsted-Lowry acid is defined as any substance which donates a hydrogen ion or proton (H⁺) in a reaction; and a base as a substance which receives a proton in a reaction. Thus other substances such as water molecules can have behaviours not defined in the common definition of an acid or base.

In the reaction between acetic acid and water, acetic acid acts as an acid by donating a proton to water, which acts as a base. The equation given is:

[\mbox_3\mbox + \mbox_2\mbox \longrightarrow \mbox_3\mbox^\mbox + \mbox_3\mbox^-]

Water can also act as an acid, for instance when it reacts with ammonia. The equation given for this reaction is:

[\mbox_3 + \mbox_2\mbox \longrightarrow \mbox_4^} + \mbox^-]

in which H₂O donates a proton to NH₃. Thus water is amphoteric: able to act as either an acid or a base. These reactions can act in reverse as well as in the forward direction. The reverse of the reaction between acetic acid and water is:

[\mbox_3\mbox^ + \mbox_3\mbox^- \longrightarrow \mbox_3\mbox + \mbox_2\mbox]

In the reverse reactions H₃O⁺ acts as an acid to donate a proton to CH₃COO^-, which is acting as a base. In the forward reaction, CH₃COOH acts as an acid to donate a proton, and water as a base to receive it. H₂O and H₃O⁺ are therefore considered one acid-base conjugate pair, and CH₃COOH and CH₃COO^- as another conjugate pair.

Brønsted-Lowry

See also