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The Bronsted-Lowry definition of acids and bases is pretty simple. An acid is a proton donor, and a base is a proton acceptor. In the example of ammonia dissolving in water (NH3 + H2O = NH4+ + OH-) the water donates a proton, so it is the acid.he hydroxide ion is accepting the proton and is called a conjugate base. Every Bronsted-Lowry acid has a conjugate base, and every Bronsted-Lowry base has a conjugate acid. 1  Conjugate acid: an acid that forms when a base gains a proton. 2  Conjugate base: a base that forms when an acid loses a proton.
Conjugate Acid-Base Pairs. Acids and bases exist as conjugate acid-base pairs. The term conjugate comes from the Latin stems meaning joined together and refers to things that are joined, particularly in pairs, such as Brnsted acids and bases. Every time a Brnsted acid acts as an H+-ion donor, it forms a conjugate base. Imagine a generic acid, HA. When this acid donates an H+ ion to water, one product of the reaction is the A- ion, which is a hydrogen-ion acceptor, or Brnsted base.