BrønstedEmäs

BrønstedEmäs refers to a Brønsted-Lowry base. This theory, developed by Johannes Nicolaus Brønsted and Thomas Martin Lowry independently in 1923, defines an acid as a proton (H+) donor and a base as a proton acceptor. Therefore, a BrønstedEmäs is a substance that can accept a proton from another substance.

When a BrønstedEmäs accepts a proton, it typically forms its conjugate acid. For example, ammonia (NH3) is a BrønstedEmäs because it can accept a proton from water, forming the ammonium ion (NH4+), which is its conjugate acid. Water acts as the Brønsted acid in this reaction. Conversely, in the reverse reaction, the ammonium ion can donate a proton, acting as a Brønsted acid, and ammonia acts as its conjugate base.

Common examples of BrønstedEmäs include hydroxide ions (OH-), ammonia (NH3), and amines (RNH2, R2NH, R3N). Many salts of weak acids, such as sodium acetate (CH3COONa), also exhibit BrønstedEmäs behavior in aqueous solutions because the anion (acetate ion, CH3COO-) can accept a proton from water. The strength of a BrønstedEmäs is related to its ability to accept protons, which is inversely related to the strength of its conjugate acid. A strong BrønstedEmäs corresponds to a weak conjugate acid, and a weak BrønstedEmäs corresponds to a strong conjugate acid. This concept is fundamental in understanding acid-base reactions and equilibrium in chemistry.