Within the Brønsted-Lowry (protonic) theory of acids and bases, a conjugate acid is the acid member, HX, of a pair of two compounds that transform into each other by gain or loss of a proton. The base produced, X-, is called the conjugate base. In aqueous solution, the chemical reaction involved is of the form Johannes Nicolaus Brønsted (February 22, 1879-December 17, 1947) was a Danish physical chemist. ... Thomas Martin Lowry (October 26, 1874–November 2, 1936) was an English physical chemist. ... For alternative meanings see proton (disambiguation). ... An acid-base reaction is a chemical reaction between an acid and a base. ...
HX + H2O ↔ X- + H3O+
This principle is discussed in detail in the article on acid-base reaction theories. An acid-base reaction is a chemical reaction between an acid and a base. ...
Tabulated below are several examples of conjugate acid-base pairs. Acid strength decreases and base strength increases down the table. (The dissociation reaction reaches equilibrium further to the right, with more X- produced.)
When the elements chlorine, bromine, and iodine were identified and the absence of oxygen in the hydrohalic acids was established by Sir Humphry Davy in 1810, this definition had to be rejected.
In general, an acid reacts with a base by forming a new covalent bond utilizing an empty orbital of the acid to share the extra electron pair of the base.
From the perspective of Molecular Orbital theory, an acid-base reaction is the combination of HOMO from base and LUMO from acid to form a stable bonding molecular orbital.
Within the Brønsted-Lowry (protonic) theory of acids and bases, a conjugateacid is the acid member, HX, of a pair of two compounds that transform into each other by gain or loss of a proton.
Tabulated below are several examples of conjugateacid-base pairs.
Acid strength decreases and base strength increases down the table.
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