To use all functions of this page, please activate cookies in your browser.
With an accout for my.chemeurope.com you can always see everything at a glance – and you can configure your own website and individual newsletter.
- My watch list
- My saved searches
- My saved topics
- My newsletter
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. A conjugate acid can also be seen as the chemical substance that releases a proton in the backward chemical reaction. Thus, the term acid. The base produced, X−, is called the conjugate base and it absorbs a proton in the backward chemical reaction. In aqueous solution, the chemical reaction involved is of the form
Additional recommended knowledge
This principle is discussed in detail in the article on acid-base reaction theories.
The conjugate base of a weak acid is a strong base, and the conjugate base of a strong acid is a weak base, and vice versa.
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.)
|This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Conjugate_acid". A list of authors is available in Wikipedia.|