In the field of chemistry, in the Brřnsted-Lowry (protonic) theory of acids and bases, a conjugate base is the basic member, X-, of a pair of compounds that differ only by the presence or absence of a proton at a certain position. The acid produced by gain of a proton, HX, is called the conjugate acid.
All acids have a conjugatebase, which is formed when their proton has been donated; likewise, all bases have a conjugate acid, formed after they have accepted a proton.
The pH of a solution is calculated as the negative logarithm in base 10 of the hydronium ion concentration—it is an expression of the molar concentration of H
A natural consequence of the Brønsted-Lowry definitions of acids and bases, perhaps a diabolical one, is that we end up with a very interesting relationship between acids and bases.
When a base accepts a proton, the resulting chemical is called the conjugate acid of that original base.
Being able to recognize conjugate pairs of acids and bases becomes important dealing with comparisons between the strengths of acids and bases, buffered solutions, and the hydrolysis of various salts.
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