CONJUGATE ACID

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
:HX + H₂O $$
ightleftarrows X⁻ + H₃O⁺
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.)

Acid	Base
HCl Hydrochloric acid	Cl− Chloride ion
H2SO4 Sulfuric acid	HSO4− Hydrogen sulfate ion
HNO3 Nitric acid	NO3− Nitrate ion
H3O+ Hydronium ion	H2O Water
HSO4− Hydrogen sulfate ion	SO42− Sulfate ion
H3PO4 Phosphoric acid	H2PO4− Dihydrogen phosphate ion
HC2H3O2 Acetic acid	C2H3O2− Acetate ion
H2CO3 Carbonic acid	HCO3− Hydrogen carbonate ion
H2S Hydrosulfuric acid	HS− Hydrogen sulfide ion
H2PO4− Dihydrogen phosphate ion	HPO42− Hydrogen phosphate ion
NH4+ Ammonium ion	NH3 Ammonia
HCO3− Hydrogencarbonate ''(bicarbonate)'' ion	CO32− Carbonate ion
HPO42− Hydrogen phosphate ion	PO43− Phosphate ion
H2O Water (neutral, pH 7)	OH− Hydroxide ion
HFSbF5 Fluoroantimonic acid	SbF5− Antimony pentafluoride ion

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See also

See also

★ protonation