Editing Chemical reaction (section)

===Acid–base reactions===
In the [[Brønsted–Lowry acid–base theory]], an [[acid–base reaction]] involves a transfer of [[proton]]s (H<sup>+</sup>) from one species (the [[acid]]) to another (the [[base (chemistry)|base]]). When a proton is removed from an acid, the resulting species is termed that acid's [[conjugate acid|conjugate base]]. When the proton is accepted by a base, the resulting species is termed that base's [[conjugate acid]].<ref>{{GoldBookRef|title=conjugate acid–base pair|file=C01266}}</ref> In other words, acids act as proton donors and bases act as proton acceptors according to the following equation:
<chem display="block">\underset{acid}{HA} + \underset{base}{B} <=> \underset{conjugated\ base}{A^-} + \underset{conjugated\ acid}{HB+}</chem>

The reverse reaction is possible, and thus the acid/base and conjugated base/acid are always in equilibrium. The equilibrium is determined by the [[acid dissociation constant|acid and base dissociation constants]] (''K''<sub>a</sub> and ''K''<sub>b</sub>) of the involved substances. A special case of the acid-base reaction is the [[neutralization (chemistry)|neutralization]] where an acid and a base, taken at the exact same amounts, form a neutral [[Salt (chemistry)|salt]].

Acid-base reactions can have different definitions depending on the acid-base concept employed. Some of the most common are:
* [[Acid–base reaction#Arrhenius definition|Arrhenius]] definition: Acids dissociate in water releasing H<sub>3</sub>O<sup>+</sup> ions; bases dissociate in water releasing OH<sup>−</sup> ions.
* [[Brønsted–Lowry acid–base theory|Brønsted–Lowry]] definition: Acids are proton (H<sup>+</sup>) donors, bases are proton acceptors; this includes the Arrhenius definition.
* [[Acid–base reaction#Lewis definition|Lewis]] definition: Acids are electron-pair acceptors, and bases are electron-pair donors; this includes the Brønsted-Lowry definition.