Acid-base reactions Bransted-Lowry theory

According to the Arrhenius theory, acids (HA) are substances that dissociate in water to produce H + (aq). Bases (MOH) are substances that dissociate to yield OH aq). The more general Bransted-Lowry theory defines an acid as a proton donor, a base as a proton acceptor, and an acid-base reaction as a proton-transfer reaction. Examples of Bronsted-Lowry acids are HC1, NH4+, and HSO4- examples of Bronsted-Lowry bases are OH-, F-, and NH3. 

In the Bransted-Lowry theory, every acid-base reaction creates its conjugate acid-base pair. In the above reaction HCl is an acid which, after giving up a proton, becomes a conjugate base, Cl . Similarly, water is a base which, after accepting a proton, becomes a conjugate acid, the hydronium ion. 

This reaction is essentially an acid-base process, which is most conveniently explained in terms of the Bransted-Lowry theory of acids and bases (see Section 1.23). 

The Bransted-Lowry Theory of Acids and Bases COAL 2 Given the equation for a Br0nsted-Lowry acid-base reaction, explain how or why it can be so classified. 

Describe an acid-base reaction in the context of Bransted-Lowry theory, and identify conjugate acid-base pairs. 

B) From the foregoing, it is clear that the Arrhenius or solvents theory cannot work for aprotic solvents most adequate here is the Bransted-Lowry or proton theory, in which an acid is defined as a proton donor and a base as a proton acceptor, and under conditions such that the acid by donating its proton is converted into its conjugate base, and the base by accepting a proton is converted into its conjugate acid. This mutual relationship is illustrated by the following equilibrium reaction ... 

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See also in sourсe #XX -- [ , ]

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