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    • Apr 17, 2022
    • 1 min read

Theories of Acids and Bases

Updated: Apr 25, 2022

An overview of three theories used to describe acids and bases.


Arrhenius Theory


Arrhenius Acids - produce H+ ions in water H+(aq) Arrhenius Bases - produce OH– ions in water OH-(aq)


The theory explains the reaction between H+ and OH- to give water (neutralisation)


Limitation

The definition is not applicable to:

  • a base that doesn’t contain OH– for example ammonia

  • species that are part of gaseous systems, such as hydrogen chloride

  • species that are insoluble.


Brønsted–Lowry Theory


THE definition for A Level Chemistry:


Brønsted acid - H+/proton donor Brønsted base - H+/proton acceptor


Much more general than the Arrhenius Theory

Species need not be soluble in water.

A Brønsted base doesn’t need to form OH-.


Lewis Theory

Lewis acids are electron pair acceptors Lewis bases are electron pair donors


There’s no need for the Lewis acid to form H+.


In the graphic above, NH3 is a Lewis base - the nitrogen in NH3 donates a lone pair of electrons.



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