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Acid strength is the tendency of an acid, symbolised by the chemical formula HA {\displaystyle {\ce {HA}}} , to dissociate into a proton, H + {\displaystyle {\ce {H+}}} , and an anion, A − {\displaystyle {\ce {A-}}} . The dissociation of a strong acid in solution is effectively complete, except in its most concentrated solutions.
Examples of strong acids are hydrochloric acid {\displaystyle {\ce {}}} , perchloric acid {\displaystyle {\ce {}}} , nitric acid {\displaystyle {\ce {}}} and sulfuric acid {\displaystyle {\ce {}}} .
A weak acid is only partially dissociated, with both the undissociated acid and its dissociation products being present, in solution, in equilibrium with each other.
Acetic acid is an example of a weak acid. The strength of a weak acid is quantified by its acid dissociation constant, K a {\displaystyle K_{{\ce {a}}}} value.