According to Bronsted
Lowery concept, a strong acid has weak conjugate base and vice
versa.
The given oxy acids of
chlorine HCIO, HCIO2, HClO3 and HClO4 and their conjugate bases are CIO-,
CIO2-, ClO3-, ClO4- respectively. These anions are stabilised to
greater extent, due to the presence of π-bond and lone pair, if number of
π-bond increase extent of stabilisation increase. In case of ClO- there is no π-bond hence if form less stable
conjugate base hence act as weak acid while in case of ClO4- it has three pπ-dπ bond which stablised greater extent and form more
stable conjugate base hence it conjugate acid (HClO4) is strongest
acid. Oxy acids of chlorine and their number of pπ-dπ bonds given as:
HOCI (0~Pπ-dπ)
HOCIO (1~Pπ-dπ)
HOClO2 (2~Pπ-dπ)
HOCIO3 (3~Pπ-dπ)
Thus overall order of
acidic strength of oxy acids of chlorine is as:
"HClO < HClO2 < HClO3 < HClO4"
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