With the help of Lowry-Bronsted concept show that `HCIO_(4)` is a stronger acid than `HCIO_(3)` when dissolved is water.

Explanation

The dissociation of both the acids in aqueous solution may be shown as :
`{:(HCIO_(4),+,H_(2)O ,hArr,H_(3)O^(+) ,+,CIO_(4)^(-)),("Acid"-I,,"Base-II",,"Acid-II",,"Base-II"):}`
`{:(HCIO_(3),+,H_(2)O ,hArr,H_(3)O^(+) ,+,CIO_(3)^(-)),("Acid"-I,,"Base-II",,"Acid-II",,"Base-II"):}`
Perchlorate `(CIO_(4)^(-))` is a weak base than chlorate `(CIO_(3)^(-))`ion because the negative charge on it is dispersed on four oxygen atoms whereas in chlorate `(CIO_(3)^(-))` ion , three oxygen atoms are available to accommodate negative charge. According to the theory a weak base has a strong conjugate acid. Therefore `HCIO_(4)` is a stronger acid than `HCIO_(3).`