(b) (i) Account for the acidic nature of HCIO_(4) In terms of Bronsted - Lowry theory, identify its conjugate base. (ii) Is it possible to store copper sulphate in an iron vessel for a long time? Given: E_(Cu^(2+)//Cu)^(@) = 0.34 V and E_(Fe^(2+)//Fe)^(@) = +0.44 V

(b) (i) Account for the acidic nature of HCIO_(4) In terms of Bronste

1.	(b) (i) Account for the acidic nature of HCIO_(4) In terms of Bronsted - Lowry theory, identify its conjugate base. (ii) Is it possible to store copper sulphate in an iron vessel for a long time? Given: E_(Cu^(2+)//Cu)^(@) = 0.34 V and E_(Fe^(2+)//Fe)^(@) = +0.44 V
Answer» Solution :(b) (i) `HClO_(4) 1) According to Lowry - Bronsted concept, a strong acid has weak conjugate base and a weak acid has a strong conjugate base. (ii) Let us consider the stabilities of the conjugate bases `ClO_(4)^(-), ClO_(3)^(-), ClO_(2)^(-)` and `CIO^(-)`formed from these acid `HClO_(4),HClO_(3),HClO_(2)`, HOCl respectively. These ANIONS are stabilized to greater extent, it has lesser attraction for proton and THEREFORE, will BEHAVE as weak base. Consequently the corresponding acid will be STRONGEST because weak conjugate base has strong acid and strong conjugate base has weak acid. `ClO_(4)^(-)` is the conjugate base of the acid `HClO_(4)`. (ii) `E_("cell")^(@) = E_("ox")^(@) + E_("red")^(@) = 0.44 V + 0.34 V = 0.78 V` These `+ve E_("cell")^(@)` values shows that iron will oxidise and copper will get reduced i.e., the vessel will dissolve. Hence it is not possible to store copper sulphate in an iron vessel.