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In many species, a transition metal has an unusually high or low oxidation state. Write a balanced equation (including states
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Ans :-

Fe3+ (aq) + ClO- (aq) -----------------> FeO42- (aq) + Cl- (aq) + H2O (l)

Reaction at anode :

Fe3+ (aq) + 4H2O (l) -----------------> FeO42- (aq) + 8H+ (aq) + 3e-

Adding 8OH- on both sides, in order to convert this equation into basic medium :

Fe3+ (aq) + 8OH- -----------------> FeO42- (aq) + 4H2O (l) + 3e- .................(1)

Reaction at cathode :

ClO- (aq) + 2H+ + 2e- -----------------> Cl- (aq) + H2O (l)

Adding 2OH- on both sides, in order to convert this equation into basic medium :

ClO- (aq) + H2O (l)  + 2e- -----------------> Cl- (aq) + 2OH-  .................(2)

Add equations (1) and (2) after multiply equation (1) by 2 and equation (2) by 3, the balanced chemical equation in basic medium is :

2Fe3+ (aq) + 3ClO- (aq) + 10OH- ----> 2FeO42- (aq) + 5H2O (l) + 3Cl- (aq)

Oxidation of transition metal is +6.

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