Value of standard electrode potential for the oxidation of Cl^(-) ions is more positive than that of water, even then in the electrolysis of aqueous sodium chloride, why is Cl^(-) oxidised at anode instead of water ?

Value of standard electrode potential for the oxidation of Cl^(-) ions

1.	Value of standard electrode potential for the oxidation of Cl^(-) ions is more positive than that of water, even then in the electrolysis of aqueous sodium chloride, why is Cl^(-) oxidised at anode instead of water ?
Answer» Solution :* Usually, the electrode with less potential undergoes OXIDATION REACTION. (i) `Cl_((aq))^(-)to (1)/(2) Cl_(2(g))+e^(-),E_(cell)^(Theta)=1.36V` (ii) `2H_(2)O_((l)) to O_(2(g))+4H_((aq))^(+)+4e^(-),E_(cell)^(Theta)=1.23V` * According to above reaction, water has low `E_(cell)^(Theta)` value, should be get oxidized but oxidation of `Cl^(-)` is observed. * Due to over potential of OXYGEN reaction (i) is possible ut reaction (ii) is not possible. for oxidation of water over potential is REQUIRED, water has low potential so it will not give oxidation reaction but `Cl^(-)` give oxidation and get converted into `Cl_(2)`.