Explain : Oxidation of Cl^(-) ion is carried out near anode when electrolysis of aqueous (Concentrated) NaCl solution is carried out using inert electrode. OR Oxidation of species depend upon its oxidation potential, oxidation reaction is possible for E^(Theta) whose value is less.

Explain : Oxidation of Cl^(-) ion is carried out near anode when elect

1.	Explain : Oxidation of Cl^(-) ion is carried out near anode when electrolysis of aqueous (Concentrated) NaCl solution is carried out using inert electrode. OR Oxidation of species depend upon its oxidation potential, oxidation reaction is possible for E^(Theta) whose value is less.
Answer» Solution :* `NaCl_((aq)) to Na_((aq))^(+)+Cl_((aq))^(+)` Here, near anode `Cl^(-)` ions of NaCl and WATER is present. So, two OXIDATION reaction is possible: (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` * "Reaction with less `E^(Theta)` value will occur near anode." So, INSTEAD of `Cl^(-)` ions oxidation of water occur. But due to over potential of oxygen, water does not GET oxidized but oxidation of `Cl^(-)` near anode is possible and produced `Cl_(2)` gas.