Statement A: The electrolysis of aqueous NaCI solution gives hydrogen gas at the cathode and chlorine gas at the anode.Statement B: Chlorine has higher oxidation potential than water.

In aqueous solution, water is available in plenty. Water can undergo both Oxidation and reduction.H2O→O2(g)+4H+1+2e-1; E0=-1.23V 2H2O+2e-1→H2(g)+2OH-1; E0=-0.83V 2Cl-1→Cl2(g)+2e-1;E0=-1.36VAt Anode, Water competes with Chloride ion to undergo Oxidation. But, due to higher over voltage, the Oxidation of Water becomes energetically unfavourable and the Chloride ion is Oxidised to Chlorine gas.At Cathode, Water competes with Na+1 ion to undergo reduction. But, the reduction of Na+1is energetically more difficult than the reduction of water as SRP of Na+1is -2.71V whereas the SRP of Water is -0.83V. So, Water is readily reduced in to Hydrogen gas.Chlorine has higher reduction potential (+1.36V) than water (+1.23V).