Given are the reactions occuring during the electrolysis of sodium chloride solution:
2Cl−→Cl2+2e−
2H2O+2e−→H2+2OH−
Which of the following is correct regarding liberation of electrolytic products?
Water plays a vital role during the electrolysis of NaCl solution. Since water can be both oxidized and reduced, it competes with the dissolved Na+ and Cl− ions. Having a greater tendency to get reduced than sodium ions, water gets reduced and produces hydrogen. Reduction takes place at cathode and hydrogen gas is evolved at the cathode. Similarly, Cl− has a greater tendency than water to get oxidised so it gets oxidised and produces chlorine gas. Oxidation takes place at anode and chlorine gas will be produced at the anode. The reactions taking place during electrolysis of NaCl solution are:
At Cathode: H2O(l)+2e−→H2(g)+2OH−
At Anode: 2Cl−→Cl2(g)+2e−