Number of faradays required to prepare one mole of ethane by the electrolysis of aqueous sodium acetate is

$$\begin{gathered} 2{\mathrm{CH}}_3\mathrm{COONa}+2{\mathrm{H}}_2\mathrm{O}\stackrel{2\mathrm{F}}{\to }\underset{ \mathrm{anode}}{{\mathrm{CH}}_3-{\mathrm{CH}}_3+2{\mathrm{CO}}_2}+2\mathrm{NaOH}+\underset{\mathrm{cathode}}{{\mathrm{H}}_2}; \\ \mathrm{Anode}: \\ 2{\mathrm{CH}}_3-{\mathrm{COO}}^{-}\to 2{\mathrm{CH}}_3-\mathrm{CO}\stackrel{\bullet }{\mathrm{O}}+\mathbf{2}\mathbf{e} \\ 2{\mathrm{CH}}_3-\mathrm{CO}\stackrel{\bullet }{\mathrm{O}}\to 2\stackrel{\bullet }{\mathrm{C}}{\mathrm{H}}_3+2{\mathrm{CO}}_2 \\ \stackrel{\bullet }{\mathrm{C}}{\mathrm{H}}_3+\stackrel{\bullet }{\mathrm{C}}{\mathrm{H}}_3\to {\mathrm{CH}}_3-{\mathrm{CH}}_3 \\ \mathrm{Cathode}: \\ 2{\mathrm{H}}_2\mathrm{O}+\mathbf{2}\mathbf{e}\to {\mathrm{H}}_2+2{\mathrm{OH}}^{-} \end{gathered}$$

The left over solution becomes richer in NaOH.  ${\mathrm{p}}^{\mathrm{H}}$ progressively increases.