Answer:
When an aqueous solution of sodium chloride is electrolysed, the following changes occur:
\[NaCl\,\xrightarrow{\,}\,N{{a}^{+}}\,\,\,+C{{l}^{-}}\]
\[{{H}_{2}}O\,\,\rightleftharpoons \underset{\text{(Cathode)}}{\mathop{{{H}^{+}}}}\,+\underset{\text{(Anode)}}{\mathop{O{{H}^{-}}}}\,\]
At cathode, \[{{H}^{+}}\]ion is discharged in preference to \[N{{a}^{+}}\] ions because the electron accepting tendency or E° value of \[{{H}^{+}}\] ion is more than that of \[N{{a}^{+}}\].
\[{{H}^{+}}+{{e}^{-}}\xrightarrow{\,}\,H;\,\,\,H+H\xrightarrow{\,}\,\,{{H}_{2}}\]
Thus, sodium metal is not formed at the cathode.
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