Statement 1: During electrolysis of aqueous solution of $N a C l, O H^{-}$ ions are oxidised in preference to $C l^{-}$ ions.
Statement 2: Standard potential of $O H^{-}$ ions is more than that of $C l^{-}$ ions.

Statement 1 is True, statement 2 is True, statement 2 is a correct explanation of statement 1.

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Statement 1 is True, statement 2 is True, statement 2 is not a correct explanation of statement 1.

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Statement 1 is true, Statement 2 is False.

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Statement 1 is False, Statement 2 is True.

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Solution

The correct option is D Statement 1 is False, Statement 2 is True.
The standard potential of ${O H}^{-}$ ions is more than that of ${C l}^{-}$ ions. Hence, during electrolysis of aqueous solution of $N a C l$ , ${O H}^{-}$ ions should be oxidized in preference to ${C l}^{-}$ ions. However experimental observations have shown that chlorine gas is produced at anode. Hence, ${C l}^{-}$ ions are oxidised in preference to ${O H}^{-}$ ions. This is due to the phenomenon of over voltage.

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Statement 1: During electrolysis of aqueous solution of NaCl, OH− ions are oxidised in preference to Cl− ions.Statement 2: Standard potential of OH− ions is more than that of Cl− ions.

Statement 1: During electrolysis of aqueous solution of $N a C l, O H^{-}$ ions are oxidised in preference to $C l^{-}$ ions.
Statement 2: Standard potential of $O H^{-}$ ions is more than that of $C l^{-}$ ions.