Which of the following pairs undergoes easier | vedclass

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(C) The ease of oxidation at the anode depends on the standard oxidation potential and the concentration of the ions.For $(iii)$,$Cl^{-}$ has a lower

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$(iii)$ $Cl^{-}$ and $H_2O$

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(C) The ease of oxidation at the anode depends on the standard oxidation potential and the concentration of the ions.For $(iii)$,$Cl^{-}$ has a lower oxidation potential than $H_2O$,but due to the overpotential of oxygen,$Cl^{-}$ is preferentially oxidized over $H_2O$ in concentrated solutions.For $(iv)$,$SO_4^{2-}$ has a very high oxidation potential,making it much harder to oxidize than $H_2O$. Therefore,$H_2O$ is oxidized more easily than $SO_4^{2-}$.Comparing the pairs,the pair $(iii)$ $Cl^{-}$ and $H_2O$ involves species where oxidation is competitive and significant,whereas $(iv)$ involves a species $(SO_4^{2-})$ that is practically impossible to oxidize in aqueous solution compared to $H_2O$. Thus,the pair $(iii)$ is the correct answer regarding the ease of oxidation.

Which of the following pairs undergoes easier oxidation at the anode?

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