Chlorine undergoes disproportionation in alkaline medium as shown below :

$$\mathrm{aCl}_{2(\mathrm{~g})}+\mathrm{b} \mathrm{OH}_{(\mathrm{aq})}^{-} \rightarrow \mathrm{c} \mathrm{ClO}_{(\mathrm{aq)}}^{-}+\mathrm{d} \mathrm{Cl}_{(\mathrm{aq})}^{-}+\mathrm{e} \mathrm{H}_2 \mathrm{O}_{(\mathrm{l})}$$

The values of $$a, b, c$$ and $$d$$ in a balanced redox reaction are respectively :

In alkaline medium, $$\mathrm{MnO}_4^{-}$$ oxidises $$\mathrm{I}^{-}$$ to

Which of the following cannot function as an oxidising agent?

Given below are two statements:

Statement I : In redox titration, the indicators used are sensitive to change in $$\mathrm{pH}$$ of the solution.

Statement II : In acid-base titration, the indicators used are sensitive to change in oxidation potential.

In the light of the above statements, choose the most appropriate answer from the options given below