Ncert Exercises & Solutions

The reaction ${Cl}_{2} (g) + 2 {OH}^{-} (aq) \to {ClO}^{-} (aq) + {Cl}^{-} (aq) + H_{2} O (l)$ represents the process of bleaching. Identify and name the species that bleaches the substances due to its oxidising action.

{\overset{0}{Cl}}_{2} (g) + 2 \overset{- 2}{O} \overset{+ 1}{H^{-}} (aq) \to \overset{+ 1}{Cl} \overset{- 2}{O^{-}} (aq) + \overset{- 1}{{Cl}^{-}} (aq) + {\overset{+ 1}{H}}_{2} \overset{- 2}{O} (l)

In this reaction, O.N. of Cl increases from 0 (in Cl₂) to 1 (in ClO^-) as well as decreases from 0 (in Cl₂) to -1 (in Cl^-). So, it acts both reducing as well as oxidisng agent. This is an example of disproportionation reaction. In this reaction, ClO^- species bleaches the substances due to its oxidising action. [In hypochlorite ion (ClO^-) Cl can decrease its oxidation number from +1 to 0 or -1.]

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