(B) The reaction is: $\underline{Cl}_2 + H_2O \longrightarrow HOCl + HCl$.In this reaction,$Cl_2$ undergoes disproportionation.The products are $HOCl$

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If the product is an oxyacid with an $-ous$ suffix.

(B) The reaction is: $\underline{Cl}_2 + H_2O \longrightarrow HOCl + HCl$.In this reaction,$Cl_2$ undergoes disproportionation.The products are $HOCl$ (hypochlorous acid) and $HCl$ (hydrochloric acid).$HOCl$ is an oxyacid of chlorine where the oxidation state of $Cl$ is $+1$,which corresponds to the $-ous$ suffix (hypochlorous acid).$HCl$ is a binary acid (hydrohalic acid),not an oxyacid.Therefore,the product $HOCl$ is an oxyacid with an $-ous$ suffix.

Class 11 Chemistry Redox Reactions Auto oxidation and Disproportionation

Difficult

In the following reaction,identify the nature of the product formed by the complete hydrolysis of the underlined atom at $R.T.$:
$\underline{Cl}_2 + H_2O \longrightarrow HOCl + HCl$

A
If the product is an oxyacid with an $-ic$ suffix.
B
If the product is an oxyacid with an $-ous$ suffix.
C
If the products are two oxyacids,one with an $-ic$ suffix and the other with an $-ous$ suffix.
D
If the product is not an oxyacid,neither with an $-ic$ suffix nor with an $-ous$ suffix.