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  4. The following reactions show the H2O2 behaviour in A and B reactions as (1) PbS(. s .)+4H2O2 (a q) arrow PbSO4 (s)+4H2O(l) (2) HOCl+H2O2 arrow H3O++Cl-+O2

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Q. The following reactions show the $H_{2}O_{2}$ behaviour in A and B reactions as
(1) $PbS_{\left(\right. s \left.\right)}+4H_{2}O_{2 \left(a q\right)} \rightarrow PbSO_{4 \left(s\right)}+4H_{2}O_{\left(l\right)}$
(2) $HOCl+H_{2}O_{2} \rightarrow H_{3}O^{+}+Cl^{-}+O_{2}$

NTA AbhyasNTA Abhyas 2022

Solution:

Hydrogen peroxide oxidise lead sulphide to lead sulphate and itself gets reduced. Thus, $H_{2}O_{2}$ acts as an oxidising agent in acidic medium.
Hydrogen peroxide reduces hypochlorous acid to chloride ion in acidic medium and itself gets oxidised.
Thus, $H_{2}O_{2}$ acts as a reducing agent in acidic medium.