An acidic solution of hydrogen peroxide behaves as an oxidising as well as reducing agent. Illustrate it with the help of a chemical equation.
(N/A) The following chemical equations indicate the oxidising and reducing nature of $H_{2}O_{2}$.
$(i)$ $H_{2}O_{2}$ acts as an oxidising agent by oxidising acidified $KI$ to $I_{2}$:
$2KI + H_{2}O_{2} + H_{2}SO_{4} \longrightarrow I_{2} + K_{2}SO_{4} + 2H_{2}O$
$(ii)$ $H_{2}O_{2}$ acts as a reducing agent by reducing acidified $KMnO_{4}$ to $Mn^{2+}$ ions:
$2KMnO_{4} + 3H_{2}SO_{4} + 5H_{2}O_{2} \longrightarrow K_{2}SO_{4} + 2MnSO_{4} + 8H_{2}O + 5O_{2}$
$(i)$ $H_{2}O_{2}$ acts as an oxidising agent by oxidising acidified $KI$ to $I_{2}$:
$2KI + H_{2}O_{2} + H_{2}SO_{4} \longrightarrow I_{2} + K_{2}SO_{4} + 2H_{2}O$
$(ii)$ $H_{2}O_{2}$ acts as a reducing agent by reducing acidified $KMnO_{4}$ to $Mn^{2+}$ ions:
$2KMnO_{4} + 3H_{2}SO_{4} + 5H_{2}O_{2} \longrightarrow K_{2}SO_{4} + 2MnSO_{4} + 8H_{2}O + 5O_{2}$
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DifficultJEE MAIN 2014
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