Answer:
\[{{H}_{2}}{{O}_{2}}\] acts as an
oxidising as well as a reducing agent both in acidic and basic mediums. This is
justified by following reactions:
Oxidising agent
Acidic
medium: (a) Acidified ferrous sulphate is oxidised to ferric sulphate.
\[2FeS{{O}_{4}}+{{H}_{2}}S{{O}_{4}}+{{H}_{2}}{{O}_{2}}\to
F{{e}_{2}}{{(S{{O}_{4}})}_{3}}+2{{H}_{2}}O\] (b) In acidic solution, mercury is
oxidised.
\[Hg+{{H}_{2}}{{O}_{2}}\xrightarrow{{{H}_{2}}S{{O}_{4}}}HgO+{{H}_{2}}O\]
(c) A
solution of acidified \[{{K}_{2}}C{{r}_{2}}{{O}_{7}}\]is oxidised to blue
peroxide of chromium\[(Cr{{O}_{5}})\].
\[{{K}_{2}}C{{r}_{2}}{{O}_{7}}+{{H}_{2}}S{{O}_{4}}+4{{H}_{2}}{{O}_{2}}\to
2Cr{{O}_{5}}+{{K}_{2}}S{{O}_{4}}+5{{H}_{2}}O\]Alkaline medium :
(a) Chromium
hydroxide is oxidised by \[{{H}_{2}}{{O}_{2}}\]in presence of \[\text{NaOH}\]
into \[\text{N}{{\text{a}}_{2}}Cr{{O}_{4}}.\]
\[2Cr{{(OH)}_{3}}+4NaOH+3{{H}_{2}}{{O}_{2}}\to
2N{{a}_{2}}Cr{{O}_{4}}+8{{H}_{2}}O\](b) \[MnS{{O}_{4}}\] is oxidised to Mn02.
\[MnS{{O}_{4}}+2NaOH+{{H}_{2}}{{O}_{2}}\to
Mn{{O}_{2}}+N{{a}_{2}}S{{O}_{4}}+2{{H}_{2}}O\]
(c) HCHO is
oxidised to HCOOH
\[HCHO+{{H}_{2}}{{O}_{2}}\to
HCOOH+{{H}_{2}}O\]
Reducing
agent
Acidic
medium: (a) \[Mn{{O}_{2}}\] in acidic medium is
reduced to \[MnS{{O}_{4}}\].
\[Mn{{O}_{2}}+{{H}_{2}}S{{O}_{4}}+{{H}_{2}}{{O}_{2}}\to
MnS{{O}_{4}}+2{{H}_{2}}O+{{O}_{2}}\](b) Red lead in presence of HN03 is reduced
to
plumbous
salt.
\[P{{b}_{3}}{{O}_{4}}+6HNN{{O}_{3}}+{{H}_{2}}{{O}_{2}}\to
3Pb{{(N{{O}_{3}})}_{2}}+4{{H}_{2}}O+{{O}_{2}}\](c) It reduces acidified\[KMn{{O}_{4}}\].
\[2KMn{{O}_{4}}+3{{H}_{2}}S{{O}_{4}}+5{{H}_{2}}{{O}_{2}}\to
{{K}_{2}}S{{O}_{4}}\]
\[+2MnS{{O}_{4}}+8{{H}_{2}}O+5{{O}_{2}}\]
Alkaline
medium:
(a)Potassium
ferricyanide is reduced to ferrocyanide in presence of\[KOH+{{H}_{2}}{{O}_{2}}\].
\[2{{K}_{3}}Fe{{(CN)}_{6}}+2KOH+{{H}_{2}}{{O}_{2}}\to
2{{K}_{4}}Fe{{(CN)}_{6}}+2{{H}_{2}}O+{{O}_{2}}\](b) Iodine is reduced.
\[{{I}_{2}}+2KOH+{{H}_{2}}{{O}_{2}}\to
2KI+2{{H}_{2}}O+{{O}_{2}}\]
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