Answer:
\[{{H}_{2}}{{O}_{2}}\] as oxidising agent in alkaline medium.
It oxidises manganese sulphate to manganese dioxide in the presence of an alkali
\[MnS{{O}_{4}}+{{H}_{2}}{{O}_{2}}+2NaOH\xrightarrow{{}}Mn{{O}_{2}}+N{{a}_{2}}S{{O}_{4}}+2{{H}_{2}}O\]
\[M{{n}^{2+}}\,+{{H}_{2}}{{O}_{2}}\,+2O{{H}^{-}}\xrightarrow{\,}\,Mn{{O}_{2}}+2{{H}_{2}}O\] (Ionic equation)
\[{{H}_{2}}{{O}_{2}}\] as reducing agent in alkaline medium.
It reduces potassium ferricyanide to potassium ferrocyanide in the presence of an alkali
\[2{{K}_{3}}[Fe{{(CN)}_{6}}]+2KOH+{{H}_{2}}{{O}_{2}}\xrightarrow{{}}2{{K}_{4}}[Fe{{(CN)}_{6}}]+2{{H}_{2}}O+{{O}_{2}}\]
\[2{{[Fe{{(CN)}_{6}}]}^{3-}}+2O{{H}^{-}}+{{H}_{2}}{{O}_{2}}\xrightarrow{{}}\,2{{[Fe{{(CN)}_{6}}]}^{4-}}\,+2{{H}_{2}}O+{{O}_{2}}\] (Ionic equation)
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