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Hydrogen peroxide oxidises [Fe(CN)6]^{4-}\: to \: [Fe(CN)_{6}]^{3-} in acidic medium but reduces  [Fe(CN)_{6}]^{3-} \: to\: [Fe(CN)_{6}]^{4-} in alkaline medium. The other products formed are, respectively?

  • Option 1)

    H_{2}O\: and\: \left ( H_{2}O+OH^{-} \right )
     

  • Option 2)

    \left ( H_{2}O+O_{2} \right )\: and\: H_{2}O

  • Option 3)

    \left ( H_{2}O+O_{2} \right )\: and\:\left ( H_{2}O+OH^{-} \right )

     

  • Option 4)

    H_{2}O\: and\: \left ( H_{2}O+O_{2} \right )

 

Answers (2)

best_answer

As we learned

 

Acidic Nature -

It is a weak acid turn blue litmus red only in pure state.

- wherein

H_{2}O_{2}\rightleftharpoons H^{+}+HO_{2}^{-}

 

 

Reducing Nature -

H2O2 acts as reducing agent.

- wherein

H2O2 get oxidised to O2

 

 

(I)    \left [ Fe(CN)_{6} \right ]^{4-}+H_{2}O_{2}\overset{H^{+}}{\rightarrow}\left [ Fe(CN)_{6} \right ]^{3-}+H_{2}O

(II)    \left [ Fe(CN)_{6} \right ]^{3-}+H_{2}O\overset{OH^{-}}{\rightarrow}\left [ Fe(CN)_{6} \right ]^{4-}+O_{2}+H_{2}O


Option 1)

H_{2}O\: and\: \left ( H_{2}O+OH^{-} \right )
 

Option 2)

\left ( H_{2}O+O_{2} \right )\: and\: H_{2}O

Option 3)

\left ( H_{2}O+O_{2} \right )\: and\:\left ( H_{2}O+OH^{-} \right )

 

Option 4)

H_{2}O\: and\: \left ( H_{2}O+O_{2} \right )

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