Write the chemical reaction to justify that hydrogen peroxide can function as an oxidizing as well as reducing agent.

Explanation

Hydrogen peroxide can act as both oxidising and reducing agent in both acid and basic medium.
Oxidation properties:
`H_(2)O_(2) + 2H^(+) + 2e^(-) overset("Acid")(rarr) 3H_(2)O , E^(@) = +1.77V`
`H_(2)O_(2) + 2e^(-) overset("Base")(rarr) 2OH^(-) , E^(@) = +087 V`
Eg. `H_(2)O_(2)` oxidises pbs to `PbSO_(4) + 4H_(2)O`
`H_(2)O_(2)` oxidise formaldehyde to formic acid in basic medium.
`2HCHO + H_(2)O_(2) to 2HCOOH + H_(2)`
Reduction properties :
`H_(2)O_(2) overset("Acid")(rarr)2H^(+) + O_(2)+2e^(-)`
`H_(2)O_(2) + 2OH^(-) overset("Base")(rarr) 2H_(2)O + O_(2)`
Eg. `H_(2)O_(2)` reduces acidified potassium permanganete in acid medium.
`2KMnO_(4) + 2H_(2)SO_(4) + 5H_(2)O_(2) rarr K_(2)SO_(4) + 2MnSO_(4) + 8H_(2)O + 5O_(2)`
`H_(2)O_(2)` reduces potassium ferrycyanide in basic medium.
`2K_(3)[Fe(CN)_(6)] + 2KOH + H_(2)O_(2) rarr 2K_(4)[Fe(CN)_(6)]+2H_(2)O + O_(2)`.