`H_(2)O_(2)` acts as on oxidizing agent as well as reducing agent Why ?

Explanation

In `H_(2)O_(2),` oxygen has - 1 oxidation state which lies between maximum `(0"or"+2"in"OF_(2))` and minimum -2 Therefore, oxygen can be oxidized to `O_(2)` (zero oxidation state) acting as reducing agent or can be reduced to `H_(2)O"or"OH^(-)` (-2 oxidation state) acting as an oxidizing agent.
`underset("Reducing agent")(O_(2)^(-1))toO_(2)^(0)+2e,orunderset("oxidising agent")(O_(2)^(-1))+2e^(-)to2O^(2-)`