$ {H_2}{O_2} $ is:
(A)oxidising agent
(B)both oxidizing and reducing agent
(C)reducing agent
(D)none of the above

Hint :Hydrogen peroxide is a colourless liquid. It is used in aqueous solution for safety reasons. It acts as a bleaching agent and it is used as a disinfectant. Concentrated hydrogen peroxide is a very reactive species of oxygen and it is used as a propellant in rocketry. The chemical formula for hydrogen peroxide is: $ {H_2}{O_2} $

Complete Step By Step Answer:
 $ {H_2}{O_2} $ ​can be reduced to $ {H_2}O $ and can also be oxidised to $ {O_2} $ ​. So, it can act as an oxidizing agent by itself getting reduced to $ {H_2}O $ as well as it can act as a reducing agent by getting oxidized to $ {O_2} $ . Therefore, Hydrogen peroxide acts as an oxidizing agent as well as the reducing agent in both acidic and basic mediums.
Some oxidation reactions of hydrogen peroxide are given below:
 $ PbS + 4{H_2}{O_2} \to PbS{O_4} + 4{H_2}O $
 $ 2KI + {H_2}{O_2} \to 2KOH + {I_2} $
 $ NaN{O_2} + {H_2}{O_2} \to NaN{O_3} + {H_2}O $
Some reduction reactions of hydrogen peroxide are given below:
 $ Ba{O_2} + {H_2}{O_2} \to BaO + {H_2}O + {O_2} $
 $ {O_3} + {H_2}{O_2} \to {H_2}O + 2{O_2} $
Therefore, option B is the correct answer.

Note :
Hydrogen peroxide decomposes when it is exposed to sunlight and this process is catalysed by traces of alkali metals. So, $ H_2O_2 $ is generally stored in wax-lined glass or plastic containers and kept in the dark. It should also be kept away from dust particles. Dust will induce explosive decomposition of this compound. In the pure state, hydrogen peroxide is almost a colourless liquid. It is miscible in water in all proportions and it forms hydrates.