There is a sample of $10$ volume of hydrogen peroxide solution. Calculate its strength in percentage (%).

How does $H_{2}O_{2}$ behave as a bleaching agent?

On reaction with a stronger oxidizing agent like $KIO_{4}$,hydrogen peroxide is oxidized with the evolution of $O_{2}$. The oxidation number of $I$ in $KIO_{4}$ changes to $..........$

$4 \ mL$ of '$X$ volume' $H_2O_2$ on heating gives $80 \ mL$ of oxygen at $STP$. The value of $X$ is:

Consider the following statements:
Statement-$I$: $H_2O_2$ acts as an oxidising as well as a reducing agent in both acidic and basic media.
Statement-$II$: $10 \ V \ H_2O_2$ sample means it contains $3.03\% \ (w/v) \ H_2O_2$.

In which of the following reactions does $H_2O_2$ act as a reducing agent?
$(I)$ $H_2O_2 + 2H^{+} + 2e^- \to 2H_2O$
$(II)$ $H_2O_2 \to O_2 + 2H^{+} + 2e^-$
$(III)$ $H_2O_2 + 2e^- \to 2OH^{-}$
$(IV)$ $H_2O_2 + 2OH^{-} \to O_2 + 2H_2O + 2e^-$