The $pH$ of a solution of $H_2O_2$ is $6.0$. Some chlorine gas is bubbled into this solution. Which of the following is correct?
- AThe $pH$ of the resultant solution becomes $8.0$
- BHydrogen gas is liberated from the resultant solution
- CThe $pH$ of the resultant solution becomes less than $6.0$ and oxygen gas is liberated
- D$Cl_2O$ is formed in the resultant solution
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Similar Questions
$H_2O_2$ reacts as a reducing agent with:
$(I)$ $KMnO_4$
$(II)$ $K_2Cr_2O_7$
$(III)$ $Ag_2O$
$(IV)$ $HNO_3$
$(I)$ $KMnO_4$
$(II)$ $K_2Cr_2O_7$
$(III)$ $Ag_2O$
$(IV)$ $HNO_3$
Medium
View SolutionThe correct increasing order of acidity is
In which of the following reactions does $H_2O_2$ act as a reducing agent?
$(I)$ $H_2O_2 + 2H^{+} + 2e^- \to 2H_2O$
$(II)$ $H_2O_2 \to O_2 + 2H^{+} + 2e^-$
$(III)$ $H_2O_2 + 2e^- \to 2OH^{-}$
$(IV)$ $H_2O_2 + 2OH^{-} \to O_2 + 2H_2O + 2e^-$
$(I)$ $H_2O_2 + 2H^{+} + 2e^- \to 2H_2O$
$(II)$ $H_2O_2 \to O_2 + 2H^{+} + 2e^-$
$(III)$ $H_2O_2 + 2e^- \to 2OH^{-}$
$(IV)$ $H_2O_2 + 2OH^{-} \to O_2 + 2H_2O + 2e^-$
Difficult
View SolutionThe oxide that gives hydrogen peroxide $H_2O_2$ on treatment with a dilute acid $H_2SO_4$ is:
Easy
View SolutionIn which of the following reactions does hydrogen peroxide act as a reducing agent?
Medium
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