The pH of an H_2O_2 solution is 6. If some ch | vedclass

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(C) The reaction between hydrogen peroxide $(H_2O_2)$ and chlorine $(Cl_2)$ is given by: $H_2O_2 + Cl_2 \rightarrow 2HCl + O_2$. In this reaction,$HCl

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The $pH$ of the resulting solution will be less than $6$ and oxygen gas will be liberated.

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(C) The reaction between hydrogen peroxide $(H_2O_2)$ and chlorine $(Cl_2)$ is given by: $H_2O_2 + Cl_2 \rightarrow 2HCl + O_2$. In this reaction,$HCl$ is produced,which is a strong acid. The production of $HCl$ increases the concentration of $H^+$ ions in the solution,thereby decreasing the $pH$ (making it less than $6$). Additionally,oxygen gas $(O_2)$ is evolved as a byproduct.

The $pH$ of an $H_2O_2$ solution is $6$. If some chlorine gas is passed through it,which of the following statements is correct?

Similar Questions

$H_2O_2$ will oxidise:

The oxidation state of oxygen in hydrogen peroxide $(H_2O_2)$ is:

How does $H_2O_2$ behave as a bleaching agent?

$I. \, H_2O_2 + O_3 \rightarrow H_2O + 2O_2$
$II. \, H_2O_2 + Ag_2O \rightarrow 2Ag + H_2O + O_2$
The role of hydrogen peroxide in the above reactions is respectively:

$Hydrogen$ $peroxide$ is reduced by:

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