In the disproportionation reaction $3 \mathrm{HClO}_{3} \longrightarrow \mathrm{HClO}_{4}+\mathrm{Cl}_{2}+2…
In the disproportionation reaction $3 \mathrm{HClO}_{3} \longrightarrow \mathrm{HClO}_{4}+\mathrm{Cl}_{2}+2 \mathrm{O}_{2}+\mathrm{H}_{2} \mathrm{O}$, the equivalent mass of the oxidizing agent is (molar mass of $\mathrm{HClO}_{3}=84.45$)
$16.89$
$32.22$
$84.45$
$28.15$
Solution
$\mathrm{ClO}_{3}^{-} \longrightarrow \mathrm{Cl}_{2}^{0}$
$x-6=-1 \quad x=0$
$\mathrm{x}=+5 \quad \mathrm{x}=0(\mathrm{x}=$ oxidation number $)$
Equivalent mass $=\frac{\text { Molecular mass }}{\text { Oxidation number }}$
$=\frac{84.45}{5}=16.89$