Explain in Detail

Q. In the disproportionation reaction 

        $3{\mathrm{HClO}}_3^{-1}\to {\mathrm{HClO}}_4 + {\mathrm{Cl}}_2 +2{\mathrm{O}}_2+{\mathrm{H}}_2\mathrm{O}$ , the equivalent mass of the oxidizing agent is (molar mass of HClO₃ = 84. 45)

       (a) 16.89                                              (b) 32.22

       (c) 84.45                                              (d) 28.15

 

Here HClO3 acts as both oxidizing agent and reducing agent. The change in oxidation number of Cl (when HClO3 is seen as oxidizing agent) in this reaction is 5. And we know that the formula for calculating the equivalent weight of oxidizing agent is given by                                                                                                        E=Molecular weight/Change in oxidation number                                               So, equivalent weight of HClO3=84.45/5      =16.89