d and f Block Elements
5.0 Potassium permanganate
5.1 Properties of potassium permanganate
5.2 Structure of manganate ion and permanganate ion
5.3 Disproportion of an oxidation state
5.4 Uses
5.0 Potassium permanganate
5.2 Structure of manganate ion and permanganate ion
5.3 Disproportion of an oxidation state
5.4 Uses
Preparation of potassium permanganate:
- Pyrolusite ($Mn{O_2}$) when fused with $KOH$ in presence of oxygen or $KN{O_3}$ or $KCl{O_4}$ produces potassium manganates. \[2Mn{O_2} + 4KOH + {O_2}\xrightarrow{\Delta }2{K_2}Mn{O_4} + 2{H_2}O\]
- The green mass is extracted with water oxidized in potassium permanganate as follows:
a) By Electrolytic Oxidation:
- The potassium manganate solution is electrolyzed by iron electrodes. $${K_2}Mn{O_4} \to 2K + Mn{O_4}^{ - 2}{\text{ }}{{\text{H}}_2}O \to {H^ + } + O{H^ - }$$
- During this process manganate ions are oxidized to permanganate ions at anode.
- Hydrogen gas is evolved at cathode.
- ${K^ + }$ and $Mn{O_4}^ - $ ions react with each other and form $KMn{O_4}$. $${K^ + } + Mn{O_4}^ - \to KMn{O_4}$$
b) By Oxidation:
${K_2}Mn{O_4}$ is oxidized in $KMn{O_4}$ by using ${H_2}S{O_4}$, $C{O_2}$, $C{l_2}$ or ${O_3}$. $$2{K_2}Mn{O_4} + 2{H_2}S{O_4} \to 2{K_2}S{O_4} + 2KMn{O_4} + 2{H_2}O + Mn{O_2}$$$$3{K_2}Mn{O_4} + 4C{O_2} + 2{H_2}O \to 2KMn{O_4} + 4KHC{O_3} + Mn{O_2}$$$$2{K_2}Mn{O_4} + C{l_2} \to 2KMn{O_4} + 2KCl$$$$2{K_2}Mn{O_4} + {O_3} + {H_2}O \to 2KMn{O_4} + 2KOH + {O_2}$$