# How do represent the oxidation of chloride anion to chlorine in acidic solution?

May 21, 2016

Permanganate can oxidize chloride anion to chlorine in acidic solution.

#### Explanation:

$\text{Reduction half-equation: } M n \left(V I I +\right) \rightarrow M n \left(I I +\right)$

$M n {O}_{4}^{-} + 8 {H}^{+} + 5 {e}^{-} \rightarrow {\underbrace{M {n}^{2 +}}}_{\text{almost colourless}} + 4 {H}_{2} O \left(l\right)$ $\left(i\right)$

$\text{Oxidation half-equation: } C l \left(- I\right) \rightarrow C l \left(0\right)$

$C {l}^{-} + \rightarrow \frac{1}{2} C {l}_{2} \left(g\right) + {e}^{-}$ $\left(i i\right)$

So the overall redox reaction is $\left(i\right) + 5 \times \left(i i\right)$

$M n {O}_{4}^{-} + 8 {H}^{+} + 5 C {l}^{-} \rightarrow M {n}^{2 +} + 4 {H}_{2} O \left(l\right) + \frac{5}{2} C {l}_{2} \left(g\right) \uparrow$

Given that permanganate ion solutions are intensely purple in colour, what would you observe in this reaction? Are mass and charge conserved in these reactions? They should be, and if they are not they are wrong!