Question

How do we represent the oxidation of `"iodide ion"` by `"hypochlorite ion"`, `ClO^(-)` to give iodine and chloride ion?

Answer 1

Another redox equation...

Explanation:

`"Iodide ion"` is oxidized to `"diiodine..."`

`I^(-)rarr 1/2I_2+e^(-)` `(i)`

`"Hypochlorite"` is reduced to `"chloride...."`

`stackrel(+I)ClO^(-) +2H^+ + 2e^(-) rarr Cl^(-)+H_2O(l)` `(ii)`

And so we take....`2xx(i)+(ii)`

`ClO^(-) +2H^+ + 2e^(-)+2I^(-)rarr I_2+2e^(-)+Cl^(-)+H_2O(l)`

...to give finally....

`ClO^(-) +2I^(-)+2H^+rarr I_2+Cl^(-)+H_2O(l)`

...the which balances mass and charge as is absolutely required...