# What does the oxidizing agent do in a redox reaction?

Jan 12, 2017

It formally accepts electrons, and thus it is REDUCED in a redox equation.

#### Explanation:

A typical oxidizing agent features a metal in a high oxidation state, for example ${\text{MnO}}_{4}^{-}$, where we have $\text{Mn(VII+)}$. I like this reagent, because it has an intense purple colour, and when you perform a redox titration it is typically reduced to COLOURLESS $M {n}^{2 +}$, and thus such a redox titration is self-indicating:

$\text{MnO"_4^(-) +"8H"^(+) + 5e^(-) rarr "Mn"^(2+) + 4"H"_2"O}$

And when you write such a redox reaction, the two questions you gots to be asking yourself, are (i) is mass balanced, and (ii) is charge balanced? Well, is it?