Why dont you....

[zibb3r]

need an indicator when a redox titration is performed using potassium permanganate solution in the burette???

Thanks

[pi]

Because it is not an acid-base reaction (its redox). The end point is instead made visible by a natural colour change that happens in the reaction.

Hope that helps

[burbs]

MNO4- changes colour as it is reduced to Mn2+, an indicator is not necessary.

[zibb3r]

Thanks for you answers guys, but I don't really understand why this occurs?

Thanks

[nacho]

I said this before, but i thought i was wrong.
redox reactions will generally contain transition metals as they are strong reductants.
transition metals (such as Mn) change colour when they give up/or take on an electron, it's just a natural property (FROM WHAT I THINK, there is generally a transition metal in a redox reaction, and so it will give off a natural colour change)
where as acid/base do not show a natural colour change and so an indicator is required
as to why this is, i am not sure,

edit: although i would assume it would have something to do with:
- subshell config, excited state/ground state, wavelength (as confirmed by huaxiadragon)
But don't take this into consideration without research, this is just some crazy logic i made up just then

[zibb3r]

makes sense, thanks

[huaxiadragon]

MNO4- changes colour as it is reduced to Mn2+, an indicator is not necessary.

Just to add a bit more

(MnO4−) is an intense purple colour. It reacts to produce the near-colourless
manganese(II) ion (Mn2+).

Since permanagate appear very frequently in the exam. It's good to memorise the colour change