[zerobladex]

0.200 of a certain uknown semimetal [X] is heated in the air, creating the correpsonding oxide, M2O3 which was then dissolved in aqueous acid. This solution was then titrated with 10.7 mL KMnO4 to reach equivalence point. The unbalanced equation is:

H3XO3 (aq) + MnO4^- (aq) ==> H3XO4 (aq) + Mn^2+ (aq)

How many moles of oxide were formed and how many moles of semimetal X were in the initial 0.200G sample?

My textbook shows me how to do this but it skips a few steps so I'm kind of confused about how thye got the asnwer. If someone could solve and explain their steps, that'd be great.

[Borek]

Start doing what you know how, we will start from the moment you hit the wall.

Balancing reaction equation would be a good beginning.