tough electrolysis question (really!!!) 1. The problem statement, all variables and given/known data When an iron sheet is made the anode during electrolysis of very conc. KOH, an anion containing iron in a high oxidation state is formed in solution. The addition of an excess of Ba(NO3)2 to this solution precipitates a red solid having the following composition by mass: Ba: 53.3% Fe: 21.7% O: 24.9% (1) Calculate the empirical formula of the red solid an dthe oxidation number of the iron in it. (2) After a current has been passed through the solution for some time, the addition of Ba(NO3)2 produces 1.00 g of the red solid. Calculate how many moles of the red solid are formed, and hence calculate how many coulombs of electricity were needed. 2. Relevant equations 3. The attempt at a solution the first part is ok, i got FeO4 as empirical formula. i got the charge on the anion to be -2 since i assumed that it is associated with Ba2+. then the OS of iron becomes +6. for the second part i dunno if i have to take the actual anion to be (FeO4)2- and find the Mr, then the number of moles. because what i have is only the empirical formula. it would be nice if someone could tell me how is that anion actually formed.