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Could someone explain this equation?
The commonest form of iron(II) sulfate is the heptahydrate, FeSO4.7H2O. On heating at 90 C this loses some of its water of crystallisation to form a different hydrated form of iron(II) sulfate, FeSO4.xH2O. 3.40g of FeSO4.xH2O was dissolved in water to form 250 cm3 of solution. A 25.0cm3 sample of this solution was acidifi ed and titrated with 0.0200 mol dm–3 potassium manganate(VII). In this titration 20.0cm3 of this potassium manganate(VII) solution was required to react fully with the Fe2+ ions present in the sample.
Complete and balance the ionic equation for the reaction between the manganate(VII) ions and the iron(II) ions.
MnO4 – (aq) + 5Fe2+(aq) + ........H+(aq) ..... +....(aq) + 5Fe3+(aq) + .......H2O(l)
? what is the part you are having difficulty with? The balance equation or finding out x?
Also this question!
Another element, Z, in the same period of the Periodic Table as A, reacts with chlorine to form a compound with empirical formula ZCl 2. The percentage composition by mass of ZCl 2 is Z, 31.13; Cl, 68.87.
Calculate the relative atomic mass, Ar , of Z. Give your answer to three significant figures.
I've attached the mark scheme for reference! http://maxpapers.com/wp-content/uploads/2012/11/9701_s14_ms_21.pdf