1.The primary standard in thiss experiment is ammonium iron(II) sulphate hexahydrate, (NH4)2Fe(SO4)2*6H2O. Calculate the number of millimoles of ammonium iron(II) sulphate hexahydrate in a 1.0000g sample.
2.Give the balanced equation for oxidation of iron(II) ion by permanganate and find how many millimoles of permanganate ion react with one millimole of ammonium iron(II) sulphate.
3.Calculate the number of millimoles of permanganate ion that titrates 1.0000g of ammonium iron(II) sulphate.
The balanced equation for 2 is MnO4^- + 8H^+ + 5Fe^2+ ---> Mn^2+ + 4H20 + 5Fe^3+
The Attempt at a Solution
For #1, would I just use 1.0000g x (1mol/molar mass of ammonium iron(II) sulphate hexahydrate) then change the answer into millimoles. I get 2.5501millimoles
For #2, would I use the moles/millimoles I got for #1 and use the ratio from the equation? But where does the ratio come from if ammonium iron(II) sulphate isnt in the balanced equation?