A level chemistry past paper question help

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Taha525
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This question is about the preparation of ammonium iron(III) sulfate-12-water,
NH4Fe(SO4)2.12H2O. It is a double salt containing ammonium ions, iron(III) ions,
sulfate ions, and water of crystallisation.
(a) The first step of a preparation is to make iron(III) sulfate solution.
0.050 mol of iron(II) sulfate-7-water is dissolved in dilute sulfuric acid.
This solution is heated to boiling and concentrated nitric acid is added in
portions of about 1cm3, until the reaction is complete.

6FeSO4(aq) + 2HNO3(aq) + 3H2SO4(aq) → 3Fe2(SO4)3(aq) + 2NO(g) + 4H2O(l)

(i) Write the ionic equation for this reaction. State symbols are not required.

(ii) Calculate the mass of 1 mol of iron(II) sulfate-7-water, FeSO4.7H2O.
[Ar Fe = 55.8, S = 32.1, O = 16, H = 1]

(iii) Calculate the mass of 0.050 mol of iron(II) sulfate-7-water.

(iv) Show that 12.5cm3
of 2.0 mol dm−3 sulfuric acid is the minimum amount of
sulfuric acid needed to react with 0.050 mol of iron(II) sulfate-7-water.
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Pigster
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l33t copy and paste skillz.

Do you want us to just do you homework for you? The Q gives you the answer in part iv!

What have you tried to do with all the information given?
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Taha525
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I figured out the rest but the ionic one is confusing, tried expanding the ones that are aqueous but doesn't seem to work
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