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Determination of the formula of Hydrated Iron(II) Sulphate Crystals Hydrated FeSO4 can come in many hydrated forms. Using two methods for better accuracy and to make a comparison, I will deduce the number of water molecules per mole of a hydrated iron(II) sulphate sample. Method 1: FeSO4.nH2O(s) › FeSO4(s) + nH2O(l) =dehydrating the FeSO4 by evaporating the water and calculating the mass lost. Hazards in this experiment include the flame from the Bunsen and the possibility of the crucible shattering. By using a gentle heat for two minute intervals and the lid slightly ajar (but not so the contents might spit) the crucible shouldn't spit and the water can escape. The reactant (FeSO4) is not dangerous, unless consumed in large doses. Results: Crucible, lid and FeSO4= 21.76g FeSO4= 1.41g Heating Mass after heating(g) Overall loss(g) 1 21.10 0.66 2 21.10 0.66 3 21.10 0.66 4 21.10 0.66 All four results show one and no further mass change meaning the water has been evaporated leaving just the iron(II) sulphate. Analysis: Out of the...

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