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A2 Chemistry - Assessed Practical Method 1 Mass (g) Total Mass Loss (g) Original Mass 1.44 0.00 Measurement 1 1.05 0.39 Measurement 2 0.90 0.54 Measurement 3 0.88 0.56 Measurement 4 0.86 0.58 Measurement 5 0.86 0.58 Calculations In theory the remaining mass after the heating will be only FeSO4, so from this the mass that was evaporated off would be entirely water. From this we can calculate: The number of moles of H2O is the n= m/Mr H=1 O=16 H2O = 18 =Mr 0.58/18 = 0.032 moles of H2O The remaining mass should be entirely FeSO4 so: Fe=56 S=32 O=16 56 + 32 + (4x16) = 152 = Mr The number of moles of FeSO4 = 0.86/152 = 5.657894737 x 10^-3 Moles To find the ratio of H2O we need to use: 0.032/5.657894737 x 10^-3 = 5.655813953 This is approximately 6 so the Formula of the Hydrated Iron (II) Sulphate Crystals is FeSO4.6 H2O. Method 2 Titration # Start Vol. (cm³) End Vol. (cm³) Difference (cm³) 1 9.0000 30.9500 21.9500 2 11.0000 33.1500 22.1500 3 15.0000 37.2500 22.0500 4 4.0000 26.1000 22.1000 Average (cm³) 22.0625 Equation 5 Fe2+ + MnO4- + 8 H+ = 5Fe3+ + Mn2+ + 4H2O By finding the number of moles of Fe2+ ions being reduced by the...

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