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Finding the concentration of sodium carbonate: Mass (Na2CO3 transferred to volumetric flask) = [mass (weighing bottle) + mass (Na2CO3)]-[mass(weighing bottle after emptying)] =15.24g - 12.59g =2.65g Molar mass (Na2CO3) Na=23 C=12 O=16 2Na x 1C x 3O = molar mass = (2 x 23) + 16 + (3 x 16) =106 Number of mols (Na2CO3) = mass/molar mass =2.65g/106 =0.025mol Number of mols (Na2CO3) = concentration x volume 1000 0.025 mol. = conc. x 250cm3 1000 Concentration (Na2CO3) = 0.1 mol.dm-3 Results Titration Initial Burette Reading (cm3) Final Burette Reading (cm3) Difference (cm3) 1 (rough) 0.00 32.00 32.00 2 5.00 36.25 31.25 3 1.10 32.30 31.20 4 0.00 31.25 31.25 5 10.00 44.30 34.30 The first and last results are not included in the average since the first is only a rough titration so that later ones can be more accurate and the last is an anomalous result. Therefore the average is: (31.25+31.20+31.25) / 3 = 31.23cm3 We can now number of moles of calcium carbonate using this equation: Number of moles = concentration x volume 1000 =0.1x25 1000 =0.0025 mol. The following reaction took place: H2SO4(aq) + Na2CO3 (aq) Na2SO4 (aq) +H2O(l) + CO2 (g) There is a 1:1 ratio of...

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