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Finding our how much acid there is in a solution. Results table Titration Rough 1 2 3 Initial burette reading 0.00 cm3 11.00 cm3 0.00 cm3 11.10 cm3 Final burette reading 11.00 cm3 21.90 cm3 11.10 cm3 22.10 cm3 Titre 11.00 cm3 10.90 cm3 11.10 cm3 11.00 cm3 Average titre = 11.0 cm3 Equation of reaction: Na2CO3 (aq) + H2SO4 (aq) H2O (l) + CO2 (g) + Na2SO4 (aq) So, one mole of sulphuric acid reacts with one mole of sodium carbonate to form water, carbon dioxide and sodium sulphide. In the sodium carbonate solution there was 1.06g of sodium carbonate made up to volume of 100cm3 with distilled water. Na2CO3 Na = 23* 2 = 46g C = 12 * 1 = 12g O = 16* 3 = 48g +106g 1 mole of Na2CO3 = 106g We used 1.06 g in our solution, 1.06/106 = 0.01 moles so, 0.01 moles of Na2CO3 in 100cm3 In each experiment we use 10cm3, so this contains 0.001 moles of Na2CO3 Since we know that the volumes of the two solutions need to...

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