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# The aim of our experiment was to find the mass of acetyl salicylic acid in an aspirin tablet and compare it with the manufactures claim.

Extracts from this document...

Introduction

Chemistry Write up # 3: Analysis of Aspirin Tablets Table showing masses and measurements of chemicals in the experiment Description Value Unit Uncertainty Percentage Uncertainty Mass of aspirin tablets x4 1.713 g ?????? 0.058% Literature value/ manufacture's claim of salicylic acid in an aspirin tablet 300 mg Amount of NaOH added 25.0 ml ??0.1?mL 0.4% Concentration of NaOH 0.998 mol dm-3 Concentration of sulphuric acid 0.0495 mol dm-3 Mols of NaOH 0.0250 mol Volume of sulphuric acid 7.28 cm3 ??0.1?mL 1.37% Table showing the volume of (0.0495 mol) sulphuric acid needed to neutralise the NaOH solution ml) Volumes Trials (ml) (ml) � 0.1 Trial 1 Trial 2 Trial 3 Trial 4 Trial 5 Average Initial Volume (ml) � 0.05 0.2 9.7 17.2 25.4 32.6 Final Volume (ml) � 0.05 7.5 17.1 24.4 32.6 39.9 Change In Volume (ml) � 0.1 7.3 7.4 7.2 7.2 7.3 7.28 � 0.1 Observations: * When adding the sulphuric acid to the NaOH, indicator and salicylic acid during titration the colour changed from blue to yellow. * There was a strong smell when the aspirin and water was boiling. ...read more.

Middle

= 0.0159875 = 0.0160 (3sf) 0.40% + 1.37% + 0. 12% + 0.5% = 2.39% 2.39% 2.39% Because of 2 : 1 ratio N(CH3COOC6H4COOH) = N = 0.00799375 N = 0.00799 (3sf) 2.39% 2.39% 2.39% Mr of (CH3COOC6H4COOH) = 180.17 m = Mr x N m = 180.17 x 0.00799375 m = 1.440233928 m = 1.44 g (3sf) m = mg 1440 / 4 tablets = 360 per tablet 1 tablet of aspirin contains 360 mg of CH3COOC6H4COOH Literature value or manufactures claim is 300mg of CH3COOC6H4COOH 0.00% + 2.39% = 2.39% 2.39% 2.39% 2.39% 2.39% � 9 % deviation = Experimental value - Literature value X 100 Literature value 1 % deviation = 360mg - 300mg X 100 300mg 1 % deviation = 20% Conclusion: The aim of our experiment was to "find the mass of acetyl salicylic acid in an aspirin tablet and compare it with the manufactures claim." The mass of acetyl salicylic acid the manufacture claims is in an aspirin tablet is 300mg. From our experiment we calculated that the mass of acetyl salicylic acid was 360mg. ...read more.

Conclusion

The titration trials were very consistent with only 0.2 mls separating the lowest and highest values. This shows that the titration was consistent but not necessarily accurate because we used a slightly faulty burette that maintained an air bubble at the bottom. This would have accounted for some of the systematic error. Improvements: An improvement that we could have made was we could have tested the mass of CH3COOC6H4COOH in more than just 4 tablets. To get a more accurate result it would have been better if we had done the experiment another ten times and with different packets of the same brand of aspirin tablets to see if the mass of CH3COOC6H4COOH is consistent in different packets. An improvement we did make was we used a magnetic stirrer during titration so that the reactions were sped up so it was easier to see if the chemicals had completely reacted. Another improvement that we could have implemented was using a water bath to keep the temperature the same over the whole experiment. The experiment was carried out over 2 days and in those three days the weather was different which could have affected our results. ?? ?? ?? ?? Thomas Bishop IB13VF ...read more.

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