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# Graphically the concentration of the unknown would be

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4. Graphically the concentration of the unknown would be about 0.0002M. Mathematically the concentration would be about 5.6 x 10 -5 M. 5. A = bce A/bc = e e = (0.122) / (1.30cm) (5.6 x 10 -5 M) = 1675.8L/mol.cm 6. (5.6 x 10 -5 M ) (180.16g/mol) = 0.0101 g/L (0.0101 g/L) (.25L) = .2.5 x 10 -4 g Conclusion: In part one, we found that all the ASA dissolved addition of extra water was not necessary to complete the solution It also took very little time for the solution to cool to room temperature after heating. In part three, we found that the solution turned a purple color when adding Stock Solution B to the FeCl 3 solution. The less of the solution we added, the lighter purple the solution was, allowing more light to pass through the solution. The unknown and the known solutions that were most similar in mass percent were the same shade of purple. There were several error sources in this lab. The Spec 20 was difficult to use at first because of out inexperience with the device and therefore are not very confident on our readings of the device and the %T numbers that were calculated. In this lab, we found that the aspirin tablet had an absorbance that was about 5.6 x 10 -5 M.
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• Fall '12
• professoridon'tknow
• Chemistry, 175, Purple

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