Experiment 8: Acetylsalicylic Acid Experiment

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Monica Perez Experiment 8: Acetylsalicylic Acid Experiment 01/25/2013 CHM Lab- 2211 Sec 0016 Instructor: Jennifer Reed Introduction: Commonly used as Aspirin, acetylsalicylic acid is an analgesic (pain reliever), which is one of the products of the esterification reaction between salicylic acid and acetic anhydride. This esterification occurs since the hydroxyl group from the salicylic acid reacts with acetic anhydride to form an ester. In this experiment, we will be able to recreate this acid catalyzed reaction, using sulfuric acid as our catalyst in order to produce acetylsalicylic acid and acetic acid. The final product of this reaction will be some crystals, which will be mainly composed of acetylsalicylic acid. In order…show more content…
Test the filtration device with water, before placing the crystals in the solution. Filter the crystalinization product for 5-10 min and finally rinse the crystals with some distilled water. Re-crystallization of Crude Acetylsalicylic Acid Dissolve crude product of previous crystalinization in a clean 125 mL Erlenmeyer flask with ethyl acetate (2-3 mL). Gently heat the solution on a hot plate to dissolve the reagents and then allow the solution to cool down at room temperature. At this point crystals should form, if not add petroleum ether to the solution. Place the flask with the solution on an ice bath until crystallization is complete. Once again, set up the vacuum filtration that was used to collect crude crystal product and vacuum dry the crystals for 10 minutes. Perform the ferric chloride test by setting up four test tubes with salicylic acid, products of crystalinization, products of re-crystalinization and distilled water respectively in order to detect the presence of phenol. Finally, after placing the products of re-crystalinization in the oven for 5-10 min record its mass and its melting point. Conclusion: Our results lead us to think that the possible reason for this low percentage, as well as for the differences between melting point range obtained and the actual melting point (128- 130 ° C 0 ° C instead of 135- 136 ° C) might have been due errors in the time that the re-crystallized sample spent in the oven. This theory is reinforced by
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