Lab 9 - Chemical Synthesis Lab 9 Author: Holly Polk Lab...

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Chemical Synthesis Lab 9 Author: Holly Polk Lab Partners: Jim Hernandez, Vanessa Jordan, and Dominic Pisciotta Instructor: Yisheng Xu Chemistry Lab 151, Section 001 Date Work Performed: April 14, 2008 Date Report Submitted: April 21, 2008 Abstract: In this experiment, we synthesized aspirin. We synthesized acetylsalicylic acid from salicylic acid and acetic anhydride, isolated the product using filtration, purified the product using rescrystallization, and confirmed the identity and determined the purity by using melting point, TLC and titration. After synthesis, our experiment found the percent yield of crude aspirin product to be 37% and the percent yield after recrystallization to be 1.1%. Based on costs of production and products, it would cost $1.16 to produce one 300mg tablet of our aspirin. This is very expensive compared to the competition: Walgreens charges $.009 to produce one aspirin. Based on our results, we determined the cost for us to produce aspirin was too expensive and not marketable.
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Introduction In this experiment we will formulate the common pain reliever, aspirin. We will synthesize acetylsalicylic acid from salicylic acid and acetic anhydride, isolate the product using filtration, purify the product using rescrystallization, and confirm the identity and determine the purity by using melting point, TLC and titration. Chemical synthesis uses reagents to perform chemical reactions to make a desired chemical, then isolate and characterize it. The first part of the experiment is the synthesis. We will react salicylic acid with acetic anhydride in the presence of an acid catalyst to make aspirin and acetic acid. The conditions under which the reaction should be conducted depend on some of the properties of the reactants and the products. Acetic anhydride is a liquid at room temperature and boils at temperatures well above 100 o C. It reacts with water to form acetic acid. Salicylic acid and aspirin are both solids that melt at temperatures well above 100 o C. They are both slightly soluble in cold water (2.2 mg/mL and 3.3 mg/mL, respectively). Water would not work as a solvent for this experiment, so we use acetic anhydride, and sulfuric acid as a catalyst. Then we will use vacuum filtration to separate the product from the solution. This uses a special apparatus that enables the aspirin crystals to form. Then, we will use recrystallization to purify the aspirin. This utilizes the different solubilities of the desired product and impurities included in the reaction mixture. So, when the solvent cools, only the impurities will remain dissolved and the “pure” product will crystallize out of the solution. The identity of the aspirin will be confirmed by finding its melting point and comparing that to the known literature value. For this we will use a “MelTemp7” melting point determination device to obtain a melting point range. We will also use thin layer chromatography, which separates similar chemicals. Pure
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Lab 9 - Chemical Synthesis Lab 9 Author: Holly Polk Lab...

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