acetylsalicylic acid (aspirin) by creating a reaction between acetic anhydride and salicylic acid. This was be accomplished through the use of recrystallization. Acetic anhydride and salicylic acid are mixed together‚ and then acidified by the addition of a few drops of concentrated sulfuric acid‚ which catalyzed the reaction. The percent yield is calculated to determine the effectiveness of the reaction in preparing the desired product (aspirin). The limiting reactant of the equation was salicylic acid. After
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Lab Report Introduction This lab has the following two concepts: synthesis of acetylsalicylic acid and analysis of acetylsalicylic acid. Synthesis is a purposeful execution of chemical reactions to obtain a product. This concept is used in the first part of the lab; when we have to produce crystals of aspirin. Analysis is the separation‚ identification‚ and quantification of the chemical components of natural and artificial materials. This concept is used throughout the lab when we are analyzing
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generated by the pharmaceutical industry is a prime example of how important organic chemistry is to our healthcare industry. In this lab‚ you will perform an organic synthesis to make aspirin. Aspirin is the trade name for the molecule acetylsalcylic acid. The earliest known use of this molecule has been traced back to fifth century B.C. The Greek physician Hippocrates described an extract of willow tree bark‚ a bitter powder that could be used to reduce fevers. In 1829‚ salicin was isolated from willow
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drug‚ via nucleophilic acid-catalyzed substitution reaction of salicyclic acid with acetic anhydride. The whole reaction is catalyzed by phosphoric acid. (The experiment involved three parts: The synthesis of aspirin‚ the isolation and purification of aspirin‚ and the estimation of the purity of the final product.) [pic] Procedure[1]: A mixture of salicylic acid (0.21g‚ 1.52 mmol) and acetic anhydride (0.52g‚ 5.1mmol‚ 0.48 ml) with one drop of concentrated phosphoric acid in a conical vial was
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absorptivity of salicylic acid To determine the concentration of dissolved aspirin in heated water at various times To determine the effective rate constant of the decomposition of aspirin in heated water at 85°C. Results and Discussion The molar absorptivity of salicylic acid‚ ε‚ can be calculated from the equation‚ A = εcl. A more accurate value can be obtained by finding the gradient of a graph of absorbance of the iron complex‚ A‚ against varying values of c‚ concentration of salicylic acid. The value
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Abstract In this piece of coursework I have been investigating the synthesis of Aspirin and checking for presence and purity of Aspirin. Throughout this coursework we have looked at the history of Aspirin; industrial manufacturing; making salicylic acid; the preparation of Aspirin; recrystallization and purity; melting point; thin layer chromatography (TLC) and titration of Aspirin. I’ve learned a lot about Aspirin‚ how it works and how it is made. We found out that the Aspirin we made and used
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Learning Goals 1. To synthesize aspirin from salicylic acid and acetic anhydride. 2. To purify the crude product by Recrystallization. Introduction Most drugs are chemical compounds which are described as "organic compounds" because they are comprised primarily of the elements carbon‚ hydrogen and oxygen. The present experiment will be the synthesis of a familiar organic compound called aspirin. The common chemical name is acetylsalicylic acid. Aspirin‚ the most widely used drug in
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Introduction Methyl Salicylate has been used for a long time for its pleasant odour and flavour. The objective of this experiment was to carry an organic synthesis; the preparation of salicylic acid from methyl salicylate. To do an organic synthesis‚ it is needed to chemically modify the molecules of another compound to end up with the desire compound. Methyl salicylate is the major constituent of wintergreen oil‚ which is why it was used in this experiment as the starting material. The new technique
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INTRODUCTION Synthesis Acetylsalicylic acid is an acetyl derivative of salicylic acid which appears as a white and crystalline and a weakly acidic substance with a melting point of 135°C and is also known to be aspirin. It is one of the most widely used drugs that can lower fever and is used as a painkiller. According to (Escobel‚ 2011)‚ Aspirin is synthesized through the reaction of salicylic acid with acetyl anhydride that causes a chemical reaction that turns salicylic acid’s hydroxyl group into an acetyl group
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determine percentage purity of aspirin. Abstract: The mass of acetylsalicylic acid was determined using a analytical balance. Sodium hydroxide (NaOH) was added to the acetylsalicylic acid and heated in order to hydrolyze acetylsalicylic acid. Iron chloride was added to each volumetric flask as the purity of the aspirin can be tested by addition of Fe+3 to a suspension of the product. Phenols such as salicylic acid react with iron chloride to form coloured (violet) complexes Aspirin easily absorbs
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