Theoretical yield of aspirin synthesis. Chemistry 104: Synthesis of Aspirin 2022-10-20
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Aspirin, also known as acetylsalicylic acid, is a widely used non-steroidal anti-inflammatory drug (NSAID) that is used to relieve pain, reduce inflammation, and lower the risk of heart attack and stroke. The synthesis of aspirin involves the conversion of salicylic acid into acetylsalicylic acid through the reaction with acetic anhydride. This reaction is known as acetylation and is typically carried out in the presence of an acid catalyst, such as sulfuric acid.
The theoretical yield of aspirin synthesis is the maximum amount of aspirin that can be produced from a given amount of reactants. It is calculated based on the stoichiometry of the reaction, which is the ratio of reactants and products in a chemical reaction. In the case of aspirin synthesis, the stoichiometry is 1 mol of salicylic acid reacting with 1 mol of acetic anhydride to produce 1 mol of acetylsalicylic acid and 1 mol of acetic acid.
The theoretical yield can be calculated by using the following equation:
Theoretical yield = (Reactant mass / Reactant molar mass) x (Product molar mass / Product molar mass)
For example, if we start with 100 grams of salicylic acid and 50 grams of acetic anhydride, the theoretical yield of aspirin can be calculated as follows:
Theoretical yield = (100 g / 138.12 g/mol) x (180.16 g/mol / 180.16 g/mol) = 72.3 g
This means that the maximum amount of aspirin that can be produced from these reactants is 72.3 grams.
However, it is important to note that the actual yield of aspirin synthesis may be less than the theoretical yield due to various factors such as incomplete reactions, side reactions, and losses during purification. These factors can affect the efficiency of the synthesis and reduce the amount of aspirin produced.
In conclusion, the theoretical yield of aspirin synthesis is the maximum amount of aspirin that can be produced from a given amount of reactants based on the stoichiometry of the reaction. The actual yield may be lower due to various factors that can affect the efficiency of the synthesis.
Synthesis Of Aspirin Lab Report [vnd5ppm7k5lx]
Discard the filtrate left in the filter flask into the waste container under the hood. Shake each test tube and observe the colors produced. Hold and partially submerge the 50 mL flask and contents in the water bath. For example Acetic Anhydride could be harmful is inhaled in large amounts. Change the mode to Events with Entry absorbance vs. It was a huge success and sales grew rapidly. Transfer as much of the solid as possible from the Buchner funnel to a clean, dry 250 mL beaker.
How do you calculate the theoretical yield of aspirin synthesis?
Measure the melting temperature of your aspirin sample. Any names, logos, brands, and other trademarks or images featured or referred to within the UHScienceResource. Answer and Explanation: Ferrocene undergoes acylation more readily than benzene. In boiling water, 1. This will convert the acetic anhydride to vinegar and dilute the sulfuric acid.
Synthesis of Acetyl Salicylic Acid (Aspirin) Essay Example
Therefore the balance did not have a very good precision and would give a percentage error in the reading. For the sample data, the calculations are as follows. Why is ferrocene more reactive than benzene towards Friedel Crafts acylation reactions? Wipe the outside, place it in the device, and close the lid. Carefully insert the capillary tube of solid into one of the sample holders of the Melt Station. Transfer the flask to an ice bath for about five minutes. Discard the cuvette contents as directed by your instructor.
Place the flask in the water bath and heat. There was no way to tell weather these had been measured out correctly. Crystals of aspirin should form. What is used for acylation of ferrocene? The factors that contributed to the inaccuracy of the experiment are the following: Reflux: The apparatus used in the experiment were quite old. The results of the spectrophotmetric test show that the percent purity of the synthesized aspirin is 75%. Phosphoric acid o-phosphoric acid : Skin and eye irritant. Put the beaker on the hot plate.
Both substances can cause painful burns if they come in contact with the skin. Friedrich Bayer, the employer of Hoffman, patented the name and began marketing the product in 1899. Why does the synthesis of ferrocene occur under an inert atmosphere? Be sure to seat the filter paper in the filter with a small amount of water. H 2SO 4 use a dropper, H 2SO 4 is highly corrosive and swirl the flask gently until the salicylic acid dissolves. Iron III nitrate: May intensity fire; oxidizer. Connect the Melt Station sensor cable to LabQuest or to a computer interface.
How do you find the theoretical yield step by step? There were many reasons to this. Moderate fire risk flash point 49°C. Ask instructor to assist with thecleaning ofany spills. Choose Linear as the Fit Equation. EXPERIMENTAL PROCEDURE FOR SYNTHESIS OF ASPIRIN 1.
How can I calculate the percent yield of aspirin synthesis?
Therefore precautions were taken with chemicals such as sulphuric acid that causes severe burns. Add 10 mL of ethanol to the beaker of aspirin sample. Now that you have a rough idea of the melting temperature, a more accurate determination of the melting temperature can be made. Its analgesic, antipyretic, and anti-inflammatory properties make it a powerful and effective drug to relive symptoms of pain, fever, and inflammation. Measure out about 0. Choose Interpolate from the Analyze menu. What is the theoretical yield of aspirin in your synthesis? Place a small amount of yield around 0.
Boil water on the hot plate and dissolve aspirin using a minimum amount of boiling solvent until all of the aspirin is completely dissolved homogeneous solution. Recrystallizing The Aspirin A. The mixture is heated to form the acetylsalicylic acid C 9H 8O 4 and acetic acid C 2H 4O 2. Make sure that the water bath is located directly under the hood at your lab bench. Collect the product by vacuum filtration and rinse out of the flask with a few milliliters of cold petroleum ether. Calculate the precise molar concentration of your stock solution and record it in your data table.
Therefore, the first step is to calculate the number of moles of salicylic acid used. Next you will crystallize the aspirin: a. Store in dedicated flammables cabinet. Prepare the remaining four salicylic acid standard solutions according to the table below, diluting the standard solution in the 100 mL flask with distilled water. Place the aspirin onto a doubled piece of paper towel and set aside to dry while performing the qualitative analysis of the aspirin.
Record the concentration of salicylic acid in your data table. Thoroughly rinse the beaker with several portions of distilled water, and transfer the rinse water to the volumetric flask. Prepare the synthesized aspirin sample for testing. Gloves were used to ensure chemicals did not come in contact with the skin as chemicals could enter the body through broken skin. In this case, one molecule salicylic acid provides both the "alcohol" and the carboxylic acid. As the kinetic energy increase, molecules move faster and collide with other molecules, therefore there are more interactions.