Synthesis of aspirin lab answers. Experiment_614_Synthesis of Aspirin_1_1_2 2022-12-25
Synthesis of aspirin lab answers Rating:
8,6/10
629
reviews
Aspirin, also known as acetylsalicylic acid, is a widely used pain reliever and anti-inflammatory medication. In this lab, students will learn about the synthesis of aspirin through the chemical reaction between salicylic acid and acetic anhydride.
The synthesis of aspirin begins by mixing salicylic acid and acetic anhydride in a flask. The flask is then heated to reflux, which means it is heated to the boiling point of the solvent and the vapor is condensed and returned to the flask. The heating and refluxing helps to speed up the reaction between the two reactants.
During the reaction, a molecule of acetic anhydride reacts with the hydroxyl group of the salicylic acid to form an ester, which is known as acetylsalicylic acid or aspirin. The reaction also produces a molecule of acetic acid as a byproduct.
To purify the synthesized aspirin, the reaction mixture is cooled and then filtered to remove any solid impurities. The filtered solution is then washed with water and dried to obtain the pure aspirin.
The synthesis of aspirin can be further confirmed through the use of thin layer chromatography (TLC), which is a technique used to separate and identify compounds in a mixture. By running the synthesized aspirin through TLC and comparing the resulting spot to a known standard of aspirin, students can confirm the purity of their synthesized sample.
Overall, the synthesis of aspirin is a useful lab for students to learn about chemical reactions and the purification of products. It also allows them to understand the practical applications of chemistry in the production of common medications.
Experiment_614_Synthesis of Aspirin_1_1_2
Aspirin is an effective analgesic pain reliever , antipyretic fever reducer and anti-inflammatory agent and is one of the most widely used non-prescription drugs. Transfer the contents of the flask to a Büchner funnel assembly. This new wonder pain killer was found in Meadowsweet Spiraea ulmaria , a wild flowering plant that grows on riverbanks over much of Europe. Then put this beaker in an ice-water bath. However, this reaction is slow and has a relatively low yield. Transfer 5 mL of the aspirin solution from the 250 mL volumetric flask to a clean and dry 100 mL volumetric flask.
Concentration as the Collection Mode. Heat for 30 minutes at a temperature of 70o C, slowly stirring the mixture gently. Thereafter, the solution was swirled causing the solution to turn cloudy-white. Discard the capillary tube and sample as directed by your instructor. It is then absorbed into the bloodstream. While doing Chemical Ideas 13.
Reacts sometimes delayed violently with water. Although salicylic acid was effective at reducing pain and fever, it also had some unpleasant side effects. Record the mass of aspirin that you use to the nearest 0. You are now ready to begin the synthesis of aspirin. Attach the vacuum pump to the flask. Moderately toxic by ingestion and inhalation. How does the melting temperature test of your aspirin compare to the accepted value? Once acetylsalicylic acid is absorbed from the intestine, it is converted back to salicylic acid Salicylic acid enters the bloodstream where it interferes with the synthesis of prostaglandins, he reversibly binds to and inhibits an enzyme called cyclooxygenase and modifies the activity of cyclo-oxygenase 2 Prostaglandins and cyclooxygenase are involved in generating a pain signal and inflaming painful areas.
Add 150 mL of distilled water to the beaker. Steps 22—25 will guide you through the set up and testing of your aspirin sample. Connect the Melt Station sensor cable to LabQuest or to a computer interface. You can use this information to calculate the purity of your aspirin sample. In 1899, the Bayer Company in Germany patented a drug they called aspirin, which was a modification of salicylic acid. After students complete the Part 1 synthesis, they will need to dry the sample. The melting point… Chemistry F334 : What's in the Medicine 1.
Wash the crystals with cold, distilled water twice more in this manner. The general trend is, nevertheless, solubility increase as the temperature rises. Just from personal experience, I know that this is what aspirin looks like. When aspirin is ingested, it is broken down to salicylic acid by the basic conditions in the small intestine. Avoid contact with your eyes, skin, and clothing. Chill for at least 10 minutes in order to obtain the maximum amount of crystalline product.
The Bayer Company replaced the phenol group with an ester group. Section 2: Safety Precautions and Waste Disposal Safety Precautions: Use of eye protection is recommended for all experimental procedures. Organic Chemistry with Vernier 3 c. Quantitatively transfer the solution from the beaker to a 250 mL volumetric flask. Lab 6: Synthesis of Aspirin Conclusion In Part 1, the purpose of the lab is to prepare acetylsalicylic acid, commonly called aspirin, and determine the experiment yield of a synthesis of Aspirin.
Wipe the outside, place it in the device, and close the lid. Calculate the precise molar concentration of your stock solution and record it in your data table. Through a series of chemical reactions with cheap raw materials beginning with beginning with methyl salicylate and, it is a cheaper and more efficient method of making salicylic acid from natural resource of benzene. At the end of your testing, turn the control knob on the Melt Station to Off. Discard the capillary tube and sample as directed by your instructor. What is the theoretical yield of aspirin in your synthesis? The active ingredient in willow bark was later found to be salicylic acid.
Lab #3 and 4: Aspirin Synthesis and Analysis Flashcards
After fully dissolving the salicylic acid with acetic anhydride, the solution is cooled and cold water is then added. Measure and record the absorbance value of the treated aspirin sample. In this experiment, sulfuric acid will be used as the catalyst. Tap the Meter tab, then tap Mode. Overall, the reaction takes place between a carboxylic acid and an acid anhydride to form an ester. When the solid begins to melt, click Mark to mark the temperature on your graph. The regression line should closely fit the five data points and pass through or near the origin of the graph.
Be sure to weigh and record the mass of the filter paper to the nearest 0. Conduct this reaction in a fume hood. Measure 80 ml of acetic anhydride. The solid was the crude product which released a noticeable smell of vinegar. The total mass of salicylic acid that we used in the beginning was 2. Crystals of aspirin should form.
And then determine the relative purity of the synthesized sample. When the temperature is within approximately 10ºC of the lowest possible melting temperature of your sample, turn the control knob to a temperature setting corresponding to your expected melting temperature. To do this, first tare a piece of weighing paper This means to put a piece of paper on the balance and press the zero or tare button. The procedure performed in our experiment involved chemically reacting salicylic acid and acetic anhydride in order to form acetyl salicylic acid. Aspirin can be made by reacting salicylic acid with acetic acid in the presence of an acid catalyst. Open and dispense in fume hood. Calculate the percent yield of your synthesis.
