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CHEM 104 Experiment 7 Organic Synthesis - Portage Learning $14.49
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CHEM 104 Experiment 7 Organic Synthesis - Portage Learning
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CHEM 104 Experiment 7 Organic Synthesis - Portage Learning Purpose: The purpose of this lab was to determine the process of synthesizing various carboncontaining organic products including aspirin, urea, & salicylic acid. In doing so, we were also able to calculate the percent yield in each of the...

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  • August 25, 2023
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  • 2023/2024
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1 Chemistry Notebook Name: Date: Experiment #: 7 Title: Organic Synthesis Purpose: The purpose of this lab was to determine the process of synthesizing various carbon - containing organic products including aspirin, urea, & salicylic acid. In doing so, we were also able to calculate the percent yield in each of these experiments. Procedure: Part 1: Synthesis of aspirin 1. Placed 2.0 g of salicylic acid & placed it in a flask 2. 5.0 mL of acetic anhydride was then added to the flask & mixed 3. 5 drops of sulfuric acid was added to the flask, which acts as a catalyst (helps the reaction to take place) & causes a yellow color change 4. Using a Bunsen burner, heat the flask in a beaker of water for 15 minutes 5. During the heat time, we expect that one of the acetyl groups to replace H 6. Most of the solid in the flask dissolved during the heating process 7. Add a couple mL of water while the flask solution is still hot to use up any unreacted acetic anhydride 8. Allow the flask to cool for a few minutes 9. Add 40.0 mL of ice water to the flask and mix, this causes a precipitate to form (white solid – that’s the aspirin) 10. Cool the flask in a beaker of ice water 11. While cooling, scratch the bottom of the flask to help induce crystallization of the solid 12. Now we need to isolate the white solid in the flask by utilizing suction filtration 13. Suction filtration is performed by attaching the flask to a water aspirator, which sucks the air out of the flask & filters the aspirin from the solution 14. Confirm the synthesis of aspiration by taking a tube & placing salicylic acid & a few drops of Fe3+ to the tube, producing a dark/deep purple color since phenolic groups are present; however, aspirin doesn’t have a phenolic group (we used all of them up in the reaction) so there will be no color change when the drops are added 15. Determine the melting point of the synthesized aspirin by using a melting point apparatus 16. Weigh the dried aspirin & then calculate the % yield Part 2: Synthesis of Urea 1. Prepare 2 solutions of potassium cyanate and lead nitrate, mixing them to create lead cyanate (which will then be prepared to make urea) 2. When mixed, notice the white precipitate that is formed 3. Cool this solution in a beaker of ice water for 15 minutes 4. After cooled, we filtered this solution to obtain the lead cyanate precipitate (white stuff on the bed of the filter)

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