Determine the percent yield for an acylation reaction if beginning with 1.12 g of salicylic acid as the limiting reagent and 1.25 g of product was recovered. If 1.3 g salicylic acid and 0.8 mL acetic anhydride are used in the synthesis of aspirin, determine which is the limiting reagent and the theoretical yield.

Determine the percent yield for an acylation reaction if beginning with 1.12 g of salicylic acid as the limiting reagent and 1.25 g of product was recovered. If 1.3 g salicylic acid and 0.8 mL acetic anhydride are used in the synthesis of aspirin, determine which is the limiting reagent and the theoretical yield.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter22: Organic And Biological Molecules

Section: Chapter Questions

Problem 157CP

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1. Write out the balanced equation for the reaction between salicylic acid and aceticanhydride .2. Calculate the percent yield for the above reaction if the amount of aspirinobtained was 2.301 g. 3. Calculate the theoretical yield of aspirin if you start with 2.687 g of salicylic acidand an excess of acetic anhydride. 4. If you were to start with 1.00 g of salicylic acid, what volume of acetic anhydridewould be needed to completely react with it? The density of acetic anhydride is1.082 g/mL.5. According to your results from part 3 of this experiment, what can you say aboutthe purity of your aspirin? Be as specific as possible.6. Explain why acetic acid is unlikely to be a contaminant in your solid aspirin.7. Look up and record the boiling point of acetic acid, and explain why only some ofit evaporates from the reaction mixture.8. If you measured the melting point of the solid product from this experiment andobtained a melting range of 122-128 ℃, what does this tell you?9. Aspirin that…
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