A student reacted 1.01g salicylic acid with 2.06mL acetic anhydride and isolated 1.40g aspirin. A) How can the result of the percent yield be explained based on the procedure used in this lab? B) Consider that a chemist accidentally added 10.1g salicylic acid instead of the 1.01 g specified. Would this procedural error have any effect on the actual yield of the synthesis? On the calculated theoretical yield? Briefly explain.

A student reacted 1.01g salicylic acid with 2.06mL acetic anhydride and isolated 1.40g aspirin. A) How can the result of the percent yield be explained based on the procedure used in this lab? B) Consider that a chemist accidentally added 10.1g salicylic acid instead of the 1.01 g specified. Would this procedural error have any effect on the actual yield of the synthesis? On the calculated theoretical yield? Briefly explain.

Macroscale and Microscale Organic Experiments

7th Edition

ISBN:9781305577190

Author:Kenneth L. Williamson, Katherine M. Masters

Publisher:Kenneth L. Williamson, Katherine M. Masters

Chapter7: Extraction

Section: Chapter Questions

Problem 6Q: To isolate benzoic acid from a bicarbonate solution, it is acidified with concentrated hydrochloric...

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How would each of the following errors affect the experimental value of your molarity of acetic? Would your Molarity value be too high, too low, or unaffected? Explain your answer. if you titrated your acid sample to a bright pink rather than faint pink endpoint? if your "acetic acid" burette was still wet inside with deionized water when you filled it with acetic acid? if you recorded the final volume of NaOH as "39.88 mL" instead of "38.88 mL"?
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To isolate benzoic acid from a bicarbonate solution, it is acidified with concentrated hydrochloric acid, as in experiment 1. What volume of acid is needed to neutralize the bicarbonate? The concentration of hydrochloric acid is expressed in various ways on the inside back cover of this laboratory manual.
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