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5-bromoacetylsalicylic acid melts at 60 °C and is inert and almost insoluble in water at room temperature. Why can't water be used as recrystallizing solvent for this compound?

5-bromoacetylsalicylic acid melts at 60 °C and is inert and almost insoluble in water at room temperature. Why can't water be used as recrystallizing solvent for this compound?

Chemistry
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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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2. 5-bromoacetylsalicylic acid melts at 60 °C and is inert and almost insoluble in water at room temperature. Why can't water be used as recrystallizing solvent for this compound? 3. What would be the effect on the yield if too much activated carbon were added? 4. A fluted filter paper is used instead of a regular cone because it minimizes its contact with the glass funnel. Why do you think is this important? 5. If the volume reduction step was skipped, what would be the implications? 6. What would be the effect on the purity of the crystals if the hot solution was immediately placed on an ice bath to cool? 7. On the molecular level, what does it mean for a solid sample to be pure? 8. Heating of the oil bath must be done slowly to get a more accurate reading of the melting point of a sample. Why must this be done slowly? 9. Why is the capillary tube placed such that the open end is above the oil level? 10. The calculated percent recovery was above 100%. What could this have meant and what should be done?
Transcribed Image Text:2. 5-bromoacetylsalicylic acid melts at 60 °C and is inert and almost insoluble in water at room temperature. Why can't water be used as recrystallizing solvent for this compound? 3. What would be the effect on the yield if too much activated carbon were added? 4. A fluted filter paper is used instead of a regular cone because it minimizes its contact with the glass funnel. Why do you think is this important? 5. If the volume reduction step was skipped, what would be the implications? 6. What would be the effect on the purity of the crystals if the hot solution was immediately placed on an ice bath to cool? 7. On the molecular level, what does it mean for a solid sample to be pure? 8. Heating of the oil bath must be done slowly to get a more accurate reading of the melting point of a sample. Why must this be done slowly? 9. Why is the capillary tube placed such that the open end is above the oil level? 10. The calculated percent recovery was above 100%. What could this have meant and what should be done?
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