4. When performing a melting point on a solid compound using a melting point apparatus, twomelting point determinations were made. One sample, which was 1 mm in height in thecapillary, possessed a melting point of 200.0-200.5°C. The other sample was 25 mm inheight. What would you expect the approximate melting point to be for this sample,assuming identical heating rates of 1°/min? (Hint: heat is applied from the bottom of thesample) (Give an actual numerical approximation!)5. For the same solid compound as the question above, if the 1 mm sample was heated at 60°per minute on a melting point apparatus, what would you expect for an approximatemelting point? (note that at this heating rate, the sample will melt rather quickly, but againgive an actual numerical approximation)

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EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter82: Physical Constants Of Liquids: The Boiling Point And Density

Section: Chapter Questions

Problem 5P

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A student was trying to prepare acetaminophen in the laboratory. She found a melting point range of 169-173. The melting of acetaminophen is reported to be 168-172c. How could the student have verified that the produce is acetaminophen? Retake the sample melting point with more material in the sample. Ask the lab partner to measure the melting point of the sample. Take a mixed melting point with an authentic sample of acetaminophen
1. What is the limitation of the sublimation laboratory technique? 2. When can sublination be applied as a process of separation?
explain how mixed melting point determination can be used to identify a solid compound.
What effect does the presence of impurity have on the melting point?
Heating of the oil bath must done slowly to get a more accurate reading of the melting point of a sample. Why must this be done slowly?
1. If all the ice were to melt just as the temperature reached 3.0 °C, would thisproduce an error in your experimental values? Explain your reasoning.
The melting-point capillary of a white crystalline substance is left to cool. The same capillary shows a substantially higher melting point of 145°C. Repeated recrystallization produces sharp melting points of about 114°C. Explain the behavior of a cooled and remelted sample.
Why would industry prefer to purify solids by sublimation or zone refining rather than recrystallization? (Hint: is there anything wasteful about recrystallization)
Filter paper is usually a poor material on which to powder a solid sample before introducing it into a capillary melting-point tube because small particles of paper may end up in the tube along with the sample. Why is this undesirable? and how might the presence of paper in the sample make the melting-point determination difficult
Calculate the change of melting point of naphthalene per atmospheric change of pressure, given melting point 80°C. latent heat = 35.5 cal/g. density of solid = 1.145 g/cc and density of liquid = 0.981 g/cc
Which of the following correctly describes the stationary and mobile phases for a reversed-phase HPLC separation? a) polar stationary phase, polar mobile phase b) non-polar stationary phase, non-polar mobile phase c) polar stationary phase, non-polar mobile phase d) non-polar stationary phase, polar mobile phase
How is the purity of a crystalized solid assessed?

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