Determination of Melting Points of Benzoic Acid and Benzamide and Composition Diagram of Their Mixtures

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PURPOSE


The purpose of this experiment is to determine the melting point of benzoic acid and benzamide and make a composition diagram for the mixtures of benzoic acid and benzamide to determine the eutectic point of the mixtures. The melting point of the given unknown will be determined using the melting point apparatus. Pure chemicals such as benzoic acid and benzamide alone have a set melting point, but when missed with impurities or each other, the melting point decreases depending on the amount of each present in the sample. This allows us to determine if the unknown is a pure chemical with a set melting point, or a mixture of two or more chemicals with a lower melting point. The sample will be loaded into a capillary tube, and the heat will be provided by either a thiel tube filled with mineral oil and a Bunsen burner flame, or a mechanical apparatus.


THEORY


It is important to remember that the vapor pressure is responsible for the exchange or transfer between the solid and liquid phases of matter. the vapor pressure of solid and liquid are at equilibrium and unless temperature, pressure or any other force is applied, the system will remain at equilibrium at the melting point. Every substance has a point where both solid and liquid phases are at equilibrium, known as the melting point. Pure substances have a set constant melting point due to the set vapor pressure for each specific pure compound. The melting point will be altered if the vapor pressure is altered in any way. Anything substance that alters the melting point of a substance can be called an impurity. According to Raoult’s Law, the vapor pressure (melting point as well) will be lowered when an impurity (another substance) is mixed or introduced to the pure compound. This mixture of substances results in the decrease of the mixture’s melting point. The more the impurity is added, the lower will be the melting point of a mixture of the impurity. This process forces the equilibrium of this mixture to be reached at a lower temperature than expected for either the pure compound of the impurity compound. The melting points of the impurity compound or the pure compound will lower than either melting point, where the components of the impure mixture are at equilibrium.


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The concept of vapor pressure and the effect of lowering the melting point of a substance via impurity addition is used to identify an unknown in this experiment. Once the melting point for a pure sample has been determined, it will be easy and quite obvious to detect an impurity when one is present due to the lowering of the mixture’s melting point. In this experiment an unknown compound is given. The task is to determine the identity of this compound using a list of candidate compounds and Raoult’s Law. If the candidate substance is not the unknown compound, the melting point will decrease. If the candidate is the unknown, the melting point of the solution should remain the same, regardless of the amount of candidate added.


Table of physical constants


Name of Compound M.W. (g/mol) M.F Molecular


Structure Density (g/mol) b.p (CF) M.P.


B.P.


(CF) Solubility Hazards


Benzoic Acid 1.1 C7H6O 1. 4. 1.4


50.0 Alcohol


Chloroform


Ether


Acetone


Benzene


Mild irritant to skin, eyes, and mucous membranes.


Benzamide 11.14 C7H7NO 1.4 88 1.1


0.0 Water


Alcohol


Pyridine


Benzene(hot)


Ether


Ammonia


RESULTS/DISCUSSION


The results followed Raoult’s Law. When either compound was treated with the other (impurity), the temperature of the mixture decreased. It was only when the mixture was equally mixed (50-50 at mixture C) was the eutectic point reached. What failed to happen is the increase of the range of the melting point of the mixtures where Benzamide was forms the majority.





Mixture Low Melting Point High Melting Point


Benzamide 14 16


A 0


C 80 8


D 8


E 87 100


Benzoic acid 10 15


One possible explanation for that an insufficient amount of mixtures A was tested. Therefore, the recorded high melting point occurred earlier than was expected. In addition, the eutectic point at mixture C was not a point. It displayed a relatively wide range compared to what was expected. It was expected, according to Raoult’s Law that there should be no discrepancy between the low and high melting points at the eutectic point. Possible explanation is that an excess amount of the mixture was inserted to the melting point capillary, causing the recorded high melting point to occur higher than what was expected. Despite the results, the overall data and graph pointed to a picture where Raoult’s Law was obeyed.


This knowledge was used to try to determine the identity of the unknown substance. Once the melting point was determined, the list of candidates shrunk to Urea and Phenacetin. Phenacetin was tested and was not determined to be the substance because its melting point decreased to 14-18 degrees Celsius. Urea then is the most likely substance since the melting point did not change.





CONCLUSION


The outcomes of the experiment were in general agreement with the concept specified in the theory. If there is a suggestion regarding the conduction of this experiment, it is suggested that the amount of the mixtures not be “approximately measured.” The amount of the mixtures, as shown in this experiment, plays a big role in the determination of the high melting point. Therefore, in future replication of this experiment, an “exact” amount of the substances must be measured prior to testing to ensure that it follows the results predicted by Raoult’s Law.





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