I. Product Background A. Introduction In this highly luxurious extravagant world‚ food and other beverages has always been one of the things which maintain the mainstream of life. Aside from being one of the basics for survival‚ gatherings are also made perfect by food preparation and stress is now often associated with food. This activities show that food intake nowadays is far different from the conventional times. Furthermore‚ this lavish lifestyle most of the people have results in an
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Experiment 5B: Ketone Reduction Objective: Using sodium borohydride as a reducing agent‚ the ketone 4-tert-butylcyclohexane is reduced to its corresponding alcohol. It is purified through extraction techniques to give the cis and trans diasteromer products. Procedure: The procedure was followed as outlined in Mayo’s book for Experiment 5B with the following modifications: 1. Reagents and Equipment – The reaction will be on a scale of 2X what is described in the text. 2. Reagents and Equipment
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drying the solid product obtained from the vacuum filtration portion of the method of experimentation. Because the product was not fully dry during the melting point portion of the experiment‚ the melting point results were skewed. The reactants and solvents in the reaction each have significantly lower melting points than the product. Specifically‚ cold petroleum ether was used to wash the crystals in the drying portion of the experiment. Petroleum ether has a melting point of ~-73.0°C.9 It is possible
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sequence. 3) Each of the following reactions will not proceed as written. Use no more than fifteen (15) words per response to explain why the reactions would fail under the given conditions. 4) THF is readily soluble in water while a similar solvent molecule‚ diethyl ether‚ is completely insoluble in water. What major intermolecular force is responsible for such a solubility property? Why is this force more likely to participate with THF than with diethyl ether? 2 Vanden Eynden CHM2510
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-grease spot test: A drop of liquid food sample was added to a filter paper and was let to dry for 5 minutes. The filter paper was held up to the light and any translucent spot was observed. The filter paper was put into an organic solvent. it was taken out and let to dry The filter paper was examine against light again. (positive result – translucent spot disappears) -Clinistix paper: A drop of liquid food sample was added to the well of a spot plate The Clinistix paper
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GROUP 2 EXPERIMENT 15 BSP2M ORGANIC CHEMISTRY LABORATORY MR. WILBERT MORALES Chemical Structure Physical Properties Hazards Acetonephenone Physical state and appearance: Liquid. (Liquid.) Odor: Not available. Taste: Not available. Molecular Weight: 120.16 g/mole Color: Colorless to light yellow. pH (1% soln/water): 7 [Neutral.] Boiling Point: 201.7°C (395.1°F) Melting Point: 19.7°C (67.5°F) Critical Temperature: Not available. Specific Gravity: 1.03 (Water
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solutions. To measure the partition coefficient of ionizable solutes‚ the pH of the aqueous phase is adjusted such that the predominant form of the compound is unionized. The logarithm of the ratio of the concentrations of the unionized solute in the solvents is called log P. The log P value is also known as a measure of lipophilicity; greater the logP value‚ higher will be the lipophilicity. The distribution coefficient for ionizable
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derived from the kola nut. The water soluble materials in the tea leaves are extracted into hot water. The hot solution is allowed to cool and the caffeine is then extracted from the water with dichloromethane (methylene chloride)‚ which is an organic solvent that is insoluble in water. Since caffeine is more soluble in dichloromethane than it is in water‚ it readily dissolves in the dichloromethane. This experiment is aims to isolate crude caffeine from tea leaves. The purity of caffeine is determined
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The experiment did not contain any form of reaction mechanism since no chemical identity had been changed. The lab demonstrates the use of chemical molecular behavior to isolate a particular set of molecules. Caffeine had already existed in the leaf itself but needed to be separated from the other chemicals. Caffeine’s chemical structure is relatively similar to the nucleic acid purine in that they use nitrogen and is bicyclic but lacks an alkene‚ amine and an amide. Caffeine has a solubility of
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will not dissolve‚ will be visible‚ and also able to separate. According to our data our hypothesis supported the experiment because CARBOSE and sand are soluble in water while naphthalene is not. The CARBOSE‚ and sand will dissolve in the liquid solvent and the naphthalene will remain in the solid phase. In the other substances methanol and mineral spirit were not soluble in both Carbose and sand. Also in naphthalene mineral spirit was not soluble.
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