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Eugenol extraction by chromatography
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Recommended: Eugenol extraction by chromatography
The purpose of this lab was to recover as much eugenol and acetyleugenol from 25 grams of cloves as possible. This lab was completed over the course of two days. The first day was dedicated to using simple distillation to collect 70 mL of distillate. The eugenol and acetyleugenol would later be recovered from the distillate. The second day was dedicated to separating the desired products from the distillate and from each other. This day was far more labor intensive and led to the completion of the lab. This lab utilized various techniques such as distillation, extraction and rotary evaporation. Separation, extraction, and recovery are key themes highlighted in this lab. Knowing where both eugenol and acetyleugenol were was vital to accomplishing …show more content…
the lab. The three phases of this lab were separaton, extraction, and recovery. Different techinques were used in each phase to help achieve the lab’s goal.
The recovery of eugenol and acetyleugenol was the objective of the lab. Due to this, it is important to note where eugenol and acetyleugenol were during each phase. Separation is done through the use of a separatory funnel. Different solutions were mixed in the separatory funnel and allowed to settle. Once settled, two distinct layers formed: one aqueous and one organic. The layers are then drawn off individually and the layer without the eugenol/acetyleugenol is discarded. The extraction portion of the lab takes place through the addition of various solvents. The eugenol and acetyleugenol were both solved in water to begin. Methylene chloride was added to the aqueous solution containing the eugenol and acetyleugenol. Once mixed the methylene chloride formed an organic layer which contained the eugenol and acetyleugenol. The aqueous layer became useless as the desired products were no longer in it. Sodium hydroxide was then added to the methylene solution which caused two distinct layers to form. The sodium hydroxide layer now contained the eugenol and the methylene chloride layer now contained the acetyleugenol. At that point, the methylene chloride layer containing the acetyleugenol was treated with anhydrous
sodium sulfate to help dry the solution. The methylene chloride layer containing the acetyleugenol then underwent rotary evaporation. This left nothing but the desired acetyleugenol. On the other hand, the sodium hydroxide layer containing the eugenol was placed in the separatory funnel and was mixed with water. After mixing, two distinct layers formed. The water layer now contained the eugenol and the sodium hydroxide layer became useless. The water solution containing the eugenol was then mixed with methylene chloride. After mixing, the methylene chloride layer now contained the eugenol while the water layer was discarded. The methylene chloride layer containing the eugenol was then dried with anhydrous sodium sulfate and subjected to rotary evaporation. This left the eugenol isolated as intended.
The unknown bacterium that was handed out by the professor labeled “E19” was an irregular and raised shaped bacteria with a smooth texture and it had a white creamy color. The slant growth pattern was filiform and there was a turbid growth in the broth. After all the tests were complete and the results were compared the unknown bacterium was defined as Shigella sonnei. The results that narrowed it down the most were the gram stain, the lactose fermentation test, the citrate utilization test and the indole test. The results for each of the tests performed are listed in Table 1.1 below.
This experiment synthesized luminol (5-Amino-2,3-dihydro-1,4-phthalazinedione) and used the product to observe how chemiluminescence would work. The starting material was 5-nitro-2,3-dihydrophthalazine-1,4-dione, which was, after addition of reaction agents, refluxed and vacuum filtered to retrieve luminol. Using two stock solutions, we missed our precipitated luminol with sodium hydroxide, potassium ferricyanide, and hydrogen peroxide, in their respective solutions, in a dark room, to observe the blue light
The boiling point of the product was conducted with the silicone oil. Lastly, for each chemical test, three test tubes were prepared with 2-methylcyclohexanol, the product, and 1-decene in each test tube, and a drop of the reagent were added to test tubes. The percent yield was calculated to be 74.8% with 12.6g of the product obtained. This result showed that most of 2-methylcyclohexanol was successfully dehydrated and produced the product. The loss of the product could be due to the incomplete reaction or distillation and through washing and extraction of the product. The boiling point range resulted as 112oC to 118oC. This boiling point range revealed that it is acceptable because the literature boiling point range included possible products, which are 1-methylcyclohexene, 3-methylcyclohexene, and methylenecyclohexane, are 110 to 111oC, 104oC, and 102 to 103 oC. For the results of IR spectroscopy, 2-methylcyclocahnol showed peaks at 3300 cm-1 and 2930 cm-1, which indicated the presence of alcohol and alkane functional group. Then, the peak from the product showed the same peak at 2930 cm-1 but the absence of the other peak, which indicated the absence of the alcohol
Benzyl bromide, an unknown nucleophile and sodium hydroxide was synthesized to form a benzyl ether product. This product was purified and analyzed to find the unknown in the compound.
The objective of this experiment was to perform extraction. This is a separation and purification technique, based on different solubility of compounds in immiscible solvent mixtures. Extraction is conducted by shaking the solution with the solvent, until two layers are formed. One layer can then be separated from the other. If the separation does not happen in one try, multiple attempts may be needed.
..., and is immiscible with water. Since there was not clear distinct two layers after steam distillation, extraction was used to separate the eugenol from water thus, steam distillation is not an effective way to isolate eugenol by itself. In order to determine how pure the isolated eugenol was, TLC was performed and compared to the standard and 1H NMR of the isolated eugenol and standard were compared to conclude that the extracted compound was eugenol with some impurities.
After performing the first Gas Chromatography, we took the organic layer, and mixed it with saturated Sodium Hydroxide. We performed this step to remove the (-OH) group from the Eugenol. The purpose was to make the water as a product, which can also be used as a solvent for the Eugenol that was ionized, for the two substances Acetyl Eugenol and Beta Caryophyllene. Again, we see the density differences in the solvents; we were able to take the organic layer. Finally, we transferred the layer into the beaker and dried, to perform the Gas Chromatography
After corking and inverting the reaction tube, the organic layer was removed and transferred to another reaction tube. Then another increment of 0.5 mL of methylene chloride was added to the first reaction tube and the extraction process was repeated. This was done a total of three times. Then in step thirteen, about five scoops of anhydrous sodium sulfate was added to the second reaction tube. Then a filter pipette was prepared and the organic solution from the second reaction tube was added to the pipette.The mixture was allowed to gravity filter and an additional 0.5 mL increment of methylene chloride was added into the pipette and the process was repeated again. Then in step 18, the collected solutions poured onto a watch glass. It was observed that the pre-weighed watch glass weighed 26.196 grams. The watch glass was placed over the beaker that was filled with 30mL of water. It was observed that it took about fifteen minutes for the solvent
That is why ethanol was used as a solvent during this lab, because due to its structure, it has both polar and non-polar regions. Ethanol has a polar alcohol end capable of dipole-dipole interactions and hydrogen bonding, but also has a relatively non-polar CH3CH2- end with mostly London dispersion forces (LDFs). The general rule for solubility is, “like dissolves like,” meaning that polar solutes will dissolve in polar solvents and non-polar solutes will dissolve in non-polar solvents. Once extracted, performing a simple separation known as thin layer chromatography (TLC), the extract can be verified to see if it contains eugenol. TLC uses ethyl acetate (a polar solvent) in order to dissolve the molecules (also polar) in the extract. The polar solvent also contains hexane (a non-polar solvent) which allows for the polar molecules to precipitate out as small spots on the TLC plate. As shown in Figure 4, the solvent will move up the TLC plate until it reaches the spotted samples: cloves extract (Our), nutmeg extract (Oth), and 10 mg/mL eugenol standard (s). Several spots on the TLC plate show the interaction between molecules in the extract and the silica on the surface of the TLC plate. If the molecules in the extract exhibit more non-polar characteristics, they will get pulled further up the
The purpose of this experiment is to learn how to use fractional distillation to separate a mix of isopropyl acetate and toluene, redistill them, and use gas chromatography to examine the separation.
The purpose of this lab was to experiment with various ways to separate mixtures into its pure components. Depending on whether a mixture is homogeneous or heterogeneous, mixtures can be separated by physical means and their physical properties. In this lab, we used chromatography, which is a technique that uses the differences in physical properties and intermolecular forces of the components in a mixture to separate them. Although there are different forms of chromatography, they all have a stationary and mobile phase. The mobile phase moves through the stationary phase and carries the components of the mixture at different rates. In this lab, paper chromatography and column chromatography will be used.
In this experiment, the goal is to separate naphthalene and benzoic acid from one gram of a crude mixture containing them both, using extraction. A general requirement of a solvent in extraction is solvating one of the pure compounds in solution but not the other. Position in the separatory funnel is determined by density of each layer. The denser layer will be on the bottom of the separatory funnel while the less dense layer will be the top layer of the separatory funnel. For extraction to be used as an effective method for separation, the components of a mixture that need to be recovered must not be soluble in the same solvent. Benzoic acid is not soluble in water, but is soluble in diethyl ether. In benzoic acid, the benzene ring is nonpolar
We were asked to extract benzoic acid from a kerosene-benzoic acid mixture. This was to be done using the stirred liquid-liquid extraction column in the senior laboratory. Fresh water was used as the continuous phase in the extraction. We were asked to measure the benzoic acid concentrations of the feed, raffinate, and extract streams. These measurements were to be made at several different steady-states. The number of theoretical stages and the height of the theoretical stages (HETS) was also to be determined. Because the liquid-liquid extraction column had not been used in several years our assignment also included discussing any problems with the process and possible solutions. The discussion of equipment, results, and experimental procedure will be discussed in the following paper entitled "Liquid-Liquid Extraction.”
Eugenol was extracted from cloves through the process called steam distillation. A total of 50ml of distillate were collected with temperature monitoring for every 5.0ml of collected liquid. The distillation curve showed that the temperature of volatilization of eugenol is from 98°C to 99°C which is way below its boiling point at 2540C. Chemically active extraction was conducted in order to remove impurities particularly eugenol acetate and caryophyllene. This involves the addition of several solvents particularly hexane, NaOH, HCl, then hexane again in succession.
The objective of the experiment Fractional Distillation and Gas Chromatography was to determine the organic liquids existent in 30 mL of an unknown mixture. This can be accomplished by fractional distillation. Distillation is a technique that allows one to separate liquids by boiling the liquids and which removes water from its impurities. Simple Distillation separates out a liquid/solid mixture. If the boiling point is greater than 40 degrees Celsius then simple distillation will be able to be used to separate two liquids, if not then Simple Distillation cannot be used. Fractional distillation splits two liquids and transfers them to their pure form by using their boiling points. In order for Fractional Distillation to be used, the boiling point has to be less than 40 degrees Celsius. The only difference between them is that in fractional distillation a column runs to the flask while in simple distillation there is no column. Of the two main types of distillation, Simple and Fractional, Fractional distillation is the one that is used to split the liquids. To get this experiment unde...