Performing this experiment, we used the technique called Acid-Base extraction to isolate Eugenol, which is one of the main ingredients of clove oil. Acid-Base extraction is the most efficient method for isolating organic component; it is efficient because it purifies the acid and base mixture based on their chemical identities. We have seen throughout this experiment that acid and base play an important role, when it comes to solubility in water. Our basic knowledge of acid and base is acid is a proton donor and base is a proton acceptor. This ideology helps us to understand why organic compounds are not soluble in water. When compounds tend to be insoluble, we have to use acid and base reaction, to change its solubility. The changes that occurred …show more content…
Starting this experiment, we knew that the extraction was going to form varies layers due to the density differences. When placing three different substances, we saw that two layers formed because the Clove Oil is soluble in MTBE, but not in water. In order, to get the organic layer we used separatory funnel to take out the excess substances and leave the oil layer. Then we transferred to a beaker and dried with Magnesium Sulfate. Lastly, we filtered the liquid using funnel; we placed the liquid to boil, let it cool to room temperature. The purpose of drying and evaporation is to help us with the Gas Chromatography analysis of the product. 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
Every 5 minutes, a small amount of mixture was dissolved in acetone (0.5 mL) and was spotted onto a thin layer chromatography (TLC) plate, which contained an eluent mixture of ethyl acetate (2 mL) and hexanes (8 mL). The bezaldehyde disappearance was monitored under an ultraviolet (UV) light. Water (10 mL) was added after the reaction was complete, and vacuum filtrated with a Buchner funnel. Cold ethanol (5 mL) was added drop-by-drop to the dried solid and stirred at room temperature for about 10 minutes. Then, the solution was removed from the stirrer and place in an ice bath until recrystallization. The recrystallized product was dried under vacuum filtration and the 0.057 g (0.22 mmol, 43%) product was analyzed via FTIR and 1H NMR
As shown in figure 2, the percentage of each isomeric alcohol in the mixture had been determined. The hydrogen atom on the carbon atom with the hydroxyl group appear at around 4.0 ppm for borneol and 3.6 ppm for isoborneol. The product ratio has been determined by integrating the peaks. A ratio of 6:1 for the Isoborneol/borneol ratio was expected and is validated by the calculations shown above, with isoborneol percentage at 83.82% and 16.17% of borneol. A CHCl3 group noted at around 7ppm and a CH2Cl2 at around 3.5ppm.
Esters are defined as molecules consisting of a carbonyl group which is adjacent to an ether linkage. They are polar molecules which are less polar than alcohols but more so than ethers, due to their degree of hydrogen bonding ability. Most often derived from reacting an alcohol with a carboxylic acid, esters are a unique, ubiquitous class of compounds with many useful applications in both natural and industrial processes 1. For example, within mammals, esters are used in triglycerides and other lipids as they are the main functional group attacking fatty acids to the glycerol chain 2. A unique property of esters is their tendency to give off distinct aromas such as the scent of apples (Ethyl caprylate) and bananas (Isoamyl acetate). This is of a unique importance especially in industries that utilize flavors and aromas such as the tobacco, candy and alcohol industry. Consistent research is conducted in order to enhance and increase the effectiveness of esters in these products 3.
Firstly, an amount of 40.90 g of NaCl was weighed using electronic balance (Adventurer™, Ohaus) and later was placed in a 500 ml beaker. Then, 6.05 g of Tris base, followed by 10.00 g of CTAB and 3.70 g of EDTA were added into the beaker. After that, 400 ml of sterilized distilled water, sdH2O was poured into the beaker to dissolve the substances. Then, the solution was stirred using the magnetic stirrer until the solution become crystal clear for about 3 hours on a hotplate stirrer (Lab Tech® LMS-1003). After the solution become clear, it was cool down to room temperature. Later, the solution was poured into 500 ml sterilized bottle. The bottle then was fully wrapped with aluminium foil to avoid from light. Next, 1 mL of 2-mercaptoethanol-β-mercapto was added into fully covered bottle. Lastly, the volume of the solution in the bottle was added with sdH2O until it reaches 500 ml. The bottle was labelled accordingly and was stored on chemical working bench.
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.
Experiment #3: The purpose of this experiment to test the chromatography of plant pigments the alcohol test strip test will be used.
...bromebutane. Unfortunately, our group was only able to obtain the chromatograph for 2-bromobutane and the rest of the three chromatographs were provided by our T.A. Some possible reasons why the chromatographs for 2-butanol, 1-butanol, and 1-bromobutane were unable to be displayed properly is due to the malfunction of the syringes. If the syringe is not air-tight, the gaseous products can escape before being inserted into the injection port. In addition, the collection tube may have had a minor gas escape from the rubber septum, resulting in less concentrated gaseous products being inserted into the injection port. A possible solution is sealing the collection tube with parafilm. All in all, the provided data chromatographs and the rendered chromatograph by the 2-bromobutane in the lab session did match the expected results for the distribution of gaseous products.
The actual amount of crude product was determined to be 3.11 grams. The percent yield of the crude product was determined to be 67.75 %. The actual amount of pure product formed was found to be 4.38 grams. The percent yield of the pure product was determined to be 95.42%. Regarding the thin layer chromatography, the line from the solvent front is 8 centimeters.
The crude extract obtained by solvent extraction was subjected to various qualitative tests to detect the presence of common chemical constituents as:
The purpose of this experiment was to learn and preform an acid-base extraction technique to separate organic compounds successfully and obtaining amounts of each component in the mixture. In this experiment, the separation will be done by separatory funnel preforming on two liquids that are immiscible from two layers when added together. The individual components of Phensuprin (Acetylsalicylic acid, Acetanilide, and Sucrose as a filler) was separated based upon their solubility and reactivity, and the amount of each component in the mixture was obtained. Also, the purity of each component will be determined by the melting point of the component.
In order to separate the mixture of fluorene, o-toluic acid, and 1, 4-dibromobenzene, the previously learned techniques of extraction and crystallization are needed to perform the experiment. First, 10.0 mL of diethyl ether would be added to the mixture in a centrifuge tube (1) and shaken until the mixture completely dissolved (2). Diethyl ether is the best solvent for dissolving the mixture, because though it is a polar molecule, its ethyl groups make it a nonpolar solvent. The compounds, fluorene and 1, 4-dibromobenzene, are also nonpolar; therefore, it would be easier for it to be dissolved in this organic solvent.
The camphor then went through reduction with sodium borohydride to make isoborneol. This reaction was able to be stereochemically controlled by limiting the amount of heat we provided. The conversion of camphor to isoborneol has a lower
Data Table 3 indicates the observations from these tests. Though a control test for each test wasn’t prepared, due to the starting reagents being unattainable, the results clearly show that the product is unsaturated. An unsaturated compound means that there is/are bonds in its structure. The product was also analyzed by infrared spectroscopy and gas chromatography. The spectrums obtained allowed one to determine the composition of 1-methylcyclohexene; any impurities and excess products were observed as well. From the infrared spectrum, there is a little peak around 3300-3500 cm-1; this indicated a very little presence of alcohol in the product and thus, most of the alcohol has been successfully removed. If one compared the IR spectrum of the product to the starting material, 2-methylcyclohexanol, one could clearly see the change in peak size of the O-H stretch. The infrared spectrum of 1-methylcyclohexene also depicted a C-H stretch and an alkene functional group at 500-1500 cm-1 and 2932.54cm-1, respectively. From the gas chromatography spectrum (Data Table 4), the area percentages show that there were three products - peaks 22 through 24 - that were formed from the dehydration experiment. Nevertheless, there are two predominant products, as shown from their high percentages, 3-methylcyclohexene (~24%) and 1-methylcyclohexene
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.
In this experiment, lipids from ground nutmeg are extracted using a combination of solvents and identify the lipids through chromatography. The purpose of using solvent combinations is to elute the lipids based on their polarity to binding of the silica gel. The chromatography is performed on a silica gel plate and the use of iodine to visualize the lipids. By calculating the Rf values for each compound and comparing them to the known lipids, we are able to distinguish the lipids within the grounded nutmeg.