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Fischer esterification
Fischer esterification
Fischer esterification
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In this lab, a sulfuric acid catalyzed Fischer Esterification reaction was conducted between p-aminobenzoic acid and ethanol in order to produce benzocaine. Once the reactants were done being heated under reflux, the precipitate was collected via vacuum filtration. This crude product weighed 1.35g and was then subject to another heating session with additional H2O while being stirred constantly. Methanol was then added to dissolve the solid and the product was then cooled to below room temperature. The pure product weighed 1.22g, giving a percent yield of 90.4%, and melting temperature as well as IR spectra and 1H-NMR were obtained.
Scheme 1: Fischer Esterification reaction between benzaldehyde and ethanol to produce benzocaine. INTRODUCTION:
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The practice of chewing the leaves from the “Coco bush” to produce mild stimulant effects had been observed in American Indian tribes surrounding the Andes mountains for years before the substance responsible for these symptoms was isolated from the Erythroxylon coca leaves.2 Cocaine was the first local anesthetic derived from this plant and it wasn’t until 1900 that German chemist Eduard Ritsert synthesized benzocaine as a non-addictive substitute to its high-risk-for-abuse counterpart.1 For a long time, however, it was not fully understood how this family of compounds interacted with the body. After cocaine’s initial discovery, it was prescribed for numerous applications from a common toothache to fighting depression.4 In recent years, the effects of cocaine’s influence as a local anesthetic are …show more content…
The mixture was stirred until all of the solid was completely dissolved. 2 mL of concentrated sulfuric acid were added dropwise before a condenser was attached and the apparatus was equipped for heating under reflux. The solution was then heated gently under reflux for 30 minutes. Since no solid was present after the first 30 minutes and the mixture was homogenous, it continued to be heated under reflux for an additional 30 minutes. After this period of time, the mixture was set aside and allowed to cool to room temperature before being poured into a beaker containing 30 mL of water. Next, the pH of the mixture was raised to 8 by slowly adding 10% aqueous sodium carbonate with stirring. The pH was tested using standard pH paper. The crude benzocaine product was then collected via vacuum filtration and then rinsed with 3 washes of cold diluted water. After dry, the crude product was weighed (1.35g) and transferred to a 50 mL Erlenmeyer flask with a stirbar and 20 mL of water. The mixture was then stirred while being heated to 60°C and then just enough methanol was added in order to dissolve the solid. Once all solid had dissolved, it was allowed to cool to room temperature before being added to an ice bath for 10-15 minutes to complete the crystallization. Once again, the product was vacuum filtered to obtain the crystal final pure
The percent yield of products that was calculated for this reaction was about 81.2%, fairly less pure than the previous product but still decently pure. A carbon NMR and H NMR were produced and used to identify the inequivalent carbons and hydrogens of the product. There were 9 constitutionally inequivalent carbons and potentially 4,5, or 6 constitutionally inequivalent hydrogens. On the H NMR there are 5 peaks, but at a closer inspection of the product, it seems there is only 4 constitutionally inequivalent hydrogens because of the symmetry held by the product and of this H’s. However, expansion of the peaks around the aromatic region on the NMR show 3 peaks, which was suppose to be only 2 peaks. In between the peaks is a peak from the solvent, xylene, that was used, which may account to for this discrepancy in the NMR. Furthermore, the product may have not been fully dissolved or was contaminated, leading to distortion (a splitting) of the peaks. The 2 peaks further down the spectrum were distinguished from two H’s, HF and HE, based off of shielding affects. The HF was closer to the O, so it experienced more of an up field shift than HE. On the C NMR, there are 9 constitutionally inequivalent carbons. A CNMR Peak Position for Typical Functional Group table was consulted to assign the carbons to their corresponding peaks. The carbonyl carbon, C1, is the farthest up field, while the carbons on the benzene ring are in the 120-140 ppm region. The sp3 hybridized carbon, C2 and C3, are the lowest on the spectrum. This reaction verifies the statement, ”Measurements have shown that while naphthalene and benzene both are considered especially stable due to their aromaticity, benzene is significantly more stable than naphthalene.” As seen in the reaction, the benzene ring is left untouched and only the naphthalene is involved in the reaction with maleic
The alcohol starting material, 2-methylcyclohexanol, was dehydrated through an E1 elimination by using of phosphoric acid as a catalyst. After a purification by simple distillation, which removed the alkene product and the by-product water from the reaction mixture, the methylcyclohexene products were analyzed by percent yield, boiling point, IR spectroscopy, and two chemical tests, Br2 in CCl4 and Jones test. By performing the simple distillation using pyrolysis, 85% of phosphoric acid and 2-methylcyclohexanol were added into the boiling flask, where the product from the collecting flask was condensed by the ice, and washed with the saturated sodium chloride. The weight of the product was determined and the percent yield of the product was
Alka Seltzer Dissolving at Different Temperatures. The variable that I will change will be the temperature of the water. that the Alka Seltzer is put in. For my results I will measure the time taken for the Alka seltzer.
In this experiment, a mixture of three substances (benzoic acid, 2-naphthol, and 1-4 dimethoxybenzene) will be separated based off acidity strength using the liquid-liquid extraction technique through a separatory funnel. Benzoic acid and 2-napthol will be converted into ionic salts when reacting with their appropriate bases (sodium bicarbonate and sodium hydroxide). Both ionic salts will then form solids through the addition of acidic HCl. Neutral 1,4 – dimethoxybenzene forms a solid through the evaporation of ether. Each compound will then be purified through recrystallization, using the processes of dissolving the solid in either water or methanol, and isolating the solid through vacuum filtration. After a week of evaporation, the compounds will then be examined for both
In the first part of the experiment, The mixture was combined with saturated sodium chloride, and the aqueous layer, containing alcohol, some acid, and water, was discarded. The organic layer was then dried with granular anhydrous sodium sulfate; this drying agent is used to absorb any water in a solution and should thus, result in a colorless solution. The final product was collected; it was mostly clear, though it has a pale yellow tint. Data Table 2 shows the results and calculations that were gathered after the completion of this experiment. No errors had occurred during the course of the experiment, which is testified by the fairly, high yield of Data Table 3 indicates the observations from these tests.
The two diastereomeric products that are made do not separate well by TLC. In order to see the two isomers, it is necessary to convert the products into derivatives. To more easily identify the stereoisomers produced in the reduction of benzil, hydrobenzoin is converted to acetonide by reacting with 2-methoxypropene and acid. The cis and trans isomers of these derivatives have different Rf values on TLC making it possible to identify the stereoisomers that have been prepared. The solution is compared with syn and anti acetonide on two different TLC plates.
The actual melting point of benzoic acid is known to be 122.4°C. Also, looking at Table1, the percent yield is shown to be 44.9%. The percent yield is how much product was recovered after the reaction was carried out. The percent yield can be used to explain why the melting point observed in the experiment didn’t match the known melting point. Obtained melting points are generally lower than the literature value melting points of a substance due to the number of impurities present in the obtained product. The percent yield of 44.9%, validates that the product could have had some impurities present, and thus the lower melting
For this experiment, a Fischer esterification reaction was observed. A Fischer esterification is a reaction that converts a carboxylic acid into an ester. Within the reaction, the hydroxyl portion, -OH, of the carboxylic acid is replaced by an -OR group. The byproduct is water which is also a nucleophile. Therefore, water can be added back into the compound and undergo hydrolysis on the newly formed ester which produces the starting carboxylic acid. To make sure the reversibility did not occur, the reaction mixture was heated to force the water to evaporate and therefore be removed from the overall reaction. The main idea of Fischer esterification is to form a carboxylic acid and make it a better electrophile under acidic conditions. This is
This experiment involves performing various techniques, including heating under reflux, separation, drying, distillation, gas chromatography (GC), infrared spectroscopy (IR spectroscopy), and nuclear magnetic resonance (1H NMR). Heating under reflux is important to overcome any activation barrier of energy that may be present in order to complete the reaction.
When benzoic acid paired with 1.0 M NaOH, it was observed that both compounds were soluble. Upon the addition of 6.0 M HCl into this solution, benzoic acid became insoluble. Benzoic acid was also insoluble in 1.0 M HCl. Ethyl 4-aminobenzoate was found to be insoluble in 1.0 M NaOH and soluble in 1.0 M HCl. But then, after adding 6.0 M NaOH into the test tube C (mixture of ethyl 4-aminobenzoate and 1.0 M HCl), a white powdery solid (undissolved compound) was formed. These demonstrate that both the acid and base became more soluble when they were ionized and less soluble when they were
The percentage yield gained was 70% from the Fischer Esterification reaction, which evaluates to be a good production of yield produced as the reaction is known to be reversible where conditions such as the concentration of the reactants, pressure and temperature could affect the extent of the reaction from performing. These white crystalline crystals were tested for impurity by conducting a melting point analysis and taking spectrospic data such as the IR spectra, HNMR and CNMR to confirm the identification of the product. These spectrospic methods and melting point analysis confirmed the white crystalline crystals were benzocaine.
In a 100ml beaker place 50mls of water, measure the temperature of the water and record this initial temperature onto a table. Set the timer and add one teaspoon of Ammonium Nitrate to the water, stir this continuously until the Ammonium Nitrate has dissolved.
9. Vispute, T. P., Zhang, H., Sanna, A., Xiao, R. & Huber, G. W. Renewable chemical commodity feedstocks from integrated catalytic processing of pyrolysis oils. Science 330, 1222–7
After the some time, we filter it through a Büchner funnel before it is recrystallized and filtered again. The mass was recorded as it was dry. By adding sodium carbonate, we will now test whether what obtained is benzoic acid or not, because one can observe bobbles if it is an acid. After that we burn it to test if it is aromatic.
There are many methods available for the synthesis of azo compounds but the classical methods for the synthesis of azo compounds are azo coupling reaction (coupling of Diazonium salt with activated aromatic compounds), Wallach reaction (transformation of azoxybenzenes in to 4-hrdroxy substituted in acid media), and Mills reaction (reaction between aromatic nitroso derivative and aniline), which are mostly used in the present investigation as well.