The goal of this lab was to synthesize benzocaine by utilizing Fischer esterification, reflux, and melting point determination techniques. These techniques were successfully performed and the synthesis was successfully performed. Although, the synthesis was not very efficient due to the low percent yield of the product (28%) and the melting point of the product not correlating to that of benzocaine.
In order to isolate benzoic acid, benzocaine and 9-fluorenone, each component needed to be separated from one another. All three compounds began together in one culture tube, dissolved in methylene chloride and formed into a homogenous mixture. In this culture tube, two milliliters of aqueous three molar hydrochloric acid was added, which immediately formed two layers, the top acidic aqueous layer was clear in color and contained benzocaine, and the bottom organic formed was yellow and contained benzoic acid and 9-fluorenone. Benzocaine’s amino group is protonated by the aqueous layer hydronium. This protonation forms the conjugate acid of benzocaine, benzocaine hydrochloride. Thus, the conjugate acid, benzocaine hydrochloride is a salt in which is soluble in water and furthermore can be isolated from the organic mixture. When testing out the pH levels in benzocaine, the pH test strip was dark blue in color, indicating a pH level of around 5 to 7. When isolating benzoic acid, two milliliters of aqueous three molar sodium hydroxide was added, which deprotonates the carboxylic group in benzoic acid, forming its conjugate base, sodium benzoate. As with benzocaine hydrochloride, sodium benzoate is a water soluble ionic salt in the aqueous layer that can then be separated from the bottom organic layer containing the 9-fluorenone. The pH test strip was a vibrant red for benzoic acid, indicating a pH of 2. Now the 9-fluorenone is left, deionized water is added to remove any excess
The product obtained had a melting point of approximately 107 °C and a weight of .324 grams. Some of the product would not dissolve in water and so was removed through vacuum filtration, which left .141 g not dissolved in solution. It took 13.2 mL of sodium hydroxide to turn the solution of the product dissolved in water pink. A molecular weight of 138.63 g/mol was calculated from the data. These results indicate that the product was 2-methylbenzoic acid, the Grignard reagent was 2-methylphenylmagnesium bromide, and the unknown bromide solution was 2-methylbromobenzene. Calculations showed that the limiting reagent of the Grignard preparation was magnesium and that the experiment had a 23.13 % yield.
The hydrobenzoin (meso) product of the benzil was isolated through the techniques of recrystallization and vacuum filtration. Because there NaBH4 was the limiting reagent in the experiment, 0.005604moles of NaBH4 should yield 1.2008g of hydrobenzoin (meso). The mass of the isolated product was 0.613g, resulting in a 51.1% yield. There are many reasons to account for the loss of 48.9% of
Abstract: This procedure demonstrates the nitration of methyl benzoate to prepare methyl m-nitrobenzoate. Methyl benzoate was treated with concentrated Nitric and Sulfuric acid to yield methyl m-nitrobenzoate. The product was then isolated and recrystallized using methanol. This reaction is an example of an electrophilic aromatic substitution reaction, in which the nitro group replaces a proton of the aromatic ring. Following recrystallization, melting point and infrared were used to identify and characterize the product of the reaction.
In this lab, liquid-liquid extraction was performed to isolate a mixture of benzocaine and benzoic acid. 2.0107 grams of the mixture was first weighed out for the trials. When HCl was added to the mixture for the first acid extraction of benzocaine, an emulsion formed during inversion and venting that prevented a defined separation of the two layers. 8 mL of water was therefore added before continuing the extraction. The addition of NaOH then turned the top aqueous layer basic, indicated by the pH strips that turned blue when tested. A vacuum filtration isolated 0.29 grams of benzocaine and a MelTemp apparatus measured the crystal’s melting point ranges to be 85.1C-87.4C. For the base extraction of benzoic acid, the aqueous layers were retrieved
In this experiment, a Fischer Esterification reaction was performed with two unknown compounds. The unknown compounds, Acid 2 and Alcohol D, were identified by using the knowledge of the reaction that took place, and the identity of the product that was synthesized. The identification of the product resulted from analysis of IR and NMR spectra.
Purpose: The purpose of the experiment was to perform the acid-catalyzed Fischer Esterification of acetic acid and isopentyl alcohol to form isopentyl acetate, or banana oil, which is used in flavor industries. The equilibrium of the reaction was changed by adding an excess amount of acetic acid. The reaction was refluxed and product was purified by extraction and distillation. Isopentyl acetate was analyzed by infrared spectroscopy and 1H NMR spectroscopy.
igure 1.2 gives the Txy diagram for the benzene/toluene system at a pressure of 1 atm. The abscissa is the mole fraction of benzene. The ordinate is temperature. The lower curve is the “saturated liquid” line that gives the mole fraction of benzene in the liquid phase x. The upper curve is the “saturated vapor” line that gives the mole fraction of benzene in the vapor phase y. Drawing a horizontal line at some temperature and reading off the intersection of this line with the two curves give the compositions of the two phases.
In an attempt to meet climate emissions goals, scientists are obtaining and using carbon dioxide emitted by power plants and other sources. In theory, carbon dioxide is easy to capture. This is because it is acidic, and it reacts effortlessly with simple bases like amines. In practice, however, amine scrubbing, the method used by some power plants to capture carbon dioxide for cleaning flue gases, is defeated because it encloses the greenhouse gas in water-based solutions. An abundance of energy is required to heat these great amounts of water in order to release the carbon dioxide that was captured and to renew the amines.
The purpose of this experiment is to practice common organic laboratory techniques inside the lab to get one oriented to the basic methods of procedure that can be used for later experiments. This experiment involves the separation of benzoic acid from a more crude form, consisting of benzoic acid, methyl orange, a common acid/base indicator, and cellulose, a natural polymer of glucose (Huston, and Liu 17-24). The technique that is used to perform this separation is called extraction. Extraction is a systematic process of separating mixtures of compounds, taking advantage of the affinity differences of compounds to separate them (Padias 128-37). This technique recognizes the principle that “like dissolves in like,” that is,
Atrazine inhibits the photosynthesis and the formation of ATP by blocking the electron transport. In photosystem 2, D1 and D2 proteins form a dimer to which all the electron-carrier cofactors are bound to. As one electron is excited and transferred from P680 to Pheophytin which rapidly transfers the electron to a protein-bound plastoquinone, QA. This QA will also rapidly give its electron to another plastoquinone QB. In this low-growing/dying scenario,electrons cannot be transferred to QB due to the presence of aatrex fertilizer which binds to the QB-binding niche of D1 protein. Therefore, it blocks the electron transport from QA to QB. As a result, there was no plastoquinol QBH2 (a fully reduced quinol form) formed in order to transfer the
After all additional product ceased to form, the reaction mixture was cooled in an ice bath to allow precipitation of benzopinacol. The final product was then filtered off from the solution using a Buchener funnel. Its melting point, yield and infrared spetrum was then obtained.
Appendix B.3 of the textbook Analysis, Synthesis, and Design of Chemical Process 4th Edition summarizes a styrene synthesis process from an equilibrium, de-hydrogenation of ethylbenzene. The equilibrium leaves various amounts of impurities as well as unspent ethylbenzene which is removed by a two stage separation process. The process can be improved upon and optimized for higher product throughput and lower operational and maintenance costs. The separation system was modeled on Aspen Plus V8.6 and a cost analysis performed on CapCost 2012.
World War II, deemed the “scientists’ war,” is unquestionably considered a turning point in history as it marked the modifying of warfare as science remarkably progressed. Although caffeine was safe and its benefits were well-noted, some military leaders believed it was incompetent for the purposes of war, thus leading to the thorough exploration of the benefits of amphetamines. Beginning in the mid-1930s, an American pharmaceutical company, Smith, Kline and French Laboratories, began producing and selling amphetamine sulfate under the brand name Benzedrine. Benzedrine’s prosperous debut into the US market spurred German pharmaceutical companies to cultivate their own stimulants. Beginning in 1938, after Temmler’s introduction of methamphetamine, labeled as Pervitin, German researchers began to investigate its effects. The department head of research at Temmler, Freidrich Hauschild, took five milligrams of Pervitin and reported that the stimulation he sensed was
Benzene is an organic chemical with the chemical formula of C6 H6. It is a chemical that appears as a colourless liquid or sometimes slight yellow at room temperature. Benzene boils at 176.2 degrees Fahrenheit and freezes below 41.9 degrees Fahrenheit. It has a sweet petrol like odour and is highly flammable. The hydrocarbon is derived from benzoic acid and is therefore named benzene. Michael Faraday an English scientist, famous for his work with electronic fields, first isolated and identified benzene in 1825 from the oily residue derived from the production of illuminating gas. In 1834 Eilhardt Mitscherlich heated benzoic acid with lime and produced benzene. In 1845 A von Hofmann isolated benzene from coal tar. Benzene dissolves only slightly in water and will sit on top of the water as they are of different density’s. Benzene evaporates into the air very quickly. Its vapour is heavier than air and may sink into low-lying areas.