Benzopinacol Of Glacial Acetic Acid

For this experiment, an organometallic reagent was used for the synthesis and isolation of benzoic acid. The Grignard reaction is the addition reaction of an organometallic reagent, which in this case was an organomagnesium reagent. An organometallic reagent is a carbon bonded to a metal. This reagent was combined with an electrophile, a carbonyl compound such as a ketone or aldehyde. Carbons are electrophilic when bound to a nonmetal thus the atoms are more electronegative than the carbon and metals are less electronegative than carbon.

After 10 minutes the reaction liquid was separated from the solid using a vacuum filtration system and toluene. The product was stored and dried until week 2 of the experiment. The product was weighed to be 0.31 g. Percent yield was calculated to be 38.75%. IR spectra data was conducted for the two starting materials and of the product. Melting point determination was performed on the product and proton NMR spectrum was given. The IR spectrum revealed peaks at 1720 cm-1, which indicated the presence of a lactone group, and 1730 cm-1, representing a functional group of a carboxylic acid (C=O), and 3300cm-1, indicating the presence of an alcohol group (O-H). All three peaks correspond with the desired product. A second TLC using the same mobile and stationary phase as the first was performed and revealed Rf Values of 0.17 and 0.43for the product. The first value was unique to the product indicating that the Diels-Alder reaction was successful. The other Rf value of 0.43 matched that of maleic anhydride indicating some

6. Purpose: to clarify the mechanism for the cycloaddition reaction between benzonitrile oxide and an alkene, and to test the regiochemistry of the reaction between benzonitrile oxide and styrene; to purify the crude product of either trans-stilbene, cis-stilbene, or styrene reaction.

The purpose of this experiment is to prepare a Grignard reagent by reacting with alkyl or aryl halide and to ultimately react the Grignard reagent with carbon dioxide in order to produce carboxylate. The formed carboxylate is then protonated with an acid to produce carboxylic acid that could be used with liquid-liquid extraction to isolate the unknown acid from the other products from side reactions. The final unknown product is identified by measuring the melting point and calculating the molecular weight obtained from titration.

The objective of the lab was to produce benzilic acid from benzoin. Benzoin was successfully oxidized with nitric acid to form benzil. The percent yield of benzil was 59.26% and the melting point range was 94.1-95.5°C. The literature melting point of pure benzil is 95°C, which indicates the correct product was obtained. Benzil was then rearranged using potassium hydroxide to form benzilic acid. The percent yield of benzilic acid was 57.94% and the melting point range was 147.9-149.8°C. The literature melting point of pure benzilic acid is 150°C; this also indicates that the correct product was isolated. Crude products were

The first liquid-liquid extraction was performed with the weak base NaHCO3 revealing one of the unknowns to be a carboxylic acid. The second liquid-liquid extraction involved NaOH (a strong base) and revealed that the second unknown in the organic mixture was a phenol. Experimentally, it was determined that the melting point of the carboxylic acid was only slightly higher than

In the following reaction, benzil was rearranged to from benzilic acid by reacting it with potassium hydroxide in ethanol. 0.100 benzil was utilized and the theoretical yield of benzilic acid was 0.109 grams (see Eq 5). The final yield and weight of benzilic acid was 0.60 grams. The final yield and theoretical yield were used to calculate the percent yield, 55% (similar to Eq 3). The melting point of benzilic acid was 148.3C and the literature value for

This lab looks at the solubility, miscibility and melting point characteristics of different organic compounds in various situations. All three of these processes are essentially controlled by the intermolecular forces and polarity an organic compound consists of. Molecules benzophenone and methanol were put into different solvents to check for miscibility and solubility. Melting point ranges of pure and impure forms of cinnamic acid and urea were recorded by a Mel-Temp® machine.

To begin benzoic acid has a melting point of 121-125C. The melting point of recovered benzoic acid was 109-115C. There is a noticeable broaden and depression of the melting point which points to impurities. For the benzoic acid in particular the impurity could have been the ice cold water. To combat this next time, essential time should be allotted for the suction filtration to the component to dry and also a heating lamp could have been used to rid the benzoic acid of water. Next, benzocaine has a melting point of 89-92C. The melting point of recovered benzocaine was 77-99C. This melting point was significantly depressed and the range was dramatically broadened. A way to ride the component of impurities, once could suction filtrate the component for a longer amount of time or use a heat lamp to fully dry the component. Lastly, fluorenone has a melting point of 80- 83C, but the measured melting point of the component in the 1:1:1 mixture was 80-81 C. This reading is fairly close to the literature value, however to ensure a more accurate reading for the isolation of fluorenone, the sample could be heated longer or a sufficient amount of a drying agent would be

1996), Brame and colleagues explored whether such rearrangement also results in the formation of levuglandin-like compounds. Their findings concluded that -ketoaldehydes are also formed via the IsoP pathway, and was termed isoketals (IsoKs).

A sample of both benzoic acid and benzocaine were separately dissolved in acetone to allow for spotting for TLC analysis. A TLC plate was spotted with a sample of benzocaine and benzoic acid that was previously extracted and a reference of benzocaine and benzoic acid to allow for comparison. Once each sample was spotted onto the TLC plate, the plate was placed in glacial acetic acid and allowed the solvent to rise.

In this experiment Benzpinacolone was synthesized in a process that contained two steps. First the photoreduction of benzophenone in 2-propanol, which was done by placing the flask under sunlightfor the absorption of the UV rays to carry out the reaction. Then the second part was the dehydration of benzpinacol to benzpinacolone, where the benzpinacol product was converted to a ketone by the acid catalyzed rearrangement of the benzpinacol to the benzpinacolone; this was done by adding iodine and acetic acid to benzpinacol. The reaction was then refluxed, cooled in an ice bath, filtered and washed with ethanol. After

The relative difference of concentration between the heat and light treatments of isomenthone was observed to become smaller with time. As a result, it could be concluded that the minimal difference in isomenthone concentrations with time was due to it isomerizing to either l-menthone or l-menthol. Isomenthone was expected to convert to l-menthone rather than l-menthol as l-menthone was seen to have alkyl residues that fall in the equatorial position, which would make it more stable than if it fell on the axial position. The resulting equatorial configuration of l-menthone makes it thermodynamically and photochemically more favorable. (Kukula et al., 2000). As time passes, one would expect the increase in the isomerization of isomenthone to L-menthone.

Naphthalene and benzoic acid are two compounds studied in this experiment. Sodium benzoate is also an important substance involved in the separation process.

The second step is a solvent-free reaction that involves grinding the crude B-citronellol with KOH, K2CO3 and tosyl chloride. KOH serves to deprotonate the O-H group to form a better nucleophile and K2CO3 maintains the slightly basic conditions for the reaction.1 The crude product is vacuum filtered, followed by column chromatography obtaining test tube fractions. Used 7:3 hexanes: ethyl acetate to run the column. Obtained thin layer chromatography for crude compounds (Figure 1) and for test tubes 1-10 shown in Figure 2. The final product was a clear liquid and due to time constraints was unable evaporate solvent, thus experimental mass was not measured.