Triphenylmethanol Synthesis Lab Report

Abstract: In this experiment, triphenylmethanol was synthesized in two steps. First, the bromobenzene was reacted with dry magnesium turnings to produce Grignard reagent. Second, the Grignard reagent was reacted with methyl benzoate and concentrated sulfuric acid to produce an alcohol. The end result of the experiment was not very successful because only 17% yield of final product triphenylmethanol was recovered, and the final product was impure based on the melting point and the IR spectrum results.

The other possibility for the unknown neutral, 1,4-dimehtoxybenzone, would have had an H NMR spectra with two peaks; however, the spectra obtained did not show chemical shifts for an aromatic ester group and had many hydrogens in the aromatic

Introduction The purpose of this week’s lab was to enhance our understanding of the Grignard reagents that were examined in lecture. In this lab, a Grignard reagent will be prepared through the reaction of magnesium turnings and bromobenzene. Instead of isolating the product it will then be combined with benzophenone, which will give the final product of triphenylmethanol. Procedure

To go in more depth, 98.2% is a high yield, despite the inaccuracies due to time constraints, and the inability to the recrystallize the benzoic acid. As mentioned earlier, product might have been lost during the many filtration procedures in the experiment, as not all of the product was poured out from the flask, onto the filter. Since, recrystallization could not be done, the benzoic acid was immediately transferred onto the watch glass, and it is when transferring some product could have been left on the filter. Overall, pouring product into the filter, and trying to get every particle of product from the flask for each filtration procedure in the experiment, is rather difficult, and is impossible to get every bit of product. Another key possibility, though it fortunately did not occur in the experiment, a green, or purple result

Using H NMR and IR spectroscopy, we were able to identify important structures in the limonene structure. As a group, we were not able to conduct the polarimetry part of the lab due to time

Consider that the difference between the reactant and product’s NMR spectrum will differ due to the change of the an 2o alcohol to a ketone. Isoborneol would there for have two more speaks than what would be seen in the camphor spectrum. These peaks would include a single peak from the OH proton along with a peak from the proton found on the carbon that that OH group is attached (approx. 3.5 ppm). Camphor would lack this two protons, thus causing smaller splitting patterns than would be seen in the isoborneol

This supports the isolated product is majority made of the desired product and is largely pure. Mass spectrometry of the crude product shows the molecular ion peak is 162.1, which is the largest fragment in the mass spectrum (Figure 4) and corresponds to the molecular weight of methyl trans-cinnamate (Table 1). The base peak is 131, inferring the fragment lost is 31 m/z in size. This 31 m/z matches the OCH3 fragment of the ester, and would not result from a trans-cinnamic acid. This is evidence the product was successfully

Through the extraction process, the mixture was separated into its pure benzocaine and benzoic acid portions. This could be proven by matching the melting points of the substituents obtained at the end of the lab to the average melting points found in several chemistry databases. In other words, the melting points of the purified benzocaine and benzoic acid compounds (93.2˚C and 131˚C, respectively) reflect a similar melting points to the documented 89˚C and 122.41˚C of the pure compounds found in nature. Although, the results was collected smoothly, the possibilities of errors are still existent. One source of error could aroused when light brown clouding forms at the interface of the two layers during acid extraction of benzocaine.

There was a lack of an OH peak for methyl benzoate spectrum, which was good because it supports the idea that this IR spectrum was for the desired product. There was a carbonyl peak at 1717.1 for the student outcome of methyl benzoate, which was probably representative of the ester group in the product. Lastly, there were a few peaks from 3064.3-2840.9 that corresponded to the methyl hydrogens and the aromatic hydrogens: they were represented

This appearance does not have any negative implications though. The experiment was carried out smoothly with no errors. Nevertheless, some mass could have been loss during the heating or during the transfer of the crystals into a vacuum filtration apparatus. When the dried crystals were collected from the Buchner funnel, some product was also lost. The loss of crystals was not significant though, as a decent percentage was found for the percent yield.

The weight of 2-methyl-2-butene recovered was 1.056 grams, so in finding percent yield I divided the two: (1.056)/(1.4) x 100 = 75.4%. For the second part of the experiment we used .20 moles of KOt-Bu and 0.02 moles of 2-methyl-2-bromobutane, again making 2-bromo-2-methylbutane the limiting reagent. In calculating the theoretical yield: (0.02 moles)(70.13 g/mol) = 1.4 grams. The weight of the major product (2-methyl-1-butene) recovered was 1.299 grams, making the percent yield: (1.299)/(1.4) x 100 =

Introduction Research in chemistry incorporates both microscopic and macroscopic properties. Essential to the properties compounds have both molecularly and environmentally is the ions and metals that make up many compounds. The properties of these chemicals depend heavily on the atoms that make up each particular chemical. Whether the compound is monoatomic, polyatomic, or even a polymer, being able to identify a compound is an essential tool in being able to make predictions and assumptions about the properties a specific chemical may have. Take for example the research being done on phosphorous and fluorine during World War II in Germany and during the Cold War which were able to be used as weapons, or during the early 1930’s when Germany

Purpose/Introduction The process of recrystallization is an important method of purifying a solid organic substance using a hot solution as a solvent. This method will allow the separation of impurities. We will analyze Benzoic Acid as it is dissolved and recrystallized in water and in a solvent of Methanol and water. Reaction/Summary

Abstract The unknown concentration of benzoic acid used when titrated with standardized 0.1031M NaOH and the solubility was calculated at two different temperatures (20◦C and 30◦C). With the aid of the Van’t Hoff equation, the enthalpy of solution of benzoic acid at those temperatures was determined as 10.82 KJ. This compares well with the value of 10.27KJ found in the literature.

The total amount of AlCl3 in the final product was 7.37 grams. 7.37 grams was found by subtracting the mass of the Erlenmeyer flask without the product from the mass of the Erlenmeyer flask with the product. Using Stoichiometry, the isolated product was calculated to be 73.5%. The complete sheet of work validates the calculation of the percent for the isolated