The purpose of this laboratory experiment was to react methyl benzoate with nitric acid and identify the position of the substituted nitro group in the final product molecule. Methyl benzoate was added to cool concentrated sulfuric acid in order to amplify the directing effect of the nitro group addition, such that without the sulfuric acid the protonation would have happened at the carbon oxygen double bond. The mixing of concentrated nitric acid with concentrated sulfuric acid was to achieve Reaction 1 from Table 1, formation of the nitronium ion. Both of these reactions were kept at temperatures around 0°C, since they are exothermic reaction and presence of heat could lead to production of unnecessary dinitro by-products. The nitronium ion mixture was slowly added to the concentrated sulfuric acid methyl benzoate mixture to prevent vigorous reaction that if present could lead to unwanted dinitro by-products. The mixture after settling and heating to room temperature was poured over ice in order to rapidly cool the sample inducing formation of the crystals. The water was allowed to melt before it was vacuum filtered to neutralize the acid that might be remaining …show more content…
So, the first reaction Table 1.1 was the formation of the electrophile. The mixture of concentrated sulfuric acid and methyl benzoate served in order to create a resonance stabilized arenium ion intermediate. In this reaction the benzine ring is deactivated by the ester in the -COOCH3 meaning that the electrophile nitronium ion was added to the meta position to form methyl m-nitrobenzoate (Table 1.2). This is the major product due to the carboxyl and nitro group being very powerful electron withdrawing groups. This was confirmed by the melting point which ranged from 73-75°C while the literature meting point has a range of
After 28 minutes, the mixture stopped boiling, and approximately 4.5 ml of bromobenzene was added drop by drop in the mixture, and color of the mixture was turned light brown orange. Then, the phenylmagnesium bromide was cooled in ice bath for a few minutes, and 10 ml of anhydrous diethyl ether was added in the mixture by using the syringe. After that, approximately 2.3 ml of methyl benzoate was added to the reaction, and it was added slowly slowly because the reaction was exothermic which needed to be cool in order to maintain a gentle reflux. Once all the methyl benzoate solution was added, the heating mantle was removed from the reaction flask and was cooled to the room temperature. During the reaction, a milky white salt began to precipitate, and the reaction flask was swirled for ten minutes until most of the reaction became visibly subdivided.
To test for the presence of the ammonia cation, a scoop of the unknown compound was mixed with NaOH to see if the resulting solution had a noticeable smell that would affirm the presence of ammonia. A moist piece of pH paper was then held near the solution to see if the ammonium would dissolve the water on the pH paper. The next cation test performed was the flame test. A gram of the unknown compound was held by a metal stick above the flame of a Bunsen burner to see what color flame the compound would produce. The chart in the lab manual on page 63 was used to determine what cation correlated with what flame color.
1. Introduction The objective of the experiments was to determine the identity of an unknown compound in order to properly dispose it. The process of disposal is very important when dealing with chemicals. Some chemicals are very
Benzyne Formation and the Diels-Alder Reaction Preparation of 1,2,3,4 Tetraphenylnaphthalene Aubree Edwards Purpose: 1,2,3,4-tetraphenylnaphthalene is prepared by first producing benzyne via the unstable diazonium salt. Then tetraphenylcyclopentadienone and benzyne undergo a diels-alder reaction to create 1,2,3,4-tetraphenylnaphthalene. Reactions: Procedure: The reaction mixture was created. Tetraphenylcyclopentadienone (0.1197g, 0.3113 mmol) a black solid powder, anthranilic acid ( 0.0482g, 0.3516 mmol) a yellowish sand, and 1,2-dimethoxyethane (1.2 ml) was added to a 5-ml conical vial.
The reaction to synthesize benzocaine was known as a Fisher esterification reaction. The Fisher esterification was reaction between alcohol and carboxylic acid in the presence of acid. The reaction was used to form an ester. In the experiment, sulfuric acid acted as a catalyst and necessary for this reaction to occur. There was a change between the –OH group of carboxylic acid to an –OCH2CH3 group in the reaction.
The product obtained was (2S, 3R)-2, 3-dibromo-3-phenylpropanoic acid and (2R, 3S)-2, 3-dibromo-3-phenylpropanoic acid, which are enantiomers. This was determined through melting point analysis. The melting point range for the product was 198 to 202 degrees Celsius, which is a lot close to the given melting point of the anti-addition product, 202-204 degrees Celsius. The given melting point range was 93.5-95 degrees Celsius. Furthermore, the syn-addition product is unlikely and difficult to produce due to stereochemistry selectivity.
The purpose of this experiment is to perform a two step reductive amination using o-vanillin with p-toluidine to synthesize an imine derivative. In this experiment, 0.386 g of o-vanillin and 0.276 g of p-toluidine were mixed into an Erlenmeyer flask. The o-vanillin turned from a green powder to orange layer as it mixed with p-toludine, which was originally a white solid. Ethanol was added as a solvent for this reaction. Sodium borohydride was added in slow portion as the reducing agent, dissolving the precipitate into a yellowish lime solution.
Abstract: The purpose of this experiment was to identify given Unknown White Compound by conducting various test and learning how to use lab techniques. Tests that are used during this experiment were a flame test, ion test, pH test, and conductivity test. The results drawn from these tests confirmed the identity of the Unknown White Compound to be sodium acetate (NaC2H3O2) because there were no presence of ions and sodium has a strong persistent orange color. The compound then will be synthesized with the compounds Na2CO3 and HC2H3O2 to find percent yield.
Add 5-6 drops of sulfanilic acid & 5-6 drops of alpha-napthylamine to each broth. a) If you get a red color, then you can stop at this point. Because color change to RED indicates a “POSITIVE nitrate reduction test”. b) No color change that means no nitrite present. That will be possible because nitrate was reduces to nitrite, then nitrite was further reduced to some other molecules.
The yield of 3-nitrochalcone was 0.786 grams after filtration (percent yield of 62.04%). Multiple peaks were observed in the IR spectrum of 3-nitrochalcone at 1348.14 (N-O bond); 1593.33 (benzene ring); 1658.86 (unsaturated ketone). The carbon-carbon bonds are widely used in the drug industry to manufacture drugs and aldor condensation is used. Figure 1: Synthesis of 3-Nitrochalcone from 3-Nitrobenzaldehyde Source: cnx.org Figure 2: Mechanism Involved in the Synthesis of 3-Nitrochalcone Source: cnx.org
The possible explanations and changes to make are similar to the previous questions. Conclusion and Future Experiment 18. The identity of the product and unknown were 4-tert-butylbenzyl phenol ether and tert-butyl phenol respectively. The key to making this discovery was the melting point and TLC results!
It is understood the mechanism is acid-catalyzed where protons coordinate with the carbonyl oxygen to make the carbonyl carbon more electropositive for nucleophilic attack (Scheme 1). In the experimental procedure all reactants were added together, this is inefficient as the protons can coordinate with either trans-cinnamic acid or methanol. Coordination with methanol is unnecessary as it reduces its nucleophilicity and makes less protons available to coordinate with the carboxylic acid. To improve
In other lab procedures, benzoic acid is sometimes substituted for anisole in the Friedel-Craft acylation. However, the reason benzoic acid
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.