Does Nitric Acid Affect The Synthesis Of Nitroacetanilide

In experiment two, 1.48g of the unknown solid was recovered. From this mass, it was determined approximately 30mL of boiling water was needed for crystallization of acetanilide and about 121mL for phenacetin. Phenacetin would require more solvent because it is less

Data Table 2 shows the results gathered after the purification of 3-nitrochalcone. Since only half of the crude product was used, the theoretical yield for the crystallized product was determined to be 2.1 g. This led to a percent yield of 39%. The melting point of the crystallized product was also determined to be 142℃, which differed slightly from the literature value of 146℃. As a result, the product, 3-nitrochalcone, was not completely pure. It probably contained water and alcohol, because any impurities would have lowered the melting point. Considering the fact that the crude product was not thoroughly dried before purification, water and ethanol were already in the product. Even after crystallization into “pure 3-nitrochalcone”, the product was also not completely dried. The yield should have been much lower than 39%. If the product is not allowed time to dry, not only water, but methanol, which was the solvent that was used to crystallize the crude, would be in the product. Both the crude and crystallized 3-nitrochalcone were analyzed by infrared spectroscopy to test and prove these

In addition, the diethyl ether solution was decanted into the round bottom flask (50 mL). Afterwards, the washed Na2SO4 and the Erlenmeyer flask with additional diethyl ether (5 mL) was added to the round bottom flask, mentioned earlier. Later, the round bottom flask was placed in the rotary evaporator. In addition, the acetanilide flask and 3-chlorobenzoic acid was weighed and tared to determine the mass. Not to mention, the mass-% of 3-chlorobenzoic acid and acetanilide was calculated. Lastly, the melting points of acetanilide and 3-chlorobenzoic acid was

The synthesis of acetaminophen involves the attraction of the electrophilic carbonyl group of acetic anhydride to the nucleophilic NH2

The solution that was performed in this experiment was to use sulfuric acid in order to form a protonated alcohol, so when the halogen or nucleophile back attacks the compound, water is displaced. Once the alcohol is protonated, the solution reacts in either an SN1 or SN2 mechanism.

The pipet was put into the top of the condenser and leaving no open spaces. The vacuum served to get rid of the nitrogen oxide gases that were formed during the oxidation reaction. The solution was heated for 30 minutes, beginning the time when the first sign of nitrogen oxide fumes were observed. After the 30 minutes, the solution was removed and cooled for a few minutes. The solution turned was a brownish-yellow color and all the crystal were dissolved, leaving a liquid. The solution was then transferred, using a Pasteur pipet, to 3 mL of water in a beaker. The reaction flask was rinsed to remove the remainder of the solution. The solution was stirred with a glass rod until room temperature of the solution was achieved. A yellow solid was to form, but instead the solution remained aqueous in the case of the specific experiment explained here. With additional scraping of the solution with a glass rod, no crystals formed at all. The next procedure, if the crystals had formed was to crush the solid with the glass rod and filter the solid until the crystals were dry. The mass would then be weighed and the crystals were to be recrystallized with 95% ethanol. The crystals were to be cooled in ice water to get full crystallization and then the crystals were to be filtered and air dried, then weighed.

The colorless solution was poured into a beaker containing 10mL of chilled water, after the designated time, to initiate recrystallization for 5-10 minutes. 9. The nitrated methyl benzoate solution was then poured onto the filtrating apparatus and left to dry for 10 minutes. 10. The white, dried crystals were weighed and dissolved in ethanol then filtrated again and

The solution was subsequently arranged into a reflux apparatus which included a wet paper towel in order to prevent vapor loss. The solution was refluxed at a temperature ranging from 180°C-185°C for thirty minutes via sand bath. The contents of the micro-test tube were then cooled to room temperature followed by an ice bath in order for crystals to form. The crystals were then collected via suction filtration using a Hirsch funnel. The product was washed with ice-cold xylene (3

2.0mL of benzaldehyde and 0.76mL of acetone were added into a test tube and slowly added to the Erlenmeyer flask, while in the ice bath and being swirled. 5. After 30 minutes of swirling in the ice bath, the mixture was vacuum filtrated so the crystals within the mixture were on the filter paper. 6. Water was added onto the vacuum filtration, where the crystals were, to clean the crystals of any bases.

An ice bath was prepared in a large beaker and a small cotton ball was obtained. 0.5 g of acetanilide, 0.9 g of NaBr, 3mL of ethanol and 2.5 mL acetic acid was measured and gathered into 50mL beakers. In a fume hood, the measured amounts of acetanilide, NaBr, ethanol and acetic acid were mixed in a 25mL Erlenmeyer flask with a stir bar. The flask was plugged with the cotton ball and placed in an ice bath on top of a stir plate. The stir feature was turned on a medium speed. 7mL of bleach was obtained and was slowly added to the stirring flask in the ice bath. Once all the bleach was added, stirring continued for another 2 minutes and then the flask was removed from the ice bath and left to warm up to room temperature. 0.8mL of saturated sodium thiosulfate solution and 0.5mL of NaOH solution were collected in small beakers. The two solutions were added to the flask at room temperature. The flask was gently stirred. Vacuum filtration was used to remove the crude product. The product was weighed and a melting point was taken. The crude product was placed into a clean 25mL Erlenmeyer flask. A large beaker with 50/50 ethanol/water

Once cooled, the mixture was then transferred to a separatory funnel using the funnel while avoiding adding the boiling chip. 10 ml of water was then added to the mixture. The mixture was gently shaken and the phases were allowed to separate. The funnel was then unstopped and the lower aqueous phase was drained into a beaker. 5 ml of 5% aqueous NaHCO3 was added and then shaken gently. A great deal of caution was taken into consideration because of the production of carbon dioxide gas which caused pressure to develop inside the funnel. The pressure needed to be released so the funnel was vented frequently. The phases were allowed to separate and the lower aqueous phases was drained into the beaker. After draining, 5 ml of saturated NaCl was added to the funnel and then shaken gently. Once again, the phases were allowed to separate and the lower aqueous phase was drained into a beaker. An ester product was produced and was transferred into a 25 ml Erlenmeyer flask. This organic product was then dried over anhydrous Na2SO4 to trap small amounts of water in its crystal lattices thus removing it from the product. Finally the ester was decanted, so that the drying agent was excluded from the final product.

Crystals were collected in a Buchner funnel, washed with alcohol, then ether, then transferred into a sample tube for storage.

The ether extracts is rinse twice with 10mL of water and dry over K2CO3. 7) Transfer the dried and filtered solution to oil after evaporate and rinse into a 50 mL Erlenmeyer flask. B: Synthesis of α-Chloro-2,6-dimethylacetanilide 1) Add 50mL of glacial acetic acid and 7.2 g (or 5.2 mL) of chloroacetyl chloride to every 7 grams of dimethylaniline from the previous step. 2) Warm the solution on a water bath at (40–50)ºC. After remove, add 1 gram of sodium acetate in 100 mL of water. 3)

An Erlenmeyer flask was used to accommodate the largest volume of recrystallization solvent calculated and was cooled in an ice bath to increase the yield of crystals. The solid was collected by vacuum filtration and washed with a small amount of ice water. The product is then dried to a constant mass by use of an oven and weighed. A small amount of the unknown was compared to two samples of acetanilide and phenacetin for a melting point range to determine the identity. The temperature of the unknown was recorded when the first trace of liquid can be seen and when the unknown was completely liquid.

The recrystallization technique utilizes the ability of a compound to dissolve within a hot solvent and produce a solution. As this solution cools, the solute reforms without impurities in a crystal lattice structure.1 For this to work properly, an appropriate solution that will not dissolve the solute at low temperatures, but will at high temperatures, must be used.1 There is no single solvent that will work well for every solute’s recrystallization; different solvents are better suited for some solutes than others.2 Some impurities that do not dissolve within the solvent can be filtered out while the solution is still hot, while other impurities that readily dissolve within the solvent shouldn’t recrystallize with the pure substance (as they are not concentrated enough to