Release of Aspirin from a Polymer Matrix

Next, aspirin was extracted from the filtrate. When the filtrate was first mixed with the sodium hydroxide and inverted a couple times, an organic layer formed underneath an aqueous layer in the separatory funnel. Dichloromethane was present in the organic layer because it has a higher density than sodium hydroxide, therefore, it’s in the bottom layer. Aspirin reacts with bases like sodium hydroxide, and it forms the salt sodium acetylsalicylate. The polar salt molecules migrate from the organic layer, where they are insoluble, to the aqueous layer, where they are soluble. After the two layers were separated into two different containers, the aqueous layer, which contained sodium acetylsalicylate, was mixed with hydrochloric acid. A white, cloudy precipitate formed, which was a purer form of the salt. The HCl

3ml of sample was taken first flask at 4 minutes and added to the appropriate tube of sodium hydroxide, from the second flask at 4.5 minute and so on, each flask was sampled at 30 second intervals. The sampling was then repeated starting at 8,12,16 minutes. The final sample from the last flask was taken at 18.5 minutes. Once the sampling was completed, measurements of absorbance were obtained for solution in each tube at 405 nm.

An automatic pipet was used to measure 0.450 mL water and 0.165 mL acetic anhydride and was added to the conical vial. A spin vane was placed into the vial and an air condenser was attached.

In determining the melting point range of the aspirin, a capillary tube (sealed at one end) was one-third-filled with the dried aspirin. The capillary tube and a thermometer were immersed in an oil bath. The temperature at which the solid started to melt and the temperature when the entire sample was completely liquefied were recorded as the melting point temperature range.

Both Aspirin and the Unknown are soluble in dichloromethane, due to their non-polar characteristics. To separate the two components, sodium bicarbonate was added (see figure 3). Sodium bicarbonate reacted with aspirin and converted it to a salt, also forming water and carbon dioxide. It was observed that the solution "fizzed" when this reaction took place, showing the release of carbon dioxide. The newly formed salt then traveled to an aqueous layer where it was soluble, while the unknown remained in the dichloromethane layer. The two layers were then separated. To collect an aspirin solid, the combination of the addition of HCl and the process of vacuum filtration helped to break down the salt and form a solid. Then the solid was placed in the Fisher Scientific Biotemp Oven to dry it to a constant mass of 0.091 g, 32.97% of the total composition. The

We made sure the solution is strongly acidic by testing it with litmus paper getting a pH of 2. We then cooled the mixture to room temperature swirling the flask occasionally in an ice bath. We collected the aspirin by vacuum filtration and washed the aspirin on the filter with cold distilled water. We let it air dry for 30-35 minutes and then weighed the aspirin. It weighed out at 0.513g. The unknown component was calculated and weighed at 0.738g.

Not all of the aspirin will be converted to sodium acetylsalicylate, so it will instead remain in the organic layer and be weighed with the unknown. Therefore, the reported weight of aspirin will be too low, while the unknown will be weighed too high.

Aspirin is one of the most consumed painkillers created up to this date due to its reliability and low expense. It is often used to relieve minor aches and pains, reduce fever and as an anti-inflammatory medication. Due to its wide range of uses, the demand for this pharmaceutical is very high. As a result, manufacturers who produce this drug must be efficient in order to reduce the time taken to produce this drug and produce the in very high quantities.

The filter paper, holding the aspirin crystals, was removed from the funnel and was left to dry before being weighed. Once the aspirin crystals were weighed, the theoretical yield and the percent yield of the experiment were calculated. The procedure was repeated once more using the same steps.

Introduction: The goal or purpose of this experiment was to determine the concentration of Allura Red in red commercially available beverage- Gatorade. Colorimeter are used to shine a LED light through the solution and hit a photocell: it will detect an absorbance or a percent transmittance value. These “value” can be charted and examined as a calibration curve. Calibration curve is a method for determining a substance concentration in an unknown sample

In order to test the predictions of the hypotonic, hypertonic, and isotonic hypothesis for the solution  made during the study,  four samples of sucrose were taken and placed into two different beakers each containing a different concentration. Beaker 1 is  250- mL and contained 150-mL of 10% sucrose with dialysis tubing A, while beaker 2 (a large bowl) contained 1% sucrose, with dialysis tubing  B, C, and D. Tubing A contained 10-mL with 1% sucrose. Tubing B

In this experiment, 0.31 g (2.87 mmol) of 2-methylphenol was suspended in a 10 mL Erlenmeyer flask along with 1 mL of water and a stir bar. The flask was clamped onto a hotplate/stirrer and turned on so that the stir bar would turn freely. Based on the amount of 2-methylphenol, 0.957 mL (0.00287 mmol) NaOH was calculated and collected in a syringe. The NaOH was then added to the 2-methylphenol solution and allowed to mix completely. In another 10 mL Erlenmeyer flask, 0.34 g (2.92 mmol) of sodium chloroacetate was calculated based on the amount of 2-methylphenol and placed into the flask along with 1 mL of water. The sodium chloroacetate solution was mixed until dissolved. The sodium chloroacetate solution was poured into the 2-methylphenol and NaOH solution after it was fully dissolved using a microscale funnel.

In order to assimilate diffusion through a permeable membrane potassium permanganate and methylene blue were used in experiment. The objective was to compare the rates at which the liquid compound of different molecular weight diffused through agar. This was achieved by obtaining agar in a petri dish with two wells to hold the liquid compounds. The rate was measured by time and diameter distance diffused. This process was observed for 60 minutes at 15 minute intervals.

2. The different concentrations of ONPG solutions and buffer solutions were incubated in the water bath at 37°C for 5 minutes.

In Figure 3.1 where the partial rates of diffusion of each substance was plotted at a three-minute intervaland also in Figure 3.2 where the comparisons are seen, Potassium Permanganate increased after three minutes ahead and remained its value until the sixth minute and it remained constant, Potassium Dichromate increased at the sixth minute and retained its increase until the ninth minute and then remained constant, while Methylene blue remained constant all throughout in the 30 minutes span of time. Although the average rate of diffusion calculated in Table 2 show no difference in Potassium Permanganate and Potassium Dichromate, as seen in Figure 3.1 and Figure 3.2, Potassium Permanganate diffused the faster in the first six minutes of diffusion than