Cinnamic Acid Lab

1. The experiment began with a clear solution of sodium benzoate, once 3 M of HCl were added to achieve a pH of 2, the clear solution became a precipitate. Sodium benzoate was water soluble, but the yield of benzoic acid became quite insoluble in water.

What is the stereochemistry for the bromination of trans-cinnamic acid, and how is it formed?

A few crystals of potassium iodide was added to the flask and then swirled to dissolve the solid potassium iodide. The volume of the liquid in the buret was read. The liquid in the buret was titrated with the thiosulfate solution until the brown color of iodine had disappeared. Afterward, 1 mL of starch solution and then thiosulfate solution was added until the blue color of the starch-iodine complex disappeared. The volume of the liquid in the buret was read again. Also, a large test tube was cleaned and dried. 50 mL of iodine solution was carefully measured with a 25 mL graduated cylinder. Next, 5.0 mL of cyclohexane was measured and added to the graduated cylinder. The test tube was stoppered with a rubber stopper. The mixture was shook for one minute at first, then for about five minutes. The process was repeated, where the 50 mL of iodine solution in a 25 mL graduated cylinder was obtained, and then a second 50 mL of iodine solution and 8.0 mL of cyclohexane was added. Next, the cyclohexane layer was removed with a Pasteur pipet from the first test tube into a beaker. In addition, 25.0 mL of the water layer was poured into a clean,

Sodium benzoate was found in the aqueous layer and methylene chloride was added to separate the immiscible layers. Once separated, and all the organic and soluble layers were combined separately, the crude samples were heated. After crystals were formed, they were weighed to find our actual yield. Acetanilide had a percent yield of 74% and Benzoic acid had a percent yield of 54%, Table 1. The results showed that there was a higher percentage of Acetanilide

Each sample of the substances was placed in separate test tubes containing 8 mL of distilled water and mixed with a stirring rod. Within seconds,

A. Figure 1: Standard curve of the phosphate concentrations and the absorbance values. This curve shows the amount of light that is absorbed by the reaction of water with 1 mM phosphate in six different test tubes, containing different volumes of water and phosphate in each tube. Tube 1 contained 1 mL of water with 0 mL of phosphate, tube 2 had 0.8 mL of water with 0.2 mL of phosphate, tube 3 consisted of 0.6 mL of water with 0.4 mL of phosphate, tube 4 had 0.4 mL of water with 0.6 mL of phosphate, tube 5 had 0.2 mL of water with 0.8 mL of phosphate, and tube 6 had 1 mL of phosphate with no water present. After all of the solution was added to the test tubes, 2.5 mL of stopping reagent was added to each test tube in order to denature the enzyme and stop the reaction. After 10 minutes, the absorbance was measured at 620 nm; which are the values used to create this curve based on phosphate concentration.

“Acid/Base” lab’s purpose was to introduce extractions of one of the four neutral organic compounds (4-chlorobenzophene, biphenyl, trans-stilbene, and trans-chalcone). We then were asked to test the solubility of our selected neutral compound with hexane, water, methanol, and ethyl acetate to find the solvent that only dissolved the neutral compound while introduced to heat. Once the solvent was chosen, we purified the compound by recrystallization, and then concluded that my neutral organic compound was trans-stilbene.

This is an experimental lab that tested how well an antacid acid tablet will dissolve in excess stomach acid. The lab can help the creators and consumers of the drug with know how efficient the drug is. Each group got a certain antacid acid tablet to test. The lab utilizes back titration to help with figuring out the amount of hydrochloric acid(HCl) that is dissolved by an antacid acid by introducing a base with a known molar concentration. The tablet effectiveness was tested by seeing how much strong base (Sodium Hydroxide-NaOH) is needed to be added to a strong acid solution (HCl and antacid acid tablet) for a color change. A color change means that the acid solution became basic, so enough base was added to neutralize the acid. The results

The results of all three concentrations all increased with time. The 30 percent concentration resulted in 2.08g at ten minutes, 3.14g at 20 minutes, 4.10 at 30 minutes, 5.11g at 40 minutes, 6.18g at 50 minutes, 6.97 at 60 minutes, 7.78 at 70 minutes, 8.42 at 80 minutes and 8.87 at 90 minutes. You can see all these results and data for 30 percent concentration in table xxx. Making the osmotic rate for 30 percent concentration 0.095g/mL. For the 20 percent concentration, at 10 mintues is was 0.60g, 0.93g at 20 minutes, 1.44g at 30 minutes, at 40 minutes is was 1.95g, 2.34g at 50 minutes, 2.60g at 60 minutes, 3.02g at 70 minutes, 3.44g at 90 minutes, and 3.38 at 90 minutes. The data for 20 percent concentration equals to a osmotic rate of 0.039g/mL.

In the reactions studied, equilibrium is often reached quite slowly, and so a catalyst (HCl) was used to increase the reaction rate. This acid was present in high enough concentrations to affect the value of the equilibrium constant of the total reaction, but its effects were consistent enough between reactions that the approximate value of the equilibrium constants are still valid.

The control (5.00g of tert-butanol) began at a temperature of 50.8 °C and rose to a maximum of 60.3 °C and ended at a temperature of 21.8°C. The first experimental trial (test tube with 5.00g of tert-butanol and 0.306g of Benzoic acid) began at a temperature of 51.4°C and rose to its maximum of 83.9°C and ended at a temperature of 15.9°C. The second experimental trial (test tube with 5.00g of tert-butanol and 0.612g of Benzoic acid) had similar results to the first experiment trial but varied slightly. It started at a temperature of 55.7°C and had a maximum of 84.0°C and finally ended at 12.0°C. The final experimental trial (test tube with 5.00g of tert-butanol and 0.386g of Camphor) began at a temperature of 57.2°C and rose to a maximum temperature of 85.3°C and finally ended at a temperature of 12.3°C.

Day 1 and day 2 of the lab had a total of six parts: interpreting structures, roamers, recognizing isomers, conformation of cyclohexane, symmetry in chemistry and functional groups. By completing the different parts, I learned different and more complex things about organic chemistry.

The mixture was boiling for 10 minutes until the solids were dissolved, and cool it to room temperature. Then, we refluxed the isolate maleic acid, 0.3ml water, and 0.25ml of concentrated of HCL for around 30 minutes. A solid was formed from the hot solution, it was collected by a Hirsch funnel, and then dry it for

The experiment conducted by scientists, Mona Howell and Emily Yau, portrayed a variety of unexpected results. The hypothesis was made that our seeds that were microwaved for 5, 10, and some of the 15 second seeds will grow, the seeds that were microwaved for 20, 30, and 60 seconds will not sprout because the radiation will kill the seed, and the radish seeds in the 1 and 2 teaspoons will sprout. However, some of our hypothesis was proved wrong because during our radiation experiment during trial 2, some of the seeds that were microwaved for a minute even grew. On the other hand, during our acidity experiments, our hypothesis was correct proving that too much acidity damages the dominant seed. A total of three trials were held for each experiment,

The resulting Ca(OH)2 solid was filtered from the NaCl liquid. The NaCl was then tested, in equal proportions, with NaOH and CaCl2 to determine the excess reagent and the limiting reagent. As different amounts of CaCl2 were added, the expected results did not match the actual results. This could be due to a number of errors in conducting the experiment such as inaccurate measurements. One point where the data does slightly reflect the expected outcomes is in the mass of precipitate recorded. These values do appear to plateau though the recorded values are much higher than the calculated ones. The actual yield did not reflect the theoretical yield accurately. Though both did increase, there is a significant difference between the values. From this experiment, concepts about reactions were learned including limiting and excess reagents as well as the disparities between actual data and experimental