Panacetin And Hydrochloric Acid Synthesis Lab Report

1. The first experiment is Preparation of a Cobalt Amine Bromide Product ; Synthesis #3 was used to create the compound. Added 5 grams of cobalt carbonate to 20 mL of hrdrobromic acid in a beaker. Noticied a slight color change to dark purple. Solution frothed after it settled I mixed in 15mL water and

From the vial labeled “AE,” aspirin (0.533 g) was placed into a 50 mL Erlenmeyer flask with a boiling stick. Toluene (20 mL) was brought to a boil on a hot plate. The boiling toluene (10 mL) was then added to the aspirin until the solid dissolved completely. After allowing the solution to reach room temperature, the solution was placed in an ice bath for 16 minutes. After the crystals

Reaction 2 - 1.Used a Beral- type pipet, added about 2mL (40 Drops) of 1M hydrochloric acid solution to a small test tube.

The purpose of this experiment is to examine the stoichiometric relationship between reagents and the identity of the products by using three acid/base neutralization reactions of a triprotic acid, phosphoric acid, and varying molar equivalents of sodium hydroxide. The data will be used to determine the formula weight of the products and identify the remaining salt for all three reactions.

In this experiment, it is very important to ensure that the deionized water is just basic and not acidic in order to obtain accurate results. Calcium oxalate does not precipitate in an acidic solution because of the formation of H2C2O4-, an ion that does not precipitate with Ca2+ . Allowing the precipitate to settle is also very

Suppose a household product label says it contains NaHCO3. How would you test this material for the presence of sodium bicarbonate?

When boiling the water before placing it in the unknown, my water never actually came to a boil. It was steaming very heavily and I was losing a considerable amount of water, especially from my smaller beaker, so I had to just assume that it was hot enough. This may have affected the amount of material that I got to dissolve. Either way, the fact that it took 51mL was a good indicator that my unknown was phenacetin, due to phenacetin having a much lower solubility than acetanilide. I also noticed that even though I had put in more hot water than phenacetin should have needed to dissolve (45.9mL), white flakes still remained in the beaker. I assumed these to be impurities.

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

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 weight of each 50ml beaker (used for weighing the mass of dissolved Potassium chloride after the evaporation of water) should be recorded. If the experimenter were to weigh the mass of one beaker and take it as a default mass, the latter may be a source of error.

3. a. The first error will be when transferring the benzoic acid from the weigh paper to the vial. The benzoic acid is spilled. Then, the second one will be when pipetting and transferring the methylene chloride because I might spill some of the methylene chloride. The third one will be when pipetting the two layers, either I could not pipet all of the bottom layer or I accidentally pipet the top layer.

Benzyltriphenylphosphonium chloride (0.201g) and 9-anthraldehyde (0.116g) were weighed and added to a short-neck round-bottomed flask (5ml). Dichloromethane (2ml) was measured using a measuring cylinder and added to the

Determine the weight of the water by subtracting the weight of the vial with water by the weight of the vial on its own.

The process was then repeated for the second reaction but using 1.00-mL of a 6.00-M phosphoric acid solution and 4.00-mL of a 3.00-M sodium hydroxide solution.

5. Part B.1. Eliseo couldn't find the 6 M HCl and so used 6 M HNO3 for testing the metals instead. His logic? Both are strong acids. Explain how the results of the experiment would have been different.