BROMINATION OF BENZENE
SYNTHESIS AND PURIFICATION OF BROMOBENZENE: PROCEDURE
DATA TABLE
Chemical Boiling point C Melting Point C Density g/mL Solubility
Benzene 80.1 5.5 0.88 Slightly in H2O
Toluene 110.6 -93 0.87 Slightly in H2O
Bromobenzene 155-156 -30.8 1.50 Insoluble
Dibromobenzene 220.40 87.31 0.96 Insoluble
MATERIALS:
Graduated cylinder
Weight scale
Buchner funnel
Filter flask
Rubber stopper
Hot plate
Thermometer
Conical funnel
Various size beakers
Fractionating column (for reflux)
Various sized round bottom flasks
Distillation head
Condenser
Vacuum adapter
Clamps and stands
Test tubes
PROCEDURE:
Pre Lab:
The experiment should be carried out AWAY from the sunlight. Before beginning the experiment, we need to make sure that the benzene used in the experiment is free of toluene and water. To do this, we must put anhydrous calcium chloride into a flask o...
Solid A was identified to be sodium chloride, solid B was identified to be sucrose, and Solid C was identified to be corn starch. Within the Information Chart – Mystery White Solid Lab there are results that distinguishes itself from the other 4 experimental results within each test. Such as: the high conductivity and high melting point of sodium chloride, and the iodine reaction of corn starch. Solid A is an ionic compound due to its high melting point and high electrical conductivity (7), within the Information Chart – Mystery White Solid Lab there is only one ionic compound which is sodium chloride, with the test results of Solid A, it can be concluded that is a sodium chloride. Solid B was identified as sucrose due to its low electrical
In a small reaction tube, the tetraphenylcyclopentadienone (0.110 g, 0.28 mmol) was added into the dimethyl acetylene dicarboxylate (0.1 mL) and nitrobenzene (1 mL) along with a boiling stick. The color of the mixed solution was purple. The solution was then heated to reflux until it turned into a tan color. After the color change has occurred, ethanol (3 mL) was stirred into the small reaction tube. After that, the small reaction tube was placed in an ice bath until the solid was formed at the bottom of the tube. Then, the solution with the precipitate was filtered through vacuum filtration and washed with ethanol. The precipitate then was dried and weighed. The final product was dimethyl tertraphenylpthalate (0.086 g, 0.172mmol, 61.42%).
This experiment was conduct to investigate the fluorescent behaviour of Leucophor PAF and to investigate the quenching of QBS with NaCl. It was found that the Leucophor PAF indeed satisfied the characteristic to act as whitening agent. It was also found that the quenching of QBS with NaCl was a diffusion-controlled collision process.
At this point the identity of the unknown compound was hypothesized to be calcium nitrate. In order to test this hypothesis, both the unknown compound and known compound were reacted with five different compounds and the results of those reactions were compared. It was important to compare the known and unknown compounds quantitatively as well to ensure that they were indeed the same compound. This was accomplished by reacting them both with a third compound which would produce an insoluble salt that could be filte...
In a separate beaker, acetone (0.587 mL, 8 mmol) and benzaldehyde (1.63 mL, 16 mmol) were charged with a stir bar and stirred on a magnetic stirrer. The beaker mixture was slowly added to the Erlenmeyer flask and stirred at room temperature for 30 minutes. Every 10 minutes, a small amount of the reaction mixture was spotted on a TLC plate, with an eluent mixture of ethyl acetate (2 mL) and hexanes (8 mL), to monitor the decrease in benzaldehyde via a UV light. When the reaction was complete, it was chilled in an ice bath until the product precipitated, which was then vacuum filtrated. The filter cake was washed with ice-cold 95% ethanol (2 x 10 mL) and 4% acetic acid in 95% ethanol (10 mL). The solid was fluffed and vacuum filtrated for about 15 minutes. The 0.688 g (2.9 mmol, 36.8%, 111.3-112.8 °C) product was analyzed via FTIR and 1H NMR spectroscopies, and the melting point was obtained via
The esterification procedure was performed first. To begin the lab, the heating mantle was set at the 6 setting, and the hot plate heat was turned on to low. In a round bottom flask, 6.1 g of benzoic acid and 21 mL of MeOH were added into the flask. Once this was added to the flask, 2 mL of sulfuric acid was added and poured carefully down the side of the flask. It was noted that after the addition of the sulfuric acid there was heat production in the flask. The contents were swirled and a boiling chip was added into the flask. The flask was connected to the hood by a clamp. Water was then ran through the condenser and connected to the round bottom flask to begin refluxing the contents in the flask. The mixture was gently heated at reflux for one hour.
Ensure gloves are worn at all times when handling strong acids and bases within the experiment of the preparation of benzocaine. 4-aminobenzoic acid (3.0g, 0.022 moles) was suspended into a dry round-bottomed flask (100cm3) followed by methylated sprits (20 cm3). Taking extra care the concentrated sulphuric acid of (3.0 cm3, 0.031 moles) was added. Immediately after the condenser was fitted on, and the components in the flask were swirled gently to mix components. It should be ensured that the reactants of the concentrated sulphuric acid and the 4-aminobenzoic acid were not clustered in the ground glass joint between the condenser itself and the flask. In order to heat the mixture to a boiling point, a heating mantle was used and then further left for gently refluxing for a constituent time of forty minutes. After the duration of the consistent forty minutes the rou...
Investigate how the concentration of hydrochloric acid effects the rate at which it reacts with calcium carbonate
Polman, H., Orobio De Castro, B. & Van Aken, M. A.G. (2008). Experimental Study of the
The procedure for this experiment can be found in Inorganic Chemistry Lab Manual prepared by Dr. Virgil Payne.
Additional credit is given...for their contributions from the dorm tap water, and the house tap water. Also, for their data given from the same lab procedure.
The Effect of Temperature on the Rate of Reaction Between Hydrochloric Acid and Calcium Carbonate
All things, living or nonliving, consist of atoms and molecules. These particles are constantly in motion, and this continuous motion allows for the disbursement of molecules, or diffusion. The overall net movement of these molecules will go from areas of higher concentration, to areas of lower concentration. Therefore, following a concentration gradient (Martini). The rate of diffusion of these molecules, in accordance with Fick’s law of diffusion, is directly proportional to the concentration gradient present. However, the concentration gradient is not static and will change over time and with distance, therefore changing the rate of diffusion. It is hypothesized that the two solutions being tested, Methylene Blue and Potassium Permanganate, will begin their initial diffusion in the agar gel at a quick rate, and then progressively regress over the allotted time of 1 hour. Another factors other that will have an effect on rate of diffusion is molecular size. There is a substantial difference in molecular weight between Methylene Blue (320 g/mol) and Potassium Permanganate (158 g/mol). The combined molecules present in Potassium Permanganate are lighter than those in Methylene Blue, and therefore should allow it to diffuse more rapidly.
In this experiment, the calcium carbonate was in the form of marble chips. The calcium carbonate reacted with hydrochloric acid when the acid was poured into marble chips. Due to calcium carbonate’s higher reactivity, it displaced hydrogen in the hydrochloric acid. As a result, products of calcium chloride, carbon dioxide and water were formed. As the chemical reaction occurred, the water in the measuring cylinder was displaced and gas bubbles that were blowing out represented carbon dioxide.
The aim of this experiment was to investigate the affect of the use of a catalyst and temperature on the rate of reaction while keeping all the other factors that affect the reaction rate constant.