Simple Distillation Of Toluene And Ethyl En

Objective: The main goal of this lab is to learn how separation of binary liquid mixtures is performed. Especially when the two liquids have boiling points varying by about 30° C. Hexane can be separated from toluene in this experiment because of the difference in their boiling points. Since toluene has a higher boiling point, it will left at the bottom while the hexane starts to boil out and collect in the Hickman still. GC measurements help us in determining how accurate our data is by making a graph of the amount of hexane and toluene in each fraction. Also this lab gives experience with semi-micro

Discussion The purpose of this experiment was to produce ethanol through fermentation of sucrose. Once the solution had fermented for a week, it was subjected to fractional distillation to remove the ethanol from the supernatant. As seen in Table 1, while the first fraction contained a moderate concentration of ethanol, the second and third fractions did not contain any ethanol at all. This can be attributed to the fact that there was little to no ethanol in the supernatant obtain from the fermentation solution.

Perform the following with three 0.05g samples of unknown and the following solvents: methanol, water and toluene

First. We weight the 10-ml graduated cylinder and record the data for 37.87g. Then put 5ml isopentyl alcohol and weight it with the 10-ml graduated cylinder for 41.94g. So, we get the isopentyl alcohol weight is 4.07g. Then, we also weight 7ml glacial acetic acid and put it into the 10-ml graduated cylinder. We add 1-ml sulfuric acid and put it into the 10-ml graduated cylinder too. After we mix all of the liquid, we put a boiling stone in the flask. Next, we good connection device like the picture. Then heating under reflux. Before reflux, we should check it. First, we should wait until the liquid began to boil and the color was changing to brown. Then, continue to heat for 75 minutes. After 75 minutes, we stop it. And we need to cool the liquid to the room temperature. Then we ready 10ml ice water to cool the liquid. After cooling it, we put the liquid in the separatory funnel. And we should add 5ml saturated aqueous sodium to separate it. After first separate it. Then add 5ml saturated aqueous sodium chloride to separate it. Then transfer the liquid to a 25-ml round-bottom flask. After one week, we first weight the sample mass. Then put our sample to another group’s graduated cylinder. And weight the combine mass. Then put the sample into a distillation unit. To begin the distillation and record the boiling point range. And we should also weight the mass after distillation. We can calculate the percentage yield.

The purpose of this lab was to see how certain substances; Naphthalene, Toulene, and and 2 unknowns (one liquid, one solid) react with 3 different solvents. To identify the two unknowns, testing needs to be done to find the density of both the liquid and the solid, determine the melting point of the solid, and the boiling point of the liquid. The Physical Properties of Pure Substances Table can then be used to compare the observed results with the accurate properties from the table. If testing is done correctly, accurate assumptions can be made to figure out what the unknown substances were.

The next step in this lab is to rinse the Erlenmeyer flask with distilled water down the drain and then repeat the experiment, this time adding 10 ml of 0.10M KI and 10 ml of distilled water to the flask instead. The flask should again be swirling to allow the solution to succumb to the same temperature as the water bath and once it has reached the same temperature, 10 ml of 3% H2O2 must then be added and a stopper must be immediately placed on the flask and recording should then begin for experiment two. After recording the times, the Erlenmeyer flask must then be rinsed again with distilled water down the drain. After rinsing the flask, the last part of the lab can now be performed. Experiment three is performed the same way, but instead, 20 ml of 0.10 ml M KI and 5 ml of distilled water will be added and after the swirling of the flask, 5 ml of 3% H2O2 will be added. After the times have been recorded, data collection should now be complete.

The purpose of the experiment was to distill cyclohexane from the toluene using to methods: simple distillation and fractional distillation. Distillation is a technique used to purify volatile liquids. Distillation involves boiling the impure liquid, condensing the vapor, and collecting pure fraction of the liquid. The mixture is heated to its boiling point where the liquid is converted into vapor, and once the boiling points are different the components can be separated by distillation.1 Fractional distillation can be effective when trying to separate volatile experiments that have similar boiling points. Fractional distillation can complete many simple distillations in one apparatus. A distillation column was used in the fractional distillation

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

The table shows the temperature Vs. volume for both the simple and fractional distillations of Cyclohexane and Toluene Graph 1 Graph one. This graph shows temperature Vs. volume of both simple and fractional distillations of Cyclohexane and Toluene. This graph also shows the boiling points of the two liquids allowing a person to see where both liquids start and

Distillation is the process of which liquid is changed into it’s vapor state which in turn is changed by condensing the vapor back to the liquid state. This process is used to separate and purify liquids. The process begins a distillation apparatus. After the evaporation process begins and ends, the vapor will have evaporated while the purified substance will condense with cool water. In this lab, the purpose is to separate two liquids, cyclohexane and toluene or cyclohexane and p-xylene. During the process, the volume and temperature were recorded at each milliliter. This would show the different boiling points. Then using gas chromatography, we would be able to identify the correct peak. If the difference between the

The first part of this experiment was to determine the individual concentrations of the reactants. In order to do

To prevent the NaOH from absorbing water from the air the initial temperature (t1) was obtained and recorded in the table. After the initial temperature was recorded from the bottom left of the screen of the Netbook, the 2.052 grams of NaOH solid were added to the cup and stirred. The data collection began after selecting Collect. Until the solution reached a peak temperature and began to drop the solution was stirred occasionally with a stirring rod being sure not the hit the temperature probe. Afterwards, the maximum temperature (t2) and the seconds it took to reach the maximum temperature was recorded in results chart. Figure 9.2 Sample: Temperature vs. Time Graph for Reaction 1 was used to confirm the initial and final temperature (t1 and t2). The metal rod of the temperature probe and the cup was rinsed wa DI water and dried. The chemicals were then disposed of safely and properly. The steps for reaction two then began. File then New were selected to reset. The same steps were then followed starting at starting at the placement of the cup into the beaker down through confirming the initial and final temperature. Some changes were made for reaction

The purpose of this lab is to identify the unknown volatile liquid, by finding its molar mass and comparing it to the known molar masses. There are two ways to identify a possible molar mass, and they are to use the Kjeldahl method or the Dumas method (Simmone, Simmone, Eitenmiller, Mills & Cresman, 1997).

“Molar Mass of a Volatile Organic Liquid” lab is focused on determining the unknown substances correct label. During the lab, 3 separate Erlenmeyer flasks were filled with the same unknown clear colourless solution #3 from the back of the lab located under the fume hood. In each of the beakers it was observed to ensure that only 2ml of the unknown solvent was placed into each of the Erlenmeyer flasks. Once the unknown solvents were prepared, the hot water baths are needed to be observed to ensure that 200mL or enough distilled water was placed to fully encapsulate the Erlenmeyer flask. Both of the flasks were placed in the water at approximately the same time. After about 10 minutes, it was witnessed that the water has come to a boil due to

The main objective of the distillation lab was to identify the composition of an unknown binary solution. The only known component is that the boiling point of the two components were at least 40˚C apart in boiling points. Due to the difference in boiling points, fractional distillation would be an easy way to determine the identity of each component of the binary solution. In the experiment, 30mL of the unknown binary solution was ran through the fractional distillation apparatus. As the solution boiled, gas from the unknown solution ran through the column, which had a temperature gradient to allow rapid and repeated distillations, and one of the components were isolated. By recording the temperature and amount of