Distiller A Results

Lastly, the water that the beakers were washed with may have steadily lowered the temperature of the glass throughout the trials and therefore affected the base temperature of the vinegar and the temperature of the

14 mL of 9 M H2SO4 was added to the separatory funnel and the mixture was shaken. The layers were given a small amount of time to separate. The remaining n-butyl alcohol was extracted by the H2SO4 solution therefore, there was only one organic top layer. The lower aqueous layer was drained and discarded. 14 mL of H2O was added to the separatory funnel. A stopper was placed on the separatory funnel and it was shaken while being vented occasionally. The layers separated and the lower layer which contained the n-butyl bromide was drained into a smaller beaker. The aqueous layer was then discarded after ensuring that the correct layer had been saved by completing the "water drop test" (adding a drop of water to the drained liquid and if the water dissolves, it confirms that it is an aqueous layer). The alkyl halide was then returned to the separatory funnel. 14 mL of saturated aqeous sodium bicarbonate was added a little at a time while the separatory funnel was being swirled. A stopper was placed on the funnel and it was shaken for 1 minute while being vented frequently to relieve any pressure that was being produced. The lower alkyl halide layer was drained into a dry Erlenmeyer flask and 1.0 g of anhydrous calcium chloride was added to dry the solution. A stopper was placed on the Erlenmeyer flask and the contents were swirled until the liquid was clear. For the distillation

The distillation that was more efficient at separating the two compounds was the cyclohexane and the p-xylene since the curve of the graph for temperature vs. volume has a slightly better curve (Table 4A). The graph for cyclohexane and toluene was more linear (Table 4B). Furthermore, the mole fraction of cyclohexane and p-xylene was higher than the mole fraction of cyclohexane and toluene. For instance, the mole fraction of cyclohexane and p-xylene (when adding the mole fraction of the first ml and the last couple of drops) was 0.6604 while the mole fraction for cyclohexane and toluene was 0.13396. A higher mole fraction means that the compounds were purer which means that they separated better—since increasing the mole fraction increases the vapor pressure. Therefore, my hypothesis was supported.

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.

(c) (2 pts) Imagine that you wanted to perform a distillation at your own home (remember, distillation as a technique is not illegal—it is only illegal if you use it to produce alcohol), but you did not have the fancy lab equipment that you saw in the video. How could you do it? How could you improvise in terms of equipment? Explain the entire setup in detail and how the

The control in the experiment is distilled water, as it does not contain sucrose solution.

With the purpose of the experiment being to identify the 30 mL of unknown liquid, the theoretical basis of simple and fractional distillation must be deconstructed and applied to the data obtained describing the liquid in question.

Distillation is a method of separating two volatile chemicals on the basis of their differing boiling points. During this lab, students were given 30 mL of an unknown solution containing two colorless chemicals. Because the chemicals may have had a relatively close boiling point, we had to employ a fractional distillation over a simple distillation. By adding a fractionating column between the boiling flask and the condenser, we were able to separate the liquids more efficiently due to the fact that more volatile liquids tend to push towards the top of the fractionating column, thereby leaving the liquid with the lower boiling point towards the bottom. After obtaining the distillates, we utilized a gas chromatograph in order to analyze the volatile substances in the gas phase and determine their composition percentage of the initial solution. Overall, through this lab we were able to enhance our knowledge on the practical utilization of chemical theories, and thus also demonstrated technical fluency involving the equipment.

The purpose of this experiment was to separate a two component mixture using fractional distillation. Distillation is a process of vaporization than condensation of a substance, used primarily to separate substances from a mixture when there are different boiling points. Fractional distillation is when the mixture has multiple substances with similar boiling points, and a fractional column is used to create multiple vaporization/condensation cycles. Fractional distillation is important when two or more substances need to be separated, but they have similar boiling points.

Aim The aim of this experiment is to test the effect of selected variables on the osmotic pressure during desalination. The variables being researched include: the size of the cation, different salinities and the solubility of a number of salts normally found in seawater. Background Information I have for a number of years been interested in environmental issues such as water consumption and the carbon footprint that characterizes our modern societies. In a previous experiment I created an organic geyser, designed to use compost to provide a source of energy to heat water.

It was important to use distilled water in Part C instead of tap water because tap water can have impurities, distilled water is the purest form of water and would give true results.

The experiment was a two-day experiment. On the first day, we did steps 1-11. In a 400-milliliter beaker, we placed five tea bags instead of 10, and approximately 150-milliliters of DI water

Step 1 and 2 was repeated by using distilled water by replacing the test solution.

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

As it reaches the distilling side arm, the temperature of the vapor is collected. The vapor pressure becomes strong enough that the vapor begins to travel down the condensing tube where it is converted back into liquid. This liquid should be distilled from any contaminants. This is capable because different molecules have different boiling points. For instance waters boiling point is roughly 100oC where as Methanol’s boiling point is 65.4oC therefore the Methanol will boil and evaporator first leaving only water in the boiling flask. Once the temperature of the vapor reaches 100oC no methanol should be left in the boiling flask and the water should now be the only vapor