Distillation Lab

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

3. What happens to the proof-rating of the brandy, as the distillation process continues? Why?

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.

Answer: The distillation apparatus consists of a round bottom flask connected through an adapter to a condenser, which is connected through another adapter to a second round bottom flask (Yee, n.d., Distillation). There is a thermometer connected through the thermometer adapter at the top (Yee, n.d., Distillation). There is also a vacuum adapter and a heating mantle. The heating mantle is a coil which heats through electrical resistance (Yee, n.d., Distillation). You use cold water and make sure that it goes in through the bottom and out through the top (Yee, n.d., Distillation).

Distillation of the first product began at 83 °C. A Pasteur pipette was used to remove 1-ml of the distillate into a vial. A second vial was filled with distillate until it reached 1-ml. As the second vial is being filled, observe the temperature and remove the apparatus from the heat source if there is an observed drop in temperature.

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.

1.) Transfer the distillate to separatory funnel. Fluid didn’t seem very clear but sufficient to finish our lab on time.

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 the fluid flow meters experiment was to determine the operating characteristics of the Venturi and orifice meters. The purpose of the tray hydraulics experiment was to study the vapor and liquid tray hydraulics parameters for sieve, or perforated, trays in a distillation column. By performing experiments based on theory and comparing results to literature values, the objectives of this experiment can be achieved.

Figure one differs from a graph the simple distillation graph in diagram 2 of the lab manual in the sharp increase in temperature at the 14 ml mark. Diagram 2 is less sharp of a slope, while figure one shows a much sharper change in slope.

The density of an object relative to the density of a liquid will determine whether the object floats or sinks in the liquid. The “Bozeman Video” says that when atoms are more compact in an object, the object is more dense. When an object is more dense than the liquid it's being put in, it sinks. If the object is less dense than the liquid it's being put in, it floats. In a lab we did, we put a regular Mountain Dew can that was full into a bucket of tap water and salt water.

Abstract: The main objective of this lab was to determine how to effectively measure and compare bacteria in different water sources, specifically in this lab by using Coleman Drinking Water Purification Tablets. The tablets did not eliminate bacteria to the level found in tap water, however they were still very effective at eliminating bacteria. The tablets as a result can be trusted by the user to remove any unnecessary health risk when drinking water from an untreated source.

This experiment was to purify salt water by constructing three different water distillers and comparing the amount of fresh water each yielded, inspired by the drinking water shortage in California and around the world. The ocean has about 35,000 ppm of salt, so we cannot directly use ocean water. Since humans can safely drink about 500 ppm of salt, ingesting ocean water is not safe for human consumption, but with distillation, people can drink this water. This issue can be resolved.

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