Conversion Of Alcohols Lab Report

Purpose: The purpose of this experiment is for students to learn how to properly and accurately separate two liquid compounds, which have two different boiling points, using simple distillation. Then be able to calculate the density of the two samples after the distillation process to determine the success of the distillation process.

Solid impurities and liquid impurities having quite different boiling points are most easily removed by distillation, but even liquids having similar boiling points can be separated. For easy separations, a "simple distillation" apparatus (Figure 1) will be used for the first part, but for more accurate separations, a "fractional distillation" apparatus (Figure 2) is necessary. In this lab we will be using both apparatuses. Unfortunately, each time a distillation is run, material is lost. Some evaporates into the air and some is left behind, stuck to the apparatus. That is why fractional distillation is the best apparatus to use. It is important to keep a careful record of the temperature at the beginning and end of every fraction you collect. Stop the distillation by removing the heat just before all the liquid in the distilling flask is completely gone. Watching the rate of temperature increase is important, allowing the temperature to increase too quickly can cause impurity. The distillation curves for our simple and fractional distillation clearly demonstrate that fractional distillation separates the two compounds more

In Part A of the experiment, isoborneol was oxidized. First, 0.5 grams of isoborneol was dissolved in 1.5 mL of glacial acetic acid inside a 25 mL Erlenmeyer flask. Next, 4.0 mL of household bleach was added to the solution with swirling. The solution was swirled for the next 15 minutes and then was tested against starch-iodine paper. If there was a blue color, then that indicated there was an excess of NaOCl. If the test was negative, a small amount of bleach (~0.5 mL) was added and tested again. The mixture was then diluted with 15 mL of water and transferred to a separatory funnel. 15 mL of diethyl ether and 0.5-1.0 mL NaHSO3 was added. The funnel was shaken and the layers were allowed to separate. The aqueous layer was removed. The ether layer was washed (separated) with 10 mL NaHCO3 solution. The aqueous layer was then tested against litmus paper to confirm that it was basic. The ether layer was dried by anhydrous Na2SO4.

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.

When the lightest liquid in the mixture of two is heated to boiling point, the liquid evaporates, leaving the denser liquid behind. Background Information Immiscible liquids can be separated with ease through simple distillation. However, separation of miscible liquids requires the application

Distillation is a wide-range laboratory technique used to separate and purify liquids based on the differences between their conditions.1 Mixtures of liquids with different boiling points are heated

Experiments such as simple distillation helped purify the neat liquid, and fractional distillation helped separate and purify the binary mixture which included high boiler (HB) and low boiler liquid (LB). Simple distillation can be used effectively to separate liquids that have large boiling differences. Fractional distillation is used when the boiling point of two liquids

Distillation is used to separate mixtures that do not work well together. The simple distillation performed during lab is done to obtain a pure liquid, such as recycling waste acetone to retrieve purified acetone (4).

The mixture of substances is placed in the flask and heated. Ideally, the substance with the lowest boiling point vaporizes first (see vaporization), the temperature remaining constant until that substance has completely distilled. The vapor is led into the condenser where, on being cooled, it reverts to the liquid (condenses) and runs off into a receiving vessel. The product so obtained is known as the distillate. Those substances having a higher boiling point remain in the flask and constitute the

For detailed procedure, refer to the lab manual (J. F. Wójcik and T. S. Ahmadi, Experimental Physical Chemistry, 2015; p.3-5.). Some modifications of the procedure are the concentration of 2-naphthol in both solutions is changed from 0.0001 M to 0.00005 M, and the acid/base concentration is changed from 0.100 M to 0.0100 M.

The crude product is dissolved in a minimal amount of boiling water (around 4 mL) and then slowly cooled to induce crystallization. After crystals formed (in ice bath) they were vacuum filtered and washed twice with 1 mL of cold deionized water and set to dry. The pure crystals weighed to be 70 mg, giving a percent yield of 39.4%. The dramatic change of product amount from crude to pure was most likely due to procedural error or the fact impurities were present in the

“It was precisely this process of getting the fragrant essence out of things with fire, water, steam and an invented apparatus.” - Patrick Süskind one of the most famous distillers of all times. The distillation process allows the most volatile substances such as alcohol and water evaporate at the temperature of about 79 degrees celsius (as a mixture) and be separated from the rest of the substance. To maintain a great quality of the product the Distiller should remove “the heads and tails from the distillate”. In other words, remove the unpleasant parts of the substance. At the end of this long process a yellow liquid is being produce with nearly 70 percent of alcohol in it. Th next step is reduction of alcohol content in this liquid, to make the taste more pleasant. To

Distillation is the process by which a solution containing two or more compounds with varying volatility are heated until the lowest of the compounds boiling points occurs, vaporizing it into the distillation head (containing a thermometer) followed by condensing it (with running water through a tube from bottom to top) until it becomes a liquid where it can again be captured in a receiving flask.1 This process works best and gives purest results when one of the compounds is volatile (easily vaporized) and the other is either non-volatile or volatile with a different boiling point.1 The means with which this process works is by giving sufficient energy to the compound, which in this case is the lighter compound, with the lowest boiling point such that it will vaporize while the (heavier) compound with the higher boiling point remains in the solution with insufficient vaporization energy. Boiling point of a liquid can be impacted in many cases by intermolecular forces such as hydrogen bonding or dipole-dipole interactions, but in this instance cyclohexane (bp: 81°C) and toluene (bp: 111°C) only experience dispersion forces with no distinct differences other than their molecular weights.2 The boiling point is signified by the vapor pressure equaling the

Distillation is a method of separating mixtures, based on the differences in the conditions required to change the phase of components of the mixture. (Helmenstine, 2017)1. You can use double distillation to purify the product even more. To separate the mixtures of liquid, the liquid can be heated to force components, which have different boiling points, in to the gas phase. The gas is the condensed into liquid form to be collected and removed. Distillation units are one of the most popular ways of separation. The most common distillation technique is the liquid-liquid separation process (Kunesh, Kister, Lockett, Fair, 1995). There are two distillation categories, these are batch distillation and continuous distillation. Batch distillation is when lots of the product is made and then the chemical reaction is over. Whereas continuous distillation is made in a continuous flow of product. Distillation can make un-useful heavy products into useful smaller molecules, for example using these techniques you can produce gasoline, distilled water, xylene, alcohol, paraffin, kerosene and many other useful liquids. Also, gas mixtures can be separated, air can be distilled to get elements of Nitrogen, Oxygen and Argon. After the process is finished a distillate is formed, this is purified version of the original liquid. If there is a chemical reaction, then you can use a catalyst or use phase equilibria to shift the equilibrium to the favourable side. There are also many techniques used

Two different types of distillations can be performed to achieve a perfect separation of a mixture. The first is a simple distillation where a liquid mixture is heated and the compound with the lower boiling point will be the first to vaporize, travel through the distillation apparatus where cold water condenses the gas back into a separate container without any of the higher boiling point compound. The