Separation Of Fractional Distillation Lab Report

* Lighter fraction make better fuels as they ignite more easily and burn well, with cleaner (less smoky) flame.

There are various techniques to separate a mixture of compounds from each other. One of the commonly used way to isolate compounds from a mixture of two compounds is called extraction. This method of extracting two compounds from each other relies on the different solubility of the compounds in two different solvents.

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

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

Steam distillation is an ideal method when using two compounds that are immiscible (i.e., water & oil or Benzene & water). Benzene being the organic solvent that is non-polar and water the inorganic solvent that is polar, creates a dilemma since the two can-not be mixed together. When vaporizing something the vapor pressure must equal the applied pressure. This results in liquid turning to gas. If two immiscible compounds have the same vapor pressure then they will have the same boiling point. Another example would be water & naphthalene, in which water depresses naphthalene’s boiling point. When water boils it creates steam. This steam can be used to pick up particles. One can use steam distillation to pick up immiscible compounds. In our case, the solvent is water and the solutes are the cloves (potentially Eugenol oil). Eugenol oil can be used as an anesthetic. To release the contents of the cloves we can boil them. We can implement the Gaffney principle

Method: Distillation is based on the fact that the matter can exist in three phases - - solid, liquid and gas. As the temperature of a pure substance is increased, it passes through these phases, making a transition at a specific temperature from solid to liquid (melting point--mp) and then at a higher temperature from liquid to gas (boiling point--bp). Distillation involves evaporating a liquid into a gas phase, then condensing the gas back into a liquid and collecting the liquid in a clean receiver. Substances that have a higher boiling point than the desired material will not distill at the

In this experiment, distillations were done. This is a technique that utilizes the differing boiling points of two or more compounds in a mixture in order to separate the compounds from the mixture. The way fractional distillation works is that the initial mixture is boiled up to the point of the lower boiling point compound; this compound then evaporates. This compound is then

The purpose of this lab is to separate a mixture and determine the percentages of each of the ingredients. Each substance will have a different boiling point due to its intrinsic properties and from that, we will be able to determine the purity of different products as we evaporate off the next level of product.

Answer: Distillation is a method for separating a liquid from a solid or from another liquid in which the liquid is boiled off and then recondensed (Yee, n.d., Distilliation). It works because the substance you are looking to distill is boiled off recondensed and separated. It can be used to purify liquids from solids or from other liquids (Yee, n.d., Distillation).

Simple distillation is a separation technique which can be used to separate and purify distillates from a liquid mixture which ideally contains one volatile and one non-volatile compound. If such ideal conditions are not possible—as is usually the case—then simple distillation can be applied as long as the liquid in question is composed of compounds that differ in volatility such that their boiling points differ by at least 40 to 50 degrees Celsius. Because

The first method, distillation, is the process of heating water to its boiling point, collecting the steam, and condensing the purified water vapor. The process is usually repeated a few times to ensure success in purification (Ocean Water Desalination). Distillation uses the property of higher boiling points in salts than in pure water. Possible contaminants that require removal for safe water consumption could include bacteria, lead, mercury, sodium, and chlorine. After boiling the water, water vapor moves through a series of tubes to a separate container where the heat source is removed, and the water is able to condense, now purified. Some strengths of distillation include the removal of heavy metals such as arsenic, lead and mercury, the removal of hardening agents such as calcium and phosphorus, and the removal of bacteria from water by heating. This elimination of bacteria is especially helpful in developing countries due to the increased risk of contamination because of unsanitary conditions. In this process, consideration needs to be given for adequate resources and infrastructure to deliver purified water to the general population of underdeveloped areas. A few disadvantages exist in that distillation does not remove chlorine and is relatively ineffective as the input is about five times the output (Water Treatment Alternatives -

1.) Briefly explain the concept of steam distillation. What is the difference between a simple distillation and a steam distillation? When a mixture of two immiscible liquids are distilled it is referred to as codistillation. This process is referred to as steam distillation when one of the liquids is water. This distillation is used to separate organic liquids from natural products and reaction mixtures in which the final product results in high boiling residues such as tars, inorganic salts, and other relatively involatile components. It is useful in isolating volatile oils from various parts of plants and not useful in the final purification of a

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.

The purpose of distillation is to purify a liquid. Distillations are use to purify contaminates out of water to obtain clean pure water, as well as, to separate mixtures of liquids into their individual components; e.g. methanol and water.