Disadvantages Of Hexane

In the first acid extraction of benzocaine, the compound was dissolved in the organic solvent of dichloromethane. When the mixture was shaken with HCl, benzocaine’s amine group gained a proton and became more soluble in water than dichloromethane. This allowed the newly formed hydrochloric salt to migrate to the aqueous layer. However, the addition of NaOH to the acidic aqueous layer regenerated benzocaine by deprotonation, making it insoluble in the aqueous layer. The precipitation of an ionic salt was therefore recovered by vacuum filtration and had a tested melting point range of 85.1C-87.4C compared to 88C-90C, the literature melting point of benzocaine. The similarity in melting point ranges, but low percent yield of 30.37% proves that the extract was somewhat successful. Lower yields may be the result of spillage performed in the lab. In the second basic extraction, the organic layer now included benzoic acid and benzamide. When treated with NaOH to deprotonate benzoic acid, the newly formed sodium benzoate transitioned to the aqueous layer as a sodium salt. Benzoic acid is regenerated once again after the addition of HCl and became insoluble in the aqueous layer after protonation. Its precipitation was then filtered out for a 65.87% recovery. Compared to its literature melting point of 122.41C, the resulting 120.9C-123.5C melting range of the sample also supports the accuracy of the separation due to its similarities and high percent yield. In conclusion, the usage of base and acid liquid extraction was mostly successful in this experiment because it was able to efficiently and properly isolate the impure mixture into two separate components of benzocaine and benzoic acid. By performing the techniques of extraction and vacuum filtration, the similarities between literature and tested

There are millions of different organic compounds. Most of them are found in mixtures and in order to achieve a pure form they need to be separated, isolated, and purified. However, there are endless numbers of possible mixtures, which make it impossible to have a pre-designed procedure for every mixture. So chemists often have to make their own procedures. The purpose of this experiment was to prepare the student to the real world by them designing their own procedure which will help them understand the techniques of separation and purification better. The goal was to extract two of the components of the

Abstract: One mixture of two unknown liquid compounds and one mixture of two unknown solid compounds were separated, isolated, purified, and characterized by boiling point. Two liquid unknowns were separated, isolated, and purified via simple distillation. Then, the process of an acid-base extraction and washing were used to separate two unknown compounds into two crude compounds: an organic acid and a neutral organic compound. Each crude compound was purified by recrystallization, resulting in a carboxylic acid (RCO2H) and a pure organic compound (RZ). The resulting mass of the pure carboxylic acid was 1.688g with a percent recovery of 31.80%, the boiling range was 244-245 °C, and its density was 2.0879g/mL. The resulting mass of the pure organic solid was 2.4902g with a percent recovery of 46.91%, the boiling range was 52.0-53.4°C, and its density was 1.5956 g/mL.

The purpose of this laboratory experiment was to isolate and characterize clove oil in order to understand how to isolate organic compounds with high boiling points, how to perform and interpret qualitative tests for organic compound functionality, and to continue to learn how to perform and interpret IR spectrometry. Steam distillation was used in order to prevent the organic compound from decomposing at temperatures approaching the compound's boiling point.

Name CHE 173 Sec # January 25, 2005 Experiment 36: Determination of the Structure of a Natural Product in Anise Oil

Experiment 4A: Determination of a Partition Coefficient for Benzoic Acid in Methylene Chloride and Water, and Experiment 4B: Solvent Extraction I: Acid-Base Extraction Using the System Benzoic Acid, Methylene Chloride, and Sodium Bicarbonate Solution

The product was precipitated out and isolated using vacuum filtration after 30 minutes. The product was then left to dry on the vacuum for 20 minutes. The weight of the crude product was 2.924 g. The percent crude yield was then determined to be 98.6%. Please note that the calculation shown in the notebook pages used the incorrect weight of the crude product; therefore obtained the incorrect percent crude yield.

One method used to isolate oils from a material is to use steam distillation. Many organic chemicals decompose before reaching their boiling point, so normal distillation will not work. However, steam is used to carry small amounts of these organic chemicals where they can condense and be collected. This is an important part process in organic chemistry which allows us to extract and test oils. The purpose of this lab is to isolate eugenol (clove oil) from cloves using steam distillation. The eugenol is further separated by using a nonpolar solvent in a separation funnel to remove it from the water and distilling the solvent to leave behind pure eugenol.

This report presents the percentage recoveries found when using the solid-liquid and liquid-liquid extraction techniques to extract a strong acid, weak acid, base, and neutral compound from a mixture. During the solid-liquid section of the experiment, 0.5 M NaHCO , 0.5 M NaOH, 0.5 M HCl, and distilled water are used to dissolve and separate the acid, phenol, and amine solutions from the mixture, leaving the neutral compound remaining. After adding 3 M HCl to the acid and phenol solutions and3 M NaOH to the amine solution, the solutions and solids formed were filtered and the percent recovery of each was calculated. The percent recovery was around a range of 20 % to 22 % for the acid, phenol, and amine, but the neutral had a much higher percentage about 60 %. After using similar techniques for the liquid-liquid extraction section of the experiment, removing the clear lower layer of the two immiscible liquids each time, the percent recovery was around 50 % - 55% for the acid and neutral. The percentages for the phenol and amine were lower. In both sections of the experiment, some percentage of the acid, phenol, amine, and neutral compounds was recovered, so that part of the experiment was successful.

The methods used for extracting oils are expensive and require someone with expertise in the process. It can take 200 pounds of rose petals just to produce 4 teaspoons of oil. This is also why some oils are so expensive. However, they are highly concentrated so it only takes a few drops to achieve the desired effect. I would not suggest buying synthetic oils because; they simply do not have the same powerful effects as natural oils although, if you are on a small budget, they are much cheaper.

There are hundreds of components, such as terpenes, aldehydes and esters found in the oils in varying degrees.

The purpose of this experiment was to use solvent extraction techniques in order to separate a mixture consisting of a carboxylic acid (p-toulic acid), a phenol (p-tert-butylphenol), and a neutral compound (acetanilide). Extraction is the process of selectively dissolving one or more of the compounds of a mixture into an appropriate solvent, the solution that contains these dissolved compounds is called an extract (Manion, 2004).

The purpose of this lab was to investigate the method of extraction as a means of isolating pure compounds. In this experiment, the acid-base extraction method was used on a mixture composed of three separate components: an acid, a base, and a neutral component. The extraction solvent used was diethyl ether. Through sequential acid-base reactions where aqueous 10% NaOH and aqueous 10% HCl were used in a separatory funnel, the three components were extracted, isolated and then recovered through precipitate reverse reactions using 10% NaOH and concentrated HCl. Once the components were isolated and recovered, a melting point analysis was performed and these values were then compared to the values in the laboratory handout in order to identify the compounds. Percent yield of each compound was also calculated. It was found that the mixture contained Benzoic Acid with a melting range of 121.6-122.9 oC and a percent yield of 292%, Meta-nitraniline with a melting range of 111.4-112.2 oC and a percent yield of 204%, and Biphenyl with a melting range of 70.6-73.5 oC with a percent yield of 128%.

In this experiment were used three separation techniques: extraction, sublimation and recrystallization. During the first method, 0.70 g sample of salicylic acid-naphthalene mixture was dissolved in 10 ml of diethyl ether. The solution was placed in a separatory funnel and 10 ml of saturated aqueous sodium bicarbonate solution was added to it. After the initial gas was

In the world of global warming, all kinds of pollution and fuel shortages going on, renewable and clean/ green energy is increasingly the ideal solution of energy related problems we have to solve one way or another. Biofuel is one of the mainstream and highly supported solutions nowadays, an idea to make renewable fuel by living organisms such as fiber, corn, vegetable oil or sugar cane. Unlike nonrenewable fossil fuels over extracted by people causing various environmental problems like generating a considerable amount greenhouse gas, current technology already lets renewable fuel like biofuels to shrink a certain amount of greenhouse gas production, making it a more ‘clean’ source of energy.