Separation Of Alantolactone Lab Report

The objective of this experiment is to separate a 50:50 mixture of benzoic acid and benzil by using macroscale extraction. In the experiment, organic solvent diethyl ether is used. After adding 1.0 gram of the 50:50 mixture of benzoic acid and benzil to a 25ml Erlenmeyer flask, diethyl ether was added to the flask to dissolve the mixture. Benzoic acid and benzil dissolve in diethyl ether. Once the mixture dissolved in

This experiment combined all the knowledge of the previous labs performed throughout the semester. An unknown mixture containing an organic acid or base and an organic neutral compound in nearly equal amounts needs to be separated to its separate components. An understanding of solubility, extraction, crystallization and vacuum filtration is necessary in order to

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 objective of this extraction experiment was to achieve a comprehensive understanding, as well as master the practice, of the technique of separating various individual components of a compound.

The purpose of this experiment is to practice common organic laboratory techniques inside the lab to get one oriented to the basic methods of procedure that can be used for later experiments. This experiment involves the separation of benzoic acid from a more crude form, consisting of benzoic acid, methyl orange, a common acid/base indicator, and cellulose, a natural polymer of glucose (Huston, and Liu 17-24). The technique that is used to perform this separation is called extraction. Extraction is a systematic process of separating mixtures of compounds, taking advantage of the affinity differences of compounds to separate them (Padias 128-37). This technique recognizes the principle that “like dissolves in like,” that is,

Objective: The objective of this experiment is to use acid-base extraction techniques to separate a mixture of organic compounds based on acidity and/or basicity. After the three compounds are separated we will recover them into their salt forms and then purify them by recrystallization and identify them by their melting points.

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 solution was placed into a separation funnel, in which the top and bottom layers were slowly filtered out into two different beakers. The bottom layer solution was heated until the ethyl acetate evaporated and only the organic compound remained. Next, a TLC technique was prepared employing silica gel as the stationary phase and 1:1 ethyl acetate hexane as the mobile phase. In order to develop a standard, a TLC plate was spotted with benzoic acid (BA), benzophenone (BZ), biphenyl (BI), and a mixture off the three. After incubating the plate in the chamber with the mobile phase, it was analyzed under a UV light.

The eluting solvent passed down the column by the gravity and an equilibrium was established between the solute absorbed by the absorbent (silica gel in this experiment) and the eluting solving flowing down. Since the components in the sample had different polarity and they interacted with the stationary phase and the mobile phase differently, the components would be carried by the solvent to a different extent and a separation of the components could be achieved.

On a thin chromatography plate, five spots were placed ( as shown in table 2) and the plate was developed using chloroform/methanol. This was later visualized with dragendorff’s reagent under the UV light. All separated components were observed, identified and recorded.

Treatment of a racemic mixture with tartaric acid which is an optically pure resolving agent helped in the separation of the racemic mixture into the R and S diastereomer salts because of their unique solubilities with methanol (2). It was evident that both diastereomers had different solubilites in methanol because one diastereomer R-(+)-amine dissolved in the solution while the other, S-(-)-amine precipitated into crystals and did not dissolve. The crystals were purified and further isolated through a vacuum filtration (1). Below, shows the treatment of a racemic mixture with tartaric acid and methanol. As mentioned before, the resulting product is diastereomeric salts, which were separated based on solubility

For the 2nd plate, caffeine, reference mixture B (ibuprofen and caffeine), and ibuprofen, iwas spotted in that following order at their appropriate lines. The 3rd plate was only spotted with the crushed and diluted Unknown C tablet, appointing our goal in this experiment, being able to discern the unknown’s identity based on comparing the TLC spot location. For each solution, the spots were at the appropriate size to recognize, to ensure no overlapping between the compounds if too big nor any spots to even be observed if too small. When the development chamber was prepared, a small amount of the development solvent was obtained and added into the chamber to fill a depth of about 0.5-0.7 cm. The spotted plates were placed in the chamber in the developing jar with their bottom edges being parallel to the bottom of the jar, one at a time.

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).

Introduction: The aim of this experiment was to observe how different procedures can be used to separate molecules base on their unique properties; such as, their electrical charge as well as their size and shape. In the ion exchange, separation is done using an equilibrium of the molecules, any disturbance in the equilibrium will greatly affect the strength and ph. of the molecules. Gel filtration, on the

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