Separation Of Fluorene And 9 Fluorenone

Experiment 55 consists of devising a separation and purification scheme for a three component mixture. The overall objective is to isolate in pure form two of the three compounds. This was done using extraction, solubility, crystallization and vacuum filtration. The experiment was carried out two times, both of which were successful.

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

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

Introduction: The fundamental techniques of organic chemistry lab, commonly known as SIPCAn, include separation, isolation, purification, characterization, and analysis (1). Through SIPCAn, students learn the fundamental techniques of organic chemistry laboratory. Mastering these techniques are necessary in order to perform more complicated experiments and to carry out organic reactions and synthesis. The information gained from SIPCAn included boiling point, melting point, and density can be used to identify unknown compounds. Simple distillation was used to purify a compound by separating it from a

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 first TLC plate showed that the fractions collected during the experiment that appeared to be the purest were fractions 4 and 6. These two fractions and fractions number 5 were combined for the final product. The Rf values for the standard carvone, fraction 4, and fraction 6 were all 0.32 indicating that these compounds were

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.

The purpose of this experiment is to familiarize oneself with the general procedures determining a partition coefficient at the microscale level and learn in weighing milligram quantities of materials on an electronic balance, the use of automatic pipets, the use of transfer pipet, and the use of a vortex mixer. Also, to familiarize oneself with extraction

First, dichloromethane was the least polar solvent, so it barely moved up the plate. Hence, the spots on the TLC plate stayed at almost the same place they were spotted on, and separation did not occur. As a result, the retention factor (Rf) values for these components were too small. In addition, the second solvent, methanol, was the most polar solvent out of the three, and the solvent moved up the plate too quickly. This resulted in the components moving up the plate based on the solvent's polarity instead of their own, and a smear of all components at the solvent front was observed. Hence, the Rf values could not be determined. Lastly, ethyl acetate, a moderately polar solvent, moved up the plate with moderate speed. This gave the components time to move up the plate according to their polarity, and the Rf values could be used to identify the unknown compound. According to the TLC method with ethyl acetate solvent, the unknown compound had the same Rf value with acetanilide (Rf = 0.40). As a result, the unknown compound was identified as

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.

In the extraction of certain compounds, solubility plays an important factor in how the procedure is performed. The identification of which solvent is best for the substance is crucial. The relation of polarity between the solute and solvent is determined at a molecular level. The relationship between the solvent and solute needed shared similar characteristics. Polar solutes are dissolved in polar solvents while nonpolar solutes are dissolved in nonpolar solvents. From a chemical level, molecules are attracted to other similar molecules closest to their properties. Polar molecules are only attracted to polar molecules in both the solute and the solvent, and the same goes for nonpolar molecules. This explanation

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.

The yellow band, ferrocene, elute from the column with the like non-polar phases of hexanes. Theoretically speaking an additional orange band, representing acetylferrocene, should have eluted after the shift in mobile phases. Considering that the mobile phase changes from a non-polar content to that of higher polarity with the addition of ethyl acetate, it is logical that a polar species like acetylferrocene would elute. After collecting and evaporating the solvent portion of the darkest yellow fraction, the resulting mass was 0.017 g, an 18% yield from the starting the amount. This yield could be raise if the additional yellow fractions were collect. The melting point of this collected fraction was 170°C, which reasonably close to the literature value of 172. Considering that the species sampled was the started reactant, thus there was no chemical change, it safe to assume the purified product is

     In liquid chromatography, the separator is called the column and consists in most cases of a tube filled with porous material called the stationary phase. A liquid, called the mobile phase, flows through the tube between the particles of stationary phase material. A liquid sample is taken from a mixture to be analyzed and introduced to a part of the system that is at elevated pressure. The sample is then transported to a separator by the flow in the system.

After wearing the gloves we obtained a chromatography vial from professor and label it with my and my peer initials. We dried up the chromatography vial in fume hood and added 1 ml of chromatography solvent to the vial. Then we took a chromatography strip and measure it 1.5 cm with ruler from one end of the strip and drew a line with pencil we cut two small pieces below the pencil line to form a pointed end. We applied spinach on the strip using quarter to rub the spinach leaf on the line that we drew on the strip and put it into the chromatography vial and placed that in fume hood. We observed as the solvent was moving up the chromatography strip by capillary action. When the solvent was reached approximately 1 cm from the top of the strip then we removed the cap from the vial. We took out the strip from the vial using forceps and marked up the location of the solvent front because it evaporates quickly. We measure out the distance as well as the pigment in order to find out the rf value. Moreover we compared rf values to the one in reference list in order to identify the