Fulorenone Synthesis Lab Report

Different procedures were used to isolate benzil from the ether layer and benzoic acid from the aqueous layers. To isolate benzil, anhydrous MgSO4 was added to the flask containing the ether layer solution. MgSO4 removes the remaining water in the ether layer solution. After making sure that enough amount of MgSO4 present in the solution, the ether solution was filtered by using gravity filtration. During filtration, MgSO4 was removed from the solution and the ether solution was collected in 25 ml flask. To separate benzil from the filtered ether solution, the beaker containing the ether solution was heated until the ether evaporated. After letting the beaker to cool to room temperature, the mass of the beaker with the benzil crystals was measured. From the combined mass of the beaker and the benzil crystals and from the predetermined mass of the beaker, the mass of the collected crystals was calculated to be 0.266 gram.

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

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

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.

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

Pre-Lab: Analgesic drugs are known for reducing pain, while antiseptic drugs reduce symptoms such as fevers and swelling. However, some of these drugs can reduce both illnesses. To obtain a pure compound in these drugs, the scientist needs to separate the desired compound by taking advantage of the different physical and chemical properties. Such as; different boiling points, melting points and their solubility properties. To do this a chemist can also asses the differences between acidic and basic substances when they are added to water soluble mixtures. Within this current experiment I will asses the

In this experiment, the reduction of a ketone to an alcohol using sodium borohydride was demonstrated. When the solution turned from yellow to colorless, sulfuric acid was added and the solution was set under reflux to allow for the complete dissolution of the solids. After cooling, the product was then isolated using vacuum filtration before mixed solvent recrystallization was used on it. An infrared (IR) spectra was obtained for the product along with the melting point and weight. The weight was further used to calculate the percent yield.

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

In Table 1, fluorene travels further up the TLC plate versus fluorenone since a more nonpolar 80:20 pentane-ether developing solvent is used. Since fluorine is more nonpolar than 9-fluorenone, it will be more soluble in the highly nonpolar solvent and enter the mobile phase easier than the polar 9-fluorenone. Fraction 2 is expected to have two different spots because this is the collection of the eluted solution between Fraction 1 and Fraction 3, where the fraction contains both the remaining fluorene and 9-fluorenone. Fraction 1, however, should not contain any 9-fluorenone since if correctly performed only fluorene and pentane should have eluted out in the mobile phase. A crack in the column during the elution of Fraction caused one section

Experiment 1: After 10% sodium bicarbonate solution adds to the dichloromethane solution, which dissolves the mixture of benzoic acid, 2-naphthol, and 1,4-dimethoxybenzene, and shake the separatory funnel, there are hissing sounds as well as when 10% sodium hydroxide solution is added. Also, when the separatory funnel is vented, gas, carbon dioxide, rushes out. The first extraction allows benzoic acid to be isolated. Through adding 10% sodium bicarbonate solution, the weak base removes the proton of benzoic acid, a stronger acid compared with 2-naphthol, which turns benzoic acid into charged form. So it dissolves in the aqueous layer while 1,4-dimethoxybenzene and 2-naphthol remain in the organic layer.

The purpose of this experiment was to separate a mixture. This was achieved by first boiling the mixture in water, then filtering it into a flask, which was then placed into a box of ice to be crystallized, then the crystals were separated from the liquid by being filtered once again. The result of this was that we were able to successfully separate the mixture and created crystals in the final step. We were also able to find the mass of the benzoic acid. The mass of it was 0.58 grams. This was found because mass of the filter paper with the acid was 1.55 grams and the mass of the filter paper was 0.97 grams. By subtracting the filter paper from the filter paper with acid, we were able to figure out that the mass of the filter paper with acid

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

Solid substances that contain impurities may be purified in a series of steps. The process known as recrystallization allowed for purification to occur. The solubility and melting point of the substances are accounted for certain substances to be dissolved in certain solvents. The melting point is a certain temperature at which a given substance, in this case a solid, is melted. The melting point of benzoic acid and naphthalene in this experiment are needed to understand at which temperature the substances are purified. The melting points were denoted in ranges that explained at which points the substance began to melt, and were completely melted. In relation, the melting points of certain substances noted, aided in the selection of which solvents were used. The solvents used were selected in terms that the substance completely will dissolve; however, the impurity is particularly insoluble to that same solvent, for the pure crystals to be collected. Benzoic acid was dissolved in water, being the solvent, because the solubility is higher at higher temperatures. The same goes for naphthalene being dissolved in ethanol. These concepts allowed the process of recrystallization to occur if followed, resulting in the products of purified crystals.

Liquid-liquid extraction is an essential technique used in organic chemistry to separate products from a reaction mixture by exploiting its various properties, such as its acidity. Overall, this then allows organic chemists to obtain a purer product. For the purpose of this experiment, liquid-liquid extraction was utilized to isolate a neutral, amine, and carboxylic acid component from an unknown mixture in order to determine their identities by performing melting point and 1H NMR analyses on each individual element.

Chromatography, which was originally discovered and developed by Mikhail Semenovich Tswett in the early 1900s, is a laboratory technique used to separate and distinguish between components of a mixture. The various components of a sample mixture are known as analytes. Chromatography was originally used to separate the various molecules that make up plant pigmentation. Because these components, carotenes, chlorophyll, and xanthophylls, are different colors, the separation of them is responsible for the name of this laboratory technique. Throughout the early to mid-1900s, different styles of chromatography were developed and allowed this technique to be applicable to a wide variety of analyses and separation processes. Chromatography can be applied to analytical process, which aim to examine the presence and relative concentrations of various analytes within a sample. The goal of preparative chromatography is to separate analytes within a mixture for isolation and purification purposes. Chromatography was originally developed by Tswett for the purpose of isolation of particular compounds (10). Moreover, more recent advancements in chromatography are facilitating the separation and distinction of analytes that are extremely comparable to one another and increasing the resolution of the technique.