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Principles of fractional distillation
Conclusion on gas chromatography
Principles of fractional distillation
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Recommended: Principles of fractional distillation
Objective: The purpose of this experiment is to learn how to use fractional distillation to separate a mix of isopropyl acetate and toluene, redistill them, and use gas chromatography to examine the separation. Techniques: Chemical Name Molecular Weight Appearance Density Amount Boiling Point Isopropyl Acetate 102.1 g/mol Colorless liquid .88 g/mL 1.5 mL 89°C Toluene 92.15 g/mol Colorless liquid .87 g/mL 1.5mL 111°C • Distillation • Gas Chromatography Physical Data Table: Procedures: The following procedures were performed using pages 27-29 in Dr. Morvant and Dr. Halterman’s Organic Chemistry Laboratory Manual. 1.5mL of Isopropyl acetate and 1.5mL of Toluene were added to a 5mL conical vial by a calibrated Pasteur pipette, and then the spin …show more content…
Aluminum foil was not used during the experiment to wrap around the Hickman still. The temperature of the hot plate continuously increased because the thermometer temperature increased very slowly. The stillhead started to collect condensate around 50°C which is much lower than the 80-90°C that the thermometer was supposed to read. A bent pipette was used to collect around 1.5mL of distillate that was put into a .5-dram vial. This vial was named “Fraction 1.” The hot plate temperature was increased a little more to increase the thermometer temperature in the Hickman still. .6mL of distillate was collected, using the same bent pipette, and put into another .5-dram vial named “Fraction 2.” The hot plate was turned off, and everything was left to cool for a little bit. After it cooled, around 1.2 mL of clear liquid was left in the original vial and transferred to another vial named “Fraction 3.” The syringe for gas chromatography was flushed with acetone and then with Fraction 1 before any reading was done. Because the syringe only collects .2µL of Fraction 1, the liquid wasn’t visible to the naked eye. The needle had to be twisted and rotated gently to insert into the injection port. When the LabQuest collected to data, there was one tall peak and a few little ones. The Percent Area for peak 1 was -197.78 and peak 2 was 297.78, and the Retention time for peak 1 was .700 …show more content…
Distillation is used to separate liquids with different boiling points. Because toluene and isopropyl acetate have different vapor and composition phases, fractional distillation was used. Isopropyl acetate’s boiling point is lower than toluene’s boiling point (89°C and 111°C), meaning that Fraction 1 was isopropyl acetate while Fraction 2 was a mixture of the two, and 3 was pure toluene. Gas chromatography was only performed on Fraction 1 and 3, and a packed column was used. Isopropyl acetate and toluene’s polarity were important because the more polar the molecule, the longer it takes to come off of the column in the GC. The number of peaks showing on the gas chromatography analysis shows how many compounds are in the sample. For example Fraction 1 had two peaks, meaning there were two compounds in the sample, while Fraction 3 only had one peak. The longer the retention time, the more polar the compound was. Fraction 3 had the longest retention time, meaning it was more polar than Fraction 1. Fraction 3 was toluene, which is a more polar compound than isopropyl acetate in Fraction 1. Gas chromatography also identifies the concentration of the compound or the size of the peaks. A tall and wide peak means that there was a lot of a compound passing over the detector in the gas
As shown in figure 2, the percentage of each isomeric alcohol in the mixture had been determined. The hydrogen atom on the carbon atom with the hydroxyl group appear at around 4.0 ppm for borneol and 3.6 ppm for isoborneol. The product ratio has been determined by integrating the peaks. A ratio of 6:1 for the Isoborneol/borneol ratio was expected and is validated by the calculations shown above, with isoborneol percentage at 83.82% and 16.17% of borneol. A CHCl3 group noted at around 7ppm and a CH2Cl2 at around 3.5ppm.
In this lab, Thin Layer Chromatography was used to identify the components of a certain drug. To do this, the compound in question, Motrin was tested against six standards in three different solvents. The three solvent were hexanes, ethyl acetate, and 75% ethyl acetate and 25% hexane; the solution of 75% ethyl acetate and 25% hexane was determined to be the best solvent. This is due to the larger variance in RF values. The six standards that Motrin was tested against were Aspirin, ibuprofen, acetaminophen, naproxen sodium, caffeine and a caffeine and ibuprofen mixture. To determine which standard was present in the chosen drug, the retention factors, or RF, were calculated. A UV light was also used to see the distance each sample traveled in
The purpose of this lab is to determine the density of a solid and an unknown liquid in order to determine the unknowns from a list of substances provided in the lab instruction. A method to identify the substance is to figure out the density (d=m/v) where d is the density equals to the mass divided by the volume of the substance. When measuring the mass, reset the balance to zero to obtain only the mass of the object in grams (g) and not anything else. When measuring the volume, read at the meniscus for an accurate measurement.
The objective of this experiment was to use a common method of separation distillation. Distillation can be used in purifying or separating liquids, when the liquid if heated the more volatile component, the molecule with the lower boiling point, vaporizes and can be condensed. This type of separation will work efficiently when the feed mixture has a decent range between the boiling points of the components. The relationship between component’s vapor pressure to the composition of the solution is Ptotal==P1+P2, Raoult’s Law. This can be used with Dalton’s Law of partial pressure,
The average mole fraction for the different types of fractional distillation with packing is less than 0.15; the fractional distillation packed with steel wool had the lowest mole fraction at 0.1386139 and the simple distillation set up had the highest mole fraction at 0.336633663. In the second fraction the mole fractions varied significantly between the different setups. The fractional distillation with steel wool had the lowest average at 0.5293501, while the fractional distillation with the empty column had the highest average at 0.821075. The fractional distillation with beads (mole fraction of 0.7008487) and rings (mole fraction of 0.7095746) had very similar average results, while the simple distillation had a mole fraction of 0.557708628. In the residual fraction, which was supposed to be almost pure Toluene, all of the distillation setups had mole fractions of Toluene above 0.94. The fractional distillation with the empty column had the highest average mole fraction with 0.97843 and the fractional distillation with the steel wool had the lowest average mole fraction with 0.9466054. While the fractional distillation with the empty column had the purest residual liquid remaining, the individual data points for all the
In this lab, solutions were separated by polarity and affinity to solids by chromatography. Chromatography is the separation of a mixture, where the components move at different rates up a medium. The medium used was chromatography paper, matched with a series of developers to aid in movement of compounds upwards. The distance moved up the paper is measured and the rf is calculated. The distance the pigments traveled is divided by the distance developer traveled. The more polar a substance the further it travels up the paper. The paper works by capillary action and absorption to separate the compounds.
In order to separate the mixture of fluorene, o-toluic acid, and 1, 4-dibromobenzene, the previously learned techniques of extraction and crystallization are needed to perform the experiment. First, 10.0 mL of diethyl ether would be added to the mixture in a centrifuge tube (1) and shaken until the mixture completely dissolved (2). Diethyl ether is the best solvent for dissolving the mixture, because though it is a polar molecule, its ethyl groups make it a nonpolar solvent. The compounds, fluorene and 1, 4-dibromobenzene, are also nonpolar; therefore, it would be easier for it to be dissolved in this organic solvent.
HPLC is abbreviated as High Performance Liquid Chromatography or High Pressure Liquid Chromatography. In pharmaceutical and biomedical analysis HPLC has utmost feature that is for the development of the characteristic of the methodology since 25 years. During the process of discovery, development and manufacturing for the identification, qualification and quantification of drug analysis in active pharmaceutical Ingredient (API) or in the formulation, HPLC is the most important analytical tool. High Performance Liquid Chromatography (HPLC) is a one of the form of column chromatography that pumps solvent (called as mobile phase) and carried sample mixture or analyte into the column has chromatographic
In conclusion Gas Chromatography has many uses to separate and analyse compounds and to be able find separate components in a mixture to identify any unknown components. Because of it's simplicity and effectiveness it is one of the most important tools to chemistry. Like most analytical techniques it has its advantages such as not being harmful to the sample be used and disadvantages such as not being particularly use with liquids that change temperate easily.
There is also the potential of human error within this experiment for example finding the meniscus is important to get an accurate amount using the graduated pipettes and burettes. There is a possibility that at one point in the experiment a chemical was measured inaccurately affecting the results. To resolve this, the experiment should have been repeated three times.
Chromatography is the technical term for a set of laboratory approaches for the separation of mixtures (Solid/Liquid/Gas). The mixture is dissolved in a fluid which called the mobile phase, which carries it through a structure holding another material known as the stationary phase. The various constituents of the mixture transport at different velocities, causing them to separate. The separation is mainly based on differential partitioning between the mobile and it’s stationary phases. Subtle differences in a compound's partition coefficient result in differential retention time on the stationary phase and thus changing the separation (Tomer, et al., 1994).
An organic solvent or a mixture of solvents (the eluent) flows down through the column. Components of the sample separate from each other by partitioning between the stationary packing material (silica or alumina) and the mobile eluent. Molecules with different polarity partition to different extents, and therefore move through the column at different rates. The eluent is collected in fractions. Fractions are typically analyzed by thin-layer chromatography to see if separation of the components was successful. Column Chromatography is the preparative application of chromatography, which is mainly used to obtain pure chemical compounds from a mixture of compounds on a scale from micrograms to kilograms using large industrial columns.
The sample was subjected to steam distillation as illustrated in Figure 1. A total of 50ml of distillate was collected while recording the temperature for every 5.0 ml of distillate. The distillate was transferred into a 250ml Erlenmeyer flask and 3.0 g of NaCl was added. The flask was cooled and the content was transferred into a 250-ml separatory funnel. Then 25.0ml of hexane was added and the mixture was shaken for 5 minutes with occasional venting. The aqueous layer was discarded and the organic layer was left inside. About 25.0ml of 10% NaOH was then added and the mixture was shaken as before. The aqueous layer was collected and then cooled in an ice bath. It was then acidified with enough 6.00 M HCl while the pH is being monitored with red litmus paper. Another 25.0 ml of hexane was added and the mixture was shaken as before. The hexane extract was saved and a small amount of anhydrous sodium sulfate was added. The mixture was then swirled for a couple of minutes then filtered. A small amount of the final extracted was tested separately with 1% FeCl3 and Bayer’s reagent.
The purpose of this experiment is to compare the processes of distillation and fractional distillation to discover which procedure enables a more pure sample of ethanol to be collected from an ethanol/water mixture.
Thin layer chromatography is a classical case of adsorption or solid/liquid chromatography or planar chromatography. In planar chromatography, the stationary phase is applied on a flat surface and movement of mobile phase is due to the capillary action. The stationary phase is normally a polar absorbent and the mobile phase can be a single solvent or combination of solvents. Adsorption is a concentration dependent process and adsorption coefficient is not constant, in contrast to partition coefficient (liquid/liquid chromatography). Hence, if the concentration of sample is more than the absorptive capacity of stationary phase, the separation of components of the mixture will be poor. TLC is a useful tool for separating and identifying