Objective: The main goal of this lab is to learn how separation of binary liquid mixtures is performed. Especially when the two liquids have boiling points varying by about 30° C. Hexane can be separated from toluene in this experiment because of the difference in their boiling points. Since toluene has a higher boiling point, it will left at the bottom while the hexane starts to boil out and collect in the Hickman still. GC measurements help us in determining how accurate our data is by making a graph of the amount of hexane and toluene in each fraction. Also this lab gives experience with semi-micro distillation in order for experiments in the future that might need this purification setup.…
Start the distillation by piling up hot sand around the distillation flask with a spatula…
A reflux condenser was assembled using a 25-mL round-bottom flask, hot plate, and aluminum block. It was equipped with a drying tube filled with calcium chloride to control vapors. Approximately 2.5 mL of isopentyl alcohol was massed and placed in the round-bottom flask that contained a stir bar. Using the same graduated cylinder, about 3.5 mL of glacial acetic acid was added to the flask. A calibrated Pasteur pipet was used to add 0.5 mL of concentrated sulfuric acid to the flask and the flask was mixed immediately. The flask was connected to the apparatus and covered with aluminum foil to help retain heat. Using rubber tubing, water was circulated into the lower attachment and out the top attachment and the mixture was brought to a boil. After heating under reflux for 60-75 minutes, the flask was removed from the heating source and left to cool down to room temperature. The reaction mixture from the flask was transferred to a culture tube and 5-mL of water was added. Upon addition of water, careful shaking, and occasional venting, the phases separated and the lower aqueous layer was removed and discarded. Using the same procedure as explained above with water, 2.5 mL of aqueous sodium bicarbonate was added and the lower aqueous layer was again removed and discarded. The same procedure was repeated one last time with 2.5 mL of saturated aqueous sodium chloride and the lower aqueous layer was removed and discarded, leaving behind the crude ester. The crude ester was transferred to…
In order to first perform the reaction, 1.5 mL of 4-methylcyclohexanol was added to a pre-weighed 5mL conical vial. The conical vial was then weighed to find the actual mass of 4-methylcycloheaxanol. Then, 0.4mL of 85% phosphoric acid was added to the conical vial using a plastic pipet. Six drops of concentrated sulfuric acid was then added to the vial using a glass pipet. A spin vane was then added before adding the Hickman head, water condenser and a drying tube packed with calcium chloride to the conical vial.…
24 mL of 4-methylcyclohexanol, 5mL of phosphoric acid, and 1mL of concentrated sulfuric acid was added to a 250 mL round bottom flask and mixed thoroughly with a magnetic stirrer. A simple distillation set up was installed with a 250mL round bottom flask, jack, stirrer, heating mantle, and variac. The solution was heated gently with a small heating mantle to distill the crude product while keeping the vapor temperature around 100C or less. The crude product was collected which contained water, 4-methylcyclohexene, and trace acid.…
In order to perform this experiment, a distillation apparatus was assembled. 4.0mL of H3PO4 and 3.0mL of cyclohexanol was placed in the round-bottom flask as sell as 5 drops of H2SO4 and a magnetic stir bar. The flow of water was then started through the condenser and the reaction mixture was heated while the magnetic stir rod began stirring. Once distillation was complete and no more liquid distilled, or the thermometer rose above 85 degrees Celsius, the heat was turned off and the products were collected in a small test tube. Once cooled, what was left was an organic top layer and a bottom layer. A Pasteur pipette was used to remove the majority of the bottom layer and was placed into a separate labeled container. Placing .25g of anhydrous calcium chloride into the test tube dried the top organic layer which was then left to stand for 5 min. a clean 5-mL vial was weighed and using a Pasteur pipette, the liquid was removed from the test tube and transferred to the tared sample vial and weighed.…
The liquid yield (acidic component) was purified by fractional distillation. The boiling point of the compound was determined afterwards.…
Through the top of the condenser, 14 mL of concentrated sulfuric acid was added drop wise over a period of ten minutes. The addition of the acid created a change in color of the solution to a rustic orange color. The mixture was refluxed for 30 minutes and the solution changed to a faded yellow-orange color. Once reflux was complete, a simple distillation was set up, with the 25 mL collection graduated cylinder placed in an ice bath. The mixture was distilled and combined with the hood partners’ distilled mixture. The distillate was placed in a separatory funnel with 10 mL of distilled water. Once separated, the distillate was added to the funnel again with 9 M sulfuric acid. The organic layer was still in the funnel after separation, as distilled water was added to the solution and then 10 mL of a saturated solution of sodium bicarbonate. The organic solution was dried with anhydrous sodium sulfate for a week. The liquid product was transferred to a 25 mL round bottom flask equipped with a stir bar and a simple distillation was set up. The solution was distilled and the density of the bromide was calculated at 1.222 grams/mL with a boiling range of 87-92◦C. The theoretical yield was calculated at 12.847 grams and the percent yield was 72.3 percent. Next was the characterization and assessment of the purity of the…
The volume of 20 mmol of 2-methylcyclohexanol was calculated and transferred into a round-bottom flask. Then 0.7 mL of 85 % phosphoric acid was mixed in. The reaction vessel was clamped to a ring stand over a suitable heat source and an apparatus was assembled for simple distillation using a Hickman still, water cooled condenser, and thermometer. Then a conical vial was weighted and recorded. After turning on the heat source in slow power, it was waited until it started to distillate. The temperature when it began was 58°C. Using a Pasteur pipet, the distillate was regularly transferred into the conical vial until only a yellow solution remained. It wasn’t left to dry completely. The temperature was 75°C when the vessel was taken from the heat source. The distillate was then washed with 1.5 mL of 5 % aqueous sodium bicarbonate. Then the aqueous lower layer was carefully removed. The upper layer was cloudy at first until it started to become clear after a few minutes. The solution was dried through anhydrous calcium chloride. Then it was weighted.…
To illustrate the use of distillation for separating a mixture of two volatile liquids with different boiling points.…
The Simple and Fractional distillation experiment was divided into two parts. We split up the procedure in this experiment. My group did the simple distillation and we received the Fractional distillation from another group in class. In this experiment, we examined the effectiveness of fractional and simple distillation to determine which is more successful at extracting a pure sample. This experiment was very successful. We are able to determine the success of the experiment but calculating refractive index of both types of distillation.…
The purpose of this experiment was to separate a mixture of ethyl acetate (EtOAc) and toluene by using the method of fractional distillation and to analyze the fractions using gas chromatography (GC).…
This week we utilized two methods of distillation (simple and fractional) to separate a mixture of two volatile compounds. We found that while the simple distillation separated the majority of the two compounds near the beginning and the end of the distilling process, fractional distillation produced much more pure fractions. In simple distillation the…
for the procedure I prepared a boiling bath using a hot plate, and filled a 400ml beaker with tap water. Then I got a 125ml Erlenmeyer flask and put in 2.00 grams of Salicylic acid using a scale. For the third step I added 5ml of Acetic Anhydride using a graduated cylinder. Then I added 5 drops of concentrated Sulfuric acid to the Acetic Anhydride and Salicylic acid in the Erlenmeyer flask using a dropper. I then heated the flask in the boiling bath for exactly 10 minutes. I then removed the flask and allowed it to cool on the counter for 4.5 minutes while adding 2 ml of cold distilled water dropwise. I then stirred to mix the contents. I Then added 40ml of distilled water in the solution and stirred until crystals began to form. My crystals formed in a matter of seconds. I then put the flask in a 400ml beaker of ice water to cool it down from room temperature for exactly 10 minutes to complete the crystallization process. I then collected the product in a filtration process by using filter paper and washing out the flask with distilled…
For as long as humans have existed, they have always found some way to entertain themselves. Even the earliest societies have left evidence of some sort of activity or hobby that they used as a form of entertainment. Perhaps the most famous building that was used as a form of entertainment is the Roman Colosseum, also known as the Flavian amphitheater. In ancient Rome, the most popular form of entertainment was the gladiator fights. These fights, usually among animals and trained public fighters, were staged in open arenas in a city's forum. There is evidence that the gladiator fights were originally staged in Rome's main town square because of a remark by the first-century B.C. Roman architect Vitruvius. He once wrote: "The custom of giving gladiatorial shows in the forum has been handed down from our ancestors." As the years passed, the fights became more and more popular so they drew more spectators. Since these spectators needed seating, games officials put up wooden seats around a forum just prior to a public show and dismantled them afterward. The name amphitheater is given to a public building of the Classical period which was used for spectator sports, games, and displays. Before the Colosseum was built, oval-shaped amphitheaters that could seat thousands of people were constructed of wood. However, many of them burned down and some collapsed. In A.D. 27, in a town not far north of Rome, an ancient wooden amphitheater collapsed because its foundations were not rested on solid ground and the wooden supports were not securely fastened. Fifty thousand people were crushed in the disaster. This made Romans realize that it was time to start building stronger, more permanent amphitheaters, ones made of stone. Building such a tremendous stone structure was no easy task. It was time…