1) Percentage yield experiment: First we measured 20cm3 of sulphuric acid into a beaker using a measuring cylinder, this will help us determine the percentage yield at the end of the experiment. We then heated the beaker containing the sulphuric acid using a Bunsen burner in order to heat it up for the copper oxide to mix with. We then weighed out 1.02g of copper oxide and added it to the acid and stirred it whilst doing so, we did that until the liquid turned blue, this proves that the chemicals have mixed together. We then weighed this liquid which will help us determine the percentage yield. We then filtered the liquid off which gave us the amount we obtained. We then left the liquid for a week so that the liquid had time to turn into crystals, …show more content…
We then added 10cm3 ethanoic anhydride to the salicylic acid and swirled the contents, this mixes together the two chemicals. We then added 5 drops of concentrated sulphuric acid to the flask and thoroughly swirled the mixture, this creates the solution that makes the aspirin. We then warmed the flask for 20 minutes in a 400cm3 beaker of hot water which was approximately 60°C, we made sure the flask did not go above 65°C because this could have caused the contents to evaporate. Part 2: Using a 25cm3 measuring cylinder we measured out 15cm3 of ethanol into a boiling tube and then prepared a beaker half filled with hot water at approx. 75°C, we got this temperature by filling the beaker with cold water and slowly adding boiling water from a kettle until we reached the right temperature. We then used a spatula to add the crude aspirin to the boiling tube and placed the tube in the beaker of hot water, and stirred it so that it will dissolve into the ethanol. We then poured the hot solution containing dissolved aspirin into approximately 40cm3 of water in a 100cm3 conical flask, the solid did not separate so we did not need to warm the contents of the flask in the water bath. We then let the conical flask cool slowly so that the white needles of aspirin separated. We did have crystals so we did …show more content…
We then used a small mortar and pestle to crush the aspirin and we placed the resulting powder into a conical flask, we crushed the aspirin tablets so that I would be easy to mix with the ethanol. We then added 5ml of ethanol using a measuring cylinder and covered the flask with a watch glass, we did this to avoid evaporation. We then gently heated the mixture over a water bath of around 60-70°C and swirled frequently, we did this so that it would dissolve the acetylsalicylic acid. We then filtered off the hot solution to remove any insoluble material in another small conical flask, we rinsed the flask with a few ml’s of chilled ethanol to collect any residue that was left on the flask. We then slowly added 25ml of chilled deionised water to the filtrate to initiate crystallization by using a measuring cylinder and a dropping pipette, once we had done this we left it for about 10 minutes to allow crystallization at room temperature. We then weighed a filter paper which we will use later in the experiment. We then collected the crystallized acetylsalicylic acid by vacuum filtration in a Buchner funnel and washed the product with a little ice-cold water. We then pre-weighed a clean, empty watch glass and labelled it with our initials and the date, we did this do we could easily identify that it was ours when we go to weigh it with the crystals on. We
Observe the reaction and record how fast the Alka-Seltzer dissolves. 7. Place an Alka-Seltzer tablet into a second empty water bottle. 8. Pour 16 oz of room-temperature water into the bottle.
After I rinsed the copper I transferred it to a watch glass that had been baked for 20 minutes so it would not contain any liquid so as to not counteract the experiment. After I put the copper on this watch glass I baked the copper in the oven for 20 minutes so there would be no liquid left in that to mess up the mass. After 20 minutes I removed the watch glass with the copper in it and weighed itm making sure to weigh the watch glass
The difference in this chemical and physical properties will aid in their separation. Processes like solubility, gravitational filtration and recrystallization will be used to separate the substances present in Panacetin. The melting and boiling point of the substances will help in concluding on which of these compounds will be presented at the end of experiment. Procedure and observation The Panacetin content was weighed approximately 3.0493g and transferred to the Erlenmeyer flask; 75ml of dichloromethane (CH¬2CL2) was added to the content. The dichloromethane (CH2Cl2) dissolved the sucrose, leaving the active unknown agent and aspirin behind.
Then the flask was filled the rest of the way with distilled water to the mark. Similar steps were taken for the rock solution. The rock solution from the prior lab was filtered into a volumetric flask (100mL), then 15 M NH4¬OH (8mL) was added to the flask. After that, the flask was filled to the mark with distilled water. Both flasks were then swirled to combine the solution
In the experiment they used probes to test for pH, dissolved oxygen, total dissolved solids, conductivity, and turbidity. The probes hook up to the computer and collected the averages for each test. They collected this data and used it for later evaluation of the contaminates. They also tested for iron, copper, and chlorine with different tablets.
The test tube was swirled to mix the solution. A small amount of ascorbic acid was added to the test tube. The exact amount of ascorbic acid needed in the solution varied from .0002 grams and .00002 grams, but the electronic scale only weighed to the nearest .01
Lab Report 5: Acetylsalicylic Acid (Aspirin) Synthesis Name: Divya Mehta Student #: 139006548 Date Conducted: November 19th 2014 Date Submitted: November 26th 2014 Partner’s Name: Kirsten Matthews Lab Section: Wednesday 2:30 L9 IAs Name: Brittany Doerr Procedure: For the procedure, see lab manual (CH110 Lab Manual, Fall 2014) pages 96-98. Wilfrid Laurier University Chemistry Department. Fall 2014. Acetylsalicylic Acid (Aspirin) Synthesis.
Glacial acetic acid and acetic anhydride were added to the mixture while refluxing, which converted the lime colored solution into a clear mixture. The flask was cooled in an ice bath and the solution
For 63.0℃, the flask was cooled when the solution in the flask become almost empty. 25 mL of chloroform and 25 mL acetone were added to the flask and distillation was started again. Samples (3V, 3L) were collected at about
The main objective of this experiment was the formation of phenacetin from the synthesis of acetaminophen. This was done through a chemical reaction known as the Williamson ether synthesis using techniques of refluxing, vacuum filtration and recrystallization incorporating a mixed solvent system. A further objective of this experiment was to study the formation of the product (phenacetin). Such validation was completed by using techniques for determining the melting point, calculating percent yield, and IR (infrared spectroscopy) of the resultant product.
Once with Tylenol, Anacin, acetaminophen and acetylsalicylic acid samples spotted separately and once with the unknown samples co-spotted with the known samples. The goal is to identify the main chemical components in Anacin and Tylenol, either acetaminophen or acetylsalicylic acid. Silica (SiO2) gel will be used as the stationary phase and an ethyl acetate (C4H8O2) containing 0.5% acetic acid (CH3COOH) solution will be used as the mobile phase. The molecular structures of the stationary and mobile phases are shown in Figures 1 and 2. The stationary phase is polar protic and the strongest intermolecular force present is hydrogen bonding.
PRACTICAL 4 Materials and Methods Measurement of DNA concentration The most common technique to measure DNA concentration is measurement of absorbance. We had used 1:20 dilution of the DNA sample and the reading was expected to be in the range of 0.1-1.5 OD260. 5µl of DNA and 95µl of PBS buffer were mixed together and inserted into a clean cuvette. Then it was put inside the spectrophotometer.
If impure, preform recrystallization procedure to remove the impurities. Then calculate Percent Recovered on crystals formed, and preform melting point procedure. 2. You find that a solid substance you are trying to purify is very soluble in ethanol, but not very soluble in water. You decide that you are going to try to recrystallize it from a solvent pair, consisting of ethanol and water.
Upon finding the actual concentrations of salicylic acid, concentration of aspirin in the flask at various times can be found using the equation [aspirin]t = [aspirin]0 – [salicylic acid], since at constant volume, number of moles of initial aspirin decrease to form salicylic acid. Initial concentration of aspirin formed as follows: [aspirin]0 = 0.212g / (180.157gmol-1 * 50/1000 L) = 0.0235 mol L-1.
II. METHODOLOGY In order to perform this experiment, the students will need a distillation set-up with a connector receiver, an iron ring and stand, a Bunsen burner, a wire gauze, a 250mL round bottom flask, a graduated cylinder, a thermometer, one or two boiling chips, an alcoholic beverage, masking tape, an ice bath, a stirring rod, and, optionally, food coloring. It is imporatnt to avoid playing with the apparatus and equipment so as to avoid breakage and injuries, especially since fire is being dealt with in this experiment.