Swab the rubber top with alcohol and allow to dry. 6. Seat the needle. Remove the cap from the needle or blunt cannula by pulling it straight off. Draw back an amount of air into the syringe that is equal to the specific dose of medication to be withdrawn.
Extraction and Drying: Using a separatory funnel, the cooled filtrate was extracted with 10ml of methylene chloride. After shaking our mixture, we broke and dried our emulsion by slowing passing the lower layer through a cotton ball layered with anhydrous magnesium sulfate. The extraction process was repeated 2 more times for maximum collection of the organic layer. Distillation: The extracts were poured into a 50ml round bottle flask and connected to a simple distillation apparatus. To obtain the caffeine, the methylene chloride was removed from the extract, leaving us with our solid caffeine residue.
I weighed the filter to find out the mass. I then folded the filter and placed the filter into the funnel and held the funnel over a paper cup while I poured the liquid into the funnel leaving the benzoic acid to adhere to the filter. I then allowed the filter to dry. Once dried I weighed the mass of the filter and benzoic acid and calculated the mass and recorded into table 1. I then allowed the remaining liquid to evaporate leaving behind salt.
Gently stir the pellets until the acid is dissolved by shaking the the apparatus. Lift the calorimeter lid and wash out its contents and the thermometer. Repeat this experiment using 50.0 mL of 1.0M acetic acid. Repeat experiment using 25.0 mL of each 2.0M sodium hydroxide and 2.0M acetic acid. Data Table(s): Reaction equation Mass of solid NaOH Initial Temp.
When I cleaned up I made sure I cleaned the surface area thoroughly and washed my hands. Conclusions and Observations: Table 1: Experiment Data | Grams | Percent of Mixture | Iron filings | 1.4g | 31.1 | Sand | 1.3g | 28.9 | Table Salt | 1.0g | 22.2 | Benzoic Acid | .8g | 17.8 | Total | 4.5g | 100 | A. My proposed procedure at the beginning of the experiment was a little different because I would have used the filter paper to get the sand out of the mixture. I did though propose to use the magnet to take out iron. B.
Once all the water from the beaker was gone the clamp was carefully replaced so there were no air bubbles in the tube. The tube connected to the aspirator was then removed and connected to the test tube. The gelatin capsule was placed in the tube before adding 10 mL of HCl that had been measured in a graduated cylinder beforehand. The stopper was quickly and firmly placed into the test tube and the pinch clamp was removed again. After a few minutes the acid dissolved the capsule creating a black foam that then turned into a clear liquid again.
During the lab every student conducting the lab should wear goggles and an apron at all times. Gloves could be worn as well to protect the hands from getting dirty. Everyone should beware of the hotplate because it may not appear to be hot but it definitely is. After the experiment the work area should be free of any spills. Goggles and aprons should be worn until the experiment is complete and all solutions are poured down the drain whereas solids should be properly disposed of by being recycled.
c Use the syringe to place 2 cm3 of amylase into the test tube. d Add 1 cm3 of buffer solution to the test tube using a syringe. e Use another syringe to add 2 cm3 of starch to the amylase/ buffer solution. Start the stop clock and leave it on throughout the test. Mix using a plastic pipette.
Once dissolved, 24.9734 (± 0.0045)mL of acid was pipetted into an Erlenmeyer flask along with 25mL of cool (recently boiled) distilled water. Three drops of acid-base indicator, phenolphthalein, is added to the acid solution. Acid is titrated with the unknown base from the burette as the Erlenmeyer flask is consistently being swirled. Near the endpoint of 24mL, drops of base are added to the acid solution until a light pink colour persists within the solution. Titration is repeated 3 more times in order to achieve more accurate results.
Terrall Brooks Organic Chemistry 203 Monday 12:50 pm -4:50 pm Dr. Shaw Fractional Distillation Abstract Distillation is the process of converting a liquid to a vapor, condensing the vapor, and then, collecting the distillate in another container. There are two types of distillation namely, simple and fractional. My group was assigned to perform fractional distillation which aims to separate the components in a liquid mixture having different boiling points. We had to record the temperature and volume collected at 1-mL intervals to compute and determine the unknown mixture we used in the process. The results were Acetone which boiled at 56 degrees and Toluene which boiled at 111 degrees.