Erlenmeyer flask Essays

450M NaOH. The actual molarity of the NaOH concentration used was found to be 1.5M NaOH. The percent error of the results resulted in 72%. The large error may have occurred due to over titration of the NaOH, as the color of the solution in the flask was a darker pink in comparison for the needed faint pink. Discussion of Theory: Titration is the basis of the Titration Lab because the goal of the lab was to titrate. Titration is determining the concentration of a solution by neutralizing it

each obtained, and then individually placed in a 100 mL erlenmeyer flask up to the 25 mL mark. Then, a UV VIS spectrometer was connected to a laptop with the program Logger Pro. It was then calibrated by filling a cuvette to the three-quarter mark with deionized water, and running it through the calibration tool present in the program. After the spectrometer was calibrated, 5 mL of yellow dye was placed in another cuvette from the erlenmeyer flask using a 5 mL transfer pipette. The absorption level

(1) The purpose of the separation lab procedure was to help my group members and I successfully formulate our own plan before completing the experiment, handling multiple materials and substances, etc. It acted as a step-by-step plan that guided us throughout the experiment and ensured that we were well prepared ahead of time (ie. knowing what kind of materials were necessary and gathering the correct measurements of each substance); this made the experiment day much less hectic for all of us. It

and three Erlenmeyer flasks are required. Set the spectrophotometer to 540nm. Number the flasks from one to three and add 30 milliliters of enzyme extract the flask marked one on it. It is best to split up the work into three groups. Next, add 20 milliliters to the flasks marked two and three. Pipette 10 milliliters of enzyme extract from flask one to flask two making a 1:3 solution of water and enzymatic solution in flask 2. Next, Pipette 10 milliners of flask twos 1:3 solution into flask three creating

Table 1 mentions the Column volumes of Gel Filtration experiment: Void Volume (Vo), Elution Volume (Ve), Included Volume (Vi), Entire Volume (Vo + Vi), and Inert Volume (Vg). Void Volume (Vo) came out to be 1.25 ml. It was calculated by adding all the fractions that contained blue dextran. Blue Dextran was the biggest substance in size which made it impossible to fit in the available pore sizes of the beads. Void Volume represents the space between the beads in column. In addition, Elution Volume

many filtration procedures in the experiment, as not all of the product was poured out from the flask, onto the filter. Since, recrystallization could not be done, the benzoic acid was immediately transferred onto the watch glass, and it is when transferring some product could have been left on the filter. Overall, pouring product into the filter, and trying to get every particle of product from the flask for each filtration procedure in the experiment, is rather difficult, and is impossible to get

both acetone and the unknown volatile liquid was caused by the deviation of mass in each trial. During the trial of the experiment aluminum foil was used as a cap for the Erlenmeyer flask and by using a pin, a hole was made into the cap to insure that the gas vapors would escape during the heating process, later the Erlenmeyer flask was measured after the heating process when the gas was fully condensed; however, this procedure effected the results collected. With the usage of the aluminum foil it had

First, we had to use the electronic balance, determine the mass of the 250-mL Erlenmeyer flask. 2. Second, we had to mass the filter paper you will use in the experiment, after you have prepared it for the funnel. Record this number. 3. Third, we had to place the weighing boat on the electronic balance. Then 0 the balance. 4. Then, we

had been prepared in steps above. d) Pour the upper solvent layer through the neck of the funnel into a clean 125 ml Erlenmeyer flask. Return the aqueous solution from the 250 ml beaker to the separatory funnel. Add another fresh 20 ml of solvent to the funnel and again extract the aqueous solution as you did in b)

the rate. Procedure Part A- Measurement of the SN1 Reaction Rate of Tert-Butyl Chloride • 100 mL of a solution of propan-2-ol and water (1:1 ratio) were collected from a container provided by the instructor, and they were placed in a 250 mL Erlenmeyer flask, which was subsequently cork-stoppered. Afterwards, 150 mL of NaOH were acquired and placed in a beaker, and in turn this 150 mL sample of NaOH was used to fill a 50 mL buret to the highest mark, and this buret was attached to a butterfly clamp

together. 6. Rinse a 500 ml volumetric flask with deionized water. 7. Label the volumetric flask so you know which solution is in it. 8. Place a clean funnel into the mouth of a 500ml volumetric flask. 9. Carefully pour the NaOH pellets into the funnel. 10. Use the wash bottle with deionised water to transfer all the NaOH pellets from the glass beaker to the funnel. 11. Rinse out all the NaOH pellets with the wash bottle from the funnel in the volumetric flask.

the fact there is no way to have 100% yield and Graph 1 did not have two different slopes there were errors, these are some: not properly pouring the solution through the filtrate losing the precipitate under the filter paper, not rinsing the Erlenmeyer flasks completely out to filter all of the solution, and spilling any solid precipitate when removing the filter paper from the Buchner funnel or after drying when taking the

milliliter Erlenmeyer flask and we poured 20 milliliters of hydrochloric into the graduated cylinder. Then we placed the 125 milliliter Erlenmeyer flask with the magnesium, the rubber stopper, and the graduated cylinder with 20 milliliters of hydrochloric acid onto a scale. After we got the different masses, we added them up until we got a final total and we put that mass into a table. Next, we poured the Hydrochloric acid into the flask and we will quickly put the rubber stopper on the flask. After

minutes and 11.5mL of concentrated sulfuric acid was carefully added while flask was swirled in bath. Flask was put into electric flask heater clamped securely to a condenser. Mixture was heated to boiling point for reflux condensation. Reflux continued for 45 minutes without allowing reactants to evaporate so that alkyl bromide and salt layers could form; afterwards, flask was removed from heat and condenser cooled and drained. Flask is removed from condenser and attached to a still head while condenser

results were recorded. After that, the 25-mL graduated cylinder and the 50-mL beaker were cleaned and dried. Next, their masses were measured on the scale, and the results were rounded to the nearest thousands decimal place. Subsequently, the Erlenmeyer flask was filled with 100 mL of distilled water. Using the thermometer, the temperature was measured and recorded. Then, the 25-mL graduated cylinder was filled with 25 mL of distilled water, and its mass was measured and recorded. The density of the

stopper in the neck of the funnel.  Shake c) Slowly remove the lower aqueous layer through the stopcock into the same 500 ml beaker in which the solution is there. d) Pour the upper solvent layer through the neck of the funnel into a clean 125 ml Erlenmeyer flask.  Return the aqueous solution from the 500 ml beaker to the separatory funnel.  Add another fresh 40 ml of solvent to the funnel and again extract the aqueous solution as you did in b)

Effect of carbon dioxide availability on photosynthetic rate of the leaves of Elodea Densa. Rosanth Anparasan1, Muhammad Ali Qazi1, Kyle Patel1, Sheldon Lui1, Hossein Bhorbani 1 1Dept. of Biological Sciences, University of Toronto Scarborough, Toronto, Canada UTSC BIOA01 Lab PRA20, BENCH5: PRA20 TA: Ashley Bramwell ________________________________________ Abstract: The process of photosynthesis is the most essential chemical processes that occurs on the planet. Most terrestrial organisms require

The acid-base titration experiment was a two week process. To begin the first week, a buret reading quiz was taken by each member of the group. When taking the quiz, it was recognized that 50 mL burrets can be measured to the nearest 0.01 mL (burrets are read from top to bottom). After the test was taken, a TA or the professor verified the accuracy of the reading. After testing the burret reading, the next step was to start the experiment by preparing approximately 0.1 M NaOH solution. First calculate

side-arm erlenmeyer flask with a stopper (50mL), pneumatic trough, tubing (50cm), electronic beam balance, graduated cylinder (50mL), spatula or chemical scoop, and weighing paper. Next, fill the graduated cylinder with water, then put a hand over it and flip into the pneumatic trough. While doing this step make sure the least bubbles get in. This can affect the results of the experiment. Stick the tubing into the cylinder and put the sodium bicarbonate into the side arm erlenmeyer flask. Put the

CLAIRE MUNTING 29/01/2018 Criterion C EFFECTS OF SURFACE AREA OF CALCIUM CARBONATE UPON RATE OF REACTION Calcium Carbonate Chips 1 Introduction: Within the current investigation, the effects of the surface area of Calcium Carbonate (CaCO3) in combination with Hydrochloric acid (HCl) upon its rate of reaction. CaCO3, commonly referred to as limestone, is an organic substance and is, in a sense, the crystallised “carbonic salt” of the element, calcium2. In addition to being a salt