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Green Crystals Lab

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To achieve the goals set forth for this laboratory experiment, the green crystals first needed to be constructed. Using the Dial-O-Gram, 8.3 grams of K2C2O4 H2O was collected and placed into a 125 mL flask. Following that step, 25 mL of deionized water was added to the same flask and the solid substance was alloted time to dissolve. Once this was completed, 4.1g of FeCl3 6H2O was collected using the Dial-O-Gram and placed into a 150 mL beaker. To aid in the dissolving of the solid, 10 mL of DI water was added to the beaker. From that point, the oxalate solution was added to the iron (III) chloride solution in the 150 mL beaker and stirred. To ensure the highest percent yield, any remaining K2C2O4 was rinsed with 3 mL of DI water and added to the 150 mL beaker. After all solutions were …show more content…

To start, two samples of 0.12501 grams and 1.2499 grams of the crystals was weighed out, using an analytical balance, and placed into two Erlenmeyer flasks. Each flask then received 60 mL of DI water, 6 mL of 6M H2SO4, and 1 mL H3PO4. Then, one flask was placed on a hotplate and heated to 80°C. While the solution was being heated, 120 mL of 6 molar potassium permanganate, KMnO4, was obtained and used to first rinse a burette and then fill the burette for titration procedures. After the solution had reached the desired temperature of 80°C, a stir bar was placed inside the flask and the titration using the KMnO4 solution began. The titration process was considered completed when the solution had changed color from clear to a light pink. Once the color change was apparent, the final volume of the KMnO4 solution used was recorded. The process was then completed once more to ensure accurate results.The number of moles of MnO4- used and the number of moles of C2O42- in the sample were then calculated and then the moles of C2O42- was converted to

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