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Transcript of Green Crystal
2. Pour the hot solution into the beaker containing the FeCl3 solution and stir.
3. Cool the solution for 30-45 minutes by placing the beaker in a larger beaker containing ice and water. Crystals should form during this time. Take care that the beaker of product does not sink in the water as the ice melts.
4. After giving the crystals time to form, carefully pour off and discard the solvent without removing any crystals (decantation).
5. Add 40 mL of distilled water to the crystals, heat gently with stirring to dissolve the crystals.
6. Cool the solution for 30 minutes by placing the beaker in a larger beaker containing ice and water. Crystals should form.
Sources of Error
1. While decanting the crystals from the water, it is impossible to prevent the crystals from escaping, resulting in too little product.
The purpose of this experiment is to synthesize a compound (Iron Oxalate) as close to 100% yield as possible. By crystallizing and decanting, the product can be purified and separated from the water of hydration.
Reactions/Equations and Results
Safety and Hazards
1. Use caution when dealing with heat(from hot plates).
2. Acetone is flammable.
3. If solutions come in contact with skin, wash with soap and water.
4. Wear goggles and aprons.
5. Iron compounds may stain clothing permanently.
6. Avoid overheating resulting in violent boiling when heating liquids.
1. Set up a vacuum filtration system, then filter the crystals vacuum filtration using a Buchner funnel and a clean filter flask.
2. Wash the crystals twice with ice water. Use less than 10 mL of ice water for each wash and work quickly to avoid dissolving the product in the wash water. Finally wash the crystals twice with 10 mL portions of acetone.
3. Spread the crystals in the bottom of a clean, dry 250 mL beaker and place in your closed drawer to air dry.
4. Using the 0.001 g balance, weigh the clean vial with its lid. Record the mass of the bottle plus lid.
5. Before the next lab period, when the crystals are dry, place them in the preweighed vial, screw on the lid, and weigh the bottle plus crystals to the nearest 0.001 g. Calculate the mass of the crystals and record it in your notebook. Wrap the vial containing your green solid in a brown bottle.
1. Assuming that all of the Fe originally in FeCl3 * H2O ends up in the product, KxFe(C2O4)y * zH2O, how many moles of product should be obtained?
A: 3.20g FeCl3 * 6H2O X (mol FeCl3 * 6H2O/270g FeCl3 * 6H2O) X (mol Fe/mol FeCl3 * 6H2O) X (mol KxFe(C2O4)y * zH2O/mol Fe)
= 0.02 mol KxFe(C2O4)y * zH2O
2. What additional information would you need to calculate a percent yield?
A: In order to calculate a percent yield, the theoretical yield is required.
In this experiment, you will react an aqueous solution containing 3.20g FeCl3 * 6H2O (270g/mol) with an aqueous solution containing excess K2C2O4 to produce product KxFe(C2O4)y * zH2O
Synthesis of Iron Oxalato (Green Crystal Formation)
2. While vacuum filtering, the crystals dissolving and decomposing from exposure to light will yield too little product.
Day 1 Results
Volume of FeCl3 used: 16.00mL
Mass of FeCl3 used : 6.40g
Mass of Potassium Oxalate used: 24.2951g
Mass of Crystals: 7.0336g
Day 2 Results
Iron (III) Chloride
Chris Lee and Jessica Lee
xK^+(aq) + Fe^3+(aq) + yC2O4^2-(aq) + zH2O --> KxFe(C2O4)y * zH2O(s)