CHEM 2070 LAB
Purposes of Experiment: To synthesize a transition metal complex, potassium tris (oxalate)ferrate(III) trihydrate in a two step process, to learn new laboratory techniques such as decantation, recrystallization, gravity and suction filtration. Also the purpose of the experiment is to determine the actual, theoretical, and percent yields of product, and characterize the final compound by determining the number of waters of hydration by gravimetric analysis
List of Observations:
After adding (15 mL distilled water/5 drops of 3 M H2SO4) to ferrous ammonium sulfate hexahydrate in the 200 mL beaker, the solution was light green/blue
After adding 25 mL of C2H2O4 to solution in beaker, the color of the solution became a pale green, and after stirring solution, it became a yellow/orange color.
After trying to decant the solution, and attempting to keep the precipitate in the beaker, which was difficult to do as some of the precipitate left the solution along with the hot supernatant liquid in the heated solution, 20 mL of distilled water was added to the precipitate.
While decanting the hot supernatant liquid from the solution for a second time, it was equally difficult trying to keep the precipitate from leaving the beaker, as it was the first time.
After adding 20 mL of potassium oxalate to the solution with the precipitate, the solution’s color became dark red.
After supporting a thermometer, using a ring stand, clamp, and split one-hole stopper, placing thermometer in solution, and adding 20 mL H2O2 slowly while using a magnetic stir-bar, and heating solution to 40 C, the solution turned black, and then became a rusty brown color later, after stirring.
After heating solution, it produced bubbles, showing us the process of oxidization in reaction, and the color of the solution became dark brown.
After stirring solution, allowing it to heat until boiling, and adding 8 mL of 1 M H2C2O4 (first 5 mL at once, the next 3 mL slowly), the solution
List of Observations:
After adding (15 mL distilled water/5 drops of 3 M H2SO4) to ferrous ammonium sulfate hexahydrate in the 200 mL beaker, the solution was light green/blue
After adding 25 mL of C2H2O4 to solution in beaker, the color of the solution became a pale green, and after stirring solution, it became a yellow/orange color.
After trying to decant the solution, and attempting to keep the precipitate in the beaker, which was difficult to do as some of the precipitate left the solution along with the hot supernatant liquid in the heated solution, 20 mL of distilled water was added to the precipitate.
While decanting the hot supernatant liquid from the solution for a second time, it was equally difficult trying to keep the precipitate from leaving the beaker, as it was the first time.
After adding 20 mL of potassium oxalate to the solution with the precipitate, the solution’s color became dark red.
After supporting a thermometer, using a ring stand, clamp, and split one-hole stopper, placing thermometer in solution, and adding 20 mL H2O2 slowly while using a magnetic stir-bar, and heating solution to 40 C, the solution turned black, and then became a rusty brown color later, after stirring.
After heating solution, it produced bubbles, showing us the process of oxidization in reaction, and the color of the solution became dark brown.
After stirring solution, allowing it to heat until boiling, and adding 8 mL of 1 M H2C2O4 (first 5 mL at once, the next 3 mL slowly), the solution