Find alternate sources of aluminum. Aluminum can be found as foil, pie pans, soda cans, ash trays, sheet scraps, and molding (as in flashing). Determine whether aluminum from any of these sources could be used to displace copper from Basic Copper Chloride(WSDTY) solution. If any are not usable, explain why.
Advance Preparation: Make this a class-sharing activity by assigning different groups to different sources of aluminum. Each student pair needs about 30 mL of 0.10 M copper(II) chloride and a piece of aluminum (2 cm x 7 cm). Foil, pie pans, and soda cans are too thin and the aluminum flakes off. Soda cans also have a plastic coating. Others work well if they are pure aluminum and not an alloy.
Determine the amount of aluminum in the filtrate. Slowly and cautiously evaporate the water from the filtrate which was saved during the laboratory exercise. Use either the Bunsen burner or hot plate. When there is about 5 mL of filtrate, use beaker grips to remove the beaker from the heat source. Turn off the heat source. Allow the water to evaporate by itself. When the salt is dry, find the mass of the beaker and salt. (Heat to a constant mass.) Since this salt is aluminum chloride, AlCl3, calculate the percent of aluminum in aluminum chloride. Calculate how many grams of aluminum reacted.
Advance Preparation: Materials needed per pair of students are a balance, a burner or hot plate, and the filtrate from the original activity in a beaker whose mass was determined. The anticipated answer is 20.2% of the aluminum chloride mass . Determine the percent of water in a hydrate such as blue copper(II) sulfate pentahydrate.
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Advance Preparation: Make this a class-sharing activity by assigning different groups to different sources of aluminum. Each student pair needs about 30 mL of 0.10 M copper(II) chloride and a piece of aluminum (2 cm x 7 cm). Foil, pie pans, and soda cans are too thin and the aluminum flakes off. Soda cans also have a plastic coating. Others work well if they are pure aluminum and not an alloy.
Determine the amount of aluminum in the filtrate. Slowly and cautiously evaporate the water from the filtrate which was saved during the laboratory exercise. Use either the Bunsen burner or hot plate. When there is about 5 mL of filtrate, use beaker grips to remove the beaker from the heat source. Turn off the heat source. Allow the water to evaporate by itself. When the salt is dry, find the mass of the beaker and salt. (Heat to a constant mass.) Since this salt is aluminum chloride, AlCl3, calculate the percent of aluminum in aluminum chloride. Calculate how many grams of aluminum reacted.
Advance Preparation: Materials needed per pair of students are a balance, a burner or hot plate, and the filtrate from the original activity in a beaker whose mass was determined. The anticipated answer is 20.2% of the aluminum chloride mass . Determine the percent of water in a hydrate such as blue copper(II) sulfate pentahydrate.
Click Copper Acetate to learn about more information
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