Recovery of Elemental Copper from Copper (II) Nitrate
Recovery of Elemental Copper from Copper (II) Nitrate
Objectives: Students should be able to… recognize evidence(s) of a chemical change convert word equations into formula equations perform a series of chemical reactions in order to recycle the element copper determine the percent recovery of elemental copper
Challenge: How good and accurate a chemist are you? Given a solution of Cu(NO3)2, what percentage of elemental copper can you recover from the original solution?
Materials: 1 M copper (II) nitrate 3 M hydrochloric acid 2 M sodium hydroxide 600 mL beaker 250 or 400 mL beaker Ice water Distilled water Stirring rod Bunsen burner Ring stand Al wire, 18 gauge or heavier Graduated cylinder pH paper Watch glass, 90 mm Goggles Acetone
Procedures:
Conversion 1: THIS IS ALREADY COMPLETED FOR YOU!!!
Copper reacts with nitric acid to produce a brownish-orange gas called nitrogen dioxide. The blue color of the solution is characteristic of many copper compounds dissolved in water. You will be provided with 25 mL of 1 M solution of copper (II) nitrate. This solution contains 1.6 grams of copper. Since the brown nitrogen dioxide produced by the reaction is toxic, I have prepared this solution in advance for you.
Conversion 2: CONVERTING COPPER (II) NITRATE TO COPPER (II) HYDROXIDE
1. Obtain 25 mL of copper (II) nitrate
2. Test the copper (II) nitrate solution with pH paper. DO NOT DIP THE PAPER INTO THE SOLUTION!!! Instead, take your clean stirring rod and dip into the solution. Carefully touch the pH paper with the tip of the stirring rod. Record the pH results in your data.
3. Obtain 25 mL of 2 M sodium hydroxide and also test it with pH paper using the same method as stated above. Remember that a pH less than 7 indicates an acid…pH greater than 7 indicates a base…pH equal to 7 indicates a neutral solution. Record your results.
4. Fill your 600 mL beaker one third full of ice water.
Objectives: Students should be able to… recognize evidence(s) of a chemical change convert word equations into formula equations perform a series of chemical reactions in order to recycle the element copper determine the percent recovery of elemental copper
Challenge: How good and accurate a chemist are you? Given a solution of Cu(NO3)2, what percentage of elemental copper can you recover from the original solution?
Materials: 1 M copper (II) nitrate 3 M hydrochloric acid 2 M sodium hydroxide 600 mL beaker 250 or 400 mL beaker Ice water Distilled water Stirring rod Bunsen burner Ring stand Al wire, 18 gauge or heavier Graduated cylinder pH paper Watch glass, 90 mm Goggles Acetone
Procedures:
Conversion 1: THIS IS ALREADY COMPLETED FOR YOU!!!
Copper reacts with nitric acid to produce a brownish-orange gas called nitrogen dioxide. The blue color of the solution is characteristic of many copper compounds dissolved in water. You will be provided with 25 mL of 1 M solution of copper (II) nitrate. This solution contains 1.6 grams of copper. Since the brown nitrogen dioxide produced by the reaction is toxic, I have prepared this solution in advance for you.
Conversion 2: CONVERTING COPPER (II) NITRATE TO COPPER (II) HYDROXIDE
1. Obtain 25 mL of copper (II) nitrate
2. Test the copper (II) nitrate solution with pH paper. DO NOT DIP THE PAPER INTO THE SOLUTION!!! Instead, take your clean stirring rod and dip into the solution. Carefully touch the pH paper with the tip of the stirring rod. Record the pH results in your data.
3. Obtain 25 mL of 2 M sodium hydroxide and also test it with pH paper using the same method as stated above. Remember that a pH less than 7 indicates an acid…pH greater than 7 indicates a base…pH equal to 7 indicates a neutral solution. Record your results.
4. Fill your 600 mL beaker one third full of ice water.