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A variety of procedural errors can impact the effectiveness of the copper reaction cycle. Comment on the following documented errors:  When NaOH (aq) is added to the Cu (NO3)2 solution in Reaction B ( Cu(NO3)2(aq) + 2NaOH(aq) --> Cu(OH)2(s) + 2NaNO3(aq) ), the Cu(OH)2(s) occasionally does not precipitate immediately, and excess NaOH must be added. What other substance present in the reaction mixture might preferentially react with the NaOH and prevent precipitation of the Cu(OH)2? Explain. Students sometimes use HNO3 (aq) instead of H2SO4(aq) in Reaction E, Step 4, assuming that both strong acids will accomplish the same purpose. Briefly describe the consequences of this error.

A variety of procedural errors can impact the effectiveness of the copper reaction cycle. Comment on the following documented errors:  When NaOH (aq) is added to the Cu (NO3)2 solution in Reaction B ( Cu(NO3)2(aq) + 2NaOH(aq) --> Cu(OH)2(s) + 2NaNO3(aq) ), the Cu(OH)2(s) occasionally does not precipitate immediately, and excess NaOH must be added. What other substance present in the reaction mixture might preferentially react with the NaOH and prevent precipitation of the Cu(OH)2? Explain. Students sometimes use HNO3 (aq) instead of H2SO4(aq) in Reaction E, Step 4, assuming that both strong acids will accomplish the same purpose. Briefly describe the consequences of this error.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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  1. A variety of procedural errors can impact the effectiveness of the copper reaction cycle. Comment on the following documented errors: 
    1. When NaOH (aq) is added to the Cu (NO3)2 solution in Reaction B ( Cu(NO3)2(aq) + 2NaOH(aq) --> Cu(OH)2(s) + 2NaNO3(aq) ), the Cu(OH)2(s) occasionally does not precipitate immediately, and excess NaOH must be added. What other substance present in the reaction mixture might preferentially react with the NaOH and prevent precipitation of the Cu(OH)2? Explain.
    2. Students sometimes use HNO3 (aq) instead of H2SO4(aq) in Reaction E, Step 4, assuming that both strong acids will accomplish the same purpose. Briefly describe the consequences of this error. (Image of Experimental Procedure is attached)
  2. Students occasionally observe the formation of a solid white side product, sometimes appearing as a white residue on the walls of the test tube, in the recovery and isolation of the copper metal in Reaction E. Speculate on the identity of this white solid. (Use of online resources may be helpful.)
  3. Errors in experimental technique can result in the percent recovery of copper being too low or too high. Give at least one specific example of each type of error in technique and explain what could be done to ensure that those errors do not occur in the recovery. (Image of Experimental Procedure is attached)
Reaction C: Copper(II) Hydroxide > Copper(II) Oxide 1. Place the test tube in the boiling water bath; observe that the precipitate changes color from blue to black, which is evidence of formation of copper(II) oxide. Continue to heat the test tube until all the precipitate, including any precipitate on the walls of the test tube, turns completely black. (Note that the contents of the test tube do not have to be heated to dryness; the contents will appear to be "wet".) 2. Reaction D: Copper(II) Oxide → Copper(II) Sulfate 1. Carefully add no more than 20 drops of 6 M sulfuric acid to the solid CuO, agitate gently, and observe the change in the test tube. Do not add excess sulfuric acid. The disappearance of the black precipitate and simultaneous appearance of a sky-blue solution is evidence of the formation of soluble copper(II) sulfate. Continue to agitate the tube gently and allow all black solid to react. Consult your instructor if any black solid remains after 2-3 minutes. 2. Use a l-mL disposable transfer pipet to add 1 mL of deionized water to the test tube containing the copper(II) sulfate solution, and agitate gently to mix. Reaction E: Copper(II) Sulfate > Copper Metal (and Dissolution of Excess Magnesium Metal) 1. Obtain two (2) 1-cm magnesium strips for each test tube. Secure each test tube in the 100-mL beaker; add the Mg strips one at a time to the copper(II) sulfate solution. A rapid reaction should be observed, with vigorous generation of gas bubbles, generation of heat, loss of blue color from the solution, and formation of red-brown copper metal on the surface of the Mg strips. 2. If necessary, use a clean glass stirring rod to guide the Mg strips into the solution, break up the Cu metal forming on the surface of the Mg strips, and expose fresh Mg to the solution. Do not agitate vigorously. 3. Allow the reaction to continue for approx. 15 minutes. The solution should fade to light blue, evidence that most of the soluble copper(II) sulfate has been removed from solution by reduction to insoluble Cu metal. Consult instructor if the solution still has a significant blue color or if no copper metal has formed, especially if all the Mg has disappeared - more magnesium may be needed. 4. Only if necessary, add 1-2 drops of 6 M sulfuric acid to consume any unreacted Mg. Continue this process until few bubbles are observed and no unreacted Mg is apparent in the test tube. Do not add excess sulfuric acid. 5. Centrifuge the test tube containing the recovered Cu metal for 60 seconds at 1000 rpm and decant the supematant into the liquid waste beaker. Wash the red-brown Cu metal with two 1- mL portions of deionized watcr, followed by two 1-mL portions of acetone. Decant the supernatant after each washing, and immediately dispose of acetone waste in the "Organic Waste" bottle. Be careful to keep the recovered red-brown Cu metal in the test tube! If quantitative analysis of "Percent Recovery of Copper" is required, continue with steps 6- 7: 6. Remove as much liquid as possible, then secure the test tubes in a dry 100-mL beaker and place in a 150 °C oven for 15 minutes to allow the Cu metal to dry. 7. Remove test tubes from the oven and confirm visually that the recovered Cu metal is dry. Allow the test tubes to cool to room temperature, and confirm that the exterior of each tube is clean and dry - remove any visible white residue with a kimwipe. Record the combined mass of each test tube and recovered copper on the Report Sheet. Determine the mass of recovered copper by subtraction and calculate percent recovery. Disposal and Cleanup Dispose of aqueous waste in 'Aqueous Hazardous Waste' container, acetone in Organic Waste and recovered solid waste in Solid Waste container. Wash all glassware and rinse with deionized water. Return all glassware and equipment to original storage locations. Dispose of used test tubes in "Sharps" container. 4 | The Copper Cycle Fall18
Transcribed Image Text:Reaction C: Copper(II) Hydroxide > Copper(II) Oxide 1. Place the test tube in the boiling water bath; observe that the precipitate changes color from blue to black, which is evidence of formation of copper(II) oxide. Continue to heat the test tube until all the precipitate, including any precipitate on the walls of the test tube, turns completely black. (Note that the contents of the test tube do not have to be heated to dryness; the contents will appear to be "wet".) 2. Reaction D: Copper(II) Oxide → Copper(II) Sulfate 1. Carefully add no more than 20 drops of 6 M sulfuric acid to the solid CuO, agitate gently, and observe the change in the test tube. Do not add excess sulfuric acid. The disappearance of the black precipitate and simultaneous appearance of a sky-blue solution is evidence of the formation of soluble copper(II) sulfate. Continue to agitate the tube gently and allow all black solid to react. Consult your instructor if any black solid remains after 2-3 minutes. 2. Use a l-mL disposable transfer pipet to add 1 mL of deionized water to the test tube containing the copper(II) sulfate solution, and agitate gently to mix. Reaction E: Copper(II) Sulfate > Copper Metal (and Dissolution of Excess Magnesium Metal) 1. Obtain two (2) 1-cm magnesium strips for each test tube. Secure each test tube in the 100-mL beaker; add the Mg strips one at a time to the copper(II) sulfate solution. A rapid reaction should be observed, with vigorous generation of gas bubbles, generation of heat, loss of blue color from the solution, and formation of red-brown copper metal on the surface of the Mg strips. 2. If necessary, use a clean glass stirring rod to guide the Mg strips into the solution, break up the Cu metal forming on the surface of the Mg strips, and expose fresh Mg to the solution. Do not agitate vigorously. 3. Allow the reaction to continue for approx. 15 minutes. The solution should fade to light blue, evidence that most of the soluble copper(II) sulfate has been removed from solution by reduction to insoluble Cu metal. Consult instructor if the solution still has a significant blue color or if no copper metal has formed, especially if all the Mg has disappeared - more magnesium may be needed. 4. Only if necessary, add 1-2 drops of 6 M sulfuric acid to consume any unreacted Mg. Continue this process until few bubbles are observed and no unreacted Mg is apparent in the test tube. Do not add excess sulfuric acid. 5. Centrifuge the test tube containing the recovered Cu metal for 60 seconds at 1000 rpm and decant the supematant into the liquid waste beaker. Wash the red-brown Cu metal with two 1- mL portions of deionized watcr, followed by two 1-mL portions of acetone. Decant the supernatant after each washing, and immediately dispose of acetone waste in the "Organic Waste" bottle. Be careful to keep the recovered red-brown Cu metal in the test tube! If quantitative analysis of "Percent Recovery of Copper" is required, continue with steps 6- 7: 6. Remove as much liquid as possible, then secure the test tubes in a dry 100-mL beaker and place in a 150 °C oven for 15 minutes to allow the Cu metal to dry. 7. Remove test tubes from the oven and confirm visually that the recovered Cu metal is dry. Allow the test tubes to cool to room temperature, and confirm that the exterior of each tube is clean and dry - remove any visible white residue with a kimwipe. Record the combined mass of each test tube and recovered copper on the Report Sheet. Determine the mass of recovered copper by subtraction and calculate percent recovery. Disposal and Cleanup Dispose of aqueous waste in 'Aqueous Hazardous Waste' container, acetone in Organic Waste and recovered solid waste in Solid Waste container. Wash all glassware and rinse with deionized water. Return all glassware and equipment to original storage locations. Dispose of used test tubes in "Sharps" container. 4 | The Copper Cycle Fall18
The Copper Cycle Experiment Procedure Materials: Two (2) large disposable test tubes, l00-mL beaker, two pre-cut copper wire pieces, disposable transfer pipets, deionized water, 15 M HNO3, 6 M NaOH, 6 M H2SO4, small waste beaker, 150-mL beaker with boiling stones, hot plate, pre-cut Mg strips, acctone General Instructions: 1. Students must wear laboratory goggles, lab aprons, and disposable gloves at all times. 2. The experiment requires use of concentrated acids and bases, a reactive metal (Mg), and acetone. Spills of any type should be reported immediately to the instructor and cleaned up carefully. 3. Bottles of concentrated acids and bases must remain in the fume hoods at all times. 4. For each Reaction A - E described below, record detailed observations, as well as a balanced molecular equation and a balanced net ionic equation, on the Report Sheet. 5. Students will complete two trials of the procedure concurrently. Using permanent marker, label test tubes with "Trial I" and "Trial 2", as well as initials. Complete identical procedural steps with each test tube. 6. Check with lab instructor to determine if quantitative analysis of the "Percent Recovery of Copper" is required for the lab report; if quantitative analysis is required, record all masses to the nearest 0,000lg. Reaction A: Copper Metal → Copper(II) Nitrate 1. If required, record the mass of labeled test tube on the Report Sheet. 2. Obtain a pre-cut length of copper wire (approx. 1.5 cm); fold the wire into a circular shape, and place in test tube. If required, record the combined mass of the test tube and copper wire on the Report Sheet and determine the mass of the copper wire by subtraction (approximately 0.02 g). 3. Place test tube in a clean 100-mL beaker. Warning - Perform this step in the fume hood and do not inhale the evolved nitrogen dioxide gas! Use a disposable 1-mL transfer pipet to add 5 - 6 drops (no more than 0.25 mL) of concentrated (15 M) nitric acid. Do not add an excess of nitric acid. Allow the copper wire to react (disappear) completely before continuing to the next step. If the copper wire has not disappeared after 10 minutes of gentle mixing, consult your instructor. 4. Add -l mL of deionized water (using plastic pipet) to the test tube and mix by gently agitating the test tube. Do not remove the test tube and beaker from the fume hood until the brown gas has dissipated. [Looking ahead – Prepare a boiling water bath for use in Part C by adding 100 mL of tap water and a few boiling stones to a 150-mL beaker, using a hot plate to heat the water to boiling.] Reaction B: Copper(II) Nitrate > Copper(II) Hydroxide 1. Slowly add 10 drops of 6 M NAOH to the test tube with gentle agitation. Fomation of the blue precipitate Cu(OH)2 should be observed; the test tube may feel warm to the touch. 2. Allow the test tube to cool briefly, then add an additional 10 drops of 6 M NAOH and gently agitate the solution to assure complete mixing. Centrifuge the test tube for 60 seconds at 1000 rpm. 3. Remove the test tube from the centrifuge and observe; a blue precipitate should be at the bottom of the test tube, and a colorless or very light blue liquid (the "supernatant") should be visible above the precipitate. Consult your instructor if no precipitate is visible, or if the supernatant still has a significant blue tint. 4. Test for complete precipitation of copper(II) hydroxide by adding 3 more drops of 6 M NaOH to the supernatant without agitation. If a “ribbon" of additional precipitate forms, add 5 more drops of NaOH, agitate gently to mix. Centrifuge the test tube for an additional 60 seconds at 1000 rpm. Remove the test tube from the centrifuge and confirm that the blue precipitate is at the bottom of the test 5. tube. Carefully decant (pour off) the colorless supernatant from the test tube into a small liquid waste beaker; alternatively, use a disposable transfer pipet to withdraw the supematant from the test tube. 3| The Copper Cycle Fall 18
Transcribed Image Text:The Copper Cycle Experiment Procedure Materials: Two (2) large disposable test tubes, l00-mL beaker, two pre-cut copper wire pieces, disposable transfer pipets, deionized water, 15 M HNO3, 6 M NaOH, 6 M H2SO4, small waste beaker, 150-mL beaker with boiling stones, hot plate, pre-cut Mg strips, acctone General Instructions: 1. Students must wear laboratory goggles, lab aprons, and disposable gloves at all times. 2. The experiment requires use of concentrated acids and bases, a reactive metal (Mg), and acetone. Spills of any type should be reported immediately to the instructor and cleaned up carefully. 3. Bottles of concentrated acids and bases must remain in the fume hoods at all times. 4. For each Reaction A - E described below, record detailed observations, as well as a balanced molecular equation and a balanced net ionic equation, on the Report Sheet. 5. Students will complete two trials of the procedure concurrently. Using permanent marker, label test tubes with "Trial I" and "Trial 2", as well as initials. Complete identical procedural steps with each test tube. 6. Check with lab instructor to determine if quantitative analysis of the "Percent Recovery of Copper" is required for the lab report; if quantitative analysis is required, record all masses to the nearest 0,000lg. Reaction A: Copper Metal → Copper(II) Nitrate 1. If required, record the mass of labeled test tube on the Report Sheet. 2. Obtain a pre-cut length of copper wire (approx. 1.5 cm); fold the wire into a circular shape, and place in test tube. If required, record the combined mass of the test tube and copper wire on the Report Sheet and determine the mass of the copper wire by subtraction (approximately 0.02 g). 3. Place test tube in a clean 100-mL beaker. Warning - Perform this step in the fume hood and do not inhale the evolved nitrogen dioxide gas! Use a disposable 1-mL transfer pipet to add 5 - 6 drops (no more than 0.25 mL) of concentrated (15 M) nitric acid. Do not add an excess of nitric acid. Allow the copper wire to react (disappear) completely before continuing to the next step. If the copper wire has not disappeared after 10 minutes of gentle mixing, consult your instructor. 4. Add -l mL of deionized water (using plastic pipet) to the test tube and mix by gently agitating the test tube. Do not remove the test tube and beaker from the fume hood until the brown gas has dissipated. [Looking ahead – Prepare a boiling water bath for use in Part C by adding 100 mL of tap water and a few boiling stones to a 150-mL beaker, using a hot plate to heat the water to boiling.] Reaction B: Copper(II) Nitrate > Copper(II) Hydroxide 1. Slowly add 10 drops of 6 M NAOH to the test tube with gentle agitation. Fomation of the blue precipitate Cu(OH)2 should be observed; the test tube may feel warm to the touch. 2. Allow the test tube to cool briefly, then add an additional 10 drops of 6 M NAOH and gently agitate the solution to assure complete mixing. Centrifuge the test tube for 60 seconds at 1000 rpm. 3. Remove the test tube from the centrifuge and observe; a blue precipitate should be at the bottom of the test tube, and a colorless or very light blue liquid (the "supernatant") should be visible above the precipitate. Consult your instructor if no precipitate is visible, or if the supernatant still has a significant blue tint. 4. Test for complete precipitation of copper(II) hydroxide by adding 3 more drops of 6 M NaOH to the supernatant without agitation. If a “ribbon" of additional precipitate forms, add 5 more drops of NaOH, agitate gently to mix. Centrifuge the test tube for an additional 60 seconds at 1000 rpm. Remove the test tube from the centrifuge and confirm that the blue precipitate is at the bottom of the test 5. tube. Carefully decant (pour off) the colorless supernatant from the test tube into a small liquid waste beaker; alternatively, use a disposable transfer pipet to withdraw the supematant from the test tube. 3| The Copper Cycle Fall 18
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