Copper Cycle. Density - Accuracy and Precision

The Copper Cycle Introduction In this experiment, you will carry out a series of reactions starting with copper metal. This will give you practice handling chemical reagents and making observations. It is typical for scientists to observe materials before they react, what happens during a reaction and how it looks when the reaction has come to completion. The product of the final reaction will be copper metal and the percent copper that is recovered will be calculated. Most of the background material for this laboratory will be covered in greater detail in the lecture course later in the semester. Here are some notes on the reactions you will perform: Step I: Chemistry The different copper species obtained in each part is shown in Equation 1 below: Cu(s) Part I Cu2+(aq) Part II Part III Cu(OH)2(s) CuO(s) Part IV Cu2+(aq) Part V Cu(s) blue I. Oxidizing Copper Metal with Concentrated Nitric Acid, HNO3(aq) The first step involves transforming Cu metal to copper(II) ions, Cu2+, using concentrated nitric acid, HNO3(aq). At the same time, the nitrate ions (NO3–) undergo a series of reactions to form nitrogen monoxide, NO. This product rapidly reacts with oxygen in the air to form NO2, a brown gas. The presence of Cu2+(aq) makes the solution blue. When the reaction mixture is diluted with water, the Cu2+ ions are hydrated (surrounded by water) to form the octahedral complex ion, [Cu(H2O)6]2+, as shown below. Six water molecules (shown as red O and white H atoms) are bonded to a Cu2+ ion (shown in gray as the central atom). Cu2+(aq) + 6 H2O(l)  [Cu(H2O)6]2+(aq) Figure 1 Step II: Chemistry II. Precipitating Cu(OH)2(s) with NaOH(aq) In Part II, two reactions are carried out by adding NaOH(aq). In the first reaction, the hydroxide ions (OH–) from the NaOH(aq) neutralize the excess hydronium ions (H3O+) left over from the previous part: H3O+(aq) + OH–(aq)  2 H2O(l) Once all the H3O+ ions are neutralized, additional OH– ions react with the Cu2+ ion to form Cu(OH)2 precipitate. Once all the Cu2+ ions have reacted, no more precipitate forms. Adding more OH– ions makes the solution basic, so it can turn red litmus paper blue. Figure 2 shows the stepwise reaction of Cu2+ with NaOH. page 1 of 9 Figure 2: Step-wise Illustration of the Precipitation of Cu(OH)2 in Part II – Remember: [Cu(H2O)]2+ indicates the same substance as Cu2+. OH- H3O+ [Cu(H2O)6]+2 H3O+ [Cu(H2O)6]+2 H3 O+ At end of Part I OH- H3O+ OH[Cu(H2O)6]+2 + OH- H3O [Cu(H2O)6]+2 [Cu(H2O)6]+2 OH- OH- OHOH- OH- [Cu(H2O)6]+2 [Cu(H2O)6]+2 OH- H3O+ OHPart II Step 1 OH- neutralizes H3O+ OH- Cu(OH)2 Part II Step 2 OH- reacts with [Cu(H 2O)6]+2 to form Cu(OH)2(s) Cu(OH)2 Part II Step 3 Excess OH - makes the solution basic  1st Beaker: At the end of Part I, hydrated copper complex, Cu2+ are present, making the solution blue, and excess hydronium ions (H3O+) remain from the nitric acid used.  2nd Beaker: Adding NaOH(aq) to the blue solution results in the OH– ions neutralizing the H3O+ ions to form water: H3O+(aq) + OH–(aq)  2 H2O(l). The Na+ ions and resulting water molecules are not shown.  3rd and 4th Beakers: Once all the H3O+ are neutralized, adding more NaOH(aq) results in the OH– ions reacting with the Cu2+ to form the blue Cu(OH)2(s) precipitate shown at the bottom of the beaker. Water molecules released from the complex ion are not shown.  5th Beaker: When all of the Cu2+ ions have been converted to Cu(OH)2(s) precipitate, adding more NaOH(aq) results in unreacted OH– ions in solution, which makes the solution basic. Red litmus paper can be used to confirm the solution is basic. Note that the solution is no longer blue since no Cu2+ ions are present in the solution. Step III: Chemistry III. Converting solid Cu(OH)2 to solid CuO In Part III of the sequence, the reaction mixture is heated. This transforms the Cu(OH)2 precipitate to CuO precipitate. The CuO precipitate is separated from the solution, called the supernatant liquid, using a method called gravity filtration. The mixture is filtered using a filter funnel, and the solid is collected on filter paper. The supernatant liquid runs through the filter paper and collects in a beaker. This resulting filtered solution is called the filtrate. Step IV: Chemistry IV. Dissolving CuO(s) with sulfuric acid, H2SO4(aq) In Part IV, the CuO precipitate is dissolved using sulfuric acid, H2SO4(aq). This redox reaction returns copper to its aqueous phase. Step V: Chemistry V. Reducing Cu2+ ions with Zinc Metal In Part V, zinc metal (Zn) is added to the copper solution to convert the copper ions back to copper metal, Cu(s). The resulting solution will contain colorless zinc ions, Zn2+(aq) and copper solid. page 2 of 9 Visible evidence of this reaction is observed as bubbles of hydrogen gas are released from the solution. (Since the H3O+ ions do not dissolve the Cu metal, the amount of copper yielded is not affected by excess acid.) Identify the gas displaced from the acid in this reaction: _________________________ When the solution becomes colorless, all of the Cu2+ ions have been converted to Cu metal. All of the excess Zn metal is also converted to Zn2+ ion by the excess H3O+ ions from the sulfuric acid, H2SO4(aq),used to dissolve the CuO precipitate in Part IV. Once all the Zn metal is dissolved, the Cu metal can be isolated by decanting, or pouring off, the supernatant liquid. The Cu will then be rinsed, dried, and weighed as described in the procedure. For more information: Chemistry: Atom’s First by OpenStax section 7.2 – “Classifying Chemical Reactions” Equations to use for the calculations: mass of evaporating dish with copper – mass of empty evaporating dish = mass of copper recovered Percent of copper recovered = mass of copper recovered X 100 mass of original copper sample Materials: weighing paper filter paper copper pieces zinc mesh balance 150-mL beaker 250-mL beaker 400-mL beaker forceps 10-mL graduated cylinder concentrated HNO3 (in fume hood) 6M NaOH 3M H2SO4 litmus paper watch glass glass stir rod ring stand wire quaze 2 ring clamps Bunsen burner hot plate striker funnel plastic pipet evaporating dish oven DI water bottle calculator Procedure Part I: Oxidizing Cu with concentrated nitric acid, HNO3(aq) 1. Use forceps to transfer about 0.35-0.40 g of Cu strips onto tared weighing paper. See techniques “Transferring solids”. Record the mass of the Cu strips. Transfer the Cu strips into a clean 250-mL beaker labeled with one of your group member’s initials. Record the appearance of the copper metal in your lab report. 2. In a fume hood, use a 10-mL graduated cylinder to carefully measure about 3 mL of concentrated nitric acid, HNO3(aq). See techniques ”Transferring liquids” and “Reading a meniscus in various pieces of glassware”. Slowly pour the nitric acid onto the Cu strips in the page 3 of 9 beaker, swirling the beaker to maximize contact between the Cu and nitric acid until all of the solid Cu has dissolved and the NO2 gas has escaped. Keep the reaction beaker in the hood until all the toxic brown NO2 gas is gone, and keep your face away from the hood to avoid inhaling nitric acid fumes and NO2 gas. Describe the reaction between HNO3 and the Cu metal in your lab report. CAUTION: Concentrated nitric acid is highly corrosive, so it can cause severe chemical burns and damage clothing. Handle with care and avoid breathing the fumes. Any nitric acid spilled on skin must be rinsed immediately with water for 15 minutes. Any acid spilled on your work area must be neutralized then the entire area should be washed and dried. CAUTION: Concentrated nitric acid reacts with copper metal to form brown toxic NO2 gas. Leave the reaction beaker in the fume hood until all of the brown gas is vented in the hood. 3. Dilute the resulting solution with about 10 mL of deionized water. Describe the appearance of the resulting solution containing Cu2+ in your lab report. Part II: Precipitating Cu(OH)2(s) with NaOH(aq) 1. While constantly stirring the Cu solution, slowly add 6M NaOH(aq) from the dropper bottles. CAUTION: Sodium hydroxide (NaOH) can easily damage eyes. It is corrosive and can cause chemical burns and damage clothing. Any NaOH splashed into eyes or spilled on skin must be rinsed immediately with water for 15 minutes. Any base spilled on your work area must be neutralized then the entire area should be washed and dried. 2. Test the solution with litmus paper until a change is observed. Think about which litmus paper you should use and what change you should be looking for. See technique “Litmus paper test for acids and bases”. Record what you observe in your lab report. Part III: Converting Cu(OH)2(s) to CuO(s) 1. Set up a ring stand as shown in the figure at the right. Set up a ring clamp, and put a wire gauze on top of it. Above it, attach another ring clamp with a diameter large enough to go around a 250-mL beaker. You are going to set your 250 mL beaker on the lower ring and gauze. The upper clamp will hold the beaker in place so it does not fall. 2. Add about 30-40 mL of deionized water to your reaction beaker from Part II. Carefully place the beaker on the ring stand inside the upper ring. See technique “Using a Bunsen burner”. CAUTION: Gently heat the beaker over a medium flame. (Set the inner cone of the Bunsen burner flame to a height of about 1.5 inch and the lower ring stand about 4 inches above the top of the Bunsen burner). Constantly stir the solution with the glass end of the stirring rod until all the blue precipitate turns black, and the solution is clear. If the solution starts to bump or boil, immediately remove the beaker from the heat and let the solution cool slightly. Describe what happens to the Cu(OH)2 precipitate upon heating in your lab report. 3. Allow the beaker and contents to cool. While they are cooling, set up the gravity filtration apparatus. See technique “Separating a liquid from a solid”. Obtain a second ring stand, and page 4 of 9 attach a ring clamp that is small enough to hold the plastic funnel. Properly fold a piece of filter paper and place it inside the plastic funnel, wetting it with DI water to hold it in place.  Place the plastic funnel in the small ring clamp, and place a 400-mL beaker beneath it to collect the filtrate (the liquid that goes through the filter paper). The funnel’s stem should be just inside the beaker to prevent splashing. Use the markings on a clean 150-mL beaker to measure out about 15 mL of deionized water. Boil the water on a hotplate to wash the precipitate from step 2.  When the 250-mL reaction beaker has cooled to room temperature, pour the CuO precipitate into the funnel to filter the contents. Transfer the last traces of the solid from the reaction beaker into the funnel, using a stream of deionized water.  Use a disposable pipet to wash the precipitate on the filter paper using the hot deionized water heated in the 150-mL beaker. Allow each portion of hot water to drain through the filter paper into the beaker below before adding the next portion. Use 15 mL of the hot deionized water to thoroughly wash the CuO precipitate.  Wash the 250-mL beaker, and rinse with deionized water. Replace the 400-mL beaker under the filter funnel with the clean 250-mL beaker. Discard the filtrate (solution) collected in the 400-mL beaker into the properly labeled waste container. Clean and dry the 400 mL beaker for use in Part V. 4. Keep the CuO solid on the filter paper for use in Part IV. Part IV: Dissolving CuO(s) with sulfuric acid, H2SO4(aq) 1. Add about 10 mL of 3M sulfuric acid, H2SO4 (check the label before pouring), to the funnel to dissolve the CuO precipitate. Allow the solution to drain through the funnel to the rinsed 250-mL beaker. Repeat the procedure until all of the CuO solid dissolves to Cu2+ ions. Use as little of the sulfuric acid as possible in this step. You may use a disposable pipet to transfer and direct the H2SO4. Describe the reaction between the CuO precipitate and the H2SO4 in your lab report. CAUTION: Sulfuric acid, H2SO4(aq), is corrosive, so it can cause severe chemical burns and damage clothing. Handle with care and avoid breathing the fumes. Any sulfuric acid spilled on skin must be rinsed immediately with water for 15 minutes. Any acid spilled on your work area must be neutralized, and the entire area should be washed and dried. 2. Use your water bottle to wash the last traces of solution from the empty funnel into the 250-mL beaker which now contains the acid solution and aqueous Cu2+ ions. Keep this resulting solution for use in the Part V. Part V: Reducing Cu2+ ions with Zn Metal 1. Perform this step in the hood. Use a weighing boat, measure and transfer about 1 g of Zn mesh to the Cu2+ solution in the 250-mL beaker. Constantly stir the mixture with a glass stirring rod. Do not use any metal object that will react with the acid to stir the solution. Continue stirring until all the Cu2+ ions have been reduced to Cu metal as indicated by the solution becoming colorless. Dissolve any excess Zn by adding a few drops of 3M H2SO4(aq). Describe your observations of the reduction of Cu2+ to Cu metal. 2. Perform this step at your desk. Allow the Cu metal to settle at the bottom of the beaker. Without losing any of the solid, carefully decant (pour off) as much of the supernatant liquid as possible into page 5 of 9 a 400-mL beaker. Some liquid will remain in the first beaker with the Cu metal. Wash the Cu metal 3 times using 20-mL portions of deionized water by stirring and then allowing the solid to resettle. Again, decant the liquid into the 400-mL beaker each time. 3. Weigh a clean, dry evaporating dish. Transfer the Cu metal and any remaining water into the evaporating dish using a stream of deionized water. Decant most of the water from the evaporating dish. Use a disposable pipet to remove as much remaining water from the evaporating dish without losing any solid. Wick any remaining water with a paper towel. 4. Write one of your group members’ names on a folded piece of paper towel. Place your group’s evaporating dish on the paper towel in the oven to let the Cu completely dry. Check it after about 10 minutes. If the copper pieces are loose then it is dry. If it appears black in color, then the copper has been heated too much and has turned to copper (II) oxide. 5. When the Cu appears completely dry, let the evaporating dish cool to room temperature, and weigh the evaporating dish with the Cu. Record the final mass in your lab report. 6. Calculate the mass of copper recovered and the percent recovery for the copper cycle. Please refer to the Laboratory Techniques Document on the CHM151LL Course Website for more detailed techniques and images of lab equipment. Clean-Up: Rinse everything well with tap water followed by a quick DI water rinse. Clean your benchtop. Put all equipment back exactly where you found it. page 6 of 9 Name: _____________________________ Partners: ________________________ The Copper Cycle Lab Report Turn in Pages 7-8 as your graded lab report Data: Data Table 1: Mass of Copper Mass of Copper Pieces (Part I) Mass of Empty Evaporating Dish Mass of Evaporating Dish with Recovered Copper (Part IV) Observations: (the observations for each step should include detailed accounts of the appearance of reactants before the reaction, the appearance of the reactants during the reaction, and the appearance of the products after the reaction. Please note you do NOT need to write a balanced chemical equation, just observe what you see. Your observations should include state(s) of matter, color, texture, smell, etc. where applicable. If your observations are not detailed, you may not receive full credit. One step also requires a specific chemical test using litmus paper to check for acidity. Be sure record the results of these tests as well.) Part I: Part II: Part III: page 7 of 9 Part IV: Part V: Calculations for Data Table 1: Results: Results Table 1: Mass and Percent of Copper Recovered Mass of Copper Recovered Percent of Copper Recovered Conclusion: (5 pts) Summarize the results from the experiment. Be sure to include data to support page 8 of 9 Post-Lab Questions – These questions will not be graded as part of your lab report grade. You will be responsible for the information in these questions and able to answer these or similar questions on the post-lab quiz at the start of next week’s lab period. Questions will also be similar to your lab report data, observations, calculations, and results. 1. A student performed the copper cycle experiment and found they had an 89.33% recovery of copper. Using the information given in the data table below, calculate the mass of copper the student must have started with in Part I of the copper cycle. Show all your work! Mass of Copper Pieces (Part I) Mass of Empty Evaporating Dish Mass of Evaporating Dish with Recovered Copper (Part IV) 2.8951 g 3.2813 g 2. Indicate whether the following procedural errors would result in an incorrectly high or incorrectly low percent recovery. Circle and explain your answer. Include names or formulas of the substances or ions that are present that helped you make your decision. a. The solution was not basic before being heated in Part III. High Low b. In Part III, the solution was poured into the funnel until it went above the top of the filter paper, and some black solid was disposed of with the filtrate. High Low c. The solution decanted in Part V was slightly blue in color. High Low d. After all the copper metal was obtained in Part V, it took too long for the excess Zn granules to dissolve, so a student added concentrated nitric acid to the solution, resulting in a brown gas. High Low e. In Part V, the copper metal was weighed while it was still damp. High Low 3. In Part IV, dissolving CuO(s) with sulfuric acid, H2SO4(aq), what ions would you expect to see in the resulting solution? Include all possible ions in the beaker. page 9 of 9