I am required to design an experiment which will allow me to produce exactly 12.5g of pure dry Copper Hydroxide. I need to include equipment required, Chemicals required, step by step method and any particular limitations/cautions which must be exercised whilst following the experiment. Thanks heaps
I don't think anyone here will be willing to write a three or four page report but allow me to give you some hints.
You really don't know the purity of many of the salts of copper; however, starting with copper wire or copper turnings might be a good possibility. Copper wire can be purchased with either essentially 100% purity. So you need to calculate how much copper to start your experiment with. Exactly 12.50 g Cu(OH)2 is 12.50/97.56 = moles Cu(OH)2 and that times molar mass Cu metal (63.546) gives 8.1419 g copper. I would dissolve that in HNO3, treat with NaOH, filter the Cu(OH)2, wash, dry. You can supply the details.
To design an experiment to produce exactly 12.5g of pure dry Copper Hydroxide, you would need the following equipment and chemicals:
Equipment:
1. Balance or scale (with precision to at least 0.01g)
2. Beakers or Erlenmeyer flasks
3. Stirring rod or magnetic stirrer
4. Bunsen burner or hot plate
5. Filter paper or funnel
6. Crucible or evaporating dish
7. Crucible tongs
8. Desiccator (optional, for drying)
Chemicals:
1. Copper sulfate (CuSO4)
2. Sodium hydroxide (NaOH)
Step-by-Step Method:
1. Weigh out the appropriate amount of copper sulfate (CuSO4) using a balance or scale. To calculate the mass, use the molar mass of CuSO4 (159.6 g/mol) and the desired amount of Copper Hydroxide (12.5g) to work out the stoichiometry. Bear in mind that the molar mass of Copper Hydroxide (Cu(OH)2) is 97.6 g/mol. Use the ratio of these molar masses to calculate the mass of CuSO4 required.
2. Dissolve the measured amount of copper sulfate (CuSO4) in a beaker or Erlenmeyer flask containing a known volume of water (e.g., 100 mL). Stir the solution until the copper sulfate is completely dissolved.
3. Prepare a sodium hydroxide (NaOH) solution by dissolving the appropriate amount of NaOH in a separate beaker or Erlenmeyer flask of water. The ratio of NaOH to CuSO4 should be 2:1 according to the balanced chemical equation: CuSO4 + 2NaOH -> Cu(OH)2 + Na2SO4.
4. Slowly add the sodium hydroxide solution to the copper sulfate solution while stirring continuously. A precipitate of copper hydroxide should form. Continue adding the solution until the reaction is complete or until all the copper sulfate is used up.
5. Allow the mixture to settle for a few minutes, and then carefully decant the liquid phase without disturbing the solid copper hydroxide precipitate. Alternatively, filter the solution using filter paper or a funnel to separate the precipitate from the solution.
6. Transfer the wet copper hydroxide precipitate to a crucible or evaporating dish using crucible tongs. Avoid splashing or touching the precipitate to minimize contamination.
7. Heat the crucible with the copper hydroxide precipitate using a Bunsen burner or hot plate. Gradually increase the temperature until the precipitate transforms into pure dry copper hydroxide, which will have a light blue color. This process may take several minutes.
8. Once the copper hydroxide has been completely dried, remove the crucible from the heat source and let it cool to room temperature. Weigh the crucible with the dried copper hydroxide using a balance or scale. Subtract the mass of the empty crucible to determine the mass of the pure dry copper hydroxide.
Limitations and Cautions:
1. Precise measurements are essential throughout the experiment. Make sure to use a balance or scale with sufficient precision for accurate mass measurements.
2. Use caution when handling chemicals. Wear appropriate personal protective equipment, such as gloves and goggles, to prevent contact with skin or eyes. Follow proper laboratory safety procedures.
3. Ensure the lab area is well-ventilated to prevent the buildup of toxic fumes. Use a fume hood if available.
4. Copper hydroxide is a solid, so be cautious when transferring and handling the precipitate to avoid spillage or contamination.
5. Use care and proper heating techniques when drying the copper hydroxide to prevent excessive heat or combustion.
Remember to consult appropriate scientific literature or references to ensure accuracy and optimize the experimental procedure.