silver ions in a solution of silver salts can be recovered by immersing copper metal in the solution. crystals of pure silver are deposited on the silver metal. design an experiment to determine the number of moles of silver atoms that form describe the procedure materials and safety procedure. explain the required calculations

see above.

To determine the number of moles of silver atoms formed when copper is immersed in a solution of silver salts, you can perform the following experiment:

Materials:
1. Copper metal sheet or copper wire
2. Solution of silver salts (e.g., silver nitrate)
3. Beaker or container to hold the solution
4. Wire or clip to attach the copper metal to the beaker
5. Weighing scale or balance
6. Graduated cylinder or measuring cup
7. Distilled water (for safety rinse)
8. Safety gloves and goggles
9. Proper waste disposal containers

Procedure:
1. Measure the mass of the copper metal to be used. Record the mass.
2. Prepare a solution of silver salts by dissolving a known quantity of silver salt (e.g., silver nitrate) in distilled water. Stir gently until fully dissolved.
3. Pour the silver salt solution into the beaker or container.
4. Attach the copper metal securely to the beaker, ensuring it is fully immersed in the silver salt solution.
5. Leave the setup undisturbed for some time, allowing the reaction to proceed.
6. After a suitable duration (e.g., overnight), carefully remove the copper metal from the solution.
7. Rinse the copper metal with distilled water to remove any residual silver salt solution.
8. Dry the copper metal and carefully scrape off any visible deposited silver crystals.
9. Weigh the copper metal again, along with the collected silver crystals. Record the final mass.

Safety Procedure:
1. Wear safety gloves and goggles to protect your hands and eyes from any possible chemical contact.
2. Work in a well-ventilated area or under a fume hood to avoid inhaling any fumes released during the experiment.
3. Dispose of any leftover silver salt solution or other waste materials properly, following local regulations.

Calculations:
1. Determine the change in mass of the copper metal. This can be calculated by subtracting the initial mass of the copper from the final mass (copper + silver) measured.
2. Convert the change in mass of the copper to moles using the molar mass of copper, which is approximately 63.546 g/mol.
3. As per the balanced equation of the reaction, for every mole of copper that is oxidized, one mole of silver is reduced. Therefore, the moles of copper obtained in step 2 represent the moles of silver atoms formed in the reaction.
4. The number of moles of silver atoms formed can be used to calculate its mass, as the molar mass of silver is approximately 107.868 g/mol.

Remember to follow proper scientific processes, safety guidelines, and proper waste disposal procedures while conducting the experiment.