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

First, I think you mean the silver plates out onto the copper metal.

There may be an easier way to do this and I've not done an experiment like this but can't you do this?
Cu ==> Cu^+2 + 2e
Ag^+e ==> Ag
Therefore, if you weigh the copper strip initially, some of the copper metal will go into solution and silver will replace it. The equations tell us that 1 mole Cu goes into solution for every 2 moles Ag that come out. The extra mass of the copper strip, after plating some silver, will be due to -x moles Cu and + 2x moles Ag.

For example, suppose the strip of copper had a mass of 1.00 g initially. When plated, the mass is 1.100 grams; therefore, the 0.100 g is due to the loss of some Cu and the acquisition of some Ag.
-xmoles Cu + 2x moles Ag = 0.1 gram.
Now change that to grams so grams = grams.
-x*molar mass Cu + (2x*molar mass Ag) = 0.100 gram.
Solve for x = moles Cu
Then 2x = moles Ag.
Wouldn't that work?
There may be a much less complicated way to do it but this is the one that came to my mind. You will need to fill in all of the pieces, the procedure, etc but this is the general idea.

If another tutor checks this out and finds I've made an "illegal" assumption, I'm sure we will hear about it, at least I hope so.

To determine the number of moles of silver atoms formed in this experiment, you need to understand the principles of stoichiometry. The reaction between silver salts and copper metal involves a redox reaction, where copper metal reduces the silver ions to pure silver. The molar ratio between copper and silver in this reaction will enable us to calculate the amount of silver formed.

Here's a step-by-step procedure to design an experiment and determine the number of moles of silver atoms formed:

Materials:
1. Silver salt solution (e.g., silver nitrate solution)
2. Copper metal
3. Beaker or container for the reaction
4. Wire or other copper metal strip
5. Filter paper or filtration setup
6. Analytical balance
7. Safety goggles and gloves
8. Distilled water
9. Bunsen burner or hot plate (optional)

Safety Procedure:
1. Wear safety goggles and gloves.
2. Work in a well-ventilated area or under a fume hood to avoid inhaling any fumes.
3. Handle the chemicals with care and avoid contact with skin or eyes.
4. Properly dispose of all waste materials following safety regulations.

Procedure:
1. Measure and record the initial mass of the copper metal strip (Cu_inital) using an analytical balance.
2. Prepare a beaker or container with the silver salt solution. Make sure it is large enough to immerse the copper metal completely.
3. Immerse the copper metal in the silver salt solution and let it react for a suitable amount of time, ensuring all copper is submerged.
4. Observe the formation of silver crystals on the copper metal. The copper metal acts as a reducing agent and transfers electrons to the silver ions.
5. Once the reaction is complete, carefully remove the copper metal strip from the solution.
6. Rinse the copper metal strip with distilled water to remove any excess silver salt solution.
7. Allow the copper metal strip to dry thoroughly, ensuring all water is evaporated.
8. Measure and record the final mass of the copper metal strip with the deposited silver crystals (Cu_final) using an analytical balance.

Calculations:
1. Calculate the change in mass of the copper metal strip: Δm = Cu_final - Cu_initial.
2. Convert the change in mass of copper to moles using the molar mass of copper (Cu). The molar mass of Cu is approximately 63.55 g/mol.
Moles of Cu = Δm / molar mass of Cu.
3. Since the reaction involves a 1:1 molar ratio between copper and silver in this redox reaction, the moles of copper (Cu) will be equal to the moles of silver (Ag) formed in the reaction.
Moles of Ag = Moles of Cu.
4. Report the final result as the number of moles of silver atoms formed.

By following this procedure and performing the required calculations, you can determine the number of moles of silver atoms formed in the given experiment.