5) Adding ammonia to a solution containing copper ions... - reduces the copper t

Question

5) Adding ammonia to a solution containing copper ions...

- reduces the copper to copper metal

- causes formation of a complex ion with copper

- removes the copper from the solution by forming a precipitate

- increases the copper concentration by shifting the reaction toward the reactants

6) After the addition of the ammonia to the copper cell, what do you expect to happen to the cell potential between the copper and the zinc?

- decrease

- increase

- stay the same

- go to zero

7) In the description of the experiment, it says that the value of Q represents the solubility of the copper (II) carbonate. Why does Q represent the solubility?

- because Q = Ksp = 1.0=x with x representing the amount of Cu2+ in the saturated solution

- because Q = [Cu2+] / [Cu 2+] = 1.0/x = x with x representing the amount of Cu2+ in saturated solution

- because Q = [Cu2+] / [ Cu2+] = x/1.0 = x with x representing the amount of Cu2+ in saturated solution

- because Q = Ksp = 1.0/x = x with x representing the amount of Cu2+ in the saturated solution

Explanation / Answer

5) Adding ammonia to a solution containing copper ions,

- causes formation of a complex ion with copper

the complex formed is [Cu(NH3)4]2+

- removes the copper from the solution by forming a precipitate

formation of complex also removes Cu2+ from the solution

6) After the addition of the ammonia to the copper cell, the cell potential between the copper and the zinc would,

- decrease

As more of complex is formes, Cu2+ concentration in solution decreases, which would reduce the log([Zn2+]/[C2+]) value and thus would decrease the cell potential.

7) In the description of the experiment, it says that the value of Q represents the solubility of the copper (II) carbonate, this is,

- because Q = [Cu2+] / [ Cu2+] = x/1.0 = x with x representing the amount of Cu2+ in saturated solution

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