[Lguitarjsm]

Hi - my first post

In a galvanic cell where there is a zinc and Copper electrode, why does the Zn electrode have to be placed in a Zn(NO3)2 solution?

I realize that the Zn electrode releases two electrons to the copper electrode.  When this happens a Zn2+ is released from the Zn electrode (causing it to dissolve) and a Cu 2+ from the Copper nitrate solution will pick up two transferred electrons from the Zn electrode and attach itself to the copper electrode.  So I see the need for the copper nitrate solution, but, I don't see the need of the zinc nitrate solution.   

Also, what gets the electrons to begin migration to the copper electrode in the first place?
Thank you for all of your help.

[Borek]

You are right - in general you don't need Zn²⁺ in the initial solution. After all after few seconds the solution surrounding Zn electrode will already contain Zn²⁺. I guess we "put" Zn²⁺ there just to make it more symmetrical. Besides, cell potential is a function of the Zn²⁺ concentration, so you need to know it to be able to calculate initial potential.

[Lguitarjsm]

So I think if I just put the zince electrode in a water solution, it should be ok and the water will build up concentration with Zn2+?
Do you agree?
thanks again, I really appreciate it.

[Borek]

Yes, that's what should happen.