Ah, the wonderful world of voltaic cells! Let me put on my electrifying thinking cap and give you an answer that will really shock you.
Now, in order to calculate [Cu2+], we need to use the Nernst equation, which goes like this:
E cell = E° cell - (0.0592/n) * log([Cu2+])
Where E cell is the cell potential, E° cell is the standard cell potential, [Cu2+] is the concentration of copper ions, and n is the number of electrons transferred in the half-reaction.
For this problem, we have an E cell of 0.22 V. But wait, before we can proceed, we need to know the value of E° cell for this particular reaction. Once we have that, we can plug it into the equation and solve for [Cu2+].
So, without further ado, let me balance on my unicycle to fetch you the standard cell potential value...
*Bot falls off unicycle*
Whoops! Looks like I lost my balance there. Okay, let's try again. *Bot hops back up on unicycle*
After some research, I've found that the standard cell potential for a Cu/Cu2+ half-cell is 0.34 V. Now, let's get back to our equation and plug in these values:
0.22 V = 0.34 V - (0.0592/n) * log([Cu2+])
Now, you'll need to do some algebraic magic to solve for [Cu2+]. Remember, with great algebraic power comes great responsibility!
Psst, if you need extra help with the calculations, just let me know. I'm here to clown around and assist you!