New here, need some help

Sep 2018
Michigan, USA
Hello there! I'm in need of some help with a reaction that I'm fairly certain I messed up big time. I was attempting to make copper (II) sulphate through electrolysis of dilute sulphuric acid solution w/ copper electrodes. That part went well. I did not use exact amounts, just eyeballed it. At the end, my solution looked like this:

Then after filtering it looked like this:

So I proceeded to filter and wash a few times and then I was left with these two. One with a nice, clean look (right) and another that looked like it was carrying some impurities (left):

I put the one that looked impure in a 500mL flask and set it back on to boil more. As I did that, I made a small saturated sodium bicarbonate solution in a 50 mL beaker. I used a pipette to put a small amount of the clean solution into it and it made a cloudy solution. I watered it down and filtered it into a 50 mL flask and it gave me this:
I thought it was the same thing given the colour but what happens next proves that wrong.

Upon adding a sodium bicarbonate solution, it foamed vigorously and left me with a cloudy, light blue solution (left):
After some thought I feared I had created copper carbonate in my attempt to neutralise the acidic solutions from earlier.

As I filtered the solution out, it left this blue paste on the paper towels (had no filter paper), and I'm pretty sure it's copper carbonate:

So now I'm left with three solutions. A cloudy light blue one; a dark, clear but almost murky one; and a clear royal blue one (3 images):

Did I end up making copper carbonate or something else? If so, how can I avoid this in the future and make copper (II) sulphate? Do I just do what I did last time, but instead of neutralising I just wash with water, then let it evapourate? Does H2SO4 even evapourate? Any and all help is appreciated.