Have a look at the colors of solutions of ferrous salts. A solution of ferrous chloride is almost colorless or very pale green. Both Fe(2+) ion and Fe(3+) ion is almost colorless. The colors, observed in iron-containoing solutions, usually is due to contamination, or due to hydrolysis or complex formation.
http://woelen.scheikunde.net/science/chem/solutions/fe.htmlCopper (I) chloride is almost insoluble in water, but it is quite soluble in solutions, containing chloride. The common ion effect does not hold here, because CuCl forms a complex with chloride. The complex ion CuCl2(-) is formed, which gives soluble species in solution.
if you really want to get rid of all copper in the solution, then add a large excess amount of iron, such that finally, some iron (and copper metal as well) remain undissolved. The liquid should become pale green. Plain iron wool or steel wool is not really suitable. That contains quite some impurities, such as nickel, chromium, and even carbon. The chromium makes the liquid appear deep green, and the nickel also adds green ions to solution. The color of chromium ions and nickel ions is MUCH stronger than the color of iron (II) ions. So, I'm afraid that your solution is very impure and has a lot of other metal ions in solution.
Copper (II) ions also form a green ion in the presence of chloride, then you get the green CuCl4(2-) complex. As you see, things are much more complicated than you initially thought.