[Count of Monte Cristo]

I was making a solution of HCl and CuCl2 safe for disposal by pouring washing soda into the solution, my predicted reaction was: Na2CO3+HCl+CuCl2 2NaCl+CO2+H2O+CuCO3 I expected the blue precipitate to form at the bottom of the beaker, however the entire solution turned blue with a white precipitate (which I assume to be excess Na2CO3 and salt). Why was the CuCO3 dispersed throughout the solution as if it was soluble and why did such a large amount of the white precipitate form?

[Hunter2]

Are you sure Carbonate was used and not sodium hydroxide?  If sodium hydroxide is used copper is soluble as copper complex. The white precipitate could be CuCl copper-I-chloride, because chloride was also present.

[Count of Monte Cristo]

I'm sure it was carbonate because I used Arm and Hammer washing soda to convert the acid, and I'm pretty sure that that doesn't have sodium hydroxide in it.

[Count of Monte Cristo]

UPDATE: I filtered out the two substances, leaving the seemingly pure copper compound in one container and the insoluble substance in the original beaker. The insoluble substance has the appearance of a salt deposit tinged slightly blue from  contamination from the copper chloride.