When copper carbonate disolves the following happens:
[tex]CuCO_3\rightarrow Cu^{+2}+CO_3^{-2}[/tex]The formula for the solubility product constant is:
[tex]Ksp=\text{ }\lbrack Cu^{+2}\rbrack x\lbrack CO_3^{-2}\rbrack[/tex]
As for every copper ion in solution there is one carbonate ion, we know that the concentration of both ions in solution is 0.57mol/l.
Now we calculate the constant:
[tex]Ksp=0.57\frac{mol}{L}\text{ x }0.57\frac{mol}{L}=\text{ }0.3249\text{ }\frac{mol^2}{L^2}[/tex]So the answer is Ksp= 0.3249 mol2/L2
