Question

How do you determine the ksp of copper carbonate with an absorption of 0.57 mol/L?

Answer 1

When copper carbonate disolves the following happens:

`CuCO_3\rightarrow Cu^(+2)+CO_3^(-2)`

The formula for the solubility product constant is:

`Ksp=\text{ }\lbrack Cu^(+2)\rbrack x\lbrack CO_3^(-2)\rbrack`

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:

`Ksp=0.57(mol)/(L)\text{ x }0.57(mol)/(L)=\text{ }0.3249\text{ }(mol^2)/(L^2)`

So the answer is Ksp= 0.3249 mol2/L2