What is the solubility of CuCl when it is in a solution of 0.35 M NaCl?(CuCl has Ksp=1.9 x 10^-7)
The Ksp is given by Ksp=[Cu+][Cl-]
if x=[Cu+]
then in our mixture we have
x moles l^-1 [Cu+]
x moles l^-1 [Cl-]
0.35 moles l^-1 [Cl-] from the NaCl
(there is also 0.35 moles l^-1 [Na+] from the NaCl but the Na+ is a spectator)
So Ksp=x(x+0.35)
if x is small wrt 0.35 then
1.9 x 10^-7=x(0.35)
hence find x
To find the value of x, we can rearrange the equation:
1.9 x 10^-7 = x(0.35)
Divide both sides of the equation by 0.35:
(1.9 x 10^-7) / 0.35 = x
Calculating the right-hand side of the equation gives us:
x ≈ 5.43 x 10^-7
Therefore, the solubility of CuCl in the solution of 0.35 M NaCl is approximately 5.43 x 10^-7 M.