Calculate the molar solubility of CuCl2 in 333x102M MgCl2 so

Calculate the molar solubility of CuCl2 in 3.33x10-2M MgCl2 solution. You must consider the activity. Ksp of CuCl2 =1.9x10-7

Given K_sp = 1.9 x 10^-7

K_sp= 1 ¹ * 2 ² * S ^{( 1+ 2 )}

K_sp = 1 ¹ * 2 ² * S ^{( 3)}

where S = solubility of CuCl₂

substitue values S = 3.6 * 10 ^-3 moles/ L

But the concentration MgCl ₂is 3.33*10^-2M

Let [ Cu ²⁺ ] = X moles / L and [ Cl ^- ] = ( X+ 0.0333 ) moles /L

Therefore K _sp = X ( X+ 0.03 ) ^ 2

1.9 x 10^-7 = X ( X ^ 2 + 0.06 X +0.0009 )

= X ^ 3 + 0.06 X ^ 2 + 0.0009 X

neglecting the higher powers we get

1.9 x 10^-7 = 0.0009 X

from this X = 2.1 * 10 ^ -4