In 1L saturated solution of AgCl[Ksp=1.6×10−10], 0.01moleofCuCl[Ksp=1×10−6] is added. The resultant concentration of Ag+ in the solution is 1.6×10−xM. The value of x is :
Open in App
Solution
Ksp(CuCl)>>Ksp(AgCl) Thus assume [Cl−] in solution comes from CuCl only [Cl−]=√KspCuCl=10−3M ForAgCl [Ag+][Cl−]=1.6×10−10 [Ag+]=1.6×10−7 x=7