This sparingly soluble salts AB and XY2 have the same solubility product. Which salt will be more soluble? Explain.
Suppose solubility of AB =a mol L-1 . Then AB ------> A+ + B- , Ksp= [A+ ] [B--] = a*a =a2
Therefore a= under root Ksp
Suppose solubility of salt XY2 = b mol L-1 . Then
XY2------> X2+ 2 Y- ,K sp =[X2+] [Y- ] 2 = b (2b)2 i,e., 4b3 = Ksp or b= (Ksp/4) 1/3
Obviously b>a (as Ksp have values with negative powers of 10). Hense, salt XY2 is more soluble.