This sparingly soluble salts AB and XY2 have the same solubility product. Which salt will be more soluble? Explain.
This sparingly soluble salts AB and XY2 have the same solubility product. Which salt will be more soluble? Explain.
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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.
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