Question

The molar solubility of AgCl in 6.5 x10^-3 M AgNO3 is 2.5x10^-8 M. In deriving Ksp from these data, which of the following assumptions is (are) reasonable

A. Ksp is the same as solubility

B. Ksp of AgCl is the same in 2.5x10^-8 M AgNO3 as in pure water

C. Solubility of AgCl is independent of the concentration of AgNO3

D. [Ag+] does not change significantly upon addition of AgCl to 6.5x10^-3 M AgNO3

E. [Ag+] after the addition of AgCl to 6.5x10^-3 M AgNO3 is the same as it would be in pure water

Answer 1

The molar solubility of AgCl in 6.5 x10^-3 M AgNO3 is 2.5x10^-8 M. In deriving Ksp from these data, which of the following assumptions is (are) reasonable

A. Ksp is the same as solubility --> FALSE, since Ksp = [Ag+][Cl-] so solubility is no the same

B. Ksp of AgCl is the same in 2.5x10^-8 M AgNO3 as in pure water --> False, since AgCl and AgNO3 is not the same

C. Solubility of AgCl is independent of the concentration of AgNO3 --> False, since Ag+ i spresent, so common ion effect will be present as well

D. [Ag+] does not change significantly upon addition of AgCl to 6.5x10^-3 M AgNO3 --> TRUE, since [Ag+] is already fixed by AgNO3

E. [Ag+] after the addition of AgCl to 6.5x10^-3 M AgNO3 is the same as it would be in pure water --> False, since it DOES changes as Ag+ is present form other salts or not