The molar solubility of AgCl in 6.5 x 10^-3 M AgNO3 is 2.5 x 10^-8 M. In derivin

Question

The molar solubility of AgCl in 6.5 x 10^-3 M AgNO3 is 2.5 x 10^-8 M. In deriving Ksp from these data, which of the following assumptions are reasonable?

A) Ksp is the same as solubility.

B) Ksp of AgCl is the same in 6.5 x 10^-3 M AgNO3 as in pure water.

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

D) [Ag+] in solution does not change significantly upon the addition of AgCl to 6.5 x 10^-3 M AgNO3.

E) [Ag+] in solution after the addition of AgCl to 6.5 x 10^-3 M AgNO3 is the same as it would be in pure water.

Explanation / Answer

Since the solubility of AgCl (2.5 x 10^-8 M) is very less than the concentration of Ag+ ions in AgNO3 (6.5 x 10^-3)
Thus it is reasonable to assume [Ag+] in solution does not change significantly upon the addition of AgCl to 6.5 x 10^-3 M AgNO3. Answer is option D

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