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

Question

The molar solubility of AgCl in 6.5 x 10 ^ -3 M AgNO3 id 2.5 x 10 ^ -8 M. In derving Ksp which of the following assumptions is (are) reasonable?

A. Ksp is the same solubility

B. Ksp of AgCl is the same in 2.5 x 10 ^ -8 M Ag NO3 as in pure H20

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

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

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

Thank you so much!

Explanation / Answer

ksp of AgCl = 2.5E-8 (

AgCl <----> Ag+ + Cl-
AgNO3 <----> Ag+ + NO3-

AgNO3 provides a 0.0065 M source of Ag+, so:

ksp = [Ag+][Cl-]

2.5E-8 = (0.0065)[Cl-]

[Cl-] = [Ag+] = 3.84E-6 M

The Ag+ from AgCl is negligible.

So answer is D. ie., [Ag+] does not change significantly upon adding addition of AgCl to 6.5 x 10 ^ -3 M AgNO3

Related Questions

Navigate

• Browse (All)
• Browse T
• Subjects

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.