Question

A solution is 0.0010 M in both Ag+ and Au+. Some solid NaCl is added slowly...

A solution is 0.0010 M in both Ag+ and Au+. Some solid NaCl is added slowly until the second solid compound just begins to precipitate. What is the concentration of Au+ ions at this point? Ksp for AgCl = 1.8 x 10-10 and for AuCl is 2.0 x 10-13

Homework Answers

Answer #1

CONCEPT: Determine the concentration of Cl- ion at which AgCl will begin to precipitate , then at the same concentration of Cl- ion determine Au+ concentration. Whole procedure is shown below.

AuCl <-----> Au+ + Cl-  Ksp = 2.8 X 10-13

AgCl <-----> Ag+ + Cl-   Ksp = 2.8 X 10-10.

Ksp = [Ag+ ] [Cl-]

1.8 x 10-10 = [Ag+ ] [Cl-]

[Cl-] = 1.8 x 10-10 / 0.0010 = 1.8 X 10-7

Hence AgCl will begin to precipitate when [Cl-] reaches 1.8 X 10-7 . Concentration of Au+ at this concentration will be determined as

Ksp = [Au+ ] [Cl-]

2.0 x 10-13 = [Au+ ] [1.8 X 10-7 ]

[Au+ ] = 1.11 X 10-6

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