The molar solubility of AgCl in 6.5 × 10 3 M AgNO 3 is 2.5 × 10 8 M . In derivin

Question

The molar solubility of AgCl in

6.5

×

103M AgNO3

is

2.5

×

108 M.

In deriving

Ksp from these data, which of the following assumptions is (are) reasonable?

Ksp is the same as solubility.

×

Solubility of AgCl is independent of the concentration of AgNO3.

[

Ag+

]

×

[

Ag+

]

×

  

Ksp is the same as solubility.

   Ksp of AgCl is the same in 2.5

×

108 M AgNO3 as in pure water.   

Solubility of AgCl is independent of the concentration of AgNO3.

  

[

Ag+

]

does not change significantly upon additon of AgCl to 6.5

×

103M AgNO3.   

[

Ag+

]

after the addition of AgCl to 6.5

×

103M AgNO3 is the same as it would be in pure water.

Explanation / Answer

AgNO3 will dissociate completely as
AgNO3 ----> Ag+ + NO3-

This makes, [Ag+] = 6.5*10^-3 M

when AgCl is added, since concentration of AgCl is very less as compared to 6.5*10^-3, concentration of Ag+ can be assumed to be equal to 6.5*10^-3 M

Answer:

[Ag+] does not change significantly upon additon of AgCl to 6.5 × 103 M AgNO3.

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