AgNO3(aq) is slowly added to a solution that is 0.280 M NaCl and also 0.0027 M KBr?
What is [Ag]+ at the point at which the second anion begins to precipitate?
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This is a solubility product questions.
You must compare the Ksp of AgCl and that of AgBr.
The Ksp of AgCl > the Ksp of AgBr
This means AgCl is more soluble than AgBr.
The AgBr will precipitate first follower by the AgCl.
You will have to calculate the [Ag+] that will initiate the precipitation of AgCl.
[Ag+] [NaCl] = Ksp of AgCl
[Ag+] (0.28) = 1.0 x 10^-10
[Ag+] = 3.57 x 10^-10
You must compare the Ksp of AgCl and that of AgBr.
The Ksp of AgCl > the Ksp of AgBr
This means AgCl is more soluble than AgBr.
The AgBr will precipitate first follower by the AgCl.
You will have to calculate the [Ag+] that will initiate the precipitation of AgCl.
[Ag+] [NaCl] = Ksp of AgCl
[Ag+] (0.28) = 1.0 x 10^-10
[Ag+] = 3.57 x 10^-10
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