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Calculate the concentration (in M) of Ag+ when AgIO3 just begins to precipitate from a solution...

Calculate the concentration (in M) of Ag+ when AgIO3 just begins to precipitate from a solution that is 0.0275 M in IO3−. (Ksp = 3.17 ✕ 10−8)

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Answer #1

Solubility product of AgIO3 ,Ksp = 3.17 x 10-8

Precipitaion starts when just the product of the available concentrations of the ions of that compound just exceed the solubility product value of the compound.

Given concentration of IO3- = 0.0275M

AgIO3 Ag+ + IO3-

Ksp = [Ag+ ] [ IO3-]

3.17 x 10-8   =  [Ag+ ] 0.0275M

concentration of Ag+ for precipitation of the given compound =   3.17 x 10-8 / 0.0275M

= 1.1527 x 10-6 M

  

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