i)
Solubility equilibrium of AgIO3 is
AgIO3(s) <-------> Ag+(aq) + IO3-(aq)
Ksp = [Ag+] [IO3-] = 3.1×10-8
[Ag+] × 0.070M= 3.1 ×10-8M2
[Ag+]= 4.43 × 10-7M
Therefore,
minimum concentration of Ag+ required to start precipitate IO3- is 4.43 ×10-7M
solubility equilibrium of Ag2CO3
Ag2CO3(s) <-------> 2Ag+(aq) + CO32-(aq)
Ksp = [Ag+]2[CO32-] = 8.1×10-12
[Ag+]2× 0.060M = 8.1 ×10-12M3
[Ag+]2 = 1.33×10-10M2
[Ag+] = 1.15 × 10-5M
minimum concentration of Ag+ required to start precipitate of CO32- is 1.15 ×10-5M
IO3- ion require low concentration of Ag+
Therefore,
IO3- would precipitate first
ii)
Substitute the concentration Ag+ required start precipitate CO32- in Ksp expression of AgIO3
[Ag+][IO3-] = 3.1 ×10-8
1.15 ×10-5 M × [IO3-] = 3.1 ×10-8M2
[IO3-] = 2.70× 10-3M
Therefore,
Concentration of IO3- when CO32- start to precipitate =
2.70 × 10-3M
iii)
℅ of IO3- remaining when CO32- start to precipitate = (0.00270M/0.070M)× 100 = 3.86%
Therefore
these two ions can not be seperated with 99.99% efficiency
Silver ion is being considered as a reagent for separating 1037 from CO3 in a solution...
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