Ionic EquilibriumHard
Question
A solution containing a mixture of 0.05 M NaCl and 0.05 M NaI is taken (Ksp of AgCl = 10-10 and Ksp of AgI = 4 × 10-16). When AgNO3 is added to such a solution.
Options
A.the concentration of Ag+ required to precipitate Cl- = 2 ×10-9 mol/L.
B.the concentration of Ag+ required to precipitate I- = 8 × 10-15 mol/L.
C.AgCl and AgI will be precipitated together.
D.first AgI will be precipitated.
Solution
[Ag+] ion required to precipitate Cl- ion = 
= 2 × 10-9 mol/L.
[Ag+] ion required to precipitate I- ion =
= 8 × 10-15 mol/L.
Since [Ag+] ion conc. required to precipitate AgI is less than the [Ag+] ion conc. required to precipitate AgCl, AgI precipitates first.
Hence choices (A),(B) and (D) are correct while (C) is incorrect.
= 2 × 10-9 mol/L.[Ag+] ion required to precipitate I- ion =
= 8 × 10-15 mol/L.Since [Ag+] ion conc. required to precipitate AgI is less than the [Ag+] ion conc. required to precipitate AgCl, AgI precipitates first.
Hence choices (A),(B) and (D) are correct while (C) is incorrect.
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