Ionic EquilibriumHard
Question
To precipitate as Ag2S(s), all Ag+ present in 250 ml of a satrurated solution of AgBrO3 requires 3.36 cm3 of H2S(g) measured at STP (Assuming H2S is enough soluble in water). Ksp of AgBrO3 is [Ksp(Ag2S) = 10-50, Ka(H2S) = 10-21]
Options
A.1.44 × 10-6
B.2.25 × 10-7
C.9 × 10-6
D.2.7 × 10-7
Solution
2Ag+ (aq) + H2S(g) → Ag2S (s) + 2H+ (aq) ; K = 1029
moles of H2S dissolved = 1.5 × 10-4
∴ moles of Ag+ precipitated = 3 × 10-4
∴ Ksp(AgBrO3) =
= 1.44 × 10-6
moles of H2S dissolved = 1.5 × 10-4
∴ moles of Ag+ precipitated = 3 × 10-4
∴ Ksp(AgBrO3) =
= 1.44 × 10-6Create a free account to view solution
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