Ionic EquilibriumHard
Question
When 0.1 mol arsenic acids (H3AsO4) is dissolved in 1L buffer solution of pH = 8, which of the following hold good? For arsenic acid K1 = 2.5 × 10-4, K2 = 5 × 10-8, K3 = 2 × 10-13. [′<<′ sign denotes that the high concentration is at least more than 100 times the lower one]
Options
A.[H3AsO4] << [H2AsO4-]
B.[H2AsO4-] << [HAsO42-]
C.[HAsO42-] << [H2AsO4-]
D.[AsO43-] << [HAsO42-]
Solution
(A) 
∴ [H3AsO4] << [H3AsO4-].
(B)
(C)
∴ [AsO43-] << [HAsO42-].
∴ [H3AsO4] << [H3AsO4-].(B)
(C)
∴ [AsO43-] << [HAsO42-].Create a free account to view solution
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