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
View Solution FreeMore Ionic Equilibrium Questions
The solubility product of AgC2O4 at 25°C is 2.3 × 10–11 M3. A solution of K2C2O4 containing 0.15 moles in 500 ml water i...The strength of an aqueous solution of I2 can be determined by titrating the solution with standard solution of:...A buffer solution is prepared in which the concentration of NH3 is 0.30 M and the concentration of NH4+ is 0.20 M. If th...The best explanation for the solubility of MnS in dilute HCl is that :...The solubility of CaF2 (Ksp = 3.4 × 10-11) in 0.1 M solution of NaF would be...