Ionic EquilibriumHard
Question
In which of the following solutions, the solubility of AgCN will be greater than that in pure water :
Given Ksp(AgCN) = 4 × 10-16, Ka (HCN) = 5 × 10-10
Given Ksp(AgCN) = 4 × 10-16, Ka (HCN) = 5 × 10-10
Options
A.0.01 M Ag NO3 solution
B.A buffer solution of pH = 12
C.0.2 M NH3 solution
D.A buffer solution of pH = 5
Solution
In AgNO3 solution, the solubility of AgCN will decrease as compared to pure water because of common ion effect of Ag+ ion.
In NH3 solution and buffer of pH = 5, the solubility of AgCN will increase due to complex formation in case of NH3 solution and hydrolysis of CN- ions in case of buffer of pH = 5.
In NH3 solution and buffer of pH = 5, the solubility of AgCN will increase due to complex formation in case of NH3 solution and hydrolysis of CN- ions in case of buffer of pH = 5.
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