Calculate the pH of 0.01 M solution of NH_(4)CN. Given that the dissociation constants are : K_(a) for HCN = 6.2xx10^(-10)and pK_(b) for NH_(3)=1.6xx10^(-5).

Calculate the pH of 0.01 M solution of NH_(4)CN. Given that the dissoc

1.	Calculate the pH of 0.01 M solution of NH_(4)CN. Given that the dissociation constants are : K_(a) for HCN = 6.2xx10^(-10)and pK_(b) for NH_(3)=1.6xx10^(-5).
Answer» Solution :`NH_(4)CN` is a SALT of weak acid, weak BASE. CALCULATE `pK_(a) and pK_(b)`. We get `pK_(a) = 9.21 , pK_(b) = 4.80`. Then `pH = 7 + (1)/(2) [pK_(a) - pK_(b)]`