The range of pH for acidic and basic buffer is where `K_(a)` and `K_(b)` are the acid base dissociation constants, respectively.

Match Column -I with Column -II : Column -I Column-II (A) Ph of water ( p ) ( 1)/( 2) p K_(w) ( B ) Ph of a salt of strong acid and strong base ( q) pH = (1)/(2) [ pK_(w) + pK_(a) + log c ] (C ) Ph of a salt of weak acid and strong base ( r ) pH = ( 1)/( 2) [ pK _(w) + pK_(a) - pK_(b)] (D) Ph of a salt of weak acid and weak base (s) 7 where K_(a) , K_(b) are dissociation constants of weak acid and weak base and K_(w) = Ionic product of water.

What is dissociation constant of a weak acid (K_(a)) .

What is dissociation constant of a weak base (K_(b)) .

What is the relationship between pK_(a)andpK_(b) values where K_(a)andK_(b) represent ionization constants of the acid and its conjugate base respectively?

If K_(a) and K_(b) are the dissociation constants of weak acid and its conjugate base , pK_(a) + pK_(b)

If K_(a) and K_(b) are the dissociation constants of weak acid and its conjugate base , pK_(a) + pK_(b)