Prove that the dergee of dissociation of weak acid is given by:
`alpha = (1)/(1+10^(pK_(a)-pH))`
where `K_(a)` is its dissociation constant of the weak acid.

pK_(a) of a weak acid is defined as :

The degree of dissociation of acetic acid in a 0.1 M solution is 1.0xx10^(-2) . The pK_(a) of acetic acid value.

Degree of dissociation of 0.1 molar acetic acid at 25^(@)C (K_(a) = 1.0 xx 10^(-5)) is

At half neutralisation of weal acid with a strong base,what is the relationship between pH and dissocaition constant (K_(a)) of weak acid ?

pH of a salt of a strong base with weak acid

The degree of dissociation of a weak monoprotic acid of concentration 1.2xx10^(-3)"M having "K_(a)=1.0xx10^(-4 is

Weak acids dissociate partially in aqueous medium. If any common ion is present in the solution, the degree of dissociation of the acid is suppressed however the dissociation constant value remains constant. In which of the following the degree of dissociation of water is maximum '?

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.

% dissociation of a 0.024M solution of a weak acid HA(K_(a)=2xx10^(-3)) is :

The dissociation constant of a base MOH is 4xx10^(-6) then calculate the dissociation constant of its conjugate acid