Degree Of Dissociation|Ionisation Constant Of Weak Acids|Questions|Relation Between Ka And Kb|Hydrolysis Of Salts And The pH Of Their Solutions|Summary

Relation between Ka and Kb||Salt Hydrolysis||Hydrolysis OF Different types OF Salts

A salt is formed when a weak acid of dissociation constant 10^(-4) and weak base of dissociation constant 10^(-5) are mixed. The pH and degree of hydrolysis of salt solution are

How is dissociation constant of a weak electrolyte related tol its degree of dissociation ?

The dissociation constant of weak acid HA is 1 xx 10^(-5) . Its concentration is 0.1 M . pH of that solution is

Dilution processes of different aqueous solutions, with water, are given in LIST-I. The effects of dilution of the solutions on [H^(+)] are given in LIST-II. (Note: Degree of dissociation (alpha) of weak acid and weak base is ltlt 1, degree of hydrolysis of salt ltlt 1, [H^(+)] represents the concentration of H^(+) ions)

When a salt reacts with water resulting into formation of acidic or basic solution, the process is referred to as salt hydrolysis. The pH of salt solution can be calculated using the following equations. pH = ( 1)/(2) ( p K_(w) + pK_(a) + log C) for salt of weak acid and strong base. pH = (1)/(2) ( pK_(w)- pK_(b) - log C ) for salt of weak base and strong acid. pH = (1)/(2) ( pK_(w) + pK_(a) - pK_(b)) for salt of weak acid and weak base equal volume of 0.1M solution of weak acid HA is titrated with 0.1M NaOH solution till the end point pK_(a) for acid is 6 and degree of hydroglysis is less compared to 1.The pH of the resultant solution at the end point is