The sodium salt of a weak acid is hydrolysed to the extent of 3% in 0.1 M solution in water at `25^@C` . If `K_a` for weak acid is `1.3xx10^(-10)` . The ionic product of water is

The sodium salt of a certain weak monobasic organic acid is hydrolysed to an extent of 3% in its 0.1 M solution at 25^@C .Given that the ionic product of water is 10^(-14) at this temperature , what is the dissociation constant of the acid ?

The sodium salt of a certain weak monobasic organic acid is hydrolysed to an extent of 3% in its 0.1 M solution at 25^@C .Given that the ionic product of water is 10^(-14) at this temperature , what is the dissociation constant of the acid ?

When a salt of strong base and weak acid is hydrolysed, the resulting solution has :

When a salt of strong base and Weak acid is hydrolysed the resulting solution has :

A weak acid HA is found to be 3% dissociated in 0.1 M solution . Calculate the value of K_a

Salt of weak acids and strong bases hydrolysis in water to form …………… solutions.

A salt of strong acid and weak base is dissolved in water. Its hydrolysis in solution is

0.2 M solution of a weak acid HA is 1 % ionised 25^(@)C . K_(a) for the acid is equal to