In the hydrolysis equilibrium
`B^(+)H_(2)OhArrBOH+H^(+),K_(b)=1xx10^(-5)`
The hydrolysis constant is

If the K_b value in the hydrolysis reaction B^(+)+H_2O hArr BOH +H^+ is 1.0 xx 10^(-6) , then the hydrolysis constant of the salt would be

If the K_b value in the hydrolysis reaction B^(+)+H_2O hArr BOH +H^+ is 1.0 xx 10^(-6) , then the hydrolysis contant of the salt would be

If the K_(a) value in the hydrolysis reaction, B^(+) + H_(2)O to BOH + H^(+) is 1.0xx10^(-6) ,then the hydrolysis constant of the salt would be :

K_b for the hydrolysis reaction : B^+ +H_2O hArr BOH +H^+ is 1.0xx10^(-6) the hydrolysis constant of the salt is :

In the equilibrium A^(-)+H_(2)OhArrHA+OH^(-)(K_(a)=1.0xx10^(-5)) . The degree of hydrolysis of 0.001 M solution of the salt is

In the hydrolytic equilibrium , A^(-) + H_(2) O hArr HA + OH^(-) K_a = 1 .0 xx 10^(-5) . The degree of hydrolysis of 0.001 M solution of the salt is

In the equilibrium A^(-)+ H_(2)O hArr HA + OH^(-) (K_(a) = 1.0 xx 10^(-4)) . The degree of hydrolysis of 0.01 M solution of the salt is

In the equilibrium A^(-)+ H_(2)O hArr HA + OH^(-) (K_(a) = 1.0 xx 10^(-4)) . The degree of hydrolysis of 0.01 M solution of the salt is