`0.5 M` ammonium benzoate is hydrolysed to `0.25` precent, hence its hydrolysis constant is

0.5 M ammonium benzoate is hydrolysed to 0.25 percent, hence, its hydrolysis constant is ?

Calculate the degree of hydrolysis of 0*2 (M) sodium acetate solution. (Hydrolysis constant of sodium acetate = 5*6 xx 10^(-10) and ionic product of H_2O = 10^(-14) at 25^@C) "" ^(**"**)

Calculate the degree of hydrolysis and pH of a 0.1 M sodium acetate solution. Hydrolysis constant for sodium acetate is 5.6 xx 10^(-10).

In 0.1M solution of salt NaA, the amion is 8% hydrolysed. Calculate the dissociation constant of acid, HA

The percentage degree of hydrolysis of a salt of weak acid (HA) and weak base (BOH) in its 0.1 M solution is found to be 10%. If the molarity of the solution is 0.05 M, the percentage hydrolysis of the salt should be :

The percentage degree of hydrolysis of a salt of weak acid (HA) and weak base (BOH) in its 0.1 M solution is found to be 10%. If the molarity of the solution is 0.05 M, the percentage hydrolysis of the salt should be :

The percentage degree of hydrolysis of a salt of weak acid (HA) and weak base (BOH) in its 0.1 M solution is found to be 10%. If the molarity of the solution is 0.05 M, the percentage hydrolysis of the salt should be :