The ionisation constant of acetic acid is `2 xx 10^(-5)` The pH of buffer containing acetic acid and sodium acetate is `4.7`. The ratio of [acid] to [salt]

If at 25^(@) the ionization constant of acetic acid is 2 xx 10^(5) the hydrolysis constant of sodium acetate will be

If at 25^(@) the ionization constant of acetic acid is 2 xx 10^(5) the hydrolysis constant of sodium acetate will be

The acid dissociation constant K_(a) of acetic acid is 1.74 xx 10^(-5) at 298 K. The pH of a solution of 0.1 M acetic acid is

The pH of a buffer solution containing 0.1M acetic acid and 0.1 M sodium acetate (pKa of a acetic acid is 4.74) is

The ionisation constant of acetic acid is 1.74xx10^(-5) . The degree of dissociation of acetic acid in its 0.05 m solution and its pH are respectively

The pK_(a) value of acetic acid is 4.7447 at 25^(@)C . How would you obtain a buffer of acetic acid and sodium acetate with pH = 4?

The ionisation constant of acetic acid is 1.74xx10^(-5). Calculate the degree of dissociation of acetic acid in its 0.05 (M) solution. Calculate the concentration of acetate ion in the solution and its pH.

If the ionization (dissociation) constant of acetic acid is k_a , what will be the pH of a solution containing equal concentrations of acetic acid and sodium acetate ?^(**"**)