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 dissociation constant of acetic acid is 8 xx 10^(-5) ta 25^(@)C . Find the pH of i. M//10 ii. M//100 solution of acetic acid.

The dissociation constant of acetic acid is 8 xx 10^(-5) ta 25^(@)C . Find the pH of i. M//10 ii. M//100 solution of acetic acid.

The dissociation constant of acetic acid at a given temperature is 1.69xx10^(-5) .The degree of dissociation of 0.01 M acetic acid in presence of 0.01 M HCl is equal to :

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

Dissociation constant of acetic acid is 1.8 xx 10^(-5) . Calculate percent dissociation of acetic acid in 0.01 M solution.

If the ionisation constant (K_a) of acetic acid at 298K si 1.8xx10^(-5) , then what will be the degree of ionisation of 0.001(M) acetic acid solution?

The ionization constant of acetic acid is 1.74 x 10^(-5) .Calculate the degree of dissociations of acetic acid in its '0.05 M' solution. Calculate the concentration of acetate ion in the solution.