A mono protic acid in 1M solution is 0.01% ionized the dissociation constant of this acid is

The molar conductivity of acetic acid solution at infinite dilution is 390.7 Omega^-1 cm^2 mol^-1 . Calculate the molar conductivity of 0.01 M acetic acid solution, given that the dissociation constant of acetic acid is 1.8 xx 10^-5

The dissociation constant of a weak monoprotic acid at 298 K is found to be numerically equal to the dissociation constant of its conjugate base. The pH of a decimolar aq. Solution of this acid at 298 K is

The dissociation constant (K_(a)) of a certain weak monoprotic acid at 298 K is 1 times 10^(-5) . The % dissociation of this acid in its decimolar aqueous solution at 298 K is

if a certain weak acid is only 0.1% ionised in its 0.1 M aq. Solution, the ionisation constant (Ka) of the acid is very close to

The 'p^H' of '0.1 M' solution of cyanic acid (HCNO) is 2.34. Calculate the ionization constant of the acid and its degree of ionization in the solution.

What is the pH of 0.001 M aniline solution. The ionization constant of aniline is 4.3× 10^-10.Cálculate the degree of ionization of aniline in the solution. Also calculate the ionization constant for the conjugate acid of aniline?

It has been found thet pH of 0.01 M solution of an organic acid is 4.15. Calculate the concentration of the anion, the ionisation constant of the acid and its pKa.

Hydrolysis constants of two potassium salts KA and KB of the weak acids HA and HB are 10^(-8) and 10^(-6) respectively. The dissociation constant of a third acid HC at the same temp is 10^(-4) . The acid strengths of the three acids are in the order