A solution of acetic acid is `1.0%` ionised. Determine the molar concentration of acid `(K_(a)=1.8xx10^(-5))` and also the `[H^(+)]`.

At 298 K, 0.1 M solution of acetic acid is 1.34 % ionised . What is the ionisation constant (K_(a)) for the acid ?

Calculate the percent ionization of 0.10M acetic acid (K_a=1.8xx10^(-5)) .

If the degree of ionisation of an acetic acid solution at 298K is 5%, then find its molar concentration. [Given: K_a(CH_3COOH)=1.8xx10^(-5) ]

In a 0.01 (M) acetic acid solution, degree of ionisation of acetic acid is 4.2%. Determine the concentration of H_(3)O^+ ions in that solution.

0.1 M CH_(3) COOH solution is 1.0% ionized. In another diluted solution acetic acid is 10% ionised. In other solution concentration of acetic acid is

0.1 M CH_(3) COOH solution is 1.0% ionized. In another diluted solution acetic acid is 10% ionised. In other solution concentration of acetic acid is

Calculate pH of 0.1 M acetic acid having K_(a)=1.8xx10^(-5)

Degree of dissociation of 0.1 molar acetic acid at 25^(@)C (K_(a) = 1.0 xx 10^(-5)) is

Degree of dissociation of 0.1 molar acetic acid at 25^(@)C (K_(a) = 1.0 xx 10^(-5)) is