Ionisation constant of `CH_(3)COOH` is `1.7 xx 10^(-5)` and concentration fo `H^(+)` in certain acetic acid solution is `3.4 xx 10^(-4) M` . The concentration of acetic acid solution is

Ionisation constant of CH_(3)COOH is 1.7xx10^(-5) and concentration of H^(+)ions is 3.4xx10^(-4) . Then, find out initial concentration of CH_(3)COOH molecules.

Ionisation constant of CH_(3)COOH is 1.7xx10^(-5) and concentration of H^(+)ions is 3.4xx10^(-4) . Then, find out initial concentration of CH_(3)COOH molecules.

ionisation constant of CH_(3)COOH is 1.7xx10^(-5) and concentration of H^(+) is 3.4xx10^(-4) . Then the initial concentration of CH_(3)COOH molecules is :

Ionisation constant of CH_(3)COOH is 1.7xx10^(-5) and concentration of H^(+)ions is 3.4xx10^(-4) . Then, find out initial concentration of CH_(3)COOH molecules. (a) 3.4xx10^(-4) (b) 3.4xx10^(-3) (c) 6.8xx10^(-4) (d) 6.8xx10^(-3)

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

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

The ionization constant of acetic acid 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 .

The ionization constant of acetic acid 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 .

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