If `K_(a)` of a weal acid is` 4xx4^(-6)` and its concentration is 0.1 M. Find pH of solution

If K_(a) of a weak acid is 4xx10^(-6) and its concentration is 0.1 M. Find pH of solution

If K_(a) of a weak acid is 4xx10^(-6) and its concentration is 0.01 M. Find pH of solution

The dissociation constant of weak acid HA is 1 xx 10^(-5) . Its concentration is 0.1 M . pH of that solution is

0.01M solution of H_(2)A has pH equal to 4. If k_(a1) for the acid is 4.45 xx 10^(-7) , the concentration of HA^(-) ion in solution would be

K_(a) for an acid HA is 4.9 xx 10^(-8) . Calculate percentage dissocitation H^(+) ion concentration for its 0.1 M aqueous solution.

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

K_(a) for butyric acid is 2.0xx10^(-5) . Calculate pH and hydroxyl ion concentration in 0.2M aqueous solution of sodium butyate.

The dissociation constant of a monobasic acid is 1.0xx10^(-9) . The pH of its 0.1 M aqueus solution is:

If K_(a_(1)) and K_(a_(2)) of sulphuric acid are 1xx10^(-2) and 1xx10^(-6) respectively, then concentration of sulphate ions in 0.01 M H_(2)SO_(4) solution will be :