`K_(a)` for `HA` is `4.9 xx 10^(-8)`. After making the necessary approximation, calculate for its decimolar solution,
a. `%` dissociation b. `overset(Θ)OH` concentration
c. `pH`

The dissociation constant of a weak acid HA si 4.9 xx 10^(-8) . After making the necessary approximations, calculate i. Percentage ionisation ii. pH iii. overset(Theta)OH concentration in a decimolar solution of the acid. Water has a pH of 7 .

The dissociation constant of weak acid HA is 4.9xx10^(-8) . After making the necessary approximations, calculate pH in 0.1 M acid.

The dissociation constant of weak acid HA is 4.9xx10^(-8) . After making the necessary approximations, calculate pH in 0.1 M acid.

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 dissociation constant of a weak acid HA is 4.9 xx 10^(-8) . Calculate for a decimolar solution of acid:. % of ionisation

The dissociation constant of a weak acid HA is 4.9 xx 10^(-8) . Calculate for a decimolar solution of acid:. % of ionisation

The dissociation constant of a weak acid HA is 4.9 xx 10^(-8) . Calculate for a decimolar solution of acid:. OH^(-) concentration

The dissociation constant of a weak acid HA is 4.9 xx 10^(-8) . Calculate for a decimolar solution of acid:. OH^(-) concentration

K_a for HF is 3.2 xx 10^(-4) . Calculate the percentage of dissociation in 0.02 M HF solution.