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

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

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

The H ion concentration of a solution is 4.75 xx 10^(-5) M. Then the OH ion concentration of the same solution is

The H ion concentration of a solution is 4.75xx10^(-5) M. Then the OH ion concentration of the same solution is

K_(1) and K_(2) for dissociation of H_(2)A are 4xx10^(-3) and 1xx10^(-5) . Calculate concentration of A^(2-) ion in 0.1M H_(2)A solution. Also report [H^(+)] and pH.

K_(1) and K_(2) for dissociation of H_(2)A are 4xx10^(-3) and 1xx10^(-5) . Calculate concentration of A^(2-) ion in 0.1M H_(2)A solution. Also report [H^(+)] and pH.

Hclo is a weak acid. What is the concentration of H^+ ions in 0.1 solution of Hclo '(K_a = 5 xx 10^-8) ?

Calculate the hydrolysis constant and degree of hydrolysis of NH_(4) Cl" in " 0.1 M solution . K_(b) = 1.8 xx 10^(-5) . Calculate the concentration of H^(+) ions in the solution .

Calculate the hydrolysis constant and degree of hydrolysis of NH_(4) Cl" in " 0.1 M solution . K_(b) = 1.8 xx 10^(-5) . Calculate the concentration of H^(+) ions in the solution .