The ionization constant of phenol is `1.0 xx 10^(-10)`. What is the concentration of phenolate ion in `0.05` M solution of phenol? What will be its degree of ionization if the solution is also `0.01M` in sodium phenolate?

The ionization constant of phenol is 1.0xx10^(-10) . What is the concentration of phenolate ion in 0.05 M solution of phenol? What will be its degree of ionization if the solution is also 0.01 M in sodium phenolate?

The ionization constant of propionic acid is 1.32xx10^(-5) . Calculate the degree of ionization of the acid in its 0.05 M solution and also its pH. What will be its degree of ionization in the solution of 0.01N HCI ?

At 25^(@)C , the dissociation constant of a base. BOH is 1.0xx10^(-12) . The concentration of hydroxyl ions in 0.01 M aqueous solution of the base would be

The ionisation constant of dimethylamine is 5.4 xx 10^(-4) Calculate its degree of ionisation in its 0.02 M solution. What percentage of dimethylamine is ionised if the solution is also 0.1 M in NaOH ?

The first ionization constant of H_(2)S is 9.1xx10^(-8) . Calculate the concentration of HS^(Θ) ion in its 0.1 M solution. How will this concentration be affected if the solution is 0.1 M in HCl also? If the second dissociation constant if H_(2)S is 1.2xx10^(-13) , calculate the concentration of S^(2-) under both conditions.

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 acid ionization (hydrolysis) constant of Zn^(2+)" is "1.0 xx 10^(-9) Calculate the pH of a 0.001 M solution of ZnCl2

The acid ionization (hydrolysis) constant of Zn^(2+)" is "1.0 xx 10^(-9) Calculate the pH of a 0.001 M solution of ZnCl2

A 0.20 M solution of methanoic acid has degree of ionization of 0.032. Its dissociation constant would be

The dissociations constant of HCN is 7.24 xx 10 ^(-10) Calculate its degree of dissociation and [H_3O^(+) ] in 0.01 M solutions.