The dissociation constant of `H_(2)S` and `HS^(-)` are respectively `10^(-7)` and `10^(-13)` . The pH of 0.1 M aqueous solution of `H_(2)S` will be

Successive dissociation constants of H_(2)CO_(3) are K_(a_(1)) = 10^(-3) and K_(a_(2)) = 10^(-6) . An aqueous solution contains 0.1 MH_(2)CO_(3) and 0.1 M HCI at 25^(@)C The concentration of CO_(3)^(2-) at equilibrium in solution is: (approximately)

The first and second dissociation constants of an acid H_(2)A are 1 xx 10^(-5) and 5 xx 10^(-10) respectively. The overall dissociation constant of the acid will 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.

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 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.