The ionization constant of `HF` is `3.2xx10^(-4)`. Calculate the degree of ionization of HF in its `0.02M` solution. Calculate the concentration of all species present in the solution and its `pH`.

The ionization constant of HF is 3.2xx10^(-4) . Calculate the degree of dissociation of HF in its 0.02M solution. Calculate the concentration of all species present ( H_(3)O^(+) , F^(-) and HF ) in the solution and its pH .

The ionization constant of base is 5.4 xx 10^(-4) . Calculate its degree of ionization in its 0.02 M solution.

The ionization constant of acetic acid is 1.74xx10^(-5) . Calculate the degree of dissociation of acetic acid in its 0.05M solution. Calculate the concentration of acetate ion in the solution and its pH .

The ionization constant of acetic acid 1.74xx10^(-5) . Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH .

The ionization constant of acetic acid 1.74xx10^(-5) . Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH .

The ionisation constant of HF is 3.2 xx 10^(-4) . a. Calculate the degree of dissociation of HF present in its 1M solution. b. Calculate the concentration of all species present (H_(3)O^(o+),F^(Θ) and HF ) in the solution.