The ionization constants of `HF, H COOH` and HCN at 298 K are `6.8x10^(-4), 1.8xx10^(-4)` and `4.7xx10^(-9)` respectively. Calculate the ionization constants of the corresponding conjugate base.

Add 6.65xx10^(4) and 8.95xx10^(3) .

The dissociation constants of H_(2)O, H_(2)S, H_(2)Se are 1.8xx10^(-6),1.4xx10^(-16), 1.3xx10^(-7) and 2.2xx10^(-5) , respectively. What do these values denote?

The solubility product constant of Ag_(2)CrO_(4) and AgBr are 1.1xx10^(-12) and 5.0xx10^(-13) respectively. Calculate the ratio of the molarities of their saturated solutions.

The dissociation coustant of H_(2)O, H _(2)Se and H_(2) Te are 1.8 xx 10 ^(-16) , 1.4 xx 10 ^(-7) , 1.3 xx 10 ^(-4)and 2.2 xx 10 ^(-3), respectively. What do these values denote ?

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

The air is a mixture of a number of gases. The major components are oxygen and nitrogen with approximate proportion of 20% is to 79% by volume at 298 K. The water is in equilibrium with air at a pressure of 10 atm. At 298 K if the Henry’s law constants for oxygen and nitrogen at 298 K are 3.30 xx10^(7) mm and 6.51 xx10^(7) mm respectively, calculate the composition of these gases in water .

K_(a_1) and K_(b_1) of oxalic acid are 6 xx 10^(-2) and 7.2 xx 10^(-5) respectively. Calculate the pH of 0.06 M oxalic acid solution