A 0.1 (M) solution of acetic acid is 1.34% ionised at 25^(@) . Calculate the ionisation constant of the acid.

Concentration of an aqueous solution of weak acid, HA is 0.1 (M) . How many times this acid solution is to be diluted so that the degree of dissociation of HA becomes 2 times that of the initial solution?

At a certain temperature, the ratio of ionisation constants of weak acids HA and HB is 100:1. if the molarity of the solution of HA is the samme as that of HB and the degrees of ionisation of HA and HB in their respective solutions are alpha_(1) and alpha_(2) respectively, then show that alpha_(1)=10alpha_(2) .

At 15^@C 0.05 N solution of a weak monobasic acid is 3.5% ionised. Calculate k_a

0.1 M solution of a solute has a water potential of

In 0.01(M) acetic acid solution, pH = 3.37. What is the degree of ionisation of the acid?

The pH of a 0.1 molar solution of the acid HQ is 3. The value of the ionisation constant K_a of this acid is

The buffer capacity of a buffer solution consisting of a weak acid, HA and its salt, NaA becomes maximum when its pH is 5.0. at this pH, what is the relation between the molar concentration of HA and NaA? Also find the value of pK_(a) of HA.

Between (a) 0.01 (M) H_(2)SO_(4) and (b) 0.01 (M) H_(3)PO_(4) solution, which one has higher equivalent conductivity? (Assume that, each solution has the same specific conductance and the degree of dissociation of each acid is equal to unity).