At a ertain temperature, the ration of ionisation constants of a weak acid HA to a weak acid HB is 100 : 1. If the degree of ionisation of HA and HB in their aqueous solutions of equimolar concentration be `alpha_1` and `alpha_2`, then show that `alpha_1=10alpha_2`.

At 25^(@)C , the value of ionisation constant of a weak monobasic acid, HA is 1.6xx10^(-4) . What is the degree of ionisation of HA in its 0.1(M) aqueous 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) .

Ionisation constant of ammonia is 1.8xx10^(-5) at 25^(@)C . Calculate the degree of ionisation of ammonia in its 0.1(M) aqueous solution at that temperature.

If cos^2alpha=sin^3alpha then show that tan^6alpha-tan^2alpha=1

If the ionisation constant (K_a) of acetic acid at 298K si 1.8xx10^(-5) , then what will be the degree of ionisation of 0.001(M) acetic acid solution?

The concentration of an aqueous solution of a weak monobasic acid is 1(M) and its degree of ionisation is 1.32%. Determine the pH of the solution.

The ionisation constant of acetic acid is 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.

A weak mono acid base has p^H=10 at 0.01 M% ionisation of base is

A monobasic weak acid solution has a majority of 0.005 and pH of 5. What is its percentage ionisation in this solution ?

The pH of 0.1M solution of cyanic acid (HCNO) is 2.34. calculate the ionisation constant of the acid and its degree of ionisation in the solution.