HA is a weak acid. The pH of 0.1 M HA solution is 2. What is the degree of dissociation `(alpha)` of HA ?

The pH of a 0.1 M aqueous solution of a weak acid (HA) is 3. What is its degree of dissociation ?

HA is a weak acid . No. of moles = 0.001, K_a = 2x 10^(-6) , HCl is added with molarity 0.01 and the solution is made 1 litre. calculate degree of dissociation of HA

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?

A monoprotic acid in 0.1 M solution has K_(a)=1.0xx10^(-5) . The degree of dissociation for acid is

A 0.1M solution of weak acid HA is 1% dissociated at 298k . what is its K_(a) ? what will be the new degree of dissociation of HA and pH when 0.2M of NaA is added to it.