Calculate the molar concentration of a weak monobasic acid if the acid dissociation constant $K_a = 1.8 \times 10^{-5}$ and the degree of dissociation $\alpha = 0.01$.

The $pH$ of $0.1 \ M$ monobasic acid is $4.50$. Calculate the concentration of species $H^{+}$,$A^{-}$ and $HA$ at equilibrium. Also,determine the value of $K_{a}$ and $pK_{a}$ of the monobasic acid.

For a weak acid $HA$ with dissociation constant $10^{-9}$,the $pOH$ of its $0.1 \ M$ solution is:

$A$ weak acid of dissociation constant $10^{-5}$ is being titrated with aqueous $NaOH$ solution. The $pH$ at the point of one-third neutralization of the acid will be

The $pH$ of a $0.01 \ M$ weak acid $HX$ $(K_{a}=4 \times 10^{-10})$ is found to be $5$. Now the acid solution is diluted with excess of water so that the $pH$ of the solution changes to $6$. The new concentration of the diluted weak acid is given as $x \times 10^{-4} \ M$. The value of $x$ is $...........$ (nearest integer)

An organic monobasic acid has a dissociation constant of $2.25 \times 10^{-6}$. What is the percent dissociation in its $0.01 \ M$ solution (in $\%$)?