Degree of dissociation is $10\%$ for $10^{-3} \ M$ solution of $H_2CO_3$. Then,the $pH$ of the solution is:

Calculate the concentration of a weak monobasic acid if its degree of dissociation and dissociation constant are $5.0 \times 10^{-4}$ and $5.0 \times 10^{-9}$ respectively (in $M$)?

For a $0.1 \ M$ solution of a weak acid $HQ$,the $pH$ is $3$. The ionization constant $K_a$ of the acid is:

An acid solution of $pH=6$ is diluted $1000$ times,the $pH$ of the final solution becomes

At $25^{\circ} C$,the percentage of ionization of $x \ M$ acetic acid is $4.242$. What is the pH of the acetic acid solution?
$(\log 4.242=0.6275) ;(\log 0.04242=-1.372) \quad (K_a=1.8 \times 10^{-5})$

For a diprotic organic acid in aqueous solution,the ionization constants are $K_1 = 4.2 \times 10^{-7}$ and $K_2 = 4.8 \times 10^{-11}$. For a $0.034 \ M$ solution of this acid,select the correct statement.