In $20 \, mL$ of $0.4 \, M$ $HA$ solution,$80 \, mL$ of water is added. Assuming volume to be additive,the $pH$ of the final solution is ($K_a$ of $HA = 4 \times 10^{-7}, \log 2 = 0.3$).

The percentage dissociation of a decinormal solution of a weak acid $HA$ is: $(K_a = 4.9 \times 10^{-8})$

Dissociation constant of $0.01 \ M$ weak acid is $10^{-4}$. What is percent dissociation of acid (in $\%$)?

If the $pH$ of $0.10 \ M$ monobasic acid at $298 \ K$ is $5.0$,the value of $p K_a$ at the same temperature is

The ionization constant of $CH_3COOH$ is $1.7 \times 10^{-5}$. In a certain solution of acetic acid,the concentration of $H^+$ is $3.4 \times 10^{-4} \ M$. The concentration of the acetic acid solution is ............ .

The dissociation constant of an acid $HA$ is $1 \times 10^{-5}$. The $pH$ of $0.1 \ M$ solution of the acid will be