The $pH$ of $0.001 \ M$ acetic acid is $.......$

The amount of acetic acid in $1 \ L$ of solution having $\alpha = 1\%$ and $K_a = 1.8 \times 10^{-5}$ is ............. $g$.

The $pK_a$ of a weak acid is $5.85$. The concentrations of the acid and its conjugate base are equal at a $pH$ of (in $.85$)

$A$ weak acid $HA$ has a degree of dissociation $x$. Which option gives the correct expression for $pH - pK_{a}$?

$K_{a}$ for butyric acid $(C_{3}H_{7}COOH)$ is $2 \times 10^{-5}$. The $pH$ of $0.2 \ M$ solution of butyric acid is $........... \times 10^{-1}$. (Nearest integer) [Given $\log 2 = 0.30$]

What is the value of $pH$ of a $NaOH$ solution that dissociates $2 \%$ in its $0.01 \ M$ solution?