What is the $pH$ of a $0.01 \ M$ solution of glycerol? (Given for glycerol: $K_{a1} = 4.5 \times 10^{-3}$,$K_{a2} = 1.7 \times 10^{-10}$)

$K_{a}$ 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 $\log 2 = 0.30$]

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)

The concentration of $[CN^{-}]$ in $0.1 \, M \, HCN$ solution is: $(K_a = 4 \times 10^{-10})$

The ionisation constant of acetic acid is $1.8 \times 10^{-5}$. The concentration at which it will be dissociated to $2\%$,is (in $M$)

Calculate the $pH$ of $0.02 \ M$ $ClCH_2COOH$. Given its $K_a = 1.36 \times 10^{-3}$,calculate its $pK_b$.