$A$ weak monoprotic acid of $0.1 \ M$ ionizes to $1\%$ in solution. What will be the $pH$ of the solution?

Sulphurous acid $(H_{2}SO_{3})$ has $Ka_{1} = 1.7 \times 10^{-2}$ and $Ka_{2} = 6.4 \times 10^{-8}$. The $pH$ of $0.588 \ M \ H_{2}SO_{3}$ is ..... . (Round off to the Nearest Integer)

The degree of ionization of $0.10 \ M$ lactic acid is $4.0 \%$. The value of $K_a$ is:

The ionization constant of $0.1$ $M$ weak acid is $1.74 \times 10^{-5}$ at $298$ $K$ temperature. Calculate the $pH$ of its $0.1$ $M$ solution. (in $.88$)

$HClO$ is a weak acid. The concentration of ${H^+}$ ions in $0.1 \ M$ solution of $HClO$ $(K_a = 5 \times 10^{-8})$ will be equal to:

At $T$ $(K)$,if the ionisation constant of ammonia in solution is $2.5 \times 10^{-5}$,the $pH$ of $0.01 \ M$ ammonia solution and the ionisation constant of its conjugate acid respectively at that temperature are $(\log 2 = 0.30)$