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 $.88$)

The $K_a$ of monobasic acid $A, B$ and $C$ are $10^{-6}, 10^{-8}$ and $10^{-10}$ respectively. The concentrations of $A, B$ and $C$ are respectively $0.1 \ M, 0.01 \ M$ and $0.001 \ M$. Which of the following is correct for $pOH$ of $A, B$ and $C$?

$A$ monobasic weak acid dissociates to $1.2 \%$ in its $0.01 \ M$ solution at $298 \ K$. Calculate the dissociation constant of it.

The $pH$ of $0.004 \, M$ hydrazine solution is $9.7$. Calculate its ionization constant $K_{b}$ and $pK_{b}$.

The $K_a$ of a weak acid $HA$ is $1.00 \times 10^{-5}$. If $0.100 \ mol$ of this acid is dissolved in $1 \ L$ of water,what is the percentage dissociation of the acid at equilibrium?

$A$ weak base is $1.3\%$ dissociated in its aqueous solution. If $K_b$ for the weak base is $1.69 \times 10^{-5}$ at $298 \text{ K}$, find the concentration of the aqueous solution of the weak base. (in $\text{ M}$)