The $pH$ of the solution formed by mixing $5 \ mL$ of $M/5$ $HCl$ and $10 \ mL$ of $M/10$ $NaOH$ is:

For a $C \ M$ solution of a weak base $BOH$ having a van't Hoff factor '$i$',the base dissociation constant $K_b$ will be:

For a weak electrolyte $A_xB_y$,the degree of dissociation $\alpha$ in terms of concentration $c$ is given by:

At $27^{\circ} C$,the degree of dissociation of $HA$ (weak acid) in $0.5 \ M$ of its solution is $1 \%$. The concentrations of $H_3O^{+}$,$A^{-}$,and $HA$ at equilibrium (in $mol \ L^{-1}$) are respectively

At $90 \, ^\circ C$,the concentration of $H^+$ and $OH^-$ ions in pure water is $10^{-6} \, M$. What is the value of $[H^+] + [OH^-]$ at this temperature?

$K_a$ for $CH_3COOH$ is $1.9 \times 10^{-5}$. Calculate the $pH$ at the equivalence point in the titration of $0.1 \ M$ $CH_3COOH$ with $0.1 \ M$ $NaOH$.