At $25^{\circ} C$, the ionic product of water is $10^{-14}$. The free energy change for the self-ionization of water in $kCal \ mol^{-1}$ is close to

$A$ $0.1 \ N$ solution of an acid at room temperature has a degree of ionisation $0.1$. The concentration of $OH^{-}$ would be

What is the $pH$ of the resulting solution when $20 \text{ mL}$ of $\frac{M}{10} \text{ NaOH}$ and $10 \text{ mL}$ of $\frac{M}{10} \text{ H}_2\text{SO}_4$ are mixed together?

The hydrolysis constants of salts $NaA$ and $NaB$ (of weak acids $HA$ and $HB$) are $10^{-8}$ and $10^{-10}$ respectively. If the dissociation constant of weak acid $HC$ is $10^{-5}$,what is the decreasing order of acidic strength?

Which of the following undergoes hydrolysis when dissolved in water?

For a $0.01 \ M \ HCN$ solution,the van't Hoff factor is $1.002$. What will be the acid dissociation constant $(K_a)$ for $HCN$?