The dissociation constant of a weak acid is $1 \times 10^{-4}$. The equilibrium constant of its reaction with a strong base is:

What is ionic equilibrium? Discuss the relation of types of substances and ionic equilibrium in solution.

Identify the correct statements from the following.
$(A)$ The ionic product of water at $100^{\circ} C$ is $< 10^{-14}$.
$(B)$ $pH$ of a solution decreases with increasing temperature.
$(C)$ $NaH_2PO_4$ on hydrolysis gives a basic solution.
$(D)$ $NH_3$ can act both as Bronsted acid and base.

If the concentration of $OH^{-}$ ions is $10^{-7} \text{ gram ions/litre}$,what is the number of $OH^{-}$ ions in one litre of water?

What is the $pH$ of a solution containing $10 \, mL$ of $0.1 \, M \, NaOH$ and $10 \, mL$ of $0.05 \, M \, H_2SO_4$?

At $STP$, the dissociation reaction of water is $H_2O \rightleftharpoons H^{+}(aq.) + OH^{-}(aq.)$, and the $pH$ of water is $7.0$. The change of standard free energy $(\Delta G^{\circ})$ for the above dissociation process is given by