The $pH$ of a solution having $[OH^{-}] = 10^{-7} \ M$ is

At $90\,^oC$,pure water has $[H^{+}] = 10^{-6}\,M$. If $100\, mL$ of $0.2\, M\, HCl$ is added to $200\, mL$ of $0.1\, M\, KOH$ at $90\,^oC$,then the $pH$ of the resulting solution will be:

If the value of the dissociation constant of water is $1.8 \times 10^{-16}$,what is the ionic product of water?

At $25 \, ^\circ C$,the ionic product of water $(K_w)$ is equal to .......

At $25^{\circ} C$,the ${H_3}{O^+}$ concentration of a solution is $1.0 \times 10^{-10} \ M$. What is the $pOH$ value of the solution (in $.0$)?

The $pH$ of $1 \ N \ H_2O$ is