At $90\,^{\circ}C$,pure water has $H_3O^{+}$ ion concentration of $10^{-6}\,mol\,L^{-1}$. The $K_w$ at $90\,^{\circ}C$ is

When the $pH$ of a solution is $2$,the hydrogen ion concentration in moles per litre is

At $90 \, ^\circ C$,the concentration of $[H_3O^+]$ in pure water is $10^{-6} \, mol \, L^{-1}$. What is the value of $K_W$ at $90 \, ^\circ C$?

If $pH$ of a solution changes from $4$ to $5$,then the $[H_3O^+]$ ion concentration of the solution:

$2$. Given below are two statements:
Statement $I$: The changes in $pH$ with temperature are so small that we often ignore them.
Statement $II$: When the hydrogen ion concentration changes by a factor of $100$,the $pH$ changes by one unit.
In the light of the above statements,identify the correct answer from the options given below:

In a solution of acid,the $H^{+}$ concentration is $10^{-10} \ M$. The $pH$ of this solution will be: