An aqueous solution with $pH = 0$ is:

At $25 \, ^\circ C$,the $pH$ value of a solution is $6$. The solution is:

The concentration of hydronium $({H_3}{O^{+}})$ ion in pure water at $298 \ K$ is:

At $90\,^{\circ}C$ pure water has $[H_3O^{+}] = 10^{-6}\,M$. The value of $K_w$ at this temperature will be:

The $pH$ of a solution is $5.0$. To this solution,sufficient acid is added to decrease the $pH$ to $2.0$. The increase in hydrogen ion concentration is $...$ times.

If the ionic product of water $(K_w)$ is $1.96 \times 10^{-14}$ at $35^{\circ} C$,what is its value at $10^{\circ} C$?