What is the $pH$ of the solution containing $1.342 \times 10^{-3} \ M \ H^{+}$ ions?
$(\log 1.342 = 0.1277)$

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

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

Calculate the $[H_3O^+]$ concentration if the $pH$ of the solution is $4.25$.

At a certain temperature $T$,if the conductivity of pure water is $5.5 \times 10^{-7} \ S \ cm^{-1}$,calculate the $pH$ of water at the given temperature. Given: $\lambda_{H^{+}}^\infty = 350 \ S \ cm^2 \ eq^{-1}$ and $\lambda_{OH^{-}}^\infty = 200 \ S \ cm^2 \ eq^{-1}$.

The $pH$ of a neutral solution in our body at normal temperature is ..........