What is the $pH$ of a neutral solution at the normal temperature of the human body $(37^{\circ}C)$?

The standard Gibbs energy change for the reaction $H_2O \rightleftharpoons H^{+} + OH^{-}$ at $25 \, ^\circ C$ is $... \ kJ$.

The ionic product of water $(K_w)$ increases if:

$A$ beer has a $pH$ of $4.30$. What is the $[H_3O^{+}]$ concentration?

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

The value of the ion product constant for water,$(K_w)$ at $60\,^{\circ}C$ is $9.6 \times 10^{-14} \,M^2$. What are the $[H_3O^{+}]$ of a neutral aqueous solution at $60\,^{\circ}C$ and the nature of an aqueous solution with a $pH = 7.0$ at $60\,^{\circ}C$,respectively?