The ionization of water $\left(\mathrm{H}_2 \mathrm{O}(\mathrm{l}) \rightleftharpoons \mathrm{H}^{+}

Question

The ionization of water $\left(\mathrm{H}_2 \mathrm{O}(\mathrm{l}) ightleftharpoons \mathrm{H}^{+}(\mathrm{aq})+\mathrm{OH}^{-}(\mathrm{aq})ight)$ has an equilibrium constant of $1 	imes 10^{-14}$ at 298 K . The $\Delta \mathrm{G}^0$ of the reaction is $\mathrm{kJ} / \mathrm{mol}$

Professor PC Thomas Classes · Answer

Ionization is endothermic; $K_w$ increases with temperature.