The equilibrium constant for the autoionization of water H2...

The equilibrium constant for the autoionization of water $$\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{H}^{+}(a q)+\mathrm{OH}^{-}(a q)$$ is $1.0 \times 10^{-14}$ at $25^{\circ} \mathrm{C}$ and $3.8 \times 10^{-14}$ at $40^{\circ} \mathrm{C} .$ Is the forward process endothermic or exothermic?

The equilibrium constant for the autoionization of water
$$\mathrm{H}_{2} \mathrm{O}(l) \rightleftarrows \mathrm{H}^{+}(a q)+\mathrm{OH}^{-}(a q)$$
is $1.0 \times 10^{-14}$ at $25^{\circ} \mathrm{C}$ and $3.8 \times 10^{-14}$ at $40^{\circ} \mathrm{C} .$ Is the forward process endothermic or exothermic?

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Key Concepts

Chemical Equilibrium

Chemical equilibrium is the state in which the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products over time. In this state, the equilibrium constant (K) quantitatively describes the ratio of product concentrations to reactant concentrations, reflecting the position of equilibrium in a reversible reaction.

Temperature Dependence of Equilibrium Constant

The value of the equilibrium constant is affected by changes in temperature. According to the van't Hoff equation, an increase in temperature will increase the equilibrium constant for endothermic reactions and decrease it for exothermic reactions. This temperature dependence provides insight into the enthalpy change of the reaction.

Endothermic vs Exothermic Reactions

An endothermic reaction absorbs heat, meaning that higher temperatures favor the forward reaction by shifting the equilibrium position toward products. In contrast, an exothermic reaction releases heat, so increasing the temperature will generally shift the equilibrium toward the reactants. This concept is essential for predicting how equilibrium systems respond to temperature changes.

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