If a neutral solution of water, with pH=7.00, is heated to 50^∘ C, the pH drops to 6.63 . Does t

step 1 Problem 27. No. In pure water, the only source of hydrogen ion is the auto -ionization reaction

If a neutral solution of water, with pH=7.00, is heated to...

If a neutral solution of water, with $\mathrm{pH}=7.00$, is heated to $50^{\circ} \mathrm{C}$, the pH drops to 6.63 . Does this mean that the concentration of $\left[\mathrm{H}^{+}\right]$ is greater than the concentration of $\left[\mathrm{OH}^{-}\right] ?$ Explain.

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Key Concepts

Ion Product of Water (Kw)

The ion product of water, Kw, is the product of the molar concentrations of hydrogen ions and hydroxide ions in water. Kw is a temperature-dependent constant, meaning that as temperature changes, the numerical value of Kw changes, which in turn affects the pH of pure water even though the solution remains neutral with equal concentrations of H? and OH?.

pH and Temperature Relationship

pH is defined as the negative logarithm of the hydrogen ion concentration and is commonly referenced relative to standard conditions (typically 25°C). However, because the ion product of water (Kw) increases with temperature, the neutral pH of water decreases below 7 at temperatures above 25°C, even though the water remains neutral, meaning that the [H?] and [OH?] concentrations are still equal.

Autoionization of Water

Autoionization of water refers to the process by which water molecules dissociate into hydrogen ions (H?) and hydroxide ions (OH?). This equilibrium process is intrinsic to water and ensures that in a pure water solution, the concentrations of H? and OH? remain equal regardless of the absolute values of these concentrations.

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