El óxido de deuterio ( D2 O, donde D es deuterio, el isótopo de hidrógeno 2) tiene una constante

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El óxido de deuterio ( D2 O, donde D es deuterio, el isótopo...

El óxido de deuterio ( $\mathrm{D}_2 \mathrm{O}$, donde $\mathrm{D}$ es deuterio, el isótopo de hidrógeno 2) tiene una constante de producto iónico, $K_{\mathrm{xu}}$ de $8.9 \times 10^{-16}$ a $20^{\circ} \mathrm{C}$. Calcule $\left[\mathrm{D}^{+}\right]$y $\left[\mathrm{OD}^{-}\right]$del $\mathrm{D}_2 \mathrm{O}$ puro (neutro) a esta temperatura.

Key Concepts

Autoionization of Water

Autoionization refers to the process by which a water molecule reacts with another water molecule to produce a pair of ions. In both ordinary water (H2O) and heavy water (D2O), autoionization is an equilibrium process where two identical molecules donate a proton (or deuteron) resulting in a hydronium (or deuteronium) ion and a hydroxide (or deuteroxide) ion. This process is fundamental to understanding the acid-base properties of the solvent.

Ion Product Constant

The ion product constant (often denoted as Kw for water) represents the equilibrium constant for the autoionization reaction. It is the product of the molar concentrations of the ions formed in this process. For heavy water, this constant is typically different in magnitude compared to ordinary water due to isotopic substitution, and it is used to determine the concentration of ions in pure heavy water under neutral conditions.

Equilibrium Concentration Calculation

In a neutral solution, the concentrations of the ions produced by autoionization are equal. Therefore, if x is the concentration of both ions, the ion product constant is given by the equation x² = K. Hence, the equilibrium concentration of each ion can be calculated by taking the square root of the ion product constant. This method is universally applicable for determining ion concentrations in weakly autoionizing solvents.

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