8.6
A Lei da Diluição de Ostwald
Considere um eletrólito binário AB com concentração 'c' que se dissocia reversivelmente em seus íons constituintes. O grau dessa dissociação é represe…
Baseada na teoria da dissociação eletrolítica de Arrhenius, a lei de diluição de Ostwald explica o equilíbrio em soluções eletrólitas aquosas.
Considere um eletrólito AB com concentração 'c' mol por litro, que dissocia reversivelmente em íons.
Se α é o grau de dissociação, cada íon tem concentração de equilíbrio de cα, enquanto a fração não dissociada (1 − α) tem concentração de c(1 − α). Esses termos definem a constante de equilíbrio K, chamada de constante de dissociação.
A lei de diluição de Ostwald se aplica apenas a eletrólitos fracos como ácido acético e NH₄OH.
Eletrólitos fortes como HCl e NaF estão quase completamente dissociados, com α próximos de um. Nessas condições, (1 − α) se aproxima de zero, tornando a lei matematicamente inválida.
A falha da lei para eletrólitos fortes ocorre porque, ao dissolver, a alta constante dielétrica da água enfraquece as forças eletrostáticas, levando a uma dissociação quase completa. Como resultado, não existe equilíbrio íon–molécula, e a lei de diluição de Ostwald torna-se inaplicável.
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Q1: What is Ostwald's dilution law and how does it relate to electrolyte dissociation?
Ostwald's dilution law explains equilibrium in aqueous electrolyte solutions based on Arrhenius' theory of electrolytic dissociation. For an electrolyte AB at concentration c, the dissociation constant K equals cα²/(1−α), where α is the degree of dissociation. This law describes how weak electrolytes like acetic acid and NH₄OH reversibly dissociate into ions at equilibrium.
Q2: Why does Ostwald's dilution law fail for strong electrolytes?
Strong electrolytes like HCl and NaF are almost completely dissociated, with α approaching one, making (1−α) approach zero. This renders the law mathematically invalid. Water's high dielectric constant weakens electrostatic forces, causing near-complete dissociation and eliminating the ion-molecule equilibrium that the law requires.
Q3: How do you calculate equilibrium concentrations using the degree of dissociation?
For an electrolyte AB with concentration c and degree of dissociation α, each ion has equilibrium concentration cα, while the undissociated fraction has concentration c(1−α). These concentrations define the dissociation constant K, which governs the equilibrium state of weak electrolyte solutions.
Q4: What is the difference between weak and strong electrolytes in terms of dissociation?
Weak electrolytes like acetic acid partially dissociate, with α significantly less than one, allowing Ostwald's dilution law to apply. Strong electrolytes like NaCl and NaF are electrovalent compounds formed by electron transfer; they dissociate almost completely with α near one, making the law inapplicable to them.
Q5: How does the dielectric constant of a solvent affect electrolyte dissociation?
According to Coulomb's law, the dielectric constant of the medium affects electrostatic force strength and conductivity. Water's high dielectric constant weakens electrostatic forces between ions, promoting near-complete dissociation of strong electrolytes and enabling ion mobility for electrical conduction in solutions.
Q6: What is the simplified form of Ostwald's dilution law for very weak electrolytes?
For very weak electrolytes where α is much less than one, the term (1−α) approximates to one. The dissociation constant simplifies to K ≈ cα², making calculations more straightforward for solutions with minimal dissociation and allowing easier prediction of equilibrium behavior.
Q7: What structural difference exists between strong electrolytes and weak electrolytes?
Strong electrolytes like NaCl and NaF are electrovalent compounds composed solely of ions in their crystal structure, not molecules. When dissolved in water, these ions gain mobility and conduct electricity. Weak electrolytes exist as molecules that partially dissociate into ions upon dissolution in solution.