“Ostwald’s dilution law”的概念、定义、翻译、参考文献-科学参考

Ostwald’s dilution law

Physics

An expression for the degree of dissociation of a weak electrolyte. For example, if a weak acid dissociates in water,

$HA ⇌ H^{+} + A^{-}$

the dissociation constant K_a is given by

$K_{a} = α^{2} n / (1 - α) V$

where α‎ is the degree of dissociation, n the initial amount of substance (before dissociation), and V the volume. If α‎ is small compared with 1, then α‎²=KV/n; i.e. the degree of dissociation is proportional to the square root of the dilution. The law was first put forward by the German physical chemist F. W. Ostwald to account for electrical conductivities of electrolyte solutions in 1888.

Chemistry

An expression for the degree of dissociation of a weak electrolyte. For example, if a weak acid dissociates in water
$HA ⇌ H^{+} {+ A}^{-} .$
The dissociation constant K_a is given by
$K_{a} {= α}^{2} n / (1 - α) V,$
where α‎ is the degree of dissociation, n the initial amount of substance (before dissociation), and V the volume. If α‎ is small compared with 1, then α‎² = KV/n; i.e. the degree of dissociation is proportional to the square root of the dilution. The law was first put forward by Wilhelm Ostwald in 1888 to account for electrical conductivities of electrolyte solutions.

单词	Ostwald’s dilution law
释义	Ostwald’s dilution law Physics An expression for the degree of dissociation of a weak electrolyte. For example, if a weak acid dissociates in water, $HA ⇌ H^{+} + A^{-}$ the dissociation constant K_a is given by $K_{a} = α^{2} n / (1 - α) V$ where α‎ is the degree of dissociation, n the initial amount of substance (before dissociation), and V the volume. If α‎ is small compared with 1, then α‎²=KV/n; i.e. the degree of dissociation is proportional to the square root of the dilution. The law was first put forward by the German physical chemist F. W. Ostwald to account for electrical conductivities of electrolyte solutions in 1888. Chemistry An expression for the degree of dissociation of a weak electrolyte. For example, if a weak acid dissociates in water $HA ⇌ H^{+} {+ A}^{-} .$ The dissociation constant K_a is given by $K_{a} {= α}^{2} n / (1 - α) V,$ where α‎ is the degree of dissociation, n the initial amount of substance (before dissociation), and V the volume. If α‎ is small compared with 1, then α‎² = KV/n; i.e. the degree of dissociation is proportional to the square root of the dilution. The law was first put forward by Wilhelm Ostwald in 1888 to account for electrical conductivities of electrolyte solutions.
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