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翻訳と辞書　辞書検索 [ 開発暫定版 ] スポンサード リンク Debye–Hückel equation ： ウィキペディア英語版 Debye–Hückel equation The chemists Peter Debye and Erich Hückel, noticed that solutions that contain ionic solutes do not behave ideally even at very low concentrations. So, while the concentration of the solutes is fundamental to the calculation of the dynamics of a solution, they theorized that an extra factor that they termed gamma is necessary to the calculation of the activity coefficients of the solution. Hence they developed the Debye–Hückel equation and Debye–Hückel limiting law. The activity is only proportional to the concentration and is altered by a factor known as the activity coefficient $\backslash \; \backslash gamma\; \backslash ,$. This factor takes into account the interaction energy of ions in the solution. == Debye–Hückel limiting law == :''For the principles used to derive this equation see'' Debye–Hückel theory In order to calculate the activity, $\backslash \; a\_C\; \backslash ,$, of an ion, C, in a solution, one must know the concentration and the activity coefficient: :$\backslash \; a\_C\; =\; \backslash gamma\; \backslash frac">)\}\backslash ,$ where :$\backslash \; \backslash gamma\; \backslash ,$ is the activity coefficient of C :$\backslash \; ()\backslash ,$ is the concentration of the chosen ''standard state'', e.g. 1 mol/kg if we work in molality. :$()$ is a measure of the concentration of C : Dividing $()$ with $()$ gives a dimensionless quantity The ''Debye–Hückel limiting law'' enables one to determine the activity coefficient of an ion in a ''dilute'' solution of known ionic strength. The equation is :$\backslash ln(\backslash gamma\_i)\; =\; -\; \backslash frac\; =\; -\; \backslash frac\}\}=\; -\; A\; z\_i^2\; \backslash sqrt$ ::$z\_i$ is the charge number of ion species i ::$q$ is the elementary charge ::$\backslash kappa$ is the inverse of the Debye screening length, defined below ::$\backslash varepsilon\_r$ is the relative permittivity of the solvent ::$\backslash varepsilon\_0$ is the permittivity of free space ::$k\_B$ is Boltzmann's constant ::$T$ is the temperature of the solution ::$N\_\backslash mathrm$ is Avogadro's number ::$I$ is the ionic strength of the solution, defined below ::$A$ is a constant that depends on temperature. If $I$ is expressed in terms of molality, instead of molarity (as in the equation above and in the rest of this article), then an experimental value for $A$ of water is $1.172\; \backslash text^\; \backslash text^$ at 25 C. It is common to use a base-10 logarithm, in which case we factor $\backslash ln\; 10$, so A is $0.509\backslash text^\; \backslash text^$. It is important to note that because the ions in the solution act together, the activity coefficient obtained from this equation is actually a mean activity coefficient. 抄文引用元・出典: フリー百科事典『 ウィキペディア（Wikipedia）』 ■ウィキペディアで「Debye–Hückel equation」の詳細全文を読む スポンサード リンク 翻訳と辞書 : 翻訳のためのインターネットリソース Copyright(C) kotoba.ne.jp 1997-2016. All Rights Reserved.