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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 Specific ion interaction theory ： ウィキペディア英語版 Specific ion interaction theory Specific ion Interaction Theory (SIT theory) is a theory used to estimate single-ion activity coefficients in electrolyte solutions at relatively high concentrations.〔〔 It does so by taking into consideration ''interaction coefficients'' between the various ions present in solution. Interaction coefficients are determined from equilibrium constant values obtained with solutions at various ionic strengths. The determination of SIT interaction coefficients also yields the value of the equilibrium constant at infinite dilution. == Background == The need for this theory arises from the need to derive activity coefficients of solutes when their concentrations are too high to be predicted accurately by Debye-Hückel theory. These activity coefficients are needed because an equilibrium constant is defined in thermodynamics as a quotient of activities but is usually measured using concentrations. The protonation of a monobasic acid will be used to simplify the exposition. The equilibrium for protonation of the conjugate base, A− of the acid, may be written as :A− + H+ AH for which :$K=\backslash frac\backslash \}$ where signifies an activity of the chemical species HA ''etc.''. The role of water in the equilibrium has been ignored as in all but the most concentrated solutions the activity of water is a constant. Note that ''K'' is defined here as an ''association'' constant, the reciprocal of an acid dissociation constant. Each activity term can be expressed as the product of a concentration and an activity coefficient. For example, : = () × γHA where the square brackets signify a concentration and γ is an activity coefficient. Thus the equilibrium constant can be expressed as a product of a concentration quotient and an activity coefficient quotient. :$K=\backslash frac\backslash times\; \backslash frac\backslash gamma\_\}$ Taking logarithms. :$\backslash log\; K\; =\backslash log\; K^0\; +\; \backslash log\; \backslash gamma\_\; -\; \backslash log\; \backslash gamma\_\; -\; \backslash log\; \backslash gamma\_$ ''K''0 is the hypothetical value that the equilibrium constant would have if the solution of the acid were so dilute that the activity coefficients were all equal to one. It is common practise to determine equilibrium constants in solutions containing an electrolyte at high ionic strength such that the activity coefficients are effectively constant. However, when the ionic strength is changed the measured equilibrium constant will also change, so there is a need to estimate individual (single ion) activity coefficients. Debye-Huckel theory provides a means to do this, but it is accurate only at very low concentrations. Hence the need for an extension to Debye-Hückel theory. Two main approaches have been used. SIT theory, discussed here and Pitzer equations. 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「Specific ion interaction theory」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.