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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 Van 't Hoff factor ： ウィキペディア英語版 Van 't Hoff factor The van 't Hoff factor $i$ (named after J. H. van 't Hoff) is a measure of the effect of a solute upon colligative properties such as osmotic pressure, relative lowering in vapor pressure, elevation of boiling point and freezing point depression. The van 't Hoff factor is the ratio between the actual concentration of particles produced when the substance is dissolved, and the concentration of a substance as calculated from its mass. For most non-electrolytes dissolved in water, the van 't Hoff factor is essentially 1. For most ionic compounds dissolved in water, the van 't Hoff factor is equal to the number of discrete ions in a formula unit of the substance. This is true for ideal solutions only, as occasionally ion pairing occurs in solution. At a given instant a small percentage of the ions are paired and count as a single particle. Ion pairing occurs to some extent in all electrolyte solutions. This causes deviation from the van 't Hoff factor. The deviation for the van 't Hoff factor tends to be greatest where the ions have multiple charges. ==Dissociated solutes== The degree of dissociation is the fraction of the original solute molecules that have dissociated. It is usually indicated by the Greek symbol $\backslash alpha$. There is a simple relationship between this parameter and the van't Hoff factor. If a fraction $\backslash alpha$ of the solute dissociates into $n$ ions, then :::$i\; =\; \backslash alpha\; n\; +\; (1-\; \backslash alpha)\; =\; 1\; +\; \backslash alpha\; (n\; -\; 1)$ For example, the dissociation :::KCl K+ + Cl− yields $n\; =\; 2$ ions, so that $i\; =\; 1\; +\; \backslash alpha$ 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「Van 't Hoff factor」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.