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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 Colligative properties ： ウィキペディア英語版 Colligative properties In chemistry, colligative properties are properties of solutions that depend upon the ratio of the number of solute particles to the number of solvent molecules in a solution, and not on the type of chemical species present.〔McQuarrie, Donald, et al. ''Colligative properties of Solutions" General Chemistry Mill Valley: Library of Congress, 2011.〕 The number ratio can be related to the various units for concentration of solutions. The independence of the nature of solute particles is exact for ideal solutions, and approximate for dilute real solutions. Here we consider only those properties which result because of the dissolution of nonvolatile solute in a volatile liquid solvent.〔KL Kapoor ''Applications of Thermodynamics'' Volume 3〕 They are independent of the nature of the solute because they are due essentially to the dilution of the solvent by the solute. The word colligative is derived from the Latin ''colligatus'' meaning ''bound together''.〔K.J. Laidler and J.L. Meiser, ''Physical Chemistry'' (Benjamin/Cummings 1982), p.196〕 Colligative properties include: * Relative lowering of vapor pressure * Elevation of boiling point * Depression of freezing point * Osmotic pressure For a given solute-solvent mass ratio, all colligative properties are inversely proportional to solute molar mass. Measurement of colligative properties for a dilute solution of a non-ionized solute such as urea or glucose in water or another solvent can lead to determinations of relative molar masses, both for small molecules and for polymers which cannot be studied by other means. Alternatively, measurements for ionized solutes can lead to an estimation of the percentage of ionization taking place. Colligative properties are mostly studied for dilute solutions, whose behavior may often be approximated as that of an ideal solution. ==Relative lowering of vapour pressure== The vapor pressure of a liquid is the pressure of a vapor in equilibrium with the liquid phase. The vapor pressure of a solvent is lowered by addition of a non-volatile solute to form a solution. For an ideal solution, the equilibrium vapor pressure is given by Raoult's law as :$p\; =\; p^\_\; x\_\; +\; p^\_\; x\_\; +\; \backslash cdots$, where $p^\_$ is the vapor pressure of the ''pure'' component (i= A, B, ...) and $x\_$ is the mole fraction of the component in the solution For a solution with a solvent (A) and one non-volatile solute (B), $p^\_\; =\; 0$ and $p\; =\; p^\_\; x\_$ The vapor pressure ''lowering'' relative to pure solvent is $\backslash Delta\; p\; =\; p^\_\; -\; p\; =\; p^\_\; (1\; -\; x\_)\; =\; p^\_\; x\_$, which is proportional to the mole fraction of solute. If the solute dissociates in solution, then the vapor pressure lowering is increased by the van 't Hoff factor $i$, which represents the true number of solute particles for each formula unit. For example, the strong electrolyte MgCl2 dissociates into one Mg2+ ion and two Cl− ions, so that if ionization is complete, i = 3 and $\backslash Delta\; p\; =\; 3\; p^\_\; x\_$. The measured colligative properties show that ''i'' is somewhat less than 3 due to ion association. 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「Colligative properties」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.