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Solutions: Osmotic Coefficient the Chemical Potential of (Solvent) Water in an Aqueous Solution Can Be Related to the Mole Fraction Composition of the Solution

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Solutions: Osmotic Coefficient the Chemical Potential of (Solvent) Water in an Aqueous Solution Can Be Related to the Mole Fraction Composition of the Solution Topic550 Chemical Potentials: Solutions: Osmotic Coefficient The chemical potential of (solvent) water in an aqueous solution can be related to the mole fraction composition of the solution. However, there is a possible disadvantage in an approach using the mole fraction scale to express the composition of a solution. We note that our interest is often in the properties of solutes in aqueous solutions, that the amount of solvent greatly exceeds the amount of solute in a solution, and that the sensitivity of equipment developed by chemists is sufficient to probe the properties of quite dilute solutions. Consequently the mole fraction scale for the solvent is not the most convenient method for expressing the composition of a given solution [1]. Hence another equation relating µ 1(aq;T;p) to the composition of a solution finds favour. By definition, for a solution containing a single solute, chemical substance j, [2], µµφ=−⋅⋅⋅⋅* 11(aq ;;) T p (;;)l T p R T M 1 m j (a) In terms of the standard chemical potential for water at temperature T, p µ (aq;T;p) = µ0 ( ;T) − φ ⋅ R ⋅ T ⋅ M ⋅ m + V* ( ) ⋅ dp (b) 1 1 l 1 j ∫ 1 l p0 M1 is the molar mass of water; φ is the practical osmotic coefficient which is characteristic of the solute, molality mj, temperature and pressure. By definition, φ is unity for ideal solutions at all temperatures and pressures. → φ limit(m j 0) = 1.0 at all T and p. (c) ∂φ ∂ Further for ideal solutions, the partial differentials ( / T) p , ∂φ22 ∂ ∂φ ∂ (/)T p and (/)p T are zero. For an ideal solution [3], µµ=−⋅⋅⋅* 11(;;;)aq T p id (;;)l T p R T M 1 m j (d) We rewrite equation (d) in the following form: µµ−=−⋅⋅⋅* 11(;;;)aqTpid (;;)l Tp R T M 1 mj (e) Hence with an increase in molality of solute in an ideal aqueous solution, the solvent is stabilised, being at a lower chemical potential than that for pure water(l) .We contrast the chemical potentials of the solvent in real and ideal solutions using an excess µ E chemical potential, 1 (;;);aq T p µE = µ − µ 1 (aq;T;p) 1 (aq;T;p) 1 (aq;id;T;p) =−⋅⋅⋅⋅φ (1 ) R T M1 m j (f) The term (1–φ) is often encountered because it expresses succinctly the impact of a solute on the properties of a solvent. At a given molality (and fixed temperature and pressure), φ is characteristic of the solute. Footnote [1] Mole fractions of solvent x1 and solute xj for aqueous solutions having gradually increasing molality of solute mj. −−1 = 3 -5 (a) mj / mol kg 10 ; x1 = 0.999982 xj = 1.8x10 −−1 = 2 -4 (b) mj / mol kg 10 ; x1 = 0.99982 xj = 1.8x10 −−1 = 1 -3 (c) mj / mol kg 10 ; x1 = 0.9982 xj = 1.8x10 −1 = -3 (d) mj / mol kg 0.5; x1 = 0.9911 xj = 8.9x10 −1 = -2 (e) mj /. mol kg 10; x1 = 0.9823 xj = 1.77x10 [J mol−1 ] = [2] . [J mol−1 ] − [1]⋅[J K -1 mol−1 ]⋅[K]⋅[kg mol−1 ]⋅[mol kg −1 ] [3] The definitions of ideal solutions expressed here and in terms of mole fraction of solvent are not in conflict. For an ideal solution these equations require that, −⋅= M11m j ln(x ) =+=−+⋅−−1 1 But ln(xMMm11 ) ln[ / (1 jj )] ln(10 . mM1 ) Bearing in mind that M1 = 0.018 kg mol-1, for dilute solutions +⋅ =⋅ ln(1.0 m jjM11) m M . .
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