Correction for solute/solvent interaction extends accurate freezing point depression theory to high concentration range

Fullerton, Gary D.; Keener, C; Cameron, Ivan L.

doi:10.1016/0165-022x(94)90034-5

Cited by 15 publications

(20 citation statements)

References 26 publications

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“…T f(peak) data were used for the determination of these parameters, as it was considered to better represent the behavior of the whole phase change. Equation was followed for a w determination:

ln a_{normalw} = Δ H_{f (w)} A_{normalw} (T_{normalf} - T_{normalf} *) / true(T_{normalf} T_{normalf} * true),

where Δ H f(w) is the pure water freezing enthalpy (specific, per water gram), A w is the water molecular weight, and T f * is the equilibrium freezing point of pure water. The osmolality was calculated using Eq.…”

Section: Methodsmentioning

confidence: 99%

“…The equilibrium freezing temperature can be related to the water activity (a w ) of the system to its osmolality (p) and to its solute content. 30,31 For comparative purposes, a "sucrose equivalent" concentration (Suc eq ) and a "sodium chloride equivalent" (NaCl eq ) were determined from T f , assuming that the only solute present was sucrose or sodium chloride, respectively. T f(peak) data were used for the determination of these parameters, as it was considered to better represent the behavior of the whole phase change.…”

Section: Differential Scanning Calorimetrymentioning

confidence: 99%

See 1 more Smart Citation

Glassy State and Cryopreservation of Mint Shoot Tips

Teixeira

González‐Benito

García

2013

Biotechnology Progress

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“…T f(peak) data were used for the determination of these parameters, as it was considered to better represent the behavior of the whole phase change. Equation was followed for a w determination:

ln a_{normalw} = Δ H_{f (w)} A_{normalw} (T_{normalf} - T_{normalf} *) / true(T_{normalf} T_{normalf} * true),

Section: Methodsmentioning

confidence: 99%

Section: Differential Scanning Calorimetrymentioning

confidence: 99%

Glassy State and Cryopreservation of Mint Shoot Tips

Teixeira

González‐Benito

García

2013

Biotechnology Progress

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“…However, Equation (1) is only justified in the case of an ideal dilution, that is at very low solute concentrations, and it was observed to break down already for 0.5 molal aqueous solutions [9]. Deviations from ideal behavior stem from specific molecular interactions, namely solute-solute, solvent-solute interactions, and solute-induced variations in solvent-solvent interactions [10]. At low concentration, solvent-solute interactions are expected to play the most important role, and empirical corrections to the ideal freezing point depression law have been devised in terms of solute-solvent interaction or activity coefficients [10][11][12].…”

Section: Introductionmentioning

confidence: 93%

“…Deviations from ideal behavior stem from specific molecular interactions, namely solute-solute, solvent-solute interactions, and solute-induced variations in solvent-solvent interactions [10]. At low concentration, solvent-solute interactions are expected to play the most important role, and empirical corrections to the ideal freezing point depression law have been devised in terms of solute-solvent interaction or activity coefficients [10][11][12]. Equation (1) can be generalised to take into account deviations from the linear behaviour due to the partial dissociation of solutes, by including the Van't Hoff dissociation factor i, so that…”

Section: Introductionmentioning

confidence: 99%

Freezing point depression in model Lennard-Jones solutions

et al. 2015

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Crystallisation of liquid solutions is of uttermost importance in a wide variety of processes in materials, atmospheric and food science. Depending on the type and concentration of solutes the freezing point shifts, thus allowing control on the thermodynamics of complex fluids. Here we investigate the basic principles of solute-induced freezing point depression by computing the melting temperature of a Lennard-Jones fluid with low concentrations of solutes, by means of equilibrium molecular dynamics simulations. The effect of solvophilic and weakly solvophobic solutes at low concentrations is analysed, scanning systematically the size and the concentration. We identify the range of parameters that produce deviations from the linear dependence of the freezing point on the molal concentration of solutes, expected for ideal solutions. Our simulations allow us also to link the shifts in coexistence temperature to the microscopic structure of the solutions.

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“…This study uses the interactioncorrected method of modifying thermodynamic expressions, which was first presented as a set of empirical equations (Fullerton et al, 1992(Fullerton et al, , 1993; Kanal et al, 1994). This method was recently more rigorously related to the existing body of thermodynamic knowledge (Fullerton et al, 1994).…”

Section: Introductionmentioning

confidence: 99%

Solution nonideality related to solute molecular characteristics of amino acids

Keener¹,

Fullerton²,

Cameron³

et al. 1995

Biophysical Journal

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By measuring the freezing-point depression for dilute, aqueous solutions of all water-soluble amino acids, we test the hypothesis that nonideality in aqueous solutions is due to solute-induced water structuring near hydrophobic surfaces and solute-induced water destructuring in the dipolar electric fields generated by the solute. Nonideality is expressed with a single solute/solvent interaction parameter I, calculated from experimental measure of delta T. A related parameter, I(n), gives a method of directly relating solute characteristics to solute-induced water structuring or destructuring. I(n)-values correlate directly with hydrophobic surface area and inversely with dipolar strength. By comparing the nonideality of amino acids with progressively larger hydrophobic side chains, structuring is shown to increase with hydrophobic surface area at a rate of one perturbed water molecule per 8.8 square angstroms, implying monolayer coverage. Destructuring is attributed to dielectric realignment as described by the Debye-Hückel theory, but with a constant separation of charges in the amino-carboxyl dipole. By using dimers and trimers of glycine and alanine, this destructuring is shown to increase with increasing dipole strength using increased separation of fixed dipolar charges. The capacity to predict nonideal solution behavior on the basis of amino acid characteristics will permit prediction of free energy of transfer to water, which may help predict the energetics of folding and unfolding of proteins based on the characteristics of constituent amino acids.

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Correction for solute/solvent interaction extends accurate freezing point depression theory to high concentration range

Cited by 15 publications

References 26 publications

Glassy State and Cryopreservation of Mint Shoot Tips

Glassy State and Cryopreservation of Mint Shoot Tips

Freezing point depression in model Lennard-Jones solutions

Solution nonideality related to solute molecular characteristics of amino acids

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