Non-linear van't Hoff solubility-temperature plots and their pharmaceutical interpretation

Grant, David J.W.; Mehdizadeh, Mehdi; Chow, Albert H.L.; Fairbrother, J.E.

doi:10.1016/0378-5173(84)90104-2

Cited by 350 publications

(219 citation statements)

References 22 publications

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“…Ethanol and propylene glycol are probably the more widely used cosolvents in parenteral medications. This investigation expands the concepts developed for this drug in cosolvent systems by Pérez et al 2 in ethanol + water, propylene glycol + water, and ethanol + propylene glycol mixtures at 25.0 °C, by Grant et al 6 in water at several temperatures, by Etman and Naggar 7 in sugar aqueous solutions at 20.0 and 37.0 °C, by Bustamante and coworkers 8 in ethanol + water, ethanol + ethyl acetate, and dioxane + water mixtures at several temperatures, and Martínez 9 in propylene glycol + water mixtures at 25.0 °C, among others.…”

Section: Introductionmentioning

confidence: 91%

Thermodynamic study of the solubility of acetaminophen in propylene glycol + water cosolvent mixtures

Jimenez¹,

Martínez²

2006

J. Braz. Chem. Soc.

107

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Baseado nas equações de van't Hoff e Gibbs, as funções termodinâmicas energia de Gibbs, entalpia e entropia de solução, mistura e solvatação de acetaminofen em misturas dos solventes propileno glicol + água (PG + W), foram avaliadas por medidas de solubilidade em diversas temperaturas. A solubilidade foi maior para 100% de PG em todas as temperaturas estudadas. A solvatação dessa droga nas misturas aumenta com o aumento da proporção de PG, atingindo um máximo em 70% de PG. De 0% até 20% de PG e de solução 70% até 100% de PG, foi encontrado um domínio da entropia sobre o processo, enquanto de água pura até 10% de PG e de 20% até 70% de PG, foi encontrado domínio da entropia. Estes fatos são explicados em termos de perda da estrutura da água, e uma diminuição na energia requerida para formação da cavidade no solvente, para misturas de 30% até 70% de PG.Based on van't Hoff and Gibbs equations the thermodynamic functions Gibbs energy, enthalpy, and entropy of solution, mixing and solvation of acetaminophen in propylene glycol + water (PG + W) cosolvent mixtures, were evaluated from solubility data determined at several temperatures. The solubility was greater at 100% of PG at all temperatures studied. The solvation of this drug in the mixtures increases as the PG proportion is also increased founding a maximum at 70% of PG. From 10% up to 20% of PG and from 70% up to 100% of PG, entropy driving was found, while from pure water up to 10% of PG and from 20% up to 70% of PG, enthalpy driving was found. These facts can be explained in terms of water-structure loss, and a diminishing in the energy required for cavity formation in the solvent, for mixtures from 30% up to 70% of PG.

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Section: Introductionmentioning

confidence: 91%

Thermodynamic study of the solubility of acetaminophen in propylene glycol + water cosolvent mixtures

Jimenez¹,

Martínez²

2006

J. Braz. Chem. Soc.

107

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“…Data processing was performed using the "Universal Analysis" software supplied with the instrument. c p,sl is frequently estimated using three assumptions, based on empirical evidence; c p,sl =0 (Yalkowsky et al, 1981;Prausnitz et al, 1986), c p,sl =0.5 S fus (Tsonopoulos, 1970) and c p,sl = S fus (Mauger et al, 1972;Grant et al, 1984) which is used in this work.…”

Section: Methodsmentioning

confidence: 99%

Solid state and sub-cooled liquid vapour pressures of substituted dicarboxylic acids using Knudsen Effusion Mass Spectrometry (KEMS) and Differential Scanning Calorimetry

et al. 2010

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Abstract. Solid state vapour pressures of a selection of atmospherically important substituted dicarboxylic acids have been measured using Knudsen Effusion Mass Spectrometry (KEMS) over a range of 20 K (298-318 K). Enthalpies of fusion and melting points obtained using Differential Scanning Calorimetry (DSC) were used to obtain sub-cooled liquid vapour pressures. They have been compared to estimation methods used on the E-AIM website. These methods are shown to poorly represent -OH groups in combination with COOH groups. Partitioning calculations have been performed to illustrate the impact of the different estimation methods on organic aerosol mass compared to the use of experimental data.

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“…The solubility data of TRIS in each solvent system at various temperatures (x T ) could be mathematically represented using the van't Hoff equation 21 = + x A B T ln T (4) where A and B are the model constants calculated using a leastsquare method. Table 3 lists the model constant and the MPD values for the back-calculated data using eq 4.…”

Section: ■ Experimental Sectionmentioning

confidence: 99%

Solubility Determination of Tris(hydroxymethyl)aminomethane in Water + Methanol Mixtures at Various Temperatures Using a Laser Monitoring Technique

Jouyban-Gharamaleki

Soleymani³

et al. 2014

J. Chem. Eng. Data

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The solubility of tris(hydroxymethyl)-aminomethane (TRIS) in various mass fractions of water + methanol solvent mixtures at (293.2, 298.2, 303.2, 308.2, and 313.2) K was measured using a laser monitoring technique. The generated data were mathematically represented using the Jouyban−Acree model. The back-calculated mole fraction solubilities are in good agreement with the corresponding experimental values as documented by an overall mean percentage deviation of 3.2 %. ■ INTRODUCTIONSolubility data enable researchers to select the most appropriate solvent system for solubilization or crystallization of a solute. Mixed solvents provide "tunable polarity solvents" to alter the solubility of a given solute. These mixtures are also used as mobile phases and/or solvents for the background electrolytes in analytical separation methods such as high-performance liquid chromatography (HPLC) or capillary electrophoresis (CE) where the low solubility of electrolytes at higher concentrations of the organic solvent might be a limiting parameter. Mixed solvents applied in this context may improve the solubility of the analyte, the resolution of the peaks of various analytes, or determine other relevant analytical parameters like pK a values, partition coefficients, or electrophoretic and electroosmotic mobilities. A quick survey on the published HPLC and CE methods for pharmaceutical analysis showed that TRIS buffer has been used primarily in the following binary solvent systems. The most frequently used mixed solvents are water + acetonitrile (55 %), followed by water + methanol (36 %), water + ethanol (4 %), methanol + acetonitrile (3 %), and water + 1-propanol (2 %). 12Because of this high practical importance, it was our intention to measure the solubility of TRIS in binary aqueous mixtures of methanol at different temperatures for validating a lab-made setup and to extend the available database of solubilities. 13 To enable the calculation of the solubility of TRIS at any composition of the binary solvent mixture and temperatures, we fitted the data to the Jouyban−Acree model and its combined version with the van't Hoff equation.

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Non-linear van't Hoff solubility-temperature plots and their pharmaceutical interpretation

Cited by 350 publications

References 22 publications

Thermodynamic study of the solubility of acetaminophen in propylene glycol + water cosolvent mixtures

Thermodynamic study of the solubility of acetaminophen in propylene glycol + water cosolvent mixtures

Solid state and sub-cooled liquid vapour pressures of substituted dicarboxylic acids using Knudsen Effusion Mass Spectrometry (KEMS) and Differential Scanning Calorimetry

Solubility Determination of Tris(hydroxymethyl)aminomethane in Water + Methanol Mixtures at Various Temperatures Using a Laser Monitoring Technique

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