Buffer interactions: Densities and solubilities of some selected biological buffers in water and in aqueous 1,4-dioxane solutions

Taha, Mohamed; Lee, Ming‐Jer

doi:10.1016/j.bej.2009.06.009

Cited by 21 publications

(17 citation statements)

References 56 publications

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“…The detailed procedure used in this work has been delineated in our earlier articles [4][5][6][7]. The uncertainty of the solubility limit is lower than ±0.8% (relative value, S B /(mol Á kg À1 )).…”

Section: Solubility Measurementsmentioning

confidence: 99%

“…To our knowledge, there are no solubility data of MOPSO in water or in organic solvents. Hence, through our extended studies of the solubility of biological buffers in various solvents [4][5][6][7], we have now determined the solubility of MOPS and MOPSO by density measurements at T = 298.15 K in water, (water + 1,4-dioxane), and (water + ethanol) mixtures containing different concentration of the organic solvents at intervals of 10% (w/w) from 0% to 90% (w/w). Ethanol was chosen as a representative of amphiprotic hydrogen bond acceptor-donor (HBA-D) solvents.…”

Section: Introductionmentioning

confidence: 99%

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Solubility and phase separation of 4-morpholinepropanesulfonic acid (MOPS), and 3-morpholino-2-hydroxypropanesulfonic acid (MOPSO) in aqueous 1,4-dioxane and ethanol solutions

Taha

Lee

2011

The Journal of Chemical Thermodynamics

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Section: Solubility Measurementsmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

Solubility and phase separation of 4-morpholinepropanesulfonic acid (MOPS), and 3-morpholino-2-hydroxypropanesulfonic acid (MOPSO) in aqueous 1,4-dioxane and ethanol solutions

Taha

Lee

2011

The Journal of Chemical Thermodynamics

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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%

“…15, 298.15, and 308.15) K (measured by acidimeteric titration of the saturated solutions), 2 in water + 2-methoxyethanol mixtures at (288. 15, 298.15, and 308.15) K (measured by acidimeteric titration of the saturated solutions), 3 in water + 1,4-dioxane mixtures at 298 K, 4 in water + ethanol mixtures at 298 K, 5 in methanol + propylene glycol at 298 K, 6 in ethylene glycol + water at 298 K, 7 in N-methylpropionamide + water at 298 K, 8 in acetonitrile + ethylene glycol at 298.15 K, 9 in water + 2-ethoxyethanol, 10 and in water + sulfolane 11 has been reported in the literature.…”

Section: ■ Introductionmentioning

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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“…The solubility of TRIS in a number of mixed solvent systems has been reported in binary mixtures of water + 2-methoxyethanol at 288.15 K, 298.15 K, and 308.15 K (measured by acidimetric titration of the saturated solutions), 7 in mixtures of water + 1,4-dioxane at 298 K, 8 in mixtures of water + ethanol at 298 K, 9 in mixtures of MeOH + propylene glycol at 298 K, 10 in mixtures of ethylene glycol + water at 298 K, 11 in mixtures of N-methylpropionamide + water at 298 K, 12 in mixtures of acetonitrile + ethylene glycol at 298.15 K, 13 in mixtures of water +2-ethoxyethanol, 14 and in mixtures of water + sulfolane 15,7 TRIS is used by biochemists as a quality control buffer of blood pH (or other physiological samples) due to its large temperature coefficient (−0.026 pH°C). 16 Phosphate buffers on the other hand cause undesirable side reactions with the biological substances in their test samples.…”

Section: ■ Introductionmentioning

confidence: 99%

Solubility of Tris(hydroxymethyl)aminomethane in Water + Methanol +1-Propanol Mixtures at Various Temperatures

Jouyban-Gharamaleki

Soleymani

et al. 2015

J. Chem. Eng. Data

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The solubility of tris(hydroxymethyl)aminomethane (TRIS) in various mass fractions of ternary solvent mixtures of water + methanol +1-propanol at 293.2 K, 298.2 K, 303.2 K, 308.2 K, and 313.2 K was measured using a laser monitoring technique. The mole fractions of water in the ternary mixtures were between 0.90 and 0.17; the mole fraction solubility of TRIS ranged between 0.0150 and 0.1187. The generated data was mathematically represented by the combined models of Jouyban−Acree and van't Hoff, enabling the solubility to be expressed as a function of both ternary solvent compositions and temperatures. The back-calculated mole fraction solubilities agreed with the corresponding experimental values by an overall mean percentage deviation of 5.6%.

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Buffer interactions: Densities and solubilities of some selected biological buffers in water and in aqueous 1,4-dioxane solutions

Cited by 21 publications

References 56 publications

Solubility and phase separation of 4-morpholinepropanesulfonic acid (MOPS), and 3-morpholino-2-hydroxypropanesulfonic acid (MOPSO) in aqueous 1,4-dioxane and ethanol solutions

Solubility and phase separation of 4-morpholinepropanesulfonic acid (MOPS), and 3-morpholino-2-hydroxypropanesulfonic acid (MOPSO) in aqueous 1,4-dioxane and ethanol solutions

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

Solubility of Tris(hydroxymethyl)aminomethane in Water + Methanol +1-Propanol Mixtures at Various Temperatures

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