Volumetric, Viscometric and Refractive Index Behaviors of α-Amino Acids in Aqueous Caffeine Solution at Varying Temperatures

Ali, Anwar; Sabir, Saba; Tariq, Mohammad

doi:10.1016/s1872-1508(07)60008-4

Cited by 9 publications

(7 citation statements)

References 22 publications

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“…The densities, ρ, of the CAF, TPY and TBR in water and in m B , (molality of NaCl in water) = 0.1, 0.25, 0.5, 0.75, and 1.0 mol·kg –1 , have been measured at T = 288.15, 298.15, 308.15 and 318.15 K. As it can be observed from Table , the ρ values increase with the molality of the solute in water as well as in aqueous NaCl solutions and decrease with the rise of temperature. The ρ values for CAF in water are in good agreement with the literature − values (Figure S2), whereas no density values are available for comparison in case of TPY and TBR. Apparent molar volumes, V 2,ϕ , for the studied solutes have been determined from the experimentally measured densities using the relation: where M and m A are the molar mass and molality of the solutes, ρ o is the density of solvent (H 2 O or NaCl + H 2 O) and ρ is the density of solution, respectively.…”

Section: Resultssupporting

confidence: 78%

“…The V 2,ϕ values of the studied solutes are positive and decrease with the molality of solute (the representative plots of ρ and V 2,ϕ versus molality, m A , for CAF and TPY in water as a function of temperature are given in Figure a,b, respectively). These observed trends in V 2,ϕ with increasing solute concentration have also been rationalized in terms of self-association of solutes in aqueous solutions. − …”

Section: Resultsmentioning

confidence: 78%

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Volumetric, Viscometric and Spectroscopic Approach to Study the Solvation Behavior of Xanthine Drugs in Aqueous Solutions of NaCl at T = 288.15–318.15 K and at p = 101.325 kPa

et al. 2016

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The densities (ρ), viscosities (η), and 1 H nuclear magnetic resonance (NMR) studies for caffeine, theophylline, and theobromine in water and in aqueous solutions of 0.10, 0.25, 0.50, 0.75, and 1.00 mol•kg −1 sodium chloride over a temperature range T = 288.15−318.15 K and at p = 101.325 kPa have been carried out using vibrating-tube digital densimeter, micro-Ubbelohde type capillary viscometer, and Bruker (AVANCE-III, HD 500 MHz) NMR spectrometer, respectively. From the density and viscosity data, apparent molar volume (V 2,ϕ ), partial molar volume at infinite dilution (V 2,ϕ 0 ), viscosity B-coefficient, corresponding transfer (Δ tr V 2,ϕ 0 and Δ tr B) and other related parameters have been calculated. The trends in transfer parameters reveal the dominance of hydrophilic−ionic interactions at lower molalities of NaCl while hydrophobic−ionic interactions at higher molalities of NaCl. The expansibilities and dB/dT data show the structurebreaking behavior of theophylline and theobromine in water and in aqueous solutions of NaCl. However, behavior of caffeine is exceptional. The increase in chemical shift (δ) values with increasing molalities of NaCl also signifies the predominance of solute−cosolute interactions over the dehydration process. The results have further been discussed and rationalized in terms of various interactions.

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Section: Resultssupporting

confidence: 78%

Section: Resultsmentioning

confidence: 78%

Volumetric, Viscometric and Spectroscopic Approach to Study the Solvation Behavior of Xanthine Drugs in Aqueous Solutions of NaCl at T = 288.15–318.15 K and at p = 101.325 kPa

et al. 2016

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“…As a result, amino acid/peptides would not be able to exert the electrostriction effect at their maximum in the presence of dye tartrazine as compared to that in the pure water, thereby, resulting in a volume expansion and, hence, in positive transfer volumes. Similar conclusions were also drawn by others for amino acids in aqueous alkali chloride solutions [20] and in aqueous tetramethylammonium bromide solutions [21] and also by Ali et al [22] for amino acids in aqueous caffeine solution.…”

Section: Resultssupporting

confidence: 89%

Study of Thermodynamic and Transport Properties of Glycine, Diglycine, and Triglycine in Aqueous Tartrazine at Different Temperatures

Ali

Patel

Khan

et al. 2009

Zeitschrift Für Naturforschung A

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The densities (ρ), viscosities (η), and refractive indices (n D ) of (0.01, 0.05, 0.10, 0.15, and 0.20 m) amino acid, glycine, and peptides, diglycine and triglycine in 0.01 m aqueous tartrazine solution were determined at 288. 15, 293.15, 298.15, 303.15, 308.15, and 313.15 K. The density data were utilized to evaluate apparent molar volumes (φ v ) which, in turn, were used to determine partial molar volumes (φ v • ) using Masson's equation. The transfer volumes were also calculated. The viscosity data were analyzed using the Jones-Dole equation to determine the viscosity coefficients and the activation parameters. The activation parameters of viscous flow were obtained to throw light on the mechanism of viscous flow. The molar refraction was calculated using the refractive index data. The results were interpreted in the light of ion-ion, ion-nonpolar, and nonpolar-nonpolar interactions and the effect of increasing hydrophobicity as we move from glycine to triglycine on these interactions in presence of the dye tartrazine was also investigated.

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“…that b and L f behave similar in nature whereas, V f and p i shows an opposite trend to each other. As pyridine molecules are basic in nature due to the presence of one lone pair of electrons [6,20], there are some possibilities of interactions between the alcohol and pyridine. Such interactions bring the components close to each other and hence b and L f is of decreasing magnitude.…”

Section: Resultsmentioning

confidence: 99%

Dipolar interaction of pyridine with isomeric butanols

Palaniappan¹,

Jaafar²,

Jafri³

2008

Main Group Chemistry

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The net interaction energy between pyridine and isomeric forms of butanol are found experimentally from the excess values of internal pressure and free volume using ultrasonic techniques. The significance of the interaction relation is given in terms of the polar van der Waals force contribution, which is primarily dependent on statistical mixing rules. The net interaction energy, which is calculated directly from the dipole moment values, and the polarizability values are related to the energy contributions resulting from the various polar and non-polar van der Waals forces active in the interaction process. These energy contributions, which make up the total interaction energy are calculated for the interaction of the isomeric butanols with pyridine. On the basis of the results obtained, the effects of chain length and functionality of the alcohol on the interaction mechanism is discussed.

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Volumetric, Viscometric and Refractive Index Behaviors of α-Amino Acids in Aqueous Caffeine Solution at Varying Temperatures

Cited by 9 publications

References 22 publications

Volumetric, Viscometric and Spectroscopic Approach to Study the Solvation Behavior of Xanthine Drugs in Aqueous Solutions of NaCl at T = 288.15–318.15 K and at p = 101.325 kPa

Volumetric, Viscometric and Spectroscopic Approach to Study the Solvation Behavior of Xanthine Drugs in Aqueous Solutions of NaCl at T = 288.15–318.15 K and at p = 101.325 kPa

Study of Thermodynamic and Transport Properties of Glycine, Diglycine, and Triglycine in Aqueous Tartrazine at Different Temperatures

Dipolar interaction of pyridine with isomeric butanols

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