Solute–solvent and solvent–solvent interactions of menthol in isopropyl alcohol and its binary mixtures with methyl salicylate by volumetric, viscometric, interferometric and refractive index techniques

Sah, Radhey Shyam; Pradhan, Prasanna; Roy, Mahendra Nath

doi:10.1016/j.tca.2009.12.001

Cited by 11 publications

(6 citation statements)

References 22 publications

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“…The greater the difference in the molar volume the greater is the fitness of the solute molecules in the solvent mixture rendering higher solute–solvent interaction. The same type of work has been done by the workers reported earlier . The limiting partial molar volume of citric acid is far greater than that of the cetrimonium bromide solution reported in Table , and the said volume of the citric acid further increases with the temperature and the concentration of the cetrimonium bromide.…”

Section: Resultssupporting

confidence: 60%

Densities and Viscosities of Citric Acid in Aqueous Cetrimonium Bromide Solutions with Reference to the Manifestation of Solvation

et al. 2011

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Apparent molar volumes (V φ ) and viscosity B-coefficients for citric acid in (0.001, 0.003, and 0.005) mol 3 dm À3 aqueous cetrimonium bromide (N-cetyl-N,N,N-trimethyl ammonium bromide, C 19 H 42 NBr) solutions have been determined from solution density and viscosity measurements at T = (298.15, 308.15, and 318.15) K and p = 0.1 MPa as a function of the concentration of citric acid. The apparent molar volumes have been extrapolated to zero concentration to obtain the limiting values at infinite dilution (V φ 0 ), using the RedlichÀMeyer equation, and the obtained parameters have been interpreted in terms of soluteÀsolvent interactions. The viscosity data were analyzed using the JonesÀDole equation, and the derived parameters A and B have also been interpreted in terms of soluteÀsolute and soluteÀsolvent interactions, respectively, in the mixed solutions. The structure-making or -breaking ability of the electrolyte has been discussed in terms of sign of dB/dT. The activation parameters of viscous flow for the ternary solutions studied have also been calculated and explained by the application of transition state theory.

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Section: Resultssupporting

confidence: 60%

Densities and Viscosities of Citric Acid in Aqueous Cetrimonium Bromide Solutions with Reference to the Manifestation of Solvation

et al. 2011

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“…The greater the difference in the volume, the greater is the fitness of the solute molecules in the solvent mixture rendering higher solute−solvent interaction. The same type of work has been done by the workers reported earlier . The limiting apparent molar volume of the three carbohydrates is far greater than the molar volume of the cetrimonium bromide solution.…”

Section: Resultsmentioning

confidence: 53%

“…The same type of work has been done by the workers reported earlier. 4 The limiting apparent molar volume of the three carbohydrates is far greater than the molar volume of the cetrimonium bromide solution. The limiting apparent molar volume of the carbohydrates further increases with the temperature and the concentration of the cetrimonium bromide.…”

Section: Resultsmentioning

confidence: 99%

Apparent Molar Volumes and Viscosity B-Coefficients of Carbohydrates in Aqueous Cetrimonium Bromide Solutions at (298.15, 308.15, and 318.15) K

et al. 2010

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Apparent molar volumes (φ V ) and viscosity B-coefficients for some carbohydrates (D-glucose, D-mannitol, and D-sucrose) in (0.001, 0.003, and 0.005) mol • kg -1 aqueous cetrimonium bromide (N-cetyl-N,N,N-trimethyl ammonium bromide) (C 19 H 42 BrN) solutions have been determined from solution density, F, and viscosity, η, measurements at (298.15, 308.15, and 318.15) K as a function of the concentration of carbohydrates. The limiting apparent molar volume (φ V 0 ) and experimental slopes (S V *) obtained from the Masson equation have been interpreted in terms of solute-solvent and solute-solute interactions, respectively. The viscosity data were analyzed using the Jones-Dole equation, and the derived parameters A and B have also been interpreted in terms of solute-solute and solute-solvent interactions, respectively, in the mixed solutions. The structuremaking or -breaking ability of carbohydrates has been discussed in terms of the sign of (δ 2 φ V 0 /δT 2 ) P as well as dB/dT. The three-dimensional representation of the investigated molecules concerned with this paper is shown below for a better understanding.

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“…It is worth noting that this behavior was also observed for many systems. We can cite the (methanol + methyl acetate) system reviewed by [30], the (methanol + ethyl acetate), the (ethanol + methyl acetate) and (ethanol + ethyl acetate) systems studied by [29], the (methanol + isopropyl alcohol), the (methyl salicylate + DMSO) and (hydroxamic acid + DMSO) examined by [31]. e V 0 ϕ values of the mixtures rise in the following order: (piperazine + methanol) < (piperazine + water) < (piperazine + acetone), which could be due-as explained by [29]-to an enhancement in the strengths of the solute to solvent interactions.…”

Section: Resultsmentioning

confidence: 99%

Densities, Apparent Molar Volume, Expansivities, Hepler’s Constant, and Isobaric Thermal Expansion Coefficients of the Binary Mixtures of Piperazine with Water, Methanol, and Acetone at T = 293.15 to 328.15 K

Omar

Jaubert

Awan

2018

International Journal of Chemical Engineering

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The properties of 3 binary mixtures containing piperazine were investigated in this work. In a first step, the densities for the two binary mixtures (piperazine + methanol) and (piperazine + acetone) were measured in the temperature range of 293.15 to 328.15 K and 293.15 to 323.15 K, respectively, at atmospheric pressure by using a Rudolph research analytical density meter (DDM 2911). The concentration of piperazine in the (piperazine + methanol) mixture was varied from 0.6978 to 14.007 mol/kg, and the concentration of piperazine in the (piperazine + acetone) mixture was varied from 0.3478 to 1.8834 mol/kg. On the other hand, the density data for the (piperazine + water) mixture were taken from the literature in the temperature range of 298.15 to 328.15 K. In a second step, for the 3 investigated systems, the apparent molar volume (Vϕ) and the limiting apparent molar volume (Vϕ0) at infinite dilution were calculated using the Redlich–Mayer equation. The limiting apparent molar volumes (Vϕ0) were used to study the influence of the solute-solvent and solute-solute interactions. The temperature dependency of the apparent molar volumes was used to estimate the apparent molar expansibility, Hepler’s constant ∂2Vϕ0/∂T2P, and isobaric thermal expansion coefficients αP.

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Solute–solvent and solvent–solvent interactions of menthol in isopropyl alcohol and its binary mixtures with methyl salicylate by volumetric, viscometric, interferometric and refractive index techniques

Cited by 11 publications

References 22 publications

Densities and Viscosities of Citric Acid in Aqueous Cetrimonium Bromide Solutions with Reference to the Manifestation of Solvation

Densities and Viscosities of Citric Acid in Aqueous Cetrimonium Bromide Solutions with Reference to the Manifestation of Solvation

Apparent Molar Volumes and Viscosity B-Coefficients of Carbohydrates in Aqueous Cetrimonium Bromide Solutions at (298.15, 308.15, and 318.15) K

Densities, Apparent Molar Volume, Expansivities, Hepler’s Constant, and Isobaric Thermal Expansion Coefficients of the Binary Mixtures of Piperazine with Water, Methanol, and Acetone at T = 293.15 to 328.15 K

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