Volumetric, acoustic and viscometric studies of solute-solute and solute-solvent interactions of glycine and its peptides in aqueous solutions of an antidepressant drug at different temperatures

Singh, Manjeet; Sharma, Shikha; Singh, Jeetinder; Sharma, Amit Kumar; Sharma, Meena

doi:10.1016/j.molliq.2022.118760

Cited by 6 publications

(8 citation statements)

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“…Supporting Information for this article can be found under DOI: https://doi.org/10.1002/ceat.202200575. This section includes additional references to primary literature relevant for this research [33][34][35][36][37][38][39][40][41][42][43][44][45][46].…”

Section: Supporting Informationmentioning

confidence: 99%

Templated Crystallization of Glycine Homopeptides: Experimental and Computational Developments

et al. 2023

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The usage of glass beads as heterogeneous additives for the crystallization of glycine homopeptides is investigated, whereby glass beads are shown experimentally to increase the rate of crystallization. Induction time analysis indicates that the presence of glass beads acts enhances the kinetic factor for nucleation. These results are compared to those previously obtained by the authors for glycine and diglycine, and it is demonstrated that the increase in nucleation rate is proportional to the peptide chain length. Molecular dynamics simulations confirm that larger molecules exhibit faster nucleation in the presence of glass beads due to an increased number of interactions as observed with the longest hydrogen bond lifetime for triglycine, followed by diglycine and glycine.

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Section: Supporting Informationmentioning

confidence: 99%

Templated Crystallization of Glycine Homopeptides: Experimental and Computational Developments

et al. 2023

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“…From the linear relationships between square root of molality (√ m ) and apparent molar volume ( V Φ ), we get limiting apparent molar volume, V o normalΦ ,, V normalΦ = V o normalΦ + S v √ m where m is the molality (mol.kg –1 ) of NTPH, i.e., the amount of solute (NTPH) per kilogram of solvent (water + ILs).…”

Section: Resultsmentioning

confidence: 99%

“…The negative values of K s , Φ demonstrate the preponderance of hydrophilic-ionic interactions, which further support our V Φ data. The values of K o s , normalΦ and S k are obtained from the extrapolation of the apparent molar compressibility K s , Φ at an infinite dilution using eq as ,, K s , normalΦ = K o s , normalΦ + S k m where m is the molality (mol.kg –1 ) of NTPH, i.e., the amount of solute (NTPH) per kilogram of solvent (water + ILs). Using K s , Φ values in eq (through least-square fitting), K o s , normalΦ and S k values with standard errors are determined collectively and presented in Table .…”

Section: Resultsmentioning

confidence: 99%

“…This further confirms that our results obtained from the d B /d T values are in good agreement with the results shown from Hepler’s constant. To determine the viscosity B -coefficient of transfer, we used the following equation: B t r = B 0.25em ( in aqueous ionic liquid ) − B 0.25em ( in water ) …”

Section: Resultsmentioning

confidence: 99%

“…The negative values of K s, Φ demonstrate the preponderance of hydrophilic-ionic interactions, which further support our V Φ data. The values of K o s, and S k are obtained from the extrapolation of the apparent molar compressibility K s, Φ at an infinite dilution using eq 11 as 28,33,34…”

Section: Apparent Molar Isentropic Compressibility the Apparent Molar...mentioning

confidence: 99%

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Molecular Interaction Studies of an Antidepressant Drug with Imidazolium-Based Ionic Liquids in an Aqueous System: A Volumetric, Acoustic, and Viscometric Approach

Singh

Sharma

et al. 2023

J. Chem. Eng. Data

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To study and comprehend the molecular interactions between ionic liquids (ILs) such as 1-ethyl-3-methylimidazolium bromide [EMIm]Br, 1-butyl-3-methylimidazolium bromide [BMIm]Br, and 1-hexyl-3-methylimidazolium bromide [HMIm]Br, and the antidepressant drug-nortriptyline hydrochloride (NTPH), we have examined the volumetric, acoustic, and viscometer properties of the binary and ternary solutions of different concentrations at different temperatures 288.15–318.15 K in the temperature interval of 10 K. The intermolecular interactions have been appraised and identified on the basis of different parameters, i.e., apparent molar properties (V Φ, K s, Φ), limiting apparent molar properties ( V o normalΦ , K o s , normalΦ ), viscosity coefficients A and B, limiting apparent molar transfer properties ( V o normalΦ , t r , K o s , normalΦ , t r ), viscosity B-coefficient of transfer (Btr ). Pair and triplet interaction coefficients are also determined using McMillan-Mayer theory. Based on the cosphere overlap model, the positive transfer values ( V o normalΦ , t r , K o s , normalΦ , t r ) demonstrate that ionic-hydrophilic and hydrophilic–hydrophilic interactions are dominant between NTPH-IL solutions. Additionally, the strength of these interactions increases as the alkyl chain length of the imidazolium ionic liquid increases. Furthermore, the negative values of temperature derivatives of B-coefficients (dB/dT) and the positive values of Hepler’s constant confirms the structure making nature of NTPH.

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Volumetric and Viscosity Properties for the Dilute Solution of [Bmim][OAc] in NMP and the Solute–Solvent Interaction from 288.15 to 318.15 K

Wang,

Hou,

Zhang

et al. 2024

J Solution Chem

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Volumetric, acoustic and viscometric studies of solute-solute and solute-solvent interactions of glycine and its peptides in aqueous solutions of an antidepressant drug at different temperatures

Cited by 6 publications

References 61 publications

Templated Crystallization of Glycine Homopeptides: Experimental and Computational Developments

Templated Crystallization of Glycine Homopeptides: Experimental and Computational Developments

Molecular Interaction Studies of an Antidepressant Drug with Imidazolium-Based Ionic Liquids in an Aqueous System: A Volumetric, Acoustic, and Viscometric Approach

Volumetric and Viscosity Properties for the Dilute Solution of [Bmim][OAc] in NMP and the Solute–Solvent Interaction from 288.15 to 318.15 K

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