Co-solubilisation of a binary mixture of isoflavones in a water micellar solution of sodium cholate or cetyltrimethylammonium bromide: Influence of micelle structure

Poša, Mihalj; Pilipović, Ana; Torović, Ljilja; Hogervorst, Jelena Cvejić

doi:10.1016/j.molliq.2018.10.007

Cited by 9 publications

(15 citation statements)

References 36 publications

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“…Micellar Solubilization. The capacity of an aqueous micellar solution to solubilize a poorly soluble particle (i.e., the solubilizate) in water is expressed by the molar solubilization ratio (MSR): 47,48 S S n MSR cmc cmc…”

Section: Resultsmentioning

confidence: 99%

Binary Mixed Micelles of Hexadecyltrimethylammonium Bromide–Sodium Deoxycholate and Dodecyltrimethylammonium Bromide–Sodium Deoxycholate: Thermodynamic Stabilization and Mixed Micelle Solubilization Capacity of Daidzein (Isoflavonoid)

Kumar,

Farkaš Agatić,

Popović

et al. 2024

Ind. Eng. Chem. Res.

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In this paper, the thermodynamic properties of binary mixtures of the surfactants hexadecyltrimethylammonium bromide (HA)−sodium deoxycholate (DC) and dodecyltrimethylammonium bromide (DA)−sodium deoxycholate (DC) in an aqueous NaCl solution (0.3 mol kg −1 ) in the temperature interval T = 273.1−323.1 K are examined. In binary mixed micelles such as HA−DC and DA−DC, there are synergistic interactions between structurally different micellar building units. The dependence of the molar excess Gibbs free energy of the formation of the binary mixed micellar pseudophase on the micellar molar fractions of the surfactants (g E = f(x i )) is a symmetric function (a first-order Margules function) where the molar excess entropy is not zero, i.e., the strict theory of regular mixtures does not apply. If the phenomenon of enthalpy−entropy compensation is valid for each partial thermodynamic process during the formation of a binary mixed micellar pseudophase (at a constant temperature) and there is an interval of surfactant mole fraction from the initial binary mixture, where each ratio between the enthalpy of a certain partial thermodynamic process and the RST enthalpy is constant, then the function g E = f(x i ) is a symmetric function. Both of the investigated binary micellar pseudophases in the solubilization of daidzein (D) exhibit synergistic solubilization in relation to the micellar solubilization of D with a system of monocomponent surfactants. The molar excess Gibbs free energies of D micellar solubilization with the mixed micelles HA−DC and DA−DC are negative, which means that binary mixed micellar pseudophases with the solubilizate D are more thermodynamically stable than systems with monocomponent micellar pseudophases containing solubilizate D.

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Section: Resultsmentioning

confidence: 99%

Binary Mixed Micelles of Hexadecyltrimethylammonium Bromide–Sodium Deoxycholate and Dodecyltrimethylammonium Bromide–Sodium Deoxycholate: Thermodynamic Stabilization and Mixed Micelle Solubilization Capacity of Daidzein (Isoflavonoid)

Kumar,

Farkaš Agatić,

Popović

et al. 2024

Ind. Eng. Chem. Res.

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“…According to the given theory of co-solubilization, the standard molar Gibbs energy of the micellar co-solubilization of the solubilizate i is given by the following equation: where is the standard molar Gibbs energy of the micellar solubilization of a monocomponent solubilizate, μ i ( s ) 0 is the chemical potential of the monocomponent solid phase of molecule i , μ i ( m ) 0 is the standard chemical potential of molecule i in the micellar pseudophase, g i e is the excess molar Gibbs energy of the solubilizate i in the micellar pseudophase with j , and is the mole fraction of the solubilizate i in the micelle pseudophase that contains hydrophobic molecule j .…”

Section: Resultsmentioning

confidence: 99%

“…The Gibbs energy of the micellar co-solubilization of the binary mixture of solubilizates i and j can be represented as the sum of the Gibbs energy of the micellar solubilization of the monocomponent solubilizates i and j and the Gibbs energy of mixing of the micellar monocomponent phases: It has been shown that in the process of co-solubilization, the Gibbs energy of mixing is equal to the excess Gibbs energy of mixing, which contains excess intermolecular interactions not included in the micellar pseudophase with monocomponent solubilizates: For the asymmetrical function of the binary mixture of solubilizates, g mix e = f ( x i ), the second order Margules function is used ( i = 1-NpOH or 2-NpOH): where a ij and a ji are parameters of the function. For the component i of the binary mixture of solubilizates in the micellar pseudophase for which the second order Margules function is valid, the molar Gibbs free energy is calculated as the derivative of the total Gibbs free energy of mixing of the binary mixture of naphthols by the amount n i ( n = n G + n D ): Therefore, with added context of the binary mixture of naphthols in the micellar pseudophase, the logarithm form of the interaction parameters can be represented as the following: …”

Section: Resultsmentioning

confidence: 99%

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Co-Solubilization of the Binary Mixture of 1-Naphthol and 2-Naphthol in the Water Micellar Solution of Sodium Cholate and Cetyltrimethylammonium Bromide

et al. 2019

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The micellar co-solubilization of αand β-naphthol and their binary mixture with surfactants sodium cholate (SC) and cetyltrimethylammonium bromide (CTAB) is examined. The micellar solubilization of 2-naphthol (2-NpOH) in SC is entropic, and it is an energetically more favored process than the micellar solubilization of 1-naphthol (1-NpOH). The capacity of the solubilization by CTAB for solubilizing 1-and 2-naphthol is about eight-times higher at 4CMC than at 2CMC (four-and two-times the critical micelle concentration, respectively), which can be explained by the change in the micelle structure with an increase in the total concentration of the CTAB surfactant. For the same CMC values of the examined surfactants, SC has a higher solubilization capacity for naphthols in comparison to the solubilization capacity of CTAB, which is explained by the existence of hydrogen bonds between the building units and solubilizates that are formed in the SC micelles. For each molar ratio of the micellar binary mixture of 1-and 2-NpOH and in both examined surfactants (except for SC solubilization with α = 0.1 and α = 0.9 at 4CMC), the interaction parameters for 1-and 2-NpOH are larger than zero, which means there is a mutual antagonistic effect of 1-and 2-naphthol on their micellar co-solubilization that is probably the consequence of the competition for the same spatial part of the hydrophobic domain of the examined micelles. The binary mixture of 1-and 2-NpOH in the micellar pseudophase possesses a higher Gibbs free energy content and is thermodynamically less stable than the monocomponent solubilizates in SC and CTAB micelles.

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“…Surfactants allow the mixing of hydrophilic molecules with hydrophobic ones, through the formation of structures called micelles which allow the association of both types of molecules in a single phase. This compatibility between molecules that do not have a natural affinity is also known as co-solubilisation (Poša et al 2019 ) and can be used to establish different applications.…”

Section: Introductionmentioning

confidence: 99%

Surfactants: physicochemical interactions with biological macromolecules

et al. 2021

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Macromolecules are essential cellular components in biological systems responsible for performing a large number of functions that are necessary for growth and perseverance of living organisms. Proteins, lipids and carbohydrates are three major classes of biological macromolecules. To predict the structure, function, and behaviour of any cluster of macromolecules, it is necessary to understand the interaction between them and other components through basic principles of chemistry and physics. An important number of macromolecules are present in mixtures with surfactants, where a combination of hydrophobic and electrostatic interactions is responsible for the specific properties of any solution. It has been demonstrated that surfactants can help the formation of helices in some proteins thereby promoting protein structure formation. On the other hand, there is extensive research towards the use of surfactants to solubilize drugs and pharmaceuticals; therefore, it is evident that the interaction between surfactants with macromolecules is important for many applications which includes environmental processes and the pharmaceutical industry. In this review, we describe the properties of different types of surfactants that are relevant for their physicochemical interactions with biological macromolecules, from macromolecules–surfactant complexes to hydrophobic and electrostatic interactions.

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Co-solubilisation of a binary mixture of isoflavones in a water micellar solution of sodium cholate or cetyltrimethylammonium bromide: Influence of micelle structure

Cited by 9 publications

References 36 publications

Binary Mixed Micelles of Hexadecyltrimethylammonium Bromide–Sodium Deoxycholate and Dodecyltrimethylammonium Bromide–Sodium Deoxycholate: Thermodynamic Stabilization and Mixed Micelle Solubilization Capacity of Daidzein (Isoflavonoid)

Binary Mixed Micelles of Hexadecyltrimethylammonium Bromide–Sodium Deoxycholate and Dodecyltrimethylammonium Bromide–Sodium Deoxycholate: Thermodynamic Stabilization and Mixed Micelle Solubilization Capacity of Daidzein (Isoflavonoid)

Co-Solubilization of the Binary Mixture of 1-Naphthol and 2-Naphthol in the Water Micellar Solution of Sodium Cholate and Cetyltrimethylammonium Bromide

Surfactants: physicochemical interactions with biological macromolecules

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