Influence of the alkyl chain length, temperature, and added salt on the thermodynamics of micellization: Alkyltrimethylammonium chlorides in NaCl aqueous solutions

Kroflič, Ana; Šarac, Bojan; Bešter‐Rogač, Marija

doi:10.1016/j.jct.2011.05.015

Cited by 36 publications

(43 citation statements)

References 25 publications

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“…displays the change of ln (χ cmc /χ * cmc ) vs. (1-T * /T+lnT * /T)•1/(2-β)R for the first CMC and ln (χ tmc /χ * tmc ) vs.(1-T t * /T+lnT t * /T)•1/(2-β t )Rfor the TMC. This plot provides heat capacity values from the slopes, resulting ∆C 0 p,m = -547.39 J•K -1 •mol -1 and ∆C 0 p,t = 554.29 J•K -1•mol -1 .The heat capacity for the micelle formation shows a negative value similar to those reported for the micellization of ionic surfactants[39]Such a negative value can be explained by the removal of hydrocarbon chains from water.…”

supporting

confidence: 59%

Thermodynamic analysis of unimer-micelle and sphere-to-rod micellar transitions of aqueous solutions of sodium dodecylbenzenesulfonate

Valente

Cascales

Romero

2014

The Journal of Chemical Thermodynamics

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supporting

confidence: 59%

Thermodynamic analysis of unimer-micelle and sphere-to-rod micellar transitions of aqueous solutions of sodium dodecylbenzenesulfonate

Valente

Cascales

Romero

2014

The Journal of Chemical Thermodynamics

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“…The existence of globular micelles at smaller surfactant concentrations (still above the CMC), as revealed by the polarizing micrographs in Figure 1 , additionally corroborates the conclusion with respect to the β parameters drawn in the present work. The comparison between alkylguanidinium cationics and their alkyltrimethylammonium homologues [ 7 , 34 , 35 , 36 ] indicates that the former form less ionized micelles. Miyake et al have explained this increased counter-ion binding by a much closer packing of the DDGC units in micelles under the action of hydrogen bonds, thereby making the surface charge density higher than that of DTAC [ 7 ].…”

Section: Resultsmentioning

confidence: 99%

Micellization Behavior of Long-Chain Substituted Alkylguanidinium Surfactants

Bouchal

Hamel

Hesemann

et al. 2016

IJMS

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Surface activity and micelle formation of alkylguanidinium chlorides containing 10, 12, 14 and 16 carbon atoms in the hydrophobic tail were studied by combining conductivity and surface tension measurements with isothermal titration calorimetry. The purity of the resulting surfactants, their temperatures of Cr→LC and LC→I transitions, as well as their propensity of forming birefringent phases, were assessed based on the results of 1H and 13C NMR, differential scanning calorimetry (DSC), and polarizing microscopy studies. Whenever possible, the resulting values of Krafft temperature (TK), critical micelle concentration (CMC), minimum surface tension above the CMC, chloride counter-ion binding to the micelle, and the standard enthalpy of micelle formation per mole of surfactant (ΔmicH°) were compared to those characterizing alkyltrimethylammonium chlorides or bromides with the same tail lengths. The value of TK ranged between 292 and 314 K and increased strongly with the increase in the chain length of the hydrophobic tail. Micellization was described as both entropy and enthalpy-driven. Based on the direct calorimetry measurements, the general trends in the CMC with the temperature, hydrophobic tail length, and NaCl addition were found to be similar to those of other types of cationic surfactants. The particularly exothermic character of micellization was ascribed to the hydrogen-binding capacity of the guanidinium head-group.

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“…46 Howev-er, it should be kept in mind, that the micellization of DTACl in that case was studied in the presence of NaCl, which also considerably affects the self-aggregation process. 47 To prove the influence of isomerism of counterions on micellization of surfactant in water without any added compound the study of micellization of [ (Figure 17) was carried out recently. 19 It was found that the temperature dependence of cmc shows a nearly U-shaped form (Figure 18 a)) but is strongly dependent on the presence and position of the -OH group in the counterion.…”

Section: Surface Active Ionic Liquidsmentioning

confidence: 99%

Ionic Liquids: Simple or Complex Electrolytes?

Bešter‐Rogač

2020

ACSi

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Ionic liquids belong to the most investigated systems in the recent years and this field is still significantly growing with an increased focus on developing ionic liquids for specific applications, along with fundamental research. In the present featured paper the similarity and differences between common, "classical" electrolytes and common surfactants and ionic liquids along with the surface-active ionic liquids are discussed in order to stress their significance and point out on their weak points. A short survey of the literature data reveals namely that ionic liquids in solutions behave like "classical" electrolytes and can be described by existing models in the range of their validity. There is still a lack of models describing well the concentrated electrolyte solutions and here ionic liquids, less limited by solubility as common electrolytes, can serve as model systems. The micellization of surface-active ionic liquids in aqueous solutions can be described in the same way as for common surfactants, but surface-active ionic liquids offer more possibilities to study specific ion and isomer effects. They are also quite promising systems to study the aggregation processes in non-aqueous solutions.

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Influence of the alkyl chain length, temperature, and added salt on the thermodynamics of micellization: Alkyltrimethylammonium chlorides in NaCl aqueous solutions

Cited by 36 publications

References 25 publications

Thermodynamic analysis of unimer-micelle and sphere-to-rod micellar transitions of aqueous solutions of sodium dodecylbenzenesulfonate

Thermodynamic analysis of unimer-micelle and sphere-to-rod micellar transitions of aqueous solutions of sodium dodecylbenzenesulfonate

Micellization Behavior of Long-Chain Substituted Alkylguanidinium Surfactants

Ionic Liquids: Simple or Complex Electrolytes?

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