Thermometric titration studies of the effect of head group, chain length, solvent, and temperature on the thermodynamics of Micelle formation

Kresheck, Gordon C.; Hargraves, Walter A.

doi:10.1016/0021-9797(74)90193-3

Cited by 147 publications

(107 citation statements)

References 44 publications

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“…Experiments on micellization show that is generally a linear function of temperature and that therefore ∆CP,mczn is constant. [26][27][28][29] Hence, these observations appear to be inconsistent with the theoretical predictions. However, the real situation is like the one shown in Figure 4, which is prepared based on the CMC data of the cationic surfactant OTAC.…”

Section: T (K)contrasting

confidence: 53%

Thermal Behavior of Critical Micelle Concentration from the Standpoint of Flory-Huggins Model

Lim

2009

Bulletin of the Korean Chemical Society

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Temperature dependence of the critical micelle concentration (CMC), x CMC, in micellization can be described by ln x CMC = A + BT + C lnT + D/T, which has been derived statistical-mechanically. Here A, B, C, and D are fitting parameters. The equation fits the CMC data better than conventionally used polynomial equations of temperature. Moreover, it yields the unique(exponent) value of 2 when the CMC is expressed in a power-law form. This finding is quite significant, because it may point to the universality of the thermal behavior of CMC. Hence, in this article, the nature of the equation ln x CMC = A + BT + C lnT + D/T is examined from a lattice-theory point of view through the Flory-Huggins model. It is found that a linear behavior of heat capacity change of micellization is responsible for the CMC equation of temperature.

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Section: T (K)contrasting

confidence: 53%

Thermal Behavior of Critical Micelle Concentration from the Standpoint of Flory-Huggins Model

Lim

2009

Bulletin of the Korean Chemical Society

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“…Furthermore, the entropy decreases with increasing temperature. These findings lead to a Gibbs energy which is either hardly or only slightly temperature dependent due to the enthalpy-entropy compensation (9)(10)(11).…”

Section: Methodsmentioning

confidence: 99%

A Titration Microcalorimetric Study of the Effects of Halide Counterions on Vesicle-Forming Aggregation in Aqueous Solution of Branched-Chain Alkylpyridinium Surfactants

Gooijer

Engberts

Blandamer

2000

Journal of Colloid and Interface Science

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Take-down policy If you believe that this document breaches copyright please contact us providing details, and we will remove access to the work immediately and investigate your claim.Downloaded from the University of Groningen/UMCG research database (Pure): http://www.rug.nl/research/portal. For technical reasons the number of authors shown on this cover page is limited to 10 maximum. Titration microcalorimetry is used to study the influences of iodide, bromide, and chloride counterions on the aggregation of vesicle-forming 1-methyl-4-(2-pentylheptyl)pyridinium halide surfactants. Formation of vesicles by these surfactants was characterised using transmission electron microscopy. When the counterion is changed at 303 K through the series iodide, bromide, to chloride, the critical vesicular concentration (cvc) increases and the enthalpy of vesicle formation changes from exo-to endothermic. With increase in temperature to 333 K, vesicle formation becomes strongly exothermic. Increasing the temperature leads to a decrease in enthalpy and entropy of vesicle formation for all three surfactants. However the standard Gibbs energy for vesicle formation is, perhaps surprisingly, largely unaffected by an increase in temperature, as a consequence of a compensating change in both standard entropy and standard enthalpy of vesicle formation. Interestingly, standard isobaric heat capacities of vesicle formation are negative, large in magnitude but not strikingly dependent on the counterion. We conclude that the driving force for vesicle formation can be understood in terms of overlap of the thermally labile hydrophobic hydration shells of the alkyl chains.

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“…u-szeged.hu. who utilized titration calorimetry in the temperature range from 293 to 308 K (6). They found the cmc of SDeS at 298 K to be 24.5 mM, in contrast with the 33.1 mM obtained from conductometry (2)(3)(4) at the same temperature.…”

Section: Introductionmentioning

confidence: 96%

A Thermometric Titration Study on the Micelle Formation of Sodium Decyl Sulfate in Water

Király

Dékány

2001

Journal of Colloid and Interface Science

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Thermometric titration studies of the effect of head group, chain length, solvent, and temperature on the thermodynamics of Micelle formation

Cited by 147 publications

References 44 publications

Thermal Behavior of Critical Micelle Concentration from the Standpoint of Flory-Huggins Model

Thermal Behavior of Critical Micelle Concentration from the Standpoint of Flory-Huggins Model

A Titration Microcalorimetric Study of the Effects of Halide Counterions on Vesicle-Forming Aggregation in Aqueous Solution of Branched-Chain Alkylpyridinium Surfactants

A Thermometric Titration Study on the Micelle Formation of Sodium Decyl Sulfate in Water

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