Thermodynamic properties of N-octyl-, N-decyl- and N-dodecylpyridinium chlorides in water

Causi, S.; Lisi, R. De; Milioto, Stefana

doi:10.1007/bf00649096

Cited by 29 publications

(29 citation statements)

References 29 publications

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“…Causi et al (16) and Fisicaro et al (18) report D dil H m at T = 298.15 K for C10PC and C12PC to values of m larger than those of this investigation. Both investigations also report D dil H m for C8PC at T = 298.15 K. We have fit D dil H m from these investigations with our equations (1) to (8) (2) to (7) for fitting 1-n-alkanepyridinium chloride apparent molar heat capacities Cp,f from the literature (16) with an equation analogous to equation (8); (2) that values of D r H°m/n are not generally affected greatly by the choice of molality range and parameters to fit these data with equation (8).…”

Section: Resultsmentioning

confidence: 65%

“…Values of f are also reported in the literature for C10PC, (16) C12PC, (8,16) and C16PC. (8) Values of practical osmotic coefficients were given in graphical form by Huff et al (8) We have digitized their results and converted them to rational osmotic coefficients f. Causi et al (16) also reported values of f for aqueous 1-n-octanepyridinium chloride, C 5 H 5 N(Cl)CH 2 (CH 2 ) 6 CH 3 , denoted by C8PC. Furthermore, Maeda and Satake (17) reported ion-selective electrode measurements on aqueous C12PC, from which we have derived mean ionic activity coefficients.…”

Section: Resultsmentioning

confidence: 85%

“…However, it is useful to inspect plots of conventional thermodynamic quantities for reaction (1) measured D dil H m , and the error bars on these symbols are our estimated total uncertainties based on the values given in table 6. Also shown in figures 8 to 12 are quantities from tables 8 and 9 for our fitting of data from the literature (16,18) for these surfactants.…”

Section: Resultsmentioning

confidence: 99%

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Thermodynamic properties of aqueous 1-n-alkanepyridinium chlorides at temperatures from 283.15 K to 343.15 K

McGinnis

Woolley

1997

The Journal of Chemical Thermodynamics

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Section: Resultsmentioning

confidence: 65%

Section: Resultsmentioning

confidence: 85%

Section: Resultsmentioning

confidence: 99%

See 1 more Smart Citation

Thermodynamic properties of aqueous 1-n-alkanepyridinium chlorides at temperatures from 283.15 K to 343.15 K

McGinnis

Woolley

1997

The Journal of Chemical Thermodynamics

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“…In the pre-micellar region, the partial molar properties Y2 have been calculated by means of Eqs (4) and (7) In the post-micellar region, Y2 values were calculated by drawing the best curve for the corresponding apparent molar quantities as functions of molality and interpolating points at regular intervals [2,3].…”

Section: Resultsmentioning

confidence: 99%

“…Recently, we have focussed on the interpretation of the effect of the nature of the head group on the profile of the bulk thermodynamic properties vs. concentration. Interesting information has been obtained by comparing these properties for alkyltrimethylammonium [1,2], N-alkylpyridinium, [3] N-alkyl-N-methylpiperidinium [4] and N-alkylpiperidinium [4] chlorides. As a consequence of these results, we decided to study octylalkyldimethylammonium chlorides where the alkyl chain ranges between methyl…”

Section: Introductionmentioning

confidence: 99%

Thermodynamic studies of octyltrimethylammonium chloride in water

Milioto

Causi

Crisantino

et al. 1992

Journal of Thermal Analysis

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Densities, heat capacities, enthalpies of dilution at 298 K and osmotic coefficients at 310 K of octyltrimethylammonium chloride were measured as functions of concentration. From the experimental data, the partial molar volumes, heat capacities, relative enthalpies, nonideal free energies and entropies at 298 K were derived as functions of concentration. A comparison between the above data and those of dodecyltrimethylammonium chloride reported in the literature shows that the increase of the alkyl chain length shifts the apparent molar volume vs. concentration curves towards greater values and the heat capacity, relative enthalpy and free energy vs. concentration curves towards smaller values. By assuming the pseudo-phase transition model the properties of micellization (AYm) were graphically evaluated. The AYm values of OTAC compared with those of DTAC are consistent with the increase of the hydrophobicity by increasing the alkyl chain length.

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Proton NMR Studies on the Structure of Water at Interfaces of Aqueous Micelles. Part 4: Effects of Cationic and Zwitterionic Headgroups

Seoud¹,

Blaskó

Bunton

1995

Ber Bunsenges Phys Chem

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Fr.actionation factors, rpM' of interfacial water at surfaces of cationic and zwitterionic surfactants were determined from the dependence of the 1H chemical shift of water on the isotopic composition of the solvent (H°p lus O 2°) .~alue~of rpM are greater than unity, showing that interfacial water is more structured than bulk water who.se fractionation factor = 1, by defin.itio.n. The structuring increases with increasing bulk of the headgroup: but IS unaffected by the length of the catiomc surfactant hydrophobic tail. The effect of zwitterionic sulfobetaine s~r~actants on the structure of their water of hydration is less than that of cationic surfactants that have otherwise slm.ll~r .headgrou~s. Values of rpM for cationic micelles are: cetyldimethylphenylammonium chloride, 1.08; cetylp~ndln1Um chlonde, 1.06; and dodecyltrimethylammonium bromide, 1.06. Values of QlM for sulfobetaine micelles are: 3-N-tetradecyl-N,N-di-n-butylammonio-I-propane sulfonate, 1.07, and 3-N-tetradecyl-N,N-diethylammonio-I-propane sulfonate, 1.03.7]. These methods often involve hydrophobic solutes whose (average) solubilization site in the micellar pseudophase is a matter of discussion, and they may perturb aggregate structure [8, 9]. In the present work, we examine effects of the nature of surfactant headgroups on the structure of interfacial water by measuring the deuterium solvent isotope effect on the 1H chemical shift of the solvent (H 20 plus D 20). Isotopic substitution in the solvent involves minimum perturbation of the micellar system. The resulting secondary isotope effect is, however, small, but 1H NMR spectroscopy is a very sensitive technique and is, therefore, suitable for measurement of such small effects [10][11][12][13][14][15][16].It is convenient to describe isotope effects in terms of fractionation factors, rp, defined for a micelle, M, as:That is, for a micelle in H 20-D20, the fractionation factor for interfacial water, rpM, describes the isotopic composition at the aggregate/water interface relative to that in bulk solvent [14][15][16].We are interested in exploiting the value of rpM to probe effects of the charge and nature of headgroups on the degree of structure of interfacial water. To date, effects of micelles of various ionic, zwitterionic and nonionic surfactants have been examined [14][15][16]. In the present work we examine effects due to aromatic or bulky alkyl headgroups in cationic and zwitterionic sulfobetaine micelles, as well as variation in the length of the surfactant hydrophobic tail.Earlier results showed that hydrophobic headgroups (phenyl or n-butyl) enhance the structure of interfacial water; electrostriction by the charged interface and hydrophobic hydration of the bulky group being the main factors.

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Thermodynamic properties of N-octyl-, N-decyl- and N-dodecylpyridinium chlorides in water

Cited by 29 publications

References 29 publications

Thermodynamic properties of aqueous 1-n-alkanepyridinium chlorides at temperatures from 283.15 K to 343.15 K

Thermodynamic properties of aqueous 1-n-alkanepyridinium chlorides at temperatures from 283.15 K to 343.15 K

Thermodynamic studies of octyltrimethylammonium chloride in water

Proton NMR Studies on the Structure of Water at Interfaces of Aqueous Micelles. Part 4: Effects of Cationic and Zwitterionic Headgroups

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