Ghosh, Kallol K

Roy, Supriya

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Iri'dial~Joumal of ChemistryVol. 37B, September 1998, pp. 875 - 880Thermodynamics of micelle formation of some cationic surfactants as afunction of temperature and solventKallol K Ghosh" & Supriya RoySchool of Studies in Chemistry, Pt. Ravishankar Shukla University, Raipur 492 010, IndiaReceived 1 August 1997; revised and accepted 4 May 1998The critical micelle concentrations (CMC) of some cationic surfactants, such as dodecyl, tetradecyl,hexadecyl (cetyl) trimethyl ammonium bromide, hexadecyl pyridinium chloride, hexadecyl dimethylethylammonium bromide and benzalkonium chloride has been determined over the temperature range 308-338 Kby the electrical conductivity method. The counterion binding and thermodynamics of micellization (~Go m,f..S> ms M-I m,) have been quantitatively determined, The micellar behaviour of hexadecyltrimethylammonium bromide have also been studied in dioxane-water solutions. A comparison with micelleformation for HTAB in other binary solvents, namely DMSO, DMF, methanol, ethanol, isopropanol,acetonitrile and THF has been made and discussed.The formation of micelles is a cooperative processwhich occurs at a critical micelle concentration(CMC), characteristic of the surfactant species andvarious factors such as temperature, salt, solventand pH of the solution. The CMC can serve as ameasure of micelle stability in a given state, thethermodynamic properties of micellization can bedetermined from a study of the temperaturedependence of the CMC. In continuation of ourinterest in the kinetics of hydrolysis of hydroxamicacids in micellar environment" we decided tostudy micellar properties of some cationic sur-factants, which are very useful for kinetic studies.Extensive investigations on the thermodynamics ofmicellization of cationic and anionic surfactantshave been reported, recentll-16'but understandingeven in this important area is still fragmentary. Thevarious effective perturbants such as counterions,temperature, salt, solvents, etc. remain a matter ofcontinued research interest. The availability ofthese thermodynamic parameters at varioustemperatures can give valuable insight into theprinciples which govern the formation of micelles.S· ifi ibuti f E I \3 1419n1 icant contn tions 0 vans et a. . ,deserve special mention in this context.In the present paper we report the results of ourstudy on the temperature dependence of CMCsome cationic surfactants namely dodecy 1,tetradecyl and hexadecyl trimethyl ammoniumbromide C12H25N+ (CH3)3Br (DTAB), C14H29N+(CH3)3Br (TT AB), CI6H33~(CH3)3Br (CTAB),hexadecyl pyridinium halide C16H33~ C5H5CI[CPC] , C16H33N+ C2H5Br [CPB] hexadecyldimethyl ethYli~mmonium bromide(CI6H33~(CH3)2 C2H5Br (CDEAB) and benzalkoniumchloride (C12H25~ (CH3) 3C7H7CIBC) which havebeen obtained from conductance measurement inthe 35 - 65' C temperature range at lO'C intervals.We have also analyzed in details the effect ofdioxane on the formation of micelles of CT AB inaqueous solutions. Dioxane is a rather commonorganic solvent and is often used as a medium formany organic reactions. It belongs to the generalgroup of aprotic solvents such as DMSO, DMF,THF, CH3CN. An attempt is made to studythermodynamics of micellization of CT AB in thesesolvents and protic solvents (MeOH and PrOH )for comparison.Materials and MethodsThe surfactants were products of Aldrich. Flukaand BDH and were used without furtherpurification. Surfactant solutions of a definiteconcentration were always freshly prepared byweighing out a certain amount of surfactant anddiluting it upto the required volume with doubledistilled water. Dioxane (Qualigens AR), DMSO(Qualigens AR), DMF (Glaxo AR), THF (Merck),876 INDIAN J CHEM, SEC.B, SEPTEMBER 1998acetonitrite, MeOH, PrOH (Glaxo AR) were usedas such. Conductance measurement were takenwith a Systronics digital conductometer (Type304).The CMC was determined by the conventionalconductivity method from the intersection of twolines on the plots of specific conductivity vsconcentration (Figures 1 and 2)_ From thetemperature dependence of f as well as CMC,Gibbs free energy I1Gom , and enthalpy MI m andentropy t:.S ms on micelle formation, were estimatedfor the respective surfactants .Results and DiscussionMicellization depends upon electrostaticrepulsions and hydrophobic interactions. TheTTAB. 0--0---0 3 5· C.___. zs'c~55·Co-o-o 65·C~ 1.0£•.uc0U 0.8::>-ec0Uu0.6uQ/a.Vlo.z-0--'022.0 z.o 6.0 8.0 10.0 12.0[Mxl0-3]Figure 1 - Plot of specific conductivity vs concentrationCTAB0'-0-4:l 35 •C....-1,5:C~55C1.0 D-{}{] 65·C~~..v~ 0.8v::>"c0u 0.6u'-v..a.Vl o.z 002z.o 5.0------10.03·0~.O[M x 103JFigure 2 - Plot of specific conductivity vs concentrationGHOSH et al. :TIfERMODYNAMICS OF MICELLE FORMA nON OF CA nONlC SURF ACTANTS 877importance of one of the two factors can beobtained from the studies of the thermodynamicproperties of the micellization in whichsurfactant's alkyl chains, head groups, counter ionsand the medium all play vital roles.Specific conductivities against concentrationsare plotted for various temperatures, from whichthe CMC values are determined. The choice ofCMC is never unambiguous, since the change inslope occurs, over a more or less narrow range ofconcentrations. It is obvious that CMC and henceCMC - derived parameters should depend on themethodology adopted. The results are presented inTable I. The effect of temperature on CMC iscomplex. Numerous changes in CMC withtemperature for ionic surfactants are known 5-16.Very few of these take place above 100°Chowever, the studies of the effects of temperatureon micellization have mostly been limited to lowertemperatures. The CMC of ionic surfactantsgenerally passes through a minimum at Tm withincreasing temperature. In many cases thedependence is highly irregular. The nature of thiseffect is hard to predict because it depends on aseries of factors, such as degree of counterionbinding to micelle, molecular charge, restructuringof water and the interaction between water and thesurfactant. Our observation can be explained interms of the two interactions responsible for themicellization, i.e.. , hydrophobic interactions andbreak-up of the water structure with increasingtemperature, the unique ordered structure of waterdiminishes and water becomes a more normal polarfluid. At lower temperature, the effect is exactlythe contrary. The net result is a balancing of thetwo effects in the temperature range studied. Foreach system CMC decreases as temperatureincreases. The length of the hydrocarbon chain in asurfactant has been shown to be a major factor inguiding the CMC. In a homologous series, theCMC normally decreases logarithmically with thenumber of carbon atoms. It is observed (Table I)that as the chain length of the alkyl group of thesurfactant increases (dodecyl to hexadecyl), theCMC decreases. Rakshit et al.17studied thermo-dynamics of micellization of some new pyrimidi-nium cationic surfactants. For each system CMCdecreased with the increase in temperature.Ionic micelles bind a considerable amount ofcounterions, which can be estimated byelectrochemical measurements. Following theprocedure of Evans18 the counterion associationU), properties of surfactants have been evaluatedfrom the ratio of the postmicellar and premicellarslopes obtained from the plots of specificconductance of the surfa~tant solution at differentconcentrations. The results are presented in TableI. Lengthening of the alkyl chain initially hindersmicelle formation, but longer chains are markedlyeffective in lowering the CMC and increasing theaggregation number, owing to enhancedhydrophobic interaction between the counterionand micellar core. Counterion binding, increaseswith increasing alkyl chain length.Thermodynamics of micellizationThermodynamic quantities of micellization likethe Gibbs free energy !1G om, the enthalpy MI m andthe entropy MOm, can be derived from thetemperature dependence of CMC. The standardfree energy of micellization per mole of monomerunit (!1Gom) of surfactants is related to the CMC bythe relations as shown in Eqn. (1)!1Gom=(l +f) RTln CMC ... (1)Table I--Critical micelle concentration and degree of counterion binding as a function of temperatureSurfactants CMC(mM)308K 318 K 328 K 338 Kf% f% f% f% f% f% f% f%DTAB 11.9 65.0 10.8 67.8 10.2 67.8 9.40 78.4TIAB 4.10 60.0 4.00 75.0 3.80 75.0 3.74 81.8CTAB 1.30 70.0 1.20 70.0 1.10 71.0 1.00 72.0CTACI 2.00 71.4 1.80 7104 1.40 71.4 1.00 71.4CDEAB 1.75 71.4 1.70 81.2 1.60 81.2 1.48 84.6CPC 1.00 60.0 0.80 69.2 0.75 74.2 0.60 74.2CPB 1.74 63.0 1.40 70.0 1.35 70.0 1.20 70.0BC 2.00 96.0 2.10 96.0 0.90 96.0 . 0.80 96.0878 INDIAN J CHEM, SEC.B, SEPTEMBER 1998Using the CMC and the 'f' values presented inTable I, the sc; values for the studied surfactantsystems have been computed and listed in TableIV.For. a complete thermodynamic understanding, theenthalpy of micellization (M!m) has also beenevaluated from the Vant Haff equation. (Eq. 2).M!m=R'P (d In (CMC)/dt) ... (2)In CMC was plotted against T and the slope isequal to d (In (CMC)/dn. The standard entropy ofmicellization can then be calculated from Eqn. (3)... . «3)All the thermodynamic parameters are given inTable IV. The formation of the different micelle isenergetically comparable. As expected, all themicellization processes end up with a considerablepositive entropy change. The su'; < T MOm resultsmanifest the micellization process to be entropycontrolled. At 308K, the entropy increase followsthe order CTACl> CPB> CPC> BC> CTAB>CDEAB> TTAB> DTAB. The tormation ofmicelles is connected with a large, negative changein sc; i.e. the aggregation process is thermo-dynamically favoured and spontaneous.Table IV shows that the enthalpies ofmicellization depend on the temperature. It is clearthat at higher temperatures whole of the systembecomes relatively more endothermic. Reports ofthe other workers also support this.The entropy of micellization is very high, thistype of entropy change is generally associated withphase change and one can assume micelles are anew phase. The positive entropy of micellizationalso indicates overall randomness in the systemsdue to release of structured water moleculesaround hydrocarbon chains. These values can alsodemonstrate the importance of hydrophobicinteractions. It is assumed that the aggregationnumber and counterion binding of the micelle arenot affected by temperature variation.Effect of counterionsThe counterions are also important for thethermodynamics of micellization. The enthalpy ofmicellization is strongly dependent on the size ofthe halide counterion. Enthalpies of micellizationare more endothermic for cationic surfactants withsmaller counterions (CTAB-CTACI : CPB-CPC).This indicates that the influence of counterion issignificant. According to Maa et. al.19, counterionsare unimportant for the thermodynamics ofmicellization.The data in Table IV also show that I!J.Gomdecreases with increasing chain length of thehydrophobic moiety (DTAB, TTAB and CTAB).This increase per CH2 group is expected due tohydrophobic Gibbs energies of transfer 20. Thechange of the aggregation number with counterionshould also be taken into account, unfortunatelythe aggregation numbers have not beendetermined .Solvent effectIt is well known that micellar properties of bothcationic and anionic surfactants are significantlyinfluenced by solvents 21-26. The physicochemicalproperties of solvents, dielectric constant,hydrogen bonding ability, polarity, and cohesive-ness parameters all play vital roles.Effects of dioxaneHerein we report the thermodynamics ofmicellization of CTAB in binary combination ofwater dioxane through the measurement of criticalmicelle concentrations employing the methods ofconductance. The results are presented in Table II.For the binary mixture of dioxane and water, theCMC values first increase upto 10% and thendecrease continuously. The features of thevariation of CMC on the solvent compositions cannot be accounted for mainly due to polarity effect.The CMC values increase as a function oftemperature. Our observation can be explained interms of the two interactions responsible for themicellization i.e. hydrophobic interactions andbreak-up of the water structure. On one hand thehigher temperatures, enhance the disruption of thewater structure, which on the other hand, diminishhydrophobic interactions.In case of CTAB, dioxane water ternarysystems, I!J.Gom value decreases with the increase ofconcentration of dioxane, and for this system ismore negative than the value determined for theformation of CTAB micelle in pure water (TableV). The enthalpy of micellization M!m is moreendothermic with respect to an increase in theconcentration of dioxane. The entropy ofGHOSH et al. :THERMODYNAMICS OF MICELLE FORMATION OF CATIONIC SURFACTANTS 879Table II----Critical micelle concentration of CT AB in various Table III----Critical micelle concentration of CT AB in variousaquo-dioxane solution at different temperatures co-solvents solution at different temperaturesSolvents CMC(mM)% Co-solvent% 308K 318 K 328 K 338 KCMC(mM)(v/v) 308K 318 K 328K 338K0 1.30 1.20 1.10 1.00 Dioxane1.71 1.00 0.99 0.6310 2.40 2.20 1.20 0.80 DMSO1.90 1.40 1.20 1.0020 1.71 1.00 0.99 0.63 DMF 2.201.39 1.00 1.0030 1.50 1.00 0.80 0.60 THF1.90 1.20 1.00 0.8040 1.30 0.90 0.70 0.40 CH3CN 2.001.61 1.20 1.0050 1.20 0.80 0.60 0.31 MeOH1.70 1.40 1.20 0.8060 1.10 0.70 0.60 0.29PrOH 1.50 1.10 1.00 0.60% of co-solvents = 20% (v/v)Table IV-Thermodynamic quantities of micellization of surfactants at different temperaturesSurfactants [~Gom] [~Hom] [~Som]KJmo r' KJmorl JKmol308 K 318 K 328K 338 K 308K 318 K 328 K 338 K 308K 318 K 328 K 338DTAB 18.7 20.0 20.9 23.4 6.03 6.43 6.84 7.26 80.4 83.4 84.8 90.7TIAB 22.6 25.5 26.6 28.5 2.50 2.67 2.84 3.01 81.5 88.7 89.7 93.3CTAB 28.9 30.2 31.7 33.3 6.80 7.33 7.80 8.28 115.9 1I8.0 120.4 123.0CTACI 27.3 28.6 30.7 33.3 18.3 19.6 20.8 22.1 148.2 151.6 157.7 163.9CDEAB 27.8 30.5 31.8 33.8 5.13 5.40 5.82 6.18 107.1 113.2 114.6 118.2CPC 28.4 31.8 33.6 36.6 14.8 15.8 16.8 17.9 140.3 149.9 153.7 160.3CPB 26.4 29.5 32.6 34.2 9.07 9.67 10.3 ·In.9 115.2 123.3 130.6 133.4BC 27.03 28.5 27.9 31.0 7.57 8.07 8.53 9.12 91.12 . 115.0 1I7.2 118.9Table V-Thermodynamic quantities of micellization of CTAB in aquo-dioxane mixtures% Dioxane [~Gom] [~Hom] [~S°mlKJmo r' KJmorl JKmol308 K 318 K 328K 338 K 308K 318 K 328 K 338 K 308 K 318 K 328 K 3380 28.2 30.2 31.7 33.3 6.80 7.33 7.80 8.28 115.9 118.0 120.4 123.010 27.9 29.2 33.2 36.2 30.8 32.8 34.9 37.1 190.0 195.8 207.1 216.620 29.6 33.2 34.3 37.6 23.7 25.2 36.8 28.5 173.3 183.9 186.9 286.530 30.5 32.9 35.6 38.1 24.1 25.7 27.4 29.1 171.6 184.4 192.2 199.140 31.6 34.5 36.8 40.8 29.8 31.8 23.8 35.9 199.6 208.5 115.5 221.350 32.5 36.6 38.2 42.9 34.2 36.4 38.8 41.2 216.8 229.4 135.5 249.160 33.1 36.5 38.4 43.4 35.7 37.5 39.8 42.5 223.2 235.2 136.6 254.3micellization ss; gradually Increases. Thisimplies that the positive free energy ofmicellization is principally that results of theentropy of terms of water CT AB-dioxane. Thisconclusion is in agreement with the generalconcept that micelle formation in aqueous solutionis an entropy directed process and arises mainlyfrom the break-up of the ordered water structure,even though the formation of aggregate by thesurfactant molecules is entropy decreasing process.Effect of co-solventThe comparison with micelle formation forCTAB in other aquo-solutions including co-solvents such as DMSO, DMF,THF, acetonitrile,methanol, n-propanal has been made (Table III).The effect of micellization of hexadecyltrimethylammonium bromide in different co-solvents(Table Illjindicate that alcoholic solvents enhancethe micelle formation while other retard it. Thisphenomena is due to hydrogen bounding andstructure of water molecule with increase intemperature. The H-bonding of -OH groupsolvents is distructed, whereas in other solvents itis not possible.Thermodynamic parameters, such as IlGom,MI rns MOm in different solvents were alsodetermined. The experimental results indicate thatmicelle formation comparatively decreases withthe rise in temperature, and solvents have880 INDIAN J CHEM, SEC.B, SEPTEMBER 1998Table VI-Thermodynamic quantities ofmicellization ofCTAB in different aquo-co-solvents mixturesSolvent [LlG°ml [LlHom] [LlS°ml(20%) KJmo r' KJmorl JKrnol308K 318 K 328K 338K 308K 318 K 328K 338 K 308K 318K 328K 338Dioxane 29.68 33.23 34.32 37.67 23.70 25.26 26.88 28.59 173.31 183.92 186.58 195.80DMSO 28.64 30.96 32.70 34.92 18.05 19.24 20.47 21.74 151.50 157.8 162.10 167.60DMF 27.25 30.18 32.74 34.83 27.04 28.82 30.67 32.57 176.20 182.50 193.30 199.40THF 29.06 32.20 34.11 36.24 21.90 23.34 24.83 26.37 165.40 174.6 179.60 185.20Methanol 29.70 31.59 33.37 36.40 19.02 20.28 21.59 22.91 158.10 163.1 167.50 175.40Acetonitrile 30.00 32.40 34.82 37.58 18.66 19.90 21.17 22.48 157.90 164.4 170.70 177.60Propanol 2-01 30.80 34.38 36.09 39.80 22.43 23.91 25.43 27.01 172.8 183.9 187.50 197.60enhancing effect on the formation of micelles of 10CT AB. This effect increases with increasingdioxane concentration. The effect of micellizationand the observed changes in I1Gom, MI rns and MOm 11can be explained in terms of interaction, such ashydrogen bonding between water and solvents 12resulting in the increase Of hydrophobic forces inthe ternary system (Table VI) :!Financial supports from the M P Council ofScience and Technology ( Bhopal, M P) and Pt.Ravishankar Shukla University, Raipur aregratefully acknowledged.References1 Ghosh K K & Roy S, Bull Chem Soc Jpn, 69, 19963417.2 Ghosh K K & Roy S, J Surface Science and Technology,10, 1996,41.3 Ghosh K K & Sar S K, Indian J Chem, 33A, 1994, 51.4 Ghosh K K & Sar S K, J Indian Chem Soc, 72, 1995,597.5 Bijma K, Engberts J B F N, Haandrikman G, Van Os NM, Blandamer M J, Butt M D & Collis P M. 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Thermodynamics of micelle formation of some cationic surfactants as a function of temperature and solvent

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Thermodynamics of micelle formation of some cationic surfactants as a function of temperature and solvent

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