Kinetic Treatment of the Reaction of Fructose and N-Bromosuccinimide in Cationic/Anionic/Nonionic Micelles
The kinetics of oxidation of fructose by N-bromosuccinimide in acidic medium in the absence and presence of cationic, anionic, and nonionic surfactants has been measured iodometrically under pseudo-first-order condition. The oxidation kinetics of fructose by N-bromosuccinimide shows a first-order dependence on N-bromosuccinimide, fractional order dependence on fructose, and negative fractional order dependence on sulfuric acid. The kinetics is treated using Berezin’s micellar model that was previously used for the catalysis and inhibition of the reaction. The determined stoichiometric ratio was 1 : 1 (fructose : N-bromosuccinimide). The variation of Hg(OAC)2 and succinimide (reaction product) has insignificant effect on reaction rate. Effects of surfactants, added acrylonitrile, added salts, and solvent composition variation have been studied. Activation parameters for the reaction have been evaluated from Arrhenius plot by studying the reaction at different temperatures. The rate law has been derived on the basis of obtained data. A plausible mechanism has been proposed from the results of kinetic studies, reaction stoichiometry, and product analysis.
It is well known that aqueous charged interphases play an important role in the enhancement of the rate of chemical reactions [1–5]. Micelles act as microreactors which both speed and inhibit the rates of a wide variety of uni- and bimolecular reactions and shift the equilibrium constants of many indicators [6–15]. Aggregate effects on chemical reactivity are generally interpreted by using pseudophase models which treat micelles and water as separate reaction media, that is, separate phases or pseudophases. This approach has been successfully applied to a wide range of chemical reactions in micellar solution, including mixed micelle, and in other types of association colloids, such as microemulsions and vesicle. Surfactant aggregates affect chemical reactivity primarily by binding or excluding reactants and only secondarily by changing the free energy of activation [16–19].
Considerable attention has centred on N-bromosuccinimide (NBS) because of its versatile behaviour as mild oxidant, halogenating agent, and N-anions, which acts both as bases and nucleophiles. NBS is well-known analytical reagent, and the mechanistic aspects of its reactions have been documented [20–25]. As a part of our mechanistic studies of oxidation of substrate by the NBS, I report the kinetics of oxidation of D-fructose by NBS in the micellar region.
Fructose, or fruit sugar, is a simple monosaccharide found in many foods. It is one of the three important dietary monosaccharides along with glucose and galactose. Honey, tree fruits, berries, melons, and some root vegetables contain significant amounts of molecular fructose, usually in combination with glucose, stored in the form of sucrose. Fructose undergoes the Maillard reaction, nonenzymatic browning, with amino acids. Fructose readily dehydrates to give hydroxymethylfurfural (“HMF”). This process may in the future be part of a low-cost, carbon-neutral system to produce replacements for petrol and diesel from plantations. Fructose is an excellent humectant and retains moisture for a long period of time even at low relative humidity (RH). Therefore, fructose can contribute to improved quality, better texture, and longer shelf life to the food products in which it is used.
D-Fructose, cetyltrimethylammonium bromide (CTAB), sodium dodecyl sulfate (SDS), TritonX-100 (TX-100), succinimide (NHS), potassium iodide (KI) (all AR, s. d. fine), mercuric acetate (Hg(OAc)2, GR, loba chemie), and sodium thiosulfate (Na2S2O3·2H2O, AR, Qualigens ExcelaR, Qualigens fine chemicals) used were of highest purity available commercially. Solutions were prepared in double distilled water. To maintain hydrogen ion concentration constant, sulfuric acid (H2SO4, AR, s. d. fine) was used. Distilled glacial acetic acid (AR, s. d. fine) was used as solvent. NBS (Aldrich, Germany) solution was standardized iodometrically and stored in an amber coloured bottle to avoid any photochemical deterioration .
2.2. Kinetic Measurements
All the kinetic measurements were carried out in an amber coloured vessel at 313 K and performed under pseudo-first-order condition with [D-fructose]≫[NBS]. The required solutions of all the reactants (except oxidant) were taken in an amber coloured reaction vessel to avoid photochemical deterioration . The reaction vessel was kept in the thermostated water bath at fixed temperature and the solution was left to stand for 30 min to attain equilibrium. The reaction was initiated by the rapid addition of known amounts of D-fructose to a reaction mixture containing the required amount of the NBS, H2SO4, mercuric acetate, acetic acid, and water in glass-stoppered Pyrex boiling tubes and thermostated at 313 K. The reaction was initiated with the addition of required volume of thermally equilibrated oxidant solution. The zero time was taken when NBS solution has been added. The progress of the reaction was followed by iodometric estimation of unconsumed NBS by pipetting out aliquots at different time intervals. The kinetics was monitored for 80% completion of the reaction. The results are reproducible to within ±2.5% with average linear regression coefficient.
2.3. Product Analysis and Stoichiometry
Different ratios of NBS to D-fructose were equilibrated at 313 K in the presence of a requisite amount of all reactants, that is, sulfuric acid, mercuric acetate, and acetic acid, under the condition of [NBS] ≫ [D-fructose] for 72 h (when [NBS] = mol , then [fructose] = mol and when [NBS] = mol , then [fructose] = mol dm−3). Estimation of residual [NBS] in each set showed that 1 mol of fructose consumed 1 mol of NBS. Accordingly, the stoichiometric equation was formulated in the following equation.
Product of Fructose Oxidation. Consider After the kinetic experiment was completed, a part of the oxidized reaction mixture was treated with alkaline hydroxylamine solution, and the presence of lactone in the reaction mixture was tested by FeCl3-HCl blue test [27, 28]. To the other part of the reaction mixture, barium carbonate was added to make the solution neutral . FeCl3 solution that had been coloured violet with phenol when added to this reaction mixture gave bright-yellow colouration , indicating the presence of aldonic acid. It is concluded that lactone, formed in the rate-determining step, is hydrolyzed to aldonic acid in neutral medium in a fast step. At higher pH, [lactone] is reduced because of the formation of aldonic acid anion that shifts the equilibrium away from lactone.
2.4. Determination of CMC Values
The role of micellar catalysis may not be understood without its critical micelle concentration. This is the concentration where surfactant will work as micelle. Therefore, it is very interesting as well as important to know this factor very correctly and accurately. The critical micelle concentration (CMC) values of surfactants (CTAB, SDS, TX-100) in the presence and absence of substrate and oxidants (Table 1) were determined from plots of the specific conductivity () versus surfactant concentration using conductometric determination method and carried out with a digital conductivity meter, model 611E, at 40°C. The values of CMC of surfactants are sensitive to the nature of the reactants and also depend upon reaction conditions. The break point of nearly two straight-line portions in the plot is taken as an indication of micelle formation, and this corresponds to the CMC of surfactant.
3. Results and Discussion
Kinetics due to molecular bromine intervention was removed by the addition of mercury (II) ions, which removed Br− ions either as HgBr2 or as . Here, mercuric acetate was added as a scavenger. Preliminary observations showed that the solution of CTAB became turbid in presence of HClO4. Turbidity increases with [HClO4] at constant [CTAB]. Therefore, H2SO4 was used to maintain the acidic strength constant.
3.1. Dependence on [Fructose]
The effect of varying the concentrations of fructose on rate in aqueous and micellar media showed that the reaction order is fractional. Further, a plot of versus was linear with a slope less than unity (Figure 1). The results are summarized in Table 2.
3.2. Dependence on [NBS]
The reaction is of first order in [NBS] in the absence and presence of surfactant as indicated by the linearity of a plot of log [NBS] versus time (Figure 2). This was further confirmed by the fact that the first-order rate constant is invariant with different initial concentrations of NBS (Table 2).
3.3. Dependence on [H2SO4]
The rate constant decreased with increasing [H2SO4]. A plot of versus log [H2SO4] was linear with a slope that is negative (Figure 4) and less than unity indicating a negative fractional order dependence on the rate on [H2SO4]. The results are summarized in Table 2.
3.4. Dependence on Solvent
The rate constant decreased with increasing acetic acid content (20–50% [v/v]). The results are summarized in Table 2. A plot of log versus 1/ was linear with a negative slope  (Figure 3, (2)). Blank experiments performed showed that the oxidation of acetic acid by NBS during the period of study was negligible. Consider where is the rate constant in a medium of infinite dielectric constant, and are the charges of reacting ions, refers to the size of activated complex, is absolute temperature, and is the dielectric constant of the medium.
3.5. Dependence on [Hg(OAc)2]
Mercuric acetate was added to the reaction mixture as scavenger to eliminate Br− formed in the reaction, which could have produced Br2 in the reaction. The formed Br2, thus, might cause another parallel oxidation. Hg(OAc)2, thus, ensures the oxidation purely through NBS.
3.6. Dependence on [Succinimide]
The reaction rate is retarded by the addition of succinimide (NHS), which is one of the products of the reaction. This points to the existence of a preequilibrium step (3). Consider The positive bromine from NBS can be transferred to the fructose through the intermediate formation of HOBr.
3.7. Dependence on [Salt]
Added salts inhibit the micellar catalysis, which is a general phenomenon. The inhibition has been explained by assuming that the counterions compete with an ionic reactant for a site on the micelle  and cause shape change from spherical to rod-like micelles. The added salts (KCl, KBr, and ) inhibit the rate of reaction. As the concentration of these electrolytes increases, the concentration of reactants at the reaction site decreases because these are responsible for rate inhibition of micellar-mediated reactions due to the exclusion of the reagent(s) from the micellar pseudophase.
3.8. Assessment for Acrylonitrile Polymerization
Addition of acrylonitrile to the reaction mixture does not induce polymerization. Therefore, the reaction does not involve the formation of free radicals. The observations demonstrate that no free radicals are formed in the reaction mechanism.
3.9. Temperature Effect and Activation Parameters
The oxidation of fructose was studied at 30–50°C and the data are presented in Table 3. Arrhenius parameters evaluated from linear plots of versus 1/ were computed from Arrhenius and Eyring equations (Figure 5) in Table 3. The catalytic behavior of CTAB and TX-100 micelles indicates that the complex of fructose-NBS has the negative charge. The cationic head group may form an ion pair with the reactive and existing complex of fructose-NBS. As a result, a large number of fructose-NBS complexes are incorporated into the small volume of cationic micelles. But the nonionic micelles form hydrogen bond with the fructose-NBS complex. In the presence of SDS, on the other hand, there is electrostatic repulsion between the negative head group of SDS micelles and the reactive species of fructose-NBS complex. The result is that slightly inhibitory effect is possible. A higher value of in the presence of SDS shows the slightly inhibitory effect on the rate of reaction whereas a low value in the presence of CTAB and TX-100 shows the catalytic effect. The large negative value of Δin the presence of CTAB and TX-100 indicates that more ordered activated complex is formed. The fairly high positive values of Δ and Δ indicate that the transition state is highly solvated. The nearly same value of Δ in the absence and presence of surfactant indicated operation of similar reaction mechanism in both cases. Here, is energy of activation, Δ is enthalpy of activation, Δ is entropy of activation, and Δ is free entropy of activation.
The monosaccharides are considered as a unit of disaccharides and on hydrolysis disaccharides give monosaccharide units. D-sucrose hydrolyzes into two monosaccharides—glucose and fructose. The monosaccharides are considered as a polyol and the reactivities of –OH groups can be influenced by the presence of the carbonyl group. Monosaccharides exist mainly as pyranoid and furanoid forms, with the former being more stable .
On the other hand, NBS exists in the following equilibria.
Reactive Species of NBS in Aqueous Medium. Consider
Since, on assumption of NBS or as the reactive species, the rate law fails to explain the negative effect of phthalimide, hence, neither of these species, NBS and , can be taken as the reactive species. When HOBr is taken as the reactive species, the rate law explains the negative effect of and [NHS]. Thus, HOBr is taken as the most reactive species, which gave the rate law capable of explaining all the kinetic observations and other effects.
According to above experimental conditions HOBr is the most reactive species of NBS and considering the fact that one mole of D-sucrose is oxidized by two moles of NBS in Scheme 2.
In Scheme 2, stands for D-sucrose, , are the equilibrium constants for steps 1 and 2, is the rate constant, and is intermediate species. Equation (8) is in good agreement with the experimental results. The rate of disappearance of [NBS] can be expressed in (10). Equations (11) and (12) satisfactorily explain the kinetic results with respect to [NBS], [D-sucrose], [H2SO4], and [NHS]. Consider where
3.11. Effect of Varying [Surfactants]
In the case of D-sucrose, the cationic surfactant CTAB and nonionic surfactant TX-100 have been found to show the rate accelerating effect whereas the anionic surfactant SDS has been found to show the rate retarding effect. In all cases, after a certain concentration of surfactant, the rate constant attains a limiting value. In presence of the cationic surfactant CTAB, both the reactants, that is, D-sucrose (it should hydrolyse into glucose and fructose with negative charge) and NBS, are preferably partitioned in the stern layer of CTAB (a cationic surfactant), bearing the positively charged micellar head groups, and consequently the rate is accelerated (Figures 6 and 7), (Table 4). In presence of the nonionic surfactant TX-100, both the reactants, that is, D-sucrose (a hydrophilic substance) and NBS, are preferably partitioned in the stern layer of TX-100 (a nonionic surfactant), bearing not any charge on micellar head groups, and consequently the rate is accelerated. The anionic species of D-sucrose (Scheme 1) and NBS is being repelled by the negatively charged micellar head groups of SDS (an anionic surfactant) and consequently the rate is retarded (Figures 8 and 9), (Table 4). A possible arrangement (although highly schematic) could be as shown in Scheme 3, which indicates the probable reaction site to be the “Stern and Gouy-Chapman layers” junctural region.
3.12. The Kinetic Model to Explain the Micellar Effects
Micellar catalysis critically depends on the interactions of the micelle with the substrate(s) and the activated complex. This is an extremely complicated problem because a number of different interactions are involved including those associated with the head group of the surfactant, the different segments of the alkyl chain, and the counterions. In Berezin’s model, a solution above the CMC may be considered as a two-phase system, consisting of an aqueous phase and a micellar pseudophase. The reactants (S and O) may be distributed as shown in Scheme 4. A quantitative rate expression for a bimolecular reaction occurring only in aqueous ( path) and micellar ( path) phase for the pseudo-first-order rate constant is given in Scheme 4. Consider where and are the association constants of D-sucrose and NBS, respectively, with surfactants, is the analytical concentration of surfactants, = (), is the molar volume of the micelle, and and are the pseudo-first-order rate constants in absence and presence of micelles, respectively. Since the oxidant will be uncharged species and the substrate is large molecules, the hydrophobic and electrostatic interactions will be large and hence it may be expected that and will be high. Since is small it may be possible that so that (13) takes the form Again, since is very small, the terms containing may be neglected, and (14) may be rearranged to Plot of versus for D-sucrose is linear (Figures 7 and 9).
In summary, the following conclusions can be drawn. Kinetic parameters for the reaction were determined, assuming that the dominant active species of NBS is HOBr. Activation and thermodynamic parameters have been evaluated for both in absence and presence of the surfactants. The CMC values are lower than those given in the literature for aqueous solutions of surfactants without added electrolyte. The reaction was found to be first and fractional order each with respect to the oxidant and the reductant. The mechanism of the reaction involves (i) hydrolysis of D-sucrose into monosaccharide units, glucose and fructose, and (ii) oxidation of both monosaccharide units. Oxidation product is lactone of aldonic acid. The rate of oxidation increases with increasing concentration of CTAB and TX-100. The SDS shows inhibitory effect. The effect of micellization can be correlated with the nature of the reducing substrates and the reaction conditions. This is in agreement with the qualitative knowledge about the nature of D-sucrose and NBS in H2SO4 medium.
Conflict of Interests
The author declares that there is no conflict of interests regarding the publication of this paper.
The author gratefully wishes to thank the Chhattisgarh Council of Science and Technology (CGCOST) for the Research Project Grant. The author also thanks Professor Laurence S. Romsted, Department of Chemistry, Wright-Rieman Laboratories, New Jersey, USA, for valuable discussions and fruitful suggestions.
J. W. Park, M.-A. Chung, and K. M. Choi, “Properties of sodium dodecyl sulfate/Triton X-100 mixed micelle,” Bulletin of the Korean Chemical Society, vol. 10, no. 5, pp. 437–442, 1989.View at: Google Scholar
B. Samiey, K. Alizadeh, M. A. Moghaddasi, M. F. Mousavi, and N. Alizadeh, “Study of kinetics of Bromophenol blue fading in the presence of SDS, DTAB and Triton X-100 by classical model,” Bulletin of the Korean Chemical Society, vol. 25, no. 5, pp. 726–736, 2004.View at: Publisher Site | Google Scholar
H. Gharibi, B. Sohrabi, S. Javadian, and M. Hashemianzadeh, “Study of the electrostatic and steric contributions to the free energy of ionic/nonionic mixed micellization,” Colloids and Surfaces A: Physicochemical and Engineering Aspects, vol. 244, no. 1–3, pp. 187–196, 2004.View at: Publisher Site | Google Scholar
Z. Zhi-Guo and Y. Hong, “Interaction of nonionic surfactant AEO9 with ionic surfactants,” Journal of Zhejiang University: Science B, vol. 6, no. 6, pp. 597–601, 2005.View at: Google Scholar
G. Briganti, S. Puvvada, and D. Blankschtein, “Effect of urea on micellar properties of aqueous solutions of nonionic surfactants,” Journal of Physical Chemistry, vol. 95, no. 22, pp. 8989–8995, 1991.View at: Google Scholar
H. H. Paradies, The Journal of Physical Chemistry A, vol. 84, p. 599, 1980.
S. K. Mehta, A. K. Malik, U. Gupta, and A. L. J. Rao, Electronic Journal of Environmental, Agricultural and Food Chemistry, vol. 3, no. 6, p. 784, 2004.
A. B. Mandal, D. V. Ramesh, and S. C. Dhar, “Physico-chemical studies of micelle formation on sepia cartilage collagen solutions in acetate buffer and its interaction with ionic and nonionic micelles. Hydrodynamic and thermodynamic studies,” European Journal of Biochemistry, vol. 169, no. 3, pp. 617–628, 1987.View at: Publisher Site | Google Scholar
H.-K. Ko, B.-D. Park, and J.-C. Lim, “Studies on phase behavior in systems containing NP series nonionic surfactant, water, and D-limonene,” Journal of Korean Industrial and Engineering Chemistry, vol. 11, no. 6, pp. 679–686, 2000.View at: Google Scholar
A. Rodríguez, M. Muñoz, M. del Mar Graciani, S. Fernández Chacón, and M. L. Moyá, “Kinetic study in water-ethylene glycol cationic, zwitterionic, nonionic, and anionic micellar solutions.,” Langmuir, vol. 9, no. 3, pp. 9945–9952, 2004.View at: Google Scholar
N. J. Buurma, A. M. Herranz, and J. B. F. N. Engberts, “The nature of the micellar Stern region as studied by reaction kinetics,” Journal of the Chemical Society—Perkin Transactions, vol. 2, no. 1, pp. 113–119, 1999.View at: Google Scholar
M. Múñoz, A. Rodríguez, and M. del Mar Graciani, “Study of the reaction 1,1,1-trichloro-2,2-bis(p-chlorophenyl)ethane + OH- in nonionic micellar solutions,” Langmuir, vol. 15, pp. 7876–7879, 1999.View at: Google Scholar
J. Perkowski, J. Mayer, and L. Kos, “Reactions of non-ionic surfactants, triton X-n type, with OH radicals. A review,” Fibres& Textiles in Eastern Europe, vol. 13, no. 2, pp. 81–85, 2005.View at: Google Scholar
F. Mahmood, M. Arif, A. Ahmed, and S. B. Niazi, “Interaction studies of tween-40 with some acidic species at 20 C,” Journal of Research (Science), vol. 11, no. 1, p. 1, 2000.View at: Google Scholar
K.-H. Chung and S. Kim, “Oxidations of cyclohexanols by N-bromosuccinimide and sodium hypochlorite,” Bulletin of the Korean Chemical Society, vol. 7, no. 2, pp. 111–113, 1986.View at: Google Scholar
S. P. Mushran, K. Singh, L. Pandey, and S. M. Pandey, Proceedings of the Indian National Science Academy, vol. 46, no. 2, p. 119, 1980.
S. K. Mavalangi, M. R. Kembhavi, and S. T. Nandibewoor, “Oxidation of ethylenediaminetetraacetic acid by N-bromosuccinimide in aqueous alkaline medium—a kinetic study,” Turkish Journal of Chemistry, vol. 25, no. 3, pp. 355–363, 2001.View at: Google Scholar
S. Pandey and S. K. Upadhyay, Indian Journal of Chemical Technology, vol. 12, no. 1, p. 35, 2005.
K. K. Sengupta, B. A. Begum, and B. B. Pal, “Kinetics and mechanism of the oxidation of some aldoses, amino sugars and methylated sugars by tris(pyridine-2-carboxylato)manganese(III) in weakly acidic medium,” Carbohydrate Research, vol. 315, no. 1-2, pp. 70–75, 1999.View at: Publisher Site | Google Scholar
E. S. Amis, Solvent Effects on Reaction Rates and Mechanism, Academic Press, New York, NY, USA, 1966.
A. S. Perlin, “Ring contraction during the lead tetraacetate oxidation of reducing sugars,” Canadian Journal of Chemistry, vol. 42, pp. 2365–2374, 1964.View at: Google Scholar