Synthesis, Self-Aggregation, Surface Characteristics, Electrochemical Property, Micelle Size, and Antimicrobial Activity of a Halogen-Free Picoline-Based Surface-Active Ionic Liquid.

We present a new approach toward the design of a halogen-free picoline-based surface-active ionic liquid (SAIL) (1-octyl-4-methyl pyridinium dodecyl sulfate) [C8γPic]DS consisting of long dodecyl sulfate (DS) as an anion. The surface properties, micellization behavior, and antimicrobial activity in an aqueous solution were investigated using tensiometry, conductometry, and ultraviolet (UV) spectroscopy. Incorporating the DS group in SAIL leads to lower critical micellar concentration (CMC) and enhanced adsorption at the air/water interface of the functionalized ionic liquid compared to the C8-alkyl chain-substituted pyridine ionic liquids. The antimicrobial activity was evaluated against a representative Gram-negative and Gram-positive bacteria panel. Antibacterial activities increased with the alkyl chain length, C8 being the homologous most effective antimicrobial agent. The micelle size of [C8γPic]DS was determined by the dynamic light-scattering (DLS) study. Cyclic voltammetry (CV) measurements have been employed to evaluate the interaction between the SAIL micelle and working electrode, diffusion coefficient, and micelle size of the SAIL solution. The diffusion coefficient explored the correlation of surface properties and the antimicrobial activity of [C8γPic]DS. This halogen-free SAIL is the future of wetting agents and emulsion studies in agriculture due to its small micelle size and surface characteristics.

Introduction

As a new class of surfactants, ionic liquid-based surfactants have recently gained considerable interest. It has been shown that ionic liquids containing long alkyl chains are similar to traditional surfactants forming aggregates in water, which have evident amphiphilic properties and were regarded as new surfactants known as surface-active ionic liquids (SAILs).[1−3] Because of their structural characteristics, SAIL based on imidazolium is a class where the head and counterion replacement can be widely varied.[4,5] At present, the number of SAIL in the last decade increased due to the emerging need for chemicals in different fields. However, some critical concerns, such as the life cycle, reactivity, stability, and biodegradability of SAILs, have been studied.[6] However, most of the SAIL narratives in the document are narrowly focused on halogen-free SAILs. Thus, in the last few years, several greener amphiphiles based on structures have emerged, pointing out alkyl carboxylate,[7,8] amino acid,[9] and alkyl sulfate-based[10] SAILs free from halogen. The high tunability of SAIL opens up a wide range of applications, for example, in micellar catalysis, analytical chemistry, and electrochemical science.[10,11] During the last decade, alternative solvents have been introduced in diver’s electrochemical applications, i.e., ionic liquid (ILs). Wang et al. reported SAILs with enhanced surface properties compared to conventional surfactants and revealed their applications.[12] SAILs can also exhibit significant biological activity against bacteria and fungi.[13] In the reaction mechanism, separation or extraction process, and product yield, the molecular state of such ionic liquids in an aqueous system is expected to play a vital role. Pandey and group explored the application of ILs in biphasic separation.[14] In addition to the application, Zeng and group discovered the S-doped porous g-C3N4, which was fabricated using an ionic liquid.[15] For example, suppose aggregates of ILs are present in the system, they can interfere in a reaction as there may be undesired solubilization within the associates or may thermodynamically affect the response.

Despite the above-listed features, few studies deal with the colloidal chemical aspects of ILs based on amphiphilic methyl pyridinium. On the other hand, some authors have noted that changing the functional group of the ILs changes the antimicrobial activity.[16,17] For example, a significant decrease in antimicrobial activity was reported for imidazolium SAILs containing amide side chains than alkyl-substituted derivatives.[9] Morrissey et al. reported a notable reduction in the antimicrobial activity containing the ether or polyether side chains of imidazolium ILs, compared with the alkyl-substituted derivatives.[18] In contrast, Garcia et al., introducing a cationic mixture of SAIL and N-lauroyl sarcosinate, observed a broad spectrum of antimicrobial activity against bacteria.[19] Ana et al. synthesized a new class of SAILs from chloroquine (CQ) and fatty acids, which shows superior in vitro antimicrobial activity compared to the parent drug.[20] Another group of Feder-Kubis discovered terpene-based ionic liquids, which behaved as selective agents in antifungal therapy.[21]

The potential of these ILs is an interest in increasing the fundamental data in such devices as rechargeable batteries, electrochromic devices, etc.[22] Cyclic voltammetry (CV) is widely regarded as one of the most important electrochemical methods due to its excellent potency. In addition, CV data give vital information about the kinetics of electron transfer of heterogeneous reactions, thermodynamics of redox and oxidation processes, and the process of adsorption or a coupled chemical reaction. Many studies were conducted to screen the electrochemical window (EW)s of ILs. This is the initial stage in determining the appropriateness of the investigated ILs for the desired electrochemical applications. Lee and group discovered that the optimized electrochemical anodization treatment could significantly improve the descaling efficiency at least 50 times faster in an ionic liquid environment.[23] Water content is one of the most important elements influencing O’mahony et al. utilized the CV method to examine the EW.[24] McEwen and group found that the EWs for [BF4]−-based ILs are approximately 3.5 and 4.0 V for bis(trifluoromethylsulfonyl)imide [TFSI]-based ILs.[25] The surfactant’s electrochemical behavior was investigated to evaluate the micellar size. The diffusion coefficient of the surfactants can be assessed using the Randles–Sevcik equation with the peak current (ip) of each solution.[22] Asit et al. determined the diffusion coefficient and CMC of the sodium dodecyl sulfate (SDS), TX-100, and Tween-80 using the Randles–Sevcik and the Stokes–Einstein relation equation.[26] The size and shape of micelles are usually determined by a light-scattering method. However, Tsuyoshi et al. revealed the solution properties of micelles composed of fluorocarbon surfactants in which they determined the diffusion coefficient with the hydrodynamic micelle radius.[27]

In addition, ILs based on pyridinium cations are promising as they are surface-active and result in a successful biodegradable soft matter.[28] As a result, a perfect understanding of the aggregation behavior of long alkyl chain amphiphilic SAILs is an attractive study field in colloid and interface science from basic and practical perspectives. Therefore, the present study reports the synthesis, aggregation behavior, micelle size, and thermodynamic and antimicrobial activity that correlate with the diffusion coefficient and the surface parameters of picoline-based SAIL. Furthermore, the present work is expected to be used to study the properties of emulsifiers and wetting agents.

Methods and Materials

Materials

4-Methylpyridine (99%), 1-chlorooctane (>99.9%), and sodium dodecyl sulfate (SDS) were used as received. The solutions of the SAIL were prepared in distilled water for measurement.

Synthesis of SAIL

In a round-bottom flask, 15.00 g (0.161 mol) of 4-methylpyridine was taken, and 23.93 g (0.161 mol) of 1-chlorooctane was added dropwise and heated at 353.15 K for 48 h. The liquid product was cooled, and ethyl acetate was added with thorough mixing. The excess ethyl acetate was decanted, and the same process was repeated 4 times. After final washing, the traces of ethyl acetate (if present) were removed by heating under a vacuum for 12 h. 1-Octyl-4-methyl pyridinium chloride [C8γPic]Cl was obtained with a worked-out yield of 85.00%. The corresponding 1H NMR spectra are shown in Figure S1.

A solution of [C8γPic]Cl (35 mmol) was mixed with sodium dodecyl sulfate (35 mmol) in CH2Cl2, and sodium chloride salt was removed by filtration. The two phases were separated with a separating funnel. The organic phase containing SAIL was washed several times with water 10 × 10 × 10 cm3 until it was free of chloride (tested by AgNO3). After removing the solvent in a rotatory evaporator, the product [C8γPic]DS was obtained as a white liquid (70.82%) (Scheme ).

Scheme 1

Chemical Structure of 1-Octyl-4-methyl Pyridinium Dodecyl Sulfate (C26H49NO4S)

The NMR chemical shifts and assigned protons atoms are: 1H NMR (400 MHz, D2O, δ−ppm): 8.68 (q, 2H, CH), 7.80 (q, 2H, CH), 4.90 (m, 2H, CH2), 3.90 (t, 2H, CH2), 2.51 (s, 3H, CH3), 1.52 (m, 2H, CH2), 1.15 (m, 30H, CH2), 0.75 (t, 6H, CH3) (Figure S2).

Experimental Section

Thermogravimetric Analysis (TGA)

A Mettler Toledo thermal analyzer under a nitrogen environment was used to determine the decomposition temperature of the SAIL.

Conductometry

A digital conductivity meter was used to determine the electrical conductivity of SAIL in the water system at 298–318 K temperature (Systronics India Ltd., India), with the conductivity cell having a cell constant of 1 cm–1. Aqueous solutions of KCl (0.01–1 M) were used to verify the cell constant θ, and the specific conductivity of the aqueous solutions was calculated. The uncertainty in the measurements was ±0.3%.

Surface Tension

The surface-active parameters for the SAIL in the aqueous system at 25 °C were determined using a tensiometer (Krϋss K12 tensiometer, Biolin Scientific, China) with an uncertainty of ±0.1 mN m–1.

DLS

Dynamic light-scattering (DLS) measurements were performed at 25 °C for an aqueous SAIL solution using a ζ-sizer (Nano-S90, Malvern Instruments) to measure the hydrodynamic particle size. The wavelengths of the laser and the scattering angle were 633 nm and 90°, respectively.

Electrochemical Measurements

Cyclic voltammetry (CV) was performed using an electrochemical workstation (CHI660 E, CHI) at −1.2 to 1.0 V at a 5 mV/S scan rate. In CV, three-electrode systems were used. A platinum wire was used as a counter, glassy carbon was used as a working electrode, and a saturated calomel electrode (SCE) was used as a reference electrode.

UV Spectroscopy

The ultraviolet (UV) absorption spectra of the sample were recorded using a UV–vis spectrophotometer (Shimadzu UV 1800, Japan). The spectra were recorded in the 180–400 nm wavelength range at 25 °C. Pyrene was used as a probe, and concentration was kept constant (1 × 10–6 mol dm–3) in all experiments.

Antimicrobial Activity

The antimicrobial activity of the synthesized SAIL was determined based on the minimum inhibitory concentration (MIC) values against two Gram-negative, Shigella dysentery (MTCC 1457) and Salmonella typhi (MTCC 98), and four Gram-positive, Staphylococcus epidermidis (MTCC 3382), Bacillus subtilis (MTCC 411), Streptococcus pneumoniae (MTCC 655), and Streptococcus aureus (MTCC 96), bacterial strains. The detailed procedure for this activity is given in Supporting Section 1.1.

Result and Discussion

Thermal Analysis

Figure depicts a typical thermogram of [C8γPic]DS. Thermogravimetric analysis was performed in the temperature range of 25–550 °C, at a heating rate of 10 °C per minute. The data from the analysis indicates that the decomposition of the SAIL occurs in three steps as shown in the figure. In the TGA and derivative thermogravimetry (DTG) thermogram, the first weight loss around 35–145 °C corresponds to the loss of a water molecule; this loss of weight is more likely linked to the thermal breakdown/hydrolysis of the SAIL (which causes the formation/vaporization of secondary byproducts).[30] The second decomposition observed in the range of 193–348 °C is attributed to the decomposition of the hydrocarbon chain (DS–), and the last decomposition indicates the degradation of the cationic moiety (C8γPic+).

Figure 1

TGA curve of [C8γPic]DS.

Conductance Measurements

Electrical conductivity measurement was applied to study the micellar aggregate formation of SAIL. Figure reveals the change in the electrical conductivity (k) depending on the concentration of [C8γPic]DS in a temperature range of 25–45 °C. It is evident that the progressive increase in the SAIL concentration results in two pieces that fit into two straight lines with a significant variation in the slope, which is caused by micelle formation, and the intersection of the two consecutive lines is ascribed to critical micellar concentration (CMC), which is shown in Table . From Table , it is seen that the reduction of CMC occurs when the anion of [C8γPic]Cl will change from Cl to DS. [C8γPic]Cl has a CMC of 175 mM, while in the case of [C8γPic]DS, it is 1.5 mM, which is 100 times lower. As the establishment of the CMC will depend upon the molecule’s hydrophobic nature, it was visually differentiated that [C8γPic]DS had 12 extra carbon chains rather than [C8γPic]Cl. With increasing temperature, the CMC values of [C8γPic]DS increase slightly, which is similar to the case for the reported SAILs, [C4mim][C12H25SO3][31] and [C12eim]Br,[32] and conventional ionic surfactants. The ratio of the slopes of postmicellar to premicellar plots of specific conductivity vs concentration plots can estimate the degree of counterion dissociation (β). As shown in Table , values of the β increase as temperature increases due to the high mobility of micelle formation (Table ).

Figure 2

Plots of electrical conductivity vs concentration of aqueous solutions of SAIL at different temperatures.

Table 2

Value of CMC with Standard Error, Temperature (T), Degree of Counterion Dissociation (β), Gibbs Free Energy of Micellization (ΔGm°), Standard Enthalpy of Micellization (ΔHm°), and Standard Entropy Change (ΔSm°) for SAILs at Different Temperaturesa

SAIL	temp (°C)	COND CMC (mM)	β	ΔGm° (kJ/mol)	ΔHm° (kJ/mol)	TΔSm°(kJ/mol)
[C8γPic]DS	25	1.50	0.44	–34.08	–7.82	26.26
	35	1.61	0.45	–35.39	–8.41	26.99
	45	1.7	0.47	–36.46	–9.02	27.44
[C8γPic]Cl[35]	25	175	0.46	–20.80	–1.59	64.60
[C8Py]Cl[35]	25	180	0.43	–20.40	–1.49	63.40
[bmim]DS[36]	25	2.04	0.61	–24.68	–7.14	17.58

Standard uncertainties are ΔGm° = ±0.02 (kJ mol–1), ΔHm° = ±0.01 (kJ mol–1), and TΔSm° = ±0.02 (kJ mol–1).

Table 1

Description of Chemicals and Solvents Used

chemical name	source	CAS no.	purity (%)
4-methylpyridine	Sigma-Aldrich	108-89-4	99
1-chlorooctane	Sigma-Aldrich	111-85-3	99.0
sodium dodecyl sulfate	Sigma-Aldrich	151-21-3	≥99.0
dichloromethane	Sigma-Aldrich	75-09-2	≥99.8

Standard Free Energy of Micellization (ΔGm°)

The determination of thermodynamic parameters of micellization standard free energy change (ΔGm°) plays an essential role in developing micelles, which is discussed as follows

where XCMC is the mole fraction, R is the gas constant, and β is the degree of counterion dissociation discussed earlier. Calculated thermodynamical parameters for [C8γPic]DS at different temperatures are reported in Table . The [C8γPic]DS moiety reduces electrostatic repulsions between the head and tail groups, preferring micellization and resulting in a more negative free energy transfer. The values of ΔGm° become more negative as temperature increases in SAIL, showing that micellization is spontaneous. The presence of DS enhances the spontaneous aggregate formation via the transfer of the hydrophobic tail from the bulk solution to the micelle phase, as shown in Table .

Standard Enthalpy Change (ΔHm°)

The enthalpy of micellization was determined using the following equationwhere [d(ln XCMC)/dT] denotes the slope of the straight line of ln XCMC vs temperatures. According to Table , the standard enthalpy of micellization value is negative. As the hydrogen bonds between water molecules weaken, less energy is required to break up the water cluster, which holds the structure’s hydrocarbon chain over the whole temperature range.

Standard Entropy Change (ΔSm°)

The entropy of micellization was determined using eq and the obtained values increased as the temperature increased, as tabulated in Table . Therefore, the micellization process is governed by the entropy gain associated with [C8γPic]DS. It stands for the fact that the negative value of ΔGm° is mainly due to ΔSm°, which implies the method of micellization of [C8γPic]DS.

Standard Free Energy of Adsorption (ΔGads°)

The standard free energy of adsorption (ΔGads°) at the air/water interface was calculated using eq ((33)where ΔGm° is the standard free energy of micellization, and ΠCMC and Γmax are listed in Table . DS is hydrophobic in nature and easy to form a micelle. The introduction of the DS as an anion into the SAIL causes an increase in the hydrophobicity nature of the molecule, as evidenced by the increase in the value of ΔGads°. Therefore, the ΔGads° value is superior to the ΔGm° value.

Table 3

CMC, Surface Excess Parameter (Γmax), Minimum Surface Area Per Molecule (Amin), Surface Pressure at CMC (πCMC), Adsorption Efficiency (pC20), Surface Tension at CMC (γCMC), Standard Free Energy of Adsorption (ΔGads°), and Free Energy at the Air/Water Interface (ΔGmins) for [C8γPic]DS at 25 °Ca

SAIL	CMC ST (mM)	CMC UV (mM)	Tmax ×1010 (mol/cm2)	Amin (Å)2	πCAC	pC20	γCMC	ΔGads°(kJ/mol)	ΔGmins (kJ/mol)
[C8γPic]DS	1.48 ± 0.3	1.50 ± 0.2	4.52	36.73	53.40	3.23	18.59	–45.85	4.11
[C8γPic]Cl[35]	175.00		1.65	101.00	40.70	2.20	31.00	–45.46	18.85
[BMPy]LS[40]	1.53 ± 0.10		4.91	34.00	35.70		36.50
[C8Py]Cl[35]	181.00		1.70	98.10	34.60	1.60	36.84	–40.75	21.76
[bmim]DS[36]	2.09	2.02	1.75	95.00	37.50			–46.12
[C8APyr]LS[19]	1.0 ± 0.1		2.0	82.00	44.30	4.10	27.70
SDS[37]	8.21		3.11	53.00	32.29		39.68	–39.53	12.76

Standard uncertainties are ΔGads°= ±0.01 (kJ mol–1) and ΔGmins = ±0.03 (kJ mol–1).

Free Energy at the Air/Water Interface (ΔGmins)

The value of ΔGmins is a transition of free energy of the bulk phase of a system at the air/water interface determined by the following equation.[34]

The value of ΔGmins is defined as a free energy shift accompanied by a transition from the bulk phase of the solution to the surface component of the solution. The lowest free energy [C8γPic]DS = 4.73 KJ/mol is more thermodynamically stable, which is measured to evaluate the synergism compared to [C8γPic]Cl = 18.85 kJ/mol and [C8Py]Cl = 21.76 kJ/mol (Table ).

Surface Parameters

The surface tension was measured to evaluate the CMC and the surface activity of the SAIL in aqueous solutions. The solutions’ surface tension (γ) was plotted against log C, as shown in Figure . The surface tension dropped rapidly as the concentration was increased before subsequently stabilizing. The surface parameters such as surface excess concentration (Γmax), minimum surface area per molecule at the interface (Amin), surface tension at CMC (γCMC), the effectiveness of the adsorption efficiency (pC20), and surface pressure at CMC (πCMC) of the SAIL are provided in Table . The CMC value for [C8γPic]DS is discovered by the break-in γ-log C curve, and γCMC is observed at the breakpoint, which is listed in Table . Therefore, the present study had a better result in the form of CMC compared with the data reported for SDS,[37] [C4mim][C12SO4],[38] [C8γPic]Cl,[35] and N-octylpyridinuim bromide [C8Py]Br,[39] which have the same hydrophobic chain length.

Figure 3

Surface tension as a function of log C of [C8γPic]DS at 25 °C.

Sastry and co-authors discovered that the increase in hydrophobicity of the SAIL decreases the CMC, which was observed for [C8γPic]DS. The results (Table ) evidently show that [C8γPic]DS has relatively lower CMC and γCMC than [C8γPic]Cl, [C8Py]Br, and SDS, which reveals that [C8γPic]DS display more excellent surface activity than ionic surfactants and imidazolium-, pyridinium-, or pyrrolium-based SAILs.[35] The difference in the surface tension of the SAILs due to the formation of micelles results because of the following two reasons: (1) the electrostatic and hydrophobic interaction at the air–water interface and (2) picoline has a bulky counterion, which makes the hydration process weaker, and counterions reduce the electrostatic repulsion between head groups. During the formation of micelles, it serves a similar role to the second hydrophobic chain (i.e., dodecyl on the counterion ring), resulting in the lower CMC and γCMC of [C8γPic]DS. In addition, Jiao et al. showed that N-butyl-N-methylpyrrolidinium dodecyl sulfate ([C4MP] [C12SO4]) could form micelles in an aqueous solution, and its CMC was 2.7 mmol/L, which is higher than that of [C8γPic]DS.[10] Interestingly, the CMC value of [C8γPic]DS is about 100-fold lower than [C8γPic]Cl and less than a quarter of that for SDS (CMC = 8.2 mM).[35,38]

Maximum Surface Excess Concentration (Γmax)

The maximum surface excess concentration (Γmax) at the air–water interface can be obtained from the slope value of (dγ/d ln C) using the Gibbs adsorption isotherm

where R is the molar gas constant (8.314 J mol–1 K–1) and T is the absolute temperature. The number of ionic species present in the solution produced by the dissociation of SAIL molecules is denoted by n. The value of n = 2 for the SAIL, [C8γPic]DS, contains a picoline ring with one positive charge and a counterion, i.e., dodecyl sulfate with one negative charge on it. The adsorption of [C8γPic]DS at the air/solution interface is enhanced by the electrostatic repulsion between the cationic head group and the anion of [C8γPic]DS, which, in turn, increases the maximum surface excess concentration, resulting in a higher value of the Γmax (4.52 mol cm–2) compared to [C8γPic]Cl (1.65 mol cm–2), as presented in Table . The property of adsorption in the bulk solution or on the interface layer of the SAIL molecule opens the door for various applications.[41] This reveals that aggregates’ concentration is high at the surface and they have high surface activity compared to halogen-based SAILs, which give good antimicrobial activity.

Area Occupied by a Single Molecule (Amin)

The values of the minimum area per molecule (Amin), i.e., the area occupied by a single surfactant that reflects the surface arrangement of SAIL at the air–liquid interface, have been obtained using eq (

where NA is Avogadro’s number (6.022 × 1023 mol–1). The calculated value of the Amin (41.5 A2) is presented in Table . These data indicate that the values of Γmax and Amin vary with the molecular structure, as replacing the Cl anion with DS allows the SAIL molecules to be more tightly packed at the air–liquid interface.

Surface Pressure at the CMC (πCMC)

The values of surface tension of the solvent (γ0) and that of the SAIL solution at the CMC (γCMC) have been used to evaluate the surface pressure at the CMC (πCMC), as shown in eq (

As the hydrophobic chain length increases, the SAIL becomes more effective in reducing surface tension, as shown by γCMC (Table ). πCMC, on the other hand, increases when the hydrophobicity of SAIL increases, indicating that the SAIL molecule is ordered asymmetrically in the lattice crystal, resulting in a more significant reduction in the micellar surface area.

Adsorption Efficiency (pC20)

The adsorption efficiency (pC20) of the SAIL at the interface was evaluated by employing eq (where pC20 is defined as the negative logarithm of the concentration of the SAIL required to reduce the surface tension of the pure solvent by 20 mN/m; the values of the efficiency of the SAILs are shown in Table . Using adsorption efficiency values, you may compare SAIL adsorption effectiveness at the air/water interfaces. A higher pC20 value decreases surface tension more effectively. For example, [C8γPic]DS has higher adsorption effectiveness at the interface than [C8γPic]Cl because of the hydrophobic chain’s elongation and the anion’s size.

The [C8γPic]DS absorbance behavior in the UV–visible region (180–300 nm) was examined in our spectrophotometric investigation. Pyrene is used as a UV probe in our studies. Figure represents the magnification of the recorded spectra in the wavelength range of 180–300 nm. Two pyrene peaks are due to the ring structure, and pyrene’s characteristic absorption peaks are at 223.46 and 258 nm, as shown in Figure . The one at 223.46 nm shows the most absorbance and is selected for different studies.

Figure 4

Absorbance spectra of [C8γPic]DS at different concentrations.

For wavelengths in this range, a typical absorption vs concentration figure indicates that up to a particular SAIL concentration, absorbance varies linearly with the concentration according to Beer–Lambert’s law.

In general, a typical plot of absorbance vs concentration at a constant wavelength, i.e., 223.46 nm of [C8γPic]DS, is shown in Figure , and the observed CMC of [C8γPic]DS is presented in Table . Sudden absorption jumps (Figure ) are caused by developed micelles, which live in a nonpolar environment.

Figure 5

Plot of absorbance vs the changing concentrations of [C8γPic]DS at a fixed wavelength of 223.46 nm.

The mechanism of SAIL’s micellization to the pyrene interaction is based on two possible factors: (1) Naturally, pyrene is driven to settle in the micelle’s nonpolar interior, which decreases the hydrophobic repulsion forces between water and pyrene and (2) there is no hydrophilic pyrene functionality that may draw pyrene to remain on the interface.[42] Nevertheless, it is clear that in this work, the CMC acquired by [C8γPic]DS through spectroscopic methods is in good agreement with the value reported by conductometry and tensiometry.

DLS Study

DLS measurements were used to investigate the hydrodynamic radius of the SAIL at 298 K. In general, the distribution of size during the aqueous mass phase depends largely on the conformational modification of the molecular system, regardless of the volumetric profile’s quantitative nature.[43] The number size distribution of [C8γPic]DS above the CMC concentration is shown in Figure . Since [C8γPic]DS behaved similarly at all concentrations, we have chosen a 5 mM solution for further study. C12MeIm-LS aggregates with a hydrodynamic diameter (Dh) of ∼35 nm consistent with elongated micelles were detected, whereas, for C14MeIm-LS, the presence of aggregates with a Dh ≥ 200 nm was observed. Amide-functionalized SAIL-LS mixtures (C8AMeIm-LS) homologues had a Dh of 22 nm, indicating micelle formation.[19] During analysis of a [C8γPic]DS aqueous solution, using Stokes–Einstein relation eq (, the diffusion coefficient value for [C8γPic]DS is 3.03 × 10–7 cm2/s, and a single peak is observed with maximum intensities in the range of 10–30 nm.where kB is denoted as the Boltzmann constant and ηo is denoted as the solvent’s viscosity. DLS results showed a single distribution of the hydrodynamic radius, Rh ∼7.9 nm. It seems that the presence of a dodecyl sulfate (DS) group as an anion and a C8 carbon chain at the γ(γ) position to picoline promotes the aggregation of the micelle and smaller size compared to the nonfunctionalized SAIL. Notably, there is a rough correspondence with CV data.

Figure 6

Size distribution curve of [C8γPic]DS.

Cyclic Voltammetry (CV)

The cathodic potential value of the [C8γPic]DS solution decreases due to electrostatic repulsion between SAIL micelles and OH– shown in Figure . Anodic peak size decreases when the adsorption process is taken by [C8γPic]DS micelles near the working electrode, taking up the space of OH–. A consequence of this interaction is the enrichment of H+ ions around the surface of [C8γPic]DS micelles due to the attraction between anionic and cationic ions. Enrichment with H+ ions leads to a higher anodic current. Figure shows the cyclic voltammograms of 5 mM [C8γPic]DS in an aqueous solution for various scan rates. The SAIL solution has the cathodic potential, which appears from −0.60 to −0.66 V, and the anodic potential appears from +0.08 to +0.12 V.

Figure 7

Schematic illustration of the mechanism of [C8γPic]DS micelle solutions near the electrode.

Figure 8

Cyclic voltammogram of the SAIL.

In cyclic voltammetry (CV), the peak ip (μA) for a redox-active system is given by eq where F = Faraday constant, A = area of the electrode (cm2), n = number of electrons involved in oxidation or reduction, D = diffusion coefficient of the electroactive species (cm2 s–1), C = concentration of SAILs (M), ν = sweep rate (V s–1), R = gas constant, and T = absolute temperature.

The potential was measured in a 5 mM solution of [C8γPic]DS at a scan rate of 0.005 V s–1. Therefore, eq is rewritten as eq . The solution species oxidized or reduced at 303 K to get linear diffusion.

where A is the electrode area, n is the number of electrons involved in oxidation or reduction, D is the diffusion coefficient, C is the SAIL concentration, and v is the scan rate.

The diffusion coefficient was calculated from the slope of ipc vs v1/2, as shown in Figure . From the slope, the diffusion coefficient value for [C8γPic]DS is 2.88 × 10–7 cm2/s. Asakawa and group investigated the properties of the solution of micelles composed of fluorocarbon surfactants and ferro-cetyltrimethylammonium bromide (FcTAB) systems. The diffusion coefficient and the hydrodynamic radius of FcTAB in water were 5.9 × 10–6cm2/s and 4.1 Å, respectively. The diffusion coefficient significantly reduced with the increase in the salt concentration, implying an increase in micellar size and a change in the micelle form.[27] The hydrodynamic radius of [C8γPic]DS obtained from the Stokes–Einstein relation (eq ) was 8.33 nm. The value of the hydrodynamic radius and the diffusion coefficient were obtained from the CV data compared with DLS data.

Figure 9

Plot of cathodic peak current vs square root of the sweep rate of 5 mM [C8γPic]DS.

This study evaluated the antibacterial property of a picoline-based SAIL with an eight-carbon chain by measuring the minimum inhibitory concentration (MIC) values first and then comparing to those of other SAILs (Table ). Compared to the decisive, broad-spectrum antibacterial action of short-chained ILs has poor biological activity. A series of microbial inhibition studies were performed on imidazolium ILs with varying chain lengths and anions.[2] Compared with other ILs, the imidazole-based SAIL with an eight-carbon chain compound 1-alkyl-3-methylimidazolium chloride, [OMIM]Cl, showed better activity than the butyl-[BMIM]Cl- and hexyl-[HMIM]Cl-substituted compounds. Their preferential adsorption at the bacterial cell wall disrupts the bacterial membrane due to the optimal hydrophilic/lipophilic balance.[44] There were also some changes in antibacterial activity between Gram-positive and Gram-negative bacteria. Gram-negative bacteria were shown to be similar or somewhat more resistant to the SAIL than Gram-positive bacteria. This might be attributed to the difference in membranes and cell walls between different types and strains of bacteria. There is an additional lipopolysaccharide membrane presenting an additional barrier to Gram-negative bacteria. This barrier contributes to Gram-negative bacteria’s high tolerance to [C8γPic]DS. In addition, the bactericidal activity from cell viability curves has been determined by the colony forming unit (CFU) (Figure ), in line with Carson et al.’s findings, which evaluate the antibiofilm activity of 1-alkyl-3-methylimidazolium chlorides to test the general applicability of ionic liquids as a biofilm. Gram-negative bacteria Escherichia coli had MIC = 722 μM and Gram-positive bacteria S. epidermidis had MIC = 361 μM for [C8mim]Cl.[45] As a result, it can be observed (Table and Figure ) that [C8γPic]DS had a greater efficacy against Gram-positive than Gram-negative bacteria. The antimicrobial activity of amide-functionalized ILs was evaluated against a panel of representative Gram-negative and Gram-positive bacteria and fungi.[9] In addition, without the functional group attached to the cation, halogen-free SAIL [C8γPic]DS has better activity than the 3-alkoxy methyl-1-methylimidazolium salts of hexafluorophosphates, tetrafluoroborates, and chlorides.[46]

Table 4

Minimum Inhibitory Concentration (MIC) Values Represent Mean (n = 3) + Standard Error of [C8γPic]DS against the Selected Gram-Positive (S. epidermidis, B. subtilis, S. pneumoniae, S. aureus) and Gram-Negative (S. dysentery, S. typhi) Bacterial Strains

	MIC (mM)			MIC (μM)
microorganism	[C8γPic]DS	[CMPy]DS[29]	[CMPy]DBS[29]	C12EPyrLS/C12EMeIm-LS[19]
Gram-Positive
S. epidermidis	1.17 ± 0.06	4.83 ± 0.16	2.33 ± 0.16	31/8
B. subtilis	2.27 ± 0.07	1.80 ± 0.00	2.00 ± 0.00	31/16
S. pneumoniae	1.40 ± 0.11	0.90 ± 0.05	1.80 ± 0.05
S. aureus	4.33 ± 0.16	5.33 ± 0.16	2.33 ± 0.16	31/16
Gram-Negative
S. dysentery	3.40 ± 0.11
S. typhi	4.83 ± 0.16

Figure 10

Growth curve of four gram-positive bacteria (S. epidermidis, B. subtilis, S. pneumoniae, S. aureus) and two gram-negative (S. dysentery, S. typhi) bacterial strains in the presence of different concentrations (0.1–5 mM) of [C8γPic]DS values represent mean of CFU/mL (n = 3) ± standard error.

Diffusion is a function of the fluid, which includes the size of the penetrant and diffusing molecule, nature of the solvent, concentration, and solubility of the molecules. Moreover, the chances of [C8γPic]DS reaching the microorganism’s surface by diffusion are high, as the small area of molecules diffuses more rapidly. This phenomenon has been proved by the maximum value of surface excess concentration (Γmax = 4.52 mol/cm2) and the minimum surface area occupied by the single SAIL molecule at the air/liquid interface (Amin = 41.50 (Å)2). Here, the diffusion coefficient was determined using the DLS and CV techniques with values of 3.03 × 10–7 and 2.88 × 10–7 cm2/s, respectively. It is a simple relation among the Γmax, Amin, and diffusion coefficient. (1) As the area occupied by each molecule decreases (Amin), it directly affects the surface of the liquid, which increases Γmax and (2) the layer of the surface occupied by small molecules of the SAIL enhances the property of diffusion in the antimicrobial activity. The correlation of these three parameters results in a smaller molecular area and more surface excess concentration, which diffuses rapidly with the small value of the diffusion coefficient.

In addition, it can be said that a smaller Amin and a higher diffusion coefficient impacted the antimicrobial activity with a small amount of the SAIL concentration used to achieve the MIC value. Thus, the data presented here for the antimicrobial activity are essential to understanding the interaction between cell surface structures and existing wetting agents in the agriculture field.

Conclusions

This study uses picoline, octyl-chloride, and dodecyl sulfate as raw materials to synthesize a halogen-free alkyl sulfate-based SAIL (1-octyl-4-methyl pyridinium dodecyl sulfate) [C8γPic]DS, and the structure was confirmed by 1H NMR spectroscopy. To investigate their adsorption at the air/liquid interface, thermodynamic parameters, and aggregation in aqueous solutions, several techniques were employed, namely, conductivity, surface tension, and UV spectroscopy. The observed study of this research is as follows:

[C8γPic]DS (1.60 mM) exhibited a 100-fold smaller CMC and interfacial and bulk properties in terms of γCMC, pC20, Amin, etc., than their parent analogue, [C8γPic]Cl (175 mM), and other conventional SAILs [Etmim][C12H25SO3] (3.32 mM)[47] and C8Pyr-LS (2.0 mM).[19] Micelle formations of SAIL were spontaneous and entropy-driven.

The improved colloidal and surface behavior of the SAIL is due to the increased hydrophobicity of the SAIL caused by replacing a Cl anion with a DS hydrophobic counterion.

The growing development of green technology demands new, biodegradable materials in which picoline-based SAILs significantly impact the microbes. Furthermore, SAILs exhibited different levels of sensitivity to Gram-positive and Gram-negative bacteria. Therefore, it can be observed that [C8γPic]DS had a greater efficacy against Gram-positive than Gram-negative bacteria and acted as a broad-spectrum antimicrobial agent.

Here, DLS and cyclic voltammetry measurements revealed that the colloidal solutions of [C8γPic]DS predominantly formed micelles having the hydrodynamic radii (Rh) ∼7.9 and ∼8.33 nm, respectively. The voltammetric analysis suggests that this reduction process occurs by the subsequent formation of an oxide phase on the electrode surface. The decreased diffusion coefficient value reflects the impact of the DS group on the SAIL as it helped decrease the micelle size and the CMC.

The lower CMC and smaller micelle size of [C8γPic]DS enhance the understanding of aggregates in colloids and surface sciences. In addition, having the lower surface tension and surface parameters is expected to build the foundation for their properties in suitable applications like a wetting agent in agriculture, drug delivery, and nanomaterial fields.