# Dispersive Surface Energy and Acid-Base Parameters of Tosylate Functionalized Poly(ethylene glycol) via Inverse Gas Chromatography

Authors: Feyza Sesigur; Dolunay Sakar; Ozlem Yazici; Fatih Cakar; Ozlem Cankurtaran; Ferdane Karaman
Journal: Journal of Chemistry
 (2014)

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## Abstract

An inverse gas chromatographic (IGC) study of the sorption properties of poly(ethylene glycol) modified with tosylate (PEG-TOS) was presented. PEG-TOS was synthesized via the tosylation of the corresponding poly(ethylene glycol) (PEG) withp-toluenesulfonyl chloride in the basic medium. The synthesized PEG-Tos was characterized by FTIR-ATR and 1HNMR techniques. The retention diagrams of n-hexane, n-heptane, n-octane, n-nonane, n-decane, dichloromethane, chloroform, acetone, tetrahydrofuran, ethyl acetate, and ethanol on the PEG and PEG-Tos were plotted at temperatures in K between 303 and 373 by inverse gas chromatography technique. The dispersive component of the surface-free energy, γSD, of studied adsorbent surface was estimated using retention times of different nonpolar organics in the infinite dilution region. Thermodynamic parameters of adsorption (free energy, ΔGAS, enthalpy, ΔHAS, and entropy, ΔSAS), dispersive components of the surface energies, γSD, and the acid, KA, and base, KD, constants for the PEG and PEG-Tos were calculated and the results were discussed.


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## Body

## 1. Introduction

PEG is widely used in the pharmaceutical and biomedical fields. It is a nonionic polymer, soluble in water, and most common organic solvents. The incorporation of a PEG segment in a macromolecule modulates its solution properties [1]. Functionalized PEG gives opportunity to synthesize water soluble block copolymers. Tosylates are good substrates for substitution reactions. When PEG is functionalized with tosylate, it can be useful to synthesize block copolymers such as water-soluble diblock copolymer of polysulfonic diphenyl aniline and poly(ethylene glycol) [2].Inverse gas chromatography (IGC) has been used for investigation of the interactions of polymers with various liquids [3, 4], hyperbranched aliphatic polyesters [5], block copolymers [6], polymer blends [7], nanocomposites [8], cement pastes [9], crude oils [10], surface properties of Schiff base [11], and liquid crystals [12, 13]. The method being simple, relatively rapid, with good accuracy, and of low cost and available equipment provide valuable thermodynamic information for physicochemical characterization of materials [14]. From the IGC measurements, the physicochemical properties can be obtained for polymeric systems including the weight fraction activity coefficients of solvents at infinite dilution, interaction parameters of polymers with solvents and polymers, surface, molar heat and free energies of mixing and sorption, solubility parameter, glass transition, melting points, and degree of crystallinity of polymers [15]. Using these parameters and appropriate models allow understanding of the intermolecular interaction responsible for solvation in the stationary phase.In this study, we aimed to understand the effect of tosylate on some thermodynamic parameters and surface properties of PEG. The retention diagrams of some solvents on the PEG and PEG-Tos were obtained by IGC, and surface parameters with the studied solvents were determined. These surface properties were the dispersive component of the surface energy, basic thermodynamic parameters of adsorption, and the degree of acidity-basicity of the surface of the PEG and PEG-Tos.


## 2. Inverse Gas Chromatography Measurements under Infinite Dilution

IGC is an adaptation of conventional gas chromatography that is used in the characterization of material surfaces. The adsorbate net retention volumes,VN, are calculated from the expression
(1)VN=QJtR-tATTf,
where tR is the retention time of the probe, tA is the retention time of air, Q is volumetric flow rate measured at column outlet and at ambient temperature, Tf (K), T (K) is the column temperature, and J is the James-Martin gas compressibility correction factor [16, 17]. The interactions experienced between an adsorbate and an adsorbent can consist of two components-specific and dispersion forces. Dispersion forces, also known as London forces, are present between all molecules, regardless of their identity. Specific forces generally rely on some compatibility between the structures of the interacting molecules, either physically or electronically [18].In the analysis of the dispersive component of the surface-free energy of solid surfaces by IGC, are used three approaches which are Riddle Jr. and Fowkes [19] (referred to as Schultz and Lavielle approach by some authors; all references are given in [19]), Dorris and Gray [20], and Flour and Papirer [21].According to Fowkes approach, the dispersive component of the surface energy,γS (Jm−2), is determined using [19]
(2)-ΔGA=RTln⁡VN=2NaγSD0.5γLD0.5+C.
Thus for a series of nonpolar probes, a plot of RTln⁡VN against a(γLD)0.5 will give a slope of 2N(γSD)0.5. Values of a(γLD)0.5 of nonpolar solvents are found in the literature [19]. The specific component of the free energy is determined from the n-alkane plot of RTln⁡VN against a(γLD)0.5. The distance between the ordinate values of the polar probe datum point and the n-alkane reference line gives the specific component of the surface-free energy, -ΔGAS.An equation may be written for this procedure,(3)-ΔGAS=RTln⁡VN,nVN,ref,
where VN,n and VN,ref are the retention volume for the polar probe and the retention volume for the nonpolar reference line, respectively.The adsorption of a polar probe onto the adsorbent surface leads to a change in the enthalpy of the system and the entropy of the system. These factors are related to the energy of adsorption by the equation(4)ΔGAS=ΔHAS-TΔSAS.
Here, ΔHAS is the adsorption enthalpy by Lewis acid-base interactions, ΔSAS is the adsorption entropy Lewis acid-base interactions, and T is the column temperature. For each polar probe, ΔHAS and ΔSAS can be determined from a plot of -ΔGAS/T against 1/T.The surface Lewis acidity and basicity constants,KA and KD, may be calculated from the following equation
(5)-ΔHAS=KADN+KDAN*.
Here, DN and AN* are Gutmann’s donor and modified acceptor numbers, respectively. The AN*, DN, and a(γLD)0.5 values of the polar probes are taken from [19].K
A and KB are obtained from a plot of -ΔHAS/AN* versus DN/AN* with KA as the slope and KD as the intercept. Parameters KA and KD reflect the ability of the examined surface to act as an electron acceptor and electron donor, respectively [19].


## 3. Experimental Part

### 3.1. Synthesis of Tosylated Poly(ethylene glycol)

Polyethylene glycol 400 for synthesis (HO(CH2CH2O)nH) (average molecular mass 380–420 g/mol, Tg=-5°C) andp-toluenesulfonyl chloride (99 wt%) were purchased from Merck. PEG-Tos was synthesized via the tosylation of the corresponding PEG withp-toluenesulfonyl chloride in a two-phase system containing THF/water: 8/3 v/v in the presence of NaOH (in Scheme 1). The detailed procedure can be described as follows. An amount of 0.0936 mol of PEG-400 and an amount of 25 mL of THF were introduced in a 250 mL, round-bottom flask possessing a magnetic stirrer. NaOH, 0.1398 mol, dissolved in 30 mL of water was introduced into the flask, and the system was mixed for a few minutes in a salt-ice bath around −5°C until a white emulsion was formed. Tosyl chloride (TosCl) was divided into two parts, and the first 0.02885 mol of TosCl dissolved in 30 mL of THF was added dropwise within 1 h, and another 0.06688 mol of TosCl (total 0.09573 mol) dissolved in 25 mL of THF was added within another 1 h also dropwise with intensive stirring. The reaction was continued for 4 h at −5°C, after which the reaction temperature was raised up to room temperature and kept at that temperature for 18 h. After reaction, 100 mL of diethyl ether was added, and then two layers were formed. The water layer was extracted three times with diethyl ether (30 mL each time), and the entire diethyl ether phase was washed with water a few times until being neutral (pH = 7). The diethyl ether solution was dried by passing through an anhydrous Na2SO4 (30 g) column until a clear diethyl ether solution was obtained. The diethyl ether was removed with a rotary evaporator. The synthesized PEG-Tos was a transparent liquid. The yield was about 80 wt%. 1HNMR and Fourier transform infrared (FTIR) measurements on an attenuated total reflection accessory (ATR) were carried out on a 500 MHz INOVA-500 and a Perkin Elmer FTIR-ATR, respectively.Scheme 1
Synthesis of PEG-Tos.


### 3.2. Inverse Gas Chromatography Measurements

Studied solvents such as n-hexane (Hx), n-heptane (Hp), n-octane (O), n-nonane (N), n-decane (D), dichloromethane (DCM), chloroform (Ch), acetone (Ac), tetrahydrofuran (THF), and ethyl acetate (EA) were also taken from Merck. They were HPLC grade at 99% purity in molecular sieve and used without further purification. The support materials being Chromosorb W (AW-DMCS-treated, 80/100 mesh) were supplied from Merck. Silane treated glass wool used to plug the ends of the column was obtained from Alltech Associates, Inc.A Hewlett-Packard 6890 Model gas chromatograph with a thermal conductivity detector was used to measure the retention time of the solvents in this study. The column was stainless steel tubing with 3.2 mm o.d. and 0.5 m in length. The PEG and PEG-Tos polymers were coated on the support by slowly evaporation of chloroform as stirring the Chromosorb W in the polymer solution. The amount of coated polymer on the support was determined as 10% by calcination. Trace amount of solvent was injected into the chromatograph. Small volumes of vapor probes were injected manually to achieve the infinite dilution conditions. The column was conditioned at 393 K for 24 h under helium atmosphere at flow rate 30 cm3/min. Zero coverage conditions were reached by injecting 5 μL of vapors of the different probes. In these conditions the interactions between adsorbate molecules themselves are negligible and the thermodynamic parameters, calculated using the retention time of each probe, depend only on the adsorbate/adsorbent interactions. In the case of IGC measurement at infinite dilution, minor amounts of vapors of the test solutes are injected into the column filled with polymer, permitting the lateral interactions between the adsorbed molecules to be neglected and the retention volumes are independent of the injection sample size.Experiments were carried out repeatedly (and reproducibly) at different temperatures. Retention data of the test solutes were collected between 303 and 373 K.


## 3.1. Synthesis of Tosylated Poly(ethylene glycol)

Polyethylene glycol 400 for synthesis (HO(CH2CH2O)nH) (average molecular mass 380–420 g/mol, Tg=-5°C) andp-toluenesulfonyl chloride (99 wt%) were purchased from Merck. PEG-Tos was synthesized via the tosylation of the corresponding PEG withp-toluenesulfonyl chloride in a two-phase system containing THF/water: 8/3 v/v in the presence of NaOH (in Scheme 1). The detailed procedure can be described as follows. An amount of 0.0936 mol of PEG-400 and an amount of 25 mL of THF were introduced in a 250 mL, round-bottom flask possessing a magnetic stirrer. NaOH, 0.1398 mol, dissolved in 30 mL of water was introduced into the flask, and the system was mixed for a few minutes in a salt-ice bath around −5°C until a white emulsion was formed. Tosyl chloride (TosCl) was divided into two parts, and the first 0.02885 mol of TosCl dissolved in 30 mL of THF was added dropwise within 1 h, and another 0.06688 mol of TosCl (total 0.09573 mol) dissolved in 25 mL of THF was added within another 1 h also dropwise with intensive stirring. The reaction was continued for 4 h at −5°C, after which the reaction temperature was raised up to room temperature and kept at that temperature for 18 h. After reaction, 100 mL of diethyl ether was added, and then two layers were formed. The water layer was extracted three times with diethyl ether (30 mL each time), and the entire diethyl ether phase was washed with water a few times until being neutral (pH = 7). The diethyl ether solution was dried by passing through an anhydrous Na2SO4 (30 g) column until a clear diethyl ether solution was obtained. The diethyl ether was removed with a rotary evaporator. The synthesized PEG-Tos was a transparent liquid. The yield was about 80 wt%. 1HNMR and Fourier transform infrared (FTIR) measurements on an attenuated total reflection accessory (ATR) were carried out on a 500 MHz INOVA-500 and a Perkin Elmer FTIR-ATR, respectively.Scheme 1
Synthesis of PEG-Tos.


## 3.2. Inverse Gas Chromatography Measurements

Studied solvents such as n-hexane (Hx), n-heptane (Hp), n-octane (O), n-nonane (N), n-decane (D), dichloromethane (DCM), chloroform (Ch), acetone (Ac), tetrahydrofuran (THF), and ethyl acetate (EA) were also taken from Merck. They were HPLC grade at 99% purity in molecular sieve and used without further purification. The support materials being Chromosorb W (AW-DMCS-treated, 80/100 mesh) were supplied from Merck. Silane treated glass wool used to plug the ends of the column was obtained from Alltech Associates, Inc.A Hewlett-Packard 6890 Model gas chromatograph with a thermal conductivity detector was used to measure the retention time of the solvents in this study. The column was stainless steel tubing with 3.2 mm o.d. and 0.5 m in length. The PEG and PEG-Tos polymers were coated on the support by slowly evaporation of chloroform as stirring the Chromosorb W in the polymer solution. The amount of coated polymer on the support was determined as 10% by calcination. Trace amount of solvent was injected into the chromatograph. Small volumes of vapor probes were injected manually to achieve the infinite dilution conditions. The column was conditioned at 393 K for 24 h under helium atmosphere at flow rate 30 cm3/min. Zero coverage conditions were reached by injecting 5 μL of vapors of the different probes. In these conditions the interactions between adsorbate molecules themselves are negligible and the thermodynamic parameters, calculated using the retention time of each probe, depend only on the adsorbate/adsorbent interactions. In the case of IGC measurement at infinite dilution, minor amounts of vapors of the test solutes are injected into the column filled with polymer, permitting the lateral interactions between the adsorbed molecules to be neglected and the retention volumes are independent of the injection sample size.Experiments were carried out repeatedly (and reproducibly) at different temperatures. Retention data of the test solutes were collected between 303 and 373 K.


## 4. Results and Discussion

### 4.1. Characterization of PEG-Tos

The aim of tosylation of PEG was to obtain PEG with active end group to synthesize water soluble block copolymer. For this purpose, tosylated PEG was synthesized (Scheme1) and examined by FTIR-ATR (Figure 1) and 1HNMR (Figure 2).Figure 1
FTIR-ATR spectrum of PEG-Tos and PEG.Figure 2
1HNMR spectrum of PEG-Tos in deuterated chloroform.In the FTIR-ATR spectra of PEG and PEG-Tos presented in Figure1, the characteristic absorption peak at about 3500 cm−1, due to the hydroxide end group of PEG, did not disappear in the spectrum of PEG-Tos and new peaks at 1735, 1597, 1189, and 773 cm−1 emerged after tosylation, which could be assigned to the stretching vibrations of the substituting phenyl hydrogen, of –COO in –SOOOC and of –SOOO in PEG-Tos, respectively. This indicates that the tosyl was connected to the PEG end generating the PEG tosylate.Furthermore, the1HNMR spectra of PEG-Tos revealed a hydroxide group capped with tosylate (see Figure 2). The signal due to the oxymethylene connected with tosylate was shifted to 4.05 ppm (2H, peak d), whereas the signal due to the oxymethylene, which was connected to the hydroxide end group of PEG before substitution, was located at 3.80 ppm. The other signals that appeared at 7.70, 7.22 ppm, and 2.4 ppm could be assigned to the phenyl hydrogen (4H, peaks b and c) and methyl hydrogen (3H, peak a) of the tosylate moiety.


### 4.2. Surface Characterization of PEG and PEG-Tos via IGC

The net retention volumes,VN, of the nonpolar and polar solvents on the PEG and PEG-Tos were obtained from IGC measurements between 303 and 373 K using (1). The retention diagrams of nonpolar and polar solvents on PEG and PEG-Tos were given in Figures 3(a), 3(b), 4(a), and 4(b), respectively.The retention diagrams,VN, of (a) nonpolar solvents and (b) polar solvents adsorbed onto PEG.
(a)
Nonpolar solvents
(b)
Polar solventsThe retention diagrams,VN, of (a) nonpolar solvents and (b) polar solvents adsorbed onto PEG-Tos.
(a)
Nonpolar solvents
(b)
Polar solventsThe diagrams drawn for PEG and PEG-Tos showed the same trends with increasing temperature.The Fowkes equation (2) [19] was used to determine the dispersive component of the surface-free energy, γSD, over a range of studied temperatures and calculated values of RTln⁡VN were plotted against a(γLD)0.5. An example of the pattern of results obtained was given in Figure 5 for PEG and Figure 6 for PEG-Tos at 303 K.Figure 5
A plot ofRTln⁡VN versus a(γLD)0.5 for nonpolar and polar probes on PEG at 303 K.Figure 6
A plot ofRTln⁡VN versus a(γLD)0.5 for nonpolar and polar probes on PEG-Tos at 303 K.The linearity was obtained by the nonpolar solvents at the studied temperature ranges. The slope (2NγSD) of the linear fit, obtained for each nonpolar solvent plot, gives the dispersive component of the surface-free energy, γSD, at that temperature. The values of γSD at studied temperature ranges belonging to PEG and PEG-Tos were given in Table 1.Table 1
γ
S
D values of PEG and PEG-Tos at studied temperatures calculated by Fowkes method.
T (K)
γ
S
D (PEG) (mJm−2)
γ
S
D (PEG-Tos) (mJm−2)
303
23.11
34.35
313
21.23
29.95
323
20.31
32.01
333
18.56
27.85
343
16.62
28.85
353
15.87
28.80
363
14.67
27.75
373
12.60
28.90TheγSD values of PEG and PEG-Tos at studied temperatures calculated by Fowkes method were decreasing with increasing temperature. Comparison of the data presented in Table 1 showed that γSD is higher for PEG-Tos than PEG. In the literature, the γSD values of PEG (MW=1100000, Tm=73°C) were ranged from 8.57 to 13.70 mJ/m2 between 340 and 400 K in agreement with this study. The γSD values of PEG and PEG-Tos were not so high as PVC 41.50, polypyrroles 106, and PMMA 40 mJ/m2 polymers [22]. This agreement revealed that dispersive surface energy of the PEG did not change with molar mass of PEG due to the fact that PEG was used as surface energy reducing agent in silica and iron oxide surfaces [23] and PEG-Tos can be used in those surfaces instead of PEG.-
Δ
G
A
S of PEG and PEG-Tos were calculated using the difference between the calculated value of RTln⁡VN and that which was derived using (3) of the linear fit of the nonpolar reference line. The straight reference line defined the London dispersive interactions, while the polar probes lied above this line, indicating that acid-base interactions were present.The variation of free energy of specific interactions,-ΔGAS, between PEG and PEG-Tos and polar probes for studied temperatures was given in Table 2.Table 2
The variation of free energy of specific interactions,-ΔGAS (kJmol−1), between PEG and PEG-Tos and polar probes for studied temperatures.
T (K)
DCM
Ch
Ac
THF
EA
PEG
PEG-Tos
PEG
PEG-Tos
PEG
PEG-Tos
PEG
PEG-Tos
PEG
PEG-Tos
303
7.8
14.8
5.2
13.0
5.8
13.4
4.1
11.47
5.3
13.5
313
6.7
14.0
4.9
11.7
4.9
12.7
3.2
10.7
4.6
12.4
323
7.9
13.2
6.5
10.8
6.2
12.0
4.9
9.9
6.1
11.4
333
6.8
14.1
5.6
12.3
5.2
13.0
3.9
11.4
4.9
12.3
343
6.0
13.3
4.8
11.6
4.5
12.3
3.2
10.7
4.2
11.4
353
5.3
12.4
4.1
10.6
3.9
11.5
2.7
9.9
3.5
10.4
363
4.8
11.7
3.4
9.8
3.5
10.8
2.2
9.2
3.0
9.3
373
5.9
11.1
5.0
9.1
4.7
9.8
3.7
8.5
4.4
8.4By plotting the values of-ΔGAS/T against 1/T, the adsorption enthalpy, ΔHAS, and the adsorption entropy, ΔSAS, of PEG and PEG-Tos were determined for each studied polar probe and the results belonging to PEG and PEG-Tos were given in Table 3.Table 3
Values of the enthalpy,ΔHAS, and entropy, ΔSAS, of adsorption on PEG and PEG-Tos for the polar probes.
Probes
-
Δ
H
A
S (kJmol−1)
Δ
S
A
S
⋅
10
3 (kJmol−1K−1)
PEG
PEG-Tos
PEG
PEG-Tos
DCM
19.4
29.4
38.4
47.2
Ch
11.4
24.8
19.0
40.5
Ac
13.7
26.3
26.3
42.5
THF
9.6
21.1
18.1
32.2
EA
13.6
32.8
26.9
40.5TheΔGAS values of polar solvents on PEG and PEG-Tos were affected as decreasing with increasing temperature. The studied polar solvents showed exothermic heat (Table 3) and positive entropy (Table 3) of sorption which was responsible for their exothermic-free energy of sorption (Table 2). The strength of the interaction between solvents and polymer was proved via the values of ΔHAS.The values ofKA and KD were calculated using (4). The plot of  -ΔHAS/AN* versus DN/AN* was given KA as the slope and KD as the intercept (Figures 7 and 8 for PEG and PEG-Tos, resp.).Figure 7
The plot of-ΔHAS/AN* versus DN/AN* for PEG.Figure 8
The plot of-ΔHAS/AN* versus DN/AN* for PEG-Tos.


## 4.1. Characterization of PEG-Tos

The aim of tosylation of PEG was to obtain PEG with active end group to synthesize water soluble block copolymer. For this purpose, tosylated PEG was synthesized (Scheme1) and examined by FTIR-ATR (Figure 1) and 1HNMR (Figure 2).Figure 1
FTIR-ATR spectrum of PEG-Tos and PEG.Figure 2
1HNMR spectrum of PEG-Tos in deuterated chloroform.In the FTIR-ATR spectra of PEG and PEG-Tos presented in Figure1, the characteristic absorption peak at about 3500 cm−1, due to the hydroxide end group of PEG, did not disappear in the spectrum of PEG-Tos and new peaks at 1735, 1597, 1189, and 773 cm−1 emerged after tosylation, which could be assigned to the stretching vibrations of the substituting phenyl hydrogen, of –COO in –SOOOC and of –SOOO in PEG-Tos, respectively. This indicates that the tosyl was connected to the PEG end generating the PEG tosylate.Furthermore, the1HNMR spectra of PEG-Tos revealed a hydroxide group capped with tosylate (see Figure 2). The signal due to the oxymethylene connected with tosylate was shifted to 4.05 ppm (2H, peak d), whereas the signal due to the oxymethylene, which was connected to the hydroxide end group of PEG before substitution, was located at 3.80 ppm. The other signals that appeared at 7.70, 7.22 ppm, and 2.4 ppm could be assigned to the phenyl hydrogen (4H, peaks b and c) and methyl hydrogen (3H, peak a) of the tosylate moiety.


## 4.2. Surface Characterization of PEG and PEG-Tos via IGC

The net retention volumes,VN, of the nonpolar and polar solvents on the PEG and PEG-Tos were obtained from IGC measurements between 303 and 373 K using (1). The retention diagrams of nonpolar and polar solvents on PEG and PEG-Tos were given in Figures 3(a), 3(b), 4(a), and 4(b), respectively.The retention diagrams,VN, of (a) nonpolar solvents and (b) polar solvents adsorbed onto PEG.
(a)
Nonpolar solvents
(b)
Polar solventsThe retention diagrams,VN, of (a) nonpolar solvents and (b) polar solvents adsorbed onto PEG-Tos.
(a)
Nonpolar solvents
(b)
Polar solventsThe diagrams drawn for PEG and PEG-Tos showed the same trends with increasing temperature.The Fowkes equation (2) [19] was used to determine the dispersive component of the surface-free energy, γSD, over a range of studied temperatures and calculated values of RTln⁡VN were plotted against a(γLD)0.5. An example of the pattern of results obtained was given in Figure 5 for PEG and Figure 6 for PEG-Tos at 303 K.Figure 5
A plot ofRTln⁡VN versus a(γLD)0.5 for nonpolar and polar probes on PEG at 303 K.Figure 6
A plot ofRTln⁡VN versus a(γLD)0.5 for nonpolar and polar probes on PEG-Tos at 303 K.The linearity was obtained by the nonpolar solvents at the studied temperature ranges. The slope (2NγSD) of the linear fit, obtained for each nonpolar solvent plot, gives the dispersive component of the surface-free energy, γSD, at that temperature. The values of γSD at studied temperature ranges belonging to PEG and PEG-Tos were given in Table 1.Table 1
γ
S
D values of PEG and PEG-Tos at studied temperatures calculated by Fowkes method.
T (K)
γ
S
D (PEG) (mJm−2)
γ
S
D (PEG-Tos) (mJm−2)
303
23.11
34.35
313
21.23
29.95
323
20.31
32.01
333
18.56
27.85
343
16.62
28.85
353
15.87
28.80
363
14.67
27.75
373
12.60
28.90TheγSD values of PEG and PEG-Tos at studied temperatures calculated by Fowkes method were decreasing with increasing temperature. Comparison of the data presented in Table 1 showed that γSD is higher for PEG-Tos than PEG. In the literature, the γSD values of PEG (MW=1100000, Tm=73°C) were ranged from 8.57 to 13.70 mJ/m2 between 340 and 400 K in agreement with this study. The γSD values of PEG and PEG-Tos were not so high as PVC 41.50, polypyrroles 106, and PMMA 40 mJ/m2 polymers [22]. This agreement revealed that dispersive surface energy of the PEG did not change with molar mass of PEG due to the fact that PEG was used as surface energy reducing agent in silica and iron oxide surfaces [23] and PEG-Tos can be used in those surfaces instead of PEG.-
Δ
G
A
S of PEG and PEG-Tos were calculated using the difference between the calculated value of RTln⁡VN and that which was derived using (3) of the linear fit of the nonpolar reference line. The straight reference line defined the London dispersive interactions, while the polar probes lied above this line, indicating that acid-base interactions were present.The variation of free energy of specific interactions,-ΔGAS, between PEG and PEG-Tos and polar probes for studied temperatures was given in Table 2.Table 2
The variation of free energy of specific interactions,-ΔGAS (kJmol−1), between PEG and PEG-Tos and polar probes for studied temperatures.
T (K)
DCM
Ch
Ac
THF
EA
PEG
PEG-Tos
PEG
PEG-Tos
PEG
PEG-Tos
PEG
PEG-Tos
PEG
PEG-Tos
303
7.8
14.8
5.2
13.0
5.8
13.4
4.1
11.47
5.3
13.5
313
6.7
14.0
4.9
11.7
4.9
12.7
3.2
10.7
4.6
12.4
323
7.9
13.2
6.5
10.8
6.2
12.0
4.9
9.9
6.1
11.4
333
6.8
14.1
5.6
12.3
5.2
13.0
3.9
11.4
4.9
12.3
343
6.0
13.3
4.8
11.6
4.5
12.3
3.2
10.7
4.2
11.4
353
5.3
12.4
4.1
10.6
3.9
11.5
2.7
9.9
3.5
10.4
363
4.8
11.7
3.4
9.8
3.5
10.8
2.2
9.2
3.0
9.3
373
5.9
11.1
5.0
9.1
4.7
9.8
3.7
8.5
4.4
8.4By plotting the values of-ΔGAS/T against 1/T, the adsorption enthalpy, ΔHAS, and the adsorption entropy, ΔSAS, of PEG and PEG-Tos were determined for each studied polar probe and the results belonging to PEG and PEG-Tos were given in Table 3.Table 3
Values of the enthalpy,ΔHAS, and entropy, ΔSAS, of adsorption on PEG and PEG-Tos for the polar probes.
Probes
-
Δ
H
A
S (kJmol−1)
Δ
S
A
S
⋅
10
3 (kJmol−1K−1)
PEG
PEG-Tos
PEG
PEG-Tos
DCM
19.4
29.4
38.4
47.2
Ch
11.4
24.8
19.0
40.5
Ac
13.7
26.3
26.3
42.5
THF
9.6
21.1
18.1
32.2
EA
13.6
32.8
26.9
40.5TheΔGAS values of polar solvents on PEG and PEG-Tos were affected as decreasing with increasing temperature. The studied polar solvents showed exothermic heat (Table 3) and positive entropy (Table 3) of sorption which was responsible for their exothermic-free energy of sorption (Table 2). The strength of the interaction between solvents and polymer was proved via the values of ΔHAS.The values ofKA and KD were calculated using (4). The plot of  -ΔHAS/AN* versus DN/AN* was given KA as the slope and KD as the intercept (Figures 7 and 8 for PEG and PEG-Tos, resp.).Figure 7
The plot of-ΔHAS/AN* versus DN/AN* for PEG.Figure 8
The plot of-ΔHAS/AN* versus DN/AN* for PEG-Tos.


## 5. Conclusions

The tosylated PEG was synthesized successfully according to FTIR-ATR and1HNMR spectrums. The thermodynamic and surface interactions of nonpolar and polar solvents with PEG and PEG-Tos were characterized via IGC. The surface energy values of PEG were ranging from 23.1 to 12.6 mJ/m2 and PEG-Tos from 34.4 to 28.9 mJ/m2 with increasing temperature. The Lewis acid-base constants, KA and KD, were found as follows: KA=0.09 and KD=0.85 for PEG and KA=0.22 and KD=1.61 for PEG-Tos. According to the results, PEG and PEG-Tos presented a Lewis basic character and tosyl moiety increased the surface energy and basic nature of PEG.



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*Source: 402325-2014-12-25.xml*