Journal of Thermodynamics
Volume 2015 (2015), Article ID 782138, 7 pages
http://dx.doi.org/10.1155/2015/782138

Research Article

Volumetric Behavior of Binary Mixtures of Alkoxyethanols and Some Selected Amines at 298.15 K

Ayasen Jermaine Kemeakegha,¹ Grace Agbizu Cookey,² and Welford-Abbey Lolo Izonfuo¹

¹Department of Chemical Sciences, Niger Delta University, Wilberforce Island, PMB 71, Yenagoa, Bayelsa State, Nigeria
²Department of Chemistry, Rivers State University of Science & Technology, PMB 5080, Port Harcourt, Rivers State, Nigeria

Received 23 September 2014; Revised 9 January 2015; Accepted 9 January 2015

Academic Editor: Felix Sharipov

Copyright © 2015 Ayasen Jermaine Kemeakegha et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract.

Densities of binary mixtures of 2-methoxyethanol (2-MeO-EtOH) and 2-ethoxyethanol (2-EtO-EtOH) with hexylamine (HLA), diethylamine (DEA), triethylamine (TEA), tert-butylamine (TBA), aniline (ANL), and benzylamine (BLA) have been determined at varying compositions of the alkoxyalkanols at 298.15 K. The excess molar volumes, VE, of the binary mixtures were calculated from the experimental density data of the mixtures and the component single solvents. The calculated excess molar volumes were fitted into the Redlich-Kister polynomial to obtain the fitting coefficients and standard deviations. The excess molar volumes of the binary mixtures of all the solvent systems investigated were negative over the entire range of the solvents composition. The negative values were attributed to stronger hydrogen bond formations between the unlike molecules of mixtures than those between the like molecules of the pure components. The magnitude of the excess molar volumes of the binary mixtures of 2-methoxyethanol and the aliphatic amines were in the order TBA > TEA > DEA > HEA. For the two aromatic amines, the magnitudes were in the order BLA > ANL. For binary mixtures of the amines and 2-ethoxyethanol, the magnitudes were in the order DEA > TEA > TBA > HEA at compositions where the mole fraction of 2-EtO-EtOH was ≤0.5 and TBA > TEA > DEA > HEA above 0.5 mole fraction of 2-EtO-EtOH.

1. Introduction

Studies of excess thermodynamic functions are useful tools in understanding the nature of molecular interactions in binary liquid mixtures [1]. In chemical industry, knowledge of the properties of binary liquid mixtures is essential in designs involving chemical separations, heat transfer, mass transfer, and fluid flow [2–7]. The mixing of two solvents has been reported to result in specific interactions such as hydrogen bonding, dipole–dipole, and charge transfer reactions [5]. Strong and weak interactions between unlike molecules in mixtures lead to deviations from ideality. Deviations from ideality in binary liquid mixtures are usually associated with synergism and are attributed to differences in the chemistry and molecular architecture of the mixing solvents [8–14] as well as the experimental conditions such as temperature and the mixing ratios of the binary liquids.

Alcohols and amines are known for their self-association through intermolecular hydrogen bonding. Amines are very important in various applications. For example, diethylamine is used as a corrosion inhibitor in the production of resins, dyes, rubbers, and pharmaceuticals. tert-Butylamine is an intermediate in the preparation of pesticides, pharmaceuticals, dyes, and other organic compounds [15]. Alcohols are very important solvents in a number of industrial processes and have several applications as reagents or solvents, hand sanitizers, antifreeze, and antiseptics as well as preservatives in science and industry [6]. Some alcohols are bifunctional in nature. Bifunctional alcohols, like alkoxypropanols, have demonstrated excellent cleaning properties as a result of their dual molecular architecture [6]. In general, bifunctional alcohols, like alkoxyethanols, are hydroxyethers which are widely used for various analytical and industrial purposes [16–21].

A survey of the literature reveals several studies on the excess properties of binary organic solvent mixtures including amines and bifunctional alcohols [22–31]. For example, Pal and Kumar have reported the excess molar volumes and viscosity deviations of binary liquid mixtures of [2-(2-butoxyethoxy) ethanol] and [2-(2-ethoxyethoxy) ethanol] with 1-propanol at different temperatures [15]. Viscosities of binary liquid mixtures of 2-(2-methoxyethoxy) ethanol, 2-(2-ethoxyethoxy) ethanol, and 2-(2-butoxyethoxy) ethanol with methyl, ethyl, and propylacetates at various temperatures have also been reported by the same authors [16]. A number of workers have also reported their findings on studies conducted on mixtures of several other bifunctional systems [15–34]. For example, Holgado et al. [35] have reported the excess molar volumes and viscosity deviations of binary mixtures of 2-methoxyethanol and 2-butanone at different temperatures. The literature is however scanty on studies regarding binary mixtures of 2-alkoxyethanols with the named amines. This study is therefore aimed at providing mixing data in terms of the excess molar volumes of binary mixtures of 2-alkoxyethanols with tert-butylamine, hexylamine, diethylamine, triethylamine, aniline, and benzylamine. 2-Methoxyethanol and 2-ethoxyethanol were used as the alkoxyethanols to see the effect of the chain length of the alkoxy group on the excess molar volumes of the binary solvent systems. The excess molar volume data obtained from the measured densities of the binary mixtures at 298.15 K over the entire range of solvents composition have been used to interpret the types and strengths of intermolecular interactions in the binary mixtures of the solvent systems investigated. Our findings on the volumetric behavior of these binary mixtures are reported hereunder.

2. Experimental

2.1. Materials

Hexylamine, diethylamine, and triethylamine of analytical grade were products of Merck, Germany. 2-Methoxyethanol (96%) was a product of Kanto Chemicals, Japan. 2-Ethoxyethanol (95% pure) and benzylamine (99% pure) were from BDH Chemicals, England, UK. tert-Butylamine (98% pure) was from Riedel-De Haenag Seelze-Hannover and aniline (99% pure) was from May and Baker, England. All the solvents were dried using molecular sieves and the pure solvents were recovered via distillation.

2.2. Measurements

Binary mixtures of the pure solvents were prepared by weight. The exact volumes of the cosolvents were calculated from their densities at 298.15 K and mixed. The compositions of the binary mixtures ranged from 0.0004 to 0.9998 mole fraction of the 2-alkoxyethanols. All weighings were done using a Sartorius Analytical Balance with a precision of ±10⁻⁴. The densities of the pure solvents and binary mixtures were determined with a 10 mL capacity single stem capillary pyknometer at the working temperature of (298.15 ± 0.01) K. The pyknometer was calibrated with doubly distilled water at atmospheric pressure and at the working temperature. The accuracy of the density measurements was estimated to be ±1 × 10⁻⁵ g cm⁻³. The calculated densities of the pure solvents at 298.15 K are shown in Table 1 and are comparable to values obtained in the literature [36–38].

Table 1: Densities, ρ (g/cm³), of pure solvents at 298.15 K.

Solvent
Acronym
Experimental
Literature

Aniline
ANL
1.0165
1.0175

Benzylamine
BLA
0.9896
0.9943

Hexylamine
HLA
0.7611
0.7620a

Diethylamine
DEA
0.7017
0.7016a, 0.6926b

Triethylamine
TEA
0.7201
0.7230a, 0.7235b

tert-Butylamine
TBA
0.6893
0.6908

2-Methoxyethanol
2-MeO-EtOH
0.9604
0.96028a, 0.96024b

2-Ethoxyethanol
2-EtO-EtOH
0.9256
0.92520a, 0.92515c

aReferences [23], b[21], and c[22].

3. Results and Discussion

The excess molar volumes, , of the binary mixtures were calculated from the measured density data using

In (1), and are the mole fractions of the alkoxyethanols and amines, respectively. , , and are the respective molar volumes of the binary mixtures and the single component solvents. was obtained from

In (2), is the density of the mixture, calculated from the experimental density data, and is the molar mass of the mixture calculated from (3) where and are the molar masses of the pure components

The densities and calculated excess molar volumes of the binary mixtures at the various mole fractions of 2-MeO-EtOH and 2-EtO-EtOH are listed in Tables 2 and 3 and shown in Figures 1 and 2, respectively.

Table 2: Densities, ρ (g/cm³), and excess molar volumes, (cm³/mol), of binary mixtures of 2-MeO-EtOH with named amines at 298.15 K.

(2MeOEtOH)
Aniline
Benzylamine
Hexylamine

ρ (g/cm³)
(cm³/mol)
ρ (g/cm³)
(cm³/mol)
ρ (g/cm³)
(cm³/mol)

0.0004
1.0165

0.9896

0.7611

0.1004
1.0168

0.9888

0.7624

0.1988
1.0175

0.9893

0.7638

0.3008
1.0178

0.9898

0.7649

0.3958
1.0180

0.9903

0.7656

0.4978
1.0179

0.9906

0.7659

0.5996
1.0177

0.9908

0.7658

0.6981
1.0173

0.9907

0.7653

0.7999
1.0168

0.9903

0.7642

0.8984
1.0164

0.9895

0.8268

0.9998
0.9604

0.9604

0.9604

(2MeOEtOH)
Diethylamine
Triethylamine
tert-Butylamine

ρ (g/cm³)
(cm³/mol)
ρ (g/cm³)
(cm³/mol)
ρ (g/cm³)
(cm³/mol)

0.0004
0.7017

0.7201

0.6893

0.1004
0.7081

0.7175

0.6957

0.1988
0.7141

0.7226

0.7018

0.3008
0.7181

0.7259

0.7062

0.3958
0.7206

0.7284

0.7096

0.4978
0.7212

0.7293

0.7105

0.5996
0.7199

0.7286

0.7101

0.6981
0.7174

0.7267

0.7073

0.7999
0.7132

0.7228

0.7025

0.8984
0.8078

0.8183

0.7957

0.9998
0.9604

0.9604

0.9604

Table 3: Densities, ρ (g/cm³), and excess molar volumes, (cm³/mol), of binary mixtures of 2-EtO-EtOH with named amines at 298.15 K.

(2EtOEtOH)
Aniline
Benzylamine
Hexylamine

ρ (g/cm³)
(cm³/mol)
ρ (g/cm³)
(cm³/mol)
ρ (g/cm³)
(cm³/mol)

0.0004
1.0165

0.9896

0.7611

0.1004
1.0177

0.9904

0.7617

0.1988
1.0188

0.9919

0.7623

0.3008
1.0199

0.9931

0.7626

0.3958
1.0206

0.9940

0.7628

0.4978
1.0211

0.9944

0.7628

0.5996
1.0211

0.9946

0.7626

0.6981
1.0207

0.9938

0.7623

0.7999
1.0199

0.9926

0.7619

0.8984
1.0184

0.9908

0.7614

0.9998
0.9256

0.9256

0.9256

(2EtOEtOH)
Diethylamine
Triethylamine
tert-Butylamine

ρ (g/cm³)
(cm³/mol)
ρ (g/cm³)
(cm³/mol)
ρ (g/cm³)
(cm³/mol)

0.0004
0.7017

0.7201

0.6893

0.1004
0.7079

0.7257

0.6938

0.1988
0.7139

0.7297

0.6983

0.3008
0.7175

0.7326

0.7020

0.3958
0.7189

0.7340

0.7039

0.4978
0.7187

0.7345

0.7046

0.5996
0.7169

0.7337

0.7041

0.6981
0.7138

0.7319

0.7019

0.7999
0.7099

0.7285

0.7785

0.8984
0.8055

0.8247

0.7938

0.9998
0.9256

0.9256

0.9256

Figure 1: Plots of excess molar volumes () versus mole fraction of 2-MeO-EtOH at 298.15 K for the binary mixtures of 2-MeO-EtOH with ANL (1), BLA (2), HEA (3), DEA (4), TEA (5), and TBA (6).

Figure 2: Plots of excess molar volumes () versus mole fraction of 2-EtO-EtOH at 298.15 K for the binary mixtures of 2-EtO-EtOH with ANL (1), BLA (2), HEA (3), DEA (4), TEA (5), and TBA (6).

The values of the calculated excess molar volumes, , of the binary mixtures were fitted into the Redlich-Kister polynomial (4) and the fitting coefficients, , were evaluated by the method of least squares

In (4), is the number of fitting coefficients and the other parameters are as defined earlier.

With the values of , and the total number of experimental data points, , the standard deviations, , of the excess molar volumes, , were calculated using (5)

The values of the fitting coefficients and the standard deviations of the excess molar volumes of the various mixtures of 2-MeO-EtOH + amines and 2-EtO-EtOH + amines are shown in Tables 4 and 5, respectively.

Table 4: Fitting coefficients and standard deviations of binary mixtures of 2-MeO-EtOH and amines at 298.15 K.

Binary mixtures

Hexylamine (/cm³mol⁻¹)

Diethylamine (/cm³mol⁻¹)

Triethylamine (/cm³mol⁻¹)

tert-Butylamine (/cm³mol⁻¹)

Aniline (/cm³mol⁻¹)

Benzylamine (/cm³mol⁻¹)

Table 5: Fitting coefficients and standard deviations of binary mixtures of 2-EtO-EtOH and amines at 298.15 K.

Binary mixtures (/cm³mol⁻¹)

Hexylamine (/cm³mol⁻¹)

Diethylamine (/cm³mol⁻¹)

Triethylamine (/cm³mol⁻¹)

tert-Butylamine (/cm³mol⁻¹)

Aniline (/cm³mol⁻¹)

Benzylamine (/cm³mol⁻¹)

4. Excess Molar Volumes, , of Binary Mixtures of 2-Alkoxyethanols and the Named Amines

The excess molar volumes, , of the binary mixtures investigated in the study were all negative over the entire range of solvents composition at 298.15 K. These are shown in Tables 2 and 3 and Figures 1 and 2. Plots of the excess molar volumes as a function of mole fraction of the alkoxyethanols in the binary mixtures show minima in the mole fraction range of 0.45–0.55 of the alkoxyethanols. In the binary mixtures of 2-methoxyethanol and the named amines, the minimum occurs at 0.50 for DEA and TEA; 0.45 for HEA and ANL; 0.55 for TBA; and 0.60 for BLA. These values compare with the values of 0.50 and 0.60 in binary mixtures of 2-methoxyethanol with DEA and TEA, respectively, reported by Kinart et al. [39]. The negative excess molar volumes, , are attributable mainly to the association between the named amines and 2-methoxyethanol through intermolecular hydrogen bonds between the –OH groups in 2-methoxyethanol and the nitrogen atoms in the amines. The magnitudes of the negative excess molar volumes were in the order TBA > TEA > DEA > HEA for the binary mixtures with the aliphatic amines while the magnitudes were in the order BLA > ANL for the binary mixtures with the aromatic amines. The strength of the associations arising from the interactions between the unlike molecules was stronger than the strength of the associations between like molecules. Large negative excess molar volumes, , for binary mixtures of alkyl amines and alcohols have also been reported by other workers [40]. It has been suggested that the large negative values are due to heteroassociation of unlike molecules which give rise to formation of cross complexes where O–H–N bonds of the mixtures are stronger than O–H–O and N–H–N bonds of the single component solvents. It is generally known that alkyl groups are electron donating. This ability increases with chain length and branching. This suggests that the nitrogen atom in the amines is electron enriched to different degrees depending upon the chain length and degree of branching of the alkyl groups attached to the nitrogen atom in the amines. The degree of electron enrichment of the nitrogen atom in the amines therefore affects the N–H dipole in the amines. The strength of the O–H–N bonds in the mixtures is thus dependent upon the degree of electron enrichment of the nitrogen atom of the amines. The magnitudes of excess molar volumes of binary mixtures of 2-methoxyethanol and the two aromatic amines are least compared to those of the mixtures with aliphatic amines. Aromatic rings attract electrons and are weakly basic. The interactions of aniline and benzylamine with 2-methoxyethanol thus result in small negative values. Since the direct attachment of –NH₂ group to a carbon atom of an aromatic ring reduces the basic strength of the NH₂ group, the magnitudes of values for the mixtures of ANL with 2-methoxyethanol are smaller than those of BLA mixtures. Another effect that could account for the negative excess molar volumes of binary mixtures of 2-methoxyethanol and the named amines is the difference in the molecular volumes between 2-methoxyethanol and the named amines. 2-Methoxyethanol has molecular volume of 1.31 × 10⁻²² cm³. The molecular volumes of aniline, benzylamine, hexylamine, diethylamine, triethylamine, and tert-butylamine are 1.35 × 10⁻²² cm³, 1.79 × 10⁻²² cm³, 2.20 × 10⁻²² cm³, 1.74 × 10⁻²² cm³, 2.33 × 10⁻²² cm³, and 1.76 × 10⁻²² cm³, respectively. The molecular volume of 2-MeO-EtOH is smaller than the molecular volume of all the amines. This situation can therefore result in the fitting of smaller 2-MeO-EtOH molecules into the amines and result in the negative excess volumes. The molecular volume of TEA is much greater than that of DEA. More molecules of 2-MeO-EtOH can therefore fit into TEA than into DEA. The more negative excess molar volumes in binary mixtures of 2-MeO-EtOH + TEA than in binary mixtures of 2-MeO-EtOH + DEA are therefore in line with the molecular volume differences between TEA and DEA. Our results in this regard are at variance with those of Kinart et al. [39], who reported that the excess molar volumes of binary mixtures of 2-methoxyethanol + DEA were more negative than those in binary mixtures of 2-methoxyethanol + TEA. The excess molar volumes, , of binary mixtures of 2-ethoxyethanol and the named amines at 298.15 K were also negative over the entire range of solvents composition. Plots of the excess molar volumes as a function of mole fraction of 2-ethoxyethanol show minima in the mole fraction range of 0.400.55. The minima for DEA and TEA occur at the mole fractions of 0.45 and 0.50, respectively, in these solvent systems. The excess molar volumes of the binary mixtures of 2-ethoxyethanol and the named aliphatic amines were less negative than those in the binary mixtures of 2-methoxyethanol and the named aliphatic amines. The excess molar volumes of binary mixtures of 2-ethoxyethanol and the named aromatic amines were more negative than the values in mixtures of 2-methoxyethanol and the named aromatic amines. As stated earlier, alkoxyethanols are associated via inter- and intramolecular hydrogen bonding. The values of the excess molar volumes, , are reported to become more negative when the alkyl chain length of the alkoxyethanol increases [41]. Our results however suggest that other factors, such as the differences in the molecular sizes of the component molecules, also play a role in the mixing behavior of the component solvents. The magnitudes of the excess molar volumes of binary mixtures of 2-ethoxyethanol and the named aliphatic amines are in the order DEA > TEA > TBA > HEA in the mole fraction range ≤0.50 2-EtO-EtOH. At mole fractions of 2-EtO-EtOH >0.50, the order of magnitudes is TBA > TEA > DEA > HEA. This trend suggests that steric hindrance dominates over specific interactions at lower concentrations of 2-EtO-EtOH. DEA, being the least bulky branched amine, therefore has strongest interaction with 2-EtO-EtOH. Interstitial fittings of smaller molecules into molecules with larger molecular volumes have also been reported in binary mixtures of ethylacetoacetate and (C₄–C₆) aliphatic ketones by Izonfuo and Kemeakegha [42], for binary mixtures of -methylpyrrolidone with (C₁–C₁₀) alkan-1-ols [43], formamide and ethanol mixtures [44, 45], and dimethylsulfoxide and alcohols [46–48]. In the binary mixed solvents with compositions above 0.50 mole fraction of 2-ethoxyethanol, intermolecular hydrogen bonding between unlike molecules predominates and the trend is similar to that in the binary mixtures of 2-methoxyethanol with the named amines. The order of magnitude of the negative excess molar volumes of mixtures of 2-EtO-EtOH + the aromatic amines follows the same trend as those in 2-MeO-EtOH + amine mixtures. In general, the magnitudes of the negative excess molar volumes of mixtures of 2-MeO-EtOH with the amines are larger than those of 2-EtO-EtOH mixtures. The increased chain length of the ethyl group in 2-EtO-EtOH may have created additional steric hindrance in 2-EtO-EtOH mixtures resulting in relative volume expansion compared to that of the methyl group in 2-methoxyethanol.

5. Conclusions

Volumetric properties of binary mixtures of 2-methoxyethanol and 2-ethoxyethanol with hexylamine, diethylamine, triethylamine, tert-butylamine, aniline, and benzylamine have been studied at 298.15 K. The results confirm what has been previously reported that, in the solvent systems investigated, the excess molar volumes are negative throughout the entire range of solvents composition. The negative excess molar volumes are attributable to stronger hydrogen bond formations between unlike molecules than those between like molecules. Interstitial fitting of molecules of smaller molecular volumes into molecules of larger molecular volume also account for the negative excess molar volumes of the solvent systems. The relative magnitudes of the negative excess volumes suggest that the excess molar volumes tend to become less negative as the chain length of the alkoxy group increases, which may be due to increased steric hindrance.

Conflict of Interests

The authors declare that there is no conflict of interests regarding the publication of this paper.

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