Thermodynamics of the acetic acid-triethylamine system

Köhler, Friedrich; Liebermann, E.; Miksch, G.; Kainz, Christina

doi:10.1021/j100663a025

Cited by 54 publications

(51 citation statements)

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“…This was also theoretically predicted by ab initio calculations for the trimethylamine-formic acid and propylamine-propionic acid systems [22,30]. The ionic nature of the complexes was confirmed by both mid and near infrared spectroscopy [20,21,[24][25], FT-Raman [17], 1 H-NMR and 13 C-NMR [15,31], dielectric spectroscopy, conductivity measurements [18,23], melting and boiling point measurements, ultrasound absorption and relaxation spectroscopy [12,24,[32][33], and combinations of different measurement techniques including density, optical refractive index, and shear viscosity [23].…”

Section: Introductionsupporting

confidence: 67%

“…The formation of the A 1 C 3 complex in triethylamine-acetic acid mixtures is supported by the sharp viscosity maximum observed at the 1:3 amine to acid mole ratio [16]. The existence of an A 1 C 2 complex has also been reported [12,18,[23][24]. When the tertiary amine is replaced with a secondary or a primary amine the situation changes dramatically.…”

Section: Introductionmentioning

confidence: 81%

“…The interactions between amines (A) and carboxylic acids (C) have been comprehensively studied [12][13][14][15][16][17][18]. Amines and carboxylic acid mixtures interact strongly via hydrogen bonding [12,15].…”

Section: Introductionmentioning

confidence: 99%

“…Amines and carboxylic acid mixtures interact strongly via hydrogen bonding [12,15]. In 1:1 mixtures they form A 1 C 1 molecular complexes in the vapor phase [19][20][21][22][23][24][25][26][27][28][29][30] or ionic complexes in the liquid phase via Brønsted-Lowry acid-base reactions [17].…”

Section: Introductionmentioning

confidence: 99%

“…The A 1 C 1 ionic complex requires stabilization and ab initio calculations showed that, at equimolar mixing ratios, the formation of an A 2 C 2 complex is more likely [17]. In the absence of water and in the presence of excess carboxylic acid, the A 1 C 1 complex is stabilized by reacting with the cyclic dimers of the carboxylic acid forming the A 1 C 3 complex [12,17,18,[21][22][23][24]. The formation of the A 1 C 3 complex in triethylamine-acetic acid mixtures is supported by the sharp viscosity maximum observed at the 1:3 amine to acid mole ratio [16].…”

Section: Introductionmentioning

confidence: 99%

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TGA–FTIR study of the vapors released by triethylamine–acetic acid mixtures

2012

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Proprietary mixtures of amines and carboxylic acids are used as volatile corrosion inhibitors (VCIs) for the protection of iron and steel components against atmospheric corrosion. This study was focused on the nature of the vapors they release. VCI model compounds comprising mixtures of triethylamine and acetic acid were studied using thermogravimetric analysis coupled with Fourier-transform infrared spectroscopy (TGA-FTIR) at 50°C. As vaporization progressed, the composition of the remaining liquid and the emitted vapor con v erged to a f i xed ami ne con ten t of ca. 27 m ol e percen t. Thi s was j ust ab ov e th e composition expected for the 1:3 amine to carboxylic acid complex. Mixtures close to this composition also featured the lowest volatility.

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Section: Introductionsupporting

confidence: 67%

Section: Introductionmentioning

confidence: 81%

Section: Introductionmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

Section: Introductionmentioning

confidence: 99%

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TGA–FTIR study of the vapors released by triethylamine–acetic acid mixtures

2012

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Cluster diffusion in liquids

Cussler

1980

AIChE Journal

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Diffusion in concentrated, non-ideal liquid solutions may take place not only through motion of single molecules but also through movement of groups of molecules, or "clusters." Analyzing this cluster diffusion leads to predictions that the diffusion coefficient can vary with the square root of the usual activity corrections to diffusion. These predictions seem consistent with experiments, particularly in highly non-ideal solutions. SCOPEThe purpose of this article is to describe diffusion in concentrated liquid solutions. Such solutions are frequently highly non-ideal. The diffusion coefficient D in liquids is often estimated from the equation a In a1 a In x1

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Mixtures with Complex Formation. Melting Curves and Model Calculations

Köhler¹

1978

Ber Bunsenges Phys Chem

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A dystecticum is considered which is caused by complex formation, where evidence of the complex in the liquid state is found by non‐thermodynamic methods. The relation between melting curve, heat of complex formation and heat of melting is derived for this case, assuming that the activities of the components are known. The theory is applied to the systems acetic acid + trifluoroacetic acid and triethylamine + trifluoroacetic acid. Model calculations are reported for carboxylic acid systems; the evaluation of the melting curves is in overall agreement with the association constants used in the model calculations.

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Thermodynamics of the acetic acid-triethylamine system

Abstract: ions and simple N03~anions. This conclusion is in Acknowledgment. S. N. wishes to acknowledge the agreement with previous work1™4'11•12 on this system. award of a Rotary Fellowship.

Cited by 54 publications

References 0 publications

TGA–FTIR study of the vapors released by triethylamine–acetic acid mixtures

TGA–FTIR study of the vapors released by triethylamine–acetic acid mixtures

Cluster diffusion in liquids

Mixtures with Complex Formation. Melting Curves and Model Calculations

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