Activity coefficients of the n‐primary, secondary and tertiary aliphatic amines in aqueous solution

Christie, A. O.; Crisp, D. J.

doi:10.1002/jctb.5010170103

Cited by 51 publications

(17 citation statements)

References 11 publications

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“…According to equation (1), linearity is expected, and 1/(K H RT) can be acquired from the slope. Our measurement of TEA's K H at 298 K is 5.75 ± 0.86 mol L À1 atm À1 , which is in good agreement with literature value of 6.69 mol L À1 atm À1 [Christie and Crisp, 1967]. Also, as seen in Figure 1b, the K H values present strong temperature dependence and increase with decreasing temperatures.…”

Section: Temperature-dependent Henry's Law Constant Of Tea In Pure Watersupporting

confidence: 92%

Effects of temperature, pH, and ionic strength on the Henry's law constant of triethylamine

Leng

Roberts

Zeng

et al. 2015

Geophysical Research Letters

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The Henry's law constants (KH) of triethylamine (TEA) in pure water and in 1‐octanol were measured for the temperatures pertinent to the lower troposphere (278–298 K) using a bubble column system coupled to a Fourier transform infrared spectrometer. The KH values of TEA in water and 1‐octanol at 298 K are 5.75 ± 0.86 mol L−1 atm−1 and 115.62 ± 5.78 mol L−1 atm−1. The KH values display strong dependence on temperature, pH, and ionic strength. The characteristic times for TEA to establish an equilibrium between gas and droplet with a size of 5.6 µm are ~33 s (298 K, pH = 5.6); ~8.9 × 102 s (278 K, pH = 5.6); ~1.3 × 103 s (298 K, pH = 4.0); and 3.6 × 104 s (278 K, pH = 4.0). The evaluation of TEA partitioning between gas phase and condensed phase implies that TEA predominantly resides in rainwater, and TEA loss to organic aerosol is negligible.

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Section: Temperature-dependent Henry's Law Constant Of Tea In Pure Watersupporting

confidence: 92%

Effects of temperature, pH, and ionic strength on the Henry's law constant of triethylamine

Leng

Roberts

Zeng

et al. 2015

Geophysical Research Letters

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“…The Gibbs energies of hydration of amines at 298 K were taken from the literature,37–39 where they had also been determined by measuring a concentration of amine or pyridine in the gas phase over a solution in pure water with a known solute concentration. Under the conditions of those experiments, the degree of ionization of amines due to their basicity (R x H 3− x N + H 2 O = R x H 4− x N + + OH − ) is up to 35%,38 for pyridines – less than 0.1%, and the Gibbs energies of hydration of amines used in calculation were corrected for the ionization process 37, 38. For pyridines, the contribution of ionization is negligible.…”

Section: Resultsmentioning

confidence: 99%

Gibbs energy of cooperative hydrogen‐bonding interactions in aqueous solutions of amines and pyridines

Solomonov

Akhmadiyarov

2009

J of Physical Organic Chem

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A method to determine the Gibbs energy of specific (hydrogen bonding) interactions of a solute with water is proposed. The energies of hydrogen bonding in bulk water are very difficult to determine by any method. The Gibbs energy of hydration of substances forming hydrogen bonds with water is considered as the sum of contributions due to non-specific interactions, the hydrophobic effect, and specific interactions. The first two terms were found to be rather accurately described by empirical equations. The Gibbs energies of hydrogen bonding of aliphatic amines and pyridines in bulk water are determined, and the results are compared with the energies of their complexes with one molecule of water. The cooperativity of hydrogen bonding is proved in aqueous solutions of amines and pyridines. To use our equations, experimental values of the Gibbs energies of solvation in 'standard' solvents need to be known. The Gibbs energies of solvation of ten amines and pyridines in dimethyl sulfoxide are determined experimentally using chromatographic head space analysis. The tendencies observed for the series of amines and pyridines are in agreement with other studies.

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“…Hydrocarbon chains are generally insoluble, however, in the context of stability of these films in aqueous environments, amine groups provide sites for water molecules to form hydrogen bonds. It is well known that primary amines are highly soluble in water, but increased cross‐linking of nitrogen into secondary and tertiary amines decreases solubility, and would therefore increase film stability. Increasing the length of the hydrocarbon chain to which the amine is attached also decreases solubility .…”

Section: Discussionmentioning

confidence: 99%

Plasma Parameter Aspects in the Fabrication of Stable Amine Functionalized Plasma Polymer Films

Daunton

Smith

Whittle

et al. 2015

Plasma Processes & Polymers

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Amine containing plasma polymer films are of interest due to their ability to bind biomolecules either covalently or electrostatically. One issue with generating such plasma polymers is the need to generate sufficient amine density on the surface to enable binding, while simultaneously maintaining the chemical, physical stability of the surface in aqueous media. Here we investigate the relationship between plasma parameters, film stability for two commonly used monomers, allylamine AA, ethylenediamine EDA. Plasma polymer films from AA, EDA were produced at radio frequency RF powers between 2 and 20 W at a constant monomer flowrate. Deposition rate, ion flux, ion energy, plasma phase mass spectrometry were used to investigate the plasma-surface interactions. Film stability was assessed by comparing X-ray photoelectron spectroscopy XPS, atomic force microscopy AFM measurements before, after washing in phosphate buffered saline PBS. The results show that films generated from EDA plasmas are generally unstable in aqueous media, while films generated from AA plasmas exhibit higher stability, particularly those deposited at high RF power. The chemical, physical stability of the films is then related to the mechanisms of deposition, the energy density provided to the surface during film growth.

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Activity coefficients of the n‐primary, secondary and tertiary aliphatic amines in aqueous solution

Cited by 51 publications

References 11 publications

Effects of temperature, pH, and ionic strength on the Henry's law constant of triethylamine

Effects of temperature, pH, and ionic strength on the Henry's law constant of triethylamine

Gibbs energy of cooperative hydrogen‐bonding interactions in aqueous solutions of amines and pyridines

Plasma Parameter Aspects in the Fabrication of Stable Amine Functionalized Plasma Polymer Films

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