Dielectric Constants of Aqueous Diisopropanolamine, Diethanolamine, N-Methyldiethanolamine, Triethanolamine, and 2-Amino-2-methyl-1-propanol Solutions

Abstract

Dielectric constants of aqueous diisopropanolamine, diethanolamine, N-methyldiethanolamine, triethanolamine, and 2-amino-2-methyl-1-propanol solutions for temperatures of (303.15 to 328.15) K were measured using a dielectric analyzer. The dielectric constants of the corresponding pure alkanolamines were also measured for the same temperature range. The measured dielectric constants of diethanolamine and propylene glycol were found to be in good agreement with literature values. The relation between the dielectric constant of alkanolamines and the concentration of the hydroxyl groups per unit volume was discussed. The Kirkwood relation was also applied to represent the temperature dependence of dielectric constants of alkanolamines, and the apparent dipole moments were obtained from the measured data. The dielectric constants of aqueous alkanolamine solutions were correlated satisfactorily by using a Redlich-Kister type equation, and the positions of the relative minimum in the plot of ∆ versus x 1 for aqueous alkanolamine solutions were presented. The compositions of the potential complexes formed from alkanolamines and water molecules were discussed.

In Situ Determination of Metastable Zone Width Using Dielectric Constant Measurement

“…The trends shown in Figure 2 are similar to those of many solution systems reported in the literature. [21][22][23] The correlations between both concentration and temperature with the dielectric constant obtained from this homogeneous condition help to interpret the more complex physical behavior of the paracetamol-ethanol solutions observed from the dielectric constant profiles during crystallization processes.…”

Solubility of H2S in Aqueous Diisopropanolamine + Piperazine Solutions: New Experimental Data and Modeling with the Electrolyte Cubic Square-Well Equation of State

“…where D s is the dielectric constant of pure solvent s. The dielectric constants for the pure solvents were taken from the literature. 5,6,13 The Born 14 contribution to the molar residual Helmholtz energy is written as…”

Effects of Polarity and Hydrogen Bonding on Physical Properties and Ion Dissociation in 1-Ethyl-3-methylimidazolium Ionic Liquid + Non-aqueous Solvent Systems

“…They were chosen because they offer a range of anion polarities and structures. EG, TEA, and Gly were selected based on their structures containing two, three, and three hydroxyl (−OH) groups, respectively, their polarity [dielectric constant (ε) values of 41.2, 28.1, and 42.5, respectively], and their range of viscosities (16.8, 610, and 910 mPa·s, respectively). In addition to the measurements required to calculate ion dissociation (density, viscosity, and ionic conductivity), we measure the excess enthalpies for mixing each IL/solvent combination to elucidate the relationship between enthalpies of mixing and ion dissociation.…”