scholarly journals Dielectric and Excess Dielectric Constants of Acetonitrile + Butyl Amine, + Ethylamine, and + Methylamine at 303, 313, and 323 K

2013 ◽  
Vol 2013 ◽  
pp. 1-4 ◽  
Author(s):  
Ch. V. V. Ramana ◽  
A. B. V. Kiran Kumar ◽  
M. Ashok Kumar ◽  
M. K. Moodley
Keyword(s):  
Dielectric Constant ◽  
Intermolecular Interactions ◽  
Mole Fraction ◽  
Entire Range ◽  
Binary Systems ◽  
Mixed Solvents ◽  
Dielectric Constants ◽  
Complete Mole ◽  
Butyl Amine ◽  
Mole Fraction Range

The dielectric constants and excess dielectric constants of the binary systems: acetonitrile + butyl amine, + ethylamine and + methylamine have been studied at 303, 313, and 323 K temperatures and over the complete mole fraction range. The dielectric constants for these mixtures were measured using a microcontroller based system. The results are positive over the entire range of composition. Symmetrical curves were observed for the systems in which the maximum occurs approximately at 0.7-mole fraction of acetonitrile. The results are discussed in terms of intermolecular interactions. The investigation of dielectric constant of mixed solvents bearing amines aims at better comprehension of their biological, chemical, pharmaceutical, technological, and laboratory applications.

Excess properties of the binary liquid systems dimethylsulfoxide + isopropanol and propylene carbonate + isopropanol

1989 ◽  
Vol 67 (6) ◽  
pp. 1105-1108 ◽  
Author(s):  
George Ritzoulis
Keyword(s):  
Dielectric Constant ◽  
Propylene Carbonate ◽  
Binary Systems ◽  
Correlation Factor ◽  
Dielectric Constants ◽  
Excess Properties ◽  
Binary Solvent ◽  
Solvent Mixtures ◽  
Liquid Systems ◽  
Mole Fraction Range

The dielectric constants, viscosities, densities, and refractive indices of the binary solvent mixtures dimethylsulfoxide–isopropanol and propylene carbonate–isopropanol were measured at 25, 30, and 35 °C over the entire mole fraction range. Excess dielectric constant, excess molar polarization, and excess viscosity were calculated. For both binary systems the variation of the Kirkwood correlation factor has been examined. Keywords: propylene carbonate, acetonitrile, correlation factor, excess properties, dielectric constant.

scholarly journals Use of Electron Paramagnetic Resonance Spectroscopy to Study Dielectric Properties of Liquids

2012 ◽  
Vol 2012 ◽  
pp. 1-8 ◽  
Author(s):  
Daniel T. Glatzhofer ◽  
Rahul S. Kadam
Keyword(s):  
Dielectric Constant ◽  
Electron Paramagnetic Resonance Spectroscopy ◽  
Mixed Solvents ◽  
Active Species ◽  
Dielectric Constants ◽  
Resonance Spectroscopy ◽  
Paramagnetic Resonance ◽  
Epr Signal ◽  
Signal Response ◽  
High Dielectric

The signal response of an EPR active species is attenuated by the medium it is in. Keeping all other parameters the same, the higher the dielectric constant of the medium, the lower the EPR signal response. This behavior is problematic in studying EPR active species in high dielectric media but can be capitalized upon to monitor changes in the dielectric constant or estimate the dielectric constant of the medium. Using a coaxial EPR cell design, the EPR signal of a stable nitroxyl radical compound (2,2,6,6-tetramethyl-piperidin-1-oxyl radical) in a low dielectric constant solvent in an inner tube is attenuated by the solvent present between the inner and outer tubes (jacket medium). The attenuation increases monotonically with an increase in the dielectric constant of the jacket medium. Calibration curves can be constructed using jacket media of known dielectric constants ranging from 2 to 80 and the dielectric constant of a sample used as the jacket medium can be estimated by interpolation. This technique is applied to estimate the dielectric constants and/or composition of mixed solvents and to monitor the rate of a reaction.

An ESR Study of Mn(II) Complexes in Water-Methanol Mixed Solvents

1971 ◽  
Vol 26 (11) ◽  
pp. 1091-1096 ◽  
Author(s):  
James R. Bard ◽  
James O. Wear
Keyword(s):  
Aqueous Solution ◽  
Dielectric Constant ◽  
Complex Formation ◽  
Mole Fraction ◽  
Coordination Sphere ◽  
Mixed Solvents ◽  
Solvent Composition ◽  
Significant Feature ◽  
Similar Data ◽  
Methanol Content

0.01 ᴍ solutions of Mn (ClO4)2, MnCl2 and MnSO4 in water-methanol mixtures were studied at 25 °C to determine the effect of these anions and of solvent composition on the ESR intensity and linewidth of Mn(II). A significant feature of the data was the large difference between the intensity of Mn(ClO4)2 and that for MnCl2 and MnSO4 in solutions containing greater than about 0.5 mole fraction methanol. A plot of linewidth versus mole fraction methanol shows little difference between Mn(ClO4)2 and MnCl2 but an increasingly greater difference between these salts and MnSO4 with increasing methanol content. These results are interpreted as being due to first coordination sphere complex formation in solutions containing Cl⊖, while the SO42⊖ data are affected by both first and second coordination sphere complexes depending upon the solvent dielectric constant. The Mn(ClO4)2 data were interpreted as showing that the primary solvation sphere of the Mn(II) ions was changing as the composition of the bulk solvent changed. These results are compared with similar data in aqueous solution and confirm that complex formation involving Cl⊖ or SO42⊖ ions and Mn(II) is extensive in water-methanol mixtures.

THE DIELECTRIC CONSTANTS OF HYDROGEN PEROXIDE-ETHER AND HYDROGEN PEROXIDE-WATER-ETHER MIXTURES

1931 ◽  
Vol 4 (4) ◽  
pp. 322-329 ◽  
Author(s):  
E. P. Linton ◽  
O. Maass
Keyword(s):  
Hydrogen Peroxide ◽  
Dielectric Constant ◽  
Mole Fraction ◽  
Unit Volume ◽  
Dielectric Constants ◽  
Pure Hydrogen ◽  
Water Mixture ◽  
Mixture Rule ◽  
Wide Range ◽  
Molecular Fraction

The dielectric constants of solutions of hydrogen peroxide and of hydrogen peroxide-water mixtures in ether have been determined over a wide range of concentrations. It was shown: (a) that the dielectric constant of hydrogen peroxide in ether is proportional to the amount of hydrogen peroxide per unit volume, and (b) that the variation of the dielectric constant with mole fraction was proportional to the dielectric constant of the solution examined, so that the logarithm of the dielectric constant varies in a linear way with the molecular fraction. By this means the dielectric constant of pure hydrogen peroxide at 0 °C. was found to be 93.7. It has been shown that hydrogen peroxide-water mixture has a higher dielectric constant than either constituent. The densities of ether-hydrogen peroxide solutions were measured and a maximum aberration from the mixture rule found at a 1:1 concentration.

Some thermodynamic and transport properties of lithium salts in mixed aprotic solvents and the effect of water on such properties

1996 ◽  
Vol 74 (2) ◽  
pp. 153-164 ◽  
Author(s):  
Lorraine Couture ◽  
Jacques E. Desnoyers ◽  
Gérald Perron
Keyword(s):  
Phase Diagrams ◽  
Propylene Carbonate ◽  
Binary Systems ◽  
Ion Pairs ◽  
Mixed Solvents ◽  
High Energy ◽  
Heat Capacities ◽  
Dielectric Constants ◽  
Aprotic Solvents ◽  
High Concentration

In a continuing study on the optimization of the electrolyte medium for high-energy lithium batteries, volumes, heat capacities, and specific conductivities of LiClO4 and LiBr were measured in mixtures of γ-butyrolactone (BUTY) and 1,2-dimethoxyethane (DME) and of propylene carbonate (PC) and BUTY. These results are compared with those of the electrolytes in the pure solvents. Phase diagrams are also reported when appropriate. The effect of addition of water to these binary and ternary systems was investigated with the same techniques. The mixtures DME–BUTY, PC–DME, DME–H2O, and BUTY–H2O are typical of mixtures of aprotic solvents and mixtures of aprotic solvents and water. The electrolytes at high concentrations in aprotic solvents of low dielectric constants are largely associated. The medium still conducts electrolytically since the ion pairs are in a state that resembles to a large extent that of a molten salt. With some systems at high concentration, stable solvates persist in the solution medium, as evidenced mostly by heat capacities, and are in equilibrium with either the excess solvent or unsolvated molten salts. In mixed solvents, the properties of electrolytes can largely be predicted from the binary systems and by the coexistence of these solvates. The properties of water in DME, BUTY, or mixtures of the two solvents are modified significantly in the presence of LiBr but only slightly with LiClO4. These specific interactions, which affect the heat capacities much more than the volumes and which are especially large with the system LiBr–DME, could be responsible for the decrease in reactivity of water with lithium metal in an aprotic medium in the presence of certain electrolytes. Key words: LiClO4, LiBr, γ-butyrolactone, dimethoxyethane, propylene carbonate, lithium battery, aprotic solvent, water, association, solvates, solid–liquid phase diagrams, volumes, heat capacities, specific conductivities.

scholarly journals Comment on “investigation of dielectric constants of water in a nano-confined pore” by H. Zhu, F. Yang, Y. Zhu, A. Li, W. He, J. Huang and G. Li, RSC Adv., 2020, 10, 8628

RSC Advances ◽  
2021 ◽  
Vol 11 (9) ◽  
pp. 5179-5181
Author(s):  
Sayantan Mondal ◽  
Biman Bagchi
Keyword(s):  
Dielectric Constant ◽  
Dielectric Constants ◽  
Static Dielectric Constant ◽  
Inherent Anisotropy ◽  
Nanoconfined Water

Neglects of inherent anisotropy and distinct dielectric boundaries may lead to completely erroneous results. We demonstrate that such mistakes can give rise to gross underestimation of the static dielectric constant of cylindrically nanoconfined water.

DIELECTRIC CONSTANT AND SEEBECK COEFFICIENT FOR SEMICONDUCTORS: THERMODYNAMIC AND DFT STUDIES

2013 ◽  
Vol 12 (06) ◽  
pp. 1350057 ◽  
Author(s):  
HSIU-YA TASI ◽  
CHAOYUAN ZHU
Keyword(s):  
Boundary Condition ◽  
Dielectric Constant ◽  
Seebeck Coefficient ◽  
Gas Phase ◽  
Present Method ◽  
Dielectric Constants ◽  
Semiconductor Materials ◽  
Electronic Polarizability ◽  
Seebeck Coefficients ◽  
Good Agreement

Dielectric constants and Seebeck coefficients for semiconductor materials are studied by thermodynamic method plus ab initio quantum density functional theory (DFT). A single molecule which is formed in semiconductor material is treated in gas phase with molecular boundary condition and then electronic polarizability is directly calculated through Mulliken and atomic polar tensor (APT) density charges in the presence of the external electric field. This electronic polarizability can be converted to dielectric constant for solid material through the Clausius–Mossotti formula. Seebeck coefficient is first simulated in gas phase by thermodynamic method and then its value divided by its dielectric constant is regarded as Seebeck coefficient for solid materials. Furthermore, unit cell of semiconductor material is calculated with periodic boundary condition and its solid structure properties such as lattice constant and band gap are obtained. In this way, proper DFT function and basis set are selected to simulate electronic polarizability directly and Seebeck coefficient through chemical potential. Three semiconductor materials Mg 2 Si , β- FeSi 2 and SiGe are extensively tested by DFT method with B3LYP, BLYP and M05 functionals, and dielectric constants simulated by the present method are in good agreement with experimental values. Seebeck coefficients simulated by the present method are in reasonable good agreement with experiments and temperature dependence of Seebeck coefficients basically follows experimental results as well. The present method works much better than the conventional energy band structure theory for Seebeck coefficients of three semiconductors mentioned above. Simulation with periodic boundary condition can be generalized directly to treat with doped semiconductor in near future.

LIMITING CONDUCTANCE OF LYONIUM AND LYATE IONS

1959 ◽  
Vol 37 (1) ◽  
pp. 173-177 ◽  
Author(s):  
Martin Kilpatrick
Keyword(s):  
Mixed Solvents ◽  
Direct Determination ◽  
Solvent Mixture ◽  
Dielectric Constants ◽  
Proton Mobility ◽  
Anhydrous Hydrogen Fluoride ◽  
Ice Leads ◽  
Hydrogen Bonded Systems ◽  
High Dielectric ◽  
Strong Acids

The problem of proton mobility has been considered in H2O–CH3OH, H2O–D2O, and H2O–H2O2 solvents from the current viewpoint of the mechanism of proton mobility for aqueous solutions. Mixed solvents are more complicated in that one must consider the relative basicity and acidity of the species competing for the protons. It is concluded that for dilute solutions of HClO4, where water is replaced by hydrogen peroxide, the decrease in equivalent conductance relative to that of KCl in the same solvent mixture is due to the partial elimination of the proton transfer process.For highly acidic non-aqueous solvents of high dielectric constants such as HF, HCN, and HCOOH, the problem of the weakness of the usual "strong" acids of aqueous solution makes a direct determination of the limiting equivalent conductances difficult. In the case of anhydrous hydrogen fluoride the available experimental evidence indicates that the limiting conductance of the lyonium ion is approximately the same as that of the potassium ion but the lyate ion has a higher limiting conductance than other stable anions.The higher proton mobility in ice leads one to expect that hydrogen-bonded systems may be found where the conductivity may approach that of electronic semiconductors.

scholarly journals The behaviour of electrolytes in mixed solvents. Part I.—The free energies and heat contents of hydrogen chloride in water—Ethyl alcohol solutions

1929 ◽  
Vol 125 (799) ◽  
pp. 694-712 ◽  
Keyword(s):  
Hydrogen Chloride ◽  
Electric Fields ◽  
Mixed Solvents ◽  
Dielectric Constants ◽  
Free Energies ◽  
Dissolved Ions ◽  
Uniform Medium ◽  
The Mean ◽  
Solvent Molecules ◽  
Water Alcohol

Previous studies on the effect of a change of medium on tire properties of dissolved electrolytes have aimed at correlating the behaviour of the electrolyte with the mean physical properties, e. g ., dielectric constants, of the medium. While this approach may be justified in the case of solvents containing molecules of only one kind, it is not sufficient to regard a mixed solvent as a uniform medium affecting the dissolved ions solely through the effect of its dielectric constant on the electric forces between them. For the electric fields of ions exert a differential attraction on molecules possessing different degrees of polarisability and since tire more polarisable molecules must tend to congregate round the ions, the properties of the latter cannot depend solely on tire mean properties of tire medium. Studies on the behaviour of ions in such cases will throw light on the interaction between ions and solvent molecules. The present paper gives tire results of measurements of the free energies and heat contents of hydrogen chloride in water-alcohol solutions, obtained by determining the electromotive forces of cells of the type:— H 2 ( g ) | HCl ( m ), AgCl ( s ) | Ag water-alcohol

scholarly journals A note on some further determinations of the dielectric constants of organic bodies and electrolytes at very low temperatures

1898 ◽  
Vol 62 (379-387) ◽  
pp. 250-266 ◽  
Keyword(s):  
Dielectric Constant ◽  
Low Temperatures ◽  
Tuning Fork ◽  
Dielectric Constants ◽  
The Past ◽  
Method Of Measurement ◽  
The Given ◽  
Past Summer

In several previous communications we have described the investigations made by us on the dielectric constants of various frozen organic bodies and electrolytes at very low temperatures. In these researches we employed a method for the measurement of the dielectric constant which consisted in charging and discharging a condenser, having the given body as dielectric, through a galvanometer 120 times in a second by means of a tuning-fork interrupter. During the past summer we have repeated some of these determinations and used a different method of measurement and a rather higher frequency. In the experiments here described we have adopted Nernst’s method for the measurement of dielectric constants, using for this purpose the apparatus as arranged by Dr. Nernst which belongs to the Davy-Faraday Laboratory.

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