Ionic association in aqueous solutions of strong electrolytes

A more accurate calculation of relaxation effects obtained with the standard Debye-Hückel-Onsager model has been presented recently and is here applied to several aqueous 1:1 electrolytes. The variation of the standard deviation between calculated and observed equivalent conductivities withK _A leads to an ill-defined minimum; but, where data over a wide concentration range are available, the minimum corresponds to values of the contact distancea which approximate to estimates from ionic dimensions. It is therefore proposed that, although preciseK _A values from conductance cannot be determined, the most probable values are those associated with realistic estimates ofa. When data cover a limited concentration range, minimum standard deviations are often indeterminate or vary greatly for duplicate runs. It is shown that reasonable values ofK _A can be obtained from such data if comparison is made at estimated values ofa.Notation The symbols not defined in the text are the following b e ²/kTa for 1:1 electrolytes - e electronic charge - k Boltzmann gas constant - T absolute temperature - dielectric constant of solvent - –(3/2y)(_e0/₀)     

Electrical conductance and ionic association of the bivalent transition metal tetrafluoroborates in acetonitrile solution

Visible absorption spectra of Co(BF₄)₂ and Ni(BF₄)² in acetonitrile (AN) indicate the existence of complex electrolytes solely of the type [M(AN)₆]²⁺·2BF ₄ ^– . Close agreement of the molar conductance curves for Mn(BF₄)₂, Co(BF₄)₂, Ni(BF₄)₂, Cu(BF₄)₂, and Zn(BF₄)₂ indicates that the same is true for the other tetrafluoroborates as well. Small specific differences in properties of the [M(AN)₆]²⁺ complex cations are reflected in the limiting molar conductances, while the first-step association constants to a good approximation are the same for the different metal cations. Penetration of the tetrafluoroborate anion in between the coordinated acetonitrile molecules is suggested as a possible explanation for the apparent independence of ionic association on the crystallographic radius of the cation.     

Ionic association in hydrogen-bonding solvents

Studies on ionic association in hydrogen-bonding solvents including water, aliphatic alcohols, fluorinated alcohols, formamide, ethylene glycol, and propanol-acetone mixtures are compared. Data were derived from measurements of conductivity, ultrasonic absorption, and viscosity of electrolyte solutions and diffusion of nonelectrolytes. It is concluded that electrolyte solvents can be divided into three categories according to whether they solvate effectively cations only, anions only, or both cations and anions. Water and most other hydrogenbonding solvents constitute the third class, a group in which patterns of ionic aggregation are very similar. Fluorinated alcohols belong to the second class, showing significantly different ion-pairing behavior.This paper was presented at the symposium, The Physical Chemistry of Aqueous Systems, held at the University of Pittsburgh, Pittsburgh, Pennsylvania, June 12–14, 1972, in honor of the 70th birthday of Professor H. S. Frank.     

Electrical conductivities of halide salts in aqueous formamide solutions

The electrical conductivities of sodium chloride and sodium iodide solutions in formamide-water mixtures of different composition have been measured at 25°C. From these data, the limiting equivalent conductances for these salts have been determined. The correspondingWalden products are compared together with the one reported for sodium bromide in the same solvent mixtures, and they are analysed as functions of the anion size. Further, the limiting ionic equivalent conductances are estimated for the different ions. The variation of the ionicWalden products with solvent composition is discussed in terms of ionic solvation and solvent structure.

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Elektrische Leitfähigkeit von Halogensalzen in wäßrigen Formamid-Lösungen

Zusammenfassung Es wurden die elektrischen Leitfähigkeiten von Natriumchlorid- und Natriumjodidlösungen in Formamid-Wasser-Mischungen verschiedener Zusammensetzung bei 25°C gemessen. Aus diesen Daten wurden die Grenzäquivalenzleitfähigkeiten für diese Salze bestimmt. Die entsprechendenWalden-Produkte wurden mit den für Natriumbromid in den gleichen Lösungsmittelgemischen berichteten verglichen und hinsichtlich der Anionengrößen analysiert. Außerdem wurden die ionischen Grenzäquivalenzleitfähigkeiten für die einzelnen Ionen abgeschätzt. Die Variation der ionischenWalden-Produkte mit der Lösungsmittelzusammensetzung wurde bezüglich Ionensolvatation und Lösungsmittelstruktur diskutiert.

     

Conductance studies on the interaction of D-glucose with alkali halides in water and formamide

The interaction of D-glucose with alkali halide in aqueous and formmide solutions has been studied by employing conductance measurements. Our results showed a break at the saturation temperature indicating a transition in the conductance values. This behaviour is explained in terms of solute-solvent interactions involved in the electrolyte-solvent-nonelectrolyte systems.     

Ionic Association of the Ionic Liquids [C4mim][BF4], [C4mim][PF6], and [Cnmim]Br in Molecular Solvents

Considering the ionic nature of ionic liquids (ILs), ionic association is expected to be essential in solutions of ILs and to have an important influence on their applications. Although numerous studies have been reported for the ionic association behavior of ILs in solution, quantitative results are quite scarce. Herein, the conductivities of the ILs [C_nmim]Br (n=4, 6, 8, 10, 12), [C₄mim][BF₄], and [C₄mim][PF₆] in various molecular solvents (water, methanol, 1‐propanol, 1‐pentanol, acetonitrile, and acetone) are determined at 298.15 K as a function of IL concentration. The conductance data are analyzed by the Lee–Wheaton conductivity equation in terms of the ionic association constant (K_A) and the limiting molar conductance (Λ_m⁰). Combined with the values for the Br^? anion reported in the literature, the limiting molar conductivities and the transference numbers of the cations and [BF₄]^? and [PF₆]^? anions are calculated in the molecular solvents. It is shown that the alkyl chain length of the cations and type of anion affect the ionic association constants and limiting molar conductivities of the ILs. For a given anion (Br^?), the Λ_m⁰ values decrease with increasing alkyl chain length of the cations in all the molecular solvents, whereas the K_A values of the ILs decrease in organic solvents but increase in water as the alkyl chain length of the cations increases. For the [C₄mim]⁺ cation, the limiting molar conductivities of the ILs decrease in the order Br^?>[BF₄]^?>[PF₆]^?, and their ionic association constants follow the order [BF₄]^?>[PF₆]^?>Br^? in water, acetone, and acetonitrile. Furthermore, and similar to the classical electrolytes, a linear relationship is observed between ln K_A of the ILs and the reciprocal of the dielectric constants of the molecular solvents. The ILs are solvated to a different extent by the molecular solvents, and ionic association is affected significantly by ionic solvation. This information is expected to be useful for the modulation of the IL conductance by the alkyl chain length of the cations, type of anion, and physical properties of the molecular solvents.     

Ionic interactions in solutions. I. The association concepts and the McMillan-Mayer theory

A review is given of the most common models of ionic-pair association used by Bjerrum, Fuoss, and Eigen to supplement the breakdown of the Debye-Hückel law for the mean activity coefficient of symmetrical electrolytes in lower-dielectric-constant solvents. The compressibility and pressure equations of Rasaiah and Friedman and the virial equation are used to rederive the activity coefficients from the distribution functions of Meeron and of Debye and Hückel. The results are compared to the well-known results of Debye and Hückel and that of Bjerrum. In each case the anion-cation pair association concept of Bjerrum is verified. Finally, a discussion is included on the best evaluation of the critical distance which distinguishes between free and associated ions. The activity equation is easily generalized to any short-range Hamiltonian model.This paper is based in part on the thesis of M.-C. Justice, Université Pierre et Marie Curie (Paris VI), in June 1974, in partial fulfillment of the requirements for the degree of Docteur d'Etat.     

Application of the Bjerrum association model to volumes of electrolytes in water and acetonitrile

The Bjerrum association model has been extended to partial and apparent molar volumes. It was tested for electrolytes in water and in acetonitrile using literature or new (n-propylammonium bromide) data to cover systems having association constants between 0 and 10⁵. The association constants and apparent distances of closest approach were obtained from conductivities. The volumes at low concentration can be fitted quantitatively to obtain by extrapolation the standard infinite dilution partial molar volume. Deviations at higher concentrations can be accounted for with a second virial coefficient.     

Ionic Transport in Dilute Solid Polymer Electrolytes with Amorphous Structure

The ionic structure and transport properties of amorphous solid polymer electrolytes in the system copolymer of acrylonitrile and butadiene (40 : 60)—lithium hexafluoroarsenate (SPE) is studied in the region of small salt concentrations (up to 0.37 mol dm⁻³) at 298–368 K. In conditions studied, LiAsF₆ is dissociated predominantly to ions. Macroscopic models of ion transport are used to analyze the results of measurements of transport characteristics of SPE. Transport of anions free of the polymer matrix is realized activationlessly and resembles the Stokes drift in viscous media. Transport of cations solvated by electron-donating groups of the polymer turns possible only at temperatures in excess of a critical value (T _crit ≈ 333 K), when the statistical mean of molecules in the first coordination sphere of the lithium cation becomes less than four (which is the coordination number for solvation) and requires the overcoming of an energy barrier of ∼6 kJ mol⁻¹. Below T _crit, the SPE are unipolar anionic conductors.__________Translated from Elektrokhimiya, Vol. 41, No. 5, 2005, pp. 537–545.Original Russian Text Copyright © 2005 by Bushkova, Sofronova, Lirova, Zhukovskii.     

NMR Diffusion Measurements as a Simple Method to Examine Solvent–Solvent and Solvent–Solute Interactions in Mixtures of the Ionic Liquid [Bmim][N(SO2CF3)2] and Acetonitrile

The self‐diffusion coefficients of each component in mixtures of 1‐butyl‐3‐methylimidazolium bis(trifluoromethanesulfonyl)imide ([Bmim][N(SO₂CF₃)₂]) and acetonitrile were determined. The results suggest that the hydrodynamic boundary conditions change from “stick” to “slip” as the solvent composition transitions from “ionic liquid dissolved in acetonitrile” (χ_IL<0.4) to “acetonitrile dissolved in ionic liquid” (χ_IL>0.4). At higher χ_IL, the acetonitrile species are affected by “cage” and “jump” events, as the acetonitrile molecules reside nearer to the charged centre on the ions than in the “non‐polar” regions. The self‐diffusion coefficients of hexan‐1‐amine, dipropylamine, 1‐hexanol and dipropylether in mixtures of [Bmim][N(SO₂CF₃)₂] and acetonitrile were determined. In general, the nitrogen‐containing solutes were found to diffuse slower than the oxygen‐containing solutes; this indicates that there are greater ionic liquid–N interactions than ionic liquid–O interactions. This work demonstrates that the self‐diffusion coefficients of species can provide valuable information about solvent–solvent and solvent–solute interactions in mixtures containing an ionic liquid.     

离子液体在锂离子电池中的应用研究进展

离子液体具有蒸汽压低、热稳定性好、不易挥发、溶解能力强、环境友好、电化学稳定窗口和液程范围宽等优点,在锂离子电池领域应用前景广泛。本文按照离子液体作为电解质溶剂、与传统电解质复配或与聚合物电解质结合的应用方式,总结其对电池的安全性和热稳定性的影响,并综述了近年来离子液体在锂离子电池电解质中的应用研究进展。     

Conductance of 1,1-electrolytes in acetonitrile solutions from −40° to 35°C

Conductance data for perchlorates of Li⁺, K⁺, Me₄N⁺, Et₄N⁺, Pr₄N⁺, Bu₄N⁺, iodides of K⁺, Me₄N⁺, i-Am₃BuN⁺, and tetraphenylborates of Na⁺, Bu₄N⁺ and i-Am₃BuN⁺ in acetonitrile solution in the temperature range −40° to 35°C are reported. Λ_° (limiting molar conductance) and K_A (association constant) are evaluated for several temperatures using a conductance equation based on the chemical model of electrolyte solutions including short range forces. Limiting molar ion conductances, λ _ΰ ⁱ , at −35°, −25°, −15°, −5°, 5°, 15° and 25°C are evaluated from temperature dependent limiting transference numbers. Enthalpies and entropies of association, obtained from the temperature dependence of the association constants, are also presented. Dedicated to the memory of Professor Raymond M. Fuoss.     

Conductance of solutions of lithium bis(trifluoromethanesulfone)imide in water,propylene carbonate,acetonitrile and methyl formate at 25°C

Conductance data for lithium bis(trifluoromethanesulfone)imide, LiN(CF ₃ SO ₂ ) ₂ , are reported for the solvents water, propylene carbonate, acetonitrile and methyl formate at 25°C. Limiting molar conductivitiesA ₀, association constants K _A , and triple ion formation constants K _t are reported where applicable. These data are compared with literature data for the commonly studied lithium salts LiClO ₄ and LiAsF ₆ . Non-coulombic energy contributions to ion pair formation are evaluated and discussed in terms of ion-ion and ion-solvent interactions.     

Ionic association and solvation in solutions of magnesium and nickel perchlorates in acetonitrile

The paper presents the conductometric data on solutions of Mg(ClO₄)₂ and Ni(ClO₄)₂ in acetonitrile over the temperature ranges 5–55°C for Mg(ClO₄)₂ and 25–75°C for Ni(ClO₄)₂. The extended Lee-Wheaton equation for unsymmetrical electrolytes was used to determine the limiting equivalent conductivities of the Mg²⁺, Ni²⁺, and ClO ₄ ^? ions and first-step ionic association constants with the formation of [KtClO₄]⁺ ion pairs. Lower ionic association constants for Ni(ClO₄)² compared with Mg(ClO₄)₂ were a consequence of stronger non-Coulomb repulsion in the formation of [KtClO₄]⁺ ion pairs because of the formation of a firmer solvation shell by the nickel compared with magnesium cation. The structure-dynamic parameter of ionic solvation was estimated. It was found that spatial-time correlations in the nearest environment of ions increased in the series ClO ₄ ^? > Mg²⁺ > Ni²⁺.     

Solvent effects on complexation of crown ethers with LiClO4, NaClO4 and KClO4 in methanol and acetonitrile

The thermodynamic formation constants K_f for complexation of Li⁺, Na⁺ and K⁺ with the crown ethers 12C4 and 15C5 have been determined in methanol and acetonitrile at 25°C using precision conductivity data. The method permits evaluation of very small K_f values (e.g., K_f=6.98 mol^–1-dm³ for LiClO₄+12C4 in methanol) as well as fairly large values (e.g., K_f=2.73×10⁴ mol^–1-dm³ for NaClO₄+15C5 in acetonitrile). The determination of K_f values from conductivity data takes into consideration the often neglected ion pair formation of both the uncomplexed and the complexed cations. Our results for K_f are generally consistent with previously reported values based on potentiometry, calorimetry and polarography, but there are significant differences in several cases which we attribute to neglect of ion association both for the uncomplexed or free cation K_a and the macrocyclic complexed cation K_a2. Our results are also consistent with the well known concepts relating the magnitude of K_f to both the cavity diameter and ion-solvent interactions. Limiting molar conductivities ₂ ⁰ for the complex salt (M-crown ether) (ClO₄) in both solvents were generally found to be smaller or very close to the corresponding quantity ₁ ⁰ for the binary MClO₄-solvent system. However, in methanol, single ion limiting molar conductivities for the cationic complexes ₂ ⁰ exhibit anomalous behavior which is attributed to solvation differences between free cations and complexed cations.     

Ionic liquid-alkane association in dilute solutions

Enthalpies and entropies of transfer were measured by gas chromatography for dilute solutions of a homologous series of eight even n-alkanes (from octane to docosane) into six different ionic liquids (ILs) (namely, 1-butyl-3-methylimidazolium chloride, bromide, iodide, triflate and hexafluorophosphate; plus N-butylmethylpyridinium bis {(trifluoromethyl) sulfonyl}-imide) over the 80–150 °C temperature range, all ILs being in the liquid state. Over a narrow concentration range, the entropic change may be consistent with a solvophobic association model of n-alkanes in ILs. A very simple model is proposed to account for the thermodynamic data. This approach can be used to approximate interionic distances and possible dielectric constants for ILs. Although the model may have some use in dilute alkane-IL solutions, more sophisticated models, particularly for the enthalpic contributions, are desirable.     

Conductance of Some 1:1 Electrolytes in N,N-Dimethylacetamide at 25°C

Precise conductance measurements of solutions of lithium chloride, lithium bromide, lithium iodide, lithium perchlorate, lithium tetrafluoroborate, lithium hexafluoroarsenate, tetrabutylammonium bromide, and tetrabutylammonium tetraphenylborate in N,N-dimethylacetamide are reported at 25°C in the concentration range 0.005–0.015 mol-dm^–3. The conductance data have been analyzed by the 1978 Fuoss conductance equation in terms of the limiting molar conductance (⁰), the association constant (K _a), and the association diameter (R). The limiting ionic conductances have been estimated from an appropriate division of the limiting molar conductivity of the reference electrolyte Bu₄NBPh₄. Slight ionic association was found for all these salts in this solvent medium. The results further indicate significant solvation of Li⁺ion, while the other ions are found to be unsolvated in N,N-dimethylacetamide.     

Structure of solvated lithium and chloride ions in formamide

Structure of solvated lithium and chloride ions in formamide was investigated by means of X-ray diffraction at 25°C. Lithium ion has, on average, 5.4 formamide molecules as nearest neighbors with an Li⁺-O distance of 224 pm, while chloride ion is coordinated with 4.5 formamide molecules with the Cl^–···N distance of 327 pm. The amino group within a formamide molecule interacts with a chloride ion in the bifurcate manner through two hydrogen atoms.Session lecture, IX International Conference on Non-Aqueous Solutions, Pittsburgh, PA, August 1984.To whom correspondence should be addressed.     

离子液体的酸性测定及其催化的二苯醚／十二烯烷基化反应

 采用乙腈探针红外光谱法测定了［bmim］Cl／AlCl3类离子液体的酸性．结果表明，乙腈可以区分离子液体的酸类型（Bronsted酸或Lewis酸），同时可以指示离子液体的Lewis酸强度．使用［bmim］Cl／AlCl3类离子液体催化二苯醚与十二烯的烷基化反应，研究了离子液体的酸强度、反应温度和醚烯比对反应的影响，并与AlCl3催化体系进行对比．结果发现，该离子液体对二苯醚与十二烯烷基化反应的催化活性明显高于AlCl3．使用离子液体作催化剂显著提高了烷基化反应的产率，简化了产物的分离与提纯，且对环境友好．当控制反应温度为80℃，原料醚烯摩尔比为7，并采用酸强度适中的离子液体时，目标产物单十二烷基二苯醚的产率接近90％．