Conductimetric studies of ionic association of tetraalkylammonium halides in iso-propanol + water mixtures at 25 °C. Part II.

1988 ◽  
Vol 66 (7) ◽  
pp. 1720-1727 ◽  
Author(s):  
Auaz Ahmad Ansari ◽  
M. R. Islam
Keyword(s):  
Dielectric Constant ◽  
Association Constant ◽  
Ionic Association ◽  
Size Parameter ◽  
Solvent Interactions ◽  
Tetraalkylammonium Ions ◽  
Conductance Data ◽  
Electrical Conductivities ◽  
Ion Size ◽  
Tetraalkylammonium Halides

Electrical conductivities of Me4NBr, Et4NBr, Pr4NBr, Bu4NBr, and Bu4PBr have been measured in isopropanol + water (2-PrOH + H2O) mixtures covering the approximate range of dielectric constant (71.40 ≥ D ≥ 19.40) at 25 °C. The conductance data have been analysed by using the Fuoss-1978 (F78) conductance equation and the results compared with those obtained from the Fuoss–Onsager–Skinner (FOS) equation. The values of the limiting equivalent conductance, Λ0, the association constant, KA, and the distance of ion-size parameter [Formula: see text] are computed from these data. A better fit of the conductance data was provided by the F78 equation. Ion–solvent interactions and effective sizes of tetraalkylammonium ions are also discussed in order to understand the magnitude of the ionic association. The overall association behaviour of these salts has been found to increase with decrease in dielectric constant of the medium.

Conductivity and ionic association of tetraalkylammonium halides in tert-butanol–water mixture at 25 °C

1988 ◽  
Vol 66 (5) ◽  
pp. 1223-1228 ◽  
Author(s):  
Aijaz Ahmad Ansari ◽  
M. R. Islam
Keyword(s):  
Ion Association ◽  
Ionic Association ◽  
Solvent Mixtures ◽  
Water Mixture ◽  
Solvent Interaction ◽  
Tert Butanol ◽  
Ion Association Constants ◽  
Conductance Data ◽  
Ion Size ◽  
Tetraalkylammonium Halides

The molar conductivities of Pr4NBr, Bu4NBr, Pr4NI, and BU4NI have been measured in tert-butanol–water (t-BuOH–H2O) mixtures (61.30 ≥ D ≥ 16.50) over the maximum concentration range (2 × D3 × 10−7 mol dm−3) along with the densities and viscosities of the solvent mixtures at 25 °C. The conductance data have been analysed by using the Fuoss-1978 (F78) conductance equation and the results compared with the values obtained from the Justice (J), Pitt's (P), and Fuoss–Onsager–Skinner (FOS) equations. Molar conductivities at infinite dilution (Λ0), the thermodynamic ion association constants (KA) and the distance or ion-size parameters (R0 or a0) are evaluated from these data. The F78 equation fitted the data better and yielded KA and R values which are in accord with the ion-association theories. The interpretation of these parameters is discussed to provide some insight on the magnitude of the ionic association and the ion–solvent interaction.

Equilibria in acetic acid: Ionic association constant of acetamidium perchlorate and acid-base equilibrium constant of acetamidium acetate at 105.7°

1965 ◽  
Vol 18 (6) ◽  
pp. 801 ◽  
Author(s):  
RJL Martin
Keyword(s):  
Dielectric Constant ◽  
Acetic Acid ◽  
Equilibrium Constant ◽  
Association Constant ◽  
Ionic Association ◽  
Equivalent Conductivity ◽  
Acid Base ◽  
Base Equilibrium ◽  
Acid Base Equilibrium

In acetic acid at 105.7� acetamidium perchlorate has an ionic association constant KA = 0.0491 x 106 l. mole-1, a limiting equivalent conductivity A, = 79.4 cm2 Ω-1 equiv.-1, and a centre-to-centre distance between the ions � = 4.67 Ǻ. The acid-base equilibrium constant for acetamidium acetate KB = [ΣNH3Ac+ OAc-]/ [NH2Ac] increases slightly with increasing dielectric constant.

Equilibria in acetic acid: ionic association constant of oxonium perchlorate, acid-base equilibrium constant of oxonium acetate, and autoprotolysisconstant of acetic acid at 105.7°

1965 ◽  
Vol 18 (3) ◽  
pp. 321 ◽  
Author(s):  
RJL Martin
Keyword(s):  
Dielectric Constant ◽  
Acetic Acid ◽  
Equilibrium Constant ◽  
Association Constant ◽  
Ionic Association ◽  
Aqueous Acetic Acid ◽  
Equivalent Conductivity ◽  
Acid Base ◽  
Base Equilibrium ◽  
Acid Base Equilibrium

In aqueous acetic acid, 0.114-0.152M H2O, at 105.7�, oxonium perchlorate has limiting equivalent conductivity Λ0 90.7, ionic association constant KA = [H3O+ClO4-]/[H3O+][ClO4]f2 = 0.0310 x 106 and centre-to-centre distance between the ions (� = 4.84 Ǻ. The acid-base equilibrium constant for oxonium acetate KB = [ΣH3O+ OAc-]/[H2O] increases with the dielectric constant so that -log KB = 1.532+29.44/D. The autoprotolysis of acetic acid also increases with the dielectric constant.

Application of the Fuoss–Onsager theory to conductance data for sodium and potassium iodide solutions in various solvents

1967 ◽  
Vol 45 (10) ◽  
pp. 1101-1108 ◽  
Author(s):  
George J. Janz ◽  
Malcolm J. Tait
Keyword(s):  
Dielectric Constant ◽  
Potassium Iodide ◽  
Ion Association ◽  
Mean Value ◽  
Lower Dielectric Constant ◽  
Conductance Data ◽  
High Dielectric ◽  
Ion Size ◽  
Onsager Theory ◽  
Sodium And Potassium

The 1957 Fuoss–Onsager conductance equation has been used to analyze data for sodium iodide and potassium iodide solutions in 13 one-component solvents, ranging from water (dielectric constant 78) to pyridine (dielectric constant 12). Values of the unknowns Λ0, åJ, an ion size parameter, and, where appropriate, Ka, the ion association constant, are calculated. In solvents of high dielectric constant it is found that the salts are completely dissociated (Ka = 0) and the mean value of åJ is 4.5 Å for each salt. However, the ion size parameters from the conductance equation do not seem to have any physical significance in solvents of lower dielectric constant, where there is evidence of ionic association. An analysis of these data is considered in which the Fuoss–Onsager equation reduces to a one-parameter equation, with Ka as the unknown. The conductance data for sodium and potassium iodide can then be understood if the closest distance of approach of the ions is 4.5 Å in all 13 solvents.

Physico-chemical studies in non-aqueous solvents. X. Conductance and solvation studies of 1 : 1 electrolytes in N,N-dimethylacetamide

1975 ◽  
Vol 28 (2) ◽  
pp. 321 ◽  
Author(s):  
RC Paul ◽  
JS Banait ◽  
SP Narula
Keyword(s):  
Potassium Thiocyanate ◽  
Transference Numbers ◽  
Size Parameter ◽  
Ionic Radii ◽  
Solvation Numbers ◽  
Physico Chemical ◽  
Conductance Data ◽  
Chemical Studies ◽  
Ionic Mobilities ◽  
Ion Size

Conductances of some 1 : 1 electrolytes have been measured in the concentration range 1-120 x 10-4 mol l-1 in N,N-dimethylacetamide at 25�. The conductance data have been analysed by Fuoss-Onsager-Skinner equations for dissociated and associated electrolytes, and limiting equivalent conductances, ion-size parameter and association constants (where appropriate) for various electrolytes have been obtained. The ion-size parameter (3.7 � 0.3Ǻ) has been found to be about the same for all the electrolytes. Alkali metal salts are fully dissociated while the substituted ammonium salts are slightly associated in this solvent. The ionic association increases with increase in the size of cations. Transference numbers of lithium chloride, potassium thiocyanate and silver perchlorate have also been measured in the concentration range 1.1-18.4 x 10-2mol l-1 in this solvent. Limiting cation transference numbers are determined from the linear plots of cation transference numbers against square root of concentration. Ionic mobilities, effective ionic radii and solvation numbers of various ions in solution have been calculated. Higher solvation numbers of cations than those of anions of comparable sizes are consistent with the aprotic nature of the solvent.

scholarly journals Ionic Conductivity of Chitosan-Lithium Electrolyte in Biodegradable Battery Cell

2020 ◽  
Vol 20 (3) ◽  
pp. 655
Author(s):  
Ali Benouar ◽  
Mohammed Reda Ahmed Bacha
Keyword(s):  
Ionic Conductivity ◽  
Lithium Battery ◽  
Empirical Equation ◽  
Ionic Association ◽  
Temperature Dependency ◽  
Battery Cell ◽  
Solvent Interactions ◽  
Temperature Range ◽  
Electrical Conductivities

The electrical conductivities of salts (LiCl, LiOH) in chitosan as an electrolyte in biodegradable batteries have been measured at the concentration range 10–100 mol m–3 in the temperature range 278–308 K. The data were interpreted in terms of ion–ion and ion–solvent interactions using the Fuoss paired ion. The fitting of Fuoss’ equation of 1978 to these data led us to an estimate of the ionic association by computing the conductimetric pairing constants. In order to optimize the use of the electrolyte in the clean lithium battery, the temperature dependency of conductivity will be studied using Arrhenius empirical equation. This equation was applied successfully in the temperature range used in this study.

scholarly journals Density and Viscosity of LiCl, LiBr, LiI and Kcl in Aqueous Methanol at 313.15K

2021 ◽  
Vol 37 (5) ◽  
pp. 1083-1090
Author(s):  
V. V. Kadam ◽  
A. B. Nikumbh ◽  
T. B. Pawar ◽  
V. A. Adole
Keyword(s):  
Experimental Data ◽  
Dielectric Constant ◽  
Apparent Molar Volumes ◽  
Strong Electrolyte ◽  
Aqueous Methanol ◽  
Molar Volumes ◽  
Solvent Interactions ◽  
Viscosity Coefficients ◽  
Physicochemical Processes ◽  
Increase With Increase

The densities and viscosities of electrolytes are essential to understand many physicochemical processes that are taking place in the solution. In the present research, the densities and viscosities of lithium halides, LiX (X = Cl, Br, I ) and KCl in (0, 20, 40, 50, 60, 80 and 100) mass % of methanol + water at 313.15K were calculated employing experimental densities (ρ), the apparent molar volumes( ϕv) and limiting apparent molar volumes (0v) of the electrolytes. The (0v) of electrolyte offer insights into solute-solution interactions. In terms of the Jones-Dole equation for strong electrolyte solution, the experimental data of viscosity were explored. Viscosity coefficients A and B have been interpreted and discussed. The B-coefficient values in these systems increase with increase of methanol in the solvents mixtures. This implied that when the dielectric constant of the solvent decreases, so do the solvent-solvent interactions in these systems.

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