The Debye—Hückel Ion Size Parameter in Terms of Individual Ionic Radii. The Activity Coefficient of Lead Chloride in Solutions of Cadmium Nitrate1

1933 ◽  
Vol 55 (2) ◽  
pp. 568-574 ◽  
Author(s):  
H. D. Crockford ◽  
Henry C. Thomas
Keyword(s):  
Activity Coefficient ◽  
Lead Chloride ◽  
Size Parameter ◽  
Ionic Radii ◽  
Ion Size

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.

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.

Osmotic and activity coefficients in dilute potassium chloride solutions at 25 °C

1980 ◽  
Vol 58 (13) ◽  
pp. 1386-1387 ◽  
Author(s):  
Chai-Fu Pan
Keyword(s):  
Vapor Pressure ◽  
Potassium Chloride ◽  
Activity Coefficients ◽  
Size Parameter ◽  
Pressure Data ◽  
Vapor Pressure Data ◽  
Chloride Solutions ◽  
Ion Size ◽  
Robinson Equation ◽  
Existing Data

Osmotic and activity coefficients of dilute aqueous potassium chloride solutions are calculated from the simplified forms of the Stokes and Robinson equation. The hydration parameters in these equations are obtained from the vapor pressure data measured at higher concentration regions and the ion-size parameter is chosen as the sum of the crystallographic radii of the cation and anion of the electrolyte. The results are very satisfactory in comparison with existing data.

Thermodynamic behaviour of some electrolytes in ethane-1,2-diol from −10 to +80 °C

1993 ◽  
Vol 71 (8) ◽  
pp. 1265-1272 ◽  
Author(s):  
Fulvio Corradini ◽  
Luigi Marcheselli ◽  
Lorenzo Tassi ◽  
Giuseppe Tosi ◽  
Salvatore Fanali
Keyword(s):  
Experimental Data ◽  
Dissociation Constant ◽  
Ion Pairs ◽  
Size Parameter ◽  
Equivalent Conductivity ◽  
Thermodynamic Behaviour ◽  
Informative Parameters ◽  
Ion Conductivities ◽  
Ion Size ◽  
Reference Electrolyte

Conductivities of the electrolytes NaBr, NaPi, HPi, NaBPh4, and Ph4PBr in ethane- 1,2-diol were determined in the −10 ≤ t ≤ +80 °C temperature range. The experimental data were analyzed by the Fuoss–Hsia equation, which provides further informative parameters such as the dissociation constant (K) of the ion pairs formed in solution, the limiting equivalent conductivity (Λ0), and the ion-size parameter (å). Thermodynamic behaviour of these electrolytes was derived from analysis of the K values. Single-ion conductivities were evaluated on the basis of the assumption of Ph4PBPh4 as reference electrolyte.

Conductance Study of Ion Pairing of Alkali Metal Tetrafluoroborates and Hexafluorophosphates in Acetonitrile

1975 ◽  
Vol 53 (22) ◽  
pp. 3448-3451 ◽  
Author(s):  
H. L. Yeager ◽  
B. Kratochvil
Keyword(s):  
Alkali Metal ◽  
High Precision ◽  
Ion Pairing ◽  
Size Parameter ◽  
Sodium Potassium ◽  
Ion Size ◽  
Best Fit ◽  
Expanded Form

High precision conductance measurements are reported for sodium, potassium, and rubidium tetrafluoroborate and hexafluorophosphate in acetonitrile at 25 °C. The results are analyzed using the expanded form of the Fuoss–Hsia conductance equation. The ion size parameter, d, was systematically varied to obtain the value which gave best fit of the data to the equation. All salts were found to be associated, and the trends in association are discussed in terms of the ability of acetonitrile to solvate cations and anions.

Electrical conductance of a mixture of sodium and potassium nitrates in aqueous medium

1990 ◽  
Vol 68 (11) ◽  
pp. 2115-2118 ◽  
Author(s):  
Ratan Lal Gupta ◽  
Kochi Ismail
Keyword(s):  
Aqueous Medium ◽  
Electrical Conductance ◽  
Potassium Nitrate ◽  
Molar Conductance ◽  
Size Parameter ◽  
Mixed Alkali ◽  
Mixed Alkali Effect ◽  
The Difference ◽  
Ion Size ◽  
Sodium And Potassium

Electrical conductance and density measurements of [xNaNO3 + (1 − x)KNO3] + RH2O system were taken as functions of x, R, and temperature. The mixed alkali effect on molar conductance (Λ) was found to be negligible upto R = 25 and becomes significant in the region where R < 25. It has been shown that for mixed electrolytic system in aqueous medium the concentration range at which the mixed alkali effect on Λ starts becoming significant can be predetermined by plotting the difference in Λ of the two pure electrolytic solutions versus R. The concentration dependence of Λ has been described satisfactorily by the expression Λ = ΛFLK exp (Bc + Cc2) where ΛFLK is the Falkenhagen–Leist–Kelbg equation for Λ, B and C are empirical constants, and c is the molar concentration. The observed values of the ion-size parameter have indicated more ionic association in KNO3 solution than in NaNO3 solution. Keywords: electrical conductance, sodium nitrate, potassium nitrate, mixed alkali effect.

Modified Linearized Poisson-Boltzmann Theory. Dynamic and Thermodynamic Properties of 1 : 1 Electrolytes

2000 ◽  
Vol 53 (12) ◽  
pp. 989
Author(s):  
Tuncer Kaya
Keyword(s):  
Distribution Function ◽  
Short Range ◽  
Pair Potential ◽  
Boltzmann Distribution ◽  
Size Parameter ◽  
Moment Conditions ◽  
Poisson Boltzmann ◽  
Short Range Part ◽  
Ion Size ◽  
Range Part

Theoretical electrolyte conductivity and osmotic and activity coefficient relationships that work well over a large range of concentrations, up to 1 mol l–1, are derived from a hypothetical modified linearized Poisson–Boltzmann distribution function. The distribution function is expressed in terms of modified Debye parameter κ and normalization constant α. Both of these parameters are evaluated in terms of concentration and ion-size parameter, d, by the help of moment conditions. The modified Debye parameter κ is also expressed as a function of the usual Debye parameter κD. Also considered is the short-range part of the pair potential crucial to obtain at least qualitative agreement with experimental results of electrolytic solutions, and it is assumed that the short-range part of the potential is discontinuous at ion-size parameter

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