Electrolyte ionization constant

Beyer synthesis, 2, 474 electrolytic oxidation, 2, 325 7r-electron density calculations, 2, 316 1-electron reduction, 2, 282, 283 electrophilic halogenation, 2, 49 electrophilic substitution, 2, 49 Emmert reaction, 2, 276 food preservative, 1,411 free radical acylation, 2, 298 free radical alkylation, 2, 45, 295 free radical amidation, 2, 299 free radical arylation, 2, 295 Friedel-Crafts reactions, 2, 208 Friedlander synthesis, 2, 70, 443 fluorination, 2, 199 halogenation, 2, 40 hydrogenation, 2, 45, 284-285, 327 hydrogen-deuterium exchange, 2, 196, 286 hydroxylation, 2, 325 iodination, 2, 202, 320 ionization constants, 2, 172 IR spectra, 2, 18 lithiation, 2, 267... 

Expression of the extent of dissociation of an electrolyte the negative logarithm of a compounds ionization constant. 

Long, F. A. Ballinger, P, Acid ionization constants of alcohols in the solvents water and deuterium oxide, in Pesce, B. (ed.), Electrolytes, Pergamon Press, New York, 1962, pp. 152-164. 

J Cai, JT Smith, Z El Rassi. Determination of the ionization constants of weak electrolytes by capillary zone electrophoresis. J. High Resolut. Chromaogr. 15 30-32 (1992). 

The papers in the second section deal primarily with the liquid phase itself rather than with its equilibrium vapor. They cover effects of electrolytes on mixed solvents with respect to solubilities, solvation and liquid structure, distribution coefficients, chemical potentials, activity coefficients, work functions, heat capacities, heats of solution, volumes of transfer, free energies of transfer, electrical potentials, conductances, ionization constants, electrostatic theory, osmotic coefficients, acidity functions, viscosities, and related properties and behavior. 

The equilibrium constant for the ionization of a weak electrolyte usually is designated as Ku which we call the ionization constant. 

Calculate the ionization constants for each of the weak electrolytes in the following table, using the experimental data given. 

This equation involves the assumption that mobilities of the ions coming from the electrolyte are constant from infinite dilution to the concentration in question. From the degree of dissociation and the concentration, the ionization constant or protolysis constant of a weak electrolyte can be obtained. 

A method for the calculation of the surface hydroxyl group ionization constants, based on the zeta potential vs. pH dependence was proposed by Sprycha [115]. This method is based on the following assumptions for the symmetric 1 1 electrolytes pzc agrees with iep, and for lower than... 

In dilute aqueous solutions, the three halides, HC1, HBr, and HI, are essentially fully ionized, but in the poorer ionizing solvent, methanol, ionization is partial. In the latter solvent, HC1 is the most weakly ionized of the three whereas HI is the most strongly ionized this order of acidities has already been discussed (p. 90 see also Exercise 14). The ionization constant for hydrofluoric acid in dilute solutions is 7.2 X 10 4, but in very concentrated solutions the degree of ionization appears to rise sharply, a behavior opposite to that of almost all other weak electrolytes. This increase in acid strength is almost certainly due to the increase in concen-... 

In this experiment we shall be concerned with electrical condnction through aqueons soln-tions. Although water is itself a very poor conductor of electricity, the presence of ionic species in solution increases the condnctance considerably. The conductance of snch electrolytic solutions depends on the concentration of the ions and also on the natnre of the ions present (through their charges and mobilities), and condnctance behavior as a fnnction of concentration is different for strong and weak electrolytes. Both strong and weak electrolytes will be studied at a number of dilute concentrations, and the ionization constant for a weak electrolyte can be calculated from the data obtained. 

Rochow " (1952-1957) laboratories the dissociation of alkylchlorostannanes in water and in organic solvents was studied extensively. The solutions of ethyl- and methylhalostannanes in water, in lower alcohols, in acetone and in pyridine displayed comparatively efficient electrolytic conduction, but their conductivity in ether, nitrobenzene and nitromethane was insignificant . The ionization constant of Me3SnCl in EtOH was 10 at 25 Rochow and coworkers found that Me2SnCl2 was... 

Our primary objective was to develop a computational technique which would correlate the ionization constant of a weak electrolyte (e.g., weak acid, ionic complexes) in water and the ionization constant of the same electrolyte in a mixed-aqueous solvent. Consideration of Equations 8, 22, and 28 suggested that plots of experimental pKa vs. some linear combination of the reciprocals of bulk dielectric constants of the two solvents might yield the desirable functions. However, an acceptable plot should have the following properties it should be continuous without any maximum or minimum the plot should include the pKa values of an acid for as many systems as possible and the plot should be preferably linear. The empirical equation that fits this plot would be the function sought. Furthermore, the function should be analogous to some theoretical model so that a physical interpretation of the ionization process is still possible. 

In capillary electrophoresis (CE), several criteria can be applied to classify solvents [e.g., for practical purposes based on the solution ability for analytes, on ultraviolet (UV) absorbance (for suitability to the UV detector), toxicity, etc.]. Another parameter could be the viscosity of the solvent, a property that influences the mobilities of analytes and that of the electro-osmotic flow (EOF) and restricts handling of the background electrolyte (BGE). For more fundamental reasons, the dielectric constant (the relative permittivity) is a well-recognized parameter for classification. It was initially considered to interpret the change of ionization constants of acids and bases according to Born s approach. This approach has lost importance in this respect because it is based on too simple assumptions limited to electrostatic interactions. Indeed, a more appropriate concept reflects solvation effects, the ability for H-bonding, or the acido-base property of the solvent. 

Because ionization constants are equilibrium constants for ionization reactions, their values indicate the extents to which weak electrolytes ionize. At the same concentrations, acids with larger ionization constants ionize to greater extents (and are stronger acids) than acids with smaller ionization constants. From Table 18-4, we see that the order of decreasing acid strength for these five weak acids is... 

In recent years much work has been carried out, particularly by H. S. Harned and his associates, on concentration cells without liquid junction for the purpose of obtaining ionization constants of weak electrolytes. The principle involved in these investigations is as follows. Galvanic cells are set up of the form ... 

However, computations made for the purpose of determining the thermodynamic ionization constants of weak electrolytes in ethyl alcohol solutions, carried out as just described, gave curves instead of straight lines for a plot of values of — log K against Vcai indicating as at least one possibility, that the electrolytes such as HC1, NaCl, and the... 

Basic equations for almost every subfield of electrochemistry from first principles, referring at all times to the soundest and most recent theories and results unusually useful as text or as reference. Covers coulometers and Faraday s Law, electrolytic conductance, the Debye-Hueckel method for the theoretical calculation of activity coefficients, concentration cells, standard electrode potentials, thermodynamic ionization constants, pH, potentiometric titrations, irreversible phenomena. Planck s equation, and much more, a indices. Appendix. 585-item bibliography. 197 figures. 94 tables, ii 4. 478pp. 5-% x 8. ... 

If more than one salt is present, then the ionic strength is calculated from the total concentration and charges of aU the different ions. For any given electrolyte, the ionic strength will be proportional to the concentration. Strong acids that are completely ionized are treated in the same manner as salts. If the acids are partially ionized, then the concentration of the ionized species must be estimated from the ionization constant before the ionic strength is computed. Very weak acids can usually be considered to be nonionized and do not contribute to the ionic strength. 

Elistorically, the equilibrium ratio Kc for ionization reactions has been called the ionization constant or the dissociation constant clearly, its value will depend on both die totd electrolyte concentration and the solvent. 

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