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Ostwalds Dilution Law

From the point of view of quantitative analysis, sufficiently accurate values for the ionisation constants of weak monoprotic acids may be obtained by using the classical Ostwald Dilution Law expression the resulting constant is sometimes called the concentration dissociation constant . [Pg.31]

The first theory of solutions of weak electrolytes was formulated in 1887 by S. Arrhenius (see Section 1.1.4). If the molar conductivity is introduced into the equations following from Arrhenius concepts of weak electrolytes, Eq. (2.4.17) is obtained, known as the Ostwald dilution law this equation... [Pg.13]

If (31) is introduced into (30), one obtains an expression analogous to the Ostwald Dilution Law ... [Pg.246]

Ostwald dilution law phys chem The law that for a sufficiently dilute solution of univalent electrolyte, the dissociation constant approximates o d( - a), where c is the concentration of electrolyte and [Pg.272]

Many substances dissolve in liquid sulfur dioxide to yield ionic, conducting solutions. It has been found that such conductance data extrapolated to very high dilution yield the limiting conductance of sulfur dioxide. Both the Ostwald dilution law and the law of independent mobility of ions hold for strong" electrolytes in highly dilute solutions. [Pg.500]

The actual molar conductivity Am relates to the hypothetical molar conductivity of a fully ionized electrolyte A m by Am = aA m, which can be approximated for low electrolyte concentration to Am = aA°m. The relation 1/a = 1 + aCIKd leads to the well-known Ostwald dilution law [30] ... [Pg.29]

The concept of employing free acids as eluents dates back to the investigations of Fritz et al. [67]. In 1981, they already demonstrated that free benzoic acid may be employed as eluent instead of the sodium or potassium salts that were utilized until then. This is understandable, taking into account that benzoic acid is partially dissociated in aqueous solution. The degree of dissociation may be calculated from the dissociation constant Ka according to the Ostwald dilution law [54] ... [Pg.104]

ACID-BASE EQUILIBRIA IN WATER OSTWALDS DILUTION LAW... [Pg.141]

How well this Ostwald dilution law holds for solutions of acetic acid is shown in Table II. In this table the first column contains... [Pg.56]

Acetic acid is a relatively weak acid, i. e., its solutions conduct rather poorly. Let us examine the application of the Ostwald dilution law... [Pg.56]

Careful studies of the conductances of weak acids, and salts of weak acids in methyl and ethyl alcohol have been made by Goldschmidt and associates.11"15 They were, in general, interpreted by the authors in terms of the Ostwald dilution law, equation (17), Chapter 3,... [Pg.362]

Plot A against c. If Ao — 362, are these values in accord with the Ostwald dilution law What is the value of the dissociation constant ... [Pg.288]

Ostwald dilution law - A relation for the concentration dependence of the molar conductivity A of an electrolyte solution. [Pg.112]

After the Arrhenius theory was first proposed, an attempt was made to fit all conductance data to the Ostwald dilution law. It soon became apparent that many substances did not conform to this law. These substances are the strong electrolytes, which are completely dissociated into ions. The discussion of the dependence of the molar conductivity of strong electrolytes on concentration is based on the ideas contained in the Debye-Hiickel theory. [Pg.774]

The large ionic interaction often renders the Onsager equation useless (it is still presumably correct) for the extrapolation to obtain A . The solutions for which the Onsager relation is valid are so dilute that it is not possible to obtain reliable measurements of their conductivity. In these cases, special methods of obtaining A are used. If the electrolyte is weakly dissociated, then the A can be obtained by application of the Ostwald dilution law, modifying it in precise work to correct for the interionic forces. [Pg.786]

According to the ionic theory, the relative strengths of different bases are given by the ionization constants as calculated from the Ostwald dilution law, these depending upon the concentrations of ionized and un-ionized substances present in solution. The equation for calculating the ionization constant (which naturally should hold for all substances in solution, not merely bases) is as follows for a substance BA, ionizing into B" " and A ... [Pg.53]

The structures of organic acids as deduced from their ionization constants in aqueous solutions will be developed. The ionization constants K X 10 ) of the acids as calculated from the Ostwald dilution law. [Pg.173]

Osmotic pressure (IT) - The excess pressure necessary to maintain osmotie equilibrium between a solution and the pure solvent separated by a membrane permeable only to the solvent. In an ideal dilute solution n = c RT, where Cb is the amount-of-substance concentration of the solute, is the molar gas constant, and T the temperature. [1,2] Ostwald dilution law - A relation forthe concentration dependence ofthe molar conductivity A of an electrolyte solution, viz.,... [Pg.112]

E W. OSTWALD (1853-1932) publishes a law, which later became known as Ostwalds dilution law (1888) Z physik Chem 2 36 ( )... [Pg.340]

Because of the low degree of dissociation, the concentration of ion pairs is practically always identical to the total initiator concentration, i.e., [NaP] [C ]. With this relation and the Ostwald dilution law,f equation... [Pg.652]

Shortly afterwards Ostwald published a paper (12) in which, by applying equilibrium theory to the dissociation process, he obtained the relationship between conductivity and concentration that we now refer to as the Ostwald dilution law. ... [Pg.66]


See other pages where Ostwalds Dilution Law is mentioned: [Pg.996]    [Pg.104]    [Pg.1265]    [Pg.155]    [Pg.441]    [Pg.287]    [Pg.56]    [Pg.343]    [Pg.774]    [Pg.145]    [Pg.150]   
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