Electrical Conductivity Of Aqueous Solutions Research Articles

Additions and Corrections - Electrical Conductance of Aqueous Solutions. I. Sodium and Potassium Bromates at 25°, and Conductance of the Bromate Ion.

Additions and Corrections - Electrical Conductance of Aqueous Solutions. I. Sodium and Potassium Bromates at 25°, and Conductance of the Bromate Ion.

Electrical Conductance of Aqueous Solutions. I. Sodium and Potassium Bromates at 25°, and the Conductance of the Bromate Ion

Electrical Conductance of Aqueous Solutions. I. Sodium and Potassium Bromates at 25°, and the Conductance of the Bromate Ion

Studies on High Molecular Weight Aliphatic Amines and their Salts. VI. Electrical Conductivities of Aqueous Solutions of the Hydrochlorides of Octyl-, Decyl-, Tetradecyl- and Hexadecylamines

Studies on High Molecular Weight Aliphatic Amines and their Salts. VI. Electrical Conductivities of Aqueous Solutions of the Hydrochlorides of Octyl-, Decyl-, Tetradecyl- and Hexadecylamines

Studies on High Molecular Weight Aliphatic Amines and their Salts. IV. Electrical Conductivities of Aqueous Solutions of the Hydrochlorides and Acetates of Dodecyl-and Octadecylamines1

Studies on High Molecular Weight Aliphatic Amines and their Salts. IV. Electrical Conductivities of Aqueous Solutions of the Hydrochlorides and Acetates of Dodecyl-and Octadecylamines¹

150. The electrical conductivities of aqueous solutions of some phenanthrenesulphonic acids

The first page of this article is displayed as the abstract.

The electrical conductivities of aqueous solutions of sodium dodecyl sulphate and sodium hexadecyl sulphate at different temperatures

The classical work of McBain on the electrical conductivity and other properties of aqueous solutions of the soaps led him to postulate the formation of the ionic micelle. This aggregate of ions has a greater mobility than that of the ions composing it, and its formation accounts for the characteristic increase in conductivity exhibited by colloidal electrolytes. The conception has resulted in great advance in the study of all classes of colloidal electrolytes e. g ., protein and gelatine salts, dyes, and other substances of high molecular weight.

XLVIII.Revised figures for the electrical conductivity of aqueous solutions of sodium and potassium hydroxides, and the limiting mobility of the hydroxyl ion at25°

XLVIII.<i>Revised figures for the electrical conductivity of aqueous solutions of sodium and potassium hydroxides, and the limiting mobility of the hydroxyl ion at</i>25°

IV.The electrical conductivities of aqueous solutions of sodium and potassium hydroxides at25°and the validity of the “Water Correction.”

IV.<i>The electrical conductivities of aqueous solutions of sodium and potassium hydroxides at</i>25°<i>and the validity of the “Water Correction.”</i>

XXXV.The electrical conductivity of aqueous solutions of sodium and potassium hydroxides and the limiting mobility of the hydroxyl ion at 25°

XXXV.<i>The electrical conductivity of aqueous solutions of sodium and potassium hydroxides and the limiting mobility of the hydroxyl ion at 25°</i>

The dissociation of acids in methyl and in ethyl alcohol

A comparison-of the electrical conductivities of aqueous solutions of salts and acids reveals a striking contrast between these two classes of substances as regards their electrolytic dissociation. In water almost all salts are largely dissociated into ions and, when no complications are introduced by hydrolysis, the conductivities of dilute salt solutions show remarkably good agreement with the theory of Debye and Hüekel as modified by Onsager. Acids, on the other hand, show a wide variation in their degree of dissociation and very few behave as strong electrolytes. This difference in behaviour between salts and acids is usually explained by the properties of the proton, which, unlike other cations, has no screen of electrons round the nucleus, and therefore is assumed to be incapable of existing uncombined in solution, There is much evidence direct and indirect in support of this view, and it seems probable that in water the proton is united with one molecule of solvent to form what Brönsted calls the oxonium ion OH 3 + . In fact, the degree of dissociation of an acid probably depends on the relative affinity of the proton for the anion and for the solvent molecule. Brönsted has developed this idea in a series of recent papers on acid and basic catalysis and considers both the anion and the solvent molecule as bases in consequence of their power of combining with protons. If the ionisation of acids is dependent on the chemical attraction of the solvent molecule for the proton, it is of interest to know how the ionisation varies in different solvents. Goldschmidt has made a detailed study of the conductivity and catalytic properties of certain acids in methyl and ethyl alcohol, and finds that the halogen hydracids behave as strong electrolytes both in aqueous and alcoholic solutions, whereas weak acids such as salicylic acid become much weaker in alcohol, their dissociation constants in methyl alcohol being smaller than in water by a factor of 10 -5 . Small additions of water to the alcoholic solutions of the halogen hydracids cause a relatively large diminution in their conductivity and catalytic properties in consequence of the reaction:— H + . ROH + H 2 O ⇆ H + . H 2 O + ROH the water molecule having a much stronger affinity than the alcohol for the proton. This accounts also for the dissociation of weak acids being greater in water than in alcohol.

XXIII.—Molecular structure in solution. Part IV. The densities, viscosities, and electrical conductivities of aqueous solutions of cobalt chloride and hydrochloric acid at different temperatures

XXIII.—Molecular structure in solution. Part IV. The densities, viscosities, and electrical conductivities of aqueous solutions of cobalt chloride and hydrochloric acid at different temperatures

CCCLXXX.—Molecular structure in solution. Part III. The electrical conductivities of aqueous solutions of cobalt chloride and hydrochloric acid, with a note on the prediction of crystal structure

CCCLXXX.—Molecular structure in solution. Part III. The electrical conductivities of aqueous solutions of cobalt chloride and hydrochloric acid, with a note on the prediction of crystal structure

The Electrical Conductivity of Aqueous Solutions . A report presented by Arthur A. Noyes, W. D. Coolidge, A. C. Melcher, H. C. Cooper, Yogoro Kato, R B. Sosman, G. W. Eastman, C. W. Kanolt and W. Böttger. .Contribution from the Research Laboratory of Physical Chemistry of the Massachusetts Institute of Technology No. 19. Carnegie Institution of Washington, Publication No. 63.

<i>The Electrical Conductivity of Aqueous Solutions</i> . A report presented by Arthur A. Noyes, W. D. Coolidge, A. C. Melcher, H. C. Cooper, Yogoro Kato, R B. Sosman, G. W. Eastman, C. W. Kanolt and W. Böttger. .Contribution from the Research Laboratory of Physical Chemistry of the Massachusetts Institute of Technology No. 19. Carnegie Institution of Washington, Publication No. 63.

The Electrical Conductivity of Aqueous Solutions at High Temperatures. I. Description of the Apparatus. Results with Sodium and Potassium Chloride up to 306°

The Electrical Conductivity of Aqueous Solutions at High Temperatures. I. Description of the Apparatus. Results with Sodium and Potassium Chloride up to 306°

VII.—An extension of Mendeléeff's theory of solution to the discussion of the electrical conductivity of aqueous solutions

VII.—An extension of Mendeléeff's theory of solution to the discussion of the electrical conductivity of aqueous solutions

Scientific Serials

Annalen der Phvsikund Chemie, No. 1, 1879.—This begins with a portion of an extended inquiry by Herr F. Kohlrausch into the electric conductivity of aqueous solutions of hydrates and salts of the light metals, as also of sulphate of copper, sulphate of zinc, and nitrate of silver. The paper is in three parts—an experimental, a practical, and a theoretical (the first two in this number). The practical part gives tables for use, and formulae of conductivity, especially of dilute solutions; specifies bodies which show a maximum of conducting power at a degree of concentration of solution below saturation, indicates liquids which commend themselves as a standard for electric conductivity, &c.—Herr W. Kohlrausch furnishes an experimental determination of the velocities of light in crystals. He employed the new instrument called a total reflectometer, and he comes to the conclusion that Fresnel's theory of double refraction in optically uni- and biaxial crystals gives a form of light wave-surfaces, which, within very small errors of measurement, is in general experimentally confirmed for uniaxial crystals, and for the principal sections of biaxial crystals.—Herr Groshaus contributes some interesting observations on the densities of substances in the gaseous and liquid states, in relation to their chemical composition.—Herr Ritter calculates that the quantity of heat radiated annually from the sun 75,000 years ago must have been about 1 per cent, less than at present (700,000 years ago about 10 per cent, less), a result which is supposed to explain the “glacial period,” while the previous tropical climate is accounted for by a less thickness of the solid cru it of the earth. He also estimates that each kilogramme of the sun's mass contains on an average about 43,000,000 units of heat.—Herr Wiedemann declines to regard the oxide containing copper separated electro-lytically from solutions of acetate of cupric oxide, as a peculiar allotropic modification of copper.—There are also papers on the thermo-electric properties of apatite, brucite, &c. (Hankel), the theory and application of electro-magnetic rotation (Margules), the influence of temperature on galvanic conductivity of liquids (Exner and Goldschmiedt), and two new fluorescent substances (Lommel).