scholarly journals XXXII.—The Boiling and Freezing Points of Concentrated Aqueous Solutions, and the Question of the Hydration of the Solute

1908 ◽  
Vol 45 (4) ◽  
pp. 855-884 ◽  
Author(s):  
S. M. Johnston
Keyword(s):  
Aqueous Solutions ◽  
Boiling Point ◽  
Freezing Point ◽  
Conductivity Data ◽  
Concentrated Aqueous Solutions ◽  
Freezing Points ◽  
Solutions Of Electrolytes

In this paper the results of observations of the elevation of the boiling point of aqueous solutions of electrolytes are given, and a few results of observations of the depression of the freezing point, together with conductivity data obtained by observations of conductivity at about 99·4° and 0° Centigrade.

PRODUCTION AND PROPERTIES OF 2,3-BUTANEDIOL: XII. ANTIFREEZE PROPERTIES OF TERNARY AQUEOUS SOLUTIONS CONTAINING LEVO-2,3-BUTANEDIOL AS A MAJOR COMPONENT

1946 ◽  
Vol 24f (5) ◽  
pp. 287-299 ◽  
Author(s):  
K. A. Clendenning ◽  
D. E. Wright
Keyword(s):  
Ethylene Glycol ◽  
Aqueous Solutions ◽  
Boiling Point ◽  
Freezing Point ◽  
Ternary Systems ◽  
Freezing Points ◽  
Point Depressant ◽  
Point Data ◽  
Considerable Range

Freezing point, viscosity, and boiling point data are presented for aqueous solutions of levo-2,3-butanediol containing methanol, ethanol, ethylene glycol, and tetrahydrofurfuryl alcohol as third components. All four ternary systems show freezing points of −50 °C. and lower over a considerable range of compositions. Among the compounds tested as third components, methanol was most effective as a thinning agent and accessory freezing point depressant. The data indicate that 20% methanol–40% butanediol–40% water is suitable for use at temperatures as low as −50 °C.

scholarly journals IX.—On the Relationship between Concentration and Electrolytic Conductivity in Concentrated Aqueous Solutions

1906 ◽  
Vol 45 (1) ◽  
pp. 241-259 ◽  
Author(s):  
John Gibson
Keyword(s):  
Aqueous Solutions ◽  
General Relationship ◽  
Electrolytic Conductivity ◽  
Dilute Solutions ◽  
Concentrated Solutions ◽  
Concentrated Aqueous Solutions ◽  
Solutions Of Electrolytes ◽  
Weak Electrolytes ◽  
The Relationship

Although great advances have been made during the last thirty years in our knowledge of dilute solutions, there has been no corresponding advance in respect of concentrated solutions. This is primarily due to the fact that hitherto no simple and general relationship has been discovered between the conductivity and the concentration of concentrated solutions of electrolytes. Ostwald's law of dilution holds only for dilute solutions of weak electrolytes, and the formulæ of Rudolphi and Van T'Hoff are applicable only to dilute solutions of good electrolytes. It seems therefore important to inquire whether the difficulty may not be to some extent overcome by an alteration in the mode of representing the facts.

THE FREEZING POINTS OF AQUEOUS SOLUTIONS. I. A FREEZING POINT APPARATUS

1932 ◽  
Vol 54 (7) ◽  
pp. 2676-2690 ◽  
Author(s):  
George Scatchard ◽  
P. T. Jones ◽  
S. S. Prentiss
Keyword(s):  
Aqueous Solutions ◽  
Freezing Point ◽  
Freezing Points

scholarly journals VIII.—On the Elevation of the Boiling Points of Aqueous Solutions of Electrolytes

1906 ◽  
Vol 45 (1) ◽  
pp. 193-240 ◽  
Author(s):  
S. M. Johnston
Keyword(s):  
Aqueous Solutions ◽  
Vapour Pressure ◽  
Boiling Point ◽  
Volatile Substance ◽  
Boiling Points ◽  
Solutions Of Electrolytes ◽  
The Subject

It has been known for a length of time that the presence of a non-volatile substance diminishes the vapour pressure of the solvent in which it is placed, and as the boiling point of a solvent or a solution is the temperature at which the vapour pressure is just equal to, or overcomes the pressure of the atmosphere, it follows that a solution has a higher boiling point than the solvent. Amongst the first experimenters in this field were Faraday, Legrand, Griffiths, and Raoult. TO Raoult we owe much for his development of the subject.

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