COMPOUND FORMATION IN THE SYSTEM UROTROPINE – ACETIC ACID: I. THE PHASE DIAGRAM

1947 ◽  
Vol 25b (5) ◽  
pp. 477-480 ◽  
Author(s):  
K. K. Carroll ◽  
R. H. Wright
Keyword(s):  
Phase Diagram ◽  
Acetic Acid ◽  
Freezing Point ◽  
Compound Formation ◽  
Solid Compound ◽  
Approximate Composition ◽  
Curve Maximum

The freezing point diagram has been plotted for mixtures of acetic acid and urotropine containing 0 to 42% urotropine. Formation of a solid compound melting at 24.8 °C., and having the approximate composition (C6H12N4)3∙(C2H4O2)13 is indicated. Repeated purification of the materials failed to shift the curve maximum to the expected ratio of 1 mole of urotropine to 4 moles of acetic acid.

SOME FREEZING POINT AND CONDUCTANCE MEASUREMENTS IN THE SYSTEM NITRIC ACID – ACETIC ACID

1951 ◽  
Vol 29 (6) ◽  
pp. 461-468 ◽  
Author(s):  
Edward G. Taylor ◽  
Alan G. Follows
Keyword(s):  
Acetic Acid ◽  
Nitric Acid ◽  
Freezing Point ◽  
Preliminary Investigation ◽  
Liquid System ◽  
Molecular Compound ◽  
Compound Formation ◽  
Vapor Equilibrium ◽  
Binary Azeotrope ◽  
Solid Liquid

An independent investigation of the phase diagram for the solid–liquid system nitric, acid – acetic acid has confirmed the findings of Miskidzh'yan and Trifonov (4), namely, that a 1: 1 molecular compound exists. Conductance measurements at 0°, 25°, and 40°C. have been made for the same system. It does not appear possible to predict compound formation from the conductance measurements alone. A preliminary investigation of the liquid–vapor equilibrium for the system nitric acid – acetic acid indicates the existence of a maximum boiling azeotrope. Diacetylorthonitric acid—(CH3COO)2N(OH)3—discovered by Pictet and Genequaud (8) is, in all probability, identical with this binary azeotrope. Some molecular weight measurements tend to confirm this view.

Zn:Tl PHASE DIAGRAM AT VERY LOW THALLIUM CONCENTRATIONS

1961 ◽  
Vol 39 (4) ◽  
pp. 588-595 ◽  
Author(s):  
E. H. McLaren ◽  
F. Weinberg
Keyword(s):  
Phase Diagram ◽  
Freezing Point ◽  
Solubility Limit ◽  
Heat Of Fusion ◽  
Kcal Mole ◽  
Solid Solubility Limit ◽  
Pure Zinc ◽  
Latent Heat Of Fusion ◽  
A Value ◽  
Resistance Thermometry

The Zn:Tl liquidus has been accurately determined from pure Zn (419.505 °C) to the monotectic transition temperature (416.926 °C at 0.42 at.% Tl) using precision resistance thermometry. The upper solidus was determined approximately from measurements of the distribution coefficient (~0.01) and the solid solubility limit (~0.004 at.% Tl) of thallium in zinc. A value 1.53 ± 0.1 kcal/mole for the latent heat of fusion of pure zinc was calculated from the freezing point depressions.

NOTE ON SOLID-LIQUID EQUILIBRIA IN SOME TWO-COMPONENT SYSTEMS INVOLVING HYDROGEN CYANIDE

1933 ◽  
Vol 8 (2) ◽  
pp. 114-118 ◽  
Author(s):  
A. L. Peiker ◽  
C. C. Coffin
Keyword(s):  
Hydrogen Cyanide ◽  
Freezing Point ◽  
Eutectic Type ◽  
Molecular Compound ◽  
Compound Formation ◽  
Component Systems ◽  
Two Component ◽  
Hydride Hydrogen ◽  
Two Component Systems ◽  
Solid Liquid

The freezing-point curves of the two-component systems hydrogen cyanide-water, hydrogen cyanide-formic acid, hydrogen cyanide-formamide and hydrogen cyanide-benzaldehyde have been determined. These systems are all of the simple eutectic type and show no evidence of molecular compound formation. A chemical reaction prohibited the investigation of solid-liquid equilibria in the case of halogen hydride-hydrogen cyanide systems.

Phase Diagram of Ternary Magnesium Acetate-Acetic Acid-Water System at 298.1 and 333.1 K

2007 ◽  
Vol 29 (1) ◽  
pp. 30-33
Author(s):  
Hong-Kun Zhao ◽  
Dao-Sen Zhang ◽  
Rong-Rong Li ◽  
Qiu-Hong Zhang ◽  
Cao Tang
Keyword(s):  
Phase Diagram ◽  
Acetic Acid ◽  
Water System ◽  
Acid Water ◽  
Magnesium Acetate ◽  
Acetic Acid Water
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