Enthalpies of mixing and complex formation of carbon tetrachloride with some methyl-substituted benzenes. Part II

1969 ◽  
pp. 2489 ◽  
Author(s):  
P. J. Howell ◽  
D. Stubley
Keyword(s):  
Carbon Tetrachloride ◽  
Complex Formation ◽  
Substituted Benzenes ◽  
Enthalpies Of Mixing

COMPLEXES OF STANNIC IODIDE WITH AROMATIC HYDROCARBONS

1965 ◽  
Vol 43 (5) ◽  
pp. 1272-1278 ◽  
Author(s):  
J. F. Murphy ◽  
D. E. Baker
Keyword(s):  
Carbon Tetrachloride ◽  
Complex Formation ◽  
Aromatic Hydrocarbon ◽  
Aromatic Hydrocarbons ◽  
Extinction Coefficient ◽  
Regular Solutions ◽  
Benzene Toluene ◽  
Yield Values ◽  
Complex Stabilities ◽  
Iodide Complex

Spectrophotometric measurements on solutions of stannic iodide were found to provide evidence for complex formation with aromatic hydrocarbons. Calculations, based on spectra for mixed solutions of benzene and stannic iodide in carbon tetrachloride, yield values of 0.26 for the equilibrium constant (mole fraction), 28 400 1/mole cm for the molar extinction coefficient of the benzene – stannic iodide complex. Kinetic evidence indicates that the order of decreasing complex stabilities is from xylene to toluene to benzene. The formation of stannic iodide – aromatic hydrocarbon complexes provides an explanation for the discrepancy between measured solubilities of stannic iodide in benzene, toluene, and xylene, and the solubilities predicted by the Hildebrand theory of regular solutions.

Complex formation of hexakis(2,3,6-tri-O-methyl)-?-cyclodextrin with substituted benzenes in aqueous solution

1988 ◽  
Vol 6 (2) ◽  
pp. 135-142 ◽  
Author(s):  
Kazuaki Harata ◽  
Keishiro Tsuda ◽  
Kaneto Uekama ◽  
Masaki Otagiri ◽  
Fumitoshi Hirayama
Keyword(s):  
Aqueous Solution ◽  
Complex Formation ◽  
Substituted Benzenes

Factor analysis as a complement to band resolution. V. Complexing of pentachlorophenol and acetone in carbon tetrachloride solution

1978 ◽  
Vol 56 (23) ◽  
pp. 2959-2965 ◽  
Author(s):  
J. Korppi-Tommola ◽  
H. F. Shurvell
Keyword(s):  
Factor Analysis ◽  
Carbon Tetrachloride ◽  
Complex Formation ◽  
Infrared Spectrum ◽  
Equilibrium Constants ◽  
Complex Model ◽  
Carbon Tetrachloride Solution ◽  
Linear Relationships

Complex formation between pentachlorophenol and acetone and acetone-d6 in carbon tetrachloride solution has been studied in both the hydroxyl and carbonyl stretching regions of the infrared spectrum. Factor analysis of the digitized spectra indicates three absorbing components for each set of solutions in the hydroxyl stretching region. Concentration studies revealed roughly linear relationships between the areas of the 'free' ν(OH) band and both of the resolved complex bands, suggesting that two different 1:1 complexes occur in CCl4 solution. In the ν(CO) region only one band due to complex formation was detected. Equilibrium constants for the isotopically different complexes at about 30 °C are reported. In the hydroxyl stretching region, band resolution was also carried out using four components which gave a better fit to the observed spectrum. A set of equilibrium constants were then obtained. However, considerable difficulties were met in the calculations and in the interpretation of these results, so that the three band, two complex model is preferred.

THE ENERGY OF HYDROGEN BONDING IN THE SYSTEM: ACETONE–CHLOROFORM

1960 ◽  
Vol 38 (5) ◽  
pp. 652-655 ◽  
Author(s):  
A. N. Campbell ◽  
E. M. Kartzmark
Keyword(s):  
Hydrogen Bonding ◽  
Solid State ◽  
Carbon Tetrachloride ◽  
Enthalpies Of Mixing

It is shown that(1) acetone and chloroform form a compound stable in the solid state;(2) acetone and carbon tetrachloride do not form a compound;(3) the enthalpies of mixing of acetone and chloroform and of acetone and carbon tetrachloride have been determined;(4) from these figures the energy of hydrogen bonding in the acetone–chloroform system is evaluated as 2.7 kcal ± 0.1.

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