Dielectric Constants of Methyl Alcohol—Benzene Mixtures

LaRochelle, John H.; Vernon, Arthur A.

doi:10.1021/ja01163a522

Cited by 13 publications

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“…BH+...B + B^BH+...B2. (57) Formation of BH + ...B2 is expected only when at least two cationic protons are available for hydrogen bonding to B.…”

Section: Ch3cn Ch2cncmentioning

confidence: 99%

Acid-base behavior in aprotic organic solvents

Davis¹

1968

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Butyl hydroperoxide and deuteroperoxide. Deuterium isotope effects on hydrogen bonding by Br0nsted acids 40 4.3. Hydrogen-bonded ion pairs 41 4.3.1. Conductance 41 a. Walden's work 42 b. Wynne-Jones' postulate 42 c. Investigations of Kraus, Fuoss, and associates... 43 d. Summary 45 4.3.2. Dielectric constants 46 a. Dielectric polarization of substituted ammonium picrates and halides in benzene 46 b. Dielectric polarization of other acid-base complexes in benzene 47 4.3.3. CoUigative properties 49 a. Cryoscopy 50 Page b. The differential vapor pressure (DVP) method... 51 104 4.5.6. Homoconjugation of other organic and inorganic acids a. Perchloric acid 105 b. Other acids 105 4.5.7. Heteroconjugate anions 105 a. Chemical behavior 105 b. Physical measurements 108 4.6. Concluding discussion of hydrogen bonding 112 4.6.1. Definition of a hydrogen bond. Systems which form hydrogen bonds 112 4.6.2! Some recent concepts of hydrogen bonding 113 5. Acidity and basicity scales in aprotic organic solvents... 114 5.1. Early attempts to determine relative acidities 114 5.2. Log Kbha scales of acidity and basicity 115 5.3. Methods used in determining values of log A^bha 116 5.4. Tables of log ^bha, and AS obtained using aprotic solvents 118 5.4.1. Aromatic and substituted aromatic hydrocarbons 118 a. Benzene 118 b. Anisole and chlorobenzene 126 5.4.3. Carbon tetrachloride 126 5.4.4. Chloroform 128 5.4.5. Miscellaneous aprotic solvents 129 6. Acid-base titrations in completely aprotic solvents 133 6.1. Introduction 133 6.2. Titrations with indicator dyes in completely aprotic solvents 133 6.3. Instrumental procedures for detecting end-points in completely aprotic solvents 133 6.3.1. Conductance titrations 133 iv Contents -Continued Page 6.3.2. Dielectrometric titrations 133 6.3.3. Photometric titrations 134 6.3.4. Thermometric titrations 135 6.3.5. Titrations by the DVP method 135 6.3.6. Cryoscopic titrations 135 6.3.7. Other possible instrumental procedures 135 a. Refractive index 135 b. Density 135 c. Optical rotation 135 6.4. Reference acids and bases for aprotic organic solvents 135 6.4.1. Acids 135 a. Hydrogen chloride 135

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“…BH+...B + B^BH+...B2. (57) Formation of BH + ...B2 is expected only when at least two cationic protons are available for hydrogen bonding to B.…”

Section: Ch3cn Ch2cncmentioning

confidence: 99%

Acid-base behavior in aprotic organic solvents

Davis¹

1968

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“…It is believed that the most likely reasons for these difficulties are (1) effects of association reactions between methanol and benzene molecules neglected by eq [14][15][16][17] (see assumption (i)), and (2) a0 has a concentration dependence which cannot be neglected. There is evidence for interaction between methanol and benzene molecules.46 However methanol-benzene association reactions must provide a significant negative contribution to a at methanol mole fractions higher than 0.4, if their inclusion in the theory is to remove difficulties described above.…”

Section: Interpretation Of the Experimental Resultsmentioning

confidence: 99%

Thermal diffusion in mixtures with association reactions. Thermal diffusion factors for methanol-benzene mixtures

Johnson¹,

Beyerlein²

1978

J. Phys. Chem.

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Experimental studies of the temperature dependence of the thermal diffusion factor a are reported for methanol-benzene mixtures which cover the entire concentration range at temperatures 15, 25, and 35 °C. The thermal diffusion factor changes from a negative to positive sign (positive sign implies that benzene diffuses in the direction of the temperature gradient) at intermediate benzene concentrations and attains a maximum at a methanol mole fraction of about 0.07. The concentrations at which a changes sign are 0.304, 0.35, and 0.42 methanol mole fraction at 15, 25, and 35 °C, respectively. The data are interpreted in terms of the following reaction model for hydrogen bond association: (CH3OH)2 -CH3OH + CH3OH, (CH3OH)3 ^(CH3OH)2 + CH3OH,... (CH3OH)" ^(CH3OH)r 3 + CH3OH. It is concluded that the concentration corresponding to maximum a is predominantly determined by the equilibrium constants characterizing the association equilibria and is nearly independent of the diffusion properties of the associated species. Calculations based on the association reaction model indicate that when a maximizes the amount of monomeric methanol becomes approximately equal to the amount of methanol consisting of the most stable associated species. At lower methanol mole fractions the monomer rapidly becomes the dominant species.

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“…Rozsa (70) also utilized the spectrograph for tlie determination. LaRochelle and Fournier (45) and Yante and Sobers (88), respectively, described procedures for determining magnesium after separation of the iron with the mercury cathode and with an ether separation.…”

Section: Methods For the Elementsmentioning

confidence: 99%

Ferrous Metallurgy

Beeghly¹

1951

Anal. Chem.

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Dielectric Constants of Methyl Alcohol—Benzene Mixtures

Cited by 13 publications

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Acid-base behavior in aprotic organic solvents

Acid-base behavior in aprotic organic solvents

Thermal diffusion in mixtures with association reactions. Thermal diffusion factors for methanol-benzene mixtures

Ferrous Metallurgy

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