Apparent molal volumes of aqueous solutions of bis-tetraalkylammonium salts at 25�C: Methylene-group contribution to the limiting molal volume

1977 ◽  
Vol 6 (9) ◽  
pp. 581-587 ◽  
Author(s):  
Patrick Carpenter ◽  
Siegfried Lindenbaum
Keyword(s):  
Aqueous Solutions ◽  
Group Contribution ◽  
Tetraalkylammonium Salts ◽  
Molal Volume ◽  
Apparent Molal Volumes ◽  
Molal Volumes ◽  
Methylene Group

Thermodynamic Properties of Aqueous Organic Solutes in Relation to their Structure. Part II. Apparent Molal Volumes and Heat Capacities of c-Alkylamine Hydrobromides in Water

1975 ◽  
Vol 53 (5) ◽  
pp. 716-722 ◽  
Author(s):  
Carmel Jolicoeur ◽  
Jeanine Boileau ◽  
Serge Bazinet ◽  
Patrick Picker
Keyword(s):  
Heat Capacities ◽  
Group Contribution ◽  
Ring Size ◽  
Solvent Structure ◽  
Apparent Molal Volumes ◽  
Molal Volumes ◽  
The Difference ◽  
Geometrical Factors ◽  
Cyclic Compounds ◽  
Methylene Group

The density and specific heat of aqueous solutions of various c-alkylamine hydrobromides, and of n-dodecylammonium bromide, have been measured at 25 °C. The limiting apparent molal volumes [Formula: see text] and heat capacities [Formula: see text] derived from these data, are compared to the corresponding quantities for n-alkylammonium and immonium salts. The methylene group contribution to[Formula: see text] and [Formula: see text] of the cyclic compounds is generally lower than that of the linear homologs; this group contribution is also found to depend markedly on ring size, in contrast to monotonous variations found in the series of the linear compounds. The difference is suggested to originate in solvation effects in which geometrical factors (solvent structure and solute geometry) play a significant role.

Effect of pressure on apparent molal volumes of nonionic surfactants in aqueous solutions

1980 ◽  
Vol 73 (1) ◽  
pp. 124-129 ◽  
Author(s):  
Shoji Kaneshina ◽  
Minoru Yoshimoto ◽  
Hideki Kobayashi ◽  
Nagamune Nishikido ◽  
Gohsuke Sugihara ◽  
...  
Keyword(s):  
Aqueous Solutions ◽  
Nonionic Surfactants ◽  
Effect Of Pressure ◽  
Apparent Molal Volumes ◽  
Molal Volumes

Apparent molal heat capacities and volumes of aqueous electrolytes at 25 °C: NaClO3, NaClO4, NaNO3, NaBrO3, NaIO3, KClO3, KBrO3, KIO3, NH4NO3, NH4Cl, and NH4ClO4

1978 ◽  
Vol 56 (1) ◽  
pp. 24-28 ◽  
Author(s):  
Alain Roux ◽  
Goolam M. Musbally ◽  
Gérald Perron ◽  
Jacques E. Desnoyers ◽  
Prem Paul Singh ◽  
...  
Keyword(s):  
Aqueous Solutions ◽  
Infinite Dilution ◽  
Heat Capacities ◽  
Aqueous Electrolytes ◽  
Apparent Molal Volumes ◽  
Hückel Theory ◽  
Standard Values ◽  
Molal Volumes ◽  
Apparent Molal Heat Capacities

Measurements at 25 °C with flow calorimeters and densimeters have led to heat capacities and densities of aqueous solutions of 11 1:1 electrolytes: NaClO3, NaBrO3, NaIO3, NaNO3, NaClO4, NH4NO3, KClO3, KBrO3, KIO3, NH4Cl, and NH4ClO4. The first 6 salts were studied up to near saturation. We have used results of these measurements to obtain apparent molal heat capacities and apparent molal volumes of the various solutes. Extrapolation to infinite dilution on the basis of the Debye–Hückel theory bas led to [Formula: see text]and [Formula: see text] values for each solute. We have compared these standard values with results of earlier investigations.

Salting-in and salting-out of polar nonelectrolytes

1969 ◽  
Vol 47 (24) ◽  
pp. 4639-4643 ◽  
Author(s):  
J. E. Desnoyers ◽  
F. M. Ichhaporia
Keyword(s):  
Benzoic Acid ◽  
Aqueous Solutions ◽  
Salting Out ◽  
Apparent Molal Volumes ◽  
Volumes Of Mixing ◽  
Molal Volumes

The solubility of toluene and benzaldehyde was measured in NaBr and (n-Pr)4NBr aqueous solutions at 25 °C, and the solubility of benzoic acid and nitrobenzene was measured in the same systems at 10, 25, and 40 °C. The apparent molal volumes of the four nonelectrolytes were also determined from the densities of the saturated aqueous solutions.The volumes of mixing of the nonelectrolytes in water are all negative but become less so as their polarity increases. With the exception of benzoic acid, the salting-out by NaBr and the salting-in by (n-Pr)4NBr both decrease with increasing polarity of the nonelectrolytes. Both salting effects increase with temperature. These trends can be explained with existing theories of salting-out and salting-in.

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