Solubility parameters: Part II

Metal Finishing

Volumn 102, Issue 4, 2004, Pages 42-50

  Durkee II, John B ^a  

^a Creative EnterpriZes   (United States)

Author keywords

[No Author keywords available]

Indexed keywords

BENZENE; COATINGS; DATA ACQUISITION; HEPTANE; PROBLEM SOLVING; SOLVENTS; SURFACE TENSION; TOLUENE; VAPORIZATION;

COHESIVE ENERGY DENSITY; HANSEN SOLUBILITY PARAMETERS (HSP); INTERMOLECULAR FORCES; SOLUBILITY PARAMETERS;

SOLUBILITY;

EID: 23944436966     PISSN: 00260576     EISSN: None     Source Type: Journal    
DOI: 10.1016/S0026-0576(04)90238-3     Document Type: Note

References (19)

1. Professor of Chemistry at the University of California Berkeley, awarded the A.C.S.'s highest recognition, the Priestley Medal in 1962. Elected President of the Sierra Club (1937-1940), appointed manager of the U.S. Olympic Ski Team in 1936, discovered that the solubility of helium was much less than that of nitrogen at a given pressure, which led to use of helium and oxygen mixtures for deep underwater diving. Authored classic books such as The Solubility of Nonelectrolytes and Regular and Related Solutions: the Solubility of Gases, Liquids, and Solids. Joel Henry Hildebrand was apparently a very good guy (1881-1983).
2. Hildebrand, J. and R.L. Scott, Regular Solutions, Prentice-Hall, Englewood Cliffs, NJ.; 1962
3. Please recall that, for ideal gasses, PV = RT.
4. Barton, A., CRC Handbook of Solubility Parameters and Other Cohesion Parameters, 2nd edition; 1991
5. Johannes van der Waals first described them in 1873. These forces do not bind together quantum particles in atoms. They exist between and among molecules of the same substance. Some thought these forces were small gravitational attractions. Van der Waals forces are actually due to electromagnetic interactions between molecules.
6. A dipole is a pair of magnetic poles, each with opposite charge, separated by a short distance.
7. Perhaps one tenth the strength of a covalent bond. Please see http://www.physlink.com/Education/AskExperts/ae206.cfm.
8. There is no OH bond in ketones, or ethers.
9. The degree of "polarity" that these temporary dipoles confer on a molecule is related to surface area. Larger molecules have a greater number of temporary dipoles and greater intermolecular attractions. Molecules with straight chains have more surface area, and thus greater dispersion forces, than branched-chain molecules of the same molecular weight. These induced attractions are also called London dispersion forces, or induced dipole-induced dipole forces. Please see http://www.stanford.edu/byauth/burke/solpar/solpar4. html.
10. A pioneer, from the mid-1960s through today in the quantification of formulation of paints, coatings, inks, etc. His list of technical publications contains more than 100 entries. Dr. Hansen is Senior Scientist at Force Technology, Park Allé 345, 2605 Brønby, Denmark, and can be reached at cmh@force.dk. And Charles Medom is also a good guy who has been kind enough to review this article.
11. Hansen, C.M., Hansen Solubility Parameters - a User's Handbook, page 3, CRC Press, New York; 2000
12. His initial work was trial and error. Today HSPs are determined solely on experiments or calculations using the data one can find for latent heat, dipole moment, group contributions, etc.
13. THOUGH THEY ARE OF IMMENSE THEORETICAL VALUE.
14. Hansen, C.M., "The Three Dimensional Solubility Parameter - Key to Paint Component Affinities," International Journal of Paint Technology, 305(511):104-117, 505-510; 1967
15. Blanks, R.F., J.M. Prausnitz, "Thermodynamics of Polymer Solubility in Polar and Nonpolar Systems," Industrial and Engineering Chemistry Fundamentals, 3(1):1-8;1964
16. Hansen, C.M. and K. Skaarup, "The Three Dimensional Solubility Parameter - Key to Paint Component Affinities," International Journal of Paint Technology, 305(511):511-514; 1967
17. Data and table from http://sul-server-2.stanford.edu/byauth/burke/solpar/ solpar6.html.
18. Hansen, C.M., Hansen Solubility Parameters - a User's Handbook, pages 168-185, CRC Press, New York; 2000
19. A unique one will be to devise a single characteristic will be able to separate / predict toxic and nontoxic solvents. An interesting and lengthy paper on this topic can be found at http://www.aber.ac.uk/~abcwww/gjsalter/solv15.htm