Electrolytic nature of aqueous sulfuric acid. 2. acidity

Journal of Physical Chemistry B

Volumn 116, Issue 38, 2012, Pages 11678-11686

  Fraenkel, Dan ^a  

^a Eltron Research & Development Inc   (United States)

Author keywords

[No Author keywords available]

Indexed keywords

DISSOCIATION; ELECTROLYTES; EQUILIBRIUM CONSTANTS; TITRATION;

BASE NEUTRALIZATION; DISSOCIATION CONSTANT; HAMMETT ACIDITY FUNCTION; HIGH CONCENTRATION; LOW CONCENTRATIONS; MEAN IONIC ACTIVITY COEFFICIENT; REACTION PATHWAYS; STRONG ELECTROLYTE SOLUTIONS; TITRATION CURVES;

SULFURIC ACID;

EID: 84866847484     PISSN: 15206106     EISSN: 15205207     Source Type: Journal    
DOI: 10.1021/jp306042q     Document Type: Article

References (18)

1. Fraenkel, D. J. Phys. Chem. B 2012, 116, DOI: 10.1021/jp3060334.
2. Fraenkel, D. J. Phys. Chem. B 2011, 115, 557-568
3. Fraenkel, D. J. Phys. Chem. B 2011, 115, 14634-14647
4. Fraenkel, D. Mol. Phys. 2010, 108, 1435-1466
5. Sakaida, H.; Kakiuchi, T. J. Phys. Chem. B 2011, 115, 13222-13226
6. Fraenkel, D. J. Phys. Chem. B 2012, 116, 3603-3612
7. CRC Handbook of Chemistry and Physics, 82 nd ed.; Lide, D. R., Ed.-in-Chief; CRC Press: Boca Raton, FL, 2001-2002.
8. Rochester, C. H. Acidity Functions; Academic Press: London, 1970.
9. Hammett, L. P. Physical Organic Chemistry, 2 nd ed.; McGraw-Hill: New York, 1970.
10. Paul, M. A.; Long, F. A. Chem. Rev. 1957, 57, 1-45
11. Bascombe, K. N.; Bell, R. P. J. Chem. Soc. 1959, 1096-1104
12. Bascombe, K. N.; Bell, R. P. Discuss. Faraday Soc. 1957, 24, 158-161
13. See, e.g.: http://www.titrations.info/acid-base-titration-sulfuric-acid.
14. King, E. J. Acid-Base Equilibria; The Macmillan Co.: New York, 1965.
15. Robinson, R. A.; Stokes, R. H. Electrolyte Solutions, 2 nd ed.; Dover Publications: Mineola, NY, 2002.
16. Harned, H. S.; Owen, B. B. The Physical Chemistry of Electrolytic Solutions, 3 rd ed.; Reinhold Publishing Co.: New York, 1958.
17. Butler, J. N. Ionic Equilibrium; John Wiley & Sons, Inc: New York, 1998. See, e.g., Figure 3.6 in this reference.
18. Cl- is 0.7633, and even at 0.01 M, the activity coefficients of the proton and the chloride are still substantially different: 0.9083 and 0.9003, respectively