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  Home > JCE Print > Journal of Chemical Education > Issues > 2001  > November  >
In the Classroom
Henderson-Hasselbalch Equation: Its History and Limitations
Henry N. Po and N. M. Senozan
Department of Chemistry and Biochemistry, California State University, Long Beach, CA 90840-3903
Cover
November 2001
Vol. 78 No. 11
p. 1499
Abstract
Many students of chemistry have wondered if putting the mass action expression in logarithmic format should have warranted immortalization of the names Henderson and Hasselbalch. With focus on this question, this article examines the evolution of the Henderson-Hasselbalch equation and presents a critical evaluation of its usefulness. The discussion centers on the titration of a weak acid with sodium hydroxide. Approximate pH values obtained from the Henderson-Hasselbalch equation are compared with exact hydrogen ion concentrations and the percentage errors are displayed as a function of the acid dissociation constant and buffer composition (titration mixture).
More Information
*  Citation
 Po, Henry N.; Senozan, N. M. J. Chem. Educ. 2001 78 1499.
*  Keywords
 Acid-Base Chemistry; Biochemistry; Equilibrium; General Chemistry; History / Philosophy
*  History
 Created:
Last Updated:		 October 8, 2001
August 31, 2005
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