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  Home > JCE Print > Journal of Chemical Education > Issues > 1998  > September  >
In the Classroom
The Ksp-Solubility Conundrum
Roy W. Clark and Judith M. Bonicamp
Department of Chemistry, Middle Tennessee State University, Murfreesboro, TN 37132
Cover
September 1998
Vol. 75 No. 9
p. 1182
Abstract
The calculation of solubility from Ksp values, and its converse have long been a part of general college chemistry textbooks. The agreement between actual solubility and simple calculations of solubility from Ksp values has been questioned many times. Incomplete dissociation, hydrolysis reactions, complex ion formation, ion pair formation and activity coefficients conspire to make such calculations crude at best. The authors sought to find those cases of partly soluble substances for which simple calculations such as Ksp=S2, and Ksp=4S3 can realistically be used for computing solubility from Ksp and the reverse calculation. Empirical solubility data are compared with solubilities calculated from reliable Ksp values that have been adjusted for activity coefficients. A table of 18 substances is suggested for textbook use.

See Letter re: this article
More Information
*  Citation
 Clark, Roy W.; Bonicamp, Judith M. J. Chem. Educ. 1998 75 1182.
*  Keywords
 aqueous solution chem, curriculum, equilibrium, teaching
*  History
 Created:
Last Updated:		 June 21, 1999
June 24, 2005
Link to Letter added (April 2004).
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  Home > JCE Print > Journal of Chemical Education > Issues > 1998 > September > Page 1182


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