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  Home > JCE Print > Journal of Chemical Education > Issues > 1999  > November  >
In the Laboratory
The Solubility of Ionic Solids and Molecular Liquids
Carl Baer and Sheila M. Adamus
Department of Chemistry, Providence College, Providence, RI 02918
Cover
November 1999
Vol. 76 No. 11
p. 1540
Abstract
Solubility is a ubiquitous concept in chemistry, but usually only sparingly soluble salts are examined in the introductory chemistry laboratory. With this two-part experiment, students study more common solubility phenomena. First, solubilities of three ionic salts (NaCl, PbCl2, and KAl(SO4)2.12H2O) in water are measured at four temperatures. The concept of recrystallization is introduced as students cool a high-temperature solution and observe crystal formation. Class data are pooled and students are expected to identify and exclude poor data. Spreadsheet calculations are performed with the group data, which are then graphed, and students observe the wide variance in solubility behavior for the three salts. In the second part of the experiment, water and six organic liquids are mixed pairwise in all possible combinations to determine which pairs are miscible. Dielectric constants are provided for each liquid as a measure of polarity and students are asked to discuss their observed solubilities in terms of polarity. The common rule of "like dissolves like" is found to be less than satisfactory as a description of liquid solubility behavior if too narrowly interpreted.
Supplement
Descriptions of the experimental write-up, instructor's notes, and results/discussion are provided in the supplementaty material.
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*  Citation
 Baer, Carl; Adamus, Sheila M. J. Chem. Educ. 1999 76 1540.
*  Keywords
 Introductory / High School Chemistry; Intermolecular Forces; Laboratory Instruction; Laboratory Computing / Interfacing; Liquids; Molecular Properties / Structure; Solutions / Solvents
*  History
 Created:
Last Updated:		 October 12, 1999
November 22, 2005
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