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Journal Articles: 22 results
Determining the Solubility Product of Fe(OH)3: An Equilibrium Study with Environmental Significance  Michelle Meighan, Joseph MacNeil, and Renee Falconer
This study explores the environmental impact of acidic mine drainage by investigating the relationship between pH and the aqueous solubility of heavy metals. Students precipitate Fe(OH)3 from acidic FeCl3 and NaOH and use the concentrations of ferric and hydroxide ionsdetermined through pH and flame spectroscopyto calculate the Ksp of Fe(OH)3.
Meighan, Michelle; MacNeil, Joseph; Falconer, Renee. J. Chem. Educ. 2008, 85, 254.
Acids / Bases |
Aqueous Solution Chemistry |
Equilibrium |
Precipitation / Solubility |
Spectroscopy
Chemical Equilibria Involving Copper(II) Ethylenediamine Complexes  Roberto Zingales
Demonstration illustrating the formation of two different complexes when copper(II) ions react with ethylenediamine.
Zingales, Roberto. J. Chem. Educ. 2003, 80, 535.
Equilibrium |
Aqueous Solution Chemistry |
Reactions |
Amines / Ammonium Compounds |
Precipitation / Solubility
Chemical Equilibria Involving Reactions of Silver(I) Ions  Roberto Zingales
Demonstrating a series of reactions involving silver(I) ions.
Zingales, Roberto. J. Chem. Educ. 2003, 80, 534.
Equilibrium |
Reactions |
Aqueous Solution Chemistry |
Qualitative Analysis |
Metals |
Precipitation / Solubility
Modification of Small-Scale One-Pot Reactions to an Inquiry-Based Laboratory Exercise  C. Jayne Wilcox
Students are given an initial handout and asked to complete a short, attention-getting exercise. They must continue to work on logical, short exercises given to them one at a time, in handout format. The inquiry-based approach is intended to increase students' comprehension of what they're doing in the laboratory and why.
Wilcox, C. Jayne. J. Chem. Educ. 2001, 78, 62.
Acids / Bases |
Aqueous Solution Chemistry |
Precipitation / Solubility |
Equilibrium
The Ksp-Solubility Conundrum  Roy W. Clark and Judith M. Bonicamp
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.
Clark, Roy W.; Bonicamp, Judith M. J. Chem. Educ. 1998, 75, 1182.
Equilibrium |
Aqueous Solution Chemistry |
Precipitation / Solubility
Will a precipitate form? Will it dissolve?: The Role of Lecture Demonstrations in Facilitating the Introduction to Solubility Product Equilibria  Pacer, Richard A.; Williams, Kathryn
Three demonstrations to illustrate solubility product equilibria.
Pacer, Richard A.; Williams, Kathryn J. Chem. Educ. 1994, 71, 69.
Precipitation / Solubility |
Aqueous Solution Chemistry |
Equilibrium
Simple soda bottle solubility and equilibria  Snyder, Cheryl A.; Snyder, Dudley C.
Using a bottle of selzter water and bromocresol green to demonstrate gas-liquid solubility (carbon dioxide in water).
Snyder, Cheryl A.; Snyder, Dudley C. J. Chem. Educ. 1992, 69, 573.
Solutions / Solvents |
Precipitation / Solubility |
Equilibrium |
Gases |
Liquids |
Aqueous Solution Chemistry |
Water / Water Chemistry
Chemical equilibrium: VIII. Precipitates   Gordus, Adon A.
The final article in a series (see previous months this year): This article focuses on ionic precipitates in water and how buffered solutions allow easier calculation of solubilities.
Gordus, Adon A. J. Chem. Educ. 1991, 68, 927.
Acids / Bases |
Equilibrium |
pH |
Precipitation / Solubility |
Aqueous Solution Chemistry |
Water / Water Chemistry
The solubility of CaSO4 (the author replies)  Sawyer, Albert K.
Reasons why the lab determination of Ksp for CaSO4 is ten times higher than the published value.
Sawyer, Albert K. J. Chem. Educ. 1985, 62, 362.
Precipitation / Solubility |
Equilibrium |
Aqueous Solution Chemistry
The solubility of CaSO4   Hawkes, Stephen J.
Reasons why the lab determination of Ksp for CaSO4 is ten times higher than the published value.
Hawkes, Stephen J. J. Chem. Educ. 1985, 62, 362.
Precipitation / Solubility |
Equilibrium |
Aqueous Solution Chemistry
The solubility of NiSO46H2O  Pacer, Richard A.
Approaches the position of equilibrium from both unsaturated and supersaturated solutions.
Pacer, Richard A. J. Chem. Educ. 1984, 61, 467.
Aqueous Solution Chemistry |
Solutions / Solvents |
Precipitation / Solubility |
Equilibrium |
UV-Vis Spectroscopy
On the misuse of Le Châtelier's principle for the prediction of the temperature dependence of the solubility of salts  Bodner, George M.
Explores why Le Châtelier's principle often fails to predict the temperature dependence of the solubility of salts.
Bodner, George M. J. Chem. Educ. 1980, 57, 117.
Equilibrium |
Precipitation / Solubility |
Solutions / Solvents |
Aqueous Solution Chemistry
Simultaneous equilibria involving insoluble salts  Baumann, Jacob B.
This demonstration is derived from and involves the same reactions as the Mohr titration of chloride ion with silver nitrate solution using potassium chromate as an indicator.
Baumann, Jacob B. J. Chem. Educ. 1977, 54, 618.
Equilibrium |
Precipitation / Solubility |
Aqueous Solution Chemistry
Ratio diagrams: A simple graphical representation of complicated equilibria  de Levie, R.
Introduces and demonstrates the usefulness and general applicability of ratio diagrams as the simplest graphical representation of equilibria involving mononuclear species.
de Levie, R. J. Chem. Educ. 1970, 47, 187.
Equilibrium |
Acids / Bases |
pH |
Aqueous Solution Chemistry |
Precipitation / Solubility
Le Chtelier's principle  Melott, Adrian L.
Adding a strong base to aqueous ammonia causes gaseous ammonia to be released.
Melott, Adrian L. J. Chem. Educ. 1968, 45, A519.
Equilibrium |
Solutions / Solvents |
Precipitation / Solubility |
Acids / Bases |
Aqueous Solution Chemistry
Calcium carbonate equilibria in lakes  Morton, Stephen D.; Lee, G. Fred
Discusses some of the problems encountered in studying the chemistry of lakes and oceans, focussing on the solubility of calcium carbonate in fresh water lakes.
Morton, Stephen D.; Lee, G. Fred J. Chem. Educ. 1968, 45, 511.
Aqueous Solution Chemistry |
Water / Water Chemistry |
Precipitation / Solubility |
Equilibrium
Is the solubility product constant? Introductory experiment in solubility equilibrium  Goodman, Robert C.; Petrucci, Ralph H.
This article describes an experiment that employs the titration of lead nitrate solutions with potassium iodide solutions as a vivid and straightforward method of determining solubility product.
Goodman, Robert C.; Petrucci, Ralph H. J. Chem. Educ. 1965, 42, 104.
Equilibrium |
Precipitation / Solubility |
Aqueous Solution Chemistry
Equilibria in ionic solutions  Kokes, R. J.; Dorfman, M. K.; Mathia, T.
In conjunction with lectures on equilibria in electrolytic solutions, students perform a set of laboratory experiments in which they determine both the ionization constant of chloroacetic acid and the solubility of its silver salt.
Kokes, R. J.; Dorfman, M. K.; Mathia, T. J. Chem. Educ. 1962, 39, 93.
Equilibrium |
Aqueous Solution Chemistry |
Acids / Bases |
Precipitation / Solubility
Potentiometric measurements of equilibria: In general chemistry laboratory  Chesick, J. P.; Patterson, Andrew, Jr.
The authors describe an experiment in which the solubility product of silver chloride, the ionization constant of the silver-ammonia complex, and the ionization constant of acetic acid can be determined with one afternoon of work.
Chesick, J. P.; Patterson, Andrew, Jr. J. Chem. Educ. 1959, 36, 496.
Electrochemistry |
Equilibrium |
Precipitation / Solubility |
Aqueous Solution Chemistry |
Acids / Bases
The analyst and the inconstant constants  Ringbom, Anders
Simple theories taught to freshmen often do not agree well with experimental data; the author examines the case of equilibrium constants and elaborates on a method of dealing with this problem.
Ringbom, Anders J. Chem. Educ. 1958, 35, 282.
Equilibrium |
Aqueous Solution Chemistry |
Precipitation / Solubility
Demonstration of dynamic nature of ions using I131  Blake, Richard F.
This demonstration presents visual evidence of the ionic nature of solid salts and the dynamic equilibrium existing between dissolved and undissolved ions.
Blake, Richard F. J. Chem. Educ. 1956, 33, 354.
Isotopes |
Aqueous Solution Chemistry |
Solids |
Precipitation / Solubility |
Equilibrium
Some lecture demonstrations in general chemistry  Klemm, L. H.
Describes three demonstrations involving the atomistic nature of matter, the controlled experiment, and the solubility product.
Klemm, L. H. J. Chem. Educ. 1951, 28, 587.
Kinetic-Molecular Theory |
Aqueous Solution Chemistry |
Precipitation / Solubility |
Equilibrium