TIGER

Journal Articles: 35 results
Connecting Solubility, Equilibrium, and Periodicity in a Green, Inquiry Experiment for the General Chemistry Laboratory  Kristen L. Cacciatore, Jose Amado, Jason J. Evans, and Hannah Sevian
Presents a novel first-year chemistry experiment that asks students to replicate procedures described in sample lab reports that lack essential information. This structure is designed to promote students' experimental design and data analysis skills as well as their understanding of the importance and essential qualities of written and verbal communication between scientists.
Cacciatore, Kristen L.; Amado, Jose; Evans, Jason J.; Sevian, Hannah. J. Chem. Educ. 2008, 85, 251.
Equilibrium |
Green Chemistry |
Periodicity / Periodic Table |
Solutions / Solvents |
Stoichiometry |
Titration / Volumetric Analysis
The Physical Meaning of the Mathematical Formalism Present in Limiting Chemical Equations; Or, How Dilute Is Dilute?  C. Contreras-Ortega, N. Bustamante, J. L. Guevara, C. Portillo, and V. Kesternich
Proposes general mathematical formulations to offer students a better understanding of the real scope of scientific expressions dealing with limiting physical conditions, such as those concerning dilute and concentrated solutions and low and high temperatures and pressures.
Contreras-Ortega, C.; Bustamante, N.; Guevara, J. L.; Portillo, C.; Kesternich, V. J. Chem. Educ. 2007, 84, 788.
Aqueous Solution Chemistry |
Equilibrium |
Gases |
Mathematics / Symbolic Mathematics |
Quantitative Analysis |
Solutions / Solvents
Flame Emission Spectrometry in General Chemistry Labs: Solubility Product (Ksp) of Potassium Hydrogen Phthalate  Frazier W. Nyasulu, William Cusworth III, David Lindquist, and John Mackin
In this general chemistry laboratory, flame emission spectrometry is used to determine the potassium ion concentration in saturated solutions of potassium hydrogen phthalate. From these data the solubility products, the Gibbs free energies of solution, the standard enthalpy of solution, and the standard entropy of solution are calculated.
Nyasulu, Frazier W.; Cusworth, William, III; Lindquist, David; Mackin, John. J. Chem. Educ. 2007, 84, 456.
Acids / Bases |
Atomic Properties / Structure |
Spectroscopy |
Equilibrium |
Quantitative Analysis |
Thermodynamics |
Titration / Volumetric Analysis |
Solutions / Solvents |
Aqueous Solution Chemistry |
Atomic Spectroscopy
Computer Simulations of Salt Solubility  Victor M. S. Gil and João C. M. Paiva
Computer Simulations of Salt Solubility provides an animated, visual interpretation of the different solubilities of related salts based on simple entropy changes associated with dissolution: configurational disorder and thermal disorder.
Gil, Victor M. S.; Paiva, João C. M. J. Chem. Educ. 2006, 83, 173.
Thermodynamics |
Equilibrium |
Solutions / Solvents |
Precipitation / Solubility |
Computational Chemistry
A New Java Animation in Peer-Reviewed JCE WebWare  William F. Coleman and Edward W. Fedosky
Just added to JCE WebWare, Computer Simulations of Salt Solubility uses a Java applet and Web browser to present an animated illustration of differences in the solubility of salts due to differences in the entropy of solvation.
Coleman, William F.; Fedosky, Edward W. J. Chem. Educ. 2006, 83, 173.
Computational Chemistry |
Equilibrium |
Thermodynamics |
Solutions / Solvents |
Precipitation / Solubility
Using Computer Simulations To Teach Salt Solubility. The Role of Entropy in Solubility Equilibrium  Victor M. S. Gil and João C. M. Paiva
Pairs of salts are discussed to illustrate the interpretation of their different behavior in water in terms of the fundamental concept of entropy. The ability of computer simulations to help improve students' understanding of these chemistry concepts is also examined.
Gil, Victor M. S.; Paiva, João C. M. J. Chem. Educ. 2006, 83, 170.
Computational Chemistry |
Equilibrium |
Thermodynamics |
Solutions / Solvents |
Precipitation / Solubility
Are Fizzing Drinks Boiling? A Chemical Insight from Chemical Education Research  Alan Goodwin
The suggestion that fizzing drinks are examples of liquids boiling at room temperature has proved to be controversial among both chemists and chemical educators. This paper presents a case for believing this everyday system to be a good example of a boiling solution and the consequent separation of carbon dioxide from the solution to exemplify fractional distillation.
Goodwin, Alan. J. Chem. Educ. 2001, 78, 385.
Aqueous Solution Chemistry |
Kinetic-Molecular Theory |
Equilibrium |
Gases |
Solutions / Solvents |
Phases / Phase Transitions / Diagrams
SolEq: Solution Equilibria, Principles and Applications, Release 1
by SolEq Project Team: L. D. Pettit, K. J. Powell, and R. W. Ramette

  Marina C. Koether
29 tutorials with simulation, calculations, and graphs, on solution equilibria.
Koether, Marina C. J. Chem. Educ. 2000, 77, 1414.
Equilibrium |
Solutions / Solvents |
Titration / Volumetric Analysis

The Effects of Salts and Nonelectrolytes on the Solubility of Potassium Bitartrate: An Introductory Chemistry Discovery Experiment  Charles J. Marzzacco
An introductory chemistry discovery experiment on the effect of the presence of various solutes on the solubility of potassium bitartrate (KHT) is presented. Aqueous solutions of KCl, NaCl, MgSO4 and glucose with concentrations ranging from 0.0 to 0.10 M are saturated with KHT. The solubility of the KHT in these various solutions is determined by titration with standardized NaOH solution.
Marzzacco, Charles J. J. Chem. Educ. 1998, 75, 1628.
Solutions / Solvents |
Equilibrium |
Quantitative Analysis
What Should We Teach Beginners about Solubility and Solubility Products?  Stephen J. Hawkes
Solubility equilibria are best taught qualitatively in introductory chemistry, leaving the calculations to higher level courses.
Hawkes, Stephen J. J. Chem. Educ. 1998, 75, 1179.
Solutions / Solvents |
Equilibrium |
Precipitation / Solubility
The reply: Ionization Constants  S. Roo, L. Vermeire, and C. Gorller-Walrand
Error regarding the first ionization constant of carbonic acid.
Roo, S.; Vermeire, L.; Gorller-Walrand, C. J. Chem. Educ. 1997, 74, 1160.
Equilibrium |
Solutions / Solvents |
Aqueous Solution Chemistry |
Acids / Bases |
Mathematics / Symbolic Mathematics
Ionization Constants  Morris Bader
Error regarding the first ionization constant of carbonic acid.
Bader, Morris. J. Chem. Educ. 1997, 74, 1160.
Equilibrium |
Solutions / Solvents |
Aqueous Solution Chemistry |
Acids / Bases
Using Quality Circles in General Chemistry  Kogut, Leonard S.
A second semester class in General Chemistry used a student Quality Circle to suggest methods to improve instruction in chemical equilibrium in solution.
Kogut, Leonard S. J. Chem. Educ. 1996, 73, 146.
Equilibrium |
Solutions / Solvents
Experiments for Modern Introductory Chemistry: Intermolecular Forces and Raoult's Law  Berka, Ladislav H.; Kildahl, Nicholas
Procedure that illustrates the liquid-vapor phase equilibrium of ideal and nonideal solutions.
Berka, Ladislav H.; Kildahl, Nicholas J. Chem. Educ. 1994, 71, 613.
Noncovalent Interactions |
Gas Chromatography |
Gases |
Liquids |
Equilibrium |
Solutions / Solvents
Demonstration of the Common Ion Effect  Koubek, E.
KCl and HCl are used in this demonstration to describe the common ion effect and to show the difference between values Q and K.
Koubek, E. J. Chem. Educ. 1993, 70, 155.
Solutions / Solvents |
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
Teaching freezing point lowering  Ball, Jenelle; Cooke, Ron C.; Willis, Grover
Using Le Chatelier's principle, the van't Hoff equation, and the empirical equation to explain the lowering of the freezing point caused by dissolving antifreeze in water.
Ball, Jenelle; Cooke, Ron C.; Willis, Grover J. Chem. Educ. 1990, 67, 676.
Physical Properties |
Solutions / Solvents |
Equilibrium |
Aqueous Solution Chemistry
Chemical principles for the introductory laboratory, CHM 384 (Johnson, James F.)  Wegner, Carol
A comprehensive review of the title program which overviews basic techniques and concepts presented in introductory laboratory courses. Topics include: titration, equilibrium, Ksp, solubility, Beer's law, coordination complexes and first-order rates of reaction.
Wegner, Carol J. Chem. Educ. 1988, 65, A47.
Acids / Bases |
Titration / Volumetric Analysis |
UV-Vis Spectroscopy |
Equilibrium |
Solutions / Solvents |
Coordination Compounds |
Kinetics
The goals of teaching solution equilibrium  Ruda, Paul T.
Using and making relevant the concepts of solution equilibrium.
Ruda, Paul T. J. Chem. Educ. 1984, 61, 784.
Equilibrium |
Solutions / Solvents
Why teach solution equilibrium?  Butler, James N.
What are the most important aspects of solution equilibrium to teach at the elementary level?
Butler, James N. J. Chem. Educ. 1984, 61, 784.
Equilibrium |
Solutions / Solvents |
Acids / Bases |
pH
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
Solubility and Ksp of calcium sulfate: a general chemistry laboratory experiment  Sawyer, Albert K.
The experiment shared in this note can be used to accompany lectures on solubility or chemical equilibrium.
Sawyer, Albert K. J. Chem. Educ. 1983, 60, 416.
Solutions / Solvents |
Aqueous Solution Chemistry |
Equilibrium
Small things and large numbers   Rosenberg, Milton H.
Some challenging solubility problems are featured in this note.
Rosenberg, Milton H. J. Chem. Educ. 1981, 58, 962.
Solutions / Solvents |
Equilibrium |
Chemometrics
Ksp made simple  Buss, Donald E.
Students often have a hard time understanding solubility products conceptually. The author provides appropriate questions that can better scaffold understanding.
Buss, Donald E. J. Chem. Educ. 1981, 58, 958.
Equilibrium |
Solutions / Solvents
Cobalt complexes in equilibrium  Ophardt, Charles E.
This equilibrium illustrates the application of LeChatelier's principle to concentration effects.
Ophardt, Charles E. J. Chem. Educ. 1980, 57, 453.
Equilibrium |
Coordination Compounds |
Aqueous Solution Chemistry |
Solutions / Solvents
"To sink or swim"  O'Connor, Rod
A problem regarding the maximum water hardness that can be permitted in a swimming pool if it is desired to avoid calcite formation given the carbonate ion concentration. [Debut]
O'Connor, Rod J. Chem. Educ. 1980, 57, 151.
Acids / Bases |
Aqueous Solution Chemistry |
Equilibrium |
Solutions / Solvents
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
Silver ion in water purification: A follow-up  Quane, Denis
Applying a previous idea on the possible use of silver ion in water purification to teaching the concept of Ksp.
Quane, Denis J. Chem. Educ. 1977, 54, 381.
Aqueous Solution Chemistry |
Water / Water Chemistry |
Equilibrium |
Solutions / Solvents
On mole fractions in equilibrium constants  Delaney, C. M.; Nash, Leonard K.
Proposes a hybrid equilibrium constant for use in introductory chemistry courses.
Delaney, C. M.; Nash, Leonard K. J. Chem. Educ. 1977, 54, 151.
Equilibrium |
Stoichiometry |
Aqueous Solution Chemistry |
Solutions / Solvents
Chemical equilibrium  Burke, Barbara A.
Demonstrates the equilibrium between blue CuSO4 and green K2(CuBr4) on an overhead projector.
Burke, Barbara A. J. Chem. Educ. 1977, 54, 29.
Equilibrium |
Solutions / Solvents |
Aqueous Solution Chemistry
Molar solubility calculations and the control equilibrium  Chaston, S. H. H.
The Control-Equilibrium method uses as its starting point a precise procedure for obtaining the equilibrium that accounts for the bulk of the decomposition of starting materials.
Chaston, S. H. H. J. Chem. Educ. 1975, 52, 206.
Solutions / Solvents |
Chemometrics |
Equilibrium
The equilibrium between a solid solution and an aqueous solution of its ions  Berndt, Alan F.; Stearns, Robert I.
It is the purpose of this paper to present the equations that describe the equilibrium between solid solutions and their ions and to outline methods for their derivation.
Berndt, Alan F.; Stearns, Robert I. J. Chem. Educ. 1973, 50, 415.
Equilibrium |
Solutions / Solvents |
Aqueous Solution Chemistry
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
Le Chtelier and ionic equilibria  Ringbom, Anders
When s solution contains several weak acids, the squares of the separately calculated hydrogen ion concentrations of all weak acids in the solution are additive.
Ringbom, Anders J. Chem. Educ. 1968, 45, 442.
Equilibrium |
Acids / Bases |
Precipitation / Solubility |
Solutions / Solvents
Solvent effect on the keto-enol equilibrium of acetoacetic ester  Lockwood, Karl L.
The purpose of the investigation is to introduce students to some of the factors that influence an equilibrium constant.
Lockwood, Karl L. J. Chem. Educ. 1965, 42, 481.
Solutions / Solvents |
Equilibrium