Click on the title of a resource to view it. To save screen space, only the first 3 resources are shown. You can display more resources by scrolling down and clicking on “View all xx results”.
For the textbook, chapter, and section you specified we found
Reactions : AcidBaseRxns (20 Variations) In order to answer the following questions, write the net ionic equation for the reaction between equal volumes of 0.10 M solutions of the following acid and base:
KOH(aq) + HBr(aq)
What are the reaction products? Does the reaction yield an acidic, basic, or neutral aqueous solution?
A 25.0 mL aliquot of a 1.44M solution of ammonia (Kb = 1.8 x 10-5) is titrated with 1.50M HCl. Use the Indicator Table below to decide which of the indicators listed would most accurately signal the equivalence point for this titration.
Write the letter corresponding to your choice of indicator in the box.
Imidazole as a pH Probe: An NMR Experiment for the General Chemistry LaboratoryWilliam J. Hagan, Jr., Dennis L. Edie, and Linda B. Cooley An experiment is described that employs the 1H-NMR signal of aqueous imidazole to determine the pH of an unknown solution. The procedure involves the preparation of a calibration curve, which is then used for the analysis of the unknown(s). Hagan, William J., Jr.; Edie, Dennis L.; Cooley, Linda B. J. Chem. Educ.2007, 84, 1188.
Acids / Bases |
Aqueous Solution Chemistry |
Aromatic Compounds |
Calibration |
NMR Spectroscopy |
pH
pH Paradoxes: Demonstrating That It Is Not True That pH ≡ -log[H+]Christopher G. McCarty and Ed Vitz Six demonstrations highlighting paradoxes that arise if pH is incorrectly defined as -log[H+] are presented as justification for the recommendation that pH should be correctly defined as pH = -log aH+ in textbooks. McCarty, Christopher G.; Vitz, Ed. J. Chem. Educ.2006, 83, 752.
Acids / Bases |
Aqueous Solution Chemistry |
Ion Selective Electrodes |
pH |
Quantitative Analysis
Using Visible Spectrophotometers and pH Measurements To Study Speciation in a Guided-Inquiry Laboratory William H. Otto, Cynthia K. Larive, Susan L. Mason, Janet B. Robinson, Joseph A. Heppert, and James D. Ellis A collective-effort, guided-inquiry laboratory investigation was developed for the second-semester general chemistry laboratory for the purpose of increasing student conceptual understanding of equilibrium and speciation phenomena. This investigation required students to employ the chemical indicator phenol red in phosphate buffer solution, computer interfaced pH probes, and visible spectrophotometers. Through a combination of potentiometric and visible absorption measurements, the students determined the pH conditions that alter equilibrium concentrations of multiple species (colored and transparent) in solution. Otto, William H.; Larive, Cynthia K.; Mason, Susan L.; Robinson, Janet B.; Heppert, Joseph A.; Ellis, James D. J. Chem. Educ.2005, 82, 1552.
