|Ch.1 - Chemical Measurements||2hrs & 8mins||0% complete|
|Ch.2 - Tools of the Trade||1hr & 26mins||0% complete|
|Ch.3 - Experimental Error||1hr & 53mins||0% complete|
|Ch.4 + 5 - Statistics, Quality Assurance and Calibration Methods||2hrs & 1min||0% complete|
|Ch.6 - Chemical Equilibrium||3hrs & 49mins||0% complete|
|Ch.7 - Activity and the Systematic Treatment of Equilibrium||1hr & 1min||0% complete|
|Ch.8 - Monoprotic Acid-Base Equilibria||1hr & 52mins||0% complete|
|Ch.9 - Polyprotic Acid-Base Equilibria||2hrs & 16mins||0% complete|
|Ch.10 - Acid-Base Titrations||2hrs & 40mins||0% complete|
|Ch.11 - EDTA Titrations||1hr & 37mins||0% complete|
|Ch.12 - Advanced Topics in Equilibrium||1hr & 18mins||0% complete|
|Ch.13 - Fundamentals of Electrochemistry||2hrs & 27mins||0% complete|
|Ch.14 - Electrodes and Potentiometry||43mins||0% complete|
|Ch.15 - Redox Titrations||1hr & 14mins||0% complete|
|Ch.16 - Electroanalytical Techniques||1hr & 3mins||0% complete|
|Ch.17 - Fundamentals of Spectrophotometry||55mins||0% complete|
|BONUS: Chemical Kinetics||Not available yet|
Concept #1: Differences in ion concentrations and ion mobility help to create junction potentials at each end of a salt bridge.
Mobility of ions is based on their size and the greater the difference in sizes between the two ions the greater the potential.
Example #1: Determine the electrical potential that results from the given galvanic cell. Assume that the junction potential is minimal.
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