Ch.13 - Fundamentals of ElectrochemistryWorksheetSee all chapters
All Chapters
Ch.1 - Chemical Measurements
Ch.2 - Tools of the Trade
Ch.3 - Experimental Error
Ch.4 + 5 - Statistics, Quality Assurance and Calibration Methods
Ch.6 - Chemical Equilibrium
Ch.7 - Activity and the Systematic Treatment of Equilibrium
Ch.8 - Monoprotic Acid-Base Equilibria
Ch.9 - Polyprotic Acid-Base Equilibria
Ch.10 - Acid-Base Titrations
Ch.11 - EDTA Titrations
Ch.12 - Advanced Topics in Equilibrium
Ch.13 - Fundamentals of Electrochemistry
Ch.14 - Electrodes and Potentiometry
Ch.15 - Redox Titrations
Ch.16 - Electroanalytical Techniques
Ch.17 - Fundamentals of Spectrophotometry
BONUS: Chemical Kinetics
Sections
Basic Concepts
Electrochemical Cells
Standard Potentials
Nernst Equation
Standard Cell Potential & the Equilibrium Constant
Galvanic or Voltaic Cell

Concept #1: Galvanic or Voltaic cells represent spontaneous electrochemical cells that produce or discharge electricity. 

Electrolytic Cell 

Concept #2: Electrolytic Cells represent nonspontaneous electrochemical cells that consume electricity. 

Line Notation 

Concept #3: Line notation is a quick, simple method to describe an electrochemical cell without having to draw it out in detail. 

Example #1: Write the half reactions as well as the overall net ionic equation for the following line notation:

Cu | Cu2+ (aq, 0.0050 M) || Ag+(aq, 0.50 M) | Ag

Example #2: Sketch the galvanic cell and determine the cell notation for the following redox reaction:

2 H+ (aq) + Fe (s) ⇌ H2 (g) + Fe2+ (aq)

Practice: Sketch the galvanic cell and determine the line notation for the following redox reaction:

Ni2+ (aq) + Mg (s) ⇌ Ni (s) + Mg 2+ (aq)