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
Basic Redox Concepts

Concept #1: OXIDATION-REDUCTION (REDOX) reactions deal with the transfer of electrons from one reactant to another. 

Concept #2: The movement of electrons from one electrode to another helps in the generation of voltage. 

Basic Redox Concepts Calculations

Example #2: Basic Redoxs Calculations 1

Practice: Solve for the missing variable in the following circuit.

Practice: Solve for the missing variable in the following circuit.

Example #3: Basic Redoxs Calculations 2

Example #4: Basic Redoxs Calculations 2

Practice: A metal forms the salt MCl 3. Electrolysis of the molten salt with a current of 0.700 A for 6.63 h produced 3.00 g of the metal. What is the molar mass of the metal?

Example #5: Basic Redoxs Calculations 3

Example #6: Basic Redoxs Calculations 3

Example #7: Basic Redoxs Calculations 3

Balancing Redox Reactions

Concept #3: Generally, you will need to balance a redox reaction in an acidic or basic solution. 

Example #8: Balance the following redox reaction in acidic solution.

Cr2O72– (aq) + H2O2 (aq)  → Cr3+ (aq) + H2O (l) + O2 (g)

 

Practice: Balance the following redox reaction in basic solution.

Cr2O72– (aq) + SO32– (aq)  →  Cr3+ (aq)  +  SO42– (aq)