Ch.6 - Chemical EquilibriumWorksheetSee 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
The Equilibrium State
The Reaction Quotient
Le Chatelier's Principle
Chemical Thermodynamics: Enthalpy
Chemical Thermodynamics: Entropy
Chemical Thermodynamics: Gibbs Free Energy
Solubilty Product Constant
Protic Acids and Bases
The pH Scale
Acid Strength

Acids and bases can be classified as either strong or weak electrolytes based on their strengths. 

Binary Acid Strength 

Concept #1: Strong acids are strong electrolytes that completely ionize while weak acids are weak electrolytes that partially ionize. 

Concept #2: When looking at the strength of binary acids we look at the electronegativity of the nonmetal or the atomic size of the nonmetal. 

Example #1: Which is the weakest acid from the following?

a) H2S                          b) HF                            c) H2Te             d) All would have the same acid strength. 

Example #2: Which of the following acids would be classified as the strongest?

a) CH4                          b) NH3                          c) H2O                          d) HF                            e) PH3

Oxyacid Strength 

Concept #3: The strength of oxyacids is based on the number of oxygens or the electronegativity of the nonmetal excluding oxygen. 

Concept #4: When comparing the strengths of oxyacids we can rely on two important rules. 

Concept #5: Oxalic acid, iodic acid and amphoteric species are the exceptions in determining the strength of oxyacids. 

Example #3: Rank the following oxyacids in terms of increasing acidity.

a) HNO3                                     b) HC7H5O2                                                 c) H2CO3                                                      d) HClO3