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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
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

The most common feature of many acids is the presence of the hydrogen ion, H+

Acid Identification 

Concept #1: Binary Acids contain the hydrogen ion, H+, connected to an electronegative nonmetal that excludes oxygen. 

Concept #2: Oxyacids contain the hydrogen ion, H+, connected to a polyatomic ion containing oxygen. 

Example #1: Which of the following compound(s) cannot be classified as an acid?

       a)  H2Se           b) HOCN           c)  HN3           d)  C3H8           e) All are acids.

Ionic Salts

Concept #3: Cations can either be acidic or neutral depending on their identity. 

Concept #4: Anions can either be basic or neutral depending on their identity. 

Concept #5: Amphoteric Species can be either acidic or basic depending on their Ka or Kb values.