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Ch.8 - Monoprotic Acid-Base EquilibriaWorksheetSee 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
Arrhenius Acids and Bases
Bronsted-Lowry Acids and Bases
Lewis Acids and Bases
Auto-Ionization
Ka and Kb of compounds
Weak Acid-Base Equilibria
Ionic Salts of Weak Acids and Bases
Buffers
Bronsted-Lowry Acids and Bases 

Concept #1: According to the Bronsted-Lowry definition, acids are considered H+ donor and bases are considered H+ acceptor. 

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Example #1: Write the formula of the conjugate base for each of the following compounds:

HSO3

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Example #2: Write the formula of the conjugate acid for each of the following compounds:

HPO32-

 

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Example #3: Identify the acid, base, conjugate acid and conjugate base in the following reactions:

HF (aq)      +      H2O (aq)   ⇌    F (aq)      +      H3O+ (aq) 

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