CHEMISTRY 110 

This course covers the principles of chemical kinetics and thermodynamics, redox processes, electrochemistry, and chemistry of solutions, including solubility and acid-base equilibria. It can be used as a prerequisite to Chem 113 for those missing secondary school Chem 12 and wishing to enroll in Chem 113/114

• Concentration.
• Dilution.
• Electrolytes and Nonelectrolytes.
• Arrhenius theory of electrolytic dissociation.
• Ionic equations.
• Solubility.
• Acids and Bases.
• Neutralization reaction.
• Solution Stoichiometry. 

Gases (Ch5):

• Units of pressure.
• Ideal Gas equation.
• Dalton’s Law of partial pressures.
• Kinetic molecular theory of gases.

Thermodynamics (Ch 6 and 18):

• Energy Changes in Chemical reactions.
• Exothermic and endothermic reactions.
• Work and heat.
• First law of thermodynamics.
• Hess’ Law.
• Thermochemical calculations.
• Energy and Enthalpy.
• Enthalpy of chemical reaction.
• Standard enthalpy of formation and reaction.
• Entropy.
• Second law of thermodynamics.
• Gibbs free energy.
• Spontaneous and nonspontaneous processes.

Chemical kinetics (Ch 14):

• Rate of reaction.
• Concentration dependence.
• Rate laws.
• Rate constant.
• First- and second-order reactions.
• Principles of collision theory.
• Temperature dependence of the rate constant.
• Activation energy.
• Arrhenius equation (?) Multistep processes.
• Energy profiles for multistep processes.
• Intermediates.
• Limiting step.
• Catalysis.
• Energy profiles for a catalyzed and an uncatalyzed reactions.

Chemical equilibria (Ch 15):

• Reversible reactions.
• Chemical equilibrium.
• Equilibrium constant.
• Reaction quotient.
• Relationship between equilibrium constant and Gibbs free energy of reaction (?)
• Net equilibrium constant of a multistep process (?)
• Calculations of equilibrium concentrations.
• Factors that affect chemical equilibrium.
• Le Chatelier’s principle.

Solubility (Ch 13 and 17):

• Molecular view of solution process.
• Enthalpy and entropy of dissolution.
• Solubility equilibrium.
• Solubility.
• Effect of temperature on solubility of solids and gases.
• Effect of pressure on solubility of gases.
• Solubility product.
• Solubility calculations.
• Common ion effect.

Acids and Bases (Ch 16 and 17):

• Bronsted-Lowry theory.
• Conjugate acid-base pairs.
• Acid-base properties of water.
• The ion product of water. pH, pOH, and pKw.
• Strong and week acids and bases.
• Ionization constants Ka and Kb.
• Relationship between Ka and Kb.
• Acid-base titration.
• Titration curves strong/weak acids/bases.
• Acid-base indicators.
• Acid-base properties of salts.
• Hydrolysis.
• Buffers.
• pH of a buffer solution.
• Henderson-Hasselbach equation (?)

Redox reactions and electrochemistry (Ch 4 and 19):

• Oxidation number.
• Oxidation.
• Reduction.
• Half-reactions.
• Balancing redox reactions (half-reaction method; acid and basic solutions).
• Galvanic cell.
• Standard reduction potential.
• Spontaneity of redox processes.
• Effect of concentration.
• Nernst equation (?)
• Batteries.
• Corrosion.
• Electrolysis (aqueous solutions, molten salts, active and inactive electrodes).
• Quantitative aspects of electrolysis.