Learning Objectives
General Chemistry II (CHEM 1474)
Buckley – Fall 2010
Textbook references are to: Chemistry: The Central Science, Brown/LeMay/Bursten/Murphy, 11th Edition, 2009
Sample Exercises
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Other Aspects of Aqueous Equilibria (Chapter 17)
The Common Ion Effect
Identify “common ions” in a given solution (17.1)
Calculate the pH and associated quantities in systems made with compounds
containing common ions (17.1)
Buffered solutions
Define and identify buffer systems (17.2)
Calculate the pH and associated quantities in buffer systems (17.2)
Calculate changes in pH when acids and bases are added to buffer solutions (17.2)
Acid-base titrations
Generate titration curves for strong acid-strong base, weak acid-strong base,
polyprotic acid titrations (17.3)
17.13-17.14
17.15-17.18
17.19-17.20
17.21-17.26
17.27-17.28
17.29-17.32
↓↓↓↓TEST 4 Objectives↓↓↓↓
Solubility equilibria
Given any chemical equation expressing the dissolution of a solid, write the
mathematical expression for the Ksp (17.4)
Given sufficient information, calculate missing information related to a solubility
situation (17.4-17..5)
Predict solubility based on the introduction of common ions (17.5)
17.33-17.38
17.39-17.46
17.49-17.50, 17.5317.56, 17.59-17.62
17.57-17.58
Learning Objectives
General Chemistry II (CHEM 1474)
Buckley – Fall 2010
Textbook references are to: Chemistry: The Central Science, Brown/LeMay/Bursten/Murphy, 11th Edition, 2009
Sample Exercises
Got it?
Needs work
Electrochemistry (Chapter 20)
Oxidation States and Oxidation-Reduction Reactions
Use oxidation number to identify the species oxidized, reduced, the oxidizing
20.11-20.16
agent and reducing agent in a redox reaction (20.1)
Balancing Oxidation-Reduction Equations
Use the half-reaction method to balance redox reactions in neutral, acidic, and
20.17-20.22
basic solution (20.2)
Voltaic Cells
Identify the anode and cathode in a voltaic cell (20.3)
20.25-20.26
Find the standard cell potential of a voltaic cell (20.4)
20.27-20.40
Identify the relative strengths of oxidizing agents and reducing agents from
20.41-20.48
standard reduction half-cell potentials (20.4)
Determine the cell potential of a cell under nonstandard conditions using the
20.37-20.68
Nernst equation (20.6)
Electrolysis
Manipulate equations relating current, time, moles of electrons, and mass to
20.87-20.89, 20.91determine missing information (20.9)
20.92
Learning Objectives
General Chemistry II (CHEM 1474)
Buckley – Fall 2010
Textbook references are to: Chemistry: The Central Science, Brown/LeMay/Bursten/Murphy, 11th Edition, 2009
Sample Exercises
Got it?
Needs work
Chemical Thermodynamics (Chapter 19)
Spontaneous Processes
Distinguish between the terms spontaneous process and nonspontaneous process
(19.1)
Distinguish between reversible and irreversible processes (19.1)
Entropy and the Second Law of Thermodynamics
Describe the role of entropy in determining the spontaneity of a process (19.2)
State and apply the Second Law of Thermodynamics (19.2)
Given sufficient information, determine the entropy change in a chemical or
physical process (19.2, 19.4)
Gibbs Free Energy
Given sufficient information, calculate the Gibbs Free Energy change for a
reaction (19.5)
Determine temperature ranges of spontaneity based on enthalpy and entropy
changes (19.6)
Free Energy and the Equilibrium Constant
Manipulate the relationships between ΔG and K and E° (19.7)
19.9-19.20
19.25-19.26
19.21-19.24, 19.2719.28, 19.43-19.50
19.53-19.60, 19.6919.72
19.61-19.68
19.73-19.82
↑↑↑↑TEST 4 Objectives↑↑↑↑