Learning Objectives For Test 3
November 18, 2010
General Chemistry II (CHEM 1474)
Sample Exercises
Acid-base equilibria (Chapter 16)
Review of current acid-base concepts
Arrhenius Theory (16.1)
Identify substances as Bronsted-Lowry acids or bases (16.2)
Identify conjugate acid-base pairs (16.2)
Determine relative acidity or basicity of substances (16.2)
The autoionization of water
Given hydronium or hydroxide concentration, determine the other (16.3)
The pH scale
Given hydronium, hydroxide, pH, and/or pOH determine the other values (16.4)
Calculations involving strong acids and bases
Determine hydronium, hydroxide, pH, and/or pOH values given a concentration of
a strong acid or base (16.5)
Calculations involving weak acids
Given sufficient information, determine hydronium, hydroxide, pH, pOH, Ka,
and/or percent ionization for a weak acid solution (16.6)
Calculations involving weak bases
Given sufficient information, determine hydronium, hydroxide, pH, pOH, Ka,
and/or percent ionization for a weak base solution (16.7)
16.15-16.16
16.17-16.24
16.25-16.28, 16.107
16.29-16.34
16.35-16.42, 16.111
16.43-16.50, 16.110,
16.112, 16.122-16.123
16.51-16.70, 16.10516.106, 16.113-16.115,
16.130
16.71-16.78, 16.11816.119,16.127
↓↓↓↓↓Test 3 Begins Here↓↓↓↓↓
Relationship between Ka and Kb
Determine Ka and Kb for a conjugate acid/base pair given one of them (16.8)
Acid-base properties of salt solutions
Given sufficient information, determine hydronium, hydroxide, pH, pOH, Ka,
and/or percent ionization for a salt solution (16.9)
Acid-base behavior and chemical structure
Identify factors that affect acid and base strengths (16.10)
Evaluate the relative acidity or basicity of a series of compounds (16.10)
Lewis acids and bases
Identify materials as Lewis acids or bases (16.11)
16.79-16.82
16.83-16.90, 16.116
16.91-16.92
16.93-16.98, 16.120
16.99-16.104, 16.125
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Learning Objectives For Test 3
November 18, 2010
General Chemistry II (CHEM 1474)
Sample Exercises
Other Aspects of Aqueous Equilibria (Chapter 17)
Common ion effect
Identify “common ions” in a given solution (17.1)
17.13-17.14
Calculate the pH and associated quantities in systems made with compounds
17.15-17.18
containing common ions (17.1)
Buffered solutions
Define and identify buffer systems (17.2)
17.19-17.20
Calculate the pH and associated quantities in buffer systems (17.2)
17.21-17.26
Calculate changes in pH when acids and bases are added to buffer solutions (17.2)
17.27-17.28
Apply the Henderson-Hasselbalch equation to buffer systems (17.2)
17.29-17.32
Acid-base titrations
Recognize titration curves for strong acid-strong base, weak acid-strong base, and
17.33-17.38
weak base-strong acid titrations (17.3)
Generate titration curves for strong acid-strong base, weak acid-strong base, and
17.39-17.46
weak base-strong acid titrations (17.3)
↑↑↑↑↑↑Test 3 Ends Here↑↑↑↑↑↑
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)
Qualitative analysis for metallic elements
Given results of particular steps in Figure 17.22, state conclusions regarding the
presence or absence of specific ions (17.7)
Mastering Chemistry Homework Sets include HW13 through HW 16
17.51-17.52
17.49-17.50, 17.5317.56, 17.59-17.62
17.57-17.58
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