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| Goal I. Apply equilibrium
theory to acid-base reactions and pH. |
Objectives: To meet the requirements of Goal
I, you must be able to:
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apply the Brønsted-Lowry
theory to acids and bases by:
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defining and recognizing from formula or name Brønsted-Lowry
acids and Brønsted-Lowry bases;
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recognizing the acid-base conjugate pairs in an acid-base
reaction;
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distinquishing between strong and weak acids and strong
and weak bases in terms of equilibria established in their aqueous solutions.
- know and give examples applying
the specialized vocabulary of the Brønsted-Lowry theory
including: hydronium ion, predominant species, amphoteric, autoionization.
- describe the equilibrium
between H+ (or H3O+) and OH- in
water or any aqueous solution and:
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know the relative concentrations of these ions
in acidic, neutral and basic solutions;
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use Kw to calculate the [H+] given
[OH-] and
vice versa.
- define pH and pOH
and interconvert among pH, pOH, [H+] and [OH-] for
any aqueous solution.
- calculate [H+]
for solutions of given concentration of a strong acid or strong base. Understand the relationship between Ka and Kb of a conjugate acid-base pair, and Kw.
- use the specialized
equilibrium constants Ka and Kb for weak acids and
bases to calculate [H+] for aqueous solutions of specified concentration.
- define hydrolysis
to give a qualitative estimate of the pH of an aqueous solution
of a soluble ionic salt using tables of Ka and Kb
for reference (sample and follow-up problems 18.11).
- describe the common
ion effect on equilibrium, and define a buffer solution and understand the terms range, capacity and pH of a buffer.
- calculate the [H+]and
pH of an aqueous solution consisting of an acid and its salt containing
a common ion (a buffer solution) when concentrations of both are specified using the Henderson -Hasselbalch equation.
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| Goal II. Apply equilibrium
theory to aqueous solutions of slightly soluble salts. |
Objectives: To meet the requirements of Goal
II, you must be able to:
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write a chemical
equation for the equilibrium between the solid and its ions in solution,
given the formula of a slightly soluble salt.
- write the equilibrium
constant expression in the form of Ksp for any slightly soluble
salt.
- calculate the solubility
in units of g salt/100 cm3 water and in units of mol/L of solution
for any slightly soluble salt from its Ksp. calculate the Ksp given the solubility, and calculate the solubility given the Ksp (sample and follow-up problems 19.5 and 19.6).
- explain specific
examples of discrepancies between solubilities observed experimentally
and solubilities calculated from Ksp which involve the common
ion effect, occurrence of side reactions, the salt effect and ion-pair
formation.
- explain the origin
and give examples of the undesirable
effects of acid rain.
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Unit 4 Assignments
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Objectives
1 through 9
Text:
Video Programs: |
Chapter
18: pp. 767-804; Chapter 19: pp. 815-832
12. Acids and Bases; pH
13. Acid-base equilibria
14. Buffer solutions |
Objectives 10 through 14
Text:
Video Programs: |
Chapter 19: pp.
832-843.
See Appendix A for
a review of logarithms.
16*. Solubility product
17. Applications of
solubility equilibria |
| Textbook
Assignments: |
Read and
Understand all "Sample Problems," "Follow Up Problems" and select any 5 blue-colored problems at the end of the chapters.
The answers
to the Follow Up Problems are at the end of each chapter; the answers to
the blue-colored problems are in Appendix E. |
| Mandatory ChemSkill Builder Assignments to be submitted for grade (Scores of 80% or higher on each section will receive full credit): |
Chapter
18.1,
18.2,
18.3,
18.4,
18.5 Acids-Bases;
Chapter
19.1,
19.2,
19.3,
19.4,
19.5 Buffers;
Chapter
20.1,
20.2,
20.3, 20.4 Solubility Equilbria NOT 20.5
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| Take Exam: |
Exam 4 |
Note: Complete
Solutions, including all units of measurement, must be done for all problems.
*There is no Video Program #15. |
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