Advance Placement Chemistry
2010-2011 Course Description and Syllabus
Contact Information
Mr. Daw (Adapted from Mrs. Graves)
Stuarts Draft High School
Room 46
School Phone: (540) 946-7600
Email: vdaw@augusta.k12.va.us or VWDaw@aol.com
Course Description
Advance Placement Chemistry is designed to be equivalent to a first-year college chemistry course. Since
this course is taught at a college level it will be very demanding in terms of both time and effort. To be
successful, students will have to spend 5-6 hours outside of class each week (45-60 minutes per day)
studying chemistry and doing homework. Students may work in groups and/or get help from teachers.
Each unit of study will consist of lectures, demonstrations, activities & laboratory experiments followed by
a comprehensive exam. The class will meet daily for 45 minutes, but may require additional time each
week to collect data and complete experiments. Students will take the AP Chemistry examination in May
2011. A score of 3/5 on the AP exam is required for credit at most universities.
Classroom Goals and Objectives
The students will be able to:
 Develop reading, writing, speaking, and studying skills essential for college.
 Set ambitious personal goals and achieve them with integrity.
 Work effectively as part of a team to accomplish complex tasks.
 Analyze and solve scientific problems using a systematic approach.
 Ask questions, make predictions, gather data, analyze results, draw conclusions and
operate safely in a scientific laboratory setting.
 Understand and appreciate the order and beauty of the natural world.
Textbook
Steven S. Zumbahl and Susan Zumbahl, Chemistry, 5th Ed., Houghton Mifflin Co., Boston, 2000.
Materials
Students are required to have the following materials and bring them to class every day:
 Pen & pencil (Dark colors work best.)
 Scientific calculator (A graphing calculator would be useful.)
 Notebook with paper & dividers (3 ring binders are easier to organize.)
 Textbook & supplementary documents (Fast Track to a 5 is a useful guide to exam success.)
 Periodic Table of the Elements (This will be supplied by teacher.)
 Laboratory Notebook (must be a “composition” notebook; NOT a spiral notebook).
Helpful Hints
A student’s success in this course will reflect the amount of time and effort put into it.
 Be in class, on time, ready to work every day. (Absences will be very difficult to make up.)
 Pre-read each chapter/section before lecture. (Have specific questions in mind.)
 Work on problems as we cover them in class. (Have examples to look at while doing homework.)
 Ask questions as soon as they arise. (Don’t wait until the test!)
 Take good notes and review them often. (Rewriting notes is a great way to “make it stick”.)
 Keep up with your assignments and due dates. (Staying organized will minimize frustration.)
 Use your text, notes, websites, office hours and classmates to help solve problems. Study groups
are good learning experiences; however, you must be able to work/solve problems on your own.
Student Responsibilities
Each student is responsible for the contents of this document including the expectations, procedures,
schedules and grading policies for AP chemistry. Students are responsible for what goes on in class
whether they are in attendance or not. If absent, please find out what was missed and make up
assignments ASAP. If possible, check with Mr. Daw beforehand to avoid falling behind. Because we will
be moving at a rapid pace, it will be very difficult to catch up once a student falls behind. If you are
unsure about a topic or class expectation, please ask! Remember, AP chemistry is designed to be the
equivalent of a college chemistry course, so be responsible for your learning!
Class Room Rules
1. Students are expected to respect safety rules, the teacher, and fellow students.
2. Students are expected to be in class, seated with materials out, and ready to begin when the
tardy bell rings.
3. Students are expected to complete all assignments before arriving to class and to bring all
necessary materials to class EVERY DAY.
4. Students are expected NOT to eat or drink, litter, “horse-play”, stray from directions, or perform
unauthorized experiments with any equipment in the classroom.
5. Class will be dismissed when all materials and/or lab equipment have been properly put way and
laboratory areas are cleaned according to laboratory procedures.
Absences
Daily attendance is essential for student success in this course. If absent, a student must obtain all
missing assignments and/or notes from a classmate. For excused absences, students will have one day to
make-up any assignments missed. Students are strongly discouraged from missing test (exam) dates.
Tests may be given early by prior arrangement. Students absent during a test (exam) period, are
expected to make up the test the day they return. Attendance/participation will count for approximately
10% of the final grade.
Homework
Homework will be assigned weekly (including weekends and school breaks). Students should complete
assignments by due dates; no late homework will be accepted. Please ask questions or get help before
homework is due. Students will be provided with solution keys to most of the homework assignments. In
order to receive full credit for homework, students must complete all assigned problems, show formulas
and steps, use the correct number of significant figures, and circle the answer with the correct units.
Homework will count for approximately 10% of the final grade.
Quizzes and Tests
There will be regular quizzes for each topic, some announced and some “pop” quizzes. There will be a
comprehensive test, similar in format to the AP test, for each unit. The quizzes and tests will consist of
multiple choice questions, short answers questions, numerical problems and essay questions. Students
will be given the opportunity to correct and return tests (as well as some quizzes) for additional
(approximately ½) credit. Do not expect to “ace” many quizzes or tests. Learn from your mistakes!
In order to prepare for the AP exam, to the extent possible, tests will be graded using the same rubric
used on the actual exam. Since the scoring system is different for the AP test, some adjustments (i.e. a
“curve”) will be used to calculate the students’ test grades for Stuarts Draft High School. (Since a 3/5 on
the AP exam is required to earn credit at most universities, that percentage (60%) will be approximately
equivalent to a D (75%) in my grade book.) Remember that students will have the opportunity to return
corrected tests for additional credit and that AP chemistry is a weighted grade. Quizzes and tests will
account for approximately 50% of the final grade.
Schedule, Text Sections & Topics for AP Chemistry
Week(s)
½
Chapter
Safety and
Technique
Summer
Ch. 1: Chemical
Foundations
Summer
Ch. 2: Atoms,
Molecules, and
Ions
Summer
+1
Ch. 3:
Stoichiometry
Topics Covered
-Discuss laboratory safety rules and expectations.
-Examine various instruments and glassware used in a laboratory.
-Identify proper laboratory techniques.
-Identify the steps and parts of the scientific method; design an experiment
using the steps.
-Define theory and law; distinguish between the two.
-Define SI base units of measurement and convert between metric units, English
units, and various temperature scales.
-Differentiate between accuracy and precision.
-Discuss various types of error and calculate percent error in an experiment.
-Define significant figures and discuss rules concerning reporting correct number
of sig. figs.
-Examine the properties of matter and classify properties as intensive or
extensive.
-Define the states (phases) of matter and their properties in terms of shape,
volume, and compressibility.
-Classify matter as a substance or mixture.
-Identify ways to separate mixtures such as filtering, chromatography, and
distillation.
-Chronologically list scientists and study of the atom; beginning with Democritus
to modern.
-Discuss Dalton’s Atomic Theory and modifications made to his postulation.
-Discuss Thomson’s and Millikan’s roles in discovering the mass and charge of
electrons.
-Describe Rutherford’s experiment and how it led to the discovery of the
nucleus.
-Define subatomic particles, their location, masses, and charges.
-Discuss the atomic scale and atomic mass units.
-Define quarks.
-Discuss and define isotopes.
-Distinguish between atomic mass, mass number, atomic number and determine
how to calculate each as it appears on the Periodic Table.
-Review parts of the Periodic Table such as group names.
-Define molecules and covalent network substances.
-Compare/contrast molecular and ionic compounds.
-Predict charges on ions and determine formulas for ionic compounds.
-Review naming rules for ionic and covalent compounds.
-Define moles and Avogadro’s number.
-Convert moles
- mol to gram (gram to mol)
- mol to particles (particles to mol)
-grams to particles (particles to grams)
-Calculate formula mass (molar mass of a compound).
-Calculate percent composition.
-Define empirical and molecular formulas; distinguish between the two.
-Discuss how ionic and molecular compounds are related to empirical and
molecular formulas.
-Calculate empirical formula and molecular formulas.
-Review chemical equations and information that may be obtained from the
equation.
Week(s)
Chapter
2
Ch. 4: Types of
Chemical
Reactions and
Solution
Stoichiometry
1
Ch. 5: Gases
1
Ch. 10: Liquids
and Solids
Topics Covered
-Review steps to solving stoichiometry problems and practice calculations.
-Identify limiting reactant (reagent) in a reaction.
-Review the classification of matter.
-Define a solution and identify parts: solute and solvent.
-Distinguish between saturate, unsaturated, and supersaturated solutions.
-Compare electrolytes and nonelectrolytes.
-Discuss dissociate and compare dissociate between ionic and molecular
compounds, and strong acids/bases and weak acids/bases.
-Define molarity.
-Calculate molarity and amount of solute needed to prepare solutions with
certain concentrations.
-Calculate concentration of diluted solutions.
-Identify types of reactions such as single-replacement, double-replacement, and
redox reactions.
-Discuss the activity series of metals and halogens.
-Determine and memorize solubility rules.
-Distinguish between oxidation and reduction.
-Discuss rules for assigning oxidation numbers.
-Predict products for redox reactions.
-Define ideal gases in terms of the Kinetic Molecular Theory.
-Discuss the nature of gases.
-Define pressure and identify ways/units of measuring pressure.
-Define standard temperature and pressure.
-Review converting between Celsius and Kelvin.
-Identify and calculate variables of the following gas laws:
-The Combined Gas Law
- Boyle’s Law
- Gay-Lussac’s Law
- Charles’ Law
- Avogadro’s Law
- The Ideal Gas Law
-Use molar volume to convert between moles and liters.
-Define density of gases and discuss the relationship between density and the
Ideal Gas Law.
-Solve gas stoichiometry problems.
-Discuss Dalton’s Law of Partial Pressures.
-Discuss the parts of the Kinetic Molecular Theory of Gases.
-Distinguish between diffusion and effusion.
-Calculate rates of effusion and diffusion using Graham’s laws.
-Compare real gases to ideal gases.
-Discuss/compare the magnitude of forces between intermolecular forces and
bonds.
-Discuss the following intermolecular forces:
-Hydrogen bonding
-London forces
-Describe how intermolecular forces are related to boiling points.
-Discuss the properties of liquids such as surface tension, viscosity, and capillary
action.
-Differentiate between the types of solids.
-Identify Bragg’s Law
-Discuss the types of crystalline structures (cubic, monoclinic, tetragonal,
orthorhombic)
Week(s)
Chapter
2
Ch. 6:
Thermochemistry
2
Ch. 8: Atomic
Structure and
Periodicity
1
Ch. 18: The
Nucleus
1
Ch. 8: Bonding:
General Concepts
Topics Covered
-Discuss the “packing” of metals.
-Examine the structure of metal alloys.
-Discuss the structure of solid molecular compounds.
-Define equilibrium vapor pressure.
-Interpret a phase diagram of water and discuss the phase changes.
-Interpret a triple-point diagram of water, carbon dioxide, carbon, and sulfur and
compare the diagrams.
-Define energy types and laws of conservation of mass (energy).
-Define heat and work in terms of the change in energy.
-Describe the relationship between work, volume, and pressure.
-Differentiate between endo- and exothermic reactions in terms of energy.
-Discuss calorimetry.
-Define joules.
-Identify a calorimeter and discuss how it works.
-Define specific heat.
-Perform calculations using specific heat.
-Identify Hess’ Law.
-Calculate the heat of reaction.
-Describe how atoms at like waves and particles.
-Discuss the electromagnetic spectrum, its components, and how it relates to
atomic structure.
-Describe the relationship between the energy of electromagnetic radiation and
frequency using the equation E = hλ.
-Discuss the relationship between wavelength, frequency, and energy.
-View the spectroscopic analysis of light.
-Discuss electron transitions and “jumps’ to different energy levels and evidence
to support this.
-Define quantum numbers and how to assign numbers.
-Utilize the Pauli Exclusion Principle to place electrons in orbitals.
-Define an orbital.
-Explain how the Schrödinger Wave Equation relates to finding electrons.
-Describe the Heinsburg Uncertainty Principle.
-Compare the different types of orbitals, their sizes, and shape.
-Describe the relationship between the Periodic Table and quantum numbers
and orbitals.
-Use the Periodic Table to fill orbital diagrams.
-Discuss some irregular electron configurations of transition metals.
-Discuss periodic trends such as atomic radii, first ionization energy, electron
affinity, electronegativity, and ionic radii.
-Identify nuclear symbols.
-Balance nuclear equations.
-Discuss and compare alpha decay and radiation, beta decay and radiation, and
gamma decay and radiation.
-Discuss the production of positrons.
-Define electron capture.
-Discuss nuclear stability.
-Define half-life and calculate the half-life of radioactive isotopes.
-Compare nuclear fission and fusion.
-Discuss how nuclear changes affect mass and energy.
-Examine a fission reactor and how it functions.
-Define electronegativity.
-Describe ionic bonding and character.
Week(s)
Chapter
1
Ch. 9: Covalent
Bonding:
Orbitals
2
Ch. 11 Properties
of Solutions
2
Spectroscopy and
Chromatography
2
Ch. 12 Chemical
Kinetics
2
Ch. 13 Chemical
Equilibrium
Topics Covered
-Identify Coulomb’s Law.
-Compare ionic radii and relationship to arrangement on Periodic Table.
-Describe and view the structure of ionic compounds, such as the crystal lattice
structure of NaCl.
-Describe covalent bonding and various intermolecular forces.
-Determine the relationship between bond length and energy and enthalpy.
-Review the Octet Rule.
-Discuss exceptions to the Octet Rule.
-Draw Lewis Structures.
-Compare double and triple bonding.
-Discuss resonance and its relationship to bond energy.
-Describe resonance in polyatomic ions.
-Use VSEPR to predict shapes of molecules.
-Discuss various molecular bonding theories including VSEPR, bond
hybridization, and molecular orbitals.
-Describe and predict geometries, bond angles, molecular polarities, and
molecular orbital configurations.
-Discuss the De-Localized Electron Model.
-Classify matter based on properties.
-Define the components of a solution.
-Perform calculations to determine mole fractions, molality, molarity, conversion
between concentration units, and dilution problems.
-Discuss trends in solubility such as temperature, surface area, pressure, and
“like dissolves like”.
-Define the different types of solutions.
-Interpret a solubility graph.
-Identify Henry’s Law and Raoult’s Law.
-Compare and contrast non-, weak- and strong electrolytes.
-Examine colligative properties and determine molar mass from colligative
properties.
-Define colloids and identify their properties.
-Describe the Tyndall Effect.
-Define spectroscopy and chromatography.
-Discuss how each is used to identify chemicals.
-Examine various spectra.
-Identify Beer’s Law.
-Research the theory and mechanisms related to spectroscopy and
chromatography.
-Examine a laboratory using spectroscopy and chromatography.
-Define reaction rate.
-Write a differential rate law.
-Determine order using concentration and time data.
-Discuss integrated rate laws.
-Calculate rate constants.
-Identify rate-determining steps and intermediates of a reaction.
-Examine the Collision Model.
-Discuss the factors that affect rate of reactions.
-Compare and contrast endo- and exothermic reactions.
-Identify and perform calculations using the Arrhenius Equation.
-Discuss catalysts and their affects on reaction rates.
-Define chemical equilibrium.
-Define and calculate equilibrium constant.
Week(s)
Chapter
2
Ch. 14 Acids and
Bases
2
Ch. 15
Applications of
Aqueous
Equilibria
2
Ch. 16
Spontaneity,
Entropy, and Free
Energy
Ch. 17
Electrochemistry
2
1
Ch. 20 Transition
Metals and
Coordination
Chemistry
1
Ch. 22 Organic
and Biological
Molecules
Topics Covered
-Interpret an equilibrium constant expression.
-Calculate the equilibrium concentration given the original concentration.
-Define LeChatlier’s Principle.
-Predict the direction of a reaction using LeChatlier’s Principle.
-Define and identify acids and bases based on different definitions.
-Discuss the relationship between pH, pOH, and [H+] [OH-] and perform
calculations.
-Discuss reactions of acids/bases in water (proper ionic notation) and acid/base
titrations.
-Interpret acid/base titration curves and determine pH at endpoint and
equivalence point.
-Define Ka, Kb (for strong acids and bases) and determine Ka from pH and
percent dissociation.
-Discuss the properties of salts.
-Discuss the reaction of weak bases with water.
-Define buffers, describe how they work, and how they are made,
-Identify Acid/salt and Base/salt buffer pairs.
-Examine a graph of a buffered solution.
-Perform calculations using the Henderson-Hasselbalch Equation.
-Define indicators and examine the pH range of various ones.
-Interpret Ksp expressions and solve solubility problems.
-Use the solubility rules to determine the formation of a precipitate.
-Describe the common ion effect.
-Define Spontaneity, Entropy, and Gibb’s Free Energy.
-Determine the values of each for reactions using data tables.
-Describe the 2nd Law of Thermodynamics.
-Describe the relationship between free energy, pressure, equilibrium, and work.
-Identify rules for assigning oxidation numbers, oxidizing and reducing agents,
and balancing redox reactions.
-Examine electrochemical cells and identify components.
-Determine the standard cell potential for a given cell.
-Perform calculations using the Nerst Equation.
-Determine the strength of oxidizing and reducing agents.
-Calculate the equilibrium constant from cell potential.
-Describe the electrolysis of water and electroplating of silver.
-Describe the electron configurations of transition metals.
-Define coordination compounds.
-Define ligands and identify some common ligands.
-Discuss rules for naming coordination compounds.
-Discuss the various types of isomerism.
-Describe bonding in complex ions.
-Explain the Crystal Field Model.
-Distinguish between alkanes, alkenes, and alkynes.
-Discuss nomenclature rules for each.
-Discuss isomerism and geometry of simple organic compounds.
AP Chemistry Laboratories
Prior to the first lab, students and parents must sign a safety contract. Students are expected to follow
proper laboratory procedures and safety rules at all times. All of our safety depends on your behavior.
Students are expected to read each experiment before the laboratory period. Laboratory periods may
include additional time outside of the regular class schedule. Students are expected to outline the
experiment and procedures before the day of a lab. To receive credit, all lab reports must be done in a
bound composition notebook and written in DARK ink. All procedures, data, calculations and conclusions
must be entered in your notebook. Do not use loose-leaf paper except for taking notes and rough drafts.
Students may work with a lab partner and/or group depending on the experiment. Each student is
responsible for entering all data and calculations in their own notebook. Lab notebooks will be graded
according to neatness & organization, data & observations, calculations & results, and the conclusion. Lab
reports will count for approximately 30% of the final grade.
Laboratory Notebook
Each student is required to have a bound composition notebook for laboratory experiments and organized
according to the following format:
1. Table of Contents: Allow two pages for the table of contents. The table of contents should be labeled and
have three columns: a column for the date of the experiment; a column for the name of the experiment;
and a column for the page number where the experiment can be found.
2. Page numbers: All pages of a lab notebook are consecutively numbered in the upper right hand corner
of the page. The first page, the Table of Contents, should be labeled “1” and the back of that page
labeled “2” and so on. Also, please date each page as you fill it in.
3. Experiments:
a. Before the experiment have the following completed and labeled:
i. Title of the lab on the top line of the first page for that experiment.
ii. Partner’s name(s)
iii. Purpose (What is the question or hypothesis being investigated?)
iv. Reactions (List the reaction(s) that will occur during your investigation.)
v. Materials: (List the equipment and reagents (chemicals) used in the experiment. A labeled
drawing is often the best way to describe the set-up.)
vi. Procedure: (Make a step-by-step description of what you will be doing and how. Be sure to
include any important or unusual safety concerns and/or key procedural hurdles.)
In order to be safe and successful in the lab, students must know what to expect and how to safely
complete the experiment. Unprepared students will not be allowed to participate in the lab and will have
to make up the experiment on their own time for reduced credit. DO NOT expect to do the “pre-lab” in
class on the day of the lab. Plan ahead if you know you’re going to be gone. It is not always possible to
have all of the materials and equipment available outside of the pre-scheduled lab time.
For the lab experience to be of value to the student, the chemical concepts being studied in the
experiment should be well understood. This does not mean that you should know exactly what to expect,
but, if you have no idea what is going on, you will miss the point of the lab. You will also lower your
grade and, perhaps, injure yourself and/or your classmates. Please take the time to be prepared for lab.
It will be much more fun and rewarding for all of us!
b. During the experiment you will need to make observations and collect data:
i. Observations: Some data is qualitative rather than quantitative. Record unusual and/or
significant occurrences. Be sure to look for signs of physical and chemical changes. Pay attention
to any conditions that might interfere with measurements or data collection.
ii. Data: This section will typically consists of data tables or an organized means of recording data
from experiments. Record data using the correct number of significant figures and proper units of
measure. If students make an error when recording data, strike through the data (with a
SINGLE LINE), initial the strike-through, and record the correct data above the “incorrect” data.
If possible, include an explanation as to why there was a mistake. Never try to make up or
“fudge” data to fit expectations. Credit will be given for clear explanations of the source of error
and opportunities to collect more (“better”) data will be provided.
c.
After the experiment has been completed you will often have calculations to do.
i. Calculations: In this section, students will perform all required calculations as well as a percent
error calculation (if possible). Include all formulas used, show every step, record the correct
number of significant figures and use the correct unit of measure. If an error is made, follow the
“strike-through” procedures above. Do not make up or “fudge” data if the calculations do not
work out as expected. Full credit will be given for adequate explanations of errors and/or
opportunities to go back and collect better data will be provided.
ii. Conclusion: Every lab report must include a conclusion that addresses the purpose, sources of
error, and significance of the experiment. (Did you accomplish the purpose? Was the hypothesis
proven or not? What could have or did cause errors in data collection and how could they be
avoided? What is the significance of the experiment in terms of the chemical topics being studied
as well as the broader context of the world?) The conclusion should be written in complete
sentences and may include several paragraphs. Be concise and clear.
4. Turning in the Lab Notebook
a. After all the sections above are complete, the lab notebook must be turned in for a grade. Students
will be given approximately two days after a lab to complete this task. Collaboration is OK, but each
student must write his/her own conclusions based on his/her own data. A discussion of the differences
in results between lab groups is appropriate in the conclusion.
b. Lab notebooks will be graded according to neatness & organization, data & observations, calculations
& results, and the conclusion. Lab reports will count for approximately 30% of the final grade.
AP Chemistry Lab Sequence, Topic, Objective & Time (approximate)
Laboratory Experiment
Chapter(s)
Objective/Purpose
Time
(hr)
Determination of the Formula of a
Compound: Magnesium Oxide
(Determination of formula of a compound)
Determination of the Percent Copper in a
Post-1982 Penny (Determination of formula
1-3
Determine the correct formula
for magnesium oxide.
2.0
1-3
Determine the percent of copper
in a post-1982 penny.
05
Percentage of Water in a Hydrate
(Determination of the percentage of water
1-3
Determine the amount of water
in an ionic hydrate.
1.5
Finding the Ratio of Moles of Reactants in a
Chemical Reaction (Determination of mass
1-3
Use the method of continuous
variations to determine the
correct stoichiometric ratio of
two reactants.
1.5
Gravimetric Analysis (Analytical gravimetric
1-3
1.5
Molecular Weight by Freezing Point
Depression (Determination of freezing
4, 11
“Flick Your Bic!” Molar Mass of Lighter Fluid
5
Test gravimetric stoichiometry
by predicting and determining
the mass of precipitate produced
by the reaction of aqueous
strontium chloride and aqueous
sodium carbonate.
Determine the molar mass of an
unknown substance by
measuring the freezing point
depression of a solution of the
unknown substance and BHT.
Determine the molar mass of
lighter fluid.
Determine the molar volume of
hydrogen gas.
Determine the NaOCl content of
laundry bleach.
1.5
Determine a value for the
equilibrium constant for the
reaction between iron (III)
nitrate and potassium
thiocyanate.
Separate a mixture of dyes in
water soluble ink.
Calculate the heat of formation
of magnesium oxide using Hess’s
Law.
Determine the orders for the
reactants, rate expression, and
the rate constant for the reaction
between iodine and acetone.
Prepare and standardize a
solution of sodium hydroxide and
1.5
of a compound)
in a compound)
and mole relationship in a chemical
reaction)
analysis)
point depression)
(Determination of the molar mass by
density)
Molar Volume of a Gas (Determination of
the molar volume of gas)
5
Oxidizing Power of Laundry Bleach
4, 11
Spectrophotometric Determination of an
Equilibrium Constant (Colorimetric or
13
Magic Marker Chromatography (Separation
-
Heat’s of Reaction and Hess’s Law
6
(Determination of concentration by a redox
titration)
spectrophotometric analysis)
by chromatography)
(Determination of enthalpy change
associated with a reaction)
Iodination of Acetone (Determine the rate
of reaction and its order)
Standardization of a Base- Analysis of
Vinegar (Standardization of a solution
12
14-15
2.5
1.0
2.0
1.0
2.0
1.5
2.5
using a primary standard; Determination of
concentration by acid-base titration,
including a weak acid or base;
determination of the appropriate indicators
for various acid-base titrations and pH
determination)
Determining the Ksp for Silver Acetate
(Determination of the equilibrium constant
for a reaction)
Identification of Solutions (Separation and
qualitative analysis of cations and anions)
use it to determine the percent
acetic acid in a commercial
vinegar sample.
15
Determine the solubility constant
for silver acetate.
2.5
15
Determine the identity of
unknown solutions by observing
the physical and chemical
properties and the reactivity of
each.
Prepare buffer solutions and
determine their buffer capacity.
2.0
Construct an activity series for a
list of metallic elements.
Measure cell voltage for different
combinations of metals using
“microvoltaic” cells.
1.5
Buffer Preparation and Buffer Capacity
15
The Activity Series of the Metals
17
Electrochemistry: Voltaic Cells
17
(Preparation and properties of buffer
solutions)
(Determination of electrochemical series)
2.5
1.5
(Measurements using electrochemical cells
and electroplating)
Laboratory Resources: Laboratory classroom includes space, facilities and equipment to conduct handson, inquiry-based investigations including molecular model kits, analytical balances, titration apparatus,
spectrophotometers, calorimeters, volumetric glassware, vacuum pump, separatory apparatus,
temperature and pH probes, and conductivity sensors.