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AP Correlations for Advanced Chemistry with Vernier

The College Board’s AP* Chemistry Curriculum Framework has undergone significant changes. The new standards will go into effect for the 2013-2014 school year.

Table 1 outlines the correlation of the Primary Learning Objective in the 16 lab investigations from AP® Chemistry Guided-Inquiry Experiments: Applying the Science Practices and the Vernier lab book Advanced Chemistry with Vernier.

Table 2 correlates Learning Objectives from the new Curriculum Framework to each lab experiment in the Vernier lab book Advanced Chemistry with Vernier.

Table 1

College Board Vernier Experiment
Lab Primary Learning Objective
1 1.15 17. Determining the Concentration of a Solution: Beer’s Law
2 1.16 17. Determining the Concentration of a Solution: Beer’s Law
3 1.19 1. The Determination of a Chemical Formula
4 1.20 7. Acid-Base Titration
7 3.5 1. The Determination of a Chemical Formula
8 3.9 8. An Oxidation-Reduction Titration: The Reaction of Fe2+ and Ce4+
9 3.10 22. The Synthesis and Analysis of Aspirin
10 4.1 12. The Decomposition of Hydrogen Peroxide
25. The Rate and Order of a Chemical Reaction
11 4.2 35. Rate Determination and Activation Energy
25. The Rate and Order of a Chemical Reaction
12 5.7 26. The Enthalpy of Neutralization of Phosphoric Acid
13 6.9 10. The Determination of an Equilibrium Constant
14 6.13 7. Acid-Base Titration
15 6.20 19. Buffers
7. Acid-Base Titration
16 6.18 19. Buffers
7. Acid-Base Titration

Table 2

Vernier Experiment Learning Objective from the AP Chemistry 2013 Framework
1. The Determination of a Chemical Formula 1.19: The student can design, and/or interpret data from, an experiment that uses gravimetric analysis to determine the concentration of an analyte in a solution.
3.3: The student is able to use stoichiometric calculations to predict the results of performing a reaction in the laboratory and/or to analyze deviations from the expected results.
3.5: The student is able to design a plan in order to collect data on the synthesis or decomposition of a compound to confirm the conservation of matter and the law of definite proportions.
2. The Determination of the Percent Water in a Compound 3.3: The student is able to use stoichiometric calculations to predict the results of performing a reaction in the laboratory and/or to analyze deviations from the expected results.
3. The Molar Mass of a Volatile Liquid 1.4: The student is able to connect the number of particles, moles, mass, and volume of substances to one another, both qualitatively and quantitatively.
4. Using Freezing-Point Depression to Find Molecular Weight (No correlation, removed from the AP Chem curriculum)
5. The Molar Volume of a Gas 1.4: The student is able to connect the number of particles, moles, mass, and volume of substances to one another, both qualitatively and quantitatively.
6. Standardizing a Solution of Sodium Hydroxide 1.20: The student can design, and/or interpret data from, an experiment that uses titration to determine the concentration of an analyte in a solution.
7. Acid-Base Titration 1.20: The student can design, and/or interpret data from, an experiment that uses titration to determine the concentration of an analyte in a solution., 6.13: The student can interpret titration data for monoprotic or polyprotic acids involving titration of a weak or strong acid by a strong base (or a weak or strong base by a strong acid) to determine the concentration of the titrant and the pKa for a weak acid, or the pKb for a weak base.
8. An Oxidation-Reduction Titration: The Reaction of Fe2+ and Ce4+ 1.20: The student can design, and/or interpret data from, an experiment that uses titration to determine the concentration of an analyte in a solution.
3.9: The student is able to design and/or interpret the results of an experiment involving a redox titration.
9. Determining the Mole Ratios in a Chemical Reaction 3.3: The student is able to use stoichiometric calculations to predict the results of performing a reaction in the laboratory and/or to analyze deviations from the expected results.
10. The Determination of an Equilibrium Constant 6.5: The student can, given data (tabular, graphical, etc.) from which the state of a system at equilibrium can be obtained, calculate the equilibrium constant, K.
6.9: The student is able to use LeChatelier’s principle to design a set of conditions that will optimize a desired outcome, such as product yield.
11. Investigating Indicators (No match to a Learning Objective)
12. The Decomposition of Hydrogen Peroxide 4.1: The student is able to design and/or interpret the results of an experiment regarding the factors (i.e., temperature, concentration, surface area) that may influence the rate of a reaction.
4.2: The student is able to analyze concentration vs. time data to determine the rate law for a zeroth-, first-, or second-order reaction.
13. Determining the Enthalpy of a Chemical Reaction 3.11: The student is able to interpret observations regarding macroscopic energy changes associated with a reaction or process to generate a relevant symbolic and/or graphical representation of the energy changes.
14 A&B. Separation and Qualitative Analysis of Cations and Anions 3.10: The student is able to evaluate the classification of a process as a physical change, chemical change, or ambiguous change based on both macroscopic observations and the distinction between rearrangement of covalent interactions and noncovalent interactions.
15 A&B. The Synthesis and Analysis of Alum 3.10: The student is able to evaluate the classification of a process as a physical change, chemical change, or ambiguous change based on both macroscopic observations and the distinction between rearrangement of covalent interactions and noncovalent interactions.
16. Conductimetric Titration and Gravimetric Determination of a Precipitate 1.19: The student can design, and/or interpret data from, an experiment that uses gravimetric analysis to determine the concentration of an analyte in a solution.
17. Determining the Concentration of a Solution: Beer’s Law 1.15: The student can justify the selection of a particular type of spectroscopy to measure properties associated with vibrational or electronic motions of molecules.
1.16: The student can design and/or interpret the results of an experiment regarding the absorption of light to determine the concentration of an absorbing species in a solution.
18. Liquid Chromatography 2.10: The student can design and/or interpret the results of a separation experiment (filtration, paper chromatography, column chromatography, or distillation) in terms of the relative strength of interactions among and between the components.
19. Buffers 6.18: The student can design a buffer solution with a target pH and buffer capacity by selecting an appropriate conjugate acid-base pair and estimating the concentrations needed to achieve the desired capacity.
6.20: The student can identify a solution as being a buffer solution and explain the buffer mechanism in terms of the reactions that would occur on addition of acid or base.
20. Electrochemistry: Voltaic Cells 3.13: The student can analyze data regarding galvanic or electrolytic cells to identify properties of the underlying redox reactions.
21. Electroplating 3.12: The student can make qualitative or quantitative predictions about galvanic or electrolytic reactions based on half-cell reactions and potentials and/ or Faraday’s laws.
3.13: The student can analyze data regarding galvanic or electrolytic cells to identify properties of the underlying redox reactions.
22. The Synthesis and Analysis of Aspirin 3.10: The student is able to evaluate the classification of a process as a physical change, chemical change, or ambiguous change based on both macroscopic observations and the distinction between rearrangement of covalent interactions and noncovalent interactions.
23. Determining the Ksp of Calcium Hydroxide 1.20: The student can design, and/or interpret data from, an experiment that uses titration to determine the concentration of an analyte in a solution.
24. Determining Ka by the Half-Titration of a Weak Acid 1.20: The student can design, and/or interpret data from, an experiment that uses titration to determine the concentration of an analyte in a solution.
25. The Rate and Order of a Chemical Reaction 4.1: The student is able to design and/or interpret the results of an experiment regarding the factors (i.e., temperature, concentration, surface area) that may influence the rate of a reaction.
4.2: The student is able to analyze concentration vs. time data to determine the rate law for a zeroth-, first-, or second-order reaction.
26. The Enthalpy of Neutralization of Phosphoric Acid 3.11: The student is able to interpret observations regarding macroscopic energy changes associated with a reaction or process to generate a relevant symbolic and/or graphical representation of the energy changes.
5.7: The student is able to design and/or interpret the results of an experiment in which calorimetry is used to determine the change in enthalpy of a chemical process (heating/cooling, phase transition, or chemical reaction) at constant pressure.
27. α, β, and γ (No match to a Learning Objective)
28. Radiation Shielding (No match to a Learning Objective)
29. The Base Hydrolysis of Ethyl Acetate (No match to a Learning Objective)
30. Exploring the Properties of Gases 2.4: The student is able to use KMT and concepts of intermolecular forces to make predictions about the macroscopic properties of gases, including both ideal and nonideal behaviors.
31. Determining Avogadro’s Number 3.12: The student can make qualitative or quantitative predictions about galvanic or electrolytic reactions based on half-cell reactions and potentials and/ or Faraday’s laws.
32. Potentiometric Titration of Hydrogen Peroxide 3.9: The student is able to design and/or interpret the results of an experiment involving a redox titration.
33. Determining the Half-Life of an Isotope (No match to a Learning Objective)
34. Vapor Pressure and Heat of Vaporization 5.6: The student is able to use calculations or estimations to relate energy changes associated with heating/cooling a substance to the heat capacity, relate energy changes associated with a phase transition to the enthalpy of fusion/vaporization, relate energy changes associated with a chemical reaction to the enthalpy of the reaction, and relate energy changes to PΔV work.
35. Rate Determination and Activation Energy 4.1: The student is able to design and/or interpret the results of an experiment regarding the factors (i.e., temperature, concentration, surface area) that may influence the rate of a reaction.
4.2: The student is able to analyze concentration vs. time data to determine the rate law for a zeroth-, first-, or second-order reaction.

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