AP Chemistry and Advanced Chemistry with Vernier

We have correlated the experiments from Advanced Chemistry with Vernier to the 21 lab experiments recommended by AP*.

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AP Recommended Experiment		Vernier Experiment and Objectives
1	Determination of the formula of a compound	Experiment 1: The Determination of a Chemical Formula Determine the water of hydration in a copper chloride hydrate sample. Conduct a reaction between a solution of copper chloride and solid aluminum. Use the results of the reaction to determine the mass and moles of Cu and Cl in the reaction. Calculate the empirical formula of the copper chloride compound.
2	Determination of the percentage of water in a hydrate	Experiment 2: The Determination of the Percent Water in a Compound Carefully heat a measured sample of a hygroscopic ionic compound. Determine the water of hydration of the compound. Complete the chemical formula of the compound.
3	Determination of Molar Mass by Vapor Density	Experiment 3: Determination of Molar Mass by Vapor Density Evaporate a liquid substance and measure its physical properties as it evaporates. Determine the molar mass of an unknown liquid.
4	Determination of molar mass by freezing-point depression	Experiment 4: Using Freezing-Point Depression to Find Molecular Weight Determine the freezing temperature of the pure solvent, lauric acid. Determine the freezing temperature of a mixture of lauric acid and benzoic acid. Calculate the freezing point depression of the mixture. Calculate the molecular weight of benzoic acid.
5	Determination of molar mass of a gas	Experiment 5: The Molar Volume of a Gas Measure the gas production of a chemical reaction by a pressure change. Determine the molar volume of the gas produced in the reaction. Calculate the molar volume of a gas at STP.
6	Standardization of a solution using a primary standard	Experiment 6: Standardizing a Solution of Sodium Hydroxide Prepare an aqueous solution of sodium hydroxide to a target molar concentration. Determine the concentration of your NaOH solution by titrating it with a solution of potassium hydrogen phthalate, abbreviated KHP, of precise molar concentration.
7	Determination of concentration by acid-base titration, including a weak acid or weak base	Experiment 7: Acid-Base Titration Accurately conduct acid-base titrations. Determine the equivalence point of a strong acid - strong base titration. Determine the equivalence point of a weak acid - strong base titration. Calculate the molar concentrations of two acid solutions.
8	Determination of concentration by oxidation-reduction titration	Experiment 8: An Oxidation-Reduction Titration: The Reaction of Fe²⁺ and Ce⁴⁺ Conduct the potentiometric titration of the reaction between ferrous ammonium sulfate hexahydrate and ammonium cerium (IV) nitrate. Measure the potential change of the reaction. Determine the molar concentration of iron (II) ions in a sample of ferrous ammonium sulfate hexahydrate.
9	Determination of mass and mole relationship in a chemical reaction	Experiment 9: Determining the Mole Ratios in a Chemical Reaction Measure the enthalpy change of a series of reactions. Determine the stoichiometry of an oxidation-reduction reaction in which the reactants are known but the products are unknown.
10	Determination of the equilibrium constant for a chemical reaction	Experiment 10: The Determination of an Equilibrium Constant Prepare and test standard solutions of FeSCN²⁺ in equilibrium. Test solutions of SCN⁻ of unknown molar concentration. Determine the molar concentrations of the ions present in an equilibrium system. Determine the value of the equilibrium constant, K_eq.
11	Determination of appropriate indicators for various acid-base titrations; pH determination	Experiment 11: Investigating Indicators Conduct strong acid-strong base titrations using solutions of hydrochloric acid and sodium hydroxide, and three different indicator solutions. Select the proper indicator to use with a titration involving a weak acid or a weak base, based on your observations and measurements.
12	Determination of the rate of a reaction and its order	Experiment 12: The Decomposition of Hydrogen Peroxide Conduct the catalyzed decomposition of hydrogen peroxide under various conditions. Calculate the rate constant for the reaction. Determine the rate law for the reaction. Calculate the activation energy for the reaction.
13	Determination of enthalpy change associated with a reaction	Experiment 13: Determining the Enthalpy of a Chemical Reaction Use Hess's Law to determine the enthalpy change of the reaction between aqueous ammonia and aqueous hydrochloric acid. Compare your calculated enthalpy change with the experimental results.
14	Separation and qualitative analysis of cations and anions	Experiment 14A: Separation and Qualitative Analysis of Cations Prepare and analyze a solution that contains ten selected cations. Analyze an unknown solution that contains a selection of cations. Experiment 14B: Separation and Qualitative Analysis of Anions Prepare and analyze a solution that contains six selected anions. Analyze an unknown solution that contains a selection of anions.
15	Synthesis of a coordination compound and its chemical analysis	Experiment 15A: The Synthesis of Alum Synthesize a sample of potassium aluminum sulfate dodecahydrate (alum). Observe and record the process of synthesizing a compound. Calculate the percent yield of your synthesis. Experiment 15B: The Analysis of Alum Determine the melting temperature of a sample of alum. Determine the water of hydration of a sample of alum. Determine the percent sulfate of a sample of alum. Verify the chemical formula of a sample of alum.
16	Analytical gravimetric determination	Experiment 16: Conductimetric Titration and Gravimetric Determination of a Precipitate Measure the conductivity of the reaction between sulfuric acid and barium hydroxide. Use conductivity values as a means of determining the equivalence point of the reaction. Measure the mass of a product of the reaction as a means of determining the equivalence point of the reaction gravimetrically. Calculate the molar concentration of a barium hydroxide solution.
17	Colorimetric or spectrophotometric analysis	Experiment 17: Determining the Concentration of a Solution: Beer's Law Prepare and test the absorbance of five standard copper (II) sulfate solutions. Calculate a standard curve from the test results of the standard solutions. Test the absorbance of a copper (II) sulfate solution of unknown molar concentration. Calculate the molar concentration of the unknown CuSO4 solution.
18	Separation by chromatography	Experiment 18: Liquid Chromatography Conduct an liquid chromatographic separation. Conduct a step gradient chromatographic separation. Complete the necessary measurements and calculations to evaluate the components of a mixture that have been separated by liquid chromatography.
19	Preparation and properties of buffer solutions	Experiment 19: Buffers Evaluate a standard buffer solution. Prepare and test an acid buffer solution. Determine the buffer capacity of the standard buffer and the prepared buffer.
20	Determination of electrochemical series	Experiment 20: Electrochemistry: Voltaic Cells Prepare a Cu-Pb voltaic cell and measure its potential. Test two voltaic cells that use unknown metal electrodes to identify the metals. Prepare copper and lead concentration cells, observe, and measure their respective cell potentials. Use the Nernst equation to calculate the K_sp of PbI₂.
21	Measurements using electrochemical cells and electroplating	Experiment 21: Electroplating Prepare and operate an electrochemical cell to plate copper onto a brass surface. Measure the amount of copper that was deposited in the electroplating process. Calculate the amount of energy used to complete the electroplating process.
22	Synthesis, purification, and analysis of an organic compound	Experiment 22: The Synthesis and Analysis of Aspirin Synthesize a sample of acetylsalicylic acid (aspirin). Calculate the percent yield of your synthesis. Measure the melting temperature of your aspirin sample. Conduct a colorimetric analysis of your aspirin sample.

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