CHM2046L Final Exam at the University of Florida, complete
with a 200-question practice exam and detailed answer
rationales. CHM2046L Final Exam Study Guide – Spring 2026
This guide is designed to help you prepare for the CHM2046L (General Chemistry II Laboratory)
final exam at the University of Florida. It covers key concepts, laboratory techniques, and
common experiments, and includes a 200-question practice exam with verified answers and
rationales. Use this as a supplementary resource to your course materials, lab manual, and
lecture notes.
Key Topics & Lab Experiments Covered
The CHM2046L course is designed to introduce you to common laboratory techniques, help you
gain proficiency in their use, and explore the process of doing experimental chemistry. The final
exam typically covers the following major topic areas and lab experiments:
Experiment 1 & 2: Analysis of Florida Water (EDTA Titrations): Hardness of water samples
(Ca²⁺, Mg²⁺), complexometric titrations with EDTA, calculation of water hardness in ppm CaCO₃,
and the use of ion-exchange resins.
Experiment 3: Beer-Lambert Law & Spectroscopy: Relationship between absorbance and
concentration (A = εlc), generation and use of a calibration curve, determination of unknown
concentrations, and the use of a spectrophotometer.
Experiment 4: Kinetics – Iodine Clock Reaction: Determining the rate law, orders of reaction
(method of initial rates), rate constant (k), and activation energy (Ea) using the Arrhenius
equation.
Experiment 5 & 6: Chemical Equilibrium – Finding Kc: Using spectrophotometry to find the
equilibrium constant for a reaction (e.g., Fe³⁺ + SCN⁻ ⇌ [FeSCN]²⁺). ICE tables and the
equilibrium expression.
Experiment 7: Le Châtelier's Principle – Buffers: Common ion effect, pH of buffer solutions
(Henderson-Hasselbalch equation), buffer capacity, and qualitative observations of equilibrium
shifts.
, Experiment 8: Titration Curves & pKa: Acid-base titrations (strong acid/strong base, weak
acid/strong base), pH curves, equivalence points, half-equivalence points, and determination of
pKa using a pH meter.
Experiment 9: Qualitative Analysis – Solubility & Complex Ions: Identification of unknown
cations and anions using selective precipitation and complex ion formation. Cation groups (e.g.,
Ag⁺, Pb²⁺, Hg₂²⁺) and anion tests (e.g., Cl⁻, SO₄²⁻, CO₃²⁻).
Experiment 10: Electrochemistry – Voltaic Cells: Construction of voltaic cells, measurement of
cell potential (E°cell), use of the Nernst equation, relationship between ΔG° and E°cell (ΔG° = -
nFE°cell).
Experiment 11: Synthesis of an Organic Compound (Aspirin): Synthesis, recrystallization, and
percent yield calculations.
Experiment 12: Introduction to Organic Chemistry and Polymer Synthesis: Preparation of
nylon, understanding of condensation polymerization.
---
200-Question Practice Exam – CHM2046L Final Exam (Spring 2026)
Instructions: Each question is followed by the correct answer and a detailed rationale. Use these
to test your knowledge and deepen your understanding of the key concepts.
---
Topic 1: Analysis of Florida Water – EDTA Titrations (Questions 1–30)
1. What is the primary goal of the "Analysis of Florida Water" experiment?
A. To determine the salinity of the water.
B. To measure the pH of the water.
C. To determine the total hardness of the water in terms of CaCO₃.
,D. To measure the concentration of dissolved oxygen in the water.
Correct Answer: C
Rationale: The main objective is to determine the water hardness by measuring the
concentration of Ca²⁺ and Mg²⁺ ions in a water sample, expressed as ppm of CaCO₃.
2. In the EDTA titration, what is the role of the indicator calmagite?
A. It binds to the EDTA to make it visible.
B. It forms a colored complex with the Ca²⁺ and Mg²⁺ ions before the titration.
C. It changes color when the solution becomes basic.
D. It buffers the solution to a specific pH.
Correct Answer: B
Rationale: Calmagite is a metal indicator that forms a wine-red complex with Ca²⁺ and Mg²⁺
ions. As EDTA is added, it preferentially binds to the metal ions, and at the endpoint, the
indicator is free and the solution turns blue.
3. A student forgot to add the ammonia-ammonium chloride buffer (pH = 10) to the water
sample before titration. What would be the expected outcome?
A. The endpoint would occur prematurely, and the calculated hardness would be too high.
B. The calculated hardness would be accurate because EDTA titrates Ca²⁺ and Mg²⁺ at any pH.
C. Mg²⁺ would precipitate as Mg(OH)₂ and would not be titrated, causing the calculated
hardness to be too low.
D. The indicator would not be able to bind to the metal ions, and no color change would occur.
, Correct Answer: C
Rationale: The buffer maintains a pH of 10, which is necessary to keep Mg²⁺ in solution. Without
it, Mg(OH)₂ precipitates and is not titrated, leading to a falsely low measurement of total water
hardness.
4. A 100.0 mL water sample required 18.35 mL of 0.01000 M EDTA to reach the endpoint.
Calculate the concentration of CaCO₃ in the sample in mg/L (ppm). (Molar mass CaCO₃ = 100.09
g/mol)
A. 36.7 ppm
B. 73.4 ppm
C. 183.5 ppm
D. 367.0 ppm
Correct Answer: C
Rationale: Moles EDTA = 0.01835 L × 0.01000 mol/L = 1.835 × 10⁻⁴ mol. Since 1 mol EDTA reacts
with 1 mol CaCO₃, moles CaCO₃ = 1.835 × 10⁻⁴ mol. Mass CaCO₃ = (1.835 × 10⁻⁴ mol)(100.09
g/mol) = 0.01836 g = 18.36 mg. Concentration = (18.36 mg)/(0.1000 L) = 183.6 ppm.
5. If the water sample had been "hard" water, which of the following would you expect to
observe during the titration?
A. The sample would require more EDTA to reach the endpoint.
B. The sample would require less EDTA to reach the endpoint.
C. The initial color of the solution would be blue instead of wine-red.
D. The titration would proceed much faster.
Correct Answer: A
with a 200-question practice exam and detailed answer
rationales. CHM2046L Final Exam Study Guide – Spring 2026
This guide is designed to help you prepare for the CHM2046L (General Chemistry II Laboratory)
final exam at the University of Florida. It covers key concepts, laboratory techniques, and
common experiments, and includes a 200-question practice exam with verified answers and
rationales. Use this as a supplementary resource to your course materials, lab manual, and
lecture notes.
Key Topics & Lab Experiments Covered
The CHM2046L course is designed to introduce you to common laboratory techniques, help you
gain proficiency in their use, and explore the process of doing experimental chemistry. The final
exam typically covers the following major topic areas and lab experiments:
Experiment 1 & 2: Analysis of Florida Water (EDTA Titrations): Hardness of water samples
(Ca²⁺, Mg²⁺), complexometric titrations with EDTA, calculation of water hardness in ppm CaCO₃,
and the use of ion-exchange resins.
Experiment 3: Beer-Lambert Law & Spectroscopy: Relationship between absorbance and
concentration (A = εlc), generation and use of a calibration curve, determination of unknown
concentrations, and the use of a spectrophotometer.
Experiment 4: Kinetics – Iodine Clock Reaction: Determining the rate law, orders of reaction
(method of initial rates), rate constant (k), and activation energy (Ea) using the Arrhenius
equation.
Experiment 5 & 6: Chemical Equilibrium – Finding Kc: Using spectrophotometry to find the
equilibrium constant for a reaction (e.g., Fe³⁺ + SCN⁻ ⇌ [FeSCN]²⁺). ICE tables and the
equilibrium expression.
Experiment 7: Le Châtelier's Principle – Buffers: Common ion effect, pH of buffer solutions
(Henderson-Hasselbalch equation), buffer capacity, and qualitative observations of equilibrium
shifts.
, Experiment 8: Titration Curves & pKa: Acid-base titrations (strong acid/strong base, weak
acid/strong base), pH curves, equivalence points, half-equivalence points, and determination of
pKa using a pH meter.
Experiment 9: Qualitative Analysis – Solubility & Complex Ions: Identification of unknown
cations and anions using selective precipitation and complex ion formation. Cation groups (e.g.,
Ag⁺, Pb²⁺, Hg₂²⁺) and anion tests (e.g., Cl⁻, SO₄²⁻, CO₃²⁻).
Experiment 10: Electrochemistry – Voltaic Cells: Construction of voltaic cells, measurement of
cell potential (E°cell), use of the Nernst equation, relationship between ΔG° and E°cell (ΔG° = -
nFE°cell).
Experiment 11: Synthesis of an Organic Compound (Aspirin): Synthesis, recrystallization, and
percent yield calculations.
Experiment 12: Introduction to Organic Chemistry and Polymer Synthesis: Preparation of
nylon, understanding of condensation polymerization.
---
200-Question Practice Exam – CHM2046L Final Exam (Spring 2026)
Instructions: Each question is followed by the correct answer and a detailed rationale. Use these
to test your knowledge and deepen your understanding of the key concepts.
---
Topic 1: Analysis of Florida Water – EDTA Titrations (Questions 1–30)
1. What is the primary goal of the "Analysis of Florida Water" experiment?
A. To determine the salinity of the water.
B. To measure the pH of the water.
C. To determine the total hardness of the water in terms of CaCO₃.
,D. To measure the concentration of dissolved oxygen in the water.
Correct Answer: C
Rationale: The main objective is to determine the water hardness by measuring the
concentration of Ca²⁺ and Mg²⁺ ions in a water sample, expressed as ppm of CaCO₃.
2. In the EDTA titration, what is the role of the indicator calmagite?
A. It binds to the EDTA to make it visible.
B. It forms a colored complex with the Ca²⁺ and Mg²⁺ ions before the titration.
C. It changes color when the solution becomes basic.
D. It buffers the solution to a specific pH.
Correct Answer: B
Rationale: Calmagite is a metal indicator that forms a wine-red complex with Ca²⁺ and Mg²⁺
ions. As EDTA is added, it preferentially binds to the metal ions, and at the endpoint, the
indicator is free and the solution turns blue.
3. A student forgot to add the ammonia-ammonium chloride buffer (pH = 10) to the water
sample before titration. What would be the expected outcome?
A. The endpoint would occur prematurely, and the calculated hardness would be too high.
B. The calculated hardness would be accurate because EDTA titrates Ca²⁺ and Mg²⁺ at any pH.
C. Mg²⁺ would precipitate as Mg(OH)₂ and would not be titrated, causing the calculated
hardness to be too low.
D. The indicator would not be able to bind to the metal ions, and no color change would occur.
, Correct Answer: C
Rationale: The buffer maintains a pH of 10, which is necessary to keep Mg²⁺ in solution. Without
it, Mg(OH)₂ precipitates and is not titrated, leading to a falsely low measurement of total water
hardness.
4. A 100.0 mL water sample required 18.35 mL of 0.01000 M EDTA to reach the endpoint.
Calculate the concentration of CaCO₃ in the sample in mg/L (ppm). (Molar mass CaCO₃ = 100.09
g/mol)
A. 36.7 ppm
B. 73.4 ppm
C. 183.5 ppm
D. 367.0 ppm
Correct Answer: C
Rationale: Moles EDTA = 0.01835 L × 0.01000 mol/L = 1.835 × 10⁻⁴ mol. Since 1 mol EDTA reacts
with 1 mol CaCO₃, moles CaCO₃ = 1.835 × 10⁻⁴ mol. Mass CaCO₃ = (1.835 × 10⁻⁴ mol)(100.09
g/mol) = 0.01836 g = 18.36 mg. Concentration = (18.36 mg)/(0.1000 L) = 183.6 ppm.
5. If the water sample had been "hard" water, which of the following would you expect to
observe during the titration?
A. The sample would require more EDTA to reach the endpoint.
B. The sample would require less EDTA to reach the endpoint.
C. The initial color of the solution would be blue instead of wine-red.
D. The titration would proceed much faster.
Correct Answer: A
