Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Educational Content: Key Equation in Titration Experiments**
**Question:**
What is the key equation used in titration experiments?
**Options:**
- \[ \circ \] \[ d = \frac{m}{V} \]
- \[ \circ \] At endpoint, mol acid = mol base
- \[ \circ \] \[ A = \epsilon bC \]
- \[ \circ \] \[ q_{rxn} = -q_{cal} \]
**Explanation:**
This question helps students to identify the fundamental concepts and equations used in titration experiments. Let's break down the options to understand which one is key for titration:
1. \[ d = \frac{m}{V} \]: This equation is used to determine density, where "d" stands for density, "m" is mass, and "V" is volume. This is not specific to titration.
2. **At endpoint, mol acid = mol base**: This is the core principle of titration. At the endpoint of a titration experiment, the number of moles of acid is equal to the number of moles of base. This signifies that the amount of titrant (a standard solution) added is stoichiometrically equivalent to the amount of substance being titrated.
3. \[ A = \epsilon bC \]: This is the Beer-Lambert Law, which relates absorbance (A) to the molar absorptivity (\[ \epsilon \]), path length (b), and concentration (C). This law is used in spectrophotometry, not titration.
4. \[ q_{rxn} = -q_{cal} \]: This is used in calorimetry, stating that the heat of the reaction (\[ q_{rxn} \]) is equal to the negative of the heat absorbed by the calorimeter (\[ q_{cal} \]). This is not relevant to titration.
Given these options, the correct answer is:
\[ \circ \] At endpoint, mol acid = mol base
This statement explains the point in a titration process where the reaction is complete, and it is crucial for calculating the unknown concentration of an analyte. Understanding this principle is fundamental for accurately conducting and interpreting titration experiments in chemistry.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7053a473-1d58-4c55-9472-40482d1da2f4%2F5c0c36ae-d902-4e75-a8de-d079a22e4b66%2Fr2whftq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Content: Key Equation in Titration Experiments**
**Question:**
What is the key equation used in titration experiments?
**Options:**
- \[ \circ \] \[ d = \frac{m}{V} \]
- \[ \circ \] At endpoint, mol acid = mol base
- \[ \circ \] \[ A = \epsilon bC \]
- \[ \circ \] \[ q_{rxn} = -q_{cal} \]
**Explanation:**
This question helps students to identify the fundamental concepts and equations used in titration experiments. Let's break down the options to understand which one is key for titration:
1. \[ d = \frac{m}{V} \]: This equation is used to determine density, where "d" stands for density, "m" is mass, and "V" is volume. This is not specific to titration.
2. **At endpoint, mol acid = mol base**: This is the core principle of titration. At the endpoint of a titration experiment, the number of moles of acid is equal to the number of moles of base. This signifies that the amount of titrant (a standard solution) added is stoichiometrically equivalent to the amount of substance being titrated.
3. \[ A = \epsilon bC \]: This is the Beer-Lambert Law, which relates absorbance (A) to the molar absorptivity (\[ \epsilon \]), path length (b), and concentration (C). This law is used in spectrophotometry, not titration.
4. \[ q_{rxn} = -q_{cal} \]: This is used in calorimetry, stating that the heat of the reaction (\[ q_{rxn} \]) is equal to the negative of the heat absorbed by the calorimeter (\[ q_{cal} \]). This is not relevant to titration.
Given these options, the correct answer is:
\[ \circ \] At endpoint, mol acid = mol base
This statement explains the point in a titration process where the reaction is complete, and it is crucial for calculating the unknown concentration of an analyte. Understanding this principle is fundamental for accurately conducting and interpreting titration experiments in chemistry.
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