A herbicide contains 2,4-D (2,4-dichlorophenoxyacetic acid), C8 H6 Cl2 O3. A 1.265-g sample of the herbicide was decomposed to liberate the chlorine as CI ion. This was precipitated as AgCl, with a mass of 0.1410 g. What is the mass percent of 2,4-D in the sample? OCH₂CO₂H H. Mass percent H C C C CL 2,4-D (2,4-dichlorophenoxyacetic acid). H %
A herbicide contains 2,4-D (2,4-dichlorophenoxyacetic acid), C8 H6 Cl2 O3. A 1.265-g sample of the herbicide was decomposed to liberate the chlorine as CI ion. This was precipitated as AgCl, with a mass of 0.1410 g. What is the mass percent of 2,4-D in the sample? OCH₂CO₂H H. Mass percent H C C C CL 2,4-D (2,4-dichlorophenoxyacetic acid). H %
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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![**Determining the Mass Percent of 2,4-D in a Herbicide Sample**
**Problem Statement:**
A herbicide contains 2,4-D (2,4-dichlorophenoxyacetic acid), \(C_8H_6Cl_2O_3\). A 1.265-g sample of the herbicide was decomposed to liberate the chlorine as \(Cl^-\) ion. This was precipitated as \(AgCl\), with a mass of 0.1410 g. What is the mass percent of 2,4-D in the sample?
**Chemical Structure:**
[Graphic of chemical structure for 2,4-D]
- The structure shows a benzene ring with the following groups attached: two chlorine atoms (at positions 2 and 4), a methylene bridge, and an acetic acid functional group.
**Calculation Steps:**
1. **Determine the amount of \(Cl^-\) from \(AgCl\):**
- Molar mass of \(AgCl\):
* Ag = 107.87 g/mol
* Cl = 35.45 g/mol
* \(107.87 + 35.45 = 143.32 \) g/mol
- Moles of \(AgCl\):
\[
\text{Moles of } AgCl = \frac{0.1410 \text{ g}}{143.32 \text{ g/mol}} = 9.84 \times 10^{-4} \text{ mol}
\]
2. **Convert moles of \(AgCl\) to moles of \(Cl^-\):**
- Each mole of \(AgCl\) contains 1 mole of \(Cl^-\), so:
\[
\text{Moles of } Cl^- = 9.84 \times 10^{-4} \text{ mol}
\]
3. **Mass of \(Cl^-\):**
- Molar mass of Cl = 35.45 g/mol
\[
\text{Mass of } Cl^- = 9.84 \times 10^{-4} \text{ mol} \times 35.45 \text{ g/mol} = 0.03488 \text{ g}
\]
4. **](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F883e3e80-624e-4e0d-88a1-3570ac65b326%2F222ce0a8-55f8-4b50-991e-63cb1ce07333%2F17qdlm_processed.png&w=3840&q=75)
Transcribed Image Text:**Determining the Mass Percent of 2,4-D in a Herbicide Sample**
**Problem Statement:**
A herbicide contains 2,4-D (2,4-dichlorophenoxyacetic acid), \(C_8H_6Cl_2O_3\). A 1.265-g sample of the herbicide was decomposed to liberate the chlorine as \(Cl^-\) ion. This was precipitated as \(AgCl\), with a mass of 0.1410 g. What is the mass percent of 2,4-D in the sample?
**Chemical Structure:**
[Graphic of chemical structure for 2,4-D]
- The structure shows a benzene ring with the following groups attached: two chlorine atoms (at positions 2 and 4), a methylene bridge, and an acetic acid functional group.
**Calculation Steps:**
1. **Determine the amount of \(Cl^-\) from \(AgCl\):**
- Molar mass of \(AgCl\):
* Ag = 107.87 g/mol
* Cl = 35.45 g/mol
* \(107.87 + 35.45 = 143.32 \) g/mol
- Moles of \(AgCl\):
\[
\text{Moles of } AgCl = \frac{0.1410 \text{ g}}{143.32 \text{ g/mol}} = 9.84 \times 10^{-4} \text{ mol}
\]
2. **Convert moles of \(AgCl\) to moles of \(Cl^-\):**
- Each mole of \(AgCl\) contains 1 mole of \(Cl^-\), so:
\[
\text{Moles of } Cl^- = 9.84 \times 10^{-4} \text{ mol}
\]
3. **Mass of \(Cl^-\):**
- Molar mass of Cl = 35.45 g/mol
\[
\text{Mass of } Cl^- = 9.84 \times 10^{-4} \text{ mol} \times 35.45 \text{ g/mol} = 0.03488 \text{ g}
\]
4. **
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