Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Sample Problem: Determining Mass Percentage of Chlorine in a Compound
#### Problem Statement:
A **0.4455 g** sample of a pure soluble **chloride** compound is dissolved in water, and all of the **chloride ion** is precipitated as **AgCl** by the addition of an excess of silver nitrate. The mass of the resulting **AgCl** is found to be **0.9496 g**.
What is the mass percentage of **chlorine** in the original compound? \[\ \%\]
#### Solution:
To find the mass percentage of chlorine in the original compound, follow these steps:
1. **Calculate moles of AgCl**:
\[ \text{Molecular weight of AgCl} = \text{atomic weight of Ag} + \text{atomic weight of Cl} \]
\[ = 107.87 \text{ g/mol} + 35.45 \text{ g/mol} = 143.32 \text{ g/mol} \]
2. **Determine moles of AgCl from mass given**:
\[ \text{Moles of AgCl} = \frac{\text{mass of AgCl}}{\text{molecular weight of AgCl}} \]
\[ = \frac{0.9496 \text{ g}}{143.32 \text{ g/mol}} \]
\[ = 0.006625 \text{ mol} \]
3. **Determine moles of Cl**:
Since AgCl is composed of a 1:1 ratio of Ag to Cl, moles of Cl = moles of AgCl.
\[ \text{Moles of Cl} = 0.006625 \text{ mol} \]
4. **Calculate mass of Cl**:
\[ \text{Mass of Cl} = \text{moles of Cl} \times \text{atomic weight of Cl} \]
\[ = 0.006625 \text{ mol} \times 35.45 \text{ g/mol} \]
\[ = 0.2347 \text{ g} \]
5. **Calculate mass percentage of Cl** in the original sample:
\[ \text{Mass percentage of Cl} = \left( \frac{\text{mass of Cl}}{\text{mass of original compound}} \right)](https://content.bartleby.com/qna-images/question/7a354f1c-cdfd-41e5-a863-9a86a504af1c/fdd72e07-f8e8-4594-b521-808c9af2ac83/yk5cktf_processed.png)
Transcribed Image Text:### Sample Problem: Determining Mass Percentage of Chlorine in a Compound
#### Problem Statement:
A **0.4455 g** sample of a pure soluble **chloride** compound is dissolved in water, and all of the **chloride ion** is precipitated as **AgCl** by the addition of an excess of silver nitrate. The mass of the resulting **AgCl** is found to be **0.9496 g**.
What is the mass percentage of **chlorine** in the original compound? \[\ \%\]
#### Solution:
To find the mass percentage of chlorine in the original compound, follow these steps:
1. **Calculate moles of AgCl**:
\[ \text{Molecular weight of AgCl} = \text{atomic weight of Ag} + \text{atomic weight of Cl} \]
\[ = 107.87 \text{ g/mol} + 35.45 \text{ g/mol} = 143.32 \text{ g/mol} \]
2. **Determine moles of AgCl from mass given**:
\[ \text{Moles of AgCl} = \frac{\text{mass of AgCl}}{\text{molecular weight of AgCl}} \]
\[ = \frac{0.9496 \text{ g}}{143.32 \text{ g/mol}} \]
\[ = 0.006625 \text{ mol} \]
3. **Determine moles of Cl**:
Since AgCl is composed of a 1:1 ratio of Ag to Cl, moles of Cl = moles of AgCl.
\[ \text{Moles of Cl} = 0.006625 \text{ mol} \]
4. **Calculate mass of Cl**:
\[ \text{Mass of Cl} = \text{moles of Cl} \times \text{atomic weight of Cl} \]
\[ = 0.006625 \text{ mol} \times 35.45 \text{ g/mol} \]
\[ = 0.2347 \text{ g} \]
5. **Calculate mass percentage of Cl** in the original sample:
\[ \text{Mass percentage of Cl} = \left( \frac{\text{mass of Cl}}{\text{mass of original compound}} \right)
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