Acetic acid dissolves in water as a weak acid. Calculate the mole fraction of acetic acid in the solution that contains 35.0 g HC2H3O2 and 250 mL of water. MM HC2H3O2 = 60.052 g/mol MM H2O = 18.016 g/mol d H₂O = 0.998 g/mL XHC₂H30₂ = [?]
Acetic acid dissolves in water as a weak acid. Calculate the mole fraction of acetic acid in the solution that contains 35.0 g HC2H3O2 and 250 mL of water. MM HC2H3O2 = 60.052 g/mol MM H2O = 18.016 g/mol d H₂O = 0.998 g/mL XHC₂H30₂ = [?]
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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![**Calculating the Mole Fraction of Acetic Acid in a Solution**
**Problem Statement:**
Acetic acid dissolves in water as a weak acid. Calculate the mole fraction of acetic acid in the solution that contains 35.0 g of \( HC_2H_3O_2 \) and 250 mL of water.
**Given Data:**
- Mass of Acetic Acid (\( HC_2H_3O_2 \)): 35.0 g
- Volume of Water (\( H_2O \)): 250 mL
- Molar Mass (MM) of \( HC_2H_3O_2 \): 60.052 g/mol
- Molar Mass (MM) of \( H_2O \): 18.016 g/mol
- Density (d) of \( H_2O \): 0.998 g/mL
**Solution:**
To find the mole fraction of acetic acid (\( X_{ HC_2H_3O_2 } \)), we need to follow these steps:
1. **Calculate the moles of acetic acid:**
\[
\text{Moles of } HC_2H_3O_2 = \frac{\text{Mass of } HC_2H_3O_2}{\text{Molar Mass of } HC_2H_3O_2} = \frac{35.0 \text{ g}}{60.052 \text{ g/mol}}
\]
2. **Calculate the mass of water:**
\[
\text{Mass of } H_2O = \text{Volume of } H_2O \times \text{Density of } H_2O = 250 \text{ mL} \times 0.998 \text{ g/mL}
\]
3. **Calculate the moles of water:**
\[
\text{Moles of } H_2O = \frac{\text{Mass of } H_2O}{\text{Molar Mass of } H_2O}
\]
4. **Calculate the mole fraction of acetic acid:**
\[
X_{ HC_2H_3O_2 } = \frac{\text{Moles of } HC_2H_3O_2}{\text{](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcc2e14b5-3b93-4ed2-ae4c-4c469da12cc7%2Feeaf41e2-36b7-4778-bd90-cc8870e06f0f%2F73792s7_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Calculating the Mole Fraction of Acetic Acid in a Solution**
**Problem Statement:**
Acetic acid dissolves in water as a weak acid. Calculate the mole fraction of acetic acid in the solution that contains 35.0 g of \( HC_2H_3O_2 \) and 250 mL of water.
**Given Data:**
- Mass of Acetic Acid (\( HC_2H_3O_2 \)): 35.0 g
- Volume of Water (\( H_2O \)): 250 mL
- Molar Mass (MM) of \( HC_2H_3O_2 \): 60.052 g/mol
- Molar Mass (MM) of \( H_2O \): 18.016 g/mol
- Density (d) of \( H_2O \): 0.998 g/mL
**Solution:**
To find the mole fraction of acetic acid (\( X_{ HC_2H_3O_2 } \)), we need to follow these steps:
1. **Calculate the moles of acetic acid:**
\[
\text{Moles of } HC_2H_3O_2 = \frac{\text{Mass of } HC_2H_3O_2}{\text{Molar Mass of } HC_2H_3O_2} = \frac{35.0 \text{ g}}{60.052 \text{ g/mol}}
\]
2. **Calculate the mass of water:**
\[
\text{Mass of } H_2O = \text{Volume of } H_2O \times \text{Density of } H_2O = 250 \text{ mL} \times 0.998 \text{ g/mL}
\]
3. **Calculate the moles of water:**
\[
\text{Moles of } H_2O = \frac{\text{Mass of } H_2O}{\text{Molar Mass of } H_2O}
\]
4. **Calculate the mole fraction of acetic acid:**
\[
X_{ HC_2H_3O_2 } = \frac{\text{Moles of } HC_2H_3O_2}{\text{
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