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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![**Title: Calculating Molarity of Ethanol Solution**
**Problem Statement:**
An aqueous solution contains 6.00% by mass ethanol, \( CH_3CH_2OH \), and has a density of 0.988 g/mL. The task is to determine the molarity of ethanol in the solution.
**Steps to Solve:**
1. **Identify the percentage by mass**: The solution is 6.00% ethanol by mass. This means 6.00 grams of ethanol are present in 100 grams of solution.
2. **Determine the density**: The solution has a density of 0.988 g/mL. Using this, convert the total mass of the solution to volume.
3. **Convert mass to volume**:
\[ \text{Volume of solution} = \frac{\text{Mass of solution}}{\text{Density of solution}} = \frac{100\, \text{g}}{0.988\, \text{g/mL}} \]
4. **Calculate the moles of ethanol**:
The molar mass of ethanol (\( CH_3CH_2OH \)) is 46.07 g/mol.
\[ \text{Moles of ethanol} = \frac{\text{Mass of ethanol}}{\text{Molar mass of ethanol}} = \frac{6\, \text{g}}{46.07\, \text{g/mol}} \]
5. **Calculate molarity**:
\[ \text{Molarity} = \frac{\text{Moles of ethanol}}{\text{Volume of solution in liters}} \]
6. **Submit your calculated answer** in the provided input box and click on "Submit Answer".
**Buttons/Options:**
- **Submit Answer**: Click this button after entering your calculated molarity to see if it's correct.
- **Try Another Version**: If your answer is not correct, you can click this button to attempt another version of the problem.
You have 7 attempts remaining to solve this problem.
Use the [References] link to access important values if needed for the question.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F60358686-21d1-41ff-a93a-9ba59c7b6516%2F353ed768-ec08-4084-b877-2a5f214a0b3e%2Fs0hq2fi_reoriented.jpeg&w=3840&q=75)
Transcribed Image Text:**Title: Calculating Molarity of Ethanol Solution**
**Problem Statement:**
An aqueous solution contains 6.00% by mass ethanol, \( CH_3CH_2OH \), and has a density of 0.988 g/mL. The task is to determine the molarity of ethanol in the solution.
**Steps to Solve:**
1. **Identify the percentage by mass**: The solution is 6.00% ethanol by mass. This means 6.00 grams of ethanol are present in 100 grams of solution.
2. **Determine the density**: The solution has a density of 0.988 g/mL. Using this, convert the total mass of the solution to volume.
3. **Convert mass to volume**:
\[ \text{Volume of solution} = \frac{\text{Mass of solution}}{\text{Density of solution}} = \frac{100\, \text{g}}{0.988\, \text{g/mL}} \]
4. **Calculate the moles of ethanol**:
The molar mass of ethanol (\( CH_3CH_2OH \)) is 46.07 g/mol.
\[ \text{Moles of ethanol} = \frac{\text{Mass of ethanol}}{\text{Molar mass of ethanol}} = \frac{6\, \text{g}}{46.07\, \text{g/mol}} \]
5. **Calculate molarity**:
\[ \text{Molarity} = \frac{\text{Moles of ethanol}}{\text{Volume of solution in liters}} \]
6. **Submit your calculated answer** in the provided input box and click on "Submit Answer".
**Buttons/Options:**
- **Submit Answer**: Click this button after entering your calculated molarity to see if it's correct.
- **Try Another Version**: If your answer is not correct, you can click this button to attempt another version of the problem.
You have 7 attempts remaining to solve this problem.
Use the [References] link to access important values if needed for the question.
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