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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![**Image Description:**
The image shows a part of a keyboard and a piece of lined notebook paper. The keyboard appears to be part of a laptop, featuring keys such as Esc, F1, F2, F3, F4, @, W, Q, Z, Caps Lock, Shift, Ctrl, and others. The notebook paper partially covers the right side of the keyboard and contains handwritten text.
**Handwritten Text on Notebook Paper:**
*What mass of NaOH is in 206 mL of a 9.37 M NaOH solution*
---
**Explanation (for the Educational Website):**
In this image, we see a typical laptop keyboard alongside a piece of notebook paper with a handwritten chemistry problem. The problem is related to determining the mass of sodium hydroxide (NaOH) in a given volume of a solution with a specific molarity.
**The Problem:**
*What mass of NaOH is in 206 mL of a 9.37 M NaOH solution*?
**Solution Explanation:**
To solve this problem, follow these steps:
1. **Understanding Molarity:**
- Molarity (M) is defined as the number of moles of a solute per liter of solution.
- Here, the solution has a molarity of 9.37 M, meaning there are 9.37 moles of NaOH in 1 liter of solution.
2. **Convert Volume to Liters:**
- The given volume of NaOH solution is 206 mL.
- Convert mL to liters by dividing by 1000.
\[
\text{Volume in liters} = \frac{206 \, \text{mL}}{1000} = 0.206 \, \text{L}
\]
3. **Calculate the Number of Moles:**
- Use the molarity to find the number of moles in the given volume.
\[
\text{Moles of NaOH} = \text{Molarity} \times \text{Volume in liters}
\]
\[
\text{Moles of NaOH} = 9.37 \, \text{M} \times 0.206 \, \text{L} = 1.92922 \, \text{moles}
\]
4. **Convert Moles to Grams:**](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F89ff4db6-6e9d-47ab-aded-f72671492205%2Fe70902c3-10c1-45f1-99ac-2d5a8213e959%2F4hmz9f6_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Image Description:**
The image shows a part of a keyboard and a piece of lined notebook paper. The keyboard appears to be part of a laptop, featuring keys such as Esc, F1, F2, F3, F4, @, W, Q, Z, Caps Lock, Shift, Ctrl, and others. The notebook paper partially covers the right side of the keyboard and contains handwritten text.
**Handwritten Text on Notebook Paper:**
*What mass of NaOH is in 206 mL of a 9.37 M NaOH solution*
---
**Explanation (for the Educational Website):**
In this image, we see a typical laptop keyboard alongside a piece of notebook paper with a handwritten chemistry problem. The problem is related to determining the mass of sodium hydroxide (NaOH) in a given volume of a solution with a specific molarity.
**The Problem:**
*What mass of NaOH is in 206 mL of a 9.37 M NaOH solution*?
**Solution Explanation:**
To solve this problem, follow these steps:
1. **Understanding Molarity:**
- Molarity (M) is defined as the number of moles of a solute per liter of solution.
- Here, the solution has a molarity of 9.37 M, meaning there are 9.37 moles of NaOH in 1 liter of solution.
2. **Convert Volume to Liters:**
- The given volume of NaOH solution is 206 mL.
- Convert mL to liters by dividing by 1000.
\[
\text{Volume in liters} = \frac{206 \, \text{mL}}{1000} = 0.206 \, \text{L}
\]
3. **Calculate the Number of Moles:**
- Use the molarity to find the number of moles in the given volume.
\[
\text{Moles of NaOH} = \text{Molarity} \times \text{Volume in liters}
\]
\[
\text{Moles of NaOH} = 9.37 \, \text{M} \times 0.206 \, \text{L} = 1.92922 \, \text{moles}
\]
4. **Convert Moles to Grams:**
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