0.456 L of a 2.2 M KCl solution Express your answer using two significant figures. • View Available Hint(s) ΑΣφ n = mol Submit Part B 1.4 L of a 0.75 M KCl solution Express your answer using two significant figures. Viow Availablo Hinticl
0.456 L of a 2.2 M KCl solution Express your answer using two significant figures. • View Available Hint(s) ΑΣφ n = mol Submit Part B 1.4 L of a 0.75 M KCl solution Express your answer using two significant figures. Viow Availablo Hinticl
Chapter80: Crystallization: Purification Of Solids
Section: Chapter Questions
Problem 1P
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![**How many moles of KCl are contained in each of the following?**
**Part A**
*0.456 L of a 2.2 M KCl solution*
- **Express your answer using two significant figures.**
- **View Available Hint(s)**
![Input Field]
n = [ ] **mol**
- **Submit Button**
---
**Part B**
*1.4 L of a 0.75 M KCl solution*
- **Express your answer using two significant figures.**
- **View Available Hint(s)**
![Input Field]
n = [ ] **mol**
---
### Explanation of the Problem:
In this exercise, you are asked to calculate the number of moles of potassium chloride (KCl) in given volumes of KCl solutions.
1. For Part A, you need to find out how many moles are in 0.456 liters of a 2.2 M (molar) KCl solution.
2. For Part B, the task is to determine the number of moles in 1.4 liters of a 0.75 M KCl solution.
### Hints:
- Remember that molarity (M) is defined as moles of solute per liter of solution.
- To find the number of moles (n), you can use the equation:
\[ \text{n} = \text{M} \times \text{V} \]
Where:
- \( \text{M} \) is the molarity (moles per liter)
- \( \text{V} \) is the volume of the solution in liters
- Ensure to report your answer to two significant figures as requested. This means you might need to round your calculation results appropriately.
*[This material can be found in Section 5.2 of your textbook, pages 168 to 173. Additional resources include watching the video clips KCV 5.2 and IWE 5.2.]*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbc7df924-6a52-4175-b6ea-9e20e03510e5%2F74c2e9cd-ba98-412f-95b7-b62fe70a2a54%2Fcnpsw8_processed.png&w=3840&q=75)
Transcribed Image Text:**How many moles of KCl are contained in each of the following?**
**Part A**
*0.456 L of a 2.2 M KCl solution*
- **Express your answer using two significant figures.**
- **View Available Hint(s)**
![Input Field]
n = [ ] **mol**
- **Submit Button**
---
**Part B**
*1.4 L of a 0.75 M KCl solution*
- **Express your answer using two significant figures.**
- **View Available Hint(s)**
![Input Field]
n = [ ] **mol**
---
### Explanation of the Problem:
In this exercise, you are asked to calculate the number of moles of potassium chloride (KCl) in given volumes of KCl solutions.
1. For Part A, you need to find out how many moles are in 0.456 liters of a 2.2 M (molar) KCl solution.
2. For Part B, the task is to determine the number of moles in 1.4 liters of a 0.75 M KCl solution.
### Hints:
- Remember that molarity (M) is defined as moles of solute per liter of solution.
- To find the number of moles (n), you can use the equation:
\[ \text{n} = \text{M} \times \text{V} \]
Where:
- \( \text{M} \) is the molarity (moles per liter)
- \( \text{V} \) is the volume of the solution in liters
- Ensure to report your answer to two significant figures as requested. This means you might need to round your calculation results appropriately.
*[This material can be found in Section 5.2 of your textbook, pages 168 to 173. Additional resources include watching the video clips KCV 5.2 and IWE 5.2.]*
![### Part C
#### Problem Statement:
Given: **134 mL of a 1.95 M KCl solution**
**Task**: Express your answer using three significant figures.
#### Instructions:
1. Convert the given volume of KCl solution from milliliters (mL) to liters (L) if needed.
2. Use the molarity equation to find the number of moles (n) of KCl.
3. Input your answer in the provided field.
#### Detailed Steps:
1. **Volume Conversion** (if necessary):
Convert 134 mL to liters by dividing by 1000.
\[
134 \, \text{mL} = 0.134 \, \text{L}
\]
2. **Using the Molarity Formula**:
Molarity (M) is defined as the number of moles of solute (n) divided by the volume of solution in liters (V).
\[
M = \frac{n}{V} \implies n = M \times V
\]
3. **Substitute the Given Values**:
Substitute \(M = 1.95 \, M\) and \(V = 0.134 \, L\) into the equation:
\[
n = 1.95 \, M \times 0.134 \, L
\]
4. **Calculate the Number of Moles**:
\[
n = 1.95 \times 0.134 = 0.2613 \, \text{mol}
\]
5. **Express the Answer with Three Significant Figures**:
\[
n = 0.261 \, \text{mol}
\]
#### Answer Input:
Please enter your answer in the box provided in moles (mol).
### Example Answer:
```
n = 0.261 mol
```
Click **Submit** to check your answer.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fbc7df924-6a52-4175-b6ea-9e20e03510e5%2F74c2e9cd-ba98-412f-95b7-b62fe70a2a54%2F30f2xpo_processed.png&w=3840&q=75)
Transcribed Image Text:### Part C
#### Problem Statement:
Given: **134 mL of a 1.95 M KCl solution**
**Task**: Express your answer using three significant figures.
#### Instructions:
1. Convert the given volume of KCl solution from milliliters (mL) to liters (L) if needed.
2. Use the molarity equation to find the number of moles (n) of KCl.
3. Input your answer in the provided field.
#### Detailed Steps:
1. **Volume Conversion** (if necessary):
Convert 134 mL to liters by dividing by 1000.
\[
134 \, \text{mL} = 0.134 \, \text{L}
\]
2. **Using the Molarity Formula**:
Molarity (M) is defined as the number of moles of solute (n) divided by the volume of solution in liters (V).
\[
M = \frac{n}{V} \implies n = M \times V
\]
3. **Substitute the Given Values**:
Substitute \(M = 1.95 \, M\) and \(V = 0.134 \, L\) into the equation:
\[
n = 1.95 \, M \times 0.134 \, L
\]
4. **Calculate the Number of Moles**:
\[
n = 1.95 \times 0.134 = 0.2613 \, \text{mol}
\]
5. **Express the Answer with Three Significant Figures**:
\[
n = 0.261 \, \text{mol}
\]
#### Answer Input:
Please enter your answer in the box provided in moles (mol).
### Example Answer:
```
n = 0.261 mol
```
Click **Submit** to check your answer.
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