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...
Related questions
Question
![**Question:**
What is the mass of the solute in 250 mL of 0.201 M lead (II) sulfate?
**Options:**
- 377 g
- 10.4 g
- 50.3 g
- 15.2 g
- 61.0 g
**Explanation:**
To find the mass of the solute, you need to use the formula:
\[
\text{Mass of solute} = \text{Molarity (M)} \times \text{Volume (L)} \times \text{Molar Mass (g/mol)}
\]
1. **Convert volume to liters:**
- 250 mL = 0.250 L
2. **Molarity (M) is given:**
- 0.201 M
3. **Find the molar mass of lead (II) sulfate (PbSO\(_4\)):**
- Lead (Pb) = 207.2 g/mol
- Sulfur (S) = 32.07 g/mol
- Oxygen (O) = 16.00 g/mol (4 oxygen atoms contribute 64.00 g/mol)
- Total molar mass = 207.2 + 32.07 + 64.00 = 303.27 g/mol
4. **Calculate mass of solute:**
- \[ 0.201 \, \text{mol/L} \times 0.250 \, \text{L} \times 303.27 \, \text{g/mol} \]
5. **Result:**
- The mass of the solute can be calculated accordingly.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa3dab484-43c7-405a-8781-b23fe682a225%2F3067af43-d347-4922-a162-52a07a903d34%2F724fppf_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question:**
What is the mass of the solute in 250 mL of 0.201 M lead (II) sulfate?
**Options:**
- 377 g
- 10.4 g
- 50.3 g
- 15.2 g
- 61.0 g
**Explanation:**
To find the mass of the solute, you need to use the formula:
\[
\text{Mass of solute} = \text{Molarity (M)} \times \text{Volume (L)} \times \text{Molar Mass (g/mol)}
\]
1. **Convert volume to liters:**
- 250 mL = 0.250 L
2. **Molarity (M) is given:**
- 0.201 M
3. **Find the molar mass of lead (II) sulfate (PbSO\(_4\)):**
- Lead (Pb) = 207.2 g/mol
- Sulfur (S) = 32.07 g/mol
- Oxygen (O) = 16.00 g/mol (4 oxygen atoms contribute 64.00 g/mol)
- Total molar mass = 207.2 + 32.07 + 64.00 = 303.27 g/mol
4. **Calculate mass of solute:**
- \[ 0.201 \, \text{mol/L} \times 0.250 \, \text{L} \times 303.27 \, \text{g/mol} \]
5. **Result:**
- The mass of the solute can be calculated accordingly.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY