If 16.3 g of glycerol (C3H8O3) is dissolved in 1500.0 mL of solution, what is the molarity (M)? a. 1.06 M b. 0.0326 M c. 0.118 M d. 0.354 M e. 0.000354 M
If 16.3 g of glycerol (C3H8O3) is dissolved in 1500.0 mL of solution, what is the molarity (M)? a. 1.06 M b. 0.0326 M c. 0.118 M d. 0.354 M e. 0.000354 M
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
![**Sample Chemistry Problem: Calculating Molarity**
**Problem Statement:**
If 16.3 g of glycerol (C₃H₈O₃) is dissolved in 1500.0 mL of solution, what is the molarity (M)?
**Options:**
a. 1.06 M
b. 0.0326 M
c. 0.118 M
d. 0.354 M
e. 0.000354 M
**Explanation:**
To solve this problem, follow these steps:
1. **Calculate the number of moles of glycerol:**
- First, determine the molar mass of glycerol (C₃H₈O₃):
\[
\text{Molar mass} = 3(\text{Atomic mass of Carbon}) + 8(\text{Atomic mass of Hydrogen}) + 3(\text{Atomic mass of Oxygen})
\]
\[
\text{Molar mass} = 3(12.01) + 8(1.01) + 3(16.00)
\]
\[
\text{Molar mass} = 36.03 + 8.08 + 48.00
\]
\[
\text{Molar mass} = 92.11 \, \text{g/mol}
\]
- Calculate the moles of glycerol using the formula:
\[
\text{Moles} = \frac{\text{Mass}}{\text{Molar mass}}
\]
\[
\text{Moles} = \frac{16.3 \, \text{g}}{92.11 \, \text{g/mol}}
\]
\[
\text{Moles} \approx 0.177 \, \text{mol}
\]
2. **Convert the volume of solution from mL to L:**
\[
1500.0 \, \text{mL} = 1.500 \, \text{L}
\]
3. **Calculate the molarity (M) using the formula:**
\[
\text{Molarity (M)} = \frac{\text{Moles of solute}}{\text{Liters of solution}}
\]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F066bb5df-9069-4300-b122-0f92c568ce58%2F754b8ad3-8e10-4036-a7f0-9bf88e32c288%2Ft2bvbe_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Sample Chemistry Problem: Calculating Molarity**
**Problem Statement:**
If 16.3 g of glycerol (C₃H₈O₃) is dissolved in 1500.0 mL of solution, what is the molarity (M)?
**Options:**
a. 1.06 M
b. 0.0326 M
c. 0.118 M
d. 0.354 M
e. 0.000354 M
**Explanation:**
To solve this problem, follow these steps:
1. **Calculate the number of moles of glycerol:**
- First, determine the molar mass of glycerol (C₃H₈O₃):
\[
\text{Molar mass} = 3(\text{Atomic mass of Carbon}) + 8(\text{Atomic mass of Hydrogen}) + 3(\text{Atomic mass of Oxygen})
\]
\[
\text{Molar mass} = 3(12.01) + 8(1.01) + 3(16.00)
\]
\[
\text{Molar mass} = 36.03 + 8.08 + 48.00
\]
\[
\text{Molar mass} = 92.11 \, \text{g/mol}
\]
- Calculate the moles of glycerol using the formula:
\[
\text{Moles} = \frac{\text{Mass}}{\text{Molar mass}}
\]
\[
\text{Moles} = \frac{16.3 \, \text{g}}{92.11 \, \text{g/mol}}
\]
\[
\text{Moles} \approx 0.177 \, \text{mol}
\]
2. **Convert the volume of solution from mL to L:**
\[
1500.0 \, \text{mL} = 1.500 \, \text{L}
\]
3. **Calculate the molarity (M) using the formula:**
\[
\text{Molarity (M)} = \frac{\text{Moles of solute}}{\text{Liters of solution}}
\]
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 4 steps with 8 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.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