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
![**Chemistry Problem: Calculation of Mass Percent**
**Problem:**
What is the mass percent of 1.39 M NaCl solution? The density of this solution is 1.05 g/mL.
---
To solve this problem, students will need to follow the concept of mass percent calculation. The guiding equation involves determining the mass of the solute (NaCl) and the mass of the solution and then expressing this ratio as a percentage.
Mass percent (%) = (mass of solute / mass of solution) x 100
1. **Step 1: Determine the mass of the solute (NaCl).**
- A 1 M solution contains 1 mole of solute per liter of solution. Therefore, a 1.39 M NaCl solution contains 1.39 moles of NaCl per liter.
- Molar mass of NaCl = 58.44 g/mol (Sodium (Na) = 22.99 g/mol, Chlorine (Cl) = 35.45 g/mol).
- Mass of NaCl in 1 liter = 1.39 moles * 58.44 g/mol = 81.2276 g.
2. **Step 2: Determine the mass of the solution.**
- Density (d) = mass/volume. The density of the NaCl solution is given as 1.05 g/mL.
- For 1 liter of solution (which is 1000 mL), the mass of the solution = 1.05 g/mL * 1000 mL = 1050 g.
3. **Step 3: Calculate the mass percent.**
- Mass percent of NaCl = (mass of NaCl / mass of solution) * 100
- Mass percent = (81.2276 g / 1050 g) * 100 ≈ 7.73%
Therefore, the mass percent of the 1.39 M NaCl solution is approximately 7.73%.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F19b0aed3-745e-4879-8577-ea35399669d0%2F9a4ec1b3-b78c-43aa-9ba2-baf42efd6a1f%2Ft81groq_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemistry Problem: Calculation of Mass Percent**
**Problem:**
What is the mass percent of 1.39 M NaCl solution? The density of this solution is 1.05 g/mL.
---
To solve this problem, students will need to follow the concept of mass percent calculation. The guiding equation involves determining the mass of the solute (NaCl) and the mass of the solution and then expressing this ratio as a percentage.
Mass percent (%) = (mass of solute / mass of solution) x 100
1. **Step 1: Determine the mass of the solute (NaCl).**
- A 1 M solution contains 1 mole of solute per liter of solution. Therefore, a 1.39 M NaCl solution contains 1.39 moles of NaCl per liter.
- Molar mass of NaCl = 58.44 g/mol (Sodium (Na) = 22.99 g/mol, Chlorine (Cl) = 35.45 g/mol).
- Mass of NaCl in 1 liter = 1.39 moles * 58.44 g/mol = 81.2276 g.
2. **Step 2: Determine the mass of the solution.**
- Density (d) = mass/volume. The density of the NaCl solution is given as 1.05 g/mL.
- For 1 liter of solution (which is 1000 mL), the mass of the solution = 1.05 g/mL * 1000 mL = 1050 g.
3. **Step 3: Calculate the mass percent.**
- Mass percent of NaCl = (mass of NaCl / mass of solution) * 100
- Mass percent = (81.2276 g / 1050 g) * 100 ≈ 7.73%
Therefore, the mass percent of the 1.39 M NaCl solution is approximately 7.73%.
Expert Solution
![](/static/compass_v2/shared-icons/check-mark.png)
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 2 steps with 2 images
![Blurred answer](/static/compass_v2/solution-images/blurred-answer.jpg)
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](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781305957404/9781305957404_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
![Chemistry](https://www.bartleby.com/isbn_cover_images/9781259911156/9781259911156_smallCoverImage.gif)
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
![Principles of Instrumental Analysis](https://www.bartleby.com/isbn_cover_images/9781305577213/9781305577213_smallCoverImage.gif)
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
![Organic Chemistry](https://www.bartleby.com/isbn_cover_images/9780078021558/9780078021558_smallCoverImage.gif)
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
![Chemistry: Principles and Reactions](https://www.bartleby.com/isbn_cover_images/9781305079373/9781305079373_smallCoverImage.gif)
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
![Elementary Principles of Chemical Processes, Bind…](https://www.bartleby.com/isbn_cover_images/9781118431221/9781118431221_smallCoverImage.gif)
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY