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
![**Problem:**
How many grams of chlorine gas are needed to make \(5.60 \times 10^6\) g of a solution that is 1.40 ppm chlorine by mass?
**Solution:**
To solve this problem, use the formula for parts per million (ppm):
\[
\text{ppm} = \left( \frac{\text{mass of solute (g)}}{\text{mass of solution (g)}} \right) \times 10^6
\]
Given:
- ppm = 1.40
- mass of solution = \(5.60 \times 10^6\) g
**Steps:**
1. Rearrange the ppm formula to find the mass of solute (chlorine):
\[
\text{mass of solute} = \frac{\text{ppm} \times \text{mass of solution}}{10^6}
\]
2. Substitute the given values:
\[
\text{mass of solute} = \frac{1.40 \times 5.60 \times 10^6}{10^6}
\]
3. Calculate the mass of chlorine:
\[
\text{mass of solute} = \frac{7.84 \times 10^6}{10^6} = 7.84 \text{ g}
\]
**Answer:**
The mass of chlorine needed is 7.84 grams.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4ef56a00-edb3-41ae-a483-7337cfe3ed88%2Fa84bb76c-8639-47d8-8982-9f9ddd52cf59%2Fg79jsto_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Problem:**
How many grams of chlorine gas are needed to make \(5.60 \times 10^6\) g of a solution that is 1.40 ppm chlorine by mass?
**Solution:**
To solve this problem, use the formula for parts per million (ppm):
\[
\text{ppm} = \left( \frac{\text{mass of solute (g)}}{\text{mass of solution (g)}} \right) \times 10^6
\]
Given:
- ppm = 1.40
- mass of solution = \(5.60 \times 10^6\) g
**Steps:**
1. Rearrange the ppm formula to find the mass of solute (chlorine):
\[
\text{mass of solute} = \frac{\text{ppm} \times \text{mass of solution}}{10^6}
\]
2. Substitute the given values:
\[
\text{mass of solute} = \frac{1.40 \times 5.60 \times 10^6}{10^6}
\]
3. Calculate the mass of chlorine:
\[
\text{mass of solute} = \frac{7.84 \times 10^6}{10^6} = 7.84 \text{ g}
\]
**Answer:**
The mass of chlorine needed is 7.84 grams.
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