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...
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![**Question 1: Determining the Molarity of a KBr Solution**
What is the molarity of KBr if 0.491 moles of KBr is dissolved in water to make a 1525 mL solution?
**Explanation:**
To calculate the molarity (M) of the solution, use the formula:
\[
\text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}}
\]
1. Convert the volume from milliliters to liters:
\[
1525 \, \text{mL} = 1.525 \, \text{L}
\]
2. Use the formula to calculate molarity:
\[
\text{Molarity (M)} = \frac{0.491 \, \text{moles}}{1.525 \, \text{L}}
\]
3. Compute the result:
\[
\text{Molarity (M)} \approx 0.322 \, \text{M}
\]
Thus, the molarity of the KBr solution is approximately 0.322 M.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9ade340b-6e5d-40f3-a11c-7a7fae38a958%2F4d4a5dbc-86b1-459f-97bd-f2870de3e520%2Flo0dz3o_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Question 1: Determining the Molarity of a KBr Solution**
What is the molarity of KBr if 0.491 moles of KBr is dissolved in water to make a 1525 mL solution?
**Explanation:**
To calculate the molarity (M) of the solution, use the formula:
\[
\text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}}
\]
1. Convert the volume from milliliters to liters:
\[
1525 \, \text{mL} = 1.525 \, \text{L}
\]
2. Use the formula to calculate molarity:
\[
\text{Molarity (M)} = \frac{0.491 \, \text{moles}}{1.525 \, \text{L}}
\]
3. Compute the result:
\[
\text{Molarity (M)} \approx 0.322 \, \text{M}
\]
Thus, the molarity of the KBr solution is approximately 0.322 M.
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