Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution. O 0.130 M O 1.18 M 1.50 M 0.768 M 2.30 M
Determine the molarity of a solution formed by dissolving 97.7 g LiBr in enough water to yield 750.0 mL of solution. O 0.130 M O 1.18 M 1.50 M 0.768 M 2.30 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...
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Could i have help with the following questions
![**Question:**
How many milliliters of a stock solution of 12.1 M HNO₃ would be needed to prepare 0.500 L of 0.500 M HNO₃?
**Options:**
- ○ 0.0484
- ○ 0.0207
- ○ 20.7
- ○ 48.4
- ○ 3.03
**Answer:**
To solve this question, you need to use the dilution formula:
\[ M_1V_1 = M_2V_2 \]
Where:
- \( M_1 \) is the molarity of the stock solution (12.1 M).
- \( V_1 \) is the volume of the stock solution needed.
- \( M_2 \) is the molarity of the diluted solution (0.500 M).
- \( V_2 \) is the volume of the diluted solution (0.500 L).
Substitute the known values into the equation and solve for \( V_1 \):
\[ 12.1 \times V_1 = 0.500 \times 0.500 \]
\[ V_1 = \frac{0.500 \times 0.500}{12.1} \]
\[ V_1 = 0.02066 \, \text{L} \]
Convert the volume from liters to milliliters:
\[ V_1 = 20.7 \, \text{mL} \]
Therefore, the correct answer is:
- ○ 20.7](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F445e38f6-3462-4c37-9713-fdd3067cbeca%2Fc9dd34f8-3cd7-418a-ac85-16a9af22b9f4%2Fy1zzbvd_processed.png&w=3840&q=75)
Transcribed Image Text:**Question:**
How many milliliters of a stock solution of 12.1 M HNO₃ would be needed to prepare 0.500 L of 0.500 M HNO₃?
**Options:**
- ○ 0.0484
- ○ 0.0207
- ○ 20.7
- ○ 48.4
- ○ 3.03
**Answer:**
To solve this question, you need to use the dilution formula:
\[ M_1V_1 = M_2V_2 \]
Where:
- \( M_1 \) is the molarity of the stock solution (12.1 M).
- \( V_1 \) is the volume of the stock solution needed.
- \( M_2 \) is the molarity of the diluted solution (0.500 M).
- \( V_2 \) is the volume of the diluted solution (0.500 L).
Substitute the known values into the equation and solve for \( V_1 \):
\[ 12.1 \times V_1 = 0.500 \times 0.500 \]
\[ V_1 = \frac{0.500 \times 0.500}{12.1} \]
\[ V_1 = 0.02066 \, \text{L} \]
Convert the volume from liters to milliliters:
\[ V_1 = 20.7 \, \text{mL} \]
Therefore, the correct answer is:
- ○ 20.7
![**Determine the Molarity of a Solution**
Calculate the molarity of a solution formed by dissolving 97.7 g of lithium bromide (LiBr) in enough water to yield 750.0 mL of solution.
**Multiple Choice Options:**
- 0.130 M
- 1.18 M
- 1.50 M
- 0.768 M
- 2.30 M
To find the correct answer, first calculate the moles of LiBr using its molar mass, and then use 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%2F445e38f6-3462-4c37-9713-fdd3067cbeca%2Fc9dd34f8-3cd7-418a-ac85-16a9af22b9f4%2Fxpepjn4_processed.png&w=3840&q=75)
Transcribed Image Text:**Determine the Molarity of a Solution**
Calculate the molarity of a solution formed by dissolving 97.7 g of lithium bromide (LiBr) in enough water to yield 750.0 mL of solution.
**Multiple Choice Options:**
- 0.130 M
- 1.18 M
- 1.50 M
- 0.768 M
- 2.30 M
To find the correct answer, first calculate the moles of LiBr using its molar mass, and then use the formula:
\[ \text{Molarity (M)} = \frac{\text{moles of solute}}{\text{liters of solution}} \]
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