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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![**Educational Chemistry Exercise: Calculating Mass of a Solute in Solution Preparation**
**Exercise Question:**
(5.2, Similar to For More Practice 5.1) What mass of NaOH (in grams) do you need to make 250.0 mL of a 1.50 M NaOH solution?
**Answer Options:**
- ( ) 6.67 g
- ( ) 22.3 g
- ( ) 44.6 g
- ( ) 15.0 g
**Explanation:**
The task involves calculating the mass of sodium hydroxide (NaOH) required to prepare a specific volume (250.0 mL) of a given molarity (1.50 M) solution. This exercise aims to test understanding of molarity and the necessary calculations to prepare a solution with a desired concentration.
**Note to Students:**
To solve this problem, you will need to use the following formula:
\[ \text{Mass (g)} = \text{Molarity (M)} \times \text{Volume (L)} \times \text{Molar Mass (g/mol)} \]
Where:
- **Molarity (M)** is the concentration of the solution (1.50 M).
- **Volume (L)** is the volume of the solution in liters (250.0 mL = 0.250 L).
- **Molar Mass (g/mol)** is the molar mass of NaOH. (The molar mass of NaOH = 23.00 + 16.00 + 1.01 = 40.01 g/mol).
**Steps in Calculation:**
1. Convert the volume from milliliters to liters.
2. Multiply the molarity by the volume in liters to find the number of moles of NaOH needed.
3. Multiply the number of moles by the molar mass of NaOH to find the mass in grams.
By following these steps, you can determine the correct option for the mass of NaOH needed.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa6aa13af-b0b4-4b84-a222-8b6a152716db%2F20749cea-0adc-441f-b3da-3bfa0eee8b7e%2F7cmhs5_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Educational Chemistry Exercise: Calculating Mass of a Solute in Solution Preparation**
**Exercise Question:**
(5.2, Similar to For More Practice 5.1) What mass of NaOH (in grams) do you need to make 250.0 mL of a 1.50 M NaOH solution?
**Answer Options:**
- ( ) 6.67 g
- ( ) 22.3 g
- ( ) 44.6 g
- ( ) 15.0 g
**Explanation:**
The task involves calculating the mass of sodium hydroxide (NaOH) required to prepare a specific volume (250.0 mL) of a given molarity (1.50 M) solution. This exercise aims to test understanding of molarity and the necessary calculations to prepare a solution with a desired concentration.
**Note to Students:**
To solve this problem, you will need to use the following formula:
\[ \text{Mass (g)} = \text{Molarity (M)} \times \text{Volume (L)} \times \text{Molar Mass (g/mol)} \]
Where:
- **Molarity (M)** is the concentration of the solution (1.50 M).
- **Volume (L)** is the volume of the solution in liters (250.0 mL = 0.250 L).
- **Molar Mass (g/mol)** is the molar mass of NaOH. (The molar mass of NaOH = 23.00 + 16.00 + 1.01 = 40.01 g/mol).
**Steps in Calculation:**
1. Convert the volume from milliliters to liters.
2. Multiply the molarity by the volume in liters to find the number of moles of NaOH needed.
3. Multiply the number of moles by the molar mass of NaOH to find the mass in grams.
By following these steps, you can determine the correct option for the mass of NaOH needed.
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