A solution is made by dissolving 23.4 g of potassium sulfate, K₂SO4, in enough water to make exactly 500. mL of solution. Calculate the molarity of each species: K₂SO4 mol/L K+ SO4²- mol/L mol/L
A solution is made by dissolving 23.4 g of potassium sulfate, K₂SO4, in enough water to make exactly 500. mL of solution. Calculate the molarity of each species: K₂SO4 mol/L K+ SO4²- mol/L mol/L
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
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![### Calculating Molarity of Ionic Species in a Potassium Sulfate Solution
**Problem Statement:**
A solution is made by dissolving 23.4 g of potassium sulfate, \( \text{K}_2\text{SO}_4 \), in enough water to make exactly 500 mL of solution. Calculate the molarity of each species.
#### Steps to Solve:
1. **Determine the Molar Mass of \( \text{K}_2\text{SO}_4 \):**
- Potassium (K): \( 2 \times 39.1 \text{ g/mol} = 78.2 \text{ g/mol} \)
- Sulfur (S): \( 1 \times 32.1 \text{ g/mol} = 32.1 \text{ g/mol} \)
- Oxygen (O): \( 4 \times 16.0 \text{ g/mol} = 64.0 \text{ g/mol} \)
- **Total molar mass:** \( 78.2 + 32.1 + 64.0 = 174.3 \text{ g/mol} \)
2. **Calculate the number of moles of \( \text{K}_2\text{SO}_4 \):**
- Mass of \( \text{K}_2\text{SO}_4 \): 23.4 g
- Molar mass of \( \text{K}_2\text{SO}_4 \): 174.3 g/mol
- Number of moles (\( n \)):
\[
n = \frac{23.4 \text{ g}}{174.3 \text{ g/mol}} = 0.134 \text{ mol}
\]
3. **Calculate the volume of the solution in liters:**
- Volume: 500 mL = 0.500 L
4. **Determine the molarity of \( \text{K}_2\text{SO}_4 \):**
\[
\text{Molarity (\( M \))} = \frac{\text{Number of moles}}{\text{Volume (in L)}}
\]
\[
M = \frac{0.134 \text{ mol}}{0.500 \text{ L}} = 0.268 \text{](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ffcaf0374-1550-4ffb-84ad-720668c0d5ec%2F71bb4975-0cf5-4944-b85d-a51e69430c44%2F87b202j_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Calculating Molarity of Ionic Species in a Potassium Sulfate Solution
**Problem Statement:**
A solution is made by dissolving 23.4 g of potassium sulfate, \( \text{K}_2\text{SO}_4 \), in enough water to make exactly 500 mL of solution. Calculate the molarity of each species.
#### Steps to Solve:
1. **Determine the Molar Mass of \( \text{K}_2\text{SO}_4 \):**
- Potassium (K): \( 2 \times 39.1 \text{ g/mol} = 78.2 \text{ g/mol} \)
- Sulfur (S): \( 1 \times 32.1 \text{ g/mol} = 32.1 \text{ g/mol} \)
- Oxygen (O): \( 4 \times 16.0 \text{ g/mol} = 64.0 \text{ g/mol} \)
- **Total molar mass:** \( 78.2 + 32.1 + 64.0 = 174.3 \text{ g/mol} \)
2. **Calculate the number of moles of \( \text{K}_2\text{SO}_4 \):**
- Mass of \( \text{K}_2\text{SO}_4 \): 23.4 g
- Molar mass of \( \text{K}_2\text{SO}_4 \): 174.3 g/mol
- Number of moles (\( n \)):
\[
n = \frac{23.4 \text{ g}}{174.3 \text{ g/mol}} = 0.134 \text{ mol}
\]
3. **Calculate the volume of the solution in liters:**
- Volume: 500 mL = 0.500 L
4. **Determine the molarity of \( \text{K}_2\text{SO}_4 \):**
\[
\text{Molarity (\( M \))} = \frac{\text{Number of moles}}{\text{Volume (in L)}}
\]
\[
M = \frac{0.134 \text{ mol}}{0.500 \text{ L}} = 0.268 \text{
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