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:**
Calculate the osmotic pressure of 0.38 M KNO₃ (electrolyte) at 25°C. Enter your answer in the provided box.
[ ] atm
**Explanation:**
To calculate the osmotic pressure (π), you can use the formula:
\[ \pi = iMRT \]
where:
- \( i \) = Van't Hoff factor (for KNO₃, \( i = 2 \) as it dissociates into K⁺ and NO₃⁻)
- \( M \) = molarity of the solution (0.38 M)
- \( R \) = ideal gas constant (0.0821 L·atm/mol·K)
- \( T \) = temperature in Kelvin (25°C = 298 K)
Plug in the values to find the osmotic pressure.
**Solution:**
\[ \pi = (2)(0.38 \, \text{M})(0.0821 \, \text{L·atm/mol·K})(298 \, \text{K}) = \text{osmotic pressure in atm} \]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F073eb5ef-2617-4d6f-9bce-a81ca84c4945%2F9d4e311e-c45e-45fb-a70a-c9bded43c0b5%2F3p630ye.jpeg&w=3840&q=75)
Transcribed Image Text:**Question:**
Calculate the osmotic pressure of 0.38 M KNO₃ (electrolyte) at 25°C. Enter your answer in the provided box.
[ ] atm
**Explanation:**
To calculate the osmotic pressure (π), you can use the formula:
\[ \pi = iMRT \]
where:
- \( i \) = Van't Hoff factor (for KNO₃, \( i = 2 \) as it dissociates into K⁺ and NO₃⁻)
- \( M \) = molarity of the solution (0.38 M)
- \( R \) = ideal gas constant (0.0821 L·atm/mol·K)
- \( T \) = temperature in Kelvin (25°C = 298 K)
Plug in the values to find the osmotic pressure.
**Solution:**
\[ \pi = (2)(0.38 \, \text{M})(0.0821 \, \text{L·atm/mol·K})(298 \, \text{K}) = \text{osmotic pressure in atm} \]
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