Table of contents

1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

14. Solutions

Osmotic Pressure

General Chemistry

14. Solutions

Osmotic Pressure

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Multiple Choice

What is the osmotic pressure of a solution formed by dissolving 44.3 mg of aspirin (C9H8O4) in 0.358 L of water at 25 °C, assuming complete dissociation and ideal behavior?

0.048 atm

0.012 atm

0.036 atm

0.024 atm

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Verified step by step guidance

First, calculate the molar mass of aspirin (C9H8O4). Add the atomic masses of all atoms in the formula: 9 carbon atoms, 8 hydrogen atoms, and 4 oxygen atoms. Use the periodic table to find the atomic masses: Carbon (C) is approximately 12.01 g/mol, Hydrogen (H) is approximately 1.01 g/mol, and Oxygen (O) is approximately 16.00 g/mol.

Convert the mass of aspirin from milligrams to grams by dividing by 1000. This gives you 0.0443 g of aspirin.

Calculate the number of moles of aspirin using the formula: \( \text{moles} = \frac{\text{mass in grams}}{\text{molar mass}} \). Use the molar mass calculated in step 1.

Use the formula for osmotic pressure: \( \Pi = \frac{nRT}{V} \), where \( \Pi \) is the osmotic pressure, \( n \) is the number of moles of solute, \( R \) is the ideal gas constant (0.0821 L·atm/mol·K), \( T \) is the temperature in Kelvin, and \( V \) is the volume of the solution in liters. Convert the temperature from Celsius to Kelvin by adding 273.15 to the Celsius temperature.

Substitute the values for \( n \), \( R \), \( T \), and \( V \) into the osmotic pressure formula to find the osmotic pressure of the solution. Ensure all units are consistent for accurate calculation.