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

6. Chemical Quantities & Aqueous Reactions

Osmolarity

General Chemistry

6. Chemical Quantities & Aqueous Reactions

Osmolarity

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Multiple Choice

0.302 grams of an antibiotic was dissolved in enough water at 23.6°C to make 500.0 mL of solution. The solution has an osmotic pressure of 8.34 mm Hg. What is the molar mass of the antibiotic?

350 g/mol

250 g/mol

150 g/mol

450 g/mol

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Verified step by step guidance

First, understand that osmotic pressure (π) can be calculated using the formula: π = (n/V)RT, where n is the number of moles, V is the volume in liters, R is the ideal gas constant, and T is the temperature in Kelvin.

Convert the given osmotic pressure from mm Hg to atm, since the ideal gas constant R is typically used in atm. Use the conversion: 1 atm = 760 mm Hg.

Convert the temperature from Celsius to Kelvin using the formula: T(K) = T(°C) + 273.15.

Rearrange the osmotic pressure formula to solve for the number of moles (n): n = (πV)/(RT). Substitute the values for π (in atm), V (in liters), R (0.0821 L·atm/mol·K), and T (in Kelvin) into the equation.

Finally, calculate the molar mass of the antibiotic by dividing the mass of the antibiotic (0.302 grams) by the number of moles calculated in the previous step. Molar mass = mass/n.