The nonvolatile, nonelectrolyte aspirin, C,H,O4 (180.10 g/mol), is soluble in diethyl ether CH3CH₂OCH₂CH3. Calculate the osmotic pressure generated when 11.5 grams of aspirin are dissolved in 207 ml of a diethyl ether solution at 298 K. The molarity of the solution is The osmotic pressure of the solution is M. atmospheres.

The nonvolatile, nonelectrolyte aspirin, C,H,O4 (180.10 g/mol), is soluble in diethyl ether CH3CH₂OCH₂CH3. Calculate the osmotic pressure generated when 11.5 grams of aspirin are dissolved in 207 ml of a diethyl ether solution at 298 K. The molarity of the solution is The osmotic pressure of the solution is M. atmospheres.

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...

See similar textbooks

Similar questions

When 225. of urea (CH,N,0) are dissolved in 1200. g Oof a certain mystery g liquid x, the freezing point of the solution is 8.4 °c lower than the freezing point of pure x. On the other hand, when 225. g of sodium chloride are dissolved in the same mass of x, the freezing point of the solution is 14.5 °C lower than the freezing point of pure x. olo Ar Calculate the van't Hoff factor for sodium chloride in x. Be sure your answer has a unit symbol, if necessary, and is rounded to the correct number of significant digits. i = |
A 0.751-g sample of protein is dissolved in 50.0 mL of solution, and the solution exhibits an osmotic pressure of 4.1 torr at 25oC. Calculate the molar mass of protein. (R = 0.08206 L.atm/(mol.K); 1 atm = 760 torr; assume the protein is nonelectrolyte)
A nonvolatile solute is dissolved in benzene and the resulting solution has a vapor pressure of 18.7 torr. What is the mole fraction of the solute? (P° of benzene is 26.5 torr).
7) A 300.0 mL aqueous solution containing 0.512 g of an unknown polymer has an osmotic pressure of 32.9 torr at 29.5°C. What is the molar mass of the polymer? 29.5°C +273 =303.5K
What mass of H2O is needed to dissolve 4.69 g KMnO4 to produce a solution having a molality of 0.299 m? Assume that the density of the solution is 1.00 g/mL. The molar mass of KMnO4 is 158.03 g/mol and the molar mass of H2O is 18.02 g/mol.
In a laboratory experiment, students synthesized a new compound and found that when 14.61 grams of the compound were dissolved to make 210.0 mL of a ethanol solution, the osmotic pressure generated was 1.91 atm at 298 K. The compound was also found to be nonvolatile and a non-electrolyte. What is the molecular weight they determined for this compound? Molar mass = g/mol
13.) 0.6674 g of an unknown non-electrolyte is dissolved in enough water to make 125.0 mL of solution at 30.6 °C, giving an osmotic pressure of 0.03905 atm. What is the molar mass, in grams per mole, of the substance? Your Answer:
When a 22.275 g sample of Compound B, is dissolved in 480.2 g of benzene, the freezing point of the following solution is 3.73 ˚C. The freezing point of benzene is 5.48 ˚C, and the Kf for benzene is 5.12 ˚C/m. Determine the molar mass of Compound B.
A certain organic compound O has a solubility in acetonitrile of 13.8 at 25. °C. Calculate the mass of O that's dissolved in L 650. mL of a saturated solution of O in acetonitrile at this temperature. Be sure your answer has the correct unit symbol and 3 significant digits. x10
13.69 g of protein are dissolved in 200.0 mL of water at 28.3 ∘C. The osmotic pressure of the solution is 1.999 mmHg. Find the molar mass of the protein.