A 1.137 g sample contains only vitamin C (CH₂O) and sucralose (C₁2H₁9Cl3 Og). When the sample is dissolved in water to a total volume of 34.9 mL, the osmotic pressure of the solution is 3.86 atm at 299 K. What is the mass percent of vitamin C and sucralose in the sample? vitamin C: sucralose: x10 TOOLS % %

A 1.137 g sample contains only vitamin C (CH₂O) and sucralose (C₁2H₁9Cl3 Og). When the sample is dissolved in water to a total volume of 34.9 mL, the osmotic pressure of the solution is 3.86 atm at 299 K. What is the mass percent of vitamin C and sucralose in the sample? vitamin C: sucralose: x10 TOOLS % %

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 153. g of glycine (C,H,NO2) are dissolved in 1400. g of a certain mystery liquid X, the freezing point of the solution is 4.9 °C lower than the freezing point of pure X. On the other hand, when 153. g of iron(III) nitrate (Fe(NO,)) are dissolved in the same mass of X, the freezing point of the solution is 4.8 °C lower than the freezing point of pure X. Calculate the van't Hoff factor for iron(III) nitrate in X. Be sure your answer has a unit symbol, if necessary, and round your answer to 2 significant digits. i = |
The nonvolatile, nonelectrolyte aspirin, C9Hg 04 (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 Rast camphor method is a cryoscopic technique for molar mass determination. Exactly 1.00 g of an isoprenoid of known formula (C5H8)n was dissolved in 5.00 g of camphor. The freezing point of the resulting solution decreased by 27.7 ℃ relative to pure camphor. Knowing that the Kf of camphor is 37.7 deg·kg/mol: Calculate for the molar mass of the isoprenoid. Calculate the value of n in the given formula of the isoprenoid. Report in whole number. The normal freezing point of camphor is 178.4 ℃. At what temperature did the isoprenoid-camphor solution freeze?
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
3. 2 g of NacI is dissolved in 500 g of water at 35°C. Determine the ff: PNacI • 2.16 cm a. Boiling point elevation b. Freezing point depression C. Vapor pressure of the solution d. Osmotic pre ssure
A solution contains 10.0 g of carbon tetrachloride, CCl4, and 20.0 g of benzene, C6H6. Calculate the mole fraction of each component if the MW are CCL4 = 153.8 g/mol and C6H6 = 78.1 g/mol. (Thanks!)
When 3.25 g of a nonelectrolyte solute is dissolved in water to make 165 mL of solution at 24 °C, the solution exerts an osmotic pressure of 879 torr.What is the molar concentration of the solution? MHow many moles of solute are in the solution? molWhat is the molar mass of the solute? g/mol
Thank you!
The osmotic pressure (in atm) of 0.499 M K2SO4 solution at 298 K is ______? Give your answer to three sig figs.
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
EJ0.939 M What is the vapor pressure of a 45.0 % solution of glucose, CH,,06, at a particular temperature, 12 6' given that the vapor pressure of pure water at that temperature is 486 mm Hg? 186 m m Ha
6. Complete the following table. Expected freezing point °C molality solution Molar Mass of Mass of Substance Mass, g/mol solute, g water ,g 0.09 Calcium chloride 111 12.0 250 g 0.10 Fructose 180 3.50 g 50.0 g -2.10 Ethylene glycol 250 g -4.0 120.3 Magnesium sulfate 250 g -3.46 60 Urea 1| |