When 225. g of urea (CH,N,0) are dissolved in 1200. g of a certain mystery 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 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 = |

When 225. g of urea (CH,N,0) are dissolved in 1200. g of a certain mystery 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 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 = |

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

Chapter11: Properties Of Solutions

Section: Chapter Questions

Problem 129CP: You make 20.0 g of a sucrose (C12H22O11) and NaCl mixture and dissolve it in 1.00 kg water. The...

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An aqueous solution containing 10.0 g of starch per liter has an osmotic pressure of 3.8 mm Hg at 25 C. (a) What is the average molar mass of starch? (The result is an average because not all starch molecules are identical.) (b) What is the freezing point of the solution? Would it be easy to determine the molecular weight of starch by measuring the freezing point depression? (Assume that the molarity and molality are the same for this solution.)
You make 20.0 g of a sucrose (C12H22O11) and NaCl mixture and dissolve it in 1.00 kg water. The freezing point of this solution is found to be 0.426C. Assuming ideal behavior, calculate the mass percent composition of the original mixture, and the mole fraction of sucrose in the original mixture.
The Rast method uses camphor (C10H16O) as a solvent for determining the molar mass of a compound. When 2.50 g of cortisone acetate are dissolved in 50.00 g of camphor (k f =40.0C/m), the freezing point of the mixture is 173.44C; that of pure camphor is 178.40C. What is the molar mass of cortisone acetate?
Juice (d=1.0g/mL) from freshly harvested grapes has about 24% sucrose by mass. What is the molality of sucrose, C12H22O11, in the grape juice after 25% (by mass) of the water content has been removed? Assume a volume of 15.0 L.