Colligative Properties of Solution naphthalene (MM=128.2 g/mol) in 650.0 g of a certain solvent X. It was determined that the freezing point of the resulting solution was 3.685°C. A solution was prepared by dissolving 30 g of a. Assuming that the solution is ideally dilute, what is the van’t Hoff factor? b. What is the molal concentration of the solute in the solution? c. If the freezing point of the pure solvent is 5.53°C, determine the KF of the solvent.

Colligative Properties of Solution naphthalene (MM=128.2 g/mol) in 650.0 g of a certain solvent X. It was determined that the freezing point of the resulting solution was 3.685°C. A solution was prepared by dissolving 30 g of a. Assuming that the solution is ideally dilute, what is the van’t Hoff factor? b. What is the molal concentration of the solute in the solution? c. If the freezing point of the pure solvent is 5.53°C, determine the KF of the solvent.

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 9RQ: Distinguish between a strong electrolyte, a weak electrolyte, and a nonelectrolyte. How can...

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Distinguish between a strong electrolyte, a weak electrolyte, and a nonelectrolyte. How can colligative properties be used to distinguish between them? What is the vant Hoff factor? Why is the observed freezing-point depression for electrolyte solutions sometimes less than the calculated value? Is the discrepancy greater for concentrated or dilute solutions?
An aqueous solution of sodium bromide freezes at 1.61 C. What is the total molality of solute particles? How many grams of sodium bromide are present in 1 kg of water? (Assume an ideal value for the vant Hoff factor.)
Erythrocytes are red blood cells containing hemoglobin. In a saline solution they shrivel when the salt concentration is high and swell when the salt concentration is low. In a 25C aqueous solution of NaCl, whose freezing point is 0.406C, erythrocytes neither swell nor shrink. If we want to calculate the osmotic pressure of the solution inside the erythrocytes under these conditions, what do we need to assume? Why? Estimate how good (or poor) of an assumption this is. Make this assumption and calculate the osmotic pressure of the solution inside the erythrocytes.
The solubility of ethylene (C2H4) in water at 20 C and 0.300 atm pressure is 1.27 104 molal. (a) Calculate the Henrys law constant for this gas in units of molal/torr. (b) How many grams of ethylene are dissolved in 1.00 kg water at 20 C if the pressure of the gas is 500 torr?