Part A At what temperature would a 1.95 m NaCl solution freeze, given that the van't Hoff factor for NaCl is 1.9? K for water is 1.86 °C/m. Express your answer with the appropriate units. ▸ View Available Hint(s) Value Submit HA Part B → Units ? A 0.050 M solution of AlCl3 had an observed osmotic pressure of 3.85 atm at 20 °C. Calculate the van't Hoff factor i for AlCl3. Express your answer numerically. ► View Available Hint(s)

Part A At what temperature would a 1.95 m NaCl solution freeze, given that the van't Hoff factor for NaCl is 1.9? K for water is 1.86 °C/m. Express your answer with the appropriate units. ▸ View Available Hint(s) Value Submit HA Part B → Units ? A 0.050 M solution of AlCl3 had an observed osmotic pressure of 3.85 atm at 20 °C. Calculate the van't Hoff factor i for AlCl3. Express your answer numerically. ► View Available Hint(s)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter12: Solutions

Section: Chapter Questions

Problem 12.103QE

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Once again, consider Fig. 10-9. Suppose instead of having a nonvolatile solute in the solvent in one beaker, the two beakers contain different volatile liquids. That is, suppose one beaker contains liquid A (Pvap = 50 torr) and the other beaker contains liquid B (Pvap = 100 torr). Explain what happens as time passes. How is this similar to the first case (shown in the figure)? How is it different?
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?
An aqueous solution containing 0.250 mole of Q, a strong electrolyte, in 5.00 102 g water freezes at 2.79C. What is the vant Hoff factor for Q? The molal freezing-point depression constant for water is 1.86C kg/mol. What is the formula of Q if it is 38.68% chlorine by mass and there are twice as many anions as cations in one formula unit of Q?
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?
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?