solution was prepared by dissolving 34.7 g of KOH in 88.0 g of ethanol (C₂H5OH). A What is the molality of the solution? B. What is the van't Hoff factor (i) and colligative molality for the solution? c. What is the boiling point of the solution? Show all work on separate paper and upload as a PDF with the rest of your exam work. Please circle all final answers. In the answer space provided, please write "see attached." For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). BIVS Paragraph V Arial SE 田出田园田 V <> (0) 10pt X² X₂ & Be V Av 2 IX ✓ 11 "152 *** B

solution was prepared by dissolving 34.7 g of KOH in 88.0 g of ethanol (C₂H5OH). A What is the molality of the solution? B. What is the van't Hoff factor (i) and colligative molality for the solution? c. What is the boiling point of the solution? Show all work on separate paper and upload as a PDF with the rest of your exam work. Please circle all final answers. In the answer space provided, please write "see attached." For the toolbar, press ALT+F10 (PC) or ALT+FN+F10 (Mac). BIVS Paragraph V Arial SE 田出田园田 V <> (0) 10pt X² X₂ & Be V Av 2 IX ✓ 11 "152 *** B

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter10: Properties Of Solutions

Section: Chapter Questions

Problem 120CP: Plants that thrive in salt water must have internal solutions (inside the plant cells) that are...

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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?
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.
Plants that thrive in salt water must have internal solutions (inside the plant cells) that are isotonic with (have the same osmotic pressure as) the surrounding solution. A leaf of a saltwater plant is able to thrive in an aqueous salt solution (at 25C) that has a freezing point equal to 0.62lC. You would like to use this information to calculate the osmotic pressure of the solution in the cell. a. In order to use the freezing-point depression to calculate osmotic pressure, what assumption must you make (in addition to ideal behavior of the solutions, which we will assume)? b. Under what conditions is the assumption (in part a) reasonable? c. Solve for the osmotic pressure (at 25C) of the solution in the plant cell. d. The plant leaf is placed in an aqueous salt solution (at 25C) that has a boiling point of l02.0C. What will happen to the plant cells in the leaf?
In terms of Raoults law, distinguish between an ideal liquid-liquid solution and a nonideal liquid-liquid solution. lf a solution is ideal, what is true about Hsoln, T for the solution formation, and the interactive forces within the pure solute and pure solvent as compared to the interactive forces within the solution? Give an example of an ideal solution. Answer the previous two questions for solutions that exhibit either negative or positive deviations from Raoults law.
A gaseous solute dissolves in water. The solution process has H=15 kJ. Its solubility at 22C and 6.00 atm is 0.0300 M. Would you expect the solubility to be greater or less at (a) 22C and 1 atm? (a) 18C and 6 atm? (a) 15C and 10 atm? (a) 35C and 3 atm?
You dissolve 1.0 mol of urea (H2NCONH2) in 270 g of water. The mole fraction of urea is (a) 3710 3 (b) 0.063 (c) 16 (d) 1.0 and its molality is (a) 1.0 (b) 3.7 (c) 0.063 (d) 0.27