0.40 M CaBr2 in water (strong electrolyte) 0.40 M KCI in water (strong electrolyte) 0.40 M HF in water (weak electrolyte; weak acid) 0.20 M NazPO4 in water (strong electrolyte) Which of the following statements is true for their solution properties? O a.0.40 mCaBr2 in water has the lowest freezing point. O b.0.40 m KCI in water has the highest freezing point. O .0.40 m HF in water has the lowest freezing point. d.0.20 m NagPO4 in water has the highest freezing point. O e. None of the above

0.40 M CaBr2 in water (strong electrolyte) 0.40 M KCI in water (strong electrolyte) 0.40 M HF in water (weak electrolyte; weak acid) 0.20 M NazPO4 in water (strong electrolyte) Which of the following statements is true for their solution properties? O a.0.40 mCaBr2 in water has the lowest freezing point. O b.0.40 m KCI in water has the highest freezing point. O .0.40 m HF in water has the lowest freezing point. d.0.20 m NagPO4 in water has the highest freezing point. O e. None of the above

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter7: Solutions And Colloids

Section: Chapter Questions

Problem 7.65E

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Vodka is advertised to be 80 proof. That means that the ethanol (C2H5OH) concentration is 40% (two significant figures) by volume. Assuming the density of the solution to be 1.0 g/mL, what is the freezing point of vodka? The density of ethanol is 0.789 g/mL.
Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol, C2H5OH. Tube C has an aqueous 1.0 m solution of NaCl. Which of the following statements are true? (Assume that for these solutions 1.0m=1.0M.) (a) The vapor pressure of the solvent over tube A is greater than the solvent pressure over tube B. (b) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube A. (c) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube C. (d) The boiling point of the solution in tube B is higher than the boiling point of the solution in tube C. (e) The osmotic pressure of the solution in tube B is greater than the osmotic pressure of the solution in tube C.
You have read that adding a solute to a solvent can both increase the boiling point and decrease the freezing point. A friend of yours explains it to you like this: The solute and solvent can be like salt in water. The salt gets in the way of freezing in that it blocks the water molecules from joining together. The salt acts like a strong bond holding the water molecules together so that it is harder to boil. What do you say to your friend?
A solution was prepared by dissolving 0.800 g of sulfur, Sg, in 100.0 g of acetic acid, HC2H3O2. Calculate the freezing point and boiling point of the solution.
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