A certain substance X condenses at a temperature of 128.4 °C. But if a 800. g sample of X is prepared with 81.06 g of urea ((NH),CO) dissolved in it, the sample is found to have a condensation point of 129.7 °C instead. Calculate the molal boiling point elevation constant K, of X. Round your answer to 2 significant digits. -1 °C-mol kg

A certain substance X condenses at a temperature of 128.4 °C. But if a 800. g sample of X is prepared with 81.06 g of urea ((NH),CO) dissolved in it, the sample is found to have a condensation point of 129.7 °C instead. Calculate the molal boiling point elevation constant K, of X. Round your answer to 2 significant digits. -1 °C-mol kg

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter11: Properties Of Solutions

Section: Chapter Questions

Problem 72E: A solution contains 3.75 g of a nonvolatile pure hydrocarbon in 95 g acetone. The boiling points of...

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A solution contains 3.75 g of a nonvolatile pure hydrocarbon in 95 g acetone. The boiling points of pure acetone and the solution are 55.95C and 56.50C, respectively. The molal boiling-point constant of acetone is 1.71 C kg/mol. What is the molar mass of the hydrocarbon?
Two samples of sodium chloride solutions are brought to a boil on a stove. One of the solutions boils at 100.10C and the other at 100.15C. a Which of the solutions is more concentrated? b Which of the solutions would have a lower freezing point? c If you split the solution that boils at 100.1C into two portions, how would the boiling points of the samples compare? Which of the following statements do you agree with regarding the determination of your answer for part c? I. The question cannot be answered with certainty without knowing the volumes of each portion. II. Making the necessary assumption that the two samples have equal volumes, I was able to correctly answer the question. III. The volumes that the sample was split into are irrelevant when determining the correct answer.
A sucrose (C12H22O11) solution that is 45.0% sucrose by mass has a density of 1.203 g/mL at 25C. Calculate its (a) molarity. (b) molality. (c) vapor pressure(vpH2Oat25C=23.76mmHg). (d) normal boiling point.
Consider two hypothetical pure substances, AB(s) and XY(s). When equal molar amounts of these substances are placed in separate 500-mL samples of water, they undergo the following reactions: AB(s)A+(aq)+B(aq)XY(s)XY(aq) a Which solution would you expect to have the lower boiling point? Why? b Would you expect the vapor pressures of the two solutions to be equal? If not, which one would you expect to have the higher vapor pressure? c Describe a procedure that would make the two solutions have the same boiling point. d If you took 250 mL of the AB(aq) solution prepared above, would it have the same boiling point as the original solution? Be sure to explain your answer. e The container of XY(aq) is left out on the bench top for several days, which allows some of the water to evaporate from the solution. How would the melting point of this solution compare to the melting point of the original solution?
Calculate the freezing point and normal boiling points of each of the following aqueous solutions. (a) 2.63 m acetic acid (b) 33.0 % by mass lactose, C12H22O11 (c) 32.15 mL of ethylene glycol, C2H6O2(d=1.113g/mL) in 624 mL of water (d=1.00g/mL)
If l-mol samples of urea, a nonelectrolyte, sodium chloride, and calcium chloride are each dissolved in equal volumes of water in separate containers: a Which solution would have the highest boiling point? b Which solution would have the highest freezing point?
In some regions of the southwest United States, the water is very hard. For example, in Las Cruces, New Mexico, the tap water contains about 560 g of dissolved solids per milliliter. Reverse osmosis units are marketed in this area to soften water. A typical unit exerts a pressure of 8.0 atm and can produce 45 L water per day. a. Assuming all of the dissolved solids are MgCO3 and assuming a temperature of 27C, what total volume of water must be processed to produce 45 L pure water? b. Would the same system work for purifying seawater? (Assume seawater is 0.60 M NaCl.)
Carbon tetrachloride (CCl4) boils at 76.8C and has a density of 1.59 g/mL. (a) A solution prepared by dissolving 0.287 mol of a nonelectrolyte in 255 mL of CCl4 boils at 80.3C. What is the boiling point constant (kb) for CCl4? (b) Another solution is prepared by dissolving 37.1 g of an electrolyte (MM=167g/mol) in 244 mL of CCl4. The resulting solution boils at 85.2C. What is i for the electrolyte?

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