Please choose correct answer Your answers are saved automatically.Lessaining Time: 22 minutes, 00 seconds.estion Completion Status:27 28 2933D34 35013014151617181920212223242630313224050678.9.101112A Moving to another question will save this response.estion 28water to lower the freezing point to 98.70°C. The molar mass of the compound is 50.0 g/mol and the Kf for water is 1.86°C kg/mol.Determine the mass of a nonvolatile, nonionizing compound that must be added to 4.76 kgO 253 gO 166 gO 575 g7.34 gO 15.0 gMoving to another question will save this response.MacBook Proesc&@#$712345T.Y* 0025

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A Moving to another question will save this response. estion 28 Determine the mass of a nonvolatile, nonionizing compound that must be added to 4.76 kg of water to lower the freezing point to 98.70°C. The molar mass of the compound is 50.0 g/mol and the Kf for water is 1.86°C kg/mol. O 253 g O 166 g O 575 g O 7.34 g O 15.0 g A Moving to another question will save this response.

A Moving to another question will save this response. estion 28 Determine the mass of a nonvolatile, nonionizing compound that must be added to 4.76 kg of water to lower the freezing point to 98.70°C. The molar mass of the compound is 50.0 g/mol and the Kf for water is 1.86°C kg/mol. O 253 g O 166 g O 575 g O 7.34 g O 15.0 g A Moving to another question will save this response.

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 142IP: Anthraquinone contains only carbon, hydrogen, and oxygen. When 4.80 mg anthraquinone is burned, 14.2...

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Instead of using NaCl to melt the ice on your sidewalk you decide to use CaCl2. If you add 35.0 g of CaCl2 to 150. g of water, what is the freezing point of the solution? (Assume i = 2.7 for CaCl2.)
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Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water, by calculating the freezing point depression of solutions containing 200. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is. it absorbs moisture from the air to give a solution and begin the process. A disadvantage is that this compound is more costly.)
What mass of a 4.00% NaOH solution by mass contains 15.0 g of NaOH?
Equal numbers of moles of two soluble, substances, substance A and substance B, are placed into separate 1.0-L samples of water. a The water samples are cooled. Sample A freezes at 0.50C, and Sample B freezes at l.00C. Explain how the solutions can have different freezing points. b You pour 500 mL of the solution containing substance B into a different beaker. How would the freezing point of this 500-mL portion of solution B compare to the freezing point of the 1.0-L sample of solution A? c Calculate the molality of the solutions of A and B. Assume that i = 1 for substance A. d If you were to add an additional 1.0 kg of water to solution B, what would be the new freezing point of the solution? Try to write an answer to this question without using a mathematical formula. e What concentration (molality) of substances A and B would result in both solutions having a freezing point of 0.25C? f Compare the boiling points, vapor pressure, and osmotic pressure of the original solutions of A and B. Dont perform the calculations; just state which is the greater in each ease.
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?
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Anthraquinone contains only carbon, hydrogen, and oxygen. When 4.80 mg anthraquinone is burned, 14.2 mg CO2 and 1.65 mg H2O are produced. The freezing point of camphor is lowered by 22.3C when 1.32 g anthraquinone is dissolved in 11.4 g camphor. Determine the empirical and molecular formulas of anthraquinone.
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Distinguish between dispersion methods and condensation methods for preparing colloidal systems.
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