12.9 When 542 mg of the nonelectrolyte compound Z is dis-solved in a certain mass of the solvent A, the A freezing point isdepressed by 1.65 times the depression observed when 679 mgof CO(NH2)2 is dissolved in the same mass of A. Find themolecular weight of Z.

Answered: 12.9 When 542 mg of the nonelectrolyte…

EBK A SMALL SCALE APPROACH TO ORGANIC L

4th Edition

ISBN:9781305446021

Author:Lampman

Publisher:Lampman

Chapter84: Fractional Distillation, Azeotropes

Section: Chapter Questions

Problem 1P

See similar textbooks

Similar questions

A solution is made by dissolving 34.0 g of NaCl in 100 g of H2O at 0C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentrated
The freezing point of 0.10 M KHSO3 is -0.38C. Which of the following equations best represents what happens when KHSO3 dissolves in water? (a) KHSO3(s)KHSO3(aq) (b) KHSO3(s) K+(aq)+HSO3(aq) (c) KHSO3(s) K+(aq)+SO32(aq)+ H+(aq)
The organic salt [(C4H9)4N][ClO4] consists of the ions (C4H9)4N+ and ClO4. The salt dissolves in chloroform. What mass (in grams) of the salt must have been dissolved if the boiling point of a solution of the salt in 25.0 g chloroform is 63.20 C? The normal boiling point of chloroform is 61.70 C and Kb = 3.63 C kg mol1. Assume that the salt dissociates completely into its ions in solution.
The freezing-point depression of a 0.091-m solution of CsCl is 0.320C. The freezing-point depression of a 0.091-m solution of CaCl2 is 0.440C. In which solution does ion association appear to be greater? Explain.
The vapor pressures of several solutions of water-propanol (CH3CH2CH2OH) were determined at various compositions, with the following data collected at 45C: H2O Vapor pressure(torr) 0 74.0 0.15 77.3 0.37 80.2 0.54 81.6 0.69 80.6 0.83 78.2 1.00 71.9 a. Are solutions of water and propanol ideal? Explain. b. Predict the sign of Hsoln for water-propanol solutions. c. Are the interactive forces between propanol and water molecules weaker than, stronger than, or equal to the interactive forces between the pure substances? Explain. d. Which of the solutions in the data would have the lowest normal boiling point?
How many theoretical plates are required to produce a solution with a mole fraction of hexane greater than 0.90? Figure B A temperature-composition diagram for hexane (C6H14)-heptane (C7H16) mixtures.
Reserpine is a natural product isolated from the roots of the shrub Rauwolfia serpenlina. It was first synthesized in 1956 by Nobel Prize winner R. B. Woodward. It is used as a tranquilizer and sedative. When 1.00 g reserpine is dissolved in 25.0 g camphor, the freezing-point depression is 2.63C (Kr for camphor is 40.C kg/mol). Calculate the molality of the solution and the molar mass of reserpine.
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?
State Raoult’s law for a solution containing volatile components. How does Raoult’s law become a special case of Henry’s law?(b) 1.00 g of a non-electrolyte solute dissolved in 50 g of benzene lowered the freezing point of benzene by 0.40 K. Find the molar mass of the solute. (Kf for benzene = 5.12 K kg mol-1)
In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride. Calculate the mass of potassium chloride present in the salt sample.
In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride. Calculate the molality of the solution.
In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride. Calculate ΔTf for the experiment.

SEE MORE QUESTIONS

Recommended textbooks for you

EBK A SMALL SCALE APPROACH TO ORGANIC L

Chemistry

ISBN:

9781305446021

Author:

Lampman

Publisher:

CENGAGE LEARNING - CONSIGNMENT

General, Organic, and Biological Chemistry

Chemistry

ISBN:

9781285853918

Author:

H. Stephen Stoker

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

EBK A SMALL SCALE APPROACH TO ORGANIC L

Chemistry

ISBN:

9781305446021

Author:

Lampman

Publisher:

CENGAGE LEARNING - CONSIGNMENT

General, Organic, and Biological Chemistry

Chemistry

ISBN:

9781285853918

Author:

H. Stephen Stoker

Publisher:

Cengage Learning

Chemistry & Chemical Reactivity

Chemistry

ISBN:

9781337399074

Author:

John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:

Cengage Learning

Chemistry: Principles and Reactions

Chemistry

ISBN:

9781305079373

Author:

William L. Masterton, Cecile N. Hurley

Publisher:

Cengage Learning

Chemistry: The Molecular Science

Chemistry

ISBN:

9781285199047

Author:

John W. Moore, Conrad L. Stanitski

Publisher:

Cengage Learning

Chemistry

ISBN:

9781305957404

Author:

Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS

12.9 When 542 mg of the nonelectrolyte compound Z is dis- solved in a certain mass of the solvent A, the A freezing point is depressed by 1.65 times the depression observed when 679 mg of CO(NH2)2 is dissolved in the same mass of A. Find the molecular weight of Z.