Boiling Point Elevation/Freezing Point DepressionT = m KWhere:T= T(solution) - T(pure solvent) *m= (# moles solute / Kg solvent)Kb= boiling point elevation constant.Kf= freezing point depression constant.Kb and Kf depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow.SolventFormulaKb (°C / m)Kf (°C / m)WaterH2O0.512-1.86EthanolCH3CH2OH1.22-1.99ChloroformCHCl33.67 BenzeneC6H62.53-5.12Diethyl etherCH3CH2OCH2CH32.02 note that ΔT as defined above will be a negative number for freezing point depression. Therefore, Kf must also be given as a negative number. The boiling point of diethyl ether, CH3CH2OCH2CH3, is 34.50°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is aspirin.A student dissolves 14.52 grams of aspirin, C9H304 (180.1 g/mol), in 156.5 grams of diethyl ether. Use the table of boiling and freezing point constants to answer the questions below.SolventFormulaKb (°C/m) Kf (°C/m)WaterH200.5121.86EthanolCH3CH2OH1.221.99ChloroformCHC133.67BenzeneC6H62.535.12Diethyl ether CH;CH2OCH2CH32.02The molality of the solution ism.The boiling point of the solution is°C. The boiling point of diethyl ether CH3CH2OCH2CH3 is 34.50°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is estrogen (estradiol).How many grams of estrogen, C18H2402 (272.4 g/mol), must be dissolved in 250.0 grams of diethyl ether to raise the boiling point by 0.450 °C ? Refer to the table for the necessary boiling or freezing point constant.SolventFormulaKb (°C/m) Kf (°C/m)WaterH200.5121.86EthanolCH3CH2OH1.221.99ChloroformCHC133.67BenzeneC6H62.535.12Diethyl ether CH3CH2OCH2CH32.02g estrogen.

The question is based on the concept of solutions. Molality is a method of expressing concentration…

Answered: A student dissolves 14.52 grams of…

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Boiling Point Elevation/Freezing Point Depression
T = m K

Where:

T	= T(solution) - T(pure solvent) *
m	= (# moles solute / Kg solvent)
K_b	= boiling point elevation constant.
K_f	= freezing point depression constant.

K_b and K_f depend only on the SOLVENT. Below are some common values. Use these values for the calculations that follow.

Solvent	Formula	K_b (°C / m)	K_f (°C / m)
Water	H₂O	0.512	-1.86
Ethanol	CH₃CH₂OH	1.22	-1.99
Chloroform	CHCl₃	3.67
Benzene	C₆H₆	2.53	-5.12
Diethyl ether	CH₃CH₂OCH₂CH₃	2.02

note that ΔT as defined above will be a negative number for freezing point depression. Therefore, K_f must also be given as a negative number.

The boiling point of diethyl ether, CH3CH2OCH2CH3, is 34.50°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is aspirin.
A student dissolves 14.52 grams of aspirin, C9H304 (180.1 g/mol), in 156.5 grams of diethyl ether. Use the table of boiling and freezing point constants to answer the questions below.
Solvent
Formula
Kb (°C/m) Kf (°C/m)
Water
H20
0.512
1.86
Ethanol
CH3CH2OH
1.22
1.99
Chloroform
CHC13
3.67
Benzene
C6H6
2.53
5.12
Diethyl ether CH;CH2OCH2CH3
2.02
The molality of the solution is
m.
The boiling point of the solution is
°C.

The boiling point of diethyl ether CH3CH2OCH2CH3 is 34.50°C at 1 atmosphere. A nonvolatile, nonelectrolyte that dissolves in diethyl ether is estrogen (estradiol).
How many grams of estrogen, C18H2402 (272.4 g/mol), must be dissolved in 250.0 grams of diethyl ether to raise the boiling point by 0.450 °C ? Refer to the table for the necessary boiling or freezing point constant.
Solvent
Formula
Kb (°C/m) Kf (°C/m)
Water
H20
0.512
1.86
Ethanol
CH3CH2OH
1.22
1.99
Chloroform
CHC13
3.67
Benzene
C6H6
2.53
5.12
Diethyl ether CH3CH2OCH2CH3
2.02
g estrogen.

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