Boiling Point Elevation/Freezing Point Depression AT = m K where, for freezing point depression: AT = T(pure solvent) - T(solution) and for boiling point elevation: AT 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. Solvent Kb(°C/m) Kf(°C / m) Water 0.512 1.86 Ethanol CH3CH₂OH 1.22 1.99 Chloroform CHCI 3 3.67 Benzene C6H6 2.53 Diethyl ether CH3CH₂OCH₂CH3 2.02 Formula H₂O 5.12
Boiling Point Elevation/Freezing Point Depression AT = m K where, for freezing point depression: AT = T(pure solvent) - T(solution) and for boiling point elevation: AT 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. Solvent Kb(°C/m) Kf(°C / m) Water 0.512 1.86 Ethanol CH3CH₂OH 1.22 1.99 Chloroform CHCI 3 3.67 Benzene C6H6 2.53 Diethyl ether CH3CH₂OCH₂CH3 2.02 Formula H₂O 5.12
Chemistry
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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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