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If a 0.890 m aqueous solution freezes at -3.00 °C, what is the van't Hoff factor, i, of the solute? Consult the table of Kf values. i = Constants for freezing-point depression and boiling-point elevation calculations at 1 atm: Kf value* Normal freezing K value Normal boiling (°C/ m) Solvent Formula (°C/ m) point ( °C) point ( °C) H20 C6H6 water 1.86 0.00 0.512 100.00 benzene 5.12 5.49 2.53 80.1 cyclohexane C 6 H 12 C2H60 20.8 6.59 2.92 80.7 ethanol 1.99 |-117.3 1.22 78.4 carbon tetrachloride CCI 4 camphor 29.8 -22.9 5.03 76.8 С 10 Н 16 0 37.8 176

If a 0.890 m aqueous solution freezes at -3.00 °C, what is the van't Hoff factor, i, of the solute? Consult the table of Kf values. i = Constants for freezing-point depression and boiling-point elevation calculations at 1 atm: Kf value* Normal freezing K value Normal boiling (°C/ m) Solvent Formula (°C/ m) point ( °C) point ( °C) H20 C6H6 water 1.86 0.00 0.512 100.00 benzene 5.12 5.49 2.53 80.1 cyclohexane C 6 H 12 C2H60 20.8 6.59 2.92 80.7 ethanol 1.99 |-117.3 1.22 78.4 carbon tetrachloride CCI 4 camphor 29.8 -22.9 5.03 76.8 С 10 Н 16 0 37.8 176

Chemistry
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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If a 0.890 m aqueous solution freezes at -3.00 °C, what is the van't Hoff factor, i, of the solute? Consult the table of Kf values. i = Constants for freezing-point depression and boiling-point elevation calculations at 1 atm: Kf value* Normal freezing K value Normal boiling (°C/ m ) Solvent Formula (°C/ m) point ( °C) point ( °C) H20 1.86 0.00 0.512 100.00 water benzene C6H6 5.12 5.49 2.53 80.1 сyclohexane C 6 Н12 C2H60 20.8 6.59 2.92 80.7 ethanol 1.99 |-117.3 1.22 78.4 carbon CCI 4 5.03 29.8 -22.9 76.8 tetrachloride camphor С 10 Н 16 0 37.8 176
Transcribed Image Text:If a 0.890 m aqueous solution freezes at -3.00 °C, what is the van't Hoff factor, i, of the solute? Consult the table of Kf values. i = Constants for freezing-point depression and boiling-point elevation calculations at 1 atm: Kf value* Normal freezing K value Normal boiling (°C/ m ) Solvent Formula (°C/ m) point ( °C) point ( °C) H20 1.86 0.00 0.512 100.00 water benzene C6H6 5.12 5.49 2.53 80.1 сyclohexane C 6 Н12 C2H60 20.8 6.59 2.92 80.7 ethanol 1.99 |-117.3 1.22 78.4 carbon CCI 4 5.03 29.8 -22.9 76.8 tetrachloride camphor С 10 Н 16 0 37.8 176
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