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Assuming 100% dissociation, calculate the freezing point (T;) and boiling point (T, ) of 2.04 m K,PO,(aq). Colligative constants can be found in the chempendix. Tf = ɔ. T, =

Assuming 100% dissociation, calculate the freezing point (T;) and boiling point (T, ) of 2.04 m K,PO,(aq). Colligative constants can be found in the chempendix. Tf = ɔ. T, =

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
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Assuming 100% dissociation, calculate the freezing point (T) and boiling point (T,) of 2.04 m K,PO,(aq). Colligative constants can be found in the chempendix. Tf = °C T =
Transcribed Image Text:Assuming 100% dissociation, calculate the freezing point (T) and boiling point (T,) of 2.04 m K,PO,(aq). Colligative constants can be found in the chempendix. Tf = °C T =
Colligative Constants Constants for freezing-point depression and boiling-point elevation calculations at 1 atm: K( value* Normal freezing K value Normal boiling (°C/ m ) Solvent Formula (°C/ m) point ( °C) point ( °C) H20 C 6 H 6 cyclohexane C6 H 12 water 1.86 0.00 0.512 100.00 benzene 5.12 5.49 2,53 80.1 20.8 6.59 2.92 80.7 ethanol C2 H60 1.99 -117.3 1.22 78.4 carbon CCI 4 29.8 -22.9 5.03 76.8 tetrachloride camphor C 10 H 16 0 37.8 176 *When using positive Kf values, assume that ATf is the absolute value of the change in temperature. If you would prefer to define AT; as "final minus initial" temperature, then AT; will be negative and so you must use negative Ke values. Either way, the freezing point of the solution should be lower than that of the pure solvent.
Transcribed Image Text:Colligative Constants Constants for freezing-point depression and boiling-point elevation calculations at 1 atm: K( value* Normal freezing K value Normal boiling (°C/ m ) Solvent Formula (°C/ m) point ( °C) point ( °C) H20 C 6 H 6 cyclohexane C6 H 12 water 1.86 0.00 0.512 100.00 benzene 5.12 5.49 2,53 80.1 20.8 6.59 2.92 80.7 ethanol C2 H60 1.99 -117.3 1.22 78.4 carbon CCI 4 29.8 -22.9 5.03 76.8 tetrachloride camphor C 10 H 16 0 37.8 176 *When using positive Kf values, assume that ATf is the absolute value of the change in temperature. If you would prefer to define AT; as "final minus initial" temperature, then AT; will be negative and so you must use negative Ke values. Either way, the freezing point of the solution should be lower than that of the pure solvent.
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