Quinine is a natural product extracted from the bark of the cinchona tree, which is native an antimalarial agent. When 1.90 g of quinine is dissolved in 25.0 g of cyclohexane, the freezing point of the so up the freezing point and Kf constant for cyclohexane in the Colligative Constants table. Calculate the molar mass of quinine. molar mass:
Quinine is a natural product extracted from the bark of the cinchona tree, which is native an antimalarial agent. When 1.90 g of quinine is dissolved in 25.0 g of cyclohexane, the freezing point of the so up the freezing point and Kf constant for cyclohexane in the Colligative Constants table. Calculate the molar mass of quinine. molar mass:
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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Transcribed Image Text:Quinine is a natural product extracted from the bark of the cinchona tree, which is native to South America. Quinine is used as
an antimalarial agent.
When 1.90 g of quinine is dissolved in 25.0 g of cyclohexane, the freezing point of the solution is lowered by 4.88 °C. Look
up the freezing point and Kf constant for cyclohexane in the Colligative Constants table.
Calculate the molar mass of quinine.
molar mass:
g/mol
Transcribed Image Text:Colligative Constants
Constants for freezing-point depression and boiling-point elevation calculations at 1 atm:
Kf value* Normal freezing Kb value Normal boiling
(°C/ m)
Solvent
Formula
(°C/ m)
point ( °C)
point ( °C)
H20
1.86
0.00
0.512
100.00
water
benzene
C6H 6
5.12
5.49
2.53
80.1
cyclohexane C 6 H 12
ethanol
20.8
6.59
2.92
80.7
C2 H60
1.99
-117.3
1.22
78.4
carbon
tetrachloride
CCI 4
29.8
-22.9
5.03
76.8
camphor
С 10 Н 160 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 ATfwill be negative and so you must use negative Kf values. Either way, the freezing point of the solution should be lower than that of the pure
solvent.
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