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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 & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter15: Principles Of Chemical Reactivity: Equilibria
Section15.6: Disturbing A Chemical Equilibrium
Problem 2.1ACP: Freezing point depression is one means of determining the molar mass of a compound. The freezing...
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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: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
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.
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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