Quinine is a natural product extracted from the bark of the cinchona tree, which is native to South America. Quinine is used asan 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. Lookup the freezing point and Kf constant for cyclohexane in the Colligative Constants table.Calculate the molar mass of quinine.molar mass:g/mol Colligative ConstantsConstants for freezing-point depression and boiling-point elevation calculations at 1 atm:Kf value* Normal freezing Kb value Normal boiling(°C/ m)SolventFormula(°C/ m)point ( °C)point ( °C)H201.860.000.512100.00waterbenzeneC6H 65.125.492.5380.1cyclohexane C 6 H 12ethanol20.86.592.9280.7C2 H601.99-117.31.2278.4carbontetrachlorideCCI 429.8-22.95.0376.8camphorС 10 Н 160 37.8176*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 puresolvent.

Molar Mass of quinine = 324g/mol.

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:

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter7: Solutions And Colloids

Section: Chapter Questions

Problem 7.87E

See similar textbooks

Similar questions

Calculate the molality of a solution made by dissolving 115.0 g ethylene glycol, HOCH2CH2OH, in 500. mL water. The density of water at this temperature is 0.978 g/mL. Calculate the molarity of the solution.
Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water, by calculating the freezing point depression of solutions containing 200. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is. it absorbs moisture from the air to give a solution and begin the process. A disadvantage is that this compound is more costly.)
The dispersed phase of a certain colloidal dispersion consists of spheres of diameter 1.0 102 nm. (a) What are the volume (V=43r2) and surface area (A = r2) of each sphere? (b) How many spheres are required to give a total volume of 1.0 cm3? What is the total surface area of these spheres in square meters?
Calcium chloride, CaCl2, has been used to melt ice from roadways. Given that the saturated solution is 32% CaCl2 by mass, estimate the freezing point.