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 2.04 g of quinine is dissolved in 25.0 g of cyclohexane, the freezing point of the solution is lowered by 5.23 °C. Look upthe freezing point and K+ constant for cyclohexane in the Colligative Constants table.Calculate the molar mass of quinine.molar mass:315.42Incorrect Answerg/mol

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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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A solution is made by dissolving 0.540 mol of nonelectrolyte solute in 757 g of benzene. Calculate the freezing point, Tf, and boiling point, Tú, of the solution. Constants can be found in the table of colligative constants. Tf = Tb = °C °C
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Biphenyl, C1,H10, is a nonvolatile, nonionizing solute that soluble in benzene, C,H6. At 25 °C, the vapor pressure of pure benzene is 100.84 Torr. What is the vapor pressure of a solution made from dissolving 17.8 g of biphenyl in 30.3 g of benzene? Psolution Torr II
1. Suppose that you add 27.5 g of an unknown molecular compound to 0.250 kg of benzene, which has a Kf of 5.12 oC/m. With the added solute, you find that there is a freezing point depression of 3.58 oC compared to pure benzene. What is the molar mass (in g/mol) of the unknown compound? 2. What is the freezing point (in degrees Celcius) of 3.70 kg of water if it contains 187.4 g of CaBr2? The freezing point depression constant for water is 1.86 oC/m and the molar mass of CaBr2 is 199.89 g/mol. 3. What mass, in grams, of NaCl needs to be added to 1.6 kg of water in order to create a solution with a freezing point of -5.6 °C? The freezing point depression constant of water is 1.86 ºC/m.
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 0.927 g of quinine is dissolved in 25.0 g of cyclohexane, the freezing point of the solution is lowered by 2.38 °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
Suppose a group of students tell you that they added solid sodium chloride NaCls to 35 mL of deionized water and they did not record how many grams of NaCl they added but they got a freezing point depression of 1.25°C. Calculate how many grams of NaCl the students added. The pure freezing point of water is 0.00°C and the freezing point depression constant (K) of water is 1.858 °C/m. Remember that NaCl is a solid salt and an ionic compound therefore it contributes a negligible amount to the overall additive volume and keep track of its van't Hoff factor. The density of water at 20°C is 0.9982 g/mL.
The boiling point of 6.05 g of a pure solvent is measured to be 48.000 ºC. When 20.00 g of an unknown solute (assume the van 't Hoff factor = 1.0000 for the solute and Kb = 4.85 °C/m for the solvent) is added to the solvent the boiling point is measured to be 55.500 ºC . What is the molality ( in m) of the solution?(give your answer to two decimal places)

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