Consider an aqueous solution containing 1.0 g/L of a protein (molar mass = 6.9 x 10* g/mol) with a density of 1.0 g/cm. Calculate the freezing-point depression of this solution. Freezing-point depression = | Calculate the osmotic pressure at 25°C of this solution. Osmotic pressure = torr Considering your answers, which colligative property, freezing-point depression or osmotic pressure, would be better used to determine the molar masses of large molecules?

Consider an aqueous solution containing 1.0 g/L of a protein (molar mass = 6.9 x 10* g/mol) with a density of 1.0 g/cm. Calculate the freezing-point depression of this solution. Freezing-point depression = | Calculate the osmotic pressure at 25°C of this solution. Osmotic pressure = torr Considering your answers, which colligative property, freezing-point depression or osmotic pressure, would be better used to determine the molar masses of large molecules?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter10: Properties Of Solutions

Section: Chapter Questions

Problem 120CP: Plants that thrive in salt water must have internal solutions (inside the plant cells) that are...

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Consider two solutions, A and B, separated by an osmotic semipermeable membrane that allows only water to pass through, as shown in the following diagram. Based on each of the following identities for solutions A and B, indicate whether the liquid level in compartment A, with time, will increase, decrease, or not change. a. A = 1.0 M NaCl solution and B = 2.0 M NaCl solution b. A = 5.0%(m/v) glucose solution and B = 4.0%(m/v) glucose solution c. A = 2.0 M KCl solution and B = 2.0 M KNO3 solution d. A = 1.0 M glucose solution and B = 1.0 M NaCl solution
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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.)
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Plants that thrive in salt water must have internal solutions (inside the plant cells) that are isotonic with (have the same osmotic pressure as) the surrounding solution. A leaf of a saltwater plant is able to thrive in an aqueous salt solution (at 25C) that has a freezing point equal to 0.62lC. You would like to use this information to calculate the osmotic pressure of the solution in the cell. a. In order to use the freezing-point depression to calculate osmotic pressure, what assumption must you make (in addition to ideal behavior of the solutions, which we will assume)? b. Under what conditions is the assumption (in part a) reasonable? c. Solve for the osmotic pressure (at 25C) of the solution in the plant cell. d. The plant leaf is placed in an aqueous salt solution (at 25C) that has a boiling point of l02.0C. What will happen to the plant cells in the leaf?
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