The freezing point of a substance is the temperature at which the solid and liquid forms can coexist indefinitely, at equilibrium. Under these conditions molecules pass between the 2 phases at equal rates because their escaping tendencies from the two phases are identical. Like the boiling point elevation, the freezing point of a solution is directly proportional to the molal concentration of the solution, that is, AT=Krm Where, ATr refers to the freezing point lowering, Kf, the freezing point depression constant, and m, the molality of the solution. Some of the Kf values are shown in Table 1. For water, Kf is 1.86 °C/m, therefore, any 1 m aqueous solution of nonvolatile solute or a 0.5 m aqueous solution of NaCI will freeze at 1.86 °C lower than pure water. EXERCISE: Problem Solving: Show your solution! 1. A solution containing a nonelectrolyte dissolved in water has a boiling point of 0.305 °C. Calculate the freezing point of the same solution.

The freezing point of a substance is the temperature at which the solid and liquid forms can coexist indefinitely, at equilibrium. Under these conditions molecules pass between the 2 phases at equal rates because their escaping tendencies from the two phases are identical. Like the boiling point elevation, the freezing point of a solution is directly proportional to the molal concentration of the solution, that is, AT=Krm Where, ATr refers to the freezing point lowering, Kf, the freezing point depression constant, and m, the molality of the solution. Some of the Kf values are shown in Table 1. For water, Kf is 1.86 °C/m, therefore, any 1 m aqueous solution of nonvolatile solute or a 0.5 m aqueous solution of NaCI will freeze at 1.86 °C lower than pure water. EXERCISE: Problem Solving: Show your solution! 1. A solution containing a nonelectrolyte dissolved in water has a boiling point of 0.305 °C. Calculate the freezing point of the same solution.

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...

See similar textbooks

Similar questions

Table sugar granules were dissolved in a glass of water. The solid sugar granules have no measurable vapor pressure, making water as the contributor to the entire vapor pressure of the resulting solution. If sugar was added to the glass of water until the water makes up a mole fraction of 0.75 in the solution, what is the vapor pressure of water in this solution? Given the following: vapor pressure of water at 25°C is 23.8 torr. A. 23.8 torr B. 5.95 torr C. 29.75 torr D. 17.9 torr
Please don't provide handwritten solution .....
Lithium chloride has a solubility of 45.80 g in 100. g of water at 25°C. Express this solubility in terms ofmass percent molality mole fraction
10.0 g of glucose is added to 300 g of water at room temperature. The vapor pressure of water at room temperature is 23.76 Torr . Calculate the vapor pressure (Torr) of the aqueous glucose solution.
Table sugar granules were dissolved in a glass of water. The solid sugar granules have no measurable vapor pressure, making water as the contributor to the entire vapor pressure of the resulting solution. If sugar was added to the glass of water until the water makes up a mole fraction of 0.75 in the solution, what is the vapor pressure of water in this solution? Given the following: vapor pressure of water at 25°C is 23.8 torr. A. 23.8 tor B. 5.95 torr C. 29.75 torr D. 17.9 torr What is the vapor pressure of the said solution if the vapor pressure of pure benzene is 100 torr at 26.1°C? A. 152.26 mmHg B. 88.00 mmHg C. 22.97 torr D. 78.12 torr A 0.25g of a certain substance is dissolved in 60g of water. The freezing point of the solution is - 0.050 °C. that the substance has a van't Hoff factor of 1 and is non-volatile, what is the molar mass of the substance? (Freezing point depression of water = - 1.86 °C/m) A. 0.00016 g/mol B. 156.25 g/mol C. 186.54 g/mol D. 1.86 g/mol
Ethanol has a Kb of 1.22 oC/m and usually boils at 78.4 oC. This means that the boiling point elevation for ethanol is give by the equation: BPE = 1.22 MT where MT is the total number of moles of solute particles per liter of solution How many moles of an nonionizing solute would need to be added to 47.32 mL of ethanol in order to raise the boiling point to 87.1 oC.
5.152g of Na2CO3(s) is added to 75.0mL of water at 21.20°C. When the dissolution is complete, the final temperature of the solution is measured at 25.00°C. The final volume of the solution is 75.8mL, and the density of water at 21.20°C is 0.99798g/mL. Identify the strongest intermolecular force present in Na2CO3(s): and in water:
Calculate the change in the chemical potential of liquid water and water vapor when the pressure is increased from 1.0 atm to 10 atm at 100°C. Discuss the effect of the pressure increase on the equilibrium between the liquid water and the water vapor. Assume that water vapor behaves perfectly and the density of water is 1 g/cm3.
The solubility of Ne in water at 25 °C is 2.1 × 10⁻⁴ M when the partial pressure of Ne is 0.20 atm. What is the value of the Henry's law constant for Ne?
At a certain temperature the vapor pressure of pure benzene and pure toluene are 380 torr and 130 torr, respectively. If the mole fraction of benzene is 0.48, what is the total vapor pressure.
The molality of a potassium fluoride solution is 3.75. Calculate the mole fraction of potassium fluoride in the solution
At a certain temperature, diethyl ether has a vapor pressure of 550.0 torr. When a sample of benzoic acid (a non-volatile compound) is dissolved in ether, the vapor pressure of the solution is 486 torr. What is the mole fraction of benzoic acid in the solution?