14. Solutions

Freezing Point Depression

14. Solutions

Freezing Point Depression

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Freezing Point Depression Concept 1

Freezing Point Depression Example 1

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13 - Solutions and Colligative Properties

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13 - Solutions and Colligative Properties

Colligative Properties Explained

Boiling point elevation and freezing point depression | Chemistry | Khan Academy

Colligative Properties - Boiling Point Elevation, Freezing Point Depression & Osmotic Pressure

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Molality and Colligative Properties

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Practice this topic

Multiple Choice

How many moles of ethylene glycol, C₂H₆O₂, must be added to 1,000 g of water to form a solution that has a freezing point of –10ºC?

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Multiple Choice

An ethylene glycol solution contains 28.3 g of ethylene glycol, C₂H₆O₂ in 97.2 mL of water. Calculate the freezing point of the solution. The density of water 1.00 g/mL.

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Multiple Choice

When 825 g of an unknown is dissolved in 3.45 L of water, the freezing point of the solution is decreased by 2.89°C. Assuming that the unknown compound is a non-electrolyte, calculate its molar mass.

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Multiple Choice

Calculate the mass of KCl used to prepare a solution in 3.00 L of water with a freezing point of –1.20 °C. Assume that the density of water = 1.00 g/mL.

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Textbook Question

How many kilograms of ethylene glycol (automobile anti- freeze, C2H6O2) dissolved in 3.55 kg of water are needed to lower the freezing point of water in an automobile radiator to - 22.0 °C? The molal freezing point depression constant for water is Kf = 1.86 1°C kg2>mol. (LO 13.13) (a) 0.865 kg (b) 0.0420 kg (c) 9.01 kg (d) 2.61 kg

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Textbook Question

Using data from Table 13.3, calculate the freezing and boiling points of each of the following solutions: (b) 0.240 mol of naphthalene 1C10H82 in 2.45 mol of chloroform, g glucose 1C6H12O62 in 188 g of water.

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Textbook Question

Using data from Table 13.3, calculate the freezing and boiling points of each of the following solutions: (b) 20.0 g of decane, C10H22, in 50.0 g CHCl3;

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Textbook Question

What is the freezing point of an aqueous solution that boils at 105.0 °C?

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Textbook Question

A glucose solution contains 55.8 g of glucose (C6H12O6) in 455 g of water. Determine the freezing point and boiling point of the solution.

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Textbook Question

Lauryl alcohol is obtained from coconut oil and is used to make detergents. A solution of 5.00 g of lauryl alcohol in 0.100 kg of benzene freezes at 4.1 °C. What is the molar mass of lauryl alcohol from this data?

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Textbook Question

Calculate the freezing point and boiling point of each aqueous solution, assuming complete dissociation of the solute. c. 5.5% NaNO3 by mass (in water)

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Textbook Question

Calculate the freezing point and boiling point of each aqueous solution, assuming complete dissociation of the solute. b. 21.5 g of CuCl2 in 4.50 * 102 g water

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Textbook Question

What mass of salt (NaCl) should you add to 1.00 L of water in an ice cream maker to make a solution that freezes at -10.0 °C? Assume complete dissociation of the NaCl and density of 1.00 g>mL for water.

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Textbook Question

Use the van't Hoff factors in Table 13.9 to calculate each colligative property: a. the melting point of a 0.100 m iron(III) chloride solution

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Textbook Question

When 9.12 g of HCl was dissolved in 190 g of water, the freezing point of the solution was - 4.65 °C. What is the value of the van't Hoff factor for HCl?

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Textbook Question

A small cube of lithium 1density = 0.535 g/cm32 measuring 1.0 mm on each edge is added to 0.500 L of water. The following reaction occurs: 2 Li1s2 + 2 H2O1l2 ¡ 2 LiOH1aq2 + H21g2 What is the freezing point of the resulting solution, assuming that the reaction goes to completion?

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Textbook Question

When HNO2 is dissolved in water, it partially dissociates according to the equation HNO2ΔH+ + NO2- . A solution is prepared that contains 7.050 g of HNO2 in 1.000 kg of water. Its freezing point is -0.2929 °C. Calculate the fraction of HNO2 that has dissociated.

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Textbook Question

A solution prepared by dissolving 3.00 g of ascorbic acid (vitamin C, C6H8O6) in 50.0 g of acetic acid has a freez- ing point that is depressed by ΔT = 1.33 °C below that ofpure acetic acid. What is the value of the molal freezing- point-depression constant for acetic acid?

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Textbook Question

A solution contains 10.05 g of unknown compound dissolved in 50.0 mL of water. (Assume a density of 1.00 g>mL for water.) The freezing point of the solution is -3.16 °C. The mass percent composition of the compound is 60.97% C, 11.94% H, and the rest is O. What is the molecular formula of the compound?

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Textbook Question

124. A 50.0-mL solution is initially 1.55% MgCl2 by mass and has a density of 1.05 g>mL. What is the freezing point of the solution after you add an additional 1.35 g MgCl2? (Use i = 2.5 for MgCl2.)

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Textbook Question

The van't Hoff factor for CaCl2 is 2.71. What is its mass % in an aqueous solution that has Tf = - 1.14 °C?

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Textbook Question

Elemental analysis of b@carotene, a dietary source of vitamin A, shows that it contains 10.51% H and 89.49% C. Dissolving 0.0250 g of b@carotene in 1.50 g of camphor gives a freezing- point depression of 1.17 °C. What are the molecular weight and formula of b@carotene? [Kf for camphor is 37.7 1°C kg2>mol.]

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Textbook Question

Treatment of 1.385 g of an unknown metal M with an excess of aqueous HCl evolved a gas that was found to have a volume of 382.6 mL at 20.0 °C and 755 mm Hg pressure. Heating the reaction mixture to evaporate the water and remaining HCl then gave a white crystalline compound, MClx. After dis- solving the compound in 25.0 g of water, the melting point of the resulting solution was - 3.53 °C. (e) What are the formula and molecular weight of MClx?

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Textbook Question

Treatment of 1.385 g of an unknown metal M with an excess of aqueous HCl evolved a gas that was found to have a volume of 382.6 mL at 20.0 °C and 755 mm Hg pressure. Heating the reaction mixture to evaporate the water and remaining HCl then gave a white crystalline compound, MClx. After dis- solving the compound in 25.0 g of water, the melting point of the resulting solution was - 3.53 °C. (c) What is the molality of particles (ions) in the solution of MClx?

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Textbook Question

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Textbook Question

A solution prepared by dissolving 100.0 g of a mixture of sugar 1C12H22O112 and table salt (NaCl) in 500.0 g of water has a freezing point of - 2.25 °C. What is the mass of each individual solute? Assume that NaCl is completely dissociated.

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Open Question

Determine the freezing point depression of a solution that contains 30.7 g glycerin (C₃H₈O₃, molar mass = 92.09 g/mol) in 376 ml of water. Some possibly useful constants for water are k_f = 1.86°C/m and k_b = 0.512°C/m.

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Open Question

Determine the freezing point of a solution that contains 78.8 g of naphthalene (C₁₀H₈, molar mass = 128.16 g/mol) dissolved in 722 ml of benzene (d = 0.877 g/ml). pure benzene has a melting point of 5.50 °C and a freezing point depression constant of 4.90 °C/m.

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Open Question

What mass of glucose (C₆H₁₂O₆) should be dissolved in 12.0 kg of water to obtain a solution with a freezing point of -5.8^∘C?

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Open Question

Calculate the freezing point of a solution containing 1.25g of benzene in 100g of chloroform

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