The solubility of oxygen in lakes high in the Rocky Mountains is affected by the altitude. If the solubility of O2 from the air is 2.67 * 10-4 M at sea level and 25°C, what is the solubility of O2 at an elevation of 12,000 ft where the atmospheric pressure is 0.657 atm? Assume the temperature is 25°C, and that the mole fraction of O2 in air is 0.209 at both 12,000 ft and at sea level.

A) 1.75 * 10-4 M B) 2.67 * 10-4 M C) 3.66 * 10-5 M D) 4.06 * 10-4 M E) None of the above. A) 1.75 * 10-4 M B) 2.67 * 10-4 M C) 3.66 * 10-5 M D) 4.06 * 10-4 M E) None of the above.

Pure benzene, C6H6, freezes at 5.5° and boils at 80.1°C. What is the boiling point of a solution consisting of cyclohexane (C6H12)dissolved in benzene if the freezing point of this solution is 0.0°C? (For benzene, Kf = 5.12 °C/m, Kb = 2.53 °C/m; for cyclohexane, Kf = 20.0 °C/m, Kb = 2.79°C/m)

A) 82.8°C B) 91.2°C C) 80.9°C D) 77.4°C E) 83.1°C A) 82.8°C B) 91.2°C C) 80.9°C D) 77.4°C E) 83.1°C

The osmotic pressure of a 0.010 M MgSO4 solution at 25°C is 0.318 atm. Calculate i, the van't Hoff factor, for this MgSO4 solution.

A) 0.013 B) 1.3 C) 1.5 D) 2.0 E) 76.8 A) 0.013 B) 1.3 C) 1.5 D) 2.0 E) 76.8

What is the percent CdSO4 by mass in a 1.0 molal aqueous CdSO4 solution?

A) 1.00 * 10-3 % B) 0.100 % C) 17.2 % D) 20.8 % E) 24.4 % A) 1.00 * 10-3 % B) 0.100 % C) 17.2 % D) 20.8 % E) 24.4 %

Calculate the molality of 6.0 M H2SO4 solution. The density of the solution is 1.34 g/mL.

A) 4.48 m B) 7.98 m C) 8.10 m D) 8.43 m E) 10.2 m A) 4.48 m B) 7.98 m C) 8.10 m D) 8.43 m E) 10.2 m

A) pure solvent diffuses through a membrane but solutes do not. B) pure solutes diffuse through a membrane but solvent does not. C) pure solvent and a solution both diffuse at the same time through a membrane. D) gases diffuse through a membrane into a solution and build up pressure. A) pure solvent diffuses through a membrane but solutes do not. B) pure solutes diffuse through a membrane but solvent does not. C) pure solvent and a solution both diffuse at the same time through a membrane. D) gases diffuse through a membrane into a solution and build up pressure.

Calculate the freezing point of a solution made from 22.0 g of octane (C8H18)dissolved in 148.0 g of benzene. Benzene freezes at 5.50°C and its Kf value is 5.12°C/m.

A) -1.16°C B) 0.98°C C) 6.66°C D) 12.2°C E) 5.49°C A) -1.16°C B) 0.98°C C) 6.66°C D) 12.2°C E) 5.49°C

Oxygen gas makes up 21 % of the atmosphere by volume.What is the solubility of O2(g)in water at 25°C if the atmospheric pressure is 741 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 * 10-3 mol/L·atm.

A) 2.7 * 10-4 M B) 1.3 * 10-3 M C) 6.2 * 10-3 M D) 9.6 * 10-3 M E) 0.96 M A) 2.7 * 10-4 M B) 1.3 * 10-3 M C) 6.2 * 10-3 M D) 9.6 * 10-3 M E) 0.96 M

Exam 12: Physical Properties of Solutions

The solubility of oxygen in lakes high in the Rocky Mountains is affected by the altitude. If the solubility of O₂ from the air is 2.67 * 10^-4 M at sea level and 25°C, what is the solubility of O₂ at an elevation of 12,000 ft where the atmospheric pressure is 0.657 atm? Assume the temperature is 25°C, and that the mole fraction of O₂ in air is 0.209 at both 12,000 ft and at sea level.

(Multiple Choice)

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Question 61

Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 * 10² g of H₂O. [K_f of water is 1.86°C/m.]

(Multiple Choice)

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Question 62

Pure benzene, C₆H₆, freezes at 5.5° and boils at 80.1°C. What is the boiling point of a solution consisting of cyclohexane (C₆H₁₂)dissolved in benzene if the freezing point of this solution is 0.0°C? (For benzene, K_f = 5.12 °C/m, K_b = 2.53 °C/m; for cyclohexane, K_f = 20.0 °C/m, K_b = 2.79°C/m)

(Multiple Choice)

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Question 63

The osmotic pressure of a 0.010 M MgSO₄ solution at 25°C is 0.318 atm. Calculate i, the van't Hoff factor, for this MgSO₄ solution.

(Multiple Choice)

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Question 64

The solubility of oxygen in water is about 4.5 * 10^-2 g/L.The water portion of an adult's total blood supply is about 5 liters.How many grams of oxygen could dissolve in 5 liters of water?

(Short Answer)

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Question 65

The concentration of nitrogen in water at 25°C was determined to be 7.2 10^-6 M.Calculate the partial pressure of nitrogen at the surface of the water in mmHg. The Henry's law constant for nitrogen gas at 25°C is 6.8 10^-4 mol/L·atm?

(Short Answer)

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Question 66

How many grams of propanol (C₃H₇OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

(Short Answer)

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Question 67

What is the percent CdSO₄ by mass in a 1.0 molal aqueous CdSO₄solution?

(Multiple Choice)

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Question 68

Calculate the molality of 6.0 M H₂SO₄ solution. The density of the solution is 1.34 g/mL.

(Multiple Choice)

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Question 69

A 100.mL sample of water is taken from the Great Salt Lake, and the water is allowed to evaporate.The salts that remain (mostly NaCl)have a mass of 31.9 g Calculate the original concentration of NaCl, in g per liter, in each water sample.

(Short Answer)

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Question 70

During osmosis

(Multiple Choice)

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Question 71

Determine the mass percent HCl in a 1.2 M solution of hydrochloric acid with a density of 1.019 g/mL?

(Multiple Choice)

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Question 72

A solution is prepared by adding 6.24 g of benzene (C₆H₆, 78.11 g/mol)to 80.74 g of cyclohexane (C₆H₁₂, 84.16 g/mol).Calculate the mole fraction and molality of benzene in this solution.

(Short Answer)

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Question 73

Calculate the freezing point of a solution made from 22.0 g of octane (C₈H₁₈)dissolved in 148.0 g of benzene. Benzene freezes at 5.50°C and its K_f value is 5.12°C/m.

(Multiple Choice)

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Question 74

Which of the following aqueous solutions has the lowest freezing point?

(Multiple Choice)

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Question 75

Oxygen gas makes up 21 % of the atmosphere by volume.What is the solubility of O₂(g)in water at 25°C if the atmospheric pressure is 741 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 * 10^-³ mol/L·atm.

(Multiple Choice)

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Question 76

When 12.1 g of the sugar sucrose (a nonelectrolyte)are dissolved in exactly 800 g of water, the solution has a freezing point of -0.082°C. What is the molar mass of sucrose? K_f of water is 1.86°C/m.

(Multiple Choice)

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Question 77

An organic compound was prepared and purified by chromatography.A conductivity measurement showed the compound to be a nonelectrolyte.Elemental analysis gave an empirical formula of CH₃O.A 0.127 g sample of the compound was dissolved in water and diluted to 100.0 mL, and the osmotic pressure of that solution was determined to 0.492 atm at 20°C. Determine the molar mass and molecular formula of the compound.(R = 0.0821 L.atm/K.mol)

(Short Answer)

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Question 78

The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7 * 10^-4 mol/L. What is the value of the Henry's Law constant in mol/L·atm?

(Multiple Choice)

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Question 79

To interconvert the concentration units molality (m)and mass percent, you must also know the density of the solution.

(True/False)

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Question 80

Showing 61 - 80 of 109

Exam 12: Physical Properties of Solutions

Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 * 102 g of H2O. [Kf of water is 1.86°C/m.]

The osmotic pressure of a 0.010 M MgSO4 solution at 25°C is 0.318 atm. Calculate i, the van't Hoff factor, for this MgSO4 solution.

The solubility of oxygen in water is about 4.5 * 10-2 g/L.The water portion of an adult's total blood supply is about 5 liters.How many grams of oxygen could dissolve in 5 liters of water?

The concentration of nitrogen in water at 25°C was determined to be 7.2 *10-6 M.Calculate the partial pressure of nitrogen at the surface of the water in mmHg. The Henry's law constant for nitrogen gas at 25°C is 6.8 *10-4 mol/L·atm?

How many grams of propanol (C3H7OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

What is the percent CdSO4 by mass in a 1.0 molal aqueous CdSO4 solution?

Calculate the molality of 6.0 M H2SO4 solution. The density of the solution is 1.34 g/mL.

A 100.mL sample of water is taken from the Great Salt Lake, and the water is allowed to evaporate.The salts that remain (mostly NaCl)have a mass of 31.9 g Calculate the original concentration of NaCl, in g per liter, in each water sample.

During osmosis

Determine the mass percent HCl in a 1.2 M solution of hydrochloric acid with a density of 1.019 g/mL?

A solution is prepared by adding 6.24 g of benzene (C6H6, 78.11 g/mol)to 80.74 g of cyclohexane (C6H12, 84.16 g/mol).Calculate the mole fraction and molality of benzene in this solution.

Calculate the freezing point of a solution made from 22.0 g of octane (C8H18)dissolved in 148.0 g of benzene. Benzene freezes at 5.50°C and its Kf value is 5.12°C/m.

Which of the following aqueous solutions has the lowest freezing point?

Oxygen gas makes up 21 % of the atmosphere by volume.What is the solubility of O2(g)in water at 25°C if the atmospheric pressure is 741 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 * 10-3 mol/L·atm.

When 12.1 g of the sugar sucrose (a nonelectrolyte)are dissolved in exactly 800 g of water, the solution has a freezing point of -0.082°C. What is the molar mass of sucrose? Kf of water is 1.86°C/m.

The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7 * 10-4 mol/L. What is the value of the Henry's Law constant in mol/L·atm?

To interconvert the concentration units molality (m)and mass percent, you must also know the density of the solution.

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Calculate the approximate freezing point of a solution made from 21.0 g NaCl and 1.00 * 10² g of H₂O. [K_f of water is 1.86°C/m.]

The osmotic pressure of a 0.010 M MgSO₄ solution at 25°C is 0.318 atm. Calculate i, the van't Hoff factor, for this MgSO₄ solution.

The solubility of oxygen in water is about 4.5 * 10^-2 g/L.The water portion of an adult's total blood supply is about 5 liters.How many grams of oxygen could dissolve in 5 liters of water?

The concentration of nitrogen in water at 25°C was determined to be 7.2 10^-6 M.Calculate the partial pressure of nitrogen at the surface of the water in mmHg. The Henry's law constant for nitrogen gas at 25°C is 6.8 10^-4 mol/L·atm?

How many grams of propanol (C₃H₇OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

What is the percent CdSO₄ by mass in a 1.0 molal aqueous CdSO₄solution?

Calculate the molality of 6.0 M H₂SO₄ solution. The density of the solution is 1.34 g/mL.

A solution is prepared by adding 6.24 g of benzene (C₆H₆, 78.11 g/mol)to 80.74 g of cyclohexane (C₆H₁₂, 84.16 g/mol).Calculate the mole fraction and molality of benzene in this solution.

Calculate the freezing point of a solution made from 22.0 g of octane (C₈H₁₈)dissolved in 148.0 g of benzene. Benzene freezes at 5.50°C and its K_f value is 5.12°C/m.

Oxygen gas makes up 21 % of the atmosphere by volume.What is the solubility of O₂(g)in water at 25°C if the atmospheric pressure is 741 mmHg? The Henry's law constant for oxygen gas at 25°C is 1.3 * 10^-³ mol/L·atm.

When 12.1 g of the sugar sucrose (a nonelectrolyte)are dissolved in exactly 800 g of water, the solution has a freezing point of -0.082°C. What is the molar mass of sucrose? K_f of water is 1.86°C/m.

The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7 * 10^-4 mol/L. What is the value of the Henry's Law constant in mol/L·atm?