Pure benzene, C6H6, freezes at 5.5$\circ$C and boils at 80.1$\circ$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$\circ$C (For benzene, Kf = 5.12 $\circ$C/m, Kb = 2.53 $\circ$C/m; for cyclohexane, Kf = 20.0 $\circ$C/m, Kb = 2.79$\circ$C/m)

A) 77.4$\circ$C B) 80.9$\circ$C C) 82.8$\circ$C D) 83.1$\circ$C E) 91.2$\circ$C A) 77.4$\circ$C B) 80.9$\circ$C C) 82.8$\circ$C D) 83.1$\circ$C E) 91.2$\circ$C

In how many grams of water should 25.31 g of potassium nitrate (KNO3) be dissolved to prepare a 0.1982 m solution

A) 250.0 g B) 792.0 g C) 1000. g D) 1,263 g E) 7,917 g A) 250.0 g B) 792.0 g C) 1000. g D) 1,263 g E) 7,917 g

What is the mole fraction of sodium phosphate in a 0.142 M Na3PO4(aq) solution that has a density of 1.015 g/mL

A) 0.00157 B) 0.00257 C) 0.00357 D) 0.00457 E) None of the above A) 0.00157 B) 0.00257 C) 0.00357 D) 0.00457 E) None of the above

What is the boiling point of a solution of 12.0 g of urea (CH4N2O) in 165.0 g of water (Kb (H2O) = 0.52 $\circ$C/m)

A) 99.4$\circ$C B) 100.0 $\circ$C C) 100.6$\circ$C D) 106.2$\circ$C E) 108.4$\circ$C A) 99.4$\circ$C B) 100.0 $\circ$C C) 100.6$\circ$C D) 106.2$\circ$C E) 108.4$\circ$C

What is the osmotic pressure of a solution that contains 13.7 g of propyl alcohol (C3H7OH) dissolved in enough water to make 500. mL of solution at 27$\circ$C

A) 0.0100 atm B) 0.0140 atm C) 0.0370 atm D) 0.456 atm E) 11.2 atm A) 0.0100 atm B) 0.0140 atm C) 0.0370 atm D) 0.456 atm E) 11.2 atm

What is the mass % of K2SO4 in an aqueous solution that has a mole fraction of K2SO4, X = 0.350

A) 80.9% B) 83.9% C) 85.9% D) 87.9% E) None of the above A) 80.9% B) 83.9% C) 85.9% D) 87.9% E) None of the above

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C2H6O2) and 85.0 g H2O Kf of water is 1.86$\circ$C/m.

A) 17.6$\circ$C B) 1.50$\circ$C C) -1.50$\circ$C D) -17.6$\circ$C E) -176$\circ$C A) 17.6$\circ$C B) 1.50$\circ$C C) -1.50$\circ$C D) -17.6$\circ$C E) -176$\circ$C

A solution of chloroform, CHCl3, and acetone, (CH3)2CO, exhibits a negative deviation from Raoult's law. This result implies that

A) chloroform-chloroform interactions are stronger than chloroform-acetone interactions. B) chloroform-chloroform interactions are weaker than chloroform-acetone interactions. C) acetone-acetone interactions are stronger than chloroform-acetone interactions. D) acetone-acetone interactions are weaker than chloroform-acetone interactions. E) Both B and D. F) Both A and C. A) chloroform-chloroform interactions are stronger than chloroform-acetone interactions. B) chloroform-chloroform interactions are weaker than chloroform-acetone interactions. C) acetone-acetone interactions are stronger than chloroform-acetone interactions. D) acetone-acetone interactions are weaker than chloroform-acetone interactions. E) Both B and D. F) Both A and C.

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$\circ$C and its Kf value is 5.12$\circ$C/m.

A) -1.16$\circ$C B) 0.98$\circ$C C) 5.49$\circ$C D) 6.66$\circ$C E) 12.2$\circ$C A) -1.16$\circ$C B) 0.98$\circ$C C) 5.49$\circ$C D) 6.66$\circ$C E) 12.2$\circ$C

Exam 12: Physical Properties of Solutions

How many liters of ethylene glycol antifreeze (C₂H₆O₂) would you add to your car radiator containing 15.0 L of water if you needed to protect your engine to -17.8^$\circ$C (The density of ethylene glycol is 1.1 g/mL. For water, K_f = 1.86^$\circ$C/m.)

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Question 1

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How many grams of sucrose (C₁₂H₂₂O₁₁, 342.3 g/mol) would be needed to make 2.5 L of a solution with an osmotic pressure of 14 atm at 25^$\circ$C (R = 0.0821 L·atm/K·mol)

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Question 2

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Which of the following concentration units will change with temperature

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Question 3

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Pure benzene, C₆H₆, freezes at 5.5^$\circ$C and boils at 80.1^$\circ$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^$\circ$C (For benzene, K_f = 5.12 ^$\circ$C/m, K_b = 2.53 ^$\circ$C/m; for cyclohexane, K_f = 20.0 ^$\circ$C/m, K_b = 2.79^$\circ$C/m)

(Multiple Choice)

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Question 4

A 23.0% by mass LiCl solution is prepared in water. What is the mole fraction of the water

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Question 5

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.

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Question 6

In how many grams of water should 25.31 g of potassium nitrate (KNO₃) be dissolved to prepare a 0.1982 m solution

(Multiple Choice)

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Question 7

At 10^$\circ$C one volume of water dissolves 3.10 volumes of chlorine gas at 1.00 atm pressure. What is the Henry's Law constant in mol/L·atm

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Question 8

Plasma is the fluid portion of blood. The concentration of acetylsalicylic acid (aspirin, C₉H₈O₄, molar mass = 180. g/mol) in your plasma is found to be 2.99 * 10^-4 M after you take two tablets of aspirin. If the volume of your plasma is 5.85 L, what is the molality, m, of aspirin in your blood (Assume density of plasma is 1.00 g/mL.)

(Multiple Choice)

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Question 9

What is the mole fraction of sodium phosphate in a 0.142 M Na₃PO₄(aq) solution that has a density of 1.015 g/mL

(Multiple Choice)

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Question 10

What is the boiling point of a solution of 12.0 g of urea (CH₄N₂O) in 165.0 g of water (K_b (H₂O) = 0.52 ^$\circ$C/m)

(Multiple Choice)

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Question 11

What is the osmotic pressure of a solution that contains 13.7 g of propyl alcohol (C₃H₇OH) dissolved in enough water to make 500. mL of solution at 27^$\circ$C

(Multiple Choice)

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Question 12

What is the mass % of K₂SO₄ in an aqueous solution that has a mole fraction of K₂SO₄, X = 0.350

(Multiple Choice)

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Question 13

Using your knowledge of osmosis or osmotic pressure decide if the following statement is true or false: -Drinking salt water actually dehydrates our tissues.

(True/False)

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Question 14

The vapor pressure of a solution depends on the chemical nature of the solvent.

(True/False)

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Question 15

Which of the following liquids would make a good solvent for iodine, I₂

(Multiple Choice)

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Question 16

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C₂H₆O₂) and 85.0 g H₂O K_f of water is 1.86^$\circ$C/m.

(Multiple Choice)

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Question 17

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

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Question 18

A solution of chloroform, CHCl₃, and acetone, (CH₃)₂CO, exhibits a negative deviation from Raoult's law. This result implies that

(Multiple Choice)

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Question 19

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^$\circ$C and its K_f value is 5.12^$\circ$C/m.

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Question 20

Showing 1 - 20 of 122

Exam 12: Physical Properties of Solutions

How many liters of ethylene glycol antifreeze (C2H6O2) would you add to your car radiator containing 15.0 L of water if you needed to protect your engine to -17.8 ∘\circ∘ C (The density of ethylene glycol is 1.1 g/mL. For water, Kf = 1.86 ∘\circ∘ C/m.)

How many grams of sucrose (C12H22O11, 342.3 g/mol) would be needed to make 2.5 L of a solution with an osmotic pressure of 14 atm at 25 ∘\circ∘ C (R = 0.0821 L·atm/K·mol)

Which of the following concentration units will change with temperature

A 23.0% by mass LiCl solution is prepared in water. What is the mole fraction of the water

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.

In how many grams of water should 25.31 g of potassium nitrate (KNO3) be dissolved to prepare a 0.1982 m solution

At 10 ∘\circ∘ C one volume of water dissolves 3.10 volumes of chlorine gas at 1.00 atm pressure. What is the Henry's Law constant in mol/L·atm

What is the mole fraction of sodium phosphate in a 0.142 M Na3PO4(aq) solution that has a density of 1.015 g/mL

What is the boiling point of a solution of 12.0 g of urea (CH4N2O) in 165.0 g of water (Kb (H2O) = 0.52 ∘\circ∘ C/m)

What is the osmotic pressure of a solution that contains 13.7 g of propyl alcohol (C3H7OH) dissolved in enough water to make 500. mL of solution at 27 ∘\circ∘ C

What is the mass % of K2SO4 in an aqueous solution that has a mole fraction of K2SO4, X = 0.350

Using your knowledge of osmosis or osmotic pressure decide if the following statement is true or false: -Drinking salt water actually dehydrates our tissues.

The vapor pressure of a solution depends on the chemical nature of the solvent.

Which of the following liquids would make a good solvent for iodine, I2

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C2H6O2) and 85.0 g H2O Kf of water is 1.86 ∘\circ∘ C/m.

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

A solution of chloroform, CHCl3, and acetone, (CH3)2CO, exhibits a negative deviation from Raoult's law. This result implies that

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 ∘\circ∘ C and its Kf value is 5.12 ∘\circ∘ C/m.

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How many liters of ethylene glycol antifreeze (C₂H₆O₂) would you add to your car radiator containing 15.0 L of water if you needed to protect your engine to -17.8^$\circ$C (The density of ethylene glycol is 1.1 g/mL. For water, K_f = 1.86^$\circ$C/m.)

How many grams of sucrose (C₁₂H₂₂O₁₁, 342.3 g/mol) would be needed to make 2.5 L of a solution with an osmotic pressure of 14 atm at 25^$\circ$C (R = 0.0821 L·atm/K·mol)

In how many grams of water should 25.31 g of potassium nitrate (KNO₃) be dissolved to prepare a 0.1982 m solution

At 10^$\circ$C one volume of water dissolves 3.10 volumes of chlorine gas at 1.00 atm pressure. What is the Henry's Law constant in mol/L·atm

What is the mole fraction of sodium phosphate in a 0.142 M Na₃PO₄(aq) solution that has a density of 1.015 g/mL

What is the boiling point of a solution of 12.0 g of urea (CH₄N₂O) in 165.0 g of water (K_b (H₂O) = 0.52 ^$\circ$C/m)

What is the osmotic pressure of a solution that contains 13.7 g of propyl alcohol (C₃H₇OH) dissolved in enough water to make 500. mL of solution at 27^$\circ$C

What is the mass % of K₂SO₄ in an aqueous solution that has a mole fraction of K₂SO₄, X = 0.350

Which of the following liquids would make a good solvent for iodine, I₂

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C₂H₆O₂) and 85.0 g H₂O K_f of water is 1.86^$\circ$C/m.

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

A solution of chloroform, CHCl₃, and acetone, (CH₃)₂CO, exhibits a negative deviation from Raoult's law. This result implies that

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^$\circ$C and its K_f value is 5.12^$\circ$C/m.