Calculate the boiling point of a 4.5 m solution of Na2SO4 in water (assume 100% dissociation, Kb (H2O) = 0.52 $\circ$C/m).

A) 93.0 $\circ$C B) 97.7 $\circ$C C) 102.3$\circ$C D) 104.7$\circ$C E) 107.0$\circ$C A) 93.0 $\circ$C B) 97.7 $\circ$C C) 102.3$\circ$C D) 104.7$\circ$C E) 107.0$\circ$C

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$\circ$C. Determine the molar mass of the compound. (R = 0.0821 L·atm/K·mol)

A) 32.1 g/mol B) 42.1 g/mol C) 52.1 g/mol D) 62.1 g/mol E) None of the above A) 32.1 g/mol B) 42.1 g/mol C) 52.1 g/mol D) 62.1 g/mol E) None of the above

What is the mass percent CH3OH of a 0.256 m CH3OH(aq) solution

A) 0.819 % B) 0.992 % C) 1.23 % D) 1.29 % E) 1.51 % A) 0.819 % B) 0.992 % C) 1.23 % D) 1.29 % E) 1.51 %

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.

Which response lists all the following pairs that are miscible liquids Pair #1: octane (C8H18) and water Pair #2: acetic acid (CH3COOH) and water Pair #3: octane (C8H18) and carbon tetrachloride(CCl4)

A) 1, 3 B) 1, 2 C) 3 D) 2 E) 2, 3 A) 1, 3 B) 1, 2 C) 3 D) 2 E) 2, 3

A 20.0 % by mass solution of phosphoric acid (H3PO4) in water has a density of 1.114 g/mL at 20$\circ$C. What is the molarity of this solution

A) 0.0114 M B) 0.0568 M C) 0.114 M D) 2.27 M E) 11.4 M A) 0.0114 M B) 0.0568 M C) 0.114 M D) 2.27 M E) 11.4 M

Exam 12: Physical Properties of Solutions

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, how many grams of aspirin are in your blood (Assume that the density of plasma is 1.00 g/mL.)

(Multiple Choice)

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Question 81

Which one of the following would be immiscible with water

(Multiple Choice)

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Question 82

What is the molarity of a solution that is 7.00% by mass magnesium sulfate and has a density of 1.071 g/mL

(Multiple Choice)

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Question 83

Calculate the boiling point of a 4.5 m solution of Na₂SO₄ in water (assume 100% dissociation, K_b (H₂O) = 0.52 ^$\circ$C/m).

(Multiple Choice)

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Question 84

Which of the following solutions has the largest molality of HCl

(Multiple Choice)

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Question 85

Using your knowledge of osmosis or osmotic pressure decide if the following statement is true or false: -In trees and plants water is drawn from the soil up into the branches and leaves through the process of diffusion, not osmosis.

(True/False)

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Question 86

If 14.2 g of Al(NO₃)₃ is dissolved in 655g of water, what is the boiling point of the solution (assume 100% dissociation, K_b (H₂O) = 0.52 ^$\circ$C/m)

(Multiple Choice)

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Question 87

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^$\circ$C. Determine the molar mass of the compound. (R = 0.0821 L·atm/K·mol)

(Multiple Choice)

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Question 88

An aqueous dextrose solution having a density of 1.04 g/cm³ freezes at -1.15^$\circ$C. Find the osmotic pressure of this solution at 25^$\circ$C. K_f of water is 1.86 ^$\circ$C/m; molecular mass of dextrose = 180.16 g/mol.

(Multiple Choice)

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Question 89

What is the mass percent CH₃OH of a 0.256 m CH₃OH(aq) solution

(Multiple Choice)

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Question 90

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C₁₂H₂₂O₁₁.

(Multiple Choice)

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Question 91

The solubility of nitrogen gas at 25^$\circ$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 92

In which of the following solvents would you expect KBr to be most soluble

(Multiple Choice)

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Question 93

A 100.-mL sample of water is taken from the Pacific Ocean, and the water is allowed to evaporate. The salts that remain (mostly NaCl) have a mass of 3.85 g. Calculate the original concentration of NaCl, in g per liter, in the water sample.

(Multiple Choice)

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Question 94

During osmosis

(Multiple Choice)

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Question 95

The solubility of gases in water always decreases with increasing temperature.

(True/False)

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Question 96

Which response lists all the following pairs that are miscible liquids Pair #1: octane (C₈H₁₈) and water Pair #2: acetic acid (CH₃COOH) and water Pair #3: octane (C₈H₁₈) and carbon tetrachloride(CCl₄)

(Multiple Choice)

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Question 97

A 20.0 % by mass solution of phosphoric acid (H₃PO₄) in water has a density of 1.114 g/mL at 20^$\circ$C. What is the molarity of this solution

(Multiple Choice)

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Question 98

The vapor pressure of water at 45.0 ^$\circ$C is 71.93 mmHg. Calculate the vapor pressure of a solution of 1.25m Al(ClO₃)₃ at this temperature (assume 100% dissociation).

(Multiple Choice)

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Question 99

When 12.1 g of the sugar sucrose (a nonelectrolyte) is dissolved in exactly 800.0 g of water, the solution has a freezing point of -0.082^$\circ$C. What is the molar mass of sucrose K_f of water is 1.86^$\circ$C/m.

(Multiple Choice)

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Question 100

Showing 81 - 100 of 122

Exam 12: Physical Properties of Solutions

Which one of the following would be immiscible with water

What is the molarity of a solution that is 7.00% by mass magnesium sulfate and has a density of 1.071 g/mL

Calculate the boiling point of a 4.5 m solution of Na2SO4 in water (assume 100% dissociation, Kb (H2O) = 0.52 ∘\circ∘ C/m).

Which of the following solutions has the largest molality of HCl

Using your knowledge of osmosis or osmotic pressure decide if the following statement is true or false: -In trees and plants water is drawn from the soil up into the branches and leaves through the process of diffusion, not osmosis.

If 14.2 g of Al(NO3)3 is dissolved in 655g of water, what is the boiling point of the solution (assume 100% dissociation, Kb (H2O) = 0.52 ∘\circ∘ C/m)

An aqueous dextrose solution having a density of 1.04 g/cm3 freezes at -1.15 ∘\circ∘ C. Find the osmotic pressure of this solution at 25 ∘\circ∘ C. Kf of water is 1.86 ∘\circ∘ C/m; molecular mass of dextrose = 180.16 g/mol.

What is the mass percent CH3OH of a 0.256 m CH3OH(aq) solution

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C12H22O11.

The solubility of nitrogen gas at 25 ∘\circ∘ 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

In which of the following solvents would you expect KBr to be most soluble

A 100.-mL sample of water is taken from the Pacific Ocean, and the water is allowed to evaporate. The salts that remain (mostly NaCl) have a mass of 3.85 g. Calculate the original concentration of NaCl, in g per liter, in the water sample.

During osmosis

The solubility of gases in water always decreases with increasing temperature.

Which response lists all the following pairs that are miscible liquids Pair #1: octane (C8H18) and water Pair #2: acetic acid (CH3COOH) and water Pair #3: octane (C8H18) and carbon tetrachloride(CCl4)

A 20.0 % by mass solution of phosphoric acid (H3PO4) in water has a density of 1.114 g/mL at 20 ∘\circ∘ C. What is the molarity of this solution

The vapor pressure of water at 45.0 ∘\circ∘ C is 71.93 mmHg. Calculate the vapor pressure of a solution of 1.25m Al(ClO3)3 at this temperature (assume 100% dissociation).

When 12.1 g of the sugar sucrose (a nonelectrolyte) is dissolved in exactly 800.0 g of water, the solution has a freezing point of -0.082 ∘\circ∘ C. What is the molar mass of sucrose Kf of water is 1.86 ∘\circ∘ C/m.

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Calculate the boiling point of a 4.5 m solution of Na₂SO₄ in water (assume 100% dissociation, K_b (H₂O) = 0.52 ^$\circ$C/m).

If 14.2 g of Al(NO₃)₃ is dissolved in 655g of water, what is the boiling point of the solution (assume 100% dissociation, K_b (H₂O) = 0.52 ^$\circ$C/m)

An aqueous dextrose solution having a density of 1.04 g/cm³ freezes at -1.15^$\circ$C. Find the osmotic pressure of this solution at 25^$\circ$C. K_f of water is 1.86 ^$\circ$C/m; molecular mass of dextrose = 180.16 g/mol.

What is the mass percent CH₃OH of a 0.256 m CH₃OH(aq) solution

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C₁₂H₂₂O₁₁.

The solubility of nitrogen gas at 25^$\circ$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

Which response lists all the following pairs that are miscible liquids Pair #1: octane (C₈H₁₈) and water Pair #2: acetic acid (CH₃COOH) and water Pair #3: octane (C₈H₁₈) and carbon tetrachloride(CCl₄)

A 20.0 % by mass solution of phosphoric acid (H₃PO₄) in water has a density of 1.114 g/mL at 20^$\circ$C. What is the molarity of this solution

The vapor pressure of water at 45.0 ^$\circ$C is 71.93 mmHg. Calculate the vapor pressure of a solution of 1.25m Al(ClO₃)₃ at this temperature (assume 100% dissociation).

When 12.1 g of the sugar sucrose (a nonelectrolyte) is dissolved in exactly 800.0 g of water, the solution has a freezing point of -0.082^$\circ$C. What is the molar mass of sucrose K_f of water is 1.86^$\circ$C/m.