Exam 13: The Properties of Mixtures: Solutions and Colloids

The mole fraction of potassium nitrate in an aqueous solution is 0.0194. The solution's density is 1.0627 g/mL. Calculate the molarity of the solution.

(Multiple Choice)

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Question 61

Barbiturates are synthetic drugs used as sedatives and hypnotics. Barbital ( = 184.2 g/mol) is one of the simplest of these drugs. What is the boiling point of a solution prepared by dissolving 42.5 g of barbital in 825 g of acetic acid? K_b = 3.07°C/m; boiling point of pure acetic acid = 117.9°C

(Multiple Choice)

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Question 62

What volume of concentrated (14.7 M) phosphoric acid is needed to prepare 25.0 L of 3.0 M H₃PO₄?

(Multiple Choice)

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Question 63

Which of the following aqueous solutions should demonstrate the most non-ideal behavior?

(Multiple Choice)

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Question 64

A solution of sucrose (sugar) in water is in equilibrium with solid sucrose. If more solid sucrose is now added, with stirring,

(Multiple Choice)

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Question 65

A 7.112 M solution of sulfuric acid (H₂SO₄) in water has a density of 1.395 g/mL. What is its molality?

(Short Answer)

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Question 66

Soda drinks bubble when the bottle is opened because

(Multiple Choice)

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Question 67

Aqueous ammonia is commercially available in a solution that is 28% (w/w) ammonia. What is the mole fraction of ammonia in such a solution?

(Multiple Choice)

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Question 68

Potassium fluoride is used for frosting glass. Calculate the molarity of a solution prepared by dissolving 78.6 g of KF in enough water to produce 225 mL of solution.

(Multiple Choice)

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Question 69

If the density of a solution is less than 1.0 g/mL, its molarity will be greater than its molality.

(True/False)

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Question 70

Potassium hydrogen phosphate is used in the preparation of non-dairy powdered creamers. Calculate the molarity of a solution prepared by dissolving 238 g of K₂HPO₄in enough water to produce 275 mL of solution.

(Multiple Choice)

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Question 71

Predict the ideal van't Hoff factor (i) for each of the following solutes: a. CaCl₂ b. Fe₂(SO₄)₃ c. NH₄Cl

(Essay)

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Question 72

A solution of ethanol (C₂H₆O) in water is sometimes used as a disinfectant. 1.00 L of this solution contains 553 g of ethanol and 335 g of water. What is the mole fraction of ethanol in this solution?

(Multiple Choice)

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Question 73

A 0.137 m solution of sodium ferrocyanide (Na₄Fe(CN)₆.10H₂O) in water has a freezing point depression of 0.755°C. Calculate the van't Hoff factor (i) under these conditions. (K_f= 1.86°C/m)

(Short Answer)

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Question 74

Which of the following pairs of ions is arranged so that the ion with the smaller charge density is listed first?

(Multiple Choice)

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Question 75

Calculate the freezing point of a solution made by dissolving 3.50 g of potassium chloride ( = 74.55 g/mol) in 100.0 g of water. Assume ideal behavior for the solution; K_f = 1.86°C/m.

(Multiple Choice)

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Question 76

Octane and nonane are liquids which are components of gasoline. Their vapor pressures at 25°C are 13.9 torr and 4.7 torr, respectively. What is the vapor pressure of a mixture consisting of 1 mole of each of these compounds?

(Short Answer)

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Question 77

Children under the age of six with more than 0.10 ppm of lead in their blood can suffer a reduction in I.Q. or have behavior problems. What is the molality of a solution which contains 0.10 ppm of lead?

(Multiple Choice)

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Question 78

Isoamyl salicylate ( = 208.25 g/mol) has a pleasant aroma and is used in perfumes and soaps. Which of the following combinations gives a 0.75 m solution of isoamyl salicylate in ethyl alcohol (d = 0.7893 g/mL)?

(Multiple Choice)

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Question 79

From the following list of aqueous solutions and water, select the one with the highest boiling point.

(Multiple Choice)

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Question 80

Showing 61 - 80 of 105

Exam 13: The Properties of Mixtures: Solutions and Colloids

The mole fraction of potassium nitrate in an aqueous solution is 0.0194. The solution's density is 1.0627 g/mL. Calculate the molarity of the solution.

Barbiturates are synthetic drugs used as sedatives and hypnotics. Barbital ( = 184.2 g/mol) is one of the simplest of these drugs. What is the boiling point of a solution prepared by dissolving 42.5 g of barbital in 825 g of acetic acid? Kb = 3.07°C/m; boiling point of pure acetic acid = 117.9°C

What volume of concentrated (14.7 M) phosphoric acid is needed to prepare 25.0 L of 3.0 M H3PO4?

Which of the following aqueous solutions should demonstrate the most non-ideal behavior?

A solution of sucrose (sugar) in water is in equilibrium with solid sucrose. If more solid sucrose is now added, with stirring,

A 7.112 M solution of sulfuric acid (H2SO4) in water has a density of 1.395 g/mL. What is its molality?

Soda drinks bubble when the bottle is opened because

Aqueous ammonia is commercially available in a solution that is 28% (w/w) ammonia. What is the mole fraction of ammonia in such a solution?

Potassium fluoride is used for frosting glass. Calculate the molarity of a solution prepared by dissolving 78.6 g of KF in enough water to produce 225 mL of solution.

If the density of a solution is less than 1.0 g/mL, its molarity will be greater than its molality.

Potassium hydrogen phosphate is used in the preparation of non-dairy powdered creamers. Calculate the molarity of a solution prepared by dissolving 238 g of K2HPO4 in enough water to produce 275 mL of solution.

Predict the ideal van't Hoff factor (i) for each of the following solutes: a. CaCl2 b. Fe2(SO4)3 c. NH4Cl

A solution of ethanol (C2H6O) in water is sometimes used as a disinfectant. 1.00 L of this solution contains 553 g of ethanol and 335 g of water. What is the mole fraction of ethanol in this solution?

A 0.137 m solution of sodium ferrocyanide (Na4Fe(CN)6.10H2O) in water has a freezing point depression of 0.755°C. Calculate the van't Hoff factor (i) under these conditions. (Kf = 1.86°C/m)

Which of the following pairs of ions is arranged so that the ion with the smaller charge density is listed first?

Calculate the freezing point of a solution made by dissolving 3.50 g of potassium chloride ( = 74.55 g/mol) in 100.0 g of water. Assume ideal behavior for the solution; Kf = 1.86°C/m.

Octane and nonane are liquids which are components of gasoline. Their vapor pressures at 25°C are 13.9 torr and 4.7 torr, respectively. What is the vapor pressure of a mixture consisting of 1 mole of each of these compounds?

Children under the age of six with more than 0.10 ppm of lead in their blood can suffer a reduction in I.Q. or have behavior problems. What is the molality of a solution which contains 0.10 ppm of lead?

Isoamyl salicylate ( = 208.25 g/mol) has a pleasant aroma and is used in perfumes and soaps. Which of the following combinations gives a 0.75 m solution of isoamyl salicylate in ethyl alcohol (d = 0.7893 g/mL)?

From the following list of aqueous solutions and water, select the one with the highest boiling point.

Keys to the Study of Chemistry

The Components of Matter

Stoichiometry of Formulas and Equations

The Major Classes of Chemical Reactions

Gases and the Kinetic-Molecular Theory

Thermochemistry: Energy Flow and Chemical Change

Quantum Theory and Atomic Structure

Electron Configuration and Chemical Periodicity

Models of Chemical Bonding

The Shapes of Molecules

Theories of Covalent Bonding

Intermolecular Forces: Liquids, Solids, and Phase Changes

Periodic Patterns in the Main Group Elements: Bonding, Structure, and Reactivity

Organic Compounds and the Atomic Properties of Carbon

Kinetics: Rates and Mechanisms of Chemical Reactions

Equilibrium: the Extent of Chemical Reactions

Acid-Base Equilibria

Ionic Equilibria in Aqueous Systems

Thermodynamics: Entropy, Free Energy, and the Direction of Chemical Reactions

Electrochemistry: Chemical Change and Electrical Work

The Elements in Nature and Industry

The Transition Elements and Their Coordination Compounds

Nuclear Reactions and Their Applications

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Barbiturates are synthetic drugs used as sedatives and hypnotics. Barbital ( = 184.2 g/mol) is one of the simplest of these drugs. What is the boiling point of a solution prepared by dissolving 42.5 g of barbital in 825 g of acetic acid? K_b = 3.07°C/m; boiling point of pure acetic acid = 117.9°C

What volume of concentrated (14.7 M) phosphoric acid is needed to prepare 25.0 L of 3.0 M H₃PO₄?

A 7.112 M solution of sulfuric acid (H₂SO₄) in water has a density of 1.395 g/mL. What is its molality?

Potassium hydrogen phosphate is used in the preparation of non-dairy powdered creamers. Calculate the molarity of a solution prepared by dissolving 238 g of K₂HPO₄in enough water to produce 275 mL of solution.

Predict the ideal van't Hoff factor (i) for each of the following solutes: a. CaCl₂ b. Fe₂(SO₄)₃ c. NH₄Cl

A solution of ethanol (C₂H₆O) in water is sometimes used as a disinfectant. 1.00 L of this solution contains 553 g of ethanol and 335 g of water. What is the mole fraction of ethanol in this solution?

A 0.137 m solution of sodium ferrocyanide (Na₄Fe(CN)₆.10H₂O) in water has a freezing point depression of 0.755°C. Calculate the van't Hoff factor (i) under these conditions. (K_f= 1.86°C/m)

Calculate the freezing point of a solution made by dissolving 3.50 g of potassium chloride ( = 74.55 g/mol) in 100.0 g of water. Assume ideal behavior for the solution; K_f = 1.86°C/m.