Solutions are made that contain 0.1 moles of each of the following compounds below in 100 g of H2O. Choose the compound whose solution will have the lowest freezing point.

A) MgCl2 B) KClO3 C) CO2 D) MgSO4 E) NaBr A) MgCl2 B) KClO3 C) CO2 D) MgSO4 E) NaBr A

What is the correct value for the weight of Na3PO4 needed to make 100 mL of a 0.50 molar solution?

A) 16.4 g B) 8.2 g C) 0.05 g D) 82 g E) 4.1 g A) 16.4 g B) 8.2 g C) 0.05 g D) 82 g E) 4.1 g B

252 mL of 3.00 M H2SO4 are added to 1.50 L of 0.500 M H2SO4. What is the concentration of the resulting solution?

A) 1.50 M B) 0.860 M C) 2.64 M D) 1.75 M E) 1.25 M A) 1.50 M B) 0.860 M C) 2.64 M D) 1.75 M E) 1.25 M

Henry's Law constants for aqueous solutions at 25°C are 8.20 × 10-7 molal/mmHg for N2 and 1.62 × 10-6 molal/mmHg for O2. Determine the solubility of oxygen in water under an atmospheric pressure of 760 mmHg, assuming that air is 80% N2 and 20% O2.

A) 6.2 × 10-3 m B) 2.5 × 10-4 m C) 1.3 × 10-4 m D) 5.0 × 10-4 m E) 1.2 × 10-3 m A) 6.2 × 10-3 m B) 2.5 × 10-4 m C) 1.3 × 10-4 m D) 5.0 × 10-4 m E) 1.2 × 10-3 m

A solution composed of 5 moles of acetone (CH3COCH3, P°A = 324 mmHg) and 5 moles of chloroform (CHCl3, P°C = 274 mmHg) has a vapor pressure of 236 mmHg. Which one of the following statements is completely true about this solution?

A) The solution shows a negative deviation from Raoult's law and thus possesses a maximum boiling azeotrope. B) The solution process is exothermic because the forces between unlike molecules are weaker than those between like molecules. C) The solution shows a positive deviation from Raoult's law. D) The solution possesses a minimum boiling azeotrope because it shows a negative deviation from Raoult's law. E) The solution obeys Raoult's Law. A) The solution shows a negative deviation from Raoult's law and thus possesses a maximum boiling azeotrope. B) The solution process is exothermic because the forces between unlike molecules are weaker than those between like molecules. C) The solution shows a positive deviation from Raoult's law. D) The solution possesses a minimum boiling azeotrope because it shows a negative deviation from Raoult's law. E) The solution obeys Raoult's Law.

Exam 13: Solutions and Their Physical Properties

Solutions are made that contain 0.1 moles of each of the following compounds below in 100 g of H₂O. Choose the compound whose solution will have the lowest freezing point.

Free

(Multiple Choice)

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Question 1

Correct Answer:

Verified

Liquid Q is a polar solvent and liquid R is a nonpolar solvent. On the basis of this information, you would expect:

Free

(Multiple Choice)

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Question 2

Correct Answer:

Verified

What is the correct value for the weight of Na₃PO₄needed to make 100 mL of a 0.50 molar solution?

Free

(Multiple Choice)

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Question 3

Correct Answer:

Verified

Which definition is INCORRECT?

(Multiple Choice)

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Question 4

The stronger the forces between solute and solvent molecules, the more exothermic the solution process.

(True/False)

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Question 5

Molality is independent of temperature, molarity is dependent on temperature.

(True/False)

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Question 6

The vapor pressures of pure hexane and pure heptane at 25°C are 151.4 mmHg and 45.62 mmHg respectively. A solution contains 0.800 mol fraction n-hexane and 0.200 mol fraction n-heptane. What is the composition of the vapor in equilibrium with this solution at 25°C?

(Multiple Choice)

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Question 7

252 mL of 3.00 M H₂SO₄are added to 1.50 L of 0.500 M H₂SO₄. What is the concentration of the resulting solution?

(Multiple Choice)

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Question 8

Exactly 375.0 mg of an unknown protein is dissolved in enough water to give 50.00 mL of solution and the osmotic pressure determined as 3.25 mmHg at 298 K. Estimate the molar mass of this protein.

(Multiple Choice)

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Question 9

0.0800 g of a compound with the empirical formula C₂H₂N is dissolved in 10.00 g benzene. The resulting solution freezes at 4.99°C. Benzene freezes at 5.48°C and has a freezing point depression constant of Kf = 4.90°C/m. What is the molecular formula of the compound?

(Multiple Choice)

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Question 10

Which of the following organic substances is most readily soluble in water?

(Multiple Choice)

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Question 11

Henry's Law states that:

(Multiple Choice)

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Question 12

An isotonic solution will produce an osmotic pressure of 7.84 atm measured against pure water at human body temperature (37.0°C). How many grams of sodium chloride must be dissolved in a liter of water to produce an isotonic solution?

(Multiple Choice)

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Question 13

A solution is called "ideal" when:

(Multiple Choice)

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Question 14

Henry's Law constants for aqueous solutions at 25°C are 8.20 × 10^-7 molal/mmHg for N₂ and 1.62 × 10^-6 molal/mmHg for O₂. Determine the solubility of oxygen in water under an atmospheric pressure of 760 mmHg, assuming that air is 80% N₂ and 20% O₂.

(Multiple Choice)

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Question 15

A solution containing 3.24 g of sulfur in 40 g of benzene boils 0.81°C above the boiling point of pure benzene. Determine the number of S atoms in one molecule of dissolved sulfur. Kb for benzene is 2.53°C m-1.

(Multiple Choice)

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Question 16

Determine the osmotic pressure at 25 °C of an aqueous solution that is 0.028 M NaNO₃.

(Multiple Choice)

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Question 17

A solution composed of 5 moles of acetone (CH₃COCH₃, P°A = 324 mmHg) and 5 moles of chloroform (CHCl₃, P°C = 274 mmHg) has a vapor pressure of 236 mmHg. Which one of the following statements is completely true about this solution?

(Multiple Choice)

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Question 18

What is the osmotic pressure in mmHg of 6.00 L of a 0.108 M solution at 30°C if three moles of ions are produced in aqueous solution for every mole of solute dissolved?

(Multiple Choice)

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Question 19

Which compound is most likely to be soluble in water?

(Multiple Choice)

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Question 20

Showing 1 - 20 of 100

Exam 13: Solutions and Their Physical Properties

Solutions are made that contain 0.1 moles of each of the following compounds below in 100 g of H2O. Choose the compound whose solution will have the lowest freezing point.

Liquid Q is a polar solvent and liquid R is a nonpolar solvent. On the basis of this information, you would expect:

What is the correct value for the weight of Na3PO4 needed to make 100 mL of a 0.50 molar solution?

Which definition is INCORRECT?

The stronger the forces between solute and solvent molecules, the more exothermic the solution process.

Molality is independent of temperature, molarity is dependent on temperature.

The vapor pressures of pure hexane and pure heptane at 25°C are 151.4 mmHg and 45.62 mmHg respectively. A solution contains 0.800 mol fraction n-hexane and 0.200 mol fraction n-heptane. What is the composition of the vapor in equilibrium with this solution at 25°C?

252 mL of 3.00 M H2SO4 are added to 1.50 L of 0.500 M H2SO4. What is the concentration of the resulting solution?

Exactly 375.0 mg of an unknown protein is dissolved in enough water to give 50.00 mL of solution and the osmotic pressure determined as 3.25 mmHg at 298 K. Estimate the molar mass of this protein.

0.0800 g of a compound with the empirical formula C2H2N is dissolved in 10.00 g benzene. The resulting solution freezes at 4.99°C. Benzene freezes at 5.48°C and has a freezing point depression constant of Kf = 4.90°C/m. What is the molecular formula of the compound?

Which of the following organic substances is most readily soluble in water?

Henry's Law states that:

An isotonic solution will produce an osmotic pressure of 7.84 atm measured against pure water at human body temperature (37.0°C). How many grams of sodium chloride must be dissolved in a liter of water to produce an isotonic solution?

A solution is called "ideal" when:

Henry's Law constants for aqueous solutions at 25°C are 8.20 × 10-7 molal/mmHg for N2 and 1.62 × 10-6 molal/mmHg for O2. Determine the solubility of oxygen in water under an atmospheric pressure of 760 mmHg, assuming that air is 80% N2 and 20% O2.

A solution containing 3.24 g of sulfur in 40 g of benzene boils 0.81°C above the boiling point of pure benzene. Determine the number of S atoms in one molecule of dissolved sulfur. Kb for benzene is 2.53°C m-1.

Determine the osmotic pressure at 25 °C of an aqueous solution that is 0.028 M NaNO3.

A solution composed of 5 moles of acetone (CH3COCH3, P°A = 324 mmHg) and 5 moles of chloroform (CHCl3, P°C = 274 mmHg) has a vapor pressure of 236 mmHg. Which one of the following statements is completely true about this solution?

What is the osmotic pressure in mmHg of 6.00 L of a 0.108 M solution at 30°C if three moles of ions are produced in aqueous solution for every mole of solute dissolved?

Which compound is most likely to be soluble in water?

Matter - Its Properties and Measurement

Atoms and the Atomic Theory

Chemical Compounds

Chemical Reactions

Introduction to Reactions in Aqueous Solutions

Gases

Thermochemistry

Electrons in Atoms

The Periodic Table and Some Atomic Properties

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Additional Aspects

Intermolecular Forces: Liquids and Solids

Chemical Kinetics

Principles of Chemical Equilibrium

Acids and Bases

Additional Aspects of Acid-Base Equilibria

Solubility and Complex-Ion Equilibria

Spontaneous Change: Entropy and Free Energy

Electrochemistry

Main Group Elements I: Groups 1, 2, 13, and 14

Main Group Elements II: Groups 18, 17, 16, 15, and Hydrogen

The Transition Elements

Complex Ions and Coordination Compounds

Nuclear Chemistry 1-41

Structures of Organic Compounds

Reactions of Organic Compounds

Chemistry of the Living State

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Solutions are made that contain 0.1 moles of each of the following compounds below in 100 g of H₂O. Choose the compound whose solution will have the lowest freezing point.

What is the correct value for the weight of Na₃PO₄needed to make 100 mL of a 0.50 molar solution?

252 mL of 3.00 M H₂SO₄are added to 1.50 L of 0.500 M H₂SO₄. What is the concentration of the resulting solution?

0.0800 g of a compound with the empirical formula C₂H₂N is dissolved in 10.00 g benzene. The resulting solution freezes at 4.99°C. Benzene freezes at 5.48°C and has a freezing point depression constant of Kf = 4.90°C/m. What is the molecular formula of the compound?

Henry's Law constants for aqueous solutions at 25°C are 8.20 × 10^-7 molal/mmHg for N₂ and 1.62 × 10^-6 molal/mmHg for O₂. Determine the solubility of oxygen in water under an atmospheric pressure of 760 mmHg, assuming that air is 80% N₂ and 20% O₂.

Determine the osmotic pressure at 25 °C of an aqueous solution that is 0.028 M NaNO₃.

A solution composed of 5 moles of acetone (CH₃COCH₃, P°A = 324 mmHg) and 5 moles of chloroform (CHCl₃, P°C = 274 mmHg) has a vapor pressure of 236 mmHg. Which one of the following statements is completely true about this solution?