The osmotic pressure of a solution formed by dissolving 45.0 mg of aspirin C9H8O4)in 0.250 L of water at 25 °C is ________ atm.

A) 24.5 B) 2.05 × 10-3 C) 0.0245 D) 4.41 E) 2.48 A) 24.5 B) 2.05 × 10-3 C) 0.0245 D) 4.41 E) 2.48

The concentration of CO2 in a soft drink bottled with a partial pressure of CO2 of 6.5 atm over the liquid at 29 °C is 2.2 × 10-1 M. The Henry's law constant for CO2 at this temperature is ________.

A) 2.2 × 10-1 mol/L-atm B) 7.6 × 10-3 mol/L-atm C) 5.6 × 10-3 mol/L-atm D) 3.4 × 10-2 mol/L-atm E) More information is needed to solve the problem. A) 2.2 × 10-1 mol/L-atm B) 7.6 × 10-3 mol/L-atm C) 5.6 × 10-3 mol/L-atm D) 3.4 × 10-2 mol/L-atm E) More information is needed to solve the problem.

The concentration of urea in a solution prepared by dissolving 16 g of urea in 25 g of H2O is ________% by mass. The molar mass of urea is 60.0 g/mol.

A) 39 B) 64 C) 0.39 D) 0.64 E) 0.48 A) 39 B) 64 C) 0.39 D) 0.64 E) 0.48

Exam 13: Properties of Solutions

A solution is prepared by dissolving 11.0 g of NH₃ in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The mole fraction of NH₃ in the solution is ________.

(Multiple Choice)

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Question 121

The solubility of Ar in water at 25 °C is 1.6 × 10^-3 M when the pressure of the Ar above the solution is 1.0 atm. The solubility of Ar at a pressure of 2.5 atm is ________ M.

(Multiple Choice)

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Question 122

When argon is placed in a container of neon, the argon spontaneously disperses throughout the neon because ________.

(Multiple Choice)

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Question 123

Which of the following statements is false?

(Multiple Choice)

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Question 124

What is the osmotic pressure (in atm)of a 0.040 M solution of a non-electrolyte at 30.0 °C?

(Short Answer)

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Question 125

Physical properties of a solution that depend on the quantity of the solute particles present, but not the kind or identity of the particles, are termed ________ properties.

(Short Answer)

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Question 126

Compounds composed of a salt and water combined in definite proportions are known as ________.

(Multiple Choice)

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Question 127

George is making spaghetti for dinner. He places 4.01 kg of water in a pan and brings it to a boil. Before adding the pasta, he adds 58 g of table salt (NaCl)to the water and again brings it to a boil. The temperature of the salty, boiling water is ________°C. Assume a pressure of 1.00 atm and negligible evaporation of water. K_b for water is 0.52 °C/m.

(Multiple Choice)

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Question 128

The vapor pressure of pure ethanol at 60 °C is 0.459 atm. Raoult's Law predicts that a solution prepared by dissolving 10.0 mmol naphthalene (nonvolatile)in 90.0 mmol ethanol will have a vapor pressure of ________ atm.

(Multiple Choice)

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Question 129

A solution contains 11% by mass of sodium chloride. This means that ________.

(Multiple Choice)

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Question 130

An aqueous solution of a soluble compound (a nonelectrolyte)is prepared by dissolving 33.2 g of the compound in sufficient water to form 250 mL of solution. The solution has an osmotic pressure of 1.2 atm at 25 °C. What is the molar mass (g/mole)of the compound?

(Multiple Choice)

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Question 131

The osmotic pressure of a solution formed by dissolving 45.0 mg of aspirin C₉H₈O₄)in 0.250 L of water at 25 °C is ________ atm.

(Multiple Choice)

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Question 132

The concentration of nitrate ion in a solution that contains 0.800 M aluminum nitrate is _______ M.

(Multiple Choice)

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Question 133

What is the mole fraction of sodium chloride in solution that is 13.0% by mass sodium chloride and that has a density of 1.10 g/mL?

(Multiple Choice)

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Question 134

The concentration of CO₂ in a soft drink bottled with a partial pressure of CO₂ of 6.5 atm over the liquid at 29 °C is 2.2 × 10^-1 M. The Henry's law constant for CO₂ at this temperature is ________.

(Multiple Choice)

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Question 135

Calculate the molarity of a 17.5% (by mass)aqueous solution of nitric acid.

(Multiple Choice)

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Question 136

The concentration of urea in a solution prepared by dissolving 16 g of urea in 25 g of H₂O is ________% by mass. The molar mass of urea is 60.0 g/mol.

(Multiple Choice)

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Question 137

A solution is prepared by dissolving 23.7 g of CaCl₂ in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl₂ in this solution is ________ molar.

(Multiple Choice)

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Question 138

A solution with a solute concentration greater than the solubility is called a supercritical solution.

(True/False)

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Question 139

Calculate the molality of a 21.6% (by mass)aqueous solution of phosphoric acid (H₃PO₄).

(Multiple Choice)

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Question 140

Showing 121 - 140 of 160

Exam 13: Properties of Solutions

A solution is prepared by dissolving 11.0 g of NH3 in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The mole fraction of NH3 in the solution is ________.

The solubility of Ar in water at 25 °C is 1.6 × 10-3 M when the pressure of the Ar above the solution is 1.0 atm. The solubility of Ar at a pressure of 2.5 atm is ________ M.

When argon is placed in a container of neon, the argon spontaneously disperses throughout the neon because ________.

Which of the following statements is false?

What is the osmotic pressure (in atm)of a 0.040 M solution of a non-electrolyte at 30.0 °C?

Physical properties of a solution that depend on the quantity of the solute particles present, but not the kind or identity of the particles, are termed ________ properties.

Compounds composed of a salt and water combined in definite proportions are known as ________.

The vapor pressure of pure ethanol at 60 °C is 0.459 atm. Raoult's Law predicts that a solution prepared by dissolving 10.0 mmol naphthalene (nonvolatile)in 90.0 mmol ethanol will have a vapor pressure of ________ atm.

A solution contains 11% by mass of sodium chloride. This means that ________.

An aqueous solution of a soluble compound (a nonelectrolyte)is prepared by dissolving 33.2 g of the compound in sufficient water to form 250 mL of solution. The solution has an osmotic pressure of 1.2 atm at 25 °C. What is the molar mass (g/mole)of the compound?

The osmotic pressure of a solution formed by dissolving 45.0 mg of aspirin C9H8O4)in 0.250 L of water at 25 °C is ________ atm.

The concentration of nitrate ion in a solution that contains 0.800 M aluminum nitrate is _______ M.

What is the mole fraction of sodium chloride in solution that is 13.0% by mass sodium chloride and that has a density of 1.10 g/mL?

The concentration of CO2 in a soft drink bottled with a partial pressure of CO2 of 6.5 atm over the liquid at 29 °C is 2.2 × 10-1 M. The Henry's law constant for CO2 at this temperature is ________.

Calculate the molarity of a 17.5% (by mass)aqueous solution of nitric acid.

The concentration of urea in a solution prepared by dissolving 16 g of urea in 25 g of H2O is ________% by mass. The molar mass of urea is 60.0 g/mol.

A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl2 in this solution is ________ molar.

A solution with a solute concentration greater than the solubility is called a supercritical solution.

Calculate the molality of a 21.6% (by mass)aqueous solution of phosphoric acid (H3PO4).

Introduction: Matter and Measurement

Atoms, Molecules, and Ions

Stoichiometry: Calculations With Chemical Formulas and Equations

Aqueous Reactions and Solution Stoichiometry

Thermochemistry

Electronic Structure of Atoms

Periodic Properties of the Elements

Basic Concepts of Chemical Bonding

Molecular Geometry and Bonding Theories

Gases

Liquids and Intermolecular Forces

Solids and Modern Materials

Chemical Kinetics

Chemical Equilibrium

Acid-Base Equilibria

Additional Aspects of Aqueous Equilibria

Chemistry of the Environment

Chemical Thermodynamics

Electrochemistry

Nuclear Chemistry

Chemistry of the Nonmetals

Transition Metals and Coordination Chemistry

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A solution is prepared by dissolving 11.0 g of NH₃ in 250.0 g of water. The density of the resulting solution is 0.974 g/mL. The mole fraction of NH₃ in the solution is ________.

The solubility of Ar in water at 25 °C is 1.6 × 10^-3 M when the pressure of the Ar above the solution is 1.0 atm. The solubility of Ar at a pressure of 2.5 atm is ________ M.

The osmotic pressure of a solution formed by dissolving 45.0 mg of aspirin C₉H₈O₄)in 0.250 L of water at 25 °C is ________ atm.

The concentration of CO₂ in a soft drink bottled with a partial pressure of CO₂ of 6.5 atm over the liquid at 29 °C is 2.2 × 10^-1 M. The Henry's law constant for CO₂ at this temperature is ________.

The concentration of urea in a solution prepared by dissolving 16 g of urea in 25 g of H₂O is ________% by mass. The molar mass of urea is 60.0 g/mol.

A solution is prepared by dissolving 23.7 g of CaCl₂ in 375 g of water. The density of the resulting solution is 1.05 g/mL. The concentration of CaCl₂ in this solution is ________ molar.

Calculate the molality of a 21.6% (by mass)aqueous solution of phosphoric acid (H₃PO₄).