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 osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C9H8O4)in 0.250 L of water at 25°C is __________ atm.

A) 13.6 B) 1.14 × 10-3 C) 0.0136 D) 2.45 E) 1.38 A) 13.6 B) 1.14 × 10-3 C) 0.0136 D) 2.45 E) 1.38

The most likely van't Hoff factor for an 0.01 m CaI2 solution is __________.

A) 1.00 B) 3.00 C) 1.27 D) 2.69 E) 3.29 A) 1.00 B) 3.00 C) 1.27 D) 2.69 E) 3.29

The solubility of MnSO4 monohydrate in water at 20°C is 70.0 g per 100.0 mL of water. A solution at 20°C that is 0.401 M in MnSO4 monohydrate is best described as a(n)__________ solution. The formula weight of MnSO4 monohydrate is 168.97 g/mol.

A) hydrated B) solvated C) saturated D) unsaturated E) supersaturated A) hydrated B) solvated C) saturated D) unsaturated E) supersaturated

Exam 13: Properties of Solutions

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 41

A solution is prepared by dissolving 7.00 g of glycerin (C₃H₈O₃)in 201 g of ethanol (C₂H₅OH). The freezing point of the solution is __________°C. The freezing point of pure ethanol is -114.6°C at 1 atm. The molal-freezing-point-depression constant (K_f)for ethanol is 1.99°C/m. The molar masses of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol, respectively.

(Multiple Choice)

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Question 42

At 20°C, a 2.32 M aqueous solution of ammonium chloride has a density of 1.0344 g/mL. What is the molality of ammonium chloride in the solution? The formula weight of NH₄Cl is 53.50 g/mol.

(Multiple Choice)

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Question 43

A solution is prepared by dissolving 2.60 g of a strong electrolyte (formula weight = 101 g/mol)in enough water to make 1.00 L of solution. The osmotic pressure of the solution is 1.25 atm at 25.0°C. What is the van't Hoff factor (i)for the unknown solute?

(Multiple Choice)

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Question 44

The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C₉H₈O₄)in 0.250 L of water at 25°C is __________ atm.

(Multiple Choice)

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Question 45

Of the following, a 0.1 M aqueous solution of __________ will have the lowest freezing point.

(Multiple Choice)

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Question 46

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 47

The most likely van't Hoff factor for an 0.01 m CaI₂ solution is __________.

(Multiple Choice)

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Question 48

The solubility of MnSO₄ monohydrate in water at 20°C is 70.0 g per 100.0 mL of water. A solution at 20°C that is 0.401 M in MnSO₄ monohydrate is best described as a(n)__________ solution. The formula weight of MnSO₄ monohydrate is 168.97 g/mol.

(Multiple Choice)

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Question 49

A solution is prepared by dissolving 14.0 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 50

Which one of the following vitamins is water soluble?

(Multiple Choice)

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Question 51

Which produces the greatest number of ions when one mole dissolves in water?

(Multiple Choice)

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Question 52

Which one of the following substances is more likely to dissolve in benzene (C₆H₆)?

(Multiple Choice)

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Question 53

Colligative properties of solutions include all of the following except __________.

(Multiple Choice)

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Question 54

A solution with a concentration higher than the solubility is __________.

(Multiple Choice)

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Question 55

If the partial pressure of oxygen in the air a diver breathes is too great, __________.

(Multiple Choice)

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Question 56

When solutions of strong electrolytes in water are formed, the ions are surrounded by water molecules. These interactions are described as a case of __________.

(Multiple Choice)

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Question 57

The freezing point of ethanol (C₂H₅OH)is -114.6°C. The molal freezing point depression constant for ethanol is 2.00°C/m. What is the freezing point (°C)of a solution prepared by dissolving 40.0 g of glycerin (C₃H₈O₃, a nonelectrolyte)in 200.0 g of ethanol?

(Multiple Choice)

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Question 58

The formula weight of FeCl₃^.6H₂O is __________.

(Short Answer)

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Question 59

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 60

Showing 41 - 60 of 151

Exam 13: Properties of Solutions

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 __________.

At 20°C, a 2.32 M aqueous solution of ammonium chloride has a density of 1.0344 g/mL. What is the molality of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol.

A solution is prepared by dissolving 2.60 g of a strong electrolyte (formula weight = 101 g/mol)in enough water to make 1.00 L of solution. The osmotic pressure of the solution is 1.25 atm at 25.0°C. What is the van't Hoff factor (i)for the unknown solute?

The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C9H8O4)in 0.250 L of water at 25°C is __________ atm.

Of the following, a 0.1 M aqueous solution of __________ will have the lowest freezing point.

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.

The most likely van't Hoff factor for an 0.01 m CaI2 solution is __________.

The solubility of MnSO4 monohydrate in water at 20°C is 70.0 g per 100.0 mL of water. A solution at 20°C that is 0.401 M in MnSO4 monohydrate is best described as a(n)__________ solution. The formula weight of MnSO4 monohydrate is 168.97 g/mol.

A solution is prepared by dissolving 14.0 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 __________.

Which one of the following vitamins is water soluble?

Which produces the greatest number of ions when one mole dissolves in water?

Which one of the following substances is more likely to dissolve in benzene (C6H6)?

Colligative properties of solutions include all of the following except __________.

A solution with a concentration higher than the solubility is __________.

If the partial pressure of oxygen in the air a diver breathes is too great, __________.

When solutions of strong electrolytes in water are formed, the ions are surrounded by water molecules. These interactions are described as a case of __________.

The freezing point of ethanol (C2H5OH)is -114.6°C. The molal freezing point depression constant for ethanol is 2.00°C/m. What is the freezing point (°C)of a solution prepared by dissolving 40.0 g of glycerin (C3H8O3, a nonelectrolyte)in 200.0 g of ethanol?

The formula weight of FeCl3.6H2O is __________.

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

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

The Chemistry of Life: Organic and Biological Chemistry

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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 __________.

At 20°C, a 2.32 M aqueous solution of ammonium chloride has a density of 1.0344 g/mL. What is the molality of ammonium chloride in the solution? The formula weight of NH₄Cl is 53.50 g/mol.

The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C₉H₈O₄)in 0.250 L of water at 25°C is __________ atm.

The most likely van't Hoff factor for an 0.01 m CaI₂ solution is __________.

The solubility of MnSO₄ monohydrate in water at 20°C is 70.0 g per 100.0 mL of water. A solution at 20°C that is 0.401 M in MnSO₄ monohydrate is best described as a(n)__________ solution. The formula weight of MnSO₄ monohydrate is 168.97 g/mol.

A solution is prepared by dissolving 14.0 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 __________.

Which one of the following substances is more likely to dissolve in benzene (C₆H₆)?

The freezing point of ethanol (C₂H₅OH)is -114.6°C. The molal freezing point depression constant for ethanol is 2.00°C/m. What is the freezing point (°C)of a solution prepared by dissolving 40.0 g of glycerin (C₃H₈O₃, a nonelectrolyte)in 200.0 g of ethanol?

The formula weight of FeCl₃^.6H₂O is __________.