What would be the freezing point of a 1.50 m solution of NaNO3 in water? (Kf = 1.86 $\degree$C)

A) 5.58 $\degree$C B) (-2.79 $\degree$ C) C) (-5.58 $\degree$ C) D) 2.79 $\degree$C E) (-1.61 $\degree$ C) A) 5.58 $\degree$C B) (-2.79 $\degree$ C) C) (-5.58 $\degree$ C) D) 2.79 $\degree$C E) (-1.61 $\degree$ C)

A solution is prepared by mixing 45.68 g of carbon disulfide (CS2, 76.13 g/mol) with 16.42 g of acetonitrile (CH3CN, 41.06 g/mol).What is the mole fraction of CS2 in the vapor phase at 25 $\degree$C?

A) 1.00 B) 0.600 C) 0.167 D) 0.273 E) 0.857 A) 1.00 B) 0.600 C) 0.167 D) 0.273 E) 0.857

Exam 11: Properties of Solutions Their Concentrations and Colligative Properties

The vapor pressure of an aqueous solution is found to be 24.9 mmHg at 25 $\degree$ C.What is the mole fraction of solute in this solution? The vapor pressure of water is 25.756 mmHg at 25 $\degree$ C.

(Multiple Choice)

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Question 101

Define the term "colligative" in relation to the properties of a solution and list four colligative properties.

(Essay)

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Question 102

Which solution, if either, would create the higher osmotic pressure compared to pure water): one prepared from 1.0 g of NaCl in 10 mL of water or one prepared from 1.0 g of CsBr in 10 mL of water?

(Multiple Choice)

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Question 103

Henry's law constant for oxygen dissolving in blood is 3.74 10^-2 mol/L . atm at body temperature, 37 $Henry's law constant for oxygen dissolving in blood is 3.74 10-2 mol/L . atm at body temperature, 37 C.Calculate the molar concentration of oxygen in blood for a free diver where the air pressure is 3.0 atm.The mole fraction of oxygen in air is 0.209.$ C.Calculate the molar concentration of oxygen in blood for a free diver where the air pressure is 3.0 atm.The mole fraction of oxygen in air is 0.209.

(Short Answer)

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Question 104

A solution is prepared by adding 0.300 mol of glucose, which is not volatile, to 4.50 mol of water.What is the vapor pressure of this solution at 25 $\degree$ C given that the vapor pressure of pure water is 23.8 torr?

(Multiple Choice)

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Question 105

Indicate which aqueous solution has the lowest vapor pressure.

(Multiple Choice)

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Question 106

The normal freezing point of benzene (C₆H₆, 78.12 g/mol) is 5.49 $\degree$ C, and its K_f value is 5.12 $\degree$ C/m.To create a solution with a freezing point of 0.00 $\degree$ C, how many grams of naphthalene (C₁₀H₈, 128.2 g/mol) would need to be dissolved in 640.0 g of benzene?

(Multiple Choice)

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Question 107

You wish to de-ice your driveway, so you consider buying 10 lb of NaCl, 10 lb of CaCl₂, or 10 lb of MgCl₂.Which of these would de-ice your driveway most effectively? Assume that ideal dissociation of the salts occurs and that colligative properties are the only consideration.

(Multiple Choice)

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Question 108

A 15.0 mg sample of a protein was dissolved in water to produce 5.00 mL of solution at 25.1 $\degree$ C.The osmotic pressure of this solution was measured and found to be 6.50 torr.What is the molar mass of this protein?

(Multiple Choice)

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Question 109

Which of the following statements regarding solutions and the van 't Hoff factor is NOT correct?

(Multiple Choice)

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Question 110

What would be the freezing point of a 1.50 m solution of NaNO₃ in water? (K_f = 1.86 $\degree$ C)

(Multiple Choice)

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Question 111

A 0.512 g sample of an unknown nondissociating solute was dissolved in 25.0 g of camphor (K_f = 39.7 $\degree$ C/m), decreasing the freezing point of camphor by 3.07 $\degree$ C.What is the molar mass of the solute?

(Multiple Choice)

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Question 112

How does the presence of solutes raise the boiling point of a solvent?

(Essay)

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Question 113

Lanterns and stoves that use n-pentane as a fuel are often difficult to light on a cold day because the fuel has a low vapor pressure at low temperatures.Determine the vapor pressure of n-pentane on a night when the temperature is 0.0 $\degree$ C.The enthalpy of vaporization of n-pentane is 27.6 kJ/mol, and its boiling point is 36.0 $\degree$ C.

(Multiple Choice)

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Question 114

Identify the following statement as true or false and choose the correct explanation: "For solutions with the same molarity at the same temperature, the pressure needed for reverse osmosis of a sodium chloride solution will always be less than the pressure needed for a calcium chloride solution."

(Multiple Choice)

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Question 115

A solution is prepared by mixing 45.68 g of carbon disulfide (CS₂, 76.13 g/mol) with 16.42 g of acetonitrile (CH₃CN, 41.06 g/mol).What is the mole fraction of CS₂ in the vapor phase at 25 $\degree$ C? $A solution is prepared by mixing 45.68 g of carbon disulfide (CS2, 76.13 g/mol) with 16.42 g of acetonitrile (CH3CN, 41.06 g/mol).What is the mole fraction of CS2 in the vapor phase at 25 \degree C?$

(Multiple Choice)

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Question 116

Which statement regarding the boiling of a mixture of liquids A and B is NOT correct?

(Multiple Choice)

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Question 117

In the process of dialysis, a special semipermeable membrane allows both small molecules and water to pass through, but not large protein molecules.These membranes are used to separate these small molecules and ions from much larger proteins.If a mixture of proteins and small molecules were separated from pure water by a dialysis membrane as shown in the figure, which way would the molecules flow?

(Multiple Choice)

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Question 118

What is the vapor pressure of an aqueous solution that has a solute mole fraction of $\chi$ =0.200? The vapor pressure of water is 25.756 mmHg at 25 $\degree$ C.

(Multiple Choice)

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Question 119

The normal boiling point of ammonia is -33.34 $\degree$ C, and its enthalpy of vaporization is 23.35 kJ/mol.What pressure would have to be applied for ammonia to boil at 25.00 $\degree$ C?

(Multiple Choice)

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Question 120

Showing 101 - 120 of 130

The vapor pressure of an aqueous solution is found to be 24.9 mmHg at 25 $\degree$ C.What is the mole fraction of solute in this solution? The vapor pressure of water is 25.756 mmHg at 25 $\degree$ C.

Define the term "colligative" in relation to the properties of a solution and list four colligative properties.

Which solution, if either, would create the higher osmotic pressure compared to pure water): one prepared from 1.0 g of NaCl in 10 mL of water or one prepared from 1.0 g of CsBr in 10 mL of water?

A solution is prepared by adding 0.300 mol of glucose, which is not volatile, to 4.50 mol of water.What is the vapor pressure of this solution at 25 $\degree$ C given that the vapor pressure of pure water is 23.8 torr?

Indicate which aqueous solution has the lowest vapor pressure.

The normal freezing point of benzene (C₆H₆, 78.12 g/mol) is 5.49 $\degree$ C, and its K_f value is 5.12 $\degree$ C/m.To create a solution with a freezing point of 0.00 $\degree$ C, how many grams of naphthalene (C₁₀H₈, 128.2 g/mol) would need to be dissolved in 640.0 g of benzene?

You wish to de-ice your driveway, so you consider buying 10 lb of NaCl, 10 lb of CaCl₂, or 10 lb of MgCl₂.Which of these would de-ice your driveway most effectively? Assume that ideal dissociation of the salts occurs and that colligative properties are the only consideration.

A 15.0 mg sample of a protein was dissolved in water to produce 5.00 mL of solution at 25.1 $\degree$ C.The osmotic pressure of this solution was measured and found to be 6.50 torr.What is the molar mass of this protein?

Which of the following statements regarding solutions and the van 't Hoff factor is NOT correct?

What would be the freezing point of a 1.50 m solution of NaNO₃ in water? (K_f = 1.86 $\degree$ C)

A 0.512 g sample of an unknown nondissociating solute was dissolved in 25.0 g of camphor (K_f = 39.7 $\degree$ C/m), decreasing the freezing point of camphor by 3.07 $\degree$ C.What is the molar mass of the solute?

How does the presence of solutes raise the boiling point of a solvent?

Identify the following statement as true or false and choose the correct explanation: "For solutions with the same molarity at the same temperature, the pressure needed for reverse osmosis of a sodium chloride solution will always be less than the pressure needed for a calcium chloride solution."

Which statement regarding the boiling of a mixture of liquids A and B is NOT correct?

What is the vapor pressure of an aqueous solution that has a solute mole fraction of $\chi$ =0.200? The vapor pressure of water is 25.756 mmHg at 25 $\degree$ C.

The normal boiling point of ammonia is -33.34 $\degree$ C, and its enthalpy of vaporization is 23.35 kJ/mol.What pressure would have to be applied for ammonia to boil at 25.00 $\degree$ C?

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Atomic Structure Explaining the Properties of Elements

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Stoichiometry Mass Relationships and Chemical Reactions

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Additional Aqueous Equilibria Chemistry and the Oceans

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

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Exam 11: Properties of Solutions Their Concentrations and Colligative Properties

The vapor pressure of an aqueous solution is found to be 24.9 mmHg at 25 °\degree° C.What is the mole fraction of solute in this solution? The vapor pressure of water is 25.756 mmHg at 25 °\degree° C.

Define the term "colligative" in relation to the properties of a solution and list four colligative properties.

Which solution, if either, would create the higher osmotic pressure compared to pure water): one prepared from 1.0 g of NaCl in 10 mL of water or one prepared from 1.0 g of CsBr in 10 mL of water?

Henry's law constant for oxygen dissolving in blood is 3.74 *10-2 mol/L . atm at body temperature, 37C.Calculate the molar concentration of oxygen in blood for a free diver where the air pressure is 3.0 atm.The mole fraction of oxygen in air is 0.209.

A solution is prepared by adding 0.300 mol of glucose, which is not volatile, to 4.50 mol of water.What is the vapor pressure of this solution at 25 °\degree° C given that the vapor pressure of pure water is 23.8 torr?

Indicate which aqueous solution has the lowest vapor pressure.

The normal freezing point of benzene (C6H6, 78.12 g/mol) is 5.49 °\degree° C, and its Kf value is 5.12 °\degree° C/m.To create a solution with a freezing point of 0.00 °\degree° C, how many grams of naphthalene (C10H8, 128.2 g/mol) would need to be dissolved in 640.0 g of benzene?

You wish to de-ice your driveway, so you consider buying 10 lb of NaCl, 10 lb of CaCl2, or 10 lb of MgCl2.Which of these would de-ice your driveway most effectively? Assume that ideal dissociation of the salts occurs and that colligative properties are the only consideration.

A 15.0 mg sample of a protein was dissolved in water to produce 5.00 mL of solution at 25.1 °\degree° C.The osmotic pressure of this solution was measured and found to be 6.50 torr.What is the molar mass of this protein?

Which of the following statements regarding solutions and the van 't Hoff factor is NOT correct?

What would be the freezing point of a 1.50 m solution of NaNO3 in water? (Kf = 1.86 °\degree° C)

A 0.512 g sample of an unknown nondissociating solute was dissolved in 25.0 g of camphor (Kf = 39.7 °\degree° C/m), decreasing the freezing point of camphor by 3.07 °\degree° C.What is the molar mass of the solute?

How does the presence of solutes raise the boiling point of a solvent?

Identify the following statement as true or false and choose the correct explanation: "For solutions with the same molarity at the same temperature, the pressure needed for reverse osmosis of a sodium chloride solution will always be less than the pressure needed for a calcium chloride solution."

A solution is prepared by mixing 45.68 g of carbon disulfide (CS2, 76.13 g/mol) with 16.42 g of acetonitrile (CH3CN, 41.06 g/mol).What is the mole fraction of CS2 in the vapor phase at 25 °\degree° C?

Which statement regarding the boiling of a mixture of liquids A and B is NOT correct?

What is the vapor pressure of an aqueous solution that has a solute mole fraction of χ\chiχ =0.200? The vapor pressure of water is 25.756 mmHg at 25 °\degree° C.

The normal boiling point of ammonia is -33.34 °\degree° C, and its enthalpy of vaporization is 23.35 kJ/mol.What pressure would have to be applied for ammonia to boil at 25.00 °\degree° C?

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Atomic Structure Explaining the Properties of Elements

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Stoichiometry Mass Relationships and Chemical Reactions

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Additional Aqueous Equilibria Chemistry and the Oceans

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

Filters

The vapor pressure of an aqueous solution is found to be 24.9 mmHg at 25 $\degree$ C.What is the mole fraction of solute in this solution? The vapor pressure of water is 25.756 mmHg at 25 $\degree$ C.

A solution is prepared by adding 0.300 mol of glucose, which is not volatile, to 4.50 mol of water.What is the vapor pressure of this solution at 25 $\degree$ C given that the vapor pressure of pure water is 23.8 torr?

The normal freezing point of benzene (C₆H₆, 78.12 g/mol) is 5.49 $\degree$ C, and its K_f value is 5.12 $\degree$ C/m.To create a solution with a freezing point of 0.00 $\degree$ C, how many grams of naphthalene (C₁₀H₈, 128.2 g/mol) would need to be dissolved in 640.0 g of benzene?

You wish to de-ice your driveway, so you consider buying 10 lb of NaCl, 10 lb of CaCl₂, or 10 lb of MgCl₂.Which of these would de-ice your driveway most effectively? Assume that ideal dissociation of the salts occurs and that colligative properties are the only consideration.

A 15.0 mg sample of a protein was dissolved in water to produce 5.00 mL of solution at 25.1 $\degree$ C.The osmotic pressure of this solution was measured and found to be 6.50 torr.What is the molar mass of this protein?

What would be the freezing point of a 1.50 m solution of NaNO₃ in water? (K_f = 1.86 $\degree$ C)

A 0.512 g sample of an unknown nondissociating solute was dissolved in 25.0 g of camphor (K_f = 39.7 $\degree$ C/m), decreasing the freezing point of camphor by 3.07 $\degree$ C.What is the molar mass of the solute?

What is the vapor pressure of an aqueous solution that has a solute mole fraction of $\chi$ =0.200? The vapor pressure of water is 25.756 mmHg at 25 $\degree$ C.

The normal boiling point of ammonia is -33.34 $\degree$ C, and its enthalpy of vaporization is 23.35 kJ/mol.What pressure would have to be applied for ammonia to boil at 25.00 $\degree$ C?