A) is never positive (\(\Delta\)H°soln \(\le\) 0), because the solute-solvent attraction is never weaker than the combination of the solute-solute attraction and solvent-solvent attraction. B) is always positive (\(\Delta\)H°soln > 0), because the solute-solvent attraction is always weaker than the combination of the solute-solute attraction and solvent-solvent attraction. C) is always zero (\(\Delta\)H°soln = 0), because the solute-solvent attraction is defined as the average of the solute-solute attraction and solvent-solvent attraction. D) is always negative (\(\Delta\)H°soln < 0), because the solute-solvent attraction is always stronger than the combination of the solute-solute attraction and solvent-solvent attraction. E) may be positive, zero, or negative, depending on the relative strength of the solute-solvent, solute-solute, and solvent-solvent attractive forces. A) is never positive (\(\Delta\)H°soln \(\le\) 0), because the solute-solvent attraction is never weaker than the combination of the solute-solute attraction and solvent-solvent attraction. B) is always positive (\(\Delta\)H°soln > 0), because the solute-solvent attraction is always weaker than the combination of the solute-solute attraction and solvent-solvent attraction. C) is always zero (\(\Delta\)H°soln = 0), because the solute-solvent attraction is defined as the average of the solute-solute attraction and solvent-solvent attraction. D) is always negative (\(\Delta\)H°soln < 0), because the solute-solvent attraction is always stronger than the combination of the solute-solute attraction and solvent-solvent attraction. E) may be positive, zero, or negative, depending on the relative strength of the solute-solvent, solute-solute, and solvent-solvent attractive forces.

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C2H6O2)and 85.0 g H2O? Kf of water is 1.86°C/m.

A) 17.6°C B) -176°C C) -1.50°C D) 1.50°C E) -17.6°C A) 17.6°C B) -176°C C) -1.50°C D) 1.50°C E) -17.6°C

A solution is 40.0% by volume benzene (C6H6)in carbon tetrachloride at 20°C. The vapor pressure of pure benzene at this temperature is 74.61 mmHg and its density is 0.87865 g/cm3; the vapor pressure of pure carbon tetrachloride is 91.32 mmHg and its density is 1.5940 g/cm3. If this solution is ideal, its total vapor pressure at 20°C is

A) 84.64 mmHg. B) 84.30 mmHg. C) 82.96 mmHg. D) 81.63 mmHg. E) 165.93 mmHg. A) 84.64 mmHg. B) 84.30 mmHg. C) 82.96 mmHg. D) 81.63 mmHg. E) 165.93 mmHg.

A 20.0 % by mass solution of phosphoric acid (H3PO4)in water has a density of 1.114 g/mL at 20°C. What is the molarity of this solution?

A) 0.0114 M B) 0.0568 M C) 0.114 M D) 2.27 M E) 11.4 M A) 0.0114 M B) 0.0568 M C) 0.114 M D) 2.27 M E) 11.4 M

Exam 13: Physical Properties of Solutions

How many grams of propanol (C₃H₇OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

(Short Answer)

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Question 61

Determine the mass percent HCl in a 1.2 M solution of hydrochloric acid with a density of 1.019 g/mL?

(Multiple Choice)

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Question 62

An aqueous fructose solution having a density of 1.049 g/cm³ is found to have an osmotic pressure of 17.0 atm at 25°C. Find the temperature at which this solution freezes. [Given: for water K_f = 1.86 °C/m; molecular mass of fructose = 180.16 g/mol]

(Multiple Choice)

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Question 63

An organic compound was prepared and purified by chromatography. A conductivity measurement showed the compound to be a nonelectrolyte. Elemental analysis gave an empirical formula of CH₃O. A 0.127 g sample of the compound was dissolved in water and diluted to 100.0 mL, and the osmotic pressure of that solution was determined to 0.492 atm at 20°C. Determine the molar mass and molecular formula of the compound. (R = 0.0821 L.atm/K.mol)

(Essay)

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Question 64

Heat of solution

(Multiple Choice)

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Question 65

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C₂H₆O₂)and 85.0 g H₂O? K_f of water is 1.86°C/m.

(Multiple Choice)

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Question 66

At 10°C one volume of water dissolves 3.10 volumes of chlorine gas at 1.00 atm pressure. What is the Henry's Law constant in mol/L·atm?

(Multiple Choice)

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Question 67

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C₁₂H₂₂O₁₁.

(Short Answer)

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Question 68

What is the molarity and molality of a solution that is 10.00 % by mass potassium hydrogen carbonate (KHCO₃, 100.11 g/mol)and has a density of 1.0650 g/mL?

(Short Answer)

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Question 69

The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7 * 10^{- 4} mol/L. What is the value of the Henry's Law constant in mol/L·atm?

(Multiple Choice)

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Question 70

It has been suggested that gold might be recovered from seawater. If seawater contains about 4.0 * 10^-9 g/L of dissolved gold, how many liters of seawater would have to be processed to get 1.00 ounce of gold? (1 oz = 28.4 g)

(Essay)

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Question 71

Which of the following has the greater molal concentration (molality)?

(Multiple Choice)

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Question 72

Arrange the following aqueous solutions in order of increasing boiling points: 0.050 m Mg(NO₃)₂; 0.100 m ethanol; 0.090 m NaCl.

(Multiple Choice)

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Question 73

For dilute aqueous solutions, the concentration units molarity and molality have almost the same values.

(True/False)

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Question 74

A solution is 40.0% by volume benzene (C₆H₆)in carbon tetrachloride at 20°C. The vapor pressure of pure benzene at this temperature is 74.61 mmHg and its density is 0.87865 g/cm³; the vapor pressure of pure carbon tetrachloride is 91.32 mmHg and its density is 1.5940 g/cm³. If this solution is ideal, its total vapor pressure at 20°C is

(Multiple Choice)

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Question 75

A 20.0 % by mass solution of phosphoric acid (H₃PO₄)in water has a density of 1.114 g/mL at 20°C. What is the molarity of this solution?

(Multiple Choice)

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Question 76

Define solvation.

(Short Answer)

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Question 77

What is the mole fraction of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

(Short Answer)

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Question 78

For water K_f = 1.86°C/m. Therefore, the freezing points of 1.0 M aqueous KCl and C₂H₅OH (ethanol)solutions are the same.

(True/False)

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Question 79

Plasma is the fluid portion of blood. The concentration of acetylsalicylic acid (aspirin, C₉H₈O₄, molar mass = 180. g/mol)in your plasma is found to be 2.99 * 10^-4 M after you take two tablets of aspirin. If the volume of your plasma is 5.85 L, what is the molality, m, of aspirin in your blood? (Assume density of plasma is 1.00 g/mL.)

(Essay)

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Question 80

Showing 61 - 80 of 109

How many grams of propanol (C₃H₇OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

Determine the mass percent HCl in a 1.2 M solution of hydrochloric acid with a density of 1.019 g/mL?

An aqueous fructose solution having a density of 1.049 g/cm³ is found to have an osmotic pressure of 17.0 atm at 25°C. Find the temperature at which this solution freezes. [Given: for water K_f = 1.86 °C/m; molecular mass of fructose = 180.16 g/mol]

Heat of solution

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C₂H₆O₂)and 85.0 g H₂O? K_f of water is 1.86°C/m.

At 10°C one volume of water dissolves 3.10 volumes of chlorine gas at 1.00 atm pressure. What is the Henry's Law constant in mol/L·atm?

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C₁₂H₂₂O₁₁.

What is the molarity and molality of a solution that is 10.00 % by mass potassium hydrogen carbonate (KHCO₃, 100.11 g/mol)and has a density of 1.0650 g/mL?

The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7 * 10^{- 4} mol/L. What is the value of the Henry's Law constant in mol/L·atm?

It has been suggested that gold might be recovered from seawater. If seawater contains about 4.0 * 10^-9 g/L of dissolved gold, how many liters of seawater would have to be processed to get 1.00 ounce of gold? (1 oz = 28.4 g)

Which of the following has the greater molal concentration (molality)?

Arrange the following aqueous solutions in order of increasing boiling points: 0.050 m Mg(NO₃)₂; 0.100 m ethanol; 0.090 m NaCl.

For dilute aqueous solutions, the concentration units molarity and molality have almost the same values.

A 20.0 % by mass solution of phosphoric acid (H₃PO₄)in water has a density of 1.114 g/mL at 20°C. What is the molarity of this solution?

Define solvation.

What is the mole fraction of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

For water K_f = 1.86°C/m. Therefore, the freezing points of 1.0 M aqueous KCl and C₂H₅OH (ethanol)solutions are the same.

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

Exam 13: Physical Properties of Solutions

How many grams of propanol (C3H7OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

Determine the mass percent HCl in a 1.2 M solution of hydrochloric acid with a density of 1.019 g/mL?

An aqueous fructose solution having a density of 1.049 g/cm3 is found to have an osmotic pressure of 17.0 atm at 25°C. Find the temperature at which this solution freezes. [Given: for water Kf = 1.86 °C/m; molecular mass of fructose = 180.16 g/mol]

Heat of solution

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C2H6O2)and 85.0 g H2O? Kf of water is 1.86°C/m.

At 10°C one volume of water dissolves 3.10 volumes of chlorine gas at 1.00 atm pressure. What is the Henry's Law constant in mol/L·atm?

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C12H22O11.

What is the molarity and molality of a solution that is 10.00 % by mass potassium hydrogen carbonate (KHCO3, 100.11 g/mol)and has a density of 1.0650 g/mL?

The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7 * 10 - 4 mol/L. What is the value of the Henry's Law constant in mol/L·atm?

It has been suggested that gold might be recovered from seawater. If seawater contains about 4.0 * 10-9 g/L of dissolved gold, how many liters of seawater would have to be processed to get 1.00 ounce of gold? (1 oz = 28.4 g)

Which of the following has the greater molal concentration (molality)?

Arrange the following aqueous solutions in order of increasing boiling points: 0.050 m Mg(NO3)2; 0.100 m ethanol; 0.090 m NaCl.

For dilute aqueous solutions, the concentration units molarity and molality have almost the same values.

A 20.0 % by mass solution of phosphoric acid (H3PO4)in water has a density of 1.114 g/mL at 20°C. What is the molarity of this solution?

Define solvation.

What is the mole fraction of sodium phosphate in a 0.142 M Na3PO4(aq)solution that has a density of 1.015 g/mL?

For water Kf = 1.86°C/m. Therefore, the freezing points of 1.0 M aqueous KCl and C2H5OH (ethanol)solutions are the same.

Introduction

Atoms, Molecules, and Ions

Stoichiometry

Reactions in Aqueous Solution

Gases

Energy Relationships in Chemical Reactions

The Electronic Structure of Atoms

The Periodic Table

Chemical Bonding I: the Covalent Bond

Chemical Bonding Ii: Molecular Geometry and Hybridization of Atomic Orbitals

Introduction to Organic Chemistry

Intermolecular Forces and Liquids and Solids

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Thermodynamics

Redox Reactions and Electrochemistry

The Chemistry of Coordination Compounds

Nuclear Chemistry

Organic Polymerssynthetic and Natural

Filters

How many grams of propanol (C₃H₇OH, 60.10 g/mol)would be needed to make 750 mL of a solution with an osmotic pressure of 25 atm at 25°C? (R = 0.0821 L.atm/K.mol)

An aqueous fructose solution having a density of 1.049 g/cm³ is found to have an osmotic pressure of 17.0 atm at 25°C. Find the temperature at which this solution freezes. [Given: for water K_f = 1.86 °C/m; molecular mass of fructose = 180.16 g/mol]

What is the freezing point of a solution prepared from 50.0 g ethylene glycol (C₂H₆O₂)and 85.0 g H₂O? K_f of water is 1.86°C/m.

Calculate the mass of solute in the following solution: 50.0 mL of 0.0300 M C₁₂H₂₂O₁₁.

What is the molarity and molality of a solution that is 10.00 % by mass potassium hydrogen carbonate (KHCO₃, 100.11 g/mol)and has a density of 1.0650 g/mL?

The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7 * 10^{- 4} mol/L. What is the value of the Henry's Law constant in mol/L·atm?

It has been suggested that gold might be recovered from seawater. If seawater contains about 4.0 * 10^-9 g/L of dissolved gold, how many liters of seawater would have to be processed to get 1.00 ounce of gold? (1 oz = 28.4 g)

Arrange the following aqueous solutions in order of increasing boiling points: 0.050 m Mg(NO₃)₂; 0.100 m ethanol; 0.090 m NaCl.

A 20.0 % by mass solution of phosphoric acid (H₃PO₄)in water has a density of 1.114 g/mL at 20°C. What is the molarity of this solution?

What is the mole fraction of sodium phosphate in a 0.142 M Na₃PO₄(aq)solution that has a density of 1.015 g/mL?

For water K_f = 1.86°C/m. Therefore, the freezing points of 1.0 M aqueous KCl and C₂H₅OH (ethanol)solutions are the same.