Question 1

The principal reason for the extremely low solubility of NaCl in benzene (C6H6)is the __________.

Accepted Answer

A) strong solvent-solvent interactions 
B) hydrogen bonding in C6H6 
C) strength of the covalent bond in NaCl 
D) weak solvation of Na+ and Cl- by C6H6 
E) increased disorder due to mixing of solute and solvent 
A) strong solvent-solvent interactions 
B) hydrogen bonding in C6H6 
C) strength of the covalent bond in NaCl 
D) weak solvation of Na+ and Cl- by C6H6 
E) increased disorder due to mixing of solute and solvent

Question 2

Formation of solutions where the process is endothermic can be spontaneous provided that __________.

Accepted Answer

A) they are accompanied by another process that is exothermic 
B) they are accompanied by an increase in order 
C) they are accompanied by an increase in disorder 
D) the solvent is a gas and the solute is a solid 
E) the solvent is water and the solute is a gas 
A) they are accompanied by another process that is exothermic 
B) they are accompanied by an increase in order 
C) they are accompanied by an increase in disorder 
D) the solvent is a gas and the solute is a solid 
E) the solvent is water and the solute is a gas

Question 3

The ideal value of i (van't Hoff factor)for (NH4)3PO4.

Accepted Answer

A) 1 
B) 2 
C) 3 
D) 4 
E) 5 
A) 1 
B) 2 
C) 3 
D) 4 
E) 5

Question 4

A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of -3.33°C. Given Kf = 1.86°C/m for water, the molar mass of the unknown liquid is ________g/mol.

Accepted Answer

A) 69.0 
B) 333 
C) 619 
D) 161 
E) 62.1 
A) 69.0 
B) 333 
C) 619 
D) 161 
E) 62.1

Question 5

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

Accepted Answer

A) 3.37 
B) 0.278 
C) 2.78 
D) 0.212 
E) The density of the solution is needed to solve the problem. 
A) 3.37 
B) 0.278 
C) 2.78 
D) 0.212 
E) The density of the solution is needed to solve the problem.

Question 6

The mole fraction of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C2H6O is __________ M. The density of the solution is 0.79 g/mL.

Accepted Answer

A) 0.027 
B) 0.034 
C) 0.028 
D) 0.035 
E) 0.151 
A) 0.027 
B) 0.034 
C) 0.028 
D) 0.035 
E) 0.151

Question 7

The concentration of HCl in a solution that is prepared by dissolving 5.5 g of HCl in 200 g of C2H6O is __________ molal.

Accepted Answer

A) 27.5 
B) 7.5 × 10-4 
C) 3.3 × 10-2 
D) 0.75 
E) 1.3 
A) 27.5 
B) 7.5 × 10-4 
C) 3.3 × 10-2 
D) 0.75 
E) 1.3

Question 8

Which of the following choices has the compounds correctly arranged in order of increasing solubility in water? (least soluble to most soluble)

Accepted Answer

A) CCl4 3 3 
B) CH3OH 4 4 3 3 
D) LiF 3 3 
E) CH3OH 4 3 
A) CCl4 3 3 
B) CH3OH 4 4 3 3 
D) LiF 3 3 
E) CH3OH 4 3

Question 9

The solubility of oxygen gas in water at 25°C and 1.0 atm pressure of oxygen is 0.041 g/L. The solubility of oxygen in water at 3.0 atm and 25°C is __________ g/L.

Accepted Answer

A) 0.041 
B) 0.014 
C) 0.31 
D) 0.12 
E) 3.0 
A) 0.041 
B) 0.014 
C) 0.31 
D) 0.12 
E) 3.0

Question 10

Molality is defined as the __________.

Accepted Answer

A) moles solute/moles solvent 
B) moles solute/liters solution 
C) moles solute/kg solution 
D) moles solute/kg solvent 
E) none (dimensionless) 
A) moles solute/moles solvent 
B) moles solute/liters solution 
C) moles solute/kg solution 
D) moles solute/kg solvent 
E) none (dimensionless)

Question 11

Which of the following liquids will have the highest freezing point?

Accepted Answer

A) pure H2O 
B) aqueous glucose (0.050 m) 
C) aqueous CoI2 (0.030 m) 
D) aqueous FeI3 (0.030 m) 
E) aqueous NaI (0.030 m) 
A) pure H2O 
B) aqueous glucose (0.050 m) 
C) aqueous CoI2 (0.030 m) 
D) aqueous FeI3 (0.030 m) 
E) aqueous NaI (0.030 m)

The principal reason for the extremely low solubility of NaCl in benzene (C₆H₆)is the __________.

Formation of solutions where the process is endothermic can be spontaneous provided that __________.

The ideal value of i (van't Hoff factor)for (NH₄)₃PO₄.

A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of -3.33°C. Given K_f = 1.86°C/m for water, the molar mass of the unknown liquid is ________g/mol.

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

The mole fraction of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C₂H₆O is __________ M. The density of the solution is 0.79 g/mL.

The concentration of HCl in a solution that is prepared by dissolving 5.5 g of HCl in 200 g of C₂H₆O is __________ molal.

Which of the following choices has the compounds correctly arranged in order of increasing solubility in water? (least soluble to most soluble)

The solubility of oxygen gas in water at 25°C and 1.0 atm pressure of oxygen is 0.041 g/L. The solubility of oxygen in water at 3.0 atm and 25°C is __________ g/L.

Molality is defined as the __________.

Which of the following liquids will have the highest freezing point?

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

Filters

Exam 13: Properties of Solutions

The principal reason for the extremely low solubility of NaCl in benzene (C6H6)is the __________.

Formation of solutions where the process is endothermic can be spontaneous provided that __________.

The ideal value of i (van't Hoff factor)for (NH4)3PO4.

A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of -3.33°C. Given Kf = 1.86°C/m for water, the molar mass of the unknown liquid is ________g/mol.

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

The mole fraction of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C2H6O is __________ M. The density of the solution is 0.79 g/mL.

The concentration of HCl in a solution that is prepared by dissolving 5.5 g of HCl in 200 g of C2H6O is __________ molal.

Which of the following choices has the compounds correctly arranged in order of increasing solubility in water? (least soluble to most soluble)

The solubility of oxygen gas in water at 25°C and 1.0 atm pressure of oxygen is 0.041 g/L. The solubility of oxygen in water at 3.0 atm and 25°C is __________ g/L.

Molality is defined as the __________.

Which of the following liquids will have the highest freezing point?

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

Filters

The principal reason for the extremely low solubility of NaCl in benzene (C₆H₆)is the __________.

The ideal value of i (van't Hoff factor)for (NH₄)₃PO₄.

A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of -3.33°C. Given K_f = 1.86°C/m for water, the molar mass of the unknown liquid is ________g/mol.

The mole fraction of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C₂H₆O is __________ M. The density of the solution is 0.79 g/mL.

The concentration of HCl in a solution that is prepared by dissolving 5.5 g of HCl in 200 g of C₂H₆O is __________ molal.