The freezing points of sodium chloride and calcium chloride has the compared and the reason why one of these solutions has lower freezing point has to be explained. Concept Introduction: Colligative properties depend on the number of solute particles in the solution. “i” is the number of particles that the solute will dissociate upon mixing with the solvent. With the help of molality of a solution and the number of particles a compound will dissolve to form, it is possible to predict the solution with lowest freezing point. General steps: 1) Each solute has to be labeled as ionic or covalent. 2) Determine the number of ions in the formula, if the solute is ionic. 3) Multiply the molality of the solution by the number of particles formed when the solution dissolves. This gives the total concentration of particles dissolved. 4) Higher the concentration, lower the freezing point.

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Answer 1

Question

Chapter 12, Problem 12.15QE

Interpretation Introduction

Interpretation:

The freezing points of sodium chloride and calcium chloride has the compared and the reason why one of these solutions has lower freezing point has to be explained.

Concept Introduction:

Colligative properties depend on the number of solute particles in the solution.

“i” is the number of particles that the solute will dissociate upon mixing with the solvent. With the help of molality of a solution and the number of particles a compound will dissolve to form, it is possible to predict the solution with lowest freezing point.

General steps:

1) Each solute has to be labeled as ionic or covalent.

2) Determine the number of ions in the formula, if the solute is ionic.

3) Multiply the molality of the solution by the number of particles formed when the solution dissolves. This gives the total concentration of particles dissolved.

4) Higher the concentration, lower the freezing point.

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Answer 2

Question

Chapter 12, Problem 12.15QE

Interpretation Introduction

Interpretation:

The freezing points of sodium chloride and calcium chloride has the compared and the reason why one of these solutions has lower freezing point has to be explained.

Concept Introduction:

Colligative properties depend on the number of solute particles in the solution.

“i” is the number of particles that the solute will dissociate upon mixing with the solvent. With the help of molality of a solution and the number of particles a compound will dissolve to form, it is possible to predict the solution with lowest freezing point.

General steps:

1) Each solute has to be labeled as ionic or covalent.

2) Determine the number of ions in the formula, if the solute is ionic.

3) Multiply the molality of the solution by the number of particles formed when the solution dissolves. This gives the total concentration of particles dissolved.

4) Higher the concentration, lower the freezing point.

Expert Solution & Answer

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Check out a sample textbook solution

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Answer 3

Question

Chapter 12, Problem 12.15QE

Interpretation Introduction

Interpretation:

The freezing points of sodium chloride and calcium chloride has the compared and the reason why one of these solutions has lower freezing point has to be explained.

Concept Introduction:

Colligative properties depend on the number of solute particles in the solution.

“i” is the number of particles that the solute will dissociate upon mixing with the solvent. With the help of molality of a solution and the number of particles a compound will dissolve to form, it is possible to predict the solution with lowest freezing point.

General steps:

1) Each solute has to be labeled as ionic or covalent.

2) Determine the number of ions in the formula, if the solute is ionic.

3) Multiply the molality of the solution by the number of particles formed when the solution dissolves. This gives the total concentration of particles dissolved.

4) Higher the concentration, lower the freezing point.

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Answer 4

Question

Chapter 12, Problem 12.15QE

Interpretation Introduction

Interpretation:

The freezing points of sodium chloride and calcium chloride has the compared and the reason why one of these solutions has lower freezing point has to be explained.

Concept Introduction:

Colligative properties depend on the number of solute particles in the solution.

“i” is the number of particles that the solute will dissociate upon mixing with the solvent. With the help of molality of a solution and the number of particles a compound will dissolve to form, it is possible to predict the solution with lowest freezing point.

General steps:

1) Each solute has to be labeled as ionic or covalent.

2) Determine the number of ions in the formula, if the solute is ionic.

3) Multiply the molality of the solution by the number of particles formed when the solution dissolves. This gives the total concentration of particles dissolved.

4) Higher the concentration, lower the freezing point.

Expert Solution & Answer

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Answer 5

Chapter 12, Problem 12.15QE

Interpretation Introduction

Interpretation:

The freezing points of sodium chloride and calcium chloride has the compared and the reason why one of these solutions has lower freezing point has to be explained.

Concept Introduction:

Colligative properties depend on the number of solute particles in the solution.

“i” is the number of particles that the solute will dissociate upon mixing with the solvent. With the help of molality of a solution and the number of particles a compound will dissolve to form, it is possible to predict the solution with lowest freezing point.

General steps:

1) Each solute has to be labeled as ionic or covalent.

2) Determine the number of ions in the formula, if the solute is ionic.

3) Multiply the molality of the solution by the number of particles formed when the solution dissolves. This gives the total concentration of particles dissolved.

4) Higher the concentration, lower the freezing point.

Answer 6

Chapter 12, Problem 12.15QE

Interpretation Introduction

Interpretation:

The freezing points of sodium chloride and calcium chloride has the compared and the reason why one of these solutions has lower freezing point has to be explained.

Concept Introduction:

Colligative properties depend on the number of solute particles in the solution.

“i” is the number of particles that the solute will dissociate upon mixing with the solvent. With the help of molality of a solution and the number of particles a compound will dissolve to form, it is possible to predict the solution with lowest freezing point.

General steps:

1) Each solute has to be labeled as ionic or covalent.

2) Determine the number of ions in the formula, if the solute is ionic.

3) Multiply the molality of the solution by the number of particles formed when the solution dissolves. This gives the total concentration of particles dissolved.

4) Higher the concentration, lower the freezing point.

Answer 7

Chapter 12, Problem 12.15QE

Interpretation Introduction

Interpretation:

The freezing points of sodium chloride and calcium chloride has the compared and the reason why one of these solutions has lower freezing point has to be explained.

Concept Introduction:

Colligative properties depend on the number of solute particles in the solution.

“i” is the number of particles that the solute will dissociate upon mixing with the solvent. With the help of molality of a solution and the number of particles a compound will dissolve to form, it is possible to predict the solution with lowest freezing point.

General steps:

1) Each solute has to be labeled as ionic or covalent.

2) Determine the number of ions in the formula, if the solute is ionic.

3) Multiply the molality of the solution by the number of particles formed when the solution dissolves. This gives the total concentration of particles dissolved.

4) Higher the concentration, lower the freezing point.

Answer 8

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Answer 10

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Answer 11

Ch. 12 - Prob. 12.1QE Ch. 12 - Prob. 12.2QE Ch. 12 - Prob. 12.3QE Ch. 12 - Prob. 12.4QE Ch. 12 - Prob. 12.5QE Ch. 12 - Prob. 12.6QE Ch. 12 - Prob. 12.7QE Ch. 12 - Prob. 12.8QE Ch. 12 - Prob. 12.9QE Ch. 12 - Prob. 12.10QE

Solution Summary: The author explains the freezing points of sodium chloride and calcium chlorides. Colligative properties depend on the number of solute particles in the solution.

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