(a) Interpretation: The value of K f for cyclohexane should be determined. Concept introduction: Freezing point depression of a solvent occurs due to the addition of nonvolatile solute. The amount that the freezing point is lowered is proportional to the mole fraction of the solute. In dilute solutions, solute mole fraction is equal to its molality. The freezing point depression can be determined by Δ T f = − K f × m Δ T f - freezing point depression ( 0 C) K f - proportionality constant ( 0 C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent) m − molality (mol/kg)

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Answer 1

Question

Chapter 14, Problem 71E

Interpretation Introduction

(a)

Interpretation:

The value of K_f for cyclohexane should be determined.

Concept introduction:

Freezing point depression of a solvent occurs due to the addition of nonvolatile solute. The amount that the freezing point is lowered is proportional to the mole fraction of the solute. In dilute solutions, solute mole fraction is equal to its molality. The freezing point depression can be determined by

ΔTf=−Kf×m

ΔTf - freezing point depression (⁰C)

Kf - proportionality constant ( ⁰C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent)

m − molality (mol/kg)

Interpretation Introduction

(b)

Interpretation:

The better solvent for molar mass determinations by freezing point depression should be determined.

Concept introduction:

The freezing point depression can be used to determine molar mass of an unknown compound. The freezing point depression can be determined by

ΔTf=−Kf×m

ΔTf - freezing point depression (⁰C)

Kf - proportionality constant (⁰C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent)

m − molality (mol/kg)

K_f indicates the extent of the depression of freezing point per 1 molal solution.

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Answer 2

Question

Chapter 14, Problem 71E

Interpretation Introduction

(a)

Interpretation:

The value of K_f for cyclohexane should be determined.

Concept introduction:

Freezing point depression of a solvent occurs due to the addition of nonvolatile solute. The amount that the freezing point is lowered is proportional to the mole fraction of the solute. In dilute solutions, solute mole fraction is equal to its molality. The freezing point depression can be determined by

ΔTf=−Kf×m

ΔTf - freezing point depression (⁰C)

Kf - proportionality constant ( ⁰C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent)

m − molality (mol/kg)

Interpretation Introduction

(b)

Interpretation:

The better solvent for molar mass determinations by freezing point depression should be determined.

Concept introduction:

The freezing point depression can be used to determine molar mass of an unknown compound. The freezing point depression can be determined by

ΔTf=−Kf×m

ΔTf - freezing point depression (⁰C)

Kf - proportionality constant (⁰C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent)

m − molality (mol/kg)

K_f indicates the extent of the depression of freezing point per 1 molal solution.

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Answer 3

Question

Chapter 14, Problem 71E

Interpretation Introduction

(a)

Interpretation:

The value of K_f for cyclohexane should be determined.

Concept introduction:

Freezing point depression of a solvent occurs due to the addition of nonvolatile solute. The amount that the freezing point is lowered is proportional to the mole fraction of the solute. In dilute solutions, solute mole fraction is equal to its molality. The freezing point depression can be determined by

ΔTf=−Kf×m

ΔTf - freezing point depression (⁰C)

Kf - proportionality constant ( ⁰C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent)

m − molality (mol/kg)

Interpretation Introduction

(b)

Interpretation:

The better solvent for molar mass determinations by freezing point depression should be determined.

Concept introduction:

The freezing point depression can be used to determine molar mass of an unknown compound. The freezing point depression can be determined by

ΔTf=−Kf×m

ΔTf - freezing point depression (⁰C)

Kf - proportionality constant (⁰C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent)

m − molality (mol/kg)

K_f indicates the extent of the depression of freezing point per 1 molal solution.

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Answer 4

Question

Chapter 14, Problem 71E

Interpretation Introduction

(a)

Interpretation:

The value of K_f for cyclohexane should be determined.

Concept introduction:

Freezing point depression of a solvent occurs due to the addition of nonvolatile solute. The amount that the freezing point is lowered is proportional to the mole fraction of the solute. In dilute solutions, solute mole fraction is equal to its molality. The freezing point depression can be determined by

ΔTf=−Kf×m

ΔTf - freezing point depression (⁰C)

Kf - proportionality constant ( ⁰C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent)

m − molality (mol/kg)

Interpretation Introduction

(b)

Interpretation:

The better solvent for molar mass determinations by freezing point depression should be determined.

Concept introduction:

The freezing point depression can be used to determine molar mass of an unknown compound. The freezing point depression can be determined by

ΔTf=−Kf×m

ΔTf - freezing point depression (⁰C)

Kf - proportionality constant (⁰C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent)

m − molality (mol/kg)

K_f indicates the extent of the depression of freezing point per 1 molal solution.

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Answer 5

Chapter 14, Problem 71E

Interpretation Introduction

(a)

Interpretation:

The value of K_f for cyclohexane should be determined.

Concept introduction:

Freezing point depression of a solvent occurs due to the addition of nonvolatile solute. The amount that the freezing point is lowered is proportional to the mole fraction of the solute. In dilute solutions, solute mole fraction is equal to its molality. The freezing point depression can be determined by

ΔTf=−Kf×m

ΔTf - freezing point depression (⁰C)

Kf - proportionality constant ( ⁰C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent)

m − molality (mol/kg)

Interpretation Introduction

(b)

Interpretation:

The better solvent for molar mass determinations by freezing point depression should be determined.

Concept introduction:

The freezing point depression can be used to determine molar mass of an unknown compound. The freezing point depression can be determined by

ΔTf=−Kf×m

ΔTf - freezing point depression (⁰C)

Kf - proportionality constant (⁰C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent)

m − molality (mol/kg)

K_f indicates the extent of the depression of freezing point per 1 molal solution.

Answer 6

Chapter 14, Problem 71E

Interpretation Introduction

(a)

Interpretation:

The value of K_f for cyclohexane should be determined.

Concept introduction:

Freezing point depression of a solvent occurs due to the addition of nonvolatile solute. The amount that the freezing point is lowered is proportional to the mole fraction of the solute. In dilute solutions, solute mole fraction is equal to its molality. The freezing point depression can be determined by

ΔTf=−Kf×m

ΔTf - freezing point depression (⁰C)

Kf - proportionality constant ( ⁰C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent)

m − molality (mol/kg)

Answer 7

Chapter 14, Problem 71E

Interpretation Introduction

(a)

Interpretation:

The value of K_f for cyclohexane should be determined.

Concept introduction:

Freezing point depression of a solvent occurs due to the addition of nonvolatile solute. The amount that the freezing point is lowered is proportional to the mole fraction of the solute. In dilute solutions, solute mole fraction is equal to its molality. The freezing point depression can be determined by

ΔTf=−Kf×m

ΔTf - freezing point depression (⁰C)

Kf - proportionality constant ( ⁰C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent)

m − molality (mol/kg)

Answer 8

Interpretation Introduction

(b)

Interpretation:

The better solvent for molar mass determinations by freezing point depression should be determined.

Concept introduction:

The freezing point depression can be used to determine molar mass of an unknown compound. The freezing point depression can be determined by

ΔTf=−Kf×m

ΔTf - freezing point depression (⁰C)

Kf - proportionality constant (⁰C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent)

m − molality (mol/kg)

K_f indicates the extent of the depression of freezing point per 1 molal solution.

Answer 9

Interpretation Introduction

(b)

Interpretation:

The better solvent for molar mass determinations by freezing point depression should be determined.

Concept introduction:

The freezing point depression can be used to determine molar mass of an unknown compound. The freezing point depression can be determined by

ΔTf=−Kf×m

ΔTf - freezing point depression (⁰C)

Kf - proportionality constant (⁰C mol-1 kg) (depends on melting point, enthalpy of fusion, molar mass of the solvent)

m − molality (mol/kg)

K_f indicates the extent of the depression of freezing point per 1 molal solution.

Answer 10

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Answer 11

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Answer 12

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Answer 13

Ch. 14 - Which of the following do you expect to be most...Ch. 14 - Which of the following is moderately soluble both...Ch. 14 - Substances that dissolve in water generally do not...Ch. 14 - Prob. 4E Ch. 14 - Two of the substances listed here highly soluble...Ch. 14 - Benzoic acid, C8H8COOH, is much more soluble in...Ch. 14 - Prob. 7E Ch. 14 - Explain the observation that all metal nitrates...Ch. 14 - A saturated aqueous solution of NaBr at 20C...Ch. 14 - Prob. 10E

Solution Summary: The author explains that the value of K f for cyclohexane should be determined. Freezing point depression occurs due to the addition of nonvolatile solute.

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