General Chemistry
General Chemistry
7th Edition
ISBN: 9780073402758
Author: Chang, Raymond/ Goldsby
Publisher: McGraw-Hill College
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Chapter 13, Problem 13.67QP

(a)

Interpretation Introduction

Interpretation:

Which of the given aqueous solution has higher boiling point, higher freezing point and the lower vapor pressure have to be explained.

Concept introduction

Boiling point is the temperature at which liquid turns into a gas. Example: boiling point of water i 100°C. That is water changes from liquid phase to gas phase.

ΔTb= Tb- Tb°

Where,

ΔTb Change in boiling point

Tb -  Boiling point of the solution

Tb° -  Boiling point of pure solvent

Boiling point elevation(ΔTb) is distinction between boiling point of the pure solvent (Tb°) and the boiling point of the solution (Tb).

ΔTb= Kbm

Where,

ΔTb Change in boiling point

Kb Molal boiling point constant

m- molality of the solution

Freezing point is the temperature at which liquid turns into solid.

Freezing point depression(ΔTf) is distinction between freezing point of the pure solvent (Tf°) and the freezing point of the solution (Tf).

ΔTf= Kfm

Where,

ΔTf Change in freezing point

Kf Molal freezing point constant

m- Molality of the solution

Vapor pressure is the pressure excreted by the molecules at the surface of the liquid in the closed container.

(a)

Expert Solution
Check Mark

Answer to Problem 13.67QP

CaCl2 Solution has higher boiling point

Explanation of Solution

Explanation ofCaCl2solution has higher boiling point than urea

CaCl2 is an ionic compound and thus strong electrolyte in water. We know that strong electrolytes completely dissociates in water (not form ion pair, van’t Hoff factor i=3).Hence the total concentration should be 1.05m (3× 0.35m) which larger value compared to concentration of Urea ( 0.90m ).More concentration shows that more particles of the solute in the solution. Therefore CaCl2 shows higher boiling point.

(b)

Interpretation Introduction

Interpretation:

Which of the given aqueous solution has higher boiling point, higher freezing point and the lower vapor pressure have to be explained.

Concept introduction

Boiling point is the temperature at which liquid turns into a gas. Example: boiling point of water is 100°C. That is water changes from liquid phase to gas phase.

ΔTb= Tb- Tb°

Where,

ΔTb Change in boiling point

Tb -  Boiling point of the solution

Tb° -  Boiling point of pure solvent

Boiling point elevation(ΔTb) is distinction between boiling point of the pure solvent (Tb°) and the boiling point of the solution (Tb).

ΔTb= Kbm

Where,

ΔTb Change in boiling point

Kb Molal boiling point constant

m- molality of the solution

Freezing point is the temperature at which liquid turns into solid.

Freezing point depression(ΔTf) is distinction between freezing point of the pure solvent (Tf°) and the freezing point of the solution (Tf).

ΔTf= Kfm

Where,

ΔTf Change in freezing point

Kf Molal freezing point constant

m- Molality of the solution

Vapor pressure is the pressure excreted by the molecules at the surface of the liquid in the closed container.

(b)

Expert Solution
Check Mark

Answer to Problem 13.67QP

CaCl2 has higher freezing point

Explanation of Solution

Explanation of Urea has higher freezing point depression thanCaCl2

Freezing point depends on the molality and van’t Hoff factor of the solute. In this case,

CaCl2 has more concentration( i = 3, 3× 0.35m = 1.05m) compare to Urea. So CaCl2 has highest freezing point depression.

(c)

Interpretation Introduction

Interpretation:

Which of the given aqueous solution has higher boiling point, higher freezing point and the lower vapor pressure have to be explained.

Concept introduction

Boiling point is the temperature at which liquid turns into a gas. Example: boiling point of water is 100°C. That is water changes from liquid phase to gas phase.

ΔTb= Tb- Tb°

Where,

ΔTb Change in boiling point

Tb -  Boiling point of the solution

Tb° -  Boiling point of pure solvent

Boiling point elevation(ΔTb) is distinction between boiling point of the pure solvent (Tb°) and the boiling point of the solution (Tb).

ΔTb= Kbm

Where,

ΔTb Change in boiling point

Kb Molal boiling point constant

m- molality of the solution

Freezing point is the temperature at which liquid turns into solid.

Freezing point depression(ΔTf) is distinction between freezing point of the pure solvent (Tf°) and the freezing point of the solution (Tf).

ΔTf= Kfm

Where,

ΔTf Change in freezing point

Kf Molal freezing point constant

m- Molality of the solution

Vapor pressure is the pressure excreted by the molecules at the surface of the liquid in the closed container.

(c)

Expert Solution
Check Mark

Answer to Problem 13.67QP

CaCl2 solution has lower vapor pressure

Explanation of Solution

Explanation of CaCl2has lower vapour pressure than urea

CaCl2 has lower vapour pressure because CaCl2 is an ionic compound and thus strong electrolyte in water. We know that strong electrolytes completely dissociates in water (not form ion pair, van’t Hoff factor i=3).Hence the total concentration should be 1.05m (3× 0.35m) which larger value compared to concentration of Urea ( 0.90m ) which is non-electrolyte.

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Chapter 13 Solutions

General Chemistry

Ch. 13.6 - Prob. 2PECh. 13.6 - Prob. 2RCCh. 13.6 - Prob. 3PECh. 13.6 - Prob. 4PECh. 13.6 - Prob. 3RCCh. 13.6 - Prob. 5PECh. 13.6 - Prob. 4RCCh. 13 - Prob. 13.1QPCh. 13 - Prob. 13.2QPCh. 13 - Prob. 13.3QPCh. 13 - 13.4 As you know, some solution processes are...Ch. 13 - Prob. 13.5QPCh. 13 - Prob. 13.6QPCh. 13 - Prob. 13.7QPCh. 13 - Prob. 13.8QPCh. 13 - 13.9 Arrange these compounds in order of...Ch. 13 - Prob. 13.10QPCh. 13 - Prob. 13.11QPCh. 13 - Prob. 13.12QPCh. 13 - Prob. 13.13QPCh. 13 - 13.14 Calculate the amount of water (in grams)...Ch. 13 - Prob. 13.15QPCh. 13 - Prob. 13.16QPCh. 13 - Prob. 13.17QPCh. 13 - 12.20 For dilute aqueous solutions in which the...Ch. 13 - Prob. 13.19QPCh. 13 - 13.20 The concentrated sulfuric acid we use in the...Ch. 13 - 13.21 Calculate the molarity and the molality of...Ch. 13 - 13.22 The density of an aqueous solution...Ch. 13 - Prob. 13.23QPCh. 13 - Prob. 13.25QPCh. 13 - 13.26 The solubility of KNO3 is 155 g per 100 g of...Ch. 13 - Prob. 13.27QPCh. 13 - Prob. 13.28QPCh. 13 - Prob. 13.29QPCh. 13 - Prob. 13.30QPCh. 13 - Prob. 13.31QPCh. 13 - 13.32 A man bought a goldfish in a pet shop. Upon...Ch. 13 - Prob. 13.33QPCh. 13 - 13.34 A miner working 260 m below sea level opened...Ch. 13 - Prob. 13.35QPCh. 13 - 13.36 The solubility of N2 in blood at 37°C and at...Ch. 13 - Prob. 13.37QPCh. 13 - Prob. 13.38QPCh. 13 - Prob. 13.39QPCh. 13 - 13.40 How is the lowering in vapor pressure...Ch. 13 - Prob. 13.41QPCh. 13 - Prob. 13.42QPCh. 13 - Prob. 13.43QPCh. 13 - Prob. 13.44QPCh. 13 - Prob. 13.45QPCh. 13 - Prob. 13.46QPCh. 13 - Prob. 13.47QPCh. 13 - 13.48 How many grams of sucrose (C12H22O11) must...Ch. 13 - Prob. 13.49QPCh. 13 - 13.50 The vapor pressures of ethanol (C2H5OH) and...Ch. 13 - Prob. 13.51QPCh. 13 - Prob. 13.52QPCh. 13 - 13.53 What are the boiling point and freezing...Ch. 13 - 13.54 An aqueous solution contains the amino acid...Ch. 13 - 13.55 Pheromones are compounds secreted by the...Ch. 13 - 12.58 The elemental analysis of an organic solid...Ch. 13 - Prob. 13.57QPCh. 13 - 13.58 A solution is prepared by condensing 4.00 L...Ch. 13 - Prob. 13.59QPCh. 13 - 13.60 A solution of 2.50 g of a compound of...Ch. 13 - Prob. 13.61QPCh. 13 - 13.62 A solution containing 0.8330 g of a protein...Ch. 13 - Prob. 13.63QPCh. 13 - 13.64 A solution of 6.85 g of a carbohydrate in...Ch. 13 - 13.65 Define ion pairs. What effect does ion-pair...Ch. 13 - Prob. 13.66QPCh. 13 - Prob. 13.67QPCh. 13 - Prob. 13.68QPCh. 13 - Prob. 13.69QPCh. 13 - Prob. 13.70QPCh. 13 - Prob. 13.71QPCh. 13 - 13.72 At 25°C the vapor pressure of pure water is...Ch. 13 - 13.73 Both NaCl and CaCl2 are used to melt ice on...Ch. 13 - Prob. 13.74QPCh. 13 - Prob. 13.75QPCh. 13 - Prob. 13.76QPCh. 13 - Prob. 13.77QPCh. 13 - Prob. 13.78QPCh. 13 - Prob. 13.79QPCh. 13 - Prob. 13.80QPCh. 13 - Prob. 13.81QPCh. 13 - Prob. 13.82QPCh. 13 - Prob. 13.83QPCh. 13 - Prob. 13.84QPCh. 13 - Prob. 13.85QPCh. 13 - Prob. 13.86QPCh. 13 - Prob. 13.87QPCh. 13 - Prob. 13.88QPCh. 13 - Prob. 13.89QPCh. 13 - Prob. 13.90QPCh. 13 - 13.91 Hydrogen peroxide with a concentration of...Ch. 13 - 13.92 Before a carbonated beverage bottle is...Ch. 13 - Prob. 13.93QPCh. 13 - 13.94 Explain each of these statements: (a) The...Ch. 13 - Prob. 13.95QPCh. 13 - Prob. 13.96QPCh. 13 - Prob. 13.97QPCh. 13 - Prob. 13.98QPCh. 13 - Prob. 13.99QPCh. 13 - Prob. 13.100QPCh. 13 - Prob. 13.101QPCh. 13 - Prob. 13.102QPCh. 13 - Prob. 13.103QPCh. 13 - Prob. 13.104QPCh. 13 - Prob. 13.105SPCh. 13 - Prob. 13.106SPCh. 13 - Prob. 13.107SPCh. 13 - Prob. 13.108SPCh. 13 - Prob. 13.109SPCh. 13 - Prob. 13.110SPCh. 13 - 13.111 A student carried out the following...Ch. 13 - Prob. 13.112SPCh. 13 - Prob. 13.113SPCh. 13 - Prob. 13.114SP
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Solutions: Crash Course Chemistry #27; Author: Crash Course;https://www.youtube.com/watch?v=9h2f1Bjr0p4;License: Standard YouTube License, CC-BY