Chemistry: The Molecular Nature of Matter and Change
Chemistry: The Molecular Nature of Matter and Change
8th Edition
ISBN: 9781259631757
Author: Martin Silberberg Dr., Patricia Amateis Professor
Publisher: McGraw-Hill Education
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Chapter 13, Problem 13.34P

(a)

Interpretation Introduction

Interpretation:

Whether Na+ or Cs+ has greater ΔHhydration is to be determined.

Concept introduction:

The charge density is defined as the ratio of ionic charge and volume. It is directly proportional to the ionic charge and inversely proportional to the ionic volume. Volume is directly related to the ionic size. Smaller ion will have the charge spread over a small space so charge density will be more and vice-versa.

The enthalpy change of hydration is the enthalpy change when one mole of the ionic species is dissolved in water to give a solution of infinite dilution. It is represented by ΔHhydration. It is always negative.

ΔHhydration is directly related to the charge density on an ion. Higher the charge density, more will be ΔHhydration and vice-versa.

(a)

Expert Solution
Check Mark

Answer to Problem 13.34P

Na+ will have a greater ΔHhydration.

Explanation of Solution

Both sodium and cesium are present in the same period of the periodic table. But sodium lies above cesium so its ionic volume is less than that of cesium and therefore Na+ will have higher charge density than that of Cs+. So ΔHhydration of Na+ is more than that of Cs+.

Conclusion

ΔHhydration depends on the charge density of the ions.

(b)

Interpretation Introduction

Interpretation:

Whether Sr2+ or Rb+ has greater ΔHhydration is to be determined.

Concept introduction:

The charge density is defined as the ratio of ionic charge and volume. It is directly proportional to the ionic charge and inversely proportional to the ionic volume. Volume is directly related to the ionic size. Smaller ion will have the charge spread over a small space so charge density will be more and vice-versa.

The enthalpy change of hydration is the enthalpy change when one mole of the ionic species is dissolved in water to give a solution of infinite dilution. It is represented by ΔHhydration. It is always negative.

ΔHhydration is directly related to the charge density on an ion. Higher the charge density, more will be ΔHhydration and vice-versa.

(b)

Expert Solution
Check Mark

Answer to Problem 13.34P

Sr2+ will have a greater ΔHhydration.

Explanation of Solution

Both rubidium and strontium are present in the same period of the periodic table. But strontium lies to the right of rubidium so its size and therefore volume are small. Also, the charge on Sr2+ is more than that of Rb+. So the charge density of Sr2+ is more than that of Rb+ and therefore ΔHhydration of Sr2+ is more than that of Rb+.

Conclusion

ΔHhydration depends on the charge density of the ions.

(c)

Interpretation Introduction

Interpretation:

Whether Na+ or Cl has greater ΔHhydration is to be determined.

Concept introduction:

The charge density is defined as the ratio of ionic charge and volume. It is directly proportional to the ionic charge and inversely proportional to the ionic volume. Volume is directly related to the ionic size. Smaller ion will have the charge spread over a small space so charge density will be more and vice-versa.

The enthalpy change of hydration is the enthalpy change when one mole of the ionic species is dissolved in water to give a solution of infinite dilution. It is represented by ΔHhydration. It is always negative.

ΔHhydration is directly related to the charge density on an ion. Higher the charge density, more will be ΔHhydration and vice-versa.

(c)

Expert Solution
Check Mark

Answer to Problem 13.34P

Na+ will have a greater ΔHhydration.

Explanation of Solution

Both sodium and chlorine are present in the same period of the periodic table. But cations are smaller than anions so the charge density of Na+ is greater than that of Cl and ΔHhydration of Na+ is greater than that of Cl.

Conclusion

ΔHhydration depends on the charge density of the ions.

(d)

Interpretation Introduction

Interpretation:

Whether O2 or F has greater ΔHhydration is to be determined.

Concept introduction:

The charge density is defined as the ratio of ionic charge and volume. It is directly proportional to the ionic charge and inversely proportional to the ionic volume. Volume is directly related to the ionic size. Smaller ion will have the charge spread over a small space so charge density will be more and vice-versa.

The enthalpy change of hydration is the enthalpy change when one mole of the ionic species is dissolved in water to give a solution of infinite dilution. It is represented by ΔHhydration. It is always negative.

ΔHhydration is directly related to the charge density on an ion. Higher the charge density, more will be ΔHhydration and vice-versa.

(d)

Expert Solution
Check Mark

Answer to Problem 13.34P

O2 will have a greater ΔHhydration.

Explanation of Solution

O2 has a greater ionic charge as compared to F. But both the ions have similar ionic volume. So O2 will have a higher charge density than that of F and therefore ΔHhydration of O2 is greater than that of F.

Conclusion

ΔHhydration depends on the charge density of the ions.

(e)

Interpretation Introduction

Interpretation:

Whether OH or SH has greater ΔHhydration is to be determined.

Concept introduction:

The charge density is defined as the ratio of ionic charge and volume. It is directly proportional to the ionic charge and inversely proportional to the ionic volume. Volume is directly related to the ionic size. Smaller ion will have the charge spread over a small space so charge density will be more and vice-versa.

The enthalpy change of hydration is the enthalpy change when one mole of the ionic species is dissolved in water to give a solution of infinite dilution. It is represented by ΔHhydration. It is always negative.

ΔHhydration is directly related to the charge density on an ion. Higher the charge density, more will be ΔHhydration and vice-versa.

(e)

Expert Solution
Check Mark

Answer to Problem 13.34P

OH will have a greater ΔHhydration.

Explanation of Solution

Oxygen and sulfur are present in the same group of the periodic table. But oxygen lies above sulfur so its size and therefore volume is smaller than that of sulfur. So the charge density of OH is larger than that of SH and therefore ΔHhydration of OH is greater than that of SH

Conclusion

ΔHhydration depends on the charge density of the ions.

(f)

Interpretation Introduction

Interpretation:

Whether Mg2+ or Ba2+ has greater ΔHhydration is to be determined.

Concept introduction:

The charge density is defined as the ratio of ionic charge and volume. It is directly proportional to the ionic charge and inversely proportional to the ionic volume. Volume is directly related to the ionic size. Smaller ion will have the charge spread over a small space so charge density will be more and vice-versa.

The enthalpy change of hydration is the enthalpy change when one mole of the ionic species is dissolved in water to give a solution of infinite dilution. It is represented by ΔHhydration. It is always negative.

ΔHhydration is directly related to the charge density on an ion. Higher the charge density, more will be ΔHhydration and vice-versa.

(f)

Expert Solution
Check Mark

Answer to Problem 13.34P

Mg2+ will have a greater ΔHhydration.

Explanation of Solution

Magnesium and barium are present in the same group of the periodic table. But magnesium lies above barium so its size, as well as volume, is smaller than that of barium. So the charge density of Mg2+ is greater than that of Ba2+ and therefore ΔHhydration of Mg2+ is greater than that of Ba2+.

Conclusion

ΔHhydration depends on the charge density of the ions.

(g)

Interpretation Introduction

Interpretation:

Whether Mg2+ or Na+ has greater ΔHhydration is to be determined.

Concept introduction:

The charge density is defined as the ratio of ionic charge and volume. It is directly proportional to the ionic charge and inversely proportional to the ionic volume. Volume is directly related to the ionic size. Smaller ion will have the charge spread over a small space so charge density will be more and vice-versa.

The enthalpy change of hydration is the enthalpy change when one mole of the ionic species is dissolved in water to give a solution of infinite dilution. It is represented by ΔHhydration. It is always negative.

ΔHhydration is directly related to the charge density on an ion. Higher the charge density, more will be ΔHhydration and vice-versa.

(g)

Expert Solution
Check Mark

Answer to Problem 13.34P

Mg2+ will have a greater ΔHhydration.

Explanation of Solution

The ionic charge of Mg2+ is greater than that of Na+. Also, the volume of Mg2+ is also smaller than that of Na+. So the charge density of Mg2+ is greater than that of Na+ and therefore ΔHhydration of Mg2+ is greater than that of Na+.

Conclusion

ΔHhydration depends on the charge density of the ions.

(h)

Interpretation Introduction

Interpretation:

Whether CO32 or NO3 has greater ΔHhydration is to be determined.

Concept introduction:

The charge density is defined as the ratio of ionic charge and volume. It is directly proportional to the ionic charge and inversely proportional to the ionic volume. Volume is directly related to the ionic size. Smaller ion will have the charge spread over a small space so charge density will be more and vice-versa.

The enthalpy change of hydration is the enthalpy change when one mole of the ionic species is dissolved in water to give a solution of infinite dilution. It is represented by ΔHhydration. It is always negative.

ΔHhydration is directly related to the charge density on an ion. Higher the charge density, more will be ΔHhydration and vice-versa.

(h)

Expert Solution
Check Mark

Answer to Problem 13.34P

CO32 will have a greater ΔHhydration.

Explanation of Solution

The ionic charge of CO32 is greater than that of NO3. Also, the volume of CO32 is also smaller than that of NO3. So the charge density of CO32 is greater than that of NO3 and therefore ΔHhydration of CO32 is greater than that of NO3.

Conclusion

ΔHhydration depends on the charge density of the ions.

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Chapter 13 Solutions

Chemistry: The Molecular Nature of Matter and Change

Ch. 13.5 - Prob. 13.6AFPCh. 13.5 - Prob. 13.6BFPCh. 13.6 - Calculate the vapor pressure lowering of a...Ch. 13.6 - Prob. 13.7BFPCh. 13.6 - Prob. 13.8AFPCh. 13.6 - Prob. 13.8BFPCh. 13.6 - Prob. 13.9AFPCh. 13.6 - Prob. 13.9BFPCh. 13.6 - A solution is made by dissolving 31.2 g of...Ch. 13.6 - Prob. 13.10BFPCh. 13.7 - Prob. B13.1PCh. 13.7 - Prob. B13.2PCh. 13 - Prob. 13.1PCh. 13 - Prob. 13.2PCh. 13 - Prob. 13.3PCh. 13 - Which would you expect to be more effective as a...Ch. 13 - Prob. 13.5PCh. 13 - Prob. 13.6PCh. 13 - Prob. 13.7PCh. 13 - Prob. 13.8PCh. 13 - Prob. 13.9PCh. 13 - Prob. 13.10PCh. 13 - Prob. 13.11PCh. 13 - What is the strongest type of intermolecular force...Ch. 13 - Prob. 13.13PCh. 13 - Prob. 13.14PCh. 13 - Prob. 13.15PCh. 13 - Prob. 13.16PCh. 13 - Prob. 13.17PCh. 13 - Prob. 13.18PCh. 13 - Prob. 13.19PCh. 13 - Prob. 13.20PCh. 13 - Prob. 13.21PCh. 13 - Prob. 13.22PCh. 13 - Prob. 13.23PCh. 13 - What is the relationship between solvation and...Ch. 13 - Prob. 13.25PCh. 13 - Prob. 13.26PCh. 13 - Prob. 13.27PCh. 13 - Prob. 13.28PCh. 13 - Prob. 13.29PCh. 13 - Prob. 13.30PCh. 13 - Prob. 13.31PCh. 13 - Prob. 13.32PCh. 13 - Prob. 13.33PCh. 13 - Prob. 13.34PCh. 13 - Prob. 13.35PCh. 13 - Use the following data to calculate the combined...Ch. 13 - Use the following data to calculate the combined...Ch. 13 - State whether the entropy of the system increases...Ch. 13 - Prob. 13.39PCh. 13 - Prob. 13.40PCh. 13 - Prob. 13.41PCh. 13 - Prob. 13.42PCh. 13 - Prob. 13.43PCh. 13 - Prob. 13.44PCh. 13 - For a saturated aqueous solution of each of the...Ch. 13 - Prob. 13.46PCh. 13 - Prob. 13.47PCh. 13 - Prob. 13.48PCh. 13 - Prob. 13.49PCh. 13 - Prob. 13.50PCh. 13 - Prob. 13.51PCh. 13 - Prob. 13.52PCh. 13 - Prob. 13.53PCh. 13 - Prob. 13.54PCh. 13 - Prob. 13.55PCh. 13 - Calculate the molarity of each aqueous...Ch. 13 - Calculate the molarity of each aqueous...Ch. 13 - Prob. 13.58PCh. 13 - Calculate the molarity of each aqueous...Ch. 13 - How would you prepare the following aqueous...Ch. 13 - Prob. 13.61PCh. 13 - Prob. 13.62PCh. 13 - Prob. 13.63PCh. 13 - Prob. 13.64PCh. 13 - Prob. 13.65PCh. 13 - Prob. 13.66PCh. 13 - Prob. 13.67PCh. 13 - Prob. 13.68PCh. 13 - Prob. 13.69PCh. 13 - Prob. 13.70PCh. 13 - Prob. 13.71PCh. 13 - Prob. 13.72PCh. 13 - Prob. 13.73PCh. 13 - Prob. 13.74PCh. 13 - Prob. 13.75PCh. 13 - Prob. 13.76PCh. 13 - Prob. 13.77PCh. 13 - Prob. 13.78PCh. 13 - Prob. 13.79PCh. 13 - Prob. 13.80PCh. 13 - Prob. 13.81PCh. 13 - What are the most important differences between...Ch. 13 - Prob. 13.83PCh. 13 - Prob. 13.84PCh. 13 - Prob. 13.85PCh. 13 - Prob. 13.86PCh. 13 - Prob. 13.87PCh. 13 - Prob. 13.88PCh. 13 - Classify each substance as a strong electrolyte,...Ch. 13 - Prob. 13.90PCh. 13 - Prob. 13.91PCh. 13 - Which solution has the lower freezing point? 11.0...Ch. 13 - Prob. 13.93PCh. 13 - Prob. 13.94PCh. 13 - Prob. 13.95PCh. 13 - Prob. 13.96PCh. 13 - Prob. 13.97PCh. 13 - Prob. 13.98PCh. 13 - Prob. 13.99PCh. 13 - The boiling point of ethanol (C2H5OH) is 78.5°C....Ch. 13 - Prob. 13.101PCh. 13 - Prob. 13.102PCh. 13 - Prob. 13.103PCh. 13 - Prob. 13.104PCh. 13 - Prob. 13.105PCh. 13 - Prob. 13.106PCh. 13 - Prob. 13.107PCh. 13 - Prob. 13.108PCh. 13 - Prob. 13.109PCh. 13 - Prob. 13.110PCh. 13 - Prob. 13.111PCh. 13 - In a study designed to prepare new...Ch. 13 - The U.S. Food and Drug Administration lists...Ch. 13 - Prob. 13.114PCh. 13 - Prob. 13.115PCh. 13 - Prob. 13.116PCh. 13 - In a movie theater, you can see the beam of...Ch. 13 - Prob. 13.118PCh. 13 - Prob. 13.119PCh. 13 - Prob. 13.120PCh. 13 - Prob. 13.121PCh. 13 - Gold occurs in seawater at an average...Ch. 13 - Prob. 13.123PCh. 13 - Prob. 13.124PCh. 13 - Prob. 13.125PCh. 13 - Prob. 13.126PCh. 13 - Pyridine (right) is an essential portion of many...Ch. 13 - Prob. 13.128PCh. 13 - Prob. 13.129PCh. 13 - Prob. 13.130PCh. 13 - Prob. 13.131PCh. 13 - Prob. 13.132PCh. 13 - Prob. 13.133PCh. 13 - Prob. 13.134PCh. 13 - Prob. 13.135PCh. 13 - Prob. 13.136PCh. 13 - Prob. 13.137PCh. 13 - Prob. 13.138PCh. 13 - Prob. 13.139PCh. 13 - Prob. 13.140PCh. 13 - Prob. 13.141PCh. 13 - Prob. 13.142PCh. 13 - Prob. 13.143PCh. 13 - The release of volatile organic compounds into the...Ch. 13 - Although other solvents are available,...Ch. 13 - Prob. 13.146PCh. 13 - Prob. 13.147PCh. 13 - Prob. 13.148PCh. 13 - Prob. 13.149PCh. 13 - Prob. 13.150PCh. 13 - Prob. 13.151PCh. 13 - Suppose coal-fired power plants used water in...Ch. 13 - Urea is a white crystalline solid used as a...Ch. 13 - Prob. 13.154PCh. 13 - Prob. 13.155PCh. 13 - Prob. 13.156PCh. 13 - Prob. 13.157PCh. 13 - Prob. 13.158PCh. 13 - Prob. 13.159PCh. 13 - Prob. 13.160PCh. 13 - Prob. 13.161PCh. 13 - Prob. 13.162PCh. 13 - Figure 12.11 shows the phase changes of pure...Ch. 13 - KNO3, KClO3, KCl, and NaCl are recrystallized as...Ch. 13 - Prob. 13.165PCh. 13 - Prob. 13.166PCh. 13 - Prob. 13.167P
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