EBK INTRODUCTION TO CHEMISTRY
EBK INTRODUCTION TO CHEMISTRY
5th Edition
ISBN: 9781260162165
Author: BAUER
Publisher: MCGRAW HILL BOOK COMPANY
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Chapter 13, Problem 74QP

(a)

Interpretation Introduction

Interpretation:

Concentration of H3O+ and OH and pOH for pH=0.40 is to be found, and nature of solution is to be determined.

(a)

Expert Solution
Check Mark

Explanation of Solution

pH of a solution gives the concentration of hydrogen ions in that solution. Range of pH values is from 0 to 14 . Solutions having pH values less than 7 are acidic, those having greater than 7 are basic. Solutions with pH=7 are neutral. pOH of a solution gives the concentration of OH ions in that solution.

Concentration of H3O+ can be found using pH as follows:

pH=logH3O+

Substitute, 0.40 for pH in the above equation

0.40=logH3O+

Taking antilog on both sides and solving above equation, H3O+=0.40 .

The relation between pH and pOH is as follows:

pH+pOH=14

Substitute, 0.40 for pH in the above equation.

0.40+pOH=14pOH=140.40pOH=13.60

Concentration of OH can be found using pOH as follows:

pOH=logOH

Substitute, 13.60 for pOH in the above equation.

13.60=logOH

Taking antilog on both sides and solving above equation, OH=2.5×1014 .

As the pH is less than 7 , so the solution is acidic in nature.

Therefore, H3O+=0.40 , OH=2.5×1014 and pOH=13.60 for the given value of pH , and the nature of the solution is acidic.

(b)

Interpretation Introduction

Interpretation:

Concentration of H3O+ , pH and pOH for OH=9.0×1010 is to be found, and nature of solution is to be determined.

(b)

Expert Solution
Check Mark

Explanation of Solution

Ionic product of water is defined as the product of concentration of H+ and OH ions present in the water. It is represented as Kw .

Expression for Kw is as follows:

Kw=H3O+OH

Here, Kw is the ionic product of water, H3O+ is the concentration of H3O+ ions and OH is the concentration of OH ions.

Substitute, 9.0×1010 for OH and 1.0×1014 for Kw in the above equation.

1.0×1014=H3O+9.0×1010H3O+=1.0×10149.0×1010H3O+=1.1×105

pH of a solution gives the concentration of hydrogen ions in that solution. Range of pH values is from 0 to 14 . Solutions having pH values less than 7 are acidic, those having greater than 7 are basic. Solutions with pH=7 are neutral. pOH of a solution gives the concentration of OH ions in that solution.

pOH can be found using concentration of OH as follows:

pOH=logOH

Substitute, 9.0×1010 for OH in the above equation.

pOH=log9.0×1010pOH=9.05

The relation between pH and pOH is as follows:

pH+pOH=14

Substitute, 9.05 for pOH in the above equation.

pH+9.05=14pH=149.05pH=4.95

As the pH is less than 7 , so the solution is acidic in nature.

Therefore, H3O+=1.1×105 , pOH=9.05 and pH=4.95 for the given value of OH , and the nature of the solution is acidic.

(c)

Interpretation Introduction

Interpretation:

Concentration of OH , pH and pOH for H3O+=1.0×108 is to be found and, nature of solution is to be determined.

(c)

Expert Solution
Check Mark

Explanation of Solution

Ionic product of water is defined as the product of concentration of H+ and OH ions present in the water. It is represented as Kw .

Expression for Kw is as follows:

Kw=H3O+OH

Here, Kw is the ionic product of water, H3O+ is the concentration of H3O+ ions and OH is the concentration of OH ions.

Substitute, 1.0×108 for H3O+ and 1.0×1014 for Kw in the above equation.

1.0×1014=1.0×108OHOH=1.0×10141.0×108OH=1.0×106

pH of a solution gives the concentration of hydrogen ions in that solution. Range of pH values is from 0 to 14 . Solutions having pH values less than 7 are acidic, those having greater than 7 are basic. Solutions with pH=7 are neutral. pOH of a solution gives the concentration of OH ions in that solution.

pOH can be found using concentration of OH as follows:

pOH=logOH

Substitute, 1.0×106 for OH in the above equation.

pOH=log1.0×106pOH=6

The relation between pH and pOH is as follows:

pH+pOH=14

Substitute, 6 for pOH in the above equation.

pH+6=14pH=146pH=8

As the pH is more than 7 , so the solution is basic in nature.

Therefore, OH=1.0×106 , pOH=6 and pH=8 for the given value of H3O+ and the nature of the solution is basic.

(d)

Interpretation Introduction

Interpretation:

Concentration of H3O+ and OH and pH for pOH=2 is to be found, and nature of solution is to be determined.

(d)

Expert Solution
Check Mark

Explanation of Solution

pH of a solution gives the concentration of hydrogen ions in that solution. Range of pH values is from 0 to 14 . Solutions having pH values less than 7 are acidic, those having greater than 7 are basic. Solutions with pH=7 are neutral. pOH of a solution gives the concentration of OH ions in that solution.

Concentration of OH can be found using pOH as follows:

pOH=logOH

Substitute, 2 for pOH in the above equation.

2.00=logOH

Taking antilog on both sides and solving above equation, OH=1.0×102 .

The relation between pH and pOH is as follows:

pH+pOH=14

Substitute, 2 for pOH in the above equation.

pH+2=14limxpH=142pH=12

As the pH is more than 7 , so the solution is basic in nature.

Concentration of H3O+ can be found using pH as follows:

pH=logH3O+

Substitute, 12 for pH in the above equation

12=logH3O+

Taking antilog on both sides and solving above equation, H3O+=1.0×1012 .

Therefore, H3O+=1.0×1012 , OH=1.0×102 and pH=12 for the given value of pOH , and the nature of the solution is basic.

(e)

Interpretation Introduction

Interpretation:

Concentration of OH , pH and pOH for H3O+=4.5×102 is to be found and, nature of solution is to be determined.

(e)

Expert Solution
Check Mark

Explanation of Solution

Ionic product of water is defined as the product of concentration of H+ and OH ions present in the water. It is represented as Kw .

Expression for Kw is as follows:

Kw=H3O+OH

Here, Kw is the ionic product of water, H3O+ is the concentration of H3O+ ions and OH is the concentration of OH ions.

Substitute, 4.5×102 for H3O+ and 1.0×1014 for Kw in the above equation.

1.0×1014=4.5×102OHOH=1.0×10144.5×102OH=2.2×1013

pH of a solution gives the concentration of hydrogen ions in that solution. Range of pH values is from 0 to 14 . Solutions having pH values less than 7 are acidic, those having greater than 7 are basic. Solutions with pH=7 are neutral. pOH of a solution gives the concentration of OH ions in that solution.

pOH can be found using concentration of OH as follows:

pOH=logOH

Substitute, 2.2×1013 for OH in the above equation.

pOH=log2.2×1013pOH=12.65

The relation between pH and pOH is as follows:

pH+pOH=14

Substitute, 12.65 for pOH in the above equation.

pH+12.65=14pH=1412.65pH=1.35

As the pH is less than 7 , so the solution is acidic in nature.

Therefore, OH=2.2×1013 , pOH=12.65 and pH=1.35 for the given value of H3O+ , and the nature of the solution is acidic.

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Chapter 13 Solutions

EBK INTRODUCTION TO CHEMISTRY

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