Introductory Chemistry: A Foundati...

9th Edition

Steven S. Zumdahl + 1 other

ISBN: 9781337399425

Textbook Problem

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. Calculate the pH corresponding to each of the following hydroxide ion concentrations, and indicate whether each solution is acidic or basic.

a. [ OH - ] = 4.85 × 10 − 5 M b. [ OH - ] = 3.96 × 10 − 7 M

c. [ OH − ] = 1.22 × 10 − 10 M d. [ OH - ] = 5.33 × 10 − 12 M

Interpretation Introduction

(a)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

Concept Introduction:

The concentration of hydrogen ions in a solution determines the acidity of a solution. If concentration of hydrogen ion is more than the solution is more acetic, if it is low, solution is less acidic.

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

pH=−log[H+]

Here, [H+] is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

pOH=−log[OH−]

Here, [OH−] is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

pH+pOH=14

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

9.69, Basic.

Given Information:

The hydroxide ion concentration is 4.85×10−5 M

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

pOH=−log[OH−]

Putting the values,

pOH=−log(4.85×10−5)=4.31

The pH of solution is calculated as follows:

pH=14−pOH

Putting the values,

pH=14−4.31=9.69

Since, the pH of solution is more than 7 thus, the solution is basic in nature.

(b)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

Concept Introduction:

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

pH=−log[H+]

Here, [H+] is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

pOH=−log[OH−]

Here, [OH−] is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

pH+pOH=14

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

7.6, Basic.

Given Information:

The hydroxide ion concentration is 3.96×10−7 M

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

pOH=−log[OH−]

Putting the values,

pOH=−log(3.96×10−7)=6.40

The pH of solution is calculated as follows:

pH=14−pOH

Putting the values,

pH=14−6.40=7.6

Since, the pH of solution is more than 7 thus, the solution is basic in nature.

(c)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

Concept Introduction:

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

pH=−log[H+]

Here, [H+] is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

pOH=−log[OH−]

Here, [OH−] is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

pH+pOH=14

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

4.09, Acidic.

Given Information:

The hydroxide ion concentration is 1.22×10−10 M

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

pOH=−log[OH−]

Putting the values,

pOH=−log(1.22×10−10)=9.91

The pH of solution is calculated as follows:

pH=14−pOH

Putting the values,

pH=14−9.91=4.09

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

(d)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

Concept Introduction:

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

pH=−log[H+]

Here, [H+] is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

pOH=−log[OH−]

Here, [OH−] is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

pH+pOH=14

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

2.7, Acidic.

Given Information:

The hydroxide ion concentration is 5.33×10−12 M

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

pOH=−log[OH−]

Putting the values,

pOH=−log(5.33×10−12)=11.3

The pH of solution is calculated as follows:

pH=14−pOH

Putting the values,

pH=14−11.3=2.7

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

Explanation

Given Information:

The hydroxide ion concentration is 4.85×10−5 M

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

pOH=−log[OH−]

Putting the values,

pOH=−log(4

Interpretation Introduction

(b)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

Concept Introduction:

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

pH=−log[H+]

Here, [H+] is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

pOH=−log[OH−]

Here, [OH−] is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

pH+pOH=14

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

7.6, Basic.

Given Information:

The hydroxide ion concentration is 3.96×10−7 M

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

pOH=−log[OH−]

Putting the values,

pOH=−log(3.96×10−7)=6.40

The pH of solution is calculated as follows:

pH=14−pOH

Putting the values,

pH=14−6.40=7.6

Since, the pH of solution is more than 7 thus, the solution is basic in nature.

(c)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

Concept Introduction:

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

pH=−log[H+]

Here, [H+] is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

pOH=−log[OH−]

Here, [OH−] is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

pH+pOH=14

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

4.09, Acidic.

Given Information:

The hydroxide ion concentration is 1.22×10−10 M

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

pOH=−log[OH−]

Putting the values,

pOH=−log(1.22×10−10)=9.91

The pH of solution is calculated as follows:

pH=14−pOH

Putting the values,

pH=14−9.91=4.09

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

(d)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

Concept Introduction:

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

pH=−log[H+]

Here, [H+] is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

pOH=−log[OH−]

Here, [OH−] is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

pH+pOH=14

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

2.7, Acidic.

Given Information:

The hydroxide ion concentration is 5.33×10−12 M

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

pOH=−log[OH−]

Putting the values,

pOH=−log(5.33×10−12)=11.3

The pH of solution is calculated as follows:

pH=14−pOH

Putting the values,

pH=14−11.3=2.7

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

Interpretation Introduction

(c)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

Concept Introduction:

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

pH=−log[H+]

Here, [H+] is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

pOH=−log[OH−]

Here, [OH−] is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

pH+pOH=14

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

4.09, Acidic.

Given Information:

The hydroxide ion concentration is 1.22×10−10 M

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

pOH=−log[OH−]

Putting the values,

pOH=−log(1.22×10−10)=9.91

The pH of solution is calculated as follows:

pH=14−pOH

Putting the values,

pH=14−9.91=4.09

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

(d)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

Concept Introduction:

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

pH=−log[H+]

Here, [H+] is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

pOH=−log[OH−]

Here, [OH−] is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

pH+pOH=14

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

2.7, Acidic.

Given Information:

The hydroxide ion concentration is 5.33×10−12 M

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

pOH=−log[OH−]

Putting the values,

pOH=−log(5.33×10−12)=11.3

The pH of solution is calculated as follows:

pH=14−pOH

Putting the values,

pH=14−11.3=2.7

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

Interpretation Introduction

(d)

Interpretation:

The pH of solution should be calculated. If the solution is acidic, neutral or basic should be indicated.

Concept Introduction:

The pH of solution is defined as negative log of hydrogen ion concentration thus, it can be calculated as follows:

pH=−log[H+]

Here, [H+] is concentration of hydrogen ion.

Similarly, pOH of a solution is defined as negative log of hydroxide ion concentration thus, it can be calculated as follows:

pOH=−log[OH−]

Here, [OH−] is concentration of hydroxide ion.

pH and pOH of a solution are related to each other as follows:

pH+pOH=14

In a pH scale, if the value of pH is below 7 the solution is said to be acidic in nature, if the Ph value is above 7 it is said to be basic in nature. At pH 7, the solution is neutral.

2.7, Acidic.

Given Information:

The hydroxide ion concentration is 5.33×10−12 M

Calculation:

From the given hydroxide ion concentration, pOH of solution can be calculated as follows:

pOH=−log[OH−]

Putting the values,

pOH=−log(5.33×10−12)=11.3

The pH of solution is calculated as follows:

pH=14−pOH

Putting the values,

pH=14−11.3=2.7

Since, the pH of solution is less than 7 thus, the solution is acidic in nature.

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Sect-16.1 P-16.1SC Sect-16.2 P-1CT Sect-16.3 P-16.2SC Sect-16.4 P-16.3SC Sect-16.4 P-1CT Sect-16.4 P-16.4SC Sect-16.4 P-16.5SC Sect-16.4 P-16.6SC Sect-16.5 P-16.7SC Ch-16 P-1ALQ

Ch-16 P-2ALQ Ch-16 P-3ALQ Ch-16 P-4ALQ Ch-16 P-5ALQ Ch-16 P-6ALQ Ch-16 P-7ALQ Ch-16 P-8ALQ Ch-16 P-9ALQ Ch-16 P-10ALQ Ch-16 P-11ALQ Ch-16 P-12ALQ Ch-16 P-13ALQ Ch-16 P-14ALQ Ch-16 P-15ALQ Ch-16 P-16ALQ Ch-16 P-17ALQ Ch-16 P-1QAP Ch-16 P-2QAP Ch-16 P-3QAP Ch-16 P-4QAP Ch-16 P-5QAP Ch-16 P-6QAP Ch-16 P-7QAP Ch-16 P-8QAP Ch-16 P-9QAP Ch-16 P-10QAP Ch-16 P-11QAP Ch-16 P-12QAP Ch-16 P-13QAP Ch-16 P-14QAP Ch-16 P-15QAP Ch-16 P-16QAP Ch-16 P-17QAP Ch-16 P-18QAP Ch-16 P-19QAP Ch-16 P-20QAP Ch-16 P-21QAP Ch-16 P-22QAP Ch-16 P-23QAP Ch-16 P-24QAP Ch-16 P-25QAP Ch-16 P-26QAP Ch-16 P-27QAP Ch-16 P-28QAP Ch-16 P-29QAP Ch-16 P-30QAP Ch-16 P-31QAP Ch-16 P-32QAP Ch-16 P-33QAP Ch-16 P-34QAP Ch-16 P-35QAP Ch-16 P-36QAP Ch-16 P-37QAP Ch-16 P-38QAP Ch-16 P-39QAP Ch-16 P-40QAP Ch-16 P-41QAP Ch-16 P-42QAP Ch-16 P-43QAP Ch-16 P-44QAP Ch-16 P-45QAP Ch-16 P-46QAP Ch-16 P-47QAP Ch-16 P-48QAP Ch-16 P-49QAP Ch-16 P-50QAP Ch-16 P-51QAP Ch-16 P-52QAP Ch-16 P-53QAP Ch-16 P-54QAP Ch-16 P-55QAP Ch-16 P-56QAP Ch-16 P-57QAP Ch-16 P-58QAP Ch-16 P-59QAP Ch-16 P-60QAP Ch-16 P-61QAP Ch-16 P-62QAP Ch-16 P-63QAP Ch-16 P-64QAP Ch-16 P-65AP Ch-16 P-66AP Ch-16 P-67AP Ch-16 P-68AP Ch-16 P-69AP Ch-16 P-70AP Ch-16 P-71AP Ch-16 P-72AP Ch-16 P-73AP Ch-16 P-74AP Ch-16 P-75AP Ch-16 P-76AP Ch-16 P-77AP Ch-16 P-78AP Ch-16 P-79AP Ch-16 P-80AP Ch-16 P-81AP Ch-16 P-82AP Ch-16 P-83AP Ch-16 P-84AP Ch-16 P-85AP Ch-16 P-86AP Ch-16 P-87AP Ch-16 P-88AP Ch-16 P-89AP Ch-16 P-90AP Ch-16 P-91AP Ch-16 P-92AP Ch-16 P-93AP Ch-16 P-94AP Ch-16 P-95AP Ch-16 P-96AP Ch-16 P-97AP Ch-16 P-98AP Ch-16 P-99AP Ch-16 P-100AP Ch-16 P-101AP Ch-16 P-102AP Ch-16 P-103AP Ch-16 P-104AP Ch-16 P-105AP Ch-16 P-106CP Ch-16 P-107CP Ch-16 P-108CP

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ScienceChemistryIntroductory Chemistry: A Foundation9th Edition

Introductory Chemistry: A Foundati...

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Introductory Chemistry: A Foundati...

. Calculate the pH corresponding to each of the following hydroxide ion concentrations, and indicate whether each solution is acidic or basic. a. [ OH - ] = 4.85 × 10 − 5 M b. [ OH - ] = 3.96 × 10 − 7 M c. [ OH − ] = 1.22 × 10 − 10 M d. [ OH - ] = 5.33 × 10 − 12 M

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Chemistry Introductory Chemistry: A Foundation 9th Edition

. Calculate the pH corresponding to each of the following hydroxide ion concentrations, and indicate whether each solution is acidic or basic.

a. [ OH - ] = 4.85 × 10 − 5 M b. [ OH - ] = 3.96 × 10 − 7 M

c. [ OH − ] = 1.22 × 10 − 10 M d. [ OH - ] = 5.33 × 10 − 12 M

The and _ systems work together to move the body and specific body parts.