   Chapter 16, Problem 48QAP ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

#### Solutions

Chapter
Section ### Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
8 views

# . For each hydrogen ion concentration listed, calculate the pH of the solution as well as the concentration of hydroxide ion in the solution. Indicate whether each solution is acidic or basic. a. [ H + ] = 1.91 × 10 − 2 M b. [ H + ] = 4.83 × 10 − 7 M c. [ H + ] = 8.92 × 10 − 11 M d. [ H + ] = 6.14 × 10 − 5 M

Interpretation Introduction

(a)

Interpretation:

The pH and concentration of hydroxide ion [OH] 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.

Explanation

Given Information:

The hydrogen ion concentration is 1.91×102 M

Calculation:

From the given hydrogen ion concentration, pH of solution can be calculated as follows:

pH=log[H+]

Putting the values,

pH=log(1.91×102)=1.72

From the pH, pOH of solution can be calculated as follows:

pOH=14pH

Putting the value,

pOH=141.72=12

Interpretation Introduction

(b)

Interpretation:

The pH and concentration of hydroxide ion [OH] 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.

Interpretation Introduction

(c)

Interpretation:

The pH and concentration of hydroxide ion [OH] 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.

Interpretation Introduction

(d)

Interpretation:

The pH and concentration of hydroxide ion [OH] 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.

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