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Introductory Chemistry: A Foundati...

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

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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. Calculate the hydrogen ion concentration and the pH of each of the following solutions of strong acids.

a. 1.4 × 10 3 M  HClO 4

b. 3.0 × 10 5 M  HCl

c. 5.0 × 10 2 M  HNO 3 d. 0.0010 M HCl

Interpretation Introduction

(a)

Interpretation:

The hydrogen ion concentration and pH of given solutions of strong acids should be calculated.

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=logH+

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=logOH

Here, OH is concentration of hydroxide ion.

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

pH+pOH=14.

Explanation

Given Information:

The concentration of strong acid, HClO4 is 1.4×103 M.

Calculation:

The dissociation reaction of the acid is as follows:

HClO4H++ClO4

Thus, if the concentration of HClO4 is 1.4×103 M thus, hydrogen ion concentration will be 1

Interpretation Introduction

(b)

Interpretation:

The hydrogen ion concentration and pH of given solutions of strong acids should be calculated.

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=logH+

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=logOH

Here, OH is concentration of hydroxide ion.

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

pH+pOH=14.

Interpretation Introduction

(c)

Interpretation:

The hydrogen ion concentration and pH of given solutions of strong acids should be calculated.

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=logH+

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=logOH

Here, OH is concentration of hydroxide ion.

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

pH+pOH=14.

Interpretation Introduction

(d)

Interpretation:

The hydrogen ion concentration and pH of given solutions of strong acids should be calculated.

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=logH+

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=logOH

Here, OH is concentration of hydroxide ion.

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

pH+pOH=14.

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