   Chapter 16, Problem 107CP ### 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
1 views

# . Complete the table for each of the following solutions: [H+] pH pOH [OH-] 0.000 M HNO3 _____ _____ _____ _____ 3.0 M KOH _____ _____ _____ _____

Interpretation Introduction

Interpretation:

The given table should be completed.

 H+ pH pOH OH− 0.0070 M HNO3 3.0 M KOH

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

The concentration of acid is 0.0070 M. Since, it is a strong acid, it can dissociate completely into hydrogen ion and conjugate base as follows:

HNO3H++NO3

Thus, concentration of hydrogen ion will be 0.0070 M

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

pH=logH+

Putting the value,

pH=log0.0070=2.15

From the pH, pOH can be calculated as follows:

pOH=14pH

Putting the value,

pOH=142.15=11.85

Now, from pOH, hydroxide ion concentration can be calculated as follows:

OH=10pOH

Putting the value,

OH=1011.85=1.41×1012 M

Similarly, the strong base is given KOH with concentration 3

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