   Chapter 16, Problem 82AP ### 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

# . A solution with pH = 9 has a (higher/lower) hydrogen ion concentration than a solution with pOH = 9.

Interpretation Introduction

Interpretation:

The hydrogen ion concentration of solution with pH 9 should be compared with the hydrogen ion concentration of solution with pOH 9.

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

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

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

pH=logH+

Here, H+ is concentration of hydrogen ion in the solution.

Rearranging,

H+=10pH

Putting the value,

H+=109=1.0×109 M

Thus, the concentration of hydrogen ion of solution with pH equals to 9 is 1.0×109 M

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