   Chapter 16, Problem 80AP ### 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

# . The ion-product constant for water, Kw, has the value _____ at 25 °C.

Interpretation Introduction

Interpretation:

The value of ion-product for water should be determined at 25 C.

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

The dissociation reaction of water is represented as follows:

H2OlH+aq+OHaq

For the above reaction, since, pure liquid is not considered in ion-product constant thus, the expression for ion-product constant for water can be written as:

Kw=H+OH

Since, pH of water is 7 because it is neutral. Thus, the concentration of hydrogen ion in water can be calculated as follows:

pH=logH+

Here, H+ is concentration of hydrogen ion

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