   Chapter 16.4, Problem 16.3SC ### 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

# Exercise 16.3 Calculate the pH value for each of the following solutions at 25 °C. a. A solution in which [ H + ] = 1.0 × 10 − 3 M b. A solution in which [ OH + ] = 5.0 × 10 − 5 M

Interpretation Introduction

(a)

Interpretation:

The pH value for a solution in which [H+] = 1.0×103M should be calculated at 25°C.

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of [H+] in aqueous solution is small, by using the p scale in the form of pH scale, it is better way to represent acidity of solution.

Thus, pH = -log [H+]

And, at 25°C, the actual concentrations of the products are:

[H+][OH]=1×1014

The mathematical product of both [H+] and [OH] concentrations are always constant known as ion product constant ( Kw )

[H+][OH]=1×1014=Kw.

Explanation

Given information:

[H+] = 1.0×103M

The relation between pH and [H+] is given by:

pH = -log [H+]

Interpretation Introduction

(b)

Interpretation:

The pH value for a solution in which [OH] = 5.0×105M should be calculated at 25°C.

Concept Introduction:

To express the small number, p scale is used, which implies to take the log of a number. Since, the concentration of [H+] in aqueous solution is small, by using the p scale in the form of pH scale, it is better way to represent acidity of solution.

Thus, pH = -log [H+]

And, at 25°C, the actual concentrations of the products are:

[H+][OH]=1×1014

The mathematical product of both [H+] and [OH] concentrations are always constant known as ion product constant ( Kw )

[H+][OH]=1×1014=Kw.

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