   # Give the pH that corresponds to each solution and classify it as acidic, basic, or neutral: a. [ H 3 O + ] = 0 .01 b. [ H 3 O + ] = 10 -9 c. [ H 3 O + ] = 10 -7 d. [ H 3 O + ] = 10 -5 ### Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692

#### Solutions

Chapter
Section ### Chemistry In Focus

7th Edition
Tro + 1 other
Publisher: Cengage Learning,
ISBN: 9781337399692
Chapter 13, Problem 37E
Textbook Problem
13 views

## Give the pH that corresponds to each solution and classify it as acidic, basic, or neutral:a. [ H 3 O + ]  = 0 .01 b. [ H 3 O + ]  = 10 -9 c. [ H 3 O + ]  = 10 -7 d. [ H 3 O + ]  = 10 -5

Interpretation Introduction

Interpretation:

For the given solutions, pH is to be calculated and nature of the solution is to be classified.

Concept Introduction:

The pH of an aqueous solution is the measurement of hydrogen ion activity. Here, pH stands for potential of hydrogen. It is represented as

pH=log[H+].

Based on the hydrogen and hydroxide ion concentrations, solutions maybe neutral, acidic, or basic in nature.

If the concentrations of hydrogen ions and hydroxide ions are equal, then the solution will be neutral; if the concentration of hydrogen ions is greater than hydroxide ions, then the solution will be acidic in nature; if the concentration of hydroxide ions is greater than hydrogen ions, then the solution will be basic in nature.

### Explanation of Solution

a) [H3O+]=0.01.

Using the equation, pH of the solution can be calculated as follows:

pH=log[H+]=log[0.01]=(2)=2

The pH of the solution is calculated to be 2. Hence, the solution is acidic in nature.

b) [H3O+]=109.

Using the equation, pH of the solution can be calculated as follows:

pH=log[H+]=log=(9)log10=9

The pH of the solution is calculated to be 9. Hence, the solution is basic in nature.

c) [H3O+]=107

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