Calculate the [H + ] of each of the following solutions at 25°C. Identity each solution as neutral, acidic, or basic. a. [OH − ] = 1.5 M b. [OH − ] = 3.6 × 10 −15 M c. [OH − ] = 1.0 × 10 −7 M d. [OH − ] = 7.3 × 10 −4 M

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

Chapter
Section

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 13, Problem 46E
Textbook Problem
10 views

Calculate the [H+] of each of the following solutions at 25°C. Identity each solution as neutral, acidic, or basic.a. [OH−] = 1.5 Mb. [OH−] = 3.6 × 10−15 Mc. [OH−] = 1.0 × 10−7 Md. [OH−] = 7.3 × 10−4 M

(a)

Interpretation Introduction

Interpretation: The [H+] of each of the given solutions is to be calculated. The solutions are to be identified as neutral, acidic or basic.

Concept introduction: A neutral species has a pH value equal to 7 , that is the [OH] is equal to the [H+] . An acidic species has a pH value less than 7 , that is the [OH] is less than the [H+] . A basic species has a pH value greater than 7 , that is the [H+] is less than the [OH] .

The equilibrium constant for water is denoted by Kw and is expressed as,

Kw=[H+][OH]

At 25°C , [H+][OH]=1×1014

Explanation of Solution

Explanation

To determine: The [H+] of each the given solution and its classification into neutral, acidic or a basic solution.

Given

[OH]=1.5M

The temperature is 25°C .

The [H+] is calculated by the formula,

Kw=[H+][OH]=1×1014

Substitute the given value of [OH] in the above expression.

[1

(b)

Interpretation Introduction

Interpretation: The [H+] of each of the given solutions is to be calculated. The solutions are to be identified as neutral, acidic or basic.

Concept introduction: A neutral species has a pH value equal to 7 , that is the [OH] is equal to the [H+] . An acidic species has a pH value less than 7 , that is the [OH] is less than the [H+] . A basic species has a pH value greater than 7 , that is the [H+] is less than the [OH] .

The equilibrium constant for water is denoted by Kw and is expressed as,

Kw=[H+][OH]

At 25°C , [H+][OH]=1×1014

(c)

Interpretation Introduction

Interpretation: The [H+] of each of the given solutions is to be calculated. The solutions are to be identified as neutral, acidic or basic.

Concept introduction: A neutral species has a pH value equal to 7 , that is the [OH] is equal to the [H+] . An acidic species has a pH value less than 7 , that is the [OH] is less than the [H+] . A basic species has a pH value greater than 7 , that is the [H+] is less than the [OH] .

The equilibrium constant for water is denoted by Kw and is expressed as,

Kw=[H+][OH]

At 25°C , [H+][OH]=1×1014

(d)

Interpretation Introduction

Interpretation: The [H+] of each of the given solutions is to be calculated. The solutions are to be identified as neutral, acidic or basic.

Concept introduction: A neutral species has a pH value equal to 7 , that is the [OH] is equal to the [H+] . An acidic species has a pH value less than 7 , that is the [OH] is less than the [H+] . A basic species has a pH value greater than 7 , that is the [H+] is less than the [OH] .

The equilibrium constant for water is denoted by Kw and is expressed as,

Kw=[H+][OH]

At 25°C , [H+][OH]=1×1014

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