   # Calculate [H + ] and [OH − ] for each solution at 25°C. Identify each solution as neutral, acidic, or basic. a. pH = 7.40 (the normal pH of blood) b. pH = 15.3 c. pH = −1.0 d. pH = 3.20 e. pOH = 5.0 f. pOH = 9.60 ### Chemistry: An Atoms First Approach

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

#### Solutions

Chapter
Section ### Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 13, Problem 50E
Textbook Problem
75 views

## Calculate [H+] and [OH−] for each solution at 25°C. Identify each solution as neutral, acidic, or basic.a. pH = 7.40 (the normal pH of blood)b. pH = 15.3c. pH = −1.0d. pH = 3.20e. pOH = 5.0f. pOH = 9.60

(a)

Interpretation Introduction

Interpretation: The classification of the given solutions into acidic, basic or neutral is to be determined and [OH] the [H+] for each of the given solutions at 25°C is to be calculated.

Concept introduction: The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution. A logarithmic scale is used on which, the value 7 corresponds to a neutral species, a value less than 7 corresponds to an acid and a value greater than 7 corresponds to a base.

The pH of a solution is calculated by the formula, pH=log[H+]

At 25°C , pH+pOH=14

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

Kw=[H+][OH]

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

### Explanation of Solution

Explanation

Given

pH=7.40

The temperature is 25°C .

The pH of a solution is calculated by the formula,

pH=log[H+]

Rearrange the above expression to calculate the value of [H+] .

[H+]=10pH

Substitute the given value of pH in the above expression.

[H+]=107.40=4.0×10-8M_

The value of [H+] is 4.0×108M

(b)

Interpretation Introduction

Interpretation: The classification of the given solutions into acidic, basic or neutral is to be determined and [OH] the [H+] for each of the given solutions at 25°C is to be calculated.

Concept introduction: The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution. A logarithmic scale is used on which, the value 7 corresponds to a neutral species, a value less than 7 corresponds to an acid and a value greater than 7 corresponds to a base.

The pH of a solution is calculated by the formula, pH=log[H+]

At 25°C , pH+pOH=14

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

Kw=[H+][OH]

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

(c)

Interpretation Introduction

Interpretation: The classification of the given solutions into acidic, basic or neutral is to be determined and [OH] the [H+] for each of the given solutions at 25°C is to be calculated.

Concept introduction: The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution. A logarithmic scale is used on which, the value 7 corresponds to a neutral species, a value less than 7 corresponds to an acid and a value greater than 7 corresponds to a base.

The pH of a solution is calculated by the formula, pH=log[H+]

At 25°C , pH+pOH=14

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

Kw=[H+][OH]

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

(d)

Interpretation Introduction

Interpretation: The classification of the given solutions into acidic, basic or neutral is to be determined and [OH] the [H+] for each of the given solutions at 25°C is to be calculated.

Concept introduction: The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution. A logarithmic scale is used on which, the value 7 corresponds to a neutral species, a value less than 7 corresponds to an acid and a value greater than 7 corresponds to a base.

The pH of a solution is calculated by the formula, pH=log[H+]

At 25°C , pH+pOH=14

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

Kw=[H+][OH]

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

(e)

Interpretation Introduction

Interpretation: The classification of the given solutions into acidic, basic or neutral is to be determined and [OH] the [H+] for each of the given solutions at 25°C is to be calculated.

Concept introduction: The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution. A logarithmic scale is used on which, the value 7 corresponds to a neutral species, a value less than 7 corresponds to an acid and a value greater than 7 corresponds to a base.

The pH of a solution is calculated by the formula, pH=log[H+]

At 25°C , pH+pOH=14

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

Kw=[H+][OH]

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

(f)

Interpretation Introduction

Interpretation: The classification of the given solutions into acidic, basic or neutral is to be determined and [OH] the [H+] for each of the given solutions at 25°C is to be calculated.

Concept introduction: The pH of a solution is define as a figure that expresses the acidity of the alkalinity of a given solution. A logarithmic scale is used on which, the value 7 corresponds to a neutral species, a value less than 7 corresponds to an acid and a value greater than 7 corresponds to a base.

The pH of a solution is calculated by the formula, pH=log[H+]

At 25°C , pH+pOH=14

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

Kw=[H+][OH]

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

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