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Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097

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BuyFindarrow_forward

Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097
Textbook Problem

Calculate the [OH] of each of the following solutions at 25°C. Identify each solution as neutral, acidic, or basic.

a. [H+] = 1.0 × 10−7 M

b. [H+] = 8.3 × 10−l6 M

c. [H+] = 12 M

d. [H+] = 5.4 × 10−5 M

(a)

Interpretation Introduction

Interpretation: The [OH] 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

Explanation

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

Given

[H+]=1.0×107M

The temperature is 25°C .

The [OH] is calculated by the formula,

Kw=[H+][OH]=1×1014

Substitute the given value of [H+] in the above expression

(b)

Interpretation Introduction

Interpretation: The [OH] 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 [OH] 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 [OH] 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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