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

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−]=1×10−14

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−]=1.5 M

The temperature is 25 °C .

The [H+] is calculated by the formula,

Kw=[H+][OH−]=1×10−14

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

[1

Answer 6

(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−]=1×10−14

Answer 7

(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−]=1×10−14

Answer 8

(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−]=1×10−14

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

Solutions

Chemistry: An Atoms First Approach

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

Explanation of Solution

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Chapter 13 Solutions

Additional Science Textbook Solutions

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

Solutions

Chemistry: An Atoms First Approach