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

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−]=1×10−14

Explanation

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

Given

[H+]=1.0×10−7 M

The temperature is 25 °C .

The [OH−] is calculated by the formula,

Kw=[H+][OH−]=1×10−14

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

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−]=1×10−14

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−]=1×10−14

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−]=1×10−14