   # At 40.°C the value of K w is 2.92 × 10 −14 . a. Calculate the [H + ] and [OH − ] in pure water at 40.°C. b. What is the pH of pure water at 40.°C? c. If the hydroxide ion concentration in a solution is 0.10 M. what is the pH at 40.°C? ### 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 48E
Textbook Problem
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## At 40.°C the value of Kw is 2.92 × 10−14.a. Calculate the [H+] and [OH−] in pure water at 40.°C.b. What is the pH of pure water at 40.°C?c. If the hydroxide ion concentration in a solution is 0.10 M. what is the pH at 40.°C?

(a)

Interpretation Introduction

Interpretation: The value of Kw at 40°C is given. The [OH] and the [H+] in a given solution of pure water, the pH of pure water and the pH of a solution having the hydroxide ion concentration as, 0.10M at 40°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+]

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

Kw=[H+][OH]

### Explanation of Solution

Explanation

To determine: The [OH] and the [H+] in a given solution of pure water at 40°C .

The [OH] and [H+] in pure water at 40°C is 1.7×10-7_ .

Given

The solution is a pure water solution.

The Kw value at 40°C is 2.92×1014 .

For a pure water solution,

[H+]=[OH]

The [H+]=[OH] is assumed to be x

(b)

Interpretation Introduction

Interpretation: The value of Kw at 40°C is given. The [OH] and the [H+] in a given solution of pure water, the pH of pure water and the pH of a solution having the hydroxide ion concentration as, 0.10M at 40°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+]

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

Kw=[H+][OH]

(c)

Interpretation Introduction

Interpretation: The value of Kw at 40°C is given. The [OH] and the [H+] in a given solution of pure water, the pH of pure water and the pH of a solution having the hydroxide ion concentration as, 0.10M at 40°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+]

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

Kw=[H+][OH]

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