   Chapter 14, Problem 91E

Chapter
Section
Textbook Problem

# What are the major species present in 0.015 M solutions of each of the following bases?a. KOHb. Ba(OH)2What is [OH−] and the pH of each of these solutions?

(a)

Interpretation Introduction

Interpretation: The major species present in 0.015M solutions of the following bases are to be stated. The [OH] and the pH value of the given solutions 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 pOH of a solution is calculated by the formula, pOH=log[OH]

The sum, pH+pOH=14

To determine: The major species present in 0.015M solution of KOH and the [OH] and the pH value of this solution.

Explanation

Explanation

KOH is a strong base. Therefore, it will completely dissociate into ions.

Therefore, [OH] =0.015M_

The pOH of a solution is calculated by the formula,

pOH=log[OH]

Substitute the value of [OH] in the above expression

(b)

Interpretation Introduction

Interpretation: The major species present in 0.015M solutions of the following bases are to be stated. The [OH] and the pH value of the given solutions 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 pOH of a solution is calculated by the formula, pOH=log[OH]

The sum, pH+pOH=14

To determine: The major species present in 0.015M solution of Ba(OH)2 and the [OH] and the pH value of this solution.

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