   Chapter 14, Problem 55E

Chapter
Section
Textbook Problem

# What are the major species present in 0.250 M solutions of each of the following acids? Calculate the pH of each of these solutions.a. HClO4b. HNO3

(a)

Interpretation Introduction

Interpretation: The major species present in 0.250M solutions of the following acids are to be stated. 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+]

To determine: The major species present in 0.250M solutions of HClO4 and the pH value of this solution.

Explanation

Explanation

The dissociation of HClO4 is, HClO4(l)  H+(aq) + ClO4(aq)

The stated reaction is,

HClO4(l)  H+(aq) + ClO4(aq)

The major species that are present are H+ and ClO4 .

The pH of the given sample is 0

(b)

Interpretation Introduction

Interpretation: The major species present in 0.250M solutions of the following acids are to be stated. 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+]

To determine: The major species present in 0.250M solutions of HClO4 and the pH value of this solution.

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