EBK FOUNDATIONS OF COLLEGE CHEMISTRY
EBK FOUNDATIONS OF COLLEGE CHEMISTRY
15th Edition
ISBN: 9781118930144
Author: Willard
Publisher: JOHN WILEY+SONS INC.
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Chapter 15, Problem 1RQ
Interpretation Introduction

Interpretation:

Difference that can exist between Arrhenius and Bronsted-Lowry definitions of an acid has to be written.

Concept Introduction:

Arrhenius gave broader picture and suggested that acids are able to release excess of H+ ion on dissolution in water while bases are able to release excess of OH ion on dissolution in water.

Bronsted-Lowry acid outlined the definition of acids that donate H+ or a proton while bases that accept H+ or a proton. The acidic strength is known from the ability of acid to donate H+ in an aqueous solution. Explicitly the acidity strength is quantified by the magnitude of a parameter called acid ionization constant. The strong acids tend to possess higher magnitudes of acid ionization constant or Ka.

Expert Solution & Answer
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Explanation of Solution

In accordance with Bronsted definition, the most usual type of acid-base reaction involves lone pair of base that reaches out for an acidic proton. Once deprotonation has occurred species assumes a negative charge and is referred to as the conjugate base of acid and other species with a positive charge as a result of proton acceptance is termed conjugate acid of given base. For example;

EBK FOUNDATIONS OF COLLEGE CHEMISTRY, Chapter 15, Problem 1RQ , additional homework tip  1

In Arrhenius concept, the acid species is one that can make water to behave as Bronsted base so that it accepts the proton and forms H3O+ as illustrated below.

EBK FOUNDATIONS OF COLLEGE CHEMISTRY, Chapter 15, Problem 1RQ , additional homework tip  2

Thus all Arrhenius acid are capable to act as Bronsted acid.

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Chapter 15 Solutions

EBK FOUNDATIONS OF COLLEGE CHEMISTRY

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