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Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097

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BuyFindarrow_forward

Chemistry

9th Edition
Steven S. Zumdahl
ISBN: 9781133611097
Textbook Problem

Aluminum hydroxide is an amphoteric substance. It can act as either a Brønsted-Lowry base or a Lewis acid. Write a reaction showing Al(OH)3 acting as a base toward H+ and as an acid toward OH.

Interpretation Introduction

Interpretation: The equations that describe Al(OH)3 acting as a Bronsted-Lowry base towards H+ and as a Lewis acid towards OH are to be stated.

Concept introduction: The species that acts as a proton acceptor is known as a Bronsted-Lowry base and the species that acts as a proton donor is termed as a Bronsted-Lowry acid.

The ionic species that is capable of accepting an electron pair from a compound that acts as a donor is known as a Lewis acid.

To determine: The equations that describe Al(OH)3 acting as a Bronsted-Lowry base towards H+ and as a Lewis acid towards OH .

Explanation

Explanation

The species that acts as a proton acceptor is known as a Bronsted-Lowry base and the species that acts as a proton donor is termed as a Bronsted-Lowry acid.

The equation that describes Al(OH)3 acting as a Bronsted-Lowry base towards H+ is,

Al(OH)3+3HNO3Al(NO3)3+3H2O

In this case, the Al(OH)3 acts as a proton acceptor and hence is termed as a Bronsted-Lowry base.

The ionic reaction that occurs is,

Al(OH)3+3H+Al3++3H2O

The equation that describes Al(OH)3 acting as a Lewis acid towards OH is,

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