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Restate the Brønsted-Lowry definitions of acids and bases and demonstrate the

Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro ISBN: 9780321910295 34

Solution for problem 9Q Chapter 14

Introductory Chemistry | 5th Edition

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Introductory Chemistry | 5th Edition | ISBN: 9780321910295 | Authors: Nivaldo J Tro

Introductory Chemistry | 5th Edition

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Problem 9Q

Problem 9Q

Restate the Brønsted-Lowry definitions of acids and bases and demonstrate the definitions with a chemical equation.

Step-by-Step Solution:
Step 1 of 3

Problem 9Q

Restate the Brønsted-Lowry definitions of acids and bases and demonstrate the definitions with a chemical equation.

Solution: Here, we are going to state the Bronsted-Lowry definitions of acids and bases.

Step1:

According to Bronsted-Lowry theory, acid is a substance that is capable of donating a hydrogen ion, H+ and bases are substances capable of accepting a hydrogen ion, H+. In short, acids are proton donors and bases are proton acceptors.

Step2:

Let us consider the example of dissolution of NH3 in H2O represented by the following equation.

In this reaction, water molecule acts as proton donor and ammonia molecule acts as proton acceptor and are thus, called Bronsted-Lowry acid and base, respectively. In the reverse reaction, H+ is transferred from NH4+ to OH-. In this case, NH4+ acts as a Bronsted acid while OH- acted as a Bronsted base. The acid-base pair that differs only by one proton is called a conjugate acid-base pair. Therefore, OH- is called the conjugate base of an acid H2O and NH4+ is called conjugate acid of the base NH3.

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Step 2 of 3

Chapter 14, Problem 9Q is Solved
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Textbook: Introductory Chemistry
Edition: 5
Author: Nivaldo J Tro
ISBN: 9780321910295

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Restate the Brønsted-Lowry definitions of acids and bases and demonstrate the