Chemistry: The Molecular Nature of Matter
Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
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Chapter 15, Problem 1PE

Which of the following are conjugate acid-base pairs? Describe why the others are not true conjugate acid-base pairs: ( a )  H 3 PO 4  and H 2 PO 4 - ( b )  HI and H + ( c )  NH 2 - and NH 3 ( d )  HNO 2  and NH 4 + ( e )  CO 3 2- and CN - ( f )  HPO 4 2- and H 2 PO 4 - . (Hint: Recall that conjugate acid-base pairs must differ by one H + .)

Expert Solution & Answer
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Interpretation Introduction

Interpretation:

The conjugate acid-base pairs are to be identified and the reason for those which are not acid-base pairs is to be described.

Concept Introduction:

There are various concepts which describe acids and bases, such as Arrhenius concept, Bronsted-Lowry concept, Lewis concept.

According to Bronsted-Lowry concept, acids are the substances which provide H+ in the solution. These are H+ donors, such as HCl, HBr, while those substances which accept H+ are termed as bases, such as NH3, Cl.

The species formed after donation of H+ by a Bronsted acid is called its conjugate base. The species formed after accepting H+ by a Bronsted base is called its conjugate acid. The acid corresponding to its conjugate base and the base corresponding to its conjugate acid are termed as conjugate acid-base pairs.

Answer to Problem 1PE

Solution:

a) This is a true conjugate acid-base pair.

b) I is the conjugate base of HI.

c) This is a true conjugate acid-base pair.

d) NO2 is the conjugate base of HNO2 and NH3 is the conjugate acid of NH4+.

e) HCO3 is the conjugate acid of CO32 and HCN is the conjugate acid of CN.

f) This is a true conjugate acid-base pair.

Explanation of Solution

a) H3PO4 and H2PO4

H3PO4 differs from H2PO4 only by H+. The dissociation occurs as follows:

H3PO4  H2PO4 + H+.

H3PO4 acts a Bronsted acid and H2PO4 as its conjugate base. So, these two form a conjugate acid-base pair.

b) HI and H+

HI acts as Bronsted acid and dissociates as follows:

HI I + H+

I is the conjugate base of HI. As HI and I differ only by H+ and form a conjugate acid-base pair, HI and H+ do not form a conjugate acid-base pair.

c) NH2 and NH3

NH2 acts as a Bronsted base and accepts H+ to form NH3. The conversion occurs as follows: NH2 + H+NH3

NH3 is the conjugate acid of NH2. Hence, these two form a conjugate acid-base pair.

d) HNO2 and NH4+

HNO2 acts as Bronsted acid and dissociates as follows:

HNO2 NO2 + H+

So, NO2 is the conjugate base of HNO2. However, NH4+ is not a part of the above equation. So, HNO2 and NH4+ do not form a conjugate acid-base pair.

e) CO32 and CN

CO32 acts as a Bronsted base and accepts H+ to form HCO3. The conversion occurs as follows:

CO32 + H+HCO3

HCO3 is the conjugate acid of CO32. However, CN is not a part of the above equation. So, CO32 and CN do not form a conjugate acid-base pair.

f) HPO42 and H2PO4

HPO42 differs from H2PO4 only by H+. Here, HPO4 acts as a Bronsted base. The conversion occurs as follows:

HPO42+H+H2PO4.

HPO4 acts a Bronsted acid and H2PO4 as its conjugate base. So, these two form a conjugate acid-base pair.

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Chapter 15 Solutions

Chemistry: The Molecular Nature of Matter

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