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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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. Which of the following bases have relatively strong conjugate acids?

a. F-

b. Cl-

c. HSO 4

d. NO 3

Interpretation Introduction

Interpretation:

The base with relatively strong conjugate acid should be determined.

Concept Introduction:

Strength of conjugate acid of a base is derived from its kb value. If a base has a relatively higher kb value, that means the base reacts with water forming more OH- ions and conjugate acid. If the kb value is smaller formation of OH- ions and the conjugate acid is smaller. Thus, which can be used to derive the strength of the base. Higher the kb, higher the formation of OH- ions and higher the strength of the base and on the other hand lower the kb, lower the formation of OH- ions and lower the strength of the base.

On the other hand, ka values determine the strength of an acid. Higher the ka, stronger the acid and lower the ka, weaker the acid. Normally if the ka >1, it is considered as a strong acid and if kb >10-14, it is considered as a relatively stronger base (effective base).

kw=ka×kb.

Explanation

For a given temperature, kw (ionic product of water) is a constant, thus for a given conjugate acid base pair, if kb of the base is higher (stronger base), ka will be smaller (weaker acid) and if kb of the base is lower (weaker base), ka will be higher (stronger acid).

Base dissociation constant is a measure of the dissociation of a base, consider the base B,

+ H2OHB++ OH

kb=[OH-][HB+][B]

B is the base, HB+ is the conjugate acid,

If the dissociation of the conjugate acid, HB+ is written

HB++ H2O+ H3O+

Expression for ka can be written as

ka=[B][H3O+][HB+]

A relationship between ka and kb can be developed as follows,

kakb=[B][H

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