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Chapter 2: Q42 P (page 139)

Predict the products of the following acid-base reactions.

(a)

(b)

(c)

(d)

(e)

(f)

(g)

(h)

Short Answer

Expert verified

(a)

(b)

(c)

(d)

(e)

(f)

(g)

(h)

Step by step solution

01

Bronsted – Lowry concept of acid and base

According to Bronsted-Lowry, an acid can be defined as any substance (molecule or ion) that has the tendency to donate a proton (H+ ) to any substance whereas a base can be defined as any substance (molecule or ion) that has the tendency to accept a proton (H+) from any other substance.

02

Conjugate acid-base pair

The residual part of acid after losing a proton will have a tendency to accept a proton (H+). Therefore, it will behave as a base. These pairs of substances which differ from one another by a proton (H+) are known as conjugate acid-base pairs. Consider a general example of an acid:

03

Prediction of the products

Bronsted-Lowry acid is a proton (H+) donor while Bronsted-Lowry base is a proton (H+) acceptor.

(a)

(b)

(c)

(d)

((e)

(f)

(g)

(h)

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Most popular questions from this chapter

Question: Each of these compounds can react as a nucleophile. In each case, use curved arrows to show how the nucleophile would react with the strong electrophile, Bf3.

(a)

(b)

(c)

(d)

(CH3)3N

(e)

CH3CH2OH

(f)

(CH3)2S

Question: Circle the functional groups in the following structures. State to which class (or classes) of compounds the structure belongs.

(a)

(b)

(c)

(d)

(e)

(f)

(g)

(h)

(i)

(j)

(k)

Consider the following compounds that vary from nearly nonacidic to strongly acidic. Draw the conjugate bases of these compounds and explain why the acidity increases so dramatically with substitution by nitro groups.

The following acids are listed in increasing order of acidity. In each case, the acidic proton is shown in red.

(a) Show the structure of the conjugate base of each acid, including any resonance forms.

(b) Explain why X is a stronger acid than W.

(c) Explain why Y is a stronger acid than X.

(d) Explain why Z is a stronger acid than Y.

Question: The pKa of ascorbic acid (vitamin C, page 9) is 4.17 , showing that it is lightly more acidic than acetic acid (CH3COOH, pKa = 4.74).

(a)Show four different conjugate bases that would be formed by deprotonation of the four different OH groups in ascorbic acid.

(b) Compare the stabilities of these four conjugate bases, and predict which OH group of ascorbic acid is the most acidic.

(c) Compare the most stable conjugate base of ascorbic acid with the conjugate base of acetic acid, and suggest why these two compounds have similar acidities, even though ascorbic acid lacks the carboxylic acid (COOH) group
See all solutions

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