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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

Draw the hydrogen bonding that takes place between

(a) two molecules of ethanol.

(b) two molecules of propylamine.

(c) a molecule of dimethyl ether and two molecules of water.

(d) two molecules of trimethylamine and a molecule of water.

Draw a Lewis structure, and classify each of the following compounds. The possible classification are as follows:

alcohol, ketone, carboxylic acid, ether, aldehyde and alkene.

(a)

(b)

(c)

(d)

(e)

(f)

(g)

(h)

(i)

The following compounds can all react as acids.

  1. For each compound, show its conjugate base. Show any resonance forms if applicable.
  2. Rank the conjugate bases in the order you would predict, from most stable to least stable.
  3. Rank the original compounds in order from strongest acid to weakest acid.

The N-F bond is more polar than N-H bond, but NF3 has smaller dipole moment than NH3. Explain the curious result.

NH3: µ= 1.5 D, NF3: µ= 0.2D

Ammonia appears in Table 2-2 as both an acid and a conjugate base.

  1. Explain how ammonia can act as both an acid and a base. Which of these roles does it commonly fill in aqueous medium?
  2. Show how water can serve both as an acid and a base.
  3. CalculateKaand pKa for the hydronium ion, H3O+ .
  4. Show how methanol (CH3OH) can serve as both an acid and a base. Write an equation for the reaction of methanol with sulfuric acid.
See all solutions

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