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Chapter 2: Q10P (page 57)

Question: Draw the conjugate acid for each of the following:

Short Answer

Expert verified

According to Bronsted-Lowry theory, the protonated form of a base is known to be its conjugated acid.

Step by step solution

01

Definition of conjugate acid.

According to Bronsted-Lowry theory, the protonated form of a base is known to be its conjugated acid.

02

Drawing the conjugate acid.

Add one hydrogen to each molecule to create their respective conjugate acids.

Subpart (a)
The conjugate acid for CH3CH2OH, isCH3CH2OH2+.

Subpart (b)
The conjugate acid for is CH3CH2OH

Subpart (c)
The conjugate acid for CH3CH2O-is

Subpart (d)
The conjugate acid for CH3CH2NH2 isCH3CH2NH3+.

Subpart (e)
The conjugate acid for

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Most popular questions from this chapter

Question:An acid has a Ka of 4.53 脳10-6 in water. What is its Keq for reaction with water in a dilute solution?

([H2O] = 55.5 M)

Which is a stronger acid?

CH3OH+CH3 or

Which is the stronger acid?

a. CH3OH or CH3CH3

b. CH3OH or HF

c. CH3NH2 or HF

d. CH3NH2 or CH3OH

You are planning to carry out a reaction that produces protons. The reaction will be buffered at pH = 10.5. Would it be better to use a protonated methylamine/methylamine buffer or a protonated ethylamine/ethylamine buffer? (pKa of protonated methylamine = 10.7; pKaof protonated ethylamine = 11.0)

An atom with a formal charge does not necessarily have more or less electron density than the atoms in the molecule without formal charges. We can see this by examining the potential maps for H2O,H30+and OH-.

  1. Which atom bears the formal negative charge in the hydroxide ion?

  2. Which atom has greater electron density in the hydroxide ion?

  3. Which atom bears the formal positive charge in the hydronium ion?

  4. Which atom has the least electron density in the hydronium ion?
See all solutions

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