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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

Citrus fruits are rich in citric acid, a compound with three COOH groups. Explain the following:

a. The first pKa (for the COOH group in the center of the molecule) is lower than the pKa of acetic acid.

b. The third pKa is greater than the pKa of acetic acid.

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?

Which of the following are not acids?

CH3COOH CO2 HNO2 HCOOH CCl4

a. For each of the acid-base reactions in section 2.3, compare the pKa values of the acids on either side of the equilibrium arrows to prove that the equilibrium lies in the direction indicated. (The pKa values you need are found in section 2.3 or in problem 13)

b. Do the same for the acid-base reaction in section 2.1

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

([H2O] = 55.5 M)
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