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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

Butyric acid, the compound responsible for the unpleasant odor and taste of sour milk, has a pKa value of 4.82. What is its Ka value? Is it a stronger acid or a weaker acid than vitamin C?

After examining the potential maps for LiH, HF and answer the following question:

  1. Which compounds are polar?
  2. Why does LiH have the largest hydrogen?

  3. Which compound has the hydrogen that would be most apt to attract a negatively charged molecule?

Estimate the pKa values of the following compounds.

(a)CH3CH2CH2NH2

(b)CH3CH2CH2OH

(c)CH3CH2COOH

(d)CH3CH2CH2NH3+

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)

Which is the stronger acid?

a. CH3CH3 or HC ≡CH

b. H2C= CH2or HC≡ CH

c. H2C =CH2 or CH3CH3
See all solutions

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