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Chapter 17: Q.16. (page 641)

Question: Rank the following compounds in the order of increasing acidity.

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01

Conjugate Acid

A conjugate acid-base pair in which the two substances differ only by the presence of a proton is known as acids and bases according to the Lowry-Bronsted concept.

By adding a proton to a base, a conjugate acid is formed, and by the removal of a proton from an acid, a conjugate base is formed.

02

Conjugate acid-base relationship

The strength of an acid or base and the strength of its conjugate base or conjugate acid are interrelated. The relation is that as the acid strength increases, the conjugate base becomes weaker. The acid is weaker, the strength of the conjugate base is strong.

03

Ranking the compound in the increasing order of acidity

The compounds with the most stable conjugate base are the most acidic.

  • For the first one, there is no delocalization due to resonance; so, it has the most unstable base and, hence, least acidic acid.
  • For the second one, there are two resonance structures; so, the acid has an intermediate acidity.
  • For the third one, an aromatic conjugate base that is most stable is present; so, the acid will be most acidic.

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Most popular questions from this chapter

Question: Which compound in each pair is the stronger acid?

Question: What orbitals are used to form the labeled bonds in the following molecule? Of the labeled bonds, which is the shortest?

Question: Early structural studies on benzene had to explain the following experimental evidence. When benzene was treated with Br2(plus a Lewis acid), a single substitution product of molecular formula C6H5Brwas formed. When this product was treated with another equivalent of Br2, three different compounds of molecular formularole="math" localid="1648727281591" C6H4Br2 were formed.

  1. Explain why a single Kekule structure is consistent with the first result, but does not explain the second result.
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