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The compounds or ions which can accept an electron pair are called Lewis acid.

For example, all the compounds containing either a highly electronegative element or an element that can show a higher valency than the compound's form an excellent Lewis acid.

When a proton is transferred from an acid to a base, the resultant counterion from the acid is known as the conjugate base. The conjugate base can act as any normal base and donate a pair of electrons to undergo bonding.

Lewis bases are compounds that can donate a lone pair of electrons.

For example, compounds containing lone pairs of electrons make a good Lewis base.

After receiving a proton from the acid, the base can now behave as an acid known as conjugate acid.

The hydrogen atom, which is released as a proton ${\text{(H}}^{+}\text{)}$from acid, is called acidic hydrogen. The acidic hydrogen is generally connected to a highly electronegative element in the acid.

The base donates the lone pair of electrons to the acidic hydrogen atom present in the lewis acid. This leads to the proton transfer from the acid to the base. After this, thecounterions are bonded.

a.

The products are mentioned below:

Reaction of a. with KOH

b.

The products are mentioned below:

Reaction of b. with KOH

c.

The products are mentioned below:

Reaction of c. with KOH

d.

The products are mentioned below:

Reaction of d. with KOH