Assertion (A): In dilute benzene solutions, equimolar addition of `R_(3)N` and `HCI` produce a substance with a dipole moment. In the same solvent, equimolar addition of `R_(3)N` and `SO_(3)` produce a substance having an almost identical dipole moment.
Reason (R) : Both `HCI` and `SO_(3)` are Lewis acids and can react with the amine base to form polar substances which undergo ionic dissociation in a solvent sufficiently more polar than benzene.
Moreover, `(N-S)` bond is a more polar bond.

Options

A. If both (A) and (R) are correc, and (R) is the correct explanation of (A).
B. If both (A) and (R) are correct but (R) is not the correct explanation of (A).
C. If (A) is correct, but (R) is incorrect.
D. If (A) is incorrect, but (R) is correct.

Answer

A

Explanation

Both (A) and (R) are correct and (R) is the correct explanation of (A)
`R_(3)N:+overset( :ddotO: )overset(|)underset( :underset(..)O: )underset(|)(S)-overset(..)underset(..)O: rarr R_(3)N-overset( :ddotO: )overset(|)underset( :underset(..)O: )underset(|)(S)-overset(..)underset(..)O:`
Sulphur can expand its electron complement in the valence shell to exceed the octet. In any case, `S`, expands its number its number of valence electrons by attaching to the lone pair on the `N` and `(N-S)` bond is more polar bond due to the big difference in `EN` between `N` and `S`.
`R_(n)N:+H-overset(..)underset(..)CI:rarrR_(3)N-H...... overset(..)underset(..)(CI):`
In this case `H` of the `HCI` attaches to the lone pair on the `N`. Here `CI` is connected to `N` by a hydrogen bond.