Which of the following is the strongest base?

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(A) To determine the basicity,we look at the availability of the lone pair of electrons on the nitrogen atom:$1$. In $Piperidine$,the nitrogen is $sp^

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Piperidine

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(A) To determine the basicity,we look at the availability of the lone pair of electrons on the nitrogen atom:$1$. In $Piperidine$,the nitrogen is $sp^3$ hybridized and the lone pair is localized,making it the most basic.$2$. In $Pyridine$,the nitrogen is $sp^2$ hybridized,and the lone pair is in an $sp^2$ orbital,which is less basic than $sp^3$.$3$. In $Pyrrole$,the lone pair on nitrogen is involved in the aromatic sextet,making it unavailable for protonation,thus it is very weakly basic.$4$. In $Aniline$,the lone pair is delocalized into the benzene ring due to resonance,reducing its availability for protonation.Therefore,$Piperidine$ is the strongest base.

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