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Which of the following is the strongest acid?
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Last updated date: 19th Jun 2024
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Hint: The basicity is inversely proportional to the acidity. In the case of the base, the acidity is determined by checking the basic strength of the bases. Least the basicity high will be the acidity.

Complete Step by step answer: The given compounds are protonated amines. Amines are basic because amines have lone pair the nitrogen atom which can be donated.
The amine which is the weakest base will be the strongest acid because that amine cannot donate proton easily, so that amine will accept proton hence will be acidic.
So, we will remove a proton form all the given amines and check their basicity as follows:
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Among all four piperidine is the strongest base because it has lone pair at nitrogen which has ${\text{s}}{{\text{p}}^{\text{3}}}$ hybridization and all other carbons of the ring are also ${\text{s}}{{\text{p}}^{\text{3}}}$ hybridized so, all are electron donating hence it is most basic.
Piperidine is a stronger base than ammonia and $1,2,3,4 - $tetrahydroisoquinoline because in ammonia inversion is found which decrease its basicity and in $1,2,3,4 - $ tetrahydroisoquinoline the electron-withdrawing effect of the attached benzene ring decreases the basicity.
$1,2,3,4 - $ Tetrahydroquinoline is the least basic because the lone pair present at nitrogen are delocalised in the attached benzene ring. So, the availability of the lone pair decreases which decreases the basic strength of the $1,2,3,4 - $tetrahydroquinoline.
So, $1,2,3,4 - $ tetrahydroquinoline will be the strongest acid.

Therefore, option (C) is correct.

Note: In the case of acids, the acidity is determined by checking the stability of the anion formed by the removal of the proton. More stable the anion formed by removal of the proton will be more acidic. The factors that stabilize the anion formed by the removal of protons increase the acidity. Resonance decreases the basicity. Weaker the base stronger the acid or vice versa.