Which of the following behaves as Lewis acid and not as Bronsted acid ?

Question

Which of the following behaves as Lewis acid and not as Bronsted acid ? (A)  HCl  (B)  H2SO4  (C)  HSO3-  (D)  SO3

Tardigrade Admin · Accepted Answer

Lewis acids have a tendency to accept electrons while Bronsted acids have a tendency to donate proton. (a) underset textBronsted acidHCl longrightarrow H ++ Cl - (b) underset textBronsted acidH 2 SO 4 longrightarrow H ++ HSO 4- (c) underset textBronsted acid HSO 3- longrightarrow H ++ SO 32- <img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/336f36e5a6299cdfc3d5a39f12111682-.png" />

Q. Which of the following behaves as Lewis acid and not as Bronsted acid ?

$H Cl$

$H_{2} S O_{4}$

$H S O_{3}^{-}$

$S O_{3}$

Lewis acids have a tendency to accept electrons while Bronsted acids have a tendency to donate proton.

(a) $Bronsted acid H Cl ⟶ H^{+} + C l^{-}$

(b) $Bronsted acid H_{2} S O_{4} ⟶ H^{+} + H S O_{4}^{-}$

(c) $Bronsted acid H S O_{3}^{-} ⟶ H^{+} + S O_{3}^{2 -}$

Q. Which of the following behaves as Lewis acid and not as Bronsted acid ?

HCl

H2​SO4​

HSO3−​

SO3​

Lewis acids have a tendency to accept electrons while Bronsted acids have a tendency to donate proton. (a) Bronsted acidHCl​⟶H++Cl− (b) Bronsted acidH2​SO4​​⟶H++HSO4−​ (c) Bronsted acid HSO3−​​⟶H++SO32−​

$H Cl$

$H_{2} S O_{4}$

$H S O_{3}^{-}$

$S O_{3}$

Lewis acids have a tendency to accept electrons while Bronsted acids have a tendency to donate proton.

(a) $Bronsted acid H Cl ⟶ H^{+} + C l^{-}$

(b) $Bronsted acid H_{2} S O_{4} ⟶ H^{+} + H S O_{4}^{-}$

(c) $Bronsted acid H S O_{3}^{-} ⟶ H^{+} + S O_{3}^{2 -}$