Question

Which of the following behaves as Lewis acid and not as Bronsted acid
(a) HCl
(b) H₂SO₄
(c) $HSO_3^-$
(d) SO₃

Answer 1

D as it cannot give H i.e it cannot donate a proton

Answer 2

$SO_3$ acts as lewis acid

Explanation:

According to the Bronsted Lowry conjugate acid-base theory, an acid is defined as a substance which donates protons and a base is defined as a substance which accepts protons.

$H_2SO_4\rightarrow HSO_4^-+H^+$

$HCl\rightarrow H^++Cl^-$

According to the Lewis concept, an acid is defined as a substance that accepts electron pairs and base is defined as a substance which donates electron pairs.

$SO_3+H_2O\rightarrow H_2SO_4$

As $SO_3$ can gain electrons as it is short of two electrons to complete its octet. Thus it acts as lewis acid.

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