Why do HCl, HNO₃, etc., show acidic characters in aqueous solutions while solutions of compounds like alcohol and glucose do not show acidic character?

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Solution

The dissociation of HCl or HNO₃ to form hydrogen ions always occurs in the presence of water. Hydrogen ions (H⁺) combine with H₂O to form hydronium ions (H₃O⁺).

The reaction is as follows:

Although aqueous solutions of glucose and alcohol contain hydrogen, these cannot dissociate in water to form hydrogen ions. Hence, they do not show acidic character.

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Why do $H C l, H_{2} S O_{4}, H N O_{3},$ etc., show acidic character in aqueous solutions while solutions of compounds like $C_{6} H_{12} O_{6}$ (glucose) and $C_{2} H_{5} O H$ (alcohol) do not show acidic character ?

Q. Question 1
Why do

HCl

{HNO}_{3}

, etc., show acidic character in aqueous solutions while solutions of compounds such as alcohol and glucose do not show acidic character?

Q. Why do

HCl

{HNO}_{3}

, etc. show acidic character in aqueous solutions while solutions of compounds like,

C_{2} H_{5} OH

and glucose do not show acidic character? Why does an aqueous solution of an acid conducts electricity?

Q.  Why do HCl,

H N O_{3}

, etc., show acidic characters in aqueous solutions while solutions of compounds like alcohol and glucose do not show acidic character?

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Why do HCl, HNO3, etc., show acidic characters in aqueous solutions while solutions of compounds like alcohol and glucose do not show acidic character?

Why do HCl, HNO₃, etc., show acidic characters in aqueous solutions while solutions of compounds like alcohol and glucose do not show acidic character?