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Question
Why do HCl, H2SO4, HNO3, etc., show acidic character in aqueous solutions while solutions of compounds like C6H12O6 (glucose) and C2H5OH (alcohol) do not show acidic character?
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Solution
HCl and HNO3 produce \[\ce{H+_{( aq)}}\] ions in aqueous solution, which are responsible for their acidic character.
\[\ce{HCl_{(aq)} -> H+_{( aq)} + Cl^-_{( aq)}}\]
\[\ce{HNO3_{(aq)} -> H+_{( aq)} + NO^-_{3 ( aq)}}\]
Alcohol (C2H5OH) and glucose (C6H12O6) are covalent compounds, and they do not undergo dissociation in aqueous solution. This is evident from the fact that their aqueous solutions do not conduct electricity. Hence, aqueous solutions of alcohol and glucose do not exhibit acidic character, even though they contain hydrogen atoms.
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