Why Do Strongly Bonded Compounds Like HCl and NaCl Ionize in Water?

AI Thread Summary
The discussion centers on the ionization of hydrogen chloride (HCl) in water, questioning why a compound with strong bonds appears to completely dissociate into H+ and Cl- ions. It highlights that despite the strong covalent nature of HCl, it readily ionizes due to the formation of a strong covalent bond between hydrogen and water, resulting in hydronium ions (H3O+). This contrasts with hydrofluoric acid (HF), which, despite having strong bonds, does not ionize completely and is classified as a weak acid. The conversation also touches on sodium chloride (NaCl), emphasizing that although Na and Cl are strongly bonded ionically, they disassociate easily in water. The interactions between the ions and water molecules are significant enough to overcome the bond energy, leading to dissociation despite the apparent strength of the original bonds. Overall, the discussion underscores the complexity of bond interactions in aqueous solutions and the role of water in facilitating ionization.
krackers
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The bonds between H and Cl are strong, almost close to ionic, right? Thus if that is the case why does HCl readily ionize into H+ and Cl- upon contact with water? It doesn't make sense that such a strongly bonded compound should completely disassociate upon contact with water. Further, why does HF, another strongly bonded compound, not do the same thus making it a weak acid?

On a similar note, why does NaCl do the same? Na and Cl are very strongly ionically bonded, requiring lots of energy to break apart the bond. Yet on contact with water, they easily disassociate. Interactions between the Na, Cl, and the H2O dipole don't seem like they have enough energy to break it apart.
 
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You should also take in mind that in the process of hydrolysis of an acid there is a new and very strong covalent bond being formed namely between H and O in ##\mathrm{H_3O^+}##.
 
HCl is covalent.
 

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