Does acidity and hydrogen bond strength go hand in hand?

AI Thread Summary
The discussion centers on the relationship between acidity, electronegativity, and dipole moments. It highlights that increased acidity correlates with higher electronegativity and dipole moments, yet liquids with low dipole moments, such as bases, tend to have lower density and surface tension, despite not always forming hydrogen bonds. The conversation questions whether acidity leads to stronger hydrogen bonds, using acetic acid as an example of a low surface tension acid. The role of hydrochloric acid is examined, noting its status as a strong acid but lack of hydrogen bonding, leading to inquiries about the nature of hydrogen bonds in acidic solutions, particularly when mixed with water. The discussion also touches on the hydronium ion (H3O+) in this context.
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More acidity means more electronegativity, and more electronegativity means more dipole moments. I observed that liquids with low dipole moments (bases) often have lower density and surface tension, but not necessarily hydrogen bonds. To contradict it, acetic acid have a low surface tension but it's an acid. Does acidity means a stronger hydrogen bond?
 
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What dipoles moments are you thinking of?
Hydrochloric acid (for example) is a strong acid but are there any hydrogen bonds in it? I don't think so.
You mean the H3O+?
 
Sorry for my mistake, I was actually trying to find if an acidic solution when mixed with water would strengthen its hydrogen bonds.
nasu said:
What dipoles moments are you thinking of?
Hydrochloric acid (for example) is a strong acid but are there any hydrogen bonds in it? I don't think so.
You mean the H3O+?
 

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