HCl, HBr, HI, etc.

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Michael Du 1E
Posts: 117
Joined: Sun Sep 22, 2019 12:16 am

HCl, HBr, HI, etc.

Postby Michael Du 1E » Thu Dec 05, 2019 12:38 pm

Is the reasoning behind HCl, HBr, etc. being a strong acid is that its anion is stable? if not whats the particular reasoning behind why they are strong acids? thank you!

Anish Patel 4B
Posts: 59
Joined: Thu Jul 11, 2019 12:17 am

Re: HCl, HBr, HI, etc.

Postby Anish Patel 4B » Thu Dec 05, 2019 12:47 pm

YEs since fluorine is the most electronegative, it has the highest electron withdrawing ability making the molecule more stable and less able to dissociate its H+ ions in water.

Kassidy Ford 1I
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Re: HCl, HBr, HI, etc.

Postby Kassidy Ford 1I » Fri Dec 06, 2019 9:25 am

You can also think of it in terms of bond length; since the bond between H-I is the longest it is the strongest acid because that bond will be easier to break, so it will dissociate the easiest. HI>HBr>HCl>HF. HF is a weak acid because F's high electronegativity and small size makes that bond short and strong so it will not break easy and it will not dissociate fully.


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