HCl, HBr, HI, etc.

Moderators: Chem_Mod, Chem_Admin

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
Posts: 103
Joined: Sat Aug 17, 2019 12:16 am
Been upvoted: 1 time

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.

Return to “Bronsted Acids & Bases”

Who is online

Users browsing this forum: No registered users and 2 guests