HCl vs. HBr

Moderators: Chem_Mod, Chem_Admin

Cecilia Cisneros 1F
Posts: 133
Joined: Wed Sep 30, 2020 9:45 pm

HCl vs. HBr

Postby Cecilia Cisneros 1F » Wed Dec 02, 2020 10:50 am

Is HCl or HBr the stronger acid? Dr. Lavelle said that HBr is the stronger acid, but the bond between HBr is longer than the bond between HCl. Longer bonds are weaker bonds. So now I'm not sure how HBr can be stronger than HCl.

Kaley Qin 1F
Posts: 89
Joined: Wed Sep 30, 2020 9:54 pm

Re: HCl vs. HBr

Postby Kaley Qin 1F » Wed Dec 02, 2020 10:54 am

Due to it's longer bond length, HBr can completely ionize more easily than HCl, meaning HBr can produce more H+ ions than HCl. Since acid strength is based on the number of protons produce, HBr is stronger than HCl.

Shrey Pawar 2A
Posts: 96
Joined: Wed Sep 30, 2020 9:42 pm
Been upvoted: 3 times

Re: HCl vs. HBr

Postby Shrey Pawar 2A » Wed Dec 02, 2020 11:07 am

Just to reinforce what was stated above, being a stronger acid or base does not necessarily have to do with the strength of a bond as much as the acids ability to ionize. In this case, because HBr would have a weaker bond it can more easily ionize and is the stronger acid. Hope this helps!

Andrew Wang 1C
Posts: 90
Joined: Wed Sep 30, 2020 10:11 pm
Been upvoted: 5 times

Re: HCl vs. HBr

Postby Andrew Wang 1C » Wed Dec 02, 2020 11:12 am

So would it be true to say that the weaker the bond, the stronger the acid since it dissociates more easily?

Janelle Gokim 3B
Posts: 110
Joined: Wed Sep 30, 2020 9:42 pm
Been upvoted: 3 times

Re: HCl vs. HBr

Postby Janelle Gokim 3B » Wed Dec 02, 2020 11:16 am

I think that is reasonable to say. That seemed to be the point Dr. Lavelle was making in lecture, that because HBr has a longer and therefore weaker bond, it could ionize more easily in water.

Marisa Gaitan 2D
Posts: 97
Joined: Wed Sep 30, 2020 9:47 pm
Been upvoted: 3 times

Re: HCl vs. HBr

Postby Marisa Gaitan 2D » Wed Dec 02, 2020 11:46 am

Andrew Wang 1G wrote:So would it be true to say that the weaker the bond, the stronger the acid since it dissociates more easily?

I think so, and that is also why HF is a weak acid since it has a shorter and therefore stronger bond than HCl and HBr.

Emmeline Phu 1G
Posts: 110
Joined: Wed Sep 30, 2020 9:52 pm
Been upvoted: 2 times

Re: HCl vs. HBr

Postby Emmeline Phu 1G » Wed Dec 02, 2020 11:59 am

Hi! The HBr bond is longer than HCl but when we are determining the strength of acids we are looking at its ability to ionize or dissociate in a solution. If the bond is weaker in a molecule, it is able to ionize easily (produce more H+ ions) whereas if a bond is stronger it is not able to do so. Strong acids are characterized by its ability to almost completely ionize or dissociate in a solution; therefore, since HBr is able to ionize more easily than HCl, it is a stronger acid. Hope this helps! :)


Return to “Bronsted Acids & Bases”

Who is online

Users browsing this forum: No registered users and 1 guest