Week 10 Sapling Q10

[KatarinaReid_3H]

I am wondering why HBr is a stronger acid than HBrO? I would think that the O would bring extra stability, thus HBrO should be stronger, but Sapling said the correct answer is the other way around.

[Anna_Mohling_1D]

I'm not completely sure what the reasoning is but HBr is a strong acid so I would just memorize all of the strong acids because then it's easy to do the process of elimination!

[KatarinaReid_3H]

It turns out they are completely different lewis structures. The H is bonded to the O in HBrO, therefore we look at the bond length and O has a much shorter, stronger bond so it is a weaker acid.

[Nick Saeedi 1I]

HBr is a strong acid and HBrO is not on the list of strong acids so HBr is stronger.

[Savannah Torella 1L]

As stated above, HBr is only the list of strong acids while HBrO is not, so HBr is automatically a stronger acid. For a reminder the list of strong acids is below.
Strong acids:
HCl
HBr
HI
H2SO4
HNO3
HClO4
HClO3

[Sonel Raj 3I]

My understanding is that you'd have to look at where the H is bonded to. I'd assume, for HBrO, the H is bonded to the O. It's easier to remove a hydrogen proton from Br than it is to break an H--O bond, so HBr would be the stronger acid. Also, like it's stated above, HBr is listed as a strong acid, so I'd recommend memorizing those.

[Ralph Zhang 2L]

There's a set list of strong acids and bases that you should memorize. HBr belongs in the list of strong acids so it is automatically stronger than the others.