HI or HCl: stronger acid

[Isabelle De Rego 1A]

On the French toast exam (#28) it lists the answer as HI as the stronger acid.
I picked HCl because I thought that since HCl had more ionic properties, it would hog electrons and make it easier for H to disassociate in water. Wouldn't HI have a harder time doing so, and thus make it a weaker acid?

[JulietOttenberg-1C]

HI has a larger atomic radius so it is dissociates easier than HCl

[Kara Justeson 1B]

is this an exception to the general trend? Because I thought more electronegative atoms formed stronger acids.

[Andrew Evans - 1G]

More electronegative what I would call "accessory atoms" would cause a stronger base. So when an H⁺ proton dissociates from an oxygen lets say, are there other electronegative atoms attached to that original molecule that will be able to pull that charge away from the O and distribute it among the rest of the molecule, stabilizing the new anion. This allows it to be a stronger base.

For acids it is not quite so and just because it is more ionic doesn't mean it's a stronger acid.

[Megan Phan 1K]

HI would be the stronger acid, as iodine's atomic radius is much larger than Cl's. So iodine is more evenly distributed when ionized

[Bingcui Guo]

How to define strong acid and weak acid depends on the easiness to lose an electron. Since the bond of H and I is easier to break than H and Cl, it is easier for HI to lose H+ and thus it is a stronger acid than HCl.

[105002507]

HI would be the stronger acid

[Sang Hyoun Hong 3G]

HI would be the stronger acid due to its larger atomic radius.

[Nawaphan Watanasirisuk 3B]

HI has longer bond than HCl, making its bond weaker. Therefore it is easier for HI to lose H+, making it a stronger acid.