Homework Question

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Homework Question

Postby 105194078 » Tue Dec 03, 2019 11:58 pm

Can anyone explain to me why H2SO3 is a Bronsted Acid? I tried to explain it to myself but I got more confused.

Nawal Dandachi 1G
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Joined: Sat Sep 28, 2019 12:16 am

Re: Homework Question

Postby Nawal Dandachi 1G » Wed Dec 04, 2019 12:01 am

so basically in H2SO3, we know that it contains SO32- sulfite anion. so we can assume that H2SO3 will donate two protons

Brynne Burrows 3K
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Joined: Thu Jul 25, 2019 12:16 am

Re: Homework Question

Postby Brynne Burrows 3K » Wed Dec 04, 2019 12:07 am

Also, this molecule is not likely to gain more protons because of its stability so it cannot be a Bronsted base (proton acceptor). If you look at the conjugate base SO3]2- this is a stable anion with resonance. It is a conjugate base of a strong acid which will completely dissociate in water and give all its protons, creating a high concentration of H30+ ions which makes the pH low, which also tells that it's very acidic.

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