Difference between Bronsted Acids and Bases

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DTingey_1C
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Joined: Fri Aug 30, 2019 12:16 am

Difference between Bronsted Acids and Bases

Postby DTingey_1C » Mon Nov 25, 2019 1:11 pm

In problem J.1, you are asked to identify bronsted acids and bases. It says NH3 is a base and H2SO3 is an acid. How can you tell the difference? Is it because NH3 has a lone pair that allows it to receive H+ ions? Or is it because it has 3 H atoms and usually molecules with more than 2 H atoms are basic? Thank you.

Qiu Ya Wu 4I
Posts: 107
Joined: Fri Sep 20, 2019 12:17 am

Re: Difference between Bronsted Acids and Bases

Postby Qiu Ya Wu 4I » Mon Nov 25, 2019 1:29 pm

Bronsted acids are defined as proton donors while Bronsted bases are defined as proton acceptors. In this case, the NH3 is a Bronsted base since a H+ ion (really just a proton) could bond to the N as it has an extra unoccupied bonding site. I'm not sure if you could make the generalization that molecules with 2 H atoms are usually basic though; I think it depends on the molecule as a whole.


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