Acids and Bases

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Acids and Bases

Postby kpang_4H » Sun Dec 01, 2019 6:05 pm

Can someone explain the difference between conjugate, Bronsted, and Lewis acids and bases?

JonathanS 1H
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Joined: Thu Jul 11, 2019 12:17 am

Re: Acids and Bases

Postby JonathanS 1H » Sun Dec 01, 2019 6:08 pm

Bronsted acids are proton, or H+ donators. Bronsted bases are proton acceptors. Conjugate acids are bronsted bases that have accepted a proton. Conjugate bases are bronsted acids that have donated a proton. Lewis acids are electron acceptors, while lewis bases are electron donators.

Nicholas Chin 1G
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Re: Acids and Bases

Postby Nicholas Chin 1G » Sun Dec 01, 2019 6:10 pm

They're basically all referring to the same thing, but just approach it differently. Lewis acids are molecules that accept an electron pair, while lewis bases donate an electron pair. Bronsted acids donate a proton, while Bronsted bases accept a proton. Conjugate acids and bases are a little different, because they are specific to reactions. They are the result of a base becoming an acid or an acid becoming a base. For example, HCl is an acid, and when it dissociates in water its conjugate base would be chlorine (which is a very weak base, but still a base).

Michelle Shin 4B
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Joined: Thu Jul 25, 2019 12:17 am

Re: Acids and Bases

Postby Michelle Shin 4B » Sun Dec 01, 2019 6:12 pm

A conjugate acid is the species that is formed after the base accepts a proton, and a conjugate base is formed after an acid donates a proton. Bronsted acids are defined as H+ donors while Lewis acids are defined as electron pair acceptors.

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