Acid vs Base

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A Raab 1K
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Joined: Sat Aug 24, 2019 12:16 am

Acid vs Base

Postby A Raab 1K » Thu Nov 28, 2019 12:31 pm

How do you tell the difference between a Bronsted acid and base?
For example, in J1, it asks you to identify (a) NH3 ; (b) HBr; (c) KOH; (d) H2SO3; (e) Ca(OH)2
I understand that for c and e, there's an OH in the compound which leads one to believe it's a base. Is this line of thinking correct?
Additionally, how do you tell for a, b, and d though?

Justin Vayakone 1C
Posts: 110
Joined: Sat Sep 07, 2019 12:19 am

Re: Acid vs Base

Postby Justin Vayakone 1C » Thu Nov 28, 2019 12:58 pm

Yeah generally, molecules with OH will indicate a bronsted base and H for bronsted acids. For part a though, NH3 (ammonia) is a base. It will gain a proton to become NH4 (ammonium). Memorizing some of the common acids and bases will help in figuring out these molecules. B and D are the acids, while A, C, and E are the bases.

Catherine Daye 1L
Posts: 104
Joined: Wed Sep 11, 2019 12:16 am

Re: Acid vs Base

Postby Catherine Daye 1L » Thu Nov 28, 2019 3:45 pm

A Bronsted acid is distinguished by starting with H, and a Bronsted base usually ends with OH.

Lauren Tanaka 1A
Posts: 109
Joined: Sat Aug 17, 2019 12:18 am

Re: Acid vs Base

Postby Lauren Tanaka 1A » Fri Nov 29, 2019 1:52 pm

Since the Bronsted acids are proton donors, you can usually identify them with an H at the beginning of the molecule. The Bronsted bases are proton acceptors and usually consist of a hydroxide group

Posts: 71
Joined: Sat Aug 24, 2019 12:16 am

Re: Acid vs Base

Postby ZainAlrawi_1J » Fri Nov 29, 2019 2:32 pm

Bronsted acids usually start with a Hydrogen "H" atom, while Bronsted bases usually end in an Oxygen and Hydrogen "OH"

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