Conjugate acids vs conjugate base

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Monica Soliman 3F
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Conjugate acids vs conjugate base

Postby Monica Soliman 3F » Thu Dec 03, 2020 7:27 pm

I understand how to identify a conjugate acid vs. conjugate base, but I do not understand how to give a formula for conjugate acid or conjugate base? example(below)
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Ryan Laureano 3I
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Re: Conjugate acids vs conjugate base

Postby Ryan Laureano 3I » Thu Dec 03, 2020 10:31 pm

Conjugate acid is the original formula plus a hydrogen ion. Conjugate base is minus a hydrogen ion.

kateraelDis1L
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Re: Conjugate acids vs conjugate base

Postby kateraelDis1L » Thu Dec 03, 2020 11:05 pm

I don't think this has been covered in lecture yet. Has it? So don't worry about now knowing how to do that rn.

Savana Maxfield 3F
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Re: Conjugate acids vs conjugate base

Postby Savana Maxfield 3F » Thu Dec 03, 2020 11:19 pm

It has not been covered in lecture quite yet, but it will be on the final!

Kamille Kibria 2A
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Re: Conjugate acids vs conjugate base

Postby Kamille Kibria 2A » Sat Dec 05, 2020 3:35 pm

an acid ionizes to make H+ and its conjugate base while a base combines w/ H+ to make its conjugate acid. basically the conjugate base you subtract one proton, so HSO4^- would become SO4^-2. for the conjugate acid you add one proton, so HSO4^- would become H2SO4.

Nan_Guan_1L
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Re: Conjugate acids vs conjugate base

Postby Nan_Guan_1L » Sun Dec 06, 2020 10:00 am

To find the conjugate base, you remove a proton, which would give you SO4-. To find the conjugate acid, you add a proton, which would give you H2SO4. Hope that helps!

David Y
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Re: Conjugate acids vs conjugate base

Postby David Y » Sun Dec 06, 2020 4:18 pm

conjugate acid has an added hydrogen ion

Karina Grover 1A
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Re: Conjugate acids vs conjugate base

Postby Karina Grover 1A » Sun Dec 06, 2020 4:24 pm

Basically, the conjugate acid includes the attachment of a proton to the base, and the conjugate base involves the removal of a proton from the acid. In this case, the conjugate base will be SO4^2- and the conjugate acid is H2SO4!

Shana Patel 1C
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Re: Conjugate acids vs conjugate base

Postby Shana Patel 1C » Sun Dec 06, 2020 4:27 pm

The conjugate base of a Bronsted-Lowry acid is the species formed after an acid donates a proton.
The conjugate acid of a Bronsted-Lowry base is the species formed after a base accepts a proton.

FionaHunter21
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Re: Conjugate acids vs conjugate base

Postby FionaHunter21 » Sun Dec 06, 2020 4:50 pm

So the acid gives a proton and the base accepts it, so the conjugate base of an acid would lose an H+ ion, and the conjugate acid of a base would gain an H+ ion?

Ava Nickman
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Re: Conjugate acids vs conjugate base

Postby Ava Nickman » Sun Dec 06, 2020 4:54 pm

The conjugate acid has an addition H+ while the conjugate base takes away an H+

Joshua Swift
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Re: Conjugate acids vs conjugate base

Postby Joshua Swift » Sun Dec 06, 2020 7:04 pm

For your conjugate acid you take the original formula and add a hydrogen. You take a hydrogen out of it to find your conjugate base.

David Facio 1K
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Re: Conjugate acids vs conjugate base

Postby David Facio 1K » Sun Dec 06, 2020 7:18 pm

Acid-base conjugate pairs differ by just one H+ ion and always occur together

For example, in the following scenarios:

A) NH3 + H2O ---> NH4+ + OH-

The conjugate base is OH-

and the conjugate acid is NH4+




Similarly in

B) HCl + H20 ---> Cl- + H3O+

The conjugate base is Cl-

and the conjugate acid is H3O+



Hope this helps :)


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