12.9 d

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Eryn Wilkinson 3H
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Joined: Fri Sep 29, 2017 7:07 am

12.9 d

Postby Eryn Wilkinson 3H » Fri Dec 08, 2017 10:31 am

I see how the equation NH4I (am) + KNH2 (am) > KI (am) + 2NH3 (l) is a Bronsted reaction, and NH4+ is the acid and NH2- is the base, but I am confused on what their conjugates would be. Do all Bronsted reactions have conjugate acid/base pairs?

Mika Sonnleitner 1A
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Joined: Fri Sep 29, 2017 7:04 am
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Re: 12.9 d

Postby Mika Sonnleitner 1A » Fri Dec 08, 2017 4:25 pm

For part (d), it is helpful to write the net ionic equation:
NH4I (am) + KNH2 (am) --> KI (am) + 2 NH3 (l)
NH4+ + I- + K+ + NH2- --> K+ + I- + 2 NH3
This simplifies to: NH4+ + NH2- --> 2 NH3
In this case, NH3 is the conjugate acid of NH2-, because when NH2- accepts a proton, it becomes NH3 (Bronsted definition).

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