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Postby JChen_2I » Thu Nov 28, 2019 5:52 pm

Which of the following can be classified as reactions between Bronsted acids and bases? For those that can be so classified, identify the acid and the base.
a) NH4I + H2O -> NH3 + H3O+ + I-
b) NH4I -> NH3 + HI
c) CH3COOH + NH3 -> CH3CONH2 + H2O
d) NH4I + KNH2 -> KI + 2NH3
Could someone explain how to go about solving this problem?

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Joined: Thu Jul 11, 2019 12:17 am

Re: 6A9

Postby SGonzales_3L » Thu Nov 28, 2019 8:36 pm

You know that a Bronsted Acid is a proton donor and a Bronsted Base is a proton acceptor. Go through each of the chemical equations and see if you can identify if one of the compounds is donating a proton to another. For example in a), NH4+ donates a proton to create H3O+. In this equation, H3O+ is the proton acceptor (Bronsted Base) and NH4+ is the proton donor (Bronsted Acid).

Minh Ngo 4G
Posts: 137
Joined: Thu Jul 25, 2019 12:17 am

Re: 6A9

Postby Minh Ngo 4G » Thu Nov 28, 2019 11:19 pm

The way I do it is to look which compound in the products side have gained or lost a H+. If it has gained then the similar reactant must have been a base and vice versa

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