Please help! ACID/BASE QUESTION?

Question

Which is not a Bronsted-Lowry reaction?
a) NH4+ + NH2- -> 2NH3
b) CO2 + OH- -> HCO3-
c) HClO4 + CH3COOH -> CH3COOH2+ + ClO4-
d) CH3CH2O- + CH3NH3+ -> CH3CH2OH + CH3NH2

I don't understand why it's b. Also, for c isnt both of them acid? So
do they both proton donate? And since HClO4 is a strong acid, does that have
something to do with it?
And for d) how do you which is an acid and which is a base?

Answer 1

Best Answer - Chosen by Asker

Identify proton donor and proton acceptor for a Bronsted-Lowry acid/base reaction.

(b) there is NO proton (H+) donated or accepted. CO2 and OH- have undergone an addition reaction to make the Hydrogen Carbonate ion.

(c) HClO4 has donated a proton to ethanoic acid, a weak acid which in this case has ACCEPTED a proton and therefore acted as a base.

(d) the ethoxide ion has accepted a proton from the methylammonium ion, so tha latter is the acid, the former is the base.

Asker's Rating:

Asker's Comment:

Thank-you so much. Your explanation is really good. o: