<p>All of the following can act as Brønsted- Lowry acids (proton donors) in aqueous solution EXCEPT</p>
<p>(A) HI (B) NH+ (C) HCO 43
(D) H2S (E) NH3</p>
<p>A Bronsted-Lowry acid is defined as a proton donor, so it is able to “donate” an H. NH3 is a bronsted-lowry base, rather it is an acceptor of an H, becoming NH4. It will never donate an H to form NH2.</p>
<p>How do you know that NH3 will never donate a proton, but H2S might?</p>
<p>NH3 cannot donate a H+ because the compound NH2 does not exist in nature; it is part of the functional group amine. H2S can donate a H+ to form HS-.</p>
<p>^What SmySmy said.</p>