From the list below, pick the one species that cannot act as both a Bronsted-Lowry acid and base.
A. HCO3-
B. H2SO4-
C. H2PO4-
D. OH-
E. HPO42-
I used to know how to do these; I understand that a conjugate acid has one more H, and a conjugate base has one fewer. I'm trying to get back in the swing of things to take Organic Chemistry 1 this Fall, so I'd appreciate any help offered...
I'm *thinking* the answer is OH-?
2007-08-12 09:10:10 · 4 answers · asked by Henry H 1 in Science & Mathematics ➔ Chemistry
H2SO4- - there is no such species. If you mean HSO4-, that is amphoteric.
OH- can both lose and gain a proton.
2007-08-12 10:31:20 · answer #1 · answered by Gervald F 7 · 0⤊ 0⤋
You are correct. If OH- were to act as a Bronsted acid, it would become O=, which is ridiculous. It can be a Bronsted base, forming H2O as the conjugate acid.
2007-08-12 10:33:56 · answer #2 · answered by steve_geo1 7 · 0⤊ 0⤋
D is the answer.it can only act as a base by accepting protons from an bronsted-lowry acid.
2007-08-12 15:41:22 · answer #3 · answered by Dr. Eddie 6 · 0⤊ 0⤋
yaaa that makes sense....D
2007-08-12 13:32:01 · answer #4 · answered by Anonymous · 0⤊ 0⤋