Which of the following is not amphiprotic?
a)H2O
c)NH4+
e)all choices are amphiprotic
b)HSO4 –
d)H2PO4–
need help!
Do you know what amphiprotic means? It means the material can act both as an acid and a base. H2O can do that.
H^+ + H2O ==> H2O^+
H2O + H2O ==> H2O^+ + OH^-
What about HSO4^-? it can donate a proton as in the first equation below; it can accept a proton as in the second equation.
I can get HSO4^- ==> H^+ + SO4^- or
HSO4^- + H^+ ==> H2SO4
Well, isn't it just a party with all these amphiprotic options? But fear not, my friend, for I shall guide you through this chemical fiesta!
Now, amphiprotic species are those marvelous molecules or ions that can both donate and accept protons. We want to find the one that is NOT on the amphiprotic guest list.
Let's take a closer look, shall we?
a) H2O: Oh, our good old friend water! It's definitely amphiprotic. It can both donate and accept protons. So, H2O is not the answer we seek.
b) HSO4 –: Well, well, well, look who showed up to the party! This lovely little ion can both donate and accept protons, making it amphiprotic. So, HSO4 – is not the answer we're looking for here.
c) NH4+: Ah, ammonium! Quite the player in the acid-base game. Ammonium ions can accept protons, becoming ammonia (NH3). So, this fellow is definitely amphiprotic!
d) H2PO4–: Phosphoric acid it is! This ion can donate not just one, but two protons - quite the overachiever! So, H2PO4– is indeed amphiprotic.
e) All choices are amphiprotic: Ah, a tempting option! But let me tell you, my curious companion, that there is one sneaky molecule that doesn't quite fit the amphiprotic bill. And that molecule is...
Bump-a-dee-bump...
The answer is: e) all choices are amphiprotic! Oh, the irony! You see, while water (H2O), HSO4 –, NH4+, and H2PO4– are indeed amphiprotic, not all options can join the amphiprotic club. It's easier to spot the odd one out when they're all the same, isn't it?
And off we go, enlightening minds with the magic of chemistry!
To determine which of the given choices is not amphiprotic, we need to understand what amphiprotic means. An amphiprotic substance is one that can both donate and accept protons (H+ ions).
a) H2O is amphiprotic because it can donate a proton to form OH- or accept a proton to form H3O+.
b) HSO4- is amphiprotic because it can donate a proton to form SO42- or accept a proton to form H2SO4.
c) NH4+ is not amphiprotic because it can only donate a proton to form NH3, it cannot accept a proton.
d) H2PO4- is amphiprotic because it can donate a proton to form HPO42- or accept a proton to form H3PO4.
e) Since NH4+ is not amphiprotic, the correct answer is option c) NH4+.
Therefore, NH4+ is the substance that is not amphiprotic among the given choices.
To determine which of the following compounds is not amphiprotic, we need to understand what it means for a substance to be amphiprotic.
Amphiprotic substances are capable of both accepting and donating a proton (H+ ion). Therefore, we need to consider whether each compound is capable of both accepting and donating a proton.
Let's go through the options:
a) H2O (water) is amphiprotic because it can act as both a proton donor (H2O → H+ + OH-) and a proton acceptor (H2O + H+ → H3O+).
b) HSO4- (bisulfate ion) is amphiprotic because it can act as both a proton donor (HSO4- → H+ + SO4^2-) and a proton acceptor (HSO4- + H+ → H2SO4).
c) NH4+ (ammonium ion) is not amphiprotic because it can only act as a proton donor (NH4+ → NH3 + H+). It cannot accept a proton.
d) H2PO4- (dihydrogen phosphate ion) is amphiprotic because it can act as both a proton donor (H2PO4- → HPO4^2- + H+) and a proton acceptor (H2PO4- + H+ → H3PO4).
e) The statement "all choices are amphiprotic" is not correct because NH4+ is not amphiprotic.
Therefore, the correct answer is: c) NH4+. It is not amphiprotic because it can only act as a proton donor, not as a proton acceptor.