April 25, 2024, 03:30:07 PM
Forum Rules: Read This Before Posting


« previous next »
Pages: 1 [2]   Go Down

Topic: Ammonium Hydroxide  (Read 14406 times)

0 Members and 1 Guest are viewing this topic.

Offline pzona69

  • Regular Member
  • ***
  • Posts: 42
  • Mole Snacks: +1/-1
Re: Ammonium Hydroxide
« Reply #15 on: January 20, 2008, 04:29:30 PM »
That's what I thought at first, that it would just be an acid base reaction, which is why I wanted to isolate NH3. 
Logged

Offline Kryolith

  • Full Member
  • ****
  • Posts: 269
  • Mole Snacks: +19/-4
  • Gender: Male
Re: Ammonium Hydroxide
« Reply #16 on: January 20, 2008, 04:35:43 PM »
The dehydration of ammonium acetate should yield acetamide. It's easier to answer questions if I know from the beginning what exactly you want to do/know.
Logged

Offline pzona69

  • Regular Member
  • ***
  • Posts: 42
  • Mole Snacks: +1/-1
Re: Ammonium Hydroxide
« Reply #17 on: January 20, 2008, 04:39:05 PM »
Yeah I realize that, my fault for not saying in the original post.
Logged

Offline Kryolith

  • Full Member
  • ****
  • Posts: 269
  • Mole Snacks: +19/-4
  • Gender: Male
Re: Ammonium Hydroxide
« Reply #18 on: January 20, 2008, 04:43:44 PM »
No problem. It resulted in an interesting discussion about the structures of ammonia in water  :)
Logged

Offline Kryolith

  • Full Member
  • ****
  • Posts: 269
  • Mole Snacks: +19/-4
  • Gender: Male
Re: Ammonium Hydroxide
« Reply #19 on: January 25, 2008, 06:23:30 PM »
Just another thought: In the case of hydrochloric acid the equilibrium is approximately complete on the right side. And does anybody call it "oxonium chloride"?  :)
Logged
Pages: 1 [2]   Go Up
« previous next »
Sponsored Links