Sciencemadness Discussion Board
Not logged in [Login ]
Go To Bottom

Printable Version  
Author: Subject: Sulfamic acid
Scratch-
Hazard to Self
**




Posts: 60
Registered: 22-2-2005
Location: U.S.
Member Is Offline

Mood: No Mood

[*] posted on 24-2-2005 at 15:38
Sulfamic acid


I have read some of the other posts here on sulfamic acid, I was wondering if I could make H2SO4 in a solution so I dont run the risk of blowing up my good glassware. When I set up some better apperatus I was going to use the S + KNO3 => SO3 + KN reaction.
View user's profile Visit user's homepage View All Posts By User This user has MSN Messenger
neutrino
International Hazard
*****




Posts: 1583
Registered: 20-8-2004
Location: USA
Member Is Offline

Mood: oscillating

[*] posted on 24-2-2005 at 17:17


H<sub>2</sub>SO<sub>4</sub> is sulfuric acid
Sulfamic acid = HSO<sub>3</sub>NH<sub>2</sub>
View user's profile View All Posts By User
JohnWW
International Hazard
*****




Posts: 2849
Registered: 27-7-2004
Location: New Zealand
Member Is Offline

Mood: No Mood

[*] posted on 24-2-2005 at 18:40


In aqueous solution, it would probably exist as a zwitterion, with both negative and positive charges, like an organic amino-acid, (-)SO3-NH3(+).
View user's profile View All Posts By User
Scratch-
Hazard to Self
**




Posts: 60
Registered: 22-2-2005
Location: U.S.
Member Is Offline

Mood: No Mood

[*] posted on 25-2-2005 at 12:44


Atually, I looked up its structure (See picture below). Its MSDS says:

"Decomposes with heat (209°C) to release sulfur dioxide (SO2), sulfur trioxide (SO3), nitrogen (N2), water (H2O), and ammonia gas (NH3)."

Also:

"Hazardous reaction in aqueous solution may occur with chlorine, hypochlorous acid, hypochlorites, cyanides, nitric acid, or sulfides. An explosion occurred when chlorine was being passed at room temperature into a reaction mixture which included sulfamic acid and water. It is suspected that nitrogen trichloride, a very sensitive explosive, was formed. Fuming nitric acid combined with sulfamic acid causes violent releases of nitrous oxide."

So wow, I'm glad I know that now.

I was using it to dissolve pennies, which I was trying to get the zinc out of. I was then going to use my pathetic Drano crystals NaOH to precipitate out fairly pure zinc powder (I would just need to remove the soap and aluminum from the NaOH, which is in clumps). Reverend Necroticus Rex tells me that zinc sulfamate (Is that name correct?) is a powerful reducing agent.

Do any of you think I could get SO3 (Safely) out of this and thus anhydrous sulfuric acid?

Sulfamic.jpg - 2kB
View user's profile Visit user's homepage View All Posts By User This user has MSN Messenger
Reverend Necroticus Rex
Hazard to Others
***




Posts: 196
Registered: 15-6-2004
Location: Right behind you.......
Member Is Offline

Mood: Poisonous

[*] posted on 25-2-2005 at 19:00


I didn't actually mean that the sulfamate salt itself was a reducing agent, I'm not too sure about that.

I read that in a few MSDS sheets, and I think they might mean, that it erodes the surface layer of oxides on the metal, in a similar way to the action of HgCl on aluminium foil, as used in for...certain types of organic chemistry;)




The sun is shining on a brand new day
Blackened corpses burn where they were slain
Self-flagellation prompts him to confess, Bless me father, for I made this mess.
View user's profile View All Posts By User This user has MSN Messenger

  Go To Top