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

Printable Version  
Author: Subject: Sodium Oxalate
Hazard to Others

Posts: 200
Registered: 9-2-2004
Member Is Offline

Mood: No Mood

[*] posted on 7-5-2006 at 10:46
Sodium Oxalate

Would a aqueous reaction between sodium bicarbonate and oxalic acid proceed to forming sodium oxalate, CO<sub>2</sub>, and water, or would I have to use a stronger base like NaOH? If bicarbonate would work, I'd much rather use it.

H<sub>2</sub>C<sub>2</sub>O<sub>4</sub> + 2NaHCO<sub>3</sub> --> Na<sub>2</sub>C<sub>2</sub>O<sub>4</sub> + 2CO<sub>2</sub> +2H<sub>2</sub>O ?
View user's profile View All Posts By User
Post Harlot

Posts: 4803
Registered: 8-3-2005
Location: oscillating
Member Is Offline

Mood: informative

[*] posted on 7-5-2006 at 11:49

As I recall, oxalic acid is strong enough. Can always look up the pKa and compare it to HCO3-.

Even if it weren't, boiling would probably make it work anyway, since heat drives out the CO2 gas that forms (driving the equation you wrote to the right).


Seven Transistor Labs LLC
Electronic Design, from Concept to Layout.
Need engineering assistance? Drop me a message!
View user's profile Visit user's homepage View All Posts By User This user has MSN Messenger

  Go To Top