03-31-04 03:26
No 498199
I searched for the solubility of oxalic acid on the internet and found this:
http://voh.chem.ucla.edu/vohtar/spring98
1. An organic chemistry lab book gives the following solubility data for oxalic acid (IUPAC name - ethanedioic acid)
9.5 g/100mL of water 23.7 g/100 mL of ethanol 16.9 g/100 mL of ether
It is nice to see that oxalic acid dissolves in ethanol, but for setting up some Mannich reaction procedure, I 'd like to know if these figures are accurate.
I found this in some basic organic chemistry textbook (Morrison & Boyd, 6th ed., Organic chemistry p 742), which has a funny cartoon on page 474.
It goes like this: Donnald duck walks towards his lab table saying: 'If I mix CH2 (edit: methylene, formed by the ultraviolet light photolysis of diazomethane
) with NH4 and boil the atoms in osmotic fog, I should get speckled nitrogen'. At the same time his 3 nephews are saying each seperately:* He 's talking chemical talk !
* But he knows nothing
* about chemicals !
Anyway, the book says (p 742) that the solubility of oxalic acid is 9 g / 100 g H2O at 20 °C.
Could someone give me an accurate figure of the solubility of oxalic acid in ethanol (this is my primary interest, because a solution of formaldehyde / amine / ethanol is going to bee dropped slowely into an ethanolic solution of ketone and oxalic acid).
(Hive Bee)
03-31-04 23:50
No 498340
I guess his ref. was:
James W. Zubrick, "The Organic Chem Lab Survival Manual", 4th Ed., John Wiley & Sons, 1997, so the info should be correct.
Post 453799 (Rhodium: "Theory of Extraction", Newbee Forum)
(acetaminophanatic)
04-17-04 07:07
No 501218
Is really, really temperature dependent too. It gets much higher than what you see. I remember calculating that if one were to take a saturated boiling soln. to almost freezing, they would gather in crystals around 90 - 95 % of their acid.
I've been chased by both cops and robbers. So what does that make me?