mcr90
Harmless
Posts: 1
Registered: 6-6-2014
Member Is Offline
Mood: No Mood
|
|
Soluble/Insoluble oxalate in spinach
I am a graduate student in nutrition. I have no lab experience but have had the opportunity to begin working in a Urology lab for my thesis research
dealing with the bioavailability of oxalate in spinach. I have been assigned the task to isolate oxalate crystals in spinach and view/quantify them
microscopically. Any ideas for a protocol?
|
|
|
blogfast25
International Hazard
Posts: 10562
Registered: 3-2-2008
Location: Neverland
Member Is Offline
Mood: No Mood
|
|
Treat filtered (perhaps centrifuged) spinach juice with calcium chloride (or any other water soluble calcium salt), this will precipitate the acid as
calcium oxalate (CaOx). Filter and wash.
Although poorly soluble it has enough solubility to be able to be displaced with sodium carbonate:
CaOx(s) + Na<sub>2</sub>CO</sub>3</sub>(aq) === > CaCO<sub>3</sub>(s) + Na<sub>2</sub>Ox(aq)
... because CaCO3 is much more insoluble than CaOx.
After filtration, this leaves you with water soluble sodium oxalate in solution. This can be quantified e.g. by titration with potassium permanganate
in acid conditions.
Acc. the wiki entry on oxalic acid, the content in spinach is around 1 g / 100 g, not really microscopic.
[Edited on 6-6-2014 by blogfast25]
|
|
|
thesmug
Hazard to Others
Posts: 370
Registered: 17-1-2014
Location: Chicago, Il (USA)
Member Is Offline
Mood: No Mood
|
|
As for getting the crystals you could either dry them in a dessicator or simply let them stand. Boiling the water might also work.
Good eyes
|
|
|
blogfast25
International Hazard
Posts: 10562
Registered: 3-2-2008
Location: Neverland
Member Is Offline
Mood: No Mood
|
|
Quote: Originally posted by thesmug  | | As for getting the crystals you could either dry them in a dessicator or simply let them stand. Boiling the water might also work.
|
There has to be a lot of other 'crap' in spinach juice. I think the OA needs to be isolated first.
|
|
|
thesmug
Hazard to Others
Posts: 370
Registered: 17-1-2014
Location: Chicago, Il (USA)
Member Is Offline
Mood: No Mood
|
|
Yeah I didn't really think about that. Do you have any ideas on isolating the oxalate?
Good eyes
|
|
|
blogfast25
International Hazard
Posts: 10562
Registered: 3-2-2008
Location: Neverland
Member Is Offline
Mood: No Mood
|
|
You mean the acid? There's various ways to isolate it but I don't see the point for his purpose. You can see oxalic crystals under the microscope all
day long and twice on Sunday: it doesn't teach you anything you can't learn from a jar of 'deck cleaner'.
It should be sufficient to isolate it in a quantifiable way, for instance as an oxalate.
[Edited on 6-6-2014 by blogfast25]
|
|
|
thesmug
Hazard to Others
Posts: 370
Registered: 17-1-2014
Location: Chicago, Il (USA)
Member Is Offline
Mood: No Mood
|
|
I think that the OP requires examining the crystals as part of their project, but I don't see why. To OP: quantifying the crystals seems unnecessary
since it is much easier to quantify oxalate in solution. Would you mind giving us more information?
[Edited on 6/6/14 by thesmug]
Good eyes
|
|
|
phlogiston
International Hazard
Posts: 1375
Registered: 26-4-2008
Location: Neon Thorium Erbium Lanthanum Neodymium Sulphur
Member Is Offline
Mood: pyrophoric
|
|
I'd guess he is interested in isolating the crystals as they occur in the leaves, rather than making a solution of oxalate and precipitating the
calcium salt from that.
I'm pretty sure you could have googled this yourself, as it appears in the first 3 results with trivial keywords but for the purpose of this thread:
Liovando Marciano da Costa et al Rev. Bras. Ciênc. Solo (2009) 33:3
"Extraction and concentration of biogenic calcium oxalate from plant leaves"
| Quote: | The leaves were washed with distilled water to remove impurities and at last rinsed in deionized water. The leaves were cut in smaller pieces, filled
in a heavy-duty blender, and covered with deionized water to 5 cm above the plant material. The device must work until obtaining a greenish juice of
the leaves. The liquefied material was sifted through a 0.20 mm sieve. A sample of 20 crystals extracted from croton leaves was measured and the
values varied from 0.004 to 0.018 mm. The 0.20 mm sieve was adequate to separate the fibrous leaf material from the plant juice and the CaOx crystals.
The plant material retained in the sieve was ground again in the blender. The procedure must be repeated until the plant juice becomes totally clear.
The volume of extracted plant juice was placed in 1000 mL test tubes for sedimentation of the calcium oxalate crystals and plant material. The
sedimentation process must be repeated until the supernatant is light-colored and free of chlorophyll, pigments as well as other organic water-soluble
compounds. The solid material containing the calcium oxalate crystals and other not water-soluble impurities were at the bottom of the test tube. The
supernatant was removed by draining off.
In the end of the extraction, the formed sediment can be transferred to smaller test tubes (100 mL) to concentrate the extracted material. After
concentrating the suspension, the solid product was dried at 60 ºC.
Hydrogen peroxide (30 %) was added to the dry material and the suspension formed was left to rest for 24 h to remove the organic impurities. Hydrogen
peroxide was added until it covering the solid material by 2 cm. After 24 h reacting with the organic substances the CaOx crystals were free of
impurities. The optical microscope was used to observe the purity of the calcium oxalate crystals. The procedure with hydrogen peroxide can be
repeated in case of any remaining impurities. The resulting solid material was washed with deionized water to remove impurities and dried at 60 ºC.
|
[Edited on 6-6-2014 by phlogiston]
-----
"If a rocket goes up, who cares where it comes down, that's not my concern said Wernher von Braun" - Tom Lehrer |
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
