Magpie
lab constructor
Posts: 5939
Registered: 1-11-2003
Location: USA
Member Is Offline
Mood: Chemistry: the subtle science.
|
|
titration of formaldehyde
The video linked below shows how to titrate for the determination of formaldehyde. I don't understand the chemistry behind this, ie, how does Na2S
react with formaldehyde. Can anyone please enlighten me?
https://www.youtube.com/watch?v=NqNZ3W5Hki8
The single most important condition for a successful synthesis is good mixing - Nicodem
|
|
|
Ozone
International Hazard
Posts: 1269
Registered: 28-7-2005
Location: Good Olde USA
Member Is Offline
Mood: Integrated
|
|
I'm figuring that the Na2S dissociates in water to give:
NaS2 + H2O --> NaHS + NaOH, overall: NaS2 + 2H2O --> H2S + 2 NaOH
The H2S reacts with the formaldehyde to give trithiane (and probably some other gunge) leaving NaOH to be titrated with sulfuric acid.
I'm also supposing that (most) all of the Na2S dissociates and some of the NaOH reacts with the formaldehyde. The remaining NaOH would be titrated. I
imagine a quantitative result being calculated by difference and by assuming that the amount of Na2S is exactly (within the error of the method) the
same every time.
I suppose this would be OK for a fixed (and high) range of formaldehyde, say a final product. Much less useful, I think, for looking at a wider range
of concentrations (without modification of sample amounts, titrant/Na2S strength, etc.).
I'd (highly) recommend the H2SO4/chromotropic acid UV-VIS assay:
http://www.cdc.gov/niosh/docs/2003-154/pdfs/3500.pdf
Or, derivatization with DNPH at pH 4.5 (citrate buffer), extraction with DCM, solvent exchange into MeCN, and quantitation via HPLC (C18, MeCN:H2O
gradient, ABS 360 nm). TLC works, too, but it is much harder to get good chromatograms by densitometry (although some freeware is available that can
work with photos, IIRC).
See, for example: http://chromsci.oxfordjournals.org/content/41/7/359.full.pdf
And, the creation of an "affordable" scanning densitometer:
http://www.framboise314.fr/docs/aflatoxines.pdf
O3
[Edited on 8-2-2016 by Ozone]
-Anyone who never made a mistake never tried anything new.
--Albert Einstein
|
|
|
Magpie
lab constructor
Posts: 5939
Registered: 1-11-2003
Location: USA
Member Is Offline
Mood: Chemistry: the subtle science.
|
|
Quote: Originally posted by Ozone  |
The H2S reacts with the formaldehyde to give trithiane (and probably some other gunge) leaving NaOH to be titrated with sulfuric acid.
|
But how does this change the amount of acid/base to be titrated?
Unless you mean it decreases the amount of the acid H2S.
I was wondering if somehow the formaldehyde was oxidized to formic acid - but I don't see how.
The single most important condition for a successful synthesis is good mixing - Nicodem
|
|
|
clearly_not_atara
International Hazard
Posts: 2786
Registered: 3-11-2013
Member Is Online
Mood: Big
|
|
First note: in the video H2SO4 is added to a solution of Na2S. While this can be done without releasing H2S (up to a point), a single mistake can
kill you, so don't do it without a hood.
Anywho the relevant equilibria are:
H2S <> H+ + SH-
3H2CO + 3H2S <> (H2CS)3 + 3H2O
H2O <> H+ + OH-
Since H2S is a stronger acid than H2O it follows that increasing the concentration of H2CO decreases the concentration of protons.
[Edited on 8-2-2016 by clearly_not_atara]
|
|
|
Magpie
lab constructor
Posts: 5939
Registered: 1-11-2003
Location: USA
Member Is Offline
Mood: Chemistry: the subtle science.
|
|
I see now if trithiane is formed this consumes the H2S and formaldehyde, thus reducing the acidity.
The single most important condition for a successful synthesis is good mixing - Nicodem
|
|
|
Dr.Bob
International Hazard
Posts: 2732
Registered: 26-1-2011
Location: USA - NC
Member Is Offline
Mood: No Mood
|
|
I would agree that forming a hydrazone (NHPH) might be easier to do as a colormetric type assay.
Perhaps you could add some urea or phenol and heat to form a polymer and then weigh the glob of goo that you get after drying it. I made Bakelite as
a kid that way.
The H2S sounds like it would work, but I found several other methods with a quick search:
http://www.jbc.org/content/105/1/157.full.pdf for more details on the acidity of formaldehyde.
The sodium sulfite method. Add an excess of sodium sulfite solution to the formaldehyde solution, then titrate with sulphuric acid and
phenolphtaleine. The following reaction applies:
CH2O + Na2SO3 + H2O → NaOH + Na[H2CSO4]
Walker, J. F.; Formaldehyde; ACS Monograph Series, 1964
---------
Abbas Afkhami and Mostafa Rezaei, Determination of Formaldehyde by Inhibition of the Malachite Green–Sulfite Reaction, Microchemical Journal 63,
243–249 (1999).
---------------
The hydroxylamine method for determining formaldehyde in my researches
The oximation reaction is carried out with hydroxylamine HCl which is very stable.
Each mole of oxime formed results in the formation of one mole of HCl which can be titrated with standard alkali to give a measure of the carbonyl in
the sample.
------------
The best way for determining formaldehyde is by using colorimetric determination using Florescence/UV-vis spectroscopy. You need to do
standardization first (using titration as mentioned by Oliver which is available in Walker, Formaldehyde book) and using known formaldehyde
concentration solutions that you prepared from your standard formaldehyde solution, you need to make your calibration curve using Florescence/UV-vis
spectroscopy.
In order to detect formaldehyde with spectroscopy method, you need to react your formaldehyde solution with acetylacetone reagent, in this reaction
each mole of formaldehyde will turn into a compound which has double bond and can be detected with spectroscopy methods. you can review this method in
the following pubs:
Nash, T. 1953. The colorimetric estimation of formaldehyde by means of the Hantzsch reaction. Biochem J 55: 416-421.
Belman, S. 1963. The fluorimetric determination of formaldehyde. Anal Chim Acta 29: 120-126
Walker, J.F. 1975. Formaldehyde: Krieger Publishing Co., Huntington, N.Y.
----------------
[Edited on 9-2-2016 by Dr.Bob]
|
|
|
Ozone
International Hazard
Posts: 1269
Registered: 28-7-2005
Location: Good Olde USA
Member Is Offline
Mood: Integrated
|
|
Pretty much. But, the dependence of NaOH on the quantity of formaldehyde present would only be proportional if the formation of trithiane drove the
dissociation of the Na2S. Because I know this dissociation in water will happen spontaneously, the proportionality would only exist for some short
while--that is, you must mix the stuff and titrate it immediately. I imagine a reagent blank would also be required.
Anyhow, yeah, the sulfite titration is probably easier, but I still like the chromotropic acid assay: Make a standard curve with formaldehyde in
water, treat with chromotropic acid (see NIOSH method) and add 75% H2SO4 (we used 98% into a small sample aliquot in Hach tubes). The complex is
bright purple and linear with concentration. The standard curve is good for months (you can keep the sealed set in a drawer or box in the hood), and
you can read Hach tubes in most (cheap, VIS only) spectrophotometers (with appropriate adapter). Easy, accurate, and reproducible if you can get the
reagent (Hach sells the pillows/reagents, but it's always cheaper to make your own) and the acid.
Apparently, you can also get away from the concentrated H2SO4 with a mixture of HCl and H2O2:
http://www.sciencedirect.com/science/article/pii/S0039914003...
I also think the Hantzsch rxn with acetylacetone looks good, too. Nice find.
Cheers,
O3
-Anyone who never made a mistake never tried anything new.
--Albert Einstein
|
|
|
blogfast25
International Hazard
Posts: 10562
Registered: 3-2-2008
Location: Neverland
Member Is Offline
Mood: No Mood
|
|
Wouldn't it be simpler to titrate CHO with KMnO4 in acidic conditions, using the permanganate's colour as a natural indicator?
|
|
|
Magpie
lab constructor
Posts: 5939
Registered: 1-11-2003
Location: USA
Member Is Offline
Mood: Chemistry: the subtle science.
|
|
I could do the sulfite and hydroxylamine HCL methods with the chemicals on hand. I don't have a spectrometer so the colorimetric methods are out.
Use of KMnO4 sounds like a possibility.
Actually I couldn't do the Na2S method either as I have no thymolphthalein indicator. BTW, that looks like it might be fun to make if thymol is OTC
at the grocery store in oil of thyme.
Thanks to all for the help.
The single most important condition for a successful synthesis is good mixing - Nicodem
|
|
|
blogfast25
International Hazard
Posts: 10562
Registered: 3-2-2008
Location: Neverland
Member Is Offline
Mood: No Mood
|
|
| Quote: Originally posted by Magpie | I could do the sulfite and hydroxylamine HCL methods with the chemicals on hand. I don't have a spectrometer so the colorimetric methods are out.
|
HCL!!!! Aaarghgh!!!! 
You don't need a spectrometer for titrations involving KMnO4, unless you call your eyes spectrometers.
My only concern is reaction speed but aldehydes are so easily oxidised, I can't see a problem there. Oxalic acid (to CO2) is used to
standardise KMnO4, so 'go figure'! 
|
|
|
Ozone
International Hazard
Posts: 1269
Registered: 28-7-2005
Location: Good Olde USA
Member Is Offline
Mood: Integrated
|
|
So long as your solutions contain only formaldehyde, then KMnO4 is a great idea. See also, Jone's reagent (Dichromate in H2SO4). While I agree that
acidic pH will help with selectivity, I've got to recommend a matrix blank to rule out oxidation of other components that might be present.
Technically, if the matrix is sound, you could also use H2O2, add KI with H2SO4 and titrate with thiosulfate. You'd have to standardize the peroxide
(KI/H2SO4 with molybdate catalyst, or other, with thiosulfate titrant) first.
http://www.h2o2.com/industrial/applications.aspx?pid=109&...
O3
[Edited on 9-2-2016 by Ozone]
[Edited on 9-2-2016 by Ozone]
-Anyone who never made a mistake never tried anything new.
--Albert Einstein
|
|
|
UC235
National Hazard
Posts: 565
Registered: 28-12-2014
Member Is Offline
Mood: No Mood
|
|
The problem with using KMnO4 is that formalin solutions contain a considerable amount of methanol.
|
|
|
Magpie
lab constructor
Posts: 5939
Registered: 1-11-2003
Location: USA
Member Is Offline
Mood: Chemistry: the subtle science.
|
|
I titrated 25mL of my aqueous formaldehyde solution made with anhydrous formaldehyde using the Na2SO3 method. The result was 1% formaldehyde in 125
ml. This is less than I had hoped for but then I only sparged for an hour.
Thanks Dr Bob for suggesting the Na2SO3 method - it's quite easy. I had perused the formaldehyde ACS monograph in the forum library before but wasn't
looking for analytical information at that time.
If you live in a salmon egg curing area you may be able to buy anhydrous Na2SO3, two lbs for $12.50 at Ace.
The single most important condition for a successful synthesis is good mixing - Nicodem
|
|
|
blogfast25
International Hazard
Posts: 10562
Registered: 3-2-2008
Location: Neverland
Member Is Offline
Mood: No Mood
|
|
@Magpie:
Nice to see a plan work out.
But what the hell is Na[H2CSO4]??
|
|
|
clearly_not_atara
International Hazard
Posts: 2786
Registered: 3-11-2013
Member Is Online
Mood: Big
|
|
He means sodium methanolsulfonate, CH2OHSO3Na. He's off by a hydrogen atom.
|
|
|
blogfast25
International Hazard
Posts: 10562
Registered: 3-2-2008
Location: Neverland
Member Is Offline
Mood: No Mood
|
|
Thought so. Thanks!
|
|
|
alexchim
Harmless
Posts: 8
Registered: 23-12-2015
Location: France
Member Is Offline
Mood: No Mood
|
|
Formaldehyde could be titrated by using aqueous solution of iodine in potassium iodide in basic media, iodine disproportionate into iodide (I-) and
hypoiodite (IO-) which oxidize formaldehyde into formiate (HCOO-) ions. Bring the mixture back into acidic media lead to the transformation of I- and
IO- ions into iodine, which could be titrated back with sodium thiosulfate. Redox equations could give the concentration of formaldehyde into a
diluted solution, and by the way give the concentration of the pure solution (if obtained from dilution).
|
|
|
unionised
International Hazard
Posts: 5126
Registered: 1-11-2003
Location: UK
Member Is Offline
Mood: No Mood
|
|
I'm pretty sure that the video is wrong. It should be sodium sulphite.
The mass taken is exactly half a mole of sodium sulphite but some odd looking fraction of a mole of sulphide.
And I have done the analysis of aldehydes by titration of the hydroxide released by reaction of sulphite with aldehyde using thymolphthalein as an
indicator.
I looked at a few titration methods and the sulphite one was the least friendly.
Even with a pH meter the endpoint is indistinct and creeps due to atmospheric CO2.
For formaldehyde the iodine based titration was the best.
For other aldehydes the reaction with hydroxylamine HCl was OK.
For the best precision I'd use gravimetric assay by precipitation of silver from a solution of silver oxide in aqueous tertiary butylamine (which
avoids the possibility of producing explosive silver amine compounds).
|
|
|
meohmix
Harmless
Posts: 6
Registered: 19-12-2017
Member Is Offline
Mood: No Mood
|
|
Having performed a catalytic oxidation of methanol vapor with air over copper, I now have a solution of formaldehyde in methanol and water. I would
like to determine the weight % of formaldehyde I have produced.
Can I assume the presence of methanol would render sulfite, H2SO4 method of titration unusable/inaccurate?
How does such a unknown mixture behave under atmospheric and vacuum distillation?
Ultimately my goal is a 37% solution of formaldehyde in H2O, varying levels of MeOH are perfectly acceptable.
Member's thoughts and advice are appreciated!
|
|
|
unionised
International Hazard
Posts: 5126
Registered: 1-11-2003
Location: UK
Member Is Offline
Mood: No Mood
|
|
| Quote: Originally posted by meohmix |
Can I assume the presence of methanol would render sulfite, H2SO4 method of titration unusable/inaccurate?
|
The methanol won't upset the titration much.
|
|
|
meohmix
Harmless
Posts: 6
Registered: 19-12-2017
Member Is Offline
Mood: No Mood
|
|
Thanks unionised.
I went to the local university library to have a look at the 3rd ed of Walker's Formaldehyde text and made a few scans. See PDF for it's description
of the sulfite method.
(I also scanned the chapter on distillation of formaldehyde solutions. I will post the PDF in another thread)
Again, member's thoughts are appreciated!
Attachment: FormTit.pdf (221kB)
This file has been downloaded 525 times
|
|
|
![[*]](images/xpblue/default_icon.gif){kind=icon}
