Adverts

Open Access Articles- Top Results for Acetoacetic acid

Acetoacetic acid

Acetoacetic acid
200px
200px
colspan=2 style="background:#f8eaba; border-top:2px solid transparent; border-bottom:2px solid transparent; text-align:center;" #REDIRECTmw:Help:Magic words#Other
This page is a soft redirect. Names

#REDIRECTmw:Help:Magic words#Other
This page is a soft redirect.-

IUPAC name
3-oxobutanoic acid, diacetic acid
colspan=2 style="background:#f8eaba; border-top:2px solid transparent; border-bottom:2px solid transparent; text-align:center;" #REDIRECTmw:Help:Magic words#Other
This page is a soft redirect. Identifiers#REDIRECTmw:Help:Magic words#Other
This page is a soft redirect.-



541-50-4 7pxY
ChEBI CHEBI:15344 7pxY
ChEMBL ChEMBL1230762 7pxN
ChemSpider 94 7pxY
DrugBank DB01762 7pxN
Jmol-3D images Image
KEGG C00164 7pxY
PubChem Template:Chembox PubChem/format
colspan=2 style="background:#f8eaba; border-top:2px solid transparent; border-bottom:2px solid transparent; text-align:center;" #REDIRECTmw:Help:Magic words#Other
This page is a soft redirect. Properties

#REDIRECTmw:Help:Magic words#Other
This page is a soft redirect.-

C4H6O3
Molar mass 102.088 g/mol
Appearance colorless, oily liquid
Melting point Script error: No such module "convert".
Boiling point Decomposes
miscible
Solubility soluble in ethanol, ether
Acidity (pKa) 3.58 [1]
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
 14pxN verify (what is10pxY/10pxN?)
Infobox references

Acetoacetic acid (also called diacetic acid) is the organic compound with the formula CH3COCH2COOH. It is the simplest beta-keto acid group and like other members of this class is unstable. The methyl and ethyl esters, which are quite stable, are produced on a large scale industrially as precursors to dyes.[2]

Synthesis and properties

In general, the esters are prepared from diketene by treatment with alcohols.[2] Acetoacetic acid can be prepared by the hydrolysis of the ethyl acetoacetate followed by acidification of the anion.[3] In general, acetoacetic acid is generated at 0 °C and used in situ immediately.[4] It decomposes at a moderate rate to acetone and carbon dioxide:

CH3C(O)CH2CO2H → CH3C(O)CH3 + CO2

The acid form has a half-life of 140 minutes at 37 °C in water, whereas the basic form (the anion) has a half-life of 130 hours. That is, it reacts about 55 times more slowly.[5]

It is a weak acid (like most alkyl carboxylic acids) with a pKa of 3.58.

Applications

Acetoacetic esters are used for the acetoacetylation reaction, which is widely used in the production of arylide yellows and diarylide dyes.[2] Although the esters can be used in this reaction, diketene also reacts with alcohols and amines to the corresponding acetoacetic acid derivatives in a process called acetoacetylation. An example is the reaction with 2-aminoindane:[6]

Diketene reaction Sai 2007
File:YellowPig5thTry.png
Pigment Yellow 16 is a typical dye containing the acetoacetyl group
.

Detection

When ketone bodies are measured by way of urine concentration, acetoacetic acid, along with beta-hydroxybutyric acid (BHB), and acetone, is what is detected. This is done using dipsticks coated in nitroprusside or similar reagents. Nitroprusside changes from pink to purple in the presence of acetoacetate, the conjugate base of acetoacetic acid, and the colour change is graded by eye. The popular dipstick used to detect ketone bodies in urine "Ketostix" by Bayer, only detects acetoacetate, not BHB or acetone.[citation needed]

See also

References

  1. ^ Dawson, R. M. C., et al., Data for Biochemical Research, Oxford, Clarendon Press, 1959.
  2. ^ a b c Franz Dietrich Klingler, Wolfgang Ebertz "Oxocarboxylic Acids" in Ullmann's Encyclopedia of Industrial Chemistry 2005, Wiley-VCH, Weinheim. doi:10.1002/14356007.a18 313
  3. ^ Robert C. Krueger (1952). "Crystalline Acetoacetic Acid". Journal of the American Chemical Society 74 (21): 5536–5536. doi:10.1021/ja01141a521. 
  4. ^ George A. Reynolds and J. A. VanAllan "Methylglyoxal-ω-Phenylhydrazone" Organic Syntheses, Collected Volume 4, p.633 (1963).http://www.orgsyn.org/orgsyn/pdfs/CV4P0633.pdf
  5. ^ Hay, R. W.; Bond, M. A. (1967). "Kinetics of decarboxilation of acetoacetic acid". Aust. J. Chem. 20 (9): 1823–8. doi:10.1071/CH9671823. 
  6. ^ Kiran Kumar Solingapuram Sai, Thomas M. Gilbert, and Douglas A. Klumpp (2007). "Knorr Cyclizations and Distonic Superelectrophiles". J. Org. Chem. 72 (25): 9761–9764. PMID 17999519. doi:10.1021/jo7013092.