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===Buffer details===
===Buffer details===
*The p''K''<sub>a</sub> declines approximately 0.03 units per degree Celsius rise in temperature.<ref name="El-Harakany">{{cite journal|last=El-Harakany| first=A.A.|author2=Abdel Halima|author3=F.M.|author4=Barakat, A.O.|title=Dissociation constants and related thermodynamic quantities of the protonated acid form of tris-(hydroxymethyl)-aminomethane in mixtures of 2-methoxyethanol and water at different temperatures|journal=J. Electroanal. Chem.|volume=162|issue=1–2|pages=285–305|year=1984|doi=10.1016/S0022-0728(84)80171-0}}</ref><ref name="Vega">{{cite journal|last=Vega| first=C.A.|author2=Butler, R.A.|title=Thermodynamics of the Dissociation of Protonated Tris(hydroxymethy1)aminomethane in 25 and 50 wt % 2-Propanol from 5 to 45 °C|journal= J. Chem. Eng. Data|volume=30|pages=376–379|year=1985|doi=10.1021/je00042a003|issue=4|display-authors=etal}}</ref>
*The p''K''<sub>a</sub> declines approximately 0.03 units per degree Celsius rise in temperature.<ref name="El-Harakany">{{cite journal|last=El-Harakany| first=A.A.|author2=Abdel Halima|author3=F.M.|author4=Barakat, A.O.|title=Dissociation constants and related thermodynamic quantities of the protonated acid form of tris-(hydroxymethyl)-aminomethane in mixtures of 2-methoxyethanol and water at different temperatures|journal=J. Electroanal. Chem.|volume=162|issue=1–2|pages=285–305|year=1984|doi=10.1016/S0022-0728(84)80171-0}}</ref><ref name="Vega">{{cite journal|last=Vega| first=C.A.|author2=Butler, R.A.|title=Thermodynamics of the Dissociation of Protonated Tris(hydroxymethy1)aminomethane in 25 and 50 wt % 2-Propanol from 5 to 45 °C|journal= J. Chem. Eng. Data|volume=30|pages=376–379|year=1985|doi=10.1021/je00042a003|issue=4|display-authors=etal}}</ref>
*[[Silver]]-containing single-junction pH electrodes (e.g., [[silver chloride electrode]]) are incompatible with Tris (Ag-tris precipitation clogs the junction). Double-junction electrodes are resistant to this problem, and non-silver containing electrodes are immune.
*[[Silver]]-containing single-junction pH electrodes (e.g., [[silverchanges in [[ionic strength]].
*Making buffer solutions by neutralizing TrisHCl requires attention to the attendant changes in [[ionic strength]].


===Buffer inhibition===
===Buffer inhibition===

Revision as of 19:56, 19 July 2017

This article is about the chemical widely used as a biochemical buffer. For other uses, see Tris (disambiguation).
Tris
Chemical structure of tris
Names
Preferred IUPAC name
2-Amino-2-(hydroxymethyl)propane-1,3-diol
Other names
TRIS, Tris, Tris base, Tris buffer, Trizma, Trisamine, THAM, Tromethamine, Trometamol, Tromethane, Trisaminol
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
ECHA InfoCard 100.000.969 Edit this at Wikidata
KEGG
RTECS number
  • TY2900000
UNII
  • InChI=1S/C4H11NO3/c5-4(1-6,2-7)3-8/h6-8H,1-3,5H2 checkY
    Key: LENZDBCJOHFCAS-UHFFFAOYSA-N checkY
  • InChI=1/C4H11NO3/c5-4(1-6,2-7)3-8/h6-8H,1-3,5H2
    Key: LENZDBCJOHFCAS-UHFFFAOYAN
  • OCC(N)(CO)CO
Properties
C4H11NO3
Molar mass 121.136 g·mol−1
Appearance White crystalline powder
Density 1.328g/cm3
Melting point >175-176 °C (448-449 K)
Boiling point 219 °C (426 °F; 492 K)
~50 g/100 mL (25 °C)
Acidity (pKa) 8.07
Pharmacology
B05BB03 (WHO) B05XX02 (WHO)
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
 Irritant
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability (red): no hazard codeInstability (yellow): no hazard codeSpecial hazards (white): no code
2
Flash point Non-flammable
Safety data sheet (SDS) External MSDS
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☒N verify (what is checkY☒N ?)

Tris, or tris(hydroxymethyl)aminomethane, or THAM, is an organic compound with the formula (HOCH2)3CNH2. It is extensively used in biochemistry and molecular biology.[1] In biochemistry, Tris is widely used as a component of buffer solutions, such as in TAE and TBE buffer, especially for solutions of nucleic acids. It contains a primary amine and thus undergoes the reactions associated with typical amines, e.g. condensations with aldehydes.

Buffering features

Tris has a pKa of 8.07 at 25 °C, which implies that the buffer has an effective pH range between 7.5 and 9.0.

Buffer details

  • The pKa declines approximately 0.03 units per degree Celsius rise in temperature.[2][3]
  • Silver-containing single-junction pH electrodes (e.g., [[silverchanges in ionic strength.

Buffer inhibition

  • Tris inhibits a number of enzymes,[4][5] and therefore it should be used with care when studying proteins.

Preparation

Tris is prepared industrially by the exhaustive condensation of nitromethane with formaldehyde under basic conditions (i.e. repeated nitroaldol reactions) to produce the intermediate (HOCH2)3CNO2, which is subsequently hydrogenated to give the final product.[6]

Uses

The useful buffer range for tris (7-9) coincides with the physiological pH typical of most living organisms. This, and its low cost, make tris one of the most common buffers in the biology/biochemistry laboratory. Tris is also used as a primary standard to standardize acid solutions for chemical analysis.

Tris is used to increase membrane permeability of cell membranes.[7]

Medical

Tris (usually known as THAM in this context) is used as alternative to sodium bicarbonate in the treatment of metabolic acidosis.[8][9]

See also

References

  1. ^ Gomori, G., Preparation of Buffers for Use in Enzyme Studies. Methods Enzymology., 1, 138-146 (1955).
  2. ^ El-Harakany, A.A.; Abdel Halima; F.M.; Barakat, A.O. (1984). "Dissociation constants and related thermodynamic quantities of the protonated acid form of tris-(hydroxymethyl)-aminomethane in mixtures of 2-methoxyethanol and water at different temperatures". J. Electroanal. Chem. 162 (1–2): 285–305. doi:10.1016/S0022-0728(84)80171-0.
  3. ^ Vega, C.A.; Butler, R.A.; et al. (1985). "Thermodynamics of the Dissociation of Protonated Tris(hydroxymethy1)aminomethane in 25 and 50 wt % 2-Propanol from 5 to 45 °C". J. Chem. Eng. Data. 30 (4): 376–379. doi:10.1021/je00042a003.
  4. ^ Desmarais, WT; et al. (2002). "The 1.20 Å resolution crystal structure of the aminopeptidase from Aeromonas proteolytica complexed with Tris: A tale of buffer inhibition". Structure. 10 (8): 1063–1072. doi:10.1016/S0969-2126(02)00810-9. PMID 12176384.
  5. ^ Ghalanbor, Z; et al. (2008). "Binding of Tris to Bacillus licheniformis alpha-amylase can affect its starch hydrolysis activity". Protein Peptide Lett. 15 (2): 212–214. doi:10.2174/092986608783489616. PMID 18289113.
  6. ^ Markofsky, Sheldon, B. (15 October 2011). "Nitro Compounds, Aliphatic". Ullmann's Encyclopedia of Industrial Chemistry. 24: 296. doi:10.1002/14356007.a17_401.pub2.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  7. ^ Irvin, R.T.; MacAlister, T.J.; Costerton, J.W. (1981). "Tris(hydroxymethyl)aminomethane Buffer Modification of Escherichia coli Outer Membrane Permeability". J. Bacteriol. 145 (3): 1397–1403.
  8. ^ Kallet, RH; Jasmer RM; Luce JM; et al. (2000). "The treatment of acidosis in acute lung injury with tris-hydroxymethyl aminomethane (THAM)". American Journal of Respiratory and Critical Care Medicine. 161 (4): 1149–1153. doi:10.1164/ajrccm.161.4.9906031. PMID 10764304.
  9. ^ Hoste, EA; Colpaert, K; Vanholder, RC; Lameire, NH; De Waele, JJ; Blot, SI; Colardyn, FA (2005). "Sodium bicarbonate versus THAM in ICU patients with mild metabolic acidosis". Journal of nephrology. 18 (3): 303–7. PMID 16013019.
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