Chemistry:Carbonic acid

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Short description: Chemical compound
Carbonic acid
Structural formula
Ball-and-stick model
Names
IUPAC name
Carbonic acid[1]
Other names
  • Oxidocarboxylic acid
  • Hydroxyformic acid
  • Hydroxymethanoic acid
  • Carbonylic acid
  • Hydroxycarboxylic acid
  • Dihydroxycarbonyl
  • Carbon dioxide solution
  • Acid of greenhouse gas[citation needed]
  • Aerial acid
  • Metacarbonic acid
Identifiers
3D model (JSmol)
ChEBI
ChEMBL
ChemSpider
DrugBank
EC Number
  • 610-295-3
25554
KEGG
UNII
Properties
H2CO3
Appearance Colorless gas
Melting point −53 °C (−63 °F; 220 K)[2] (sublimes)
Boiling point 127 °C (261 °F; 400 K) (decomposes)
Reacts to form carbon dioxide and water
Acidity (pKa) pKa1 = 3.6 at 25 °C
pKa2 = 10.329
Conjugate base Bicarbonate, carbonate
Hazards
NFPA 704 (fire diamond)
Flammability code 0: Will not burn. E.g. waterHealth code 0: Exposure under fire conditions would offer no hazard beyond that of ordinary combustible material. E.g. sodium chlorideReactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazards (white): no codeNFPA 704 four-colored diamond
0
0
1
Structure
monoclinic
p21/c, No. 14
-
a = 5.392 Å, b = 6.661 Å, c = 5.690 Å
α = 90°, β = 92.66°, γ = 90°[3]
(D2CO3 at 1.85 GPa, 298 K)
204.12 Å3
4 formula per cell
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
☑Y verify (what is ☑Y☒N ?)
Infobox references

Carbonic acid is a chemical compound with the chemical formula H
2CO
3. The molecule rapidly converts to water and carbon dioxide in the presence of water. However, in the absence of water, it is (contrary to popular belief) quite stable at room temperature.[4][5] The interconversion of carbon dioxide and carbonic acid is related to the breathing cycle of animals and the acidification of natural waters.[3]

In biochemistry and physiology, the name "carbonic acid" is sometimes applied to aqueous solutions of carbon dioxide. These chemical species play an important role in the bicarbonate buffer system, used to maintain acid–base homeostasis.[6]

Terminology in biochemical literature

In chemistry, the term "carbonic acid" strictly refers to the chemical compound with the formula H2CO3. Some biochemistry literature effaces the distinction between carbonic acid and carbon dioxide dissolved in extracellular fluid.

In physiology, carbon dioxide excreted by the lungs may be called volatile acid or respiratory acid.

Anhydrous carbonic acid

At ambient temperatures, pure carbonic acid is a stable gas.[5] There are two main methods to produce anhydrous carbonic acid: reaction of hydrogen chloride and potassium bicarbonate at 100 K in methanol and proton irradiation of pure solid carbon dioxide.[2] Chemically, it behaves as a diprotic Brønsted acid.[7][8]

Carbonic acid monomers exhibit three conformational isomers: cis–cis, cis–trans, and trans–trans.[9]

At low temperatures and atmospheric pressure, solid carbonic acid is amorphous and lacks Bragg peaks in X-ray diffraction.[10] But at high pressure, carbonic acid crystallizes, and modern analytical spectroscopy can measure its geometry.

According to neutron diffraction of dideuterated carbonic acid (D2CO3) in a hybrid clamped cell (Russian alloy/copper-beryllium) at 1.85 GPa, the molecules are planar and form dimers joined by pairs of hydrogen bonds. All three C-O bonds are nearly equidistant at 1.34 Å, intermediate between typical C-O and C=O distances (respectively 1.43 and 1.23 Å). The unusual C-O bond lengths are attributed to delocalized π bonding in the molecule's center and extraordinarily strong hydrogen bonds. The same effects also induce a very short O—O separation (2.13 Å), through the 136° O-H-O angle imposed by the doubly hydrogen-bonded 8-membered rings.[3] Longer O—O distances are observed in strong intramolecular hydrogen bonds, e.g. in oxalic acid, where the distances exceed 2.4 Å.[10]

In aqueous solution

In even a slight presence of water, carbonic acid dehydrates to carbon dioxide and water, which then catalyzes further decomposition.[5] For this reason, carbon dioxide can be considered the carbonic acid anhydride.

The hydration equilibrium constant at 25 °C is [H2CO3]/[CO
2] ≈ 1.7×10−3 in pure water[11] and ≈ 1.2×10−3 in seawater.[12] Hence the majority of carbon dioxide at geophysical or biological air-water interfaces does not convert to carbonic acid, remaining dissolved CO
2 gas. However, the uncatalyzed equilibrium is reached quite slowly: the rate constants are 0.039 s−1 for hydration and 23 s−1 for dehydration.

In biological solutions

In the presence of the enzyme carbonic anhydrase, equilibrium is instead reached rapidly, and the following reaction takes precedence:[13] [math]\ce{ HCO3^- {+} H^+ <=> CO2 {+} H2O }[/math]

When the created carbon dioxide exceeds its solubility, gas evolves and a third equilibrium [math]\ce{ CO_2 (soln) <=> CO_2 (g) }[/math] must also be taken into consideration. The equilibrium constant for this reaction is defined by Henry's law.

The two reactions can be combined for the equilibrium in solution: [math]\displaystyle{ \begin{align} \ce{HCO3^{-}{} + H+{} \lt =\gt CO2(soln){} + H2O} && K_3 = \frac{[\ce{H+}][\ce{HCO3^-}]}{[\ce{CO2(soln)}]} \end{align} }[/math] When Henry's law is used to calculate the denominator care is needed with regard to units since Henry's Law constant can be commonly expressed with 8 different dimensionalities.[14]

Under high CO2 partial pressure

In the beverage industry, sparkling or "fizzy water" is usually referred to as carbonated water. It is made by dissolving carbon dioxide under a small positive pressure in water. Many soft drinks treated the same way effervesce.

Significant amounts of molecular H2CO3 exist in aqueous solutions subjected to pressures of multiple gigapascals (tens of thousands of atmospheres) in planetary interiors.[15][16] Pressures of 0.6–1.6 GPa at 100 K, and 0.75–1.75 GPa at 300 K are attained in the cores of large icy satellites such as Ganymede, Callisto, and Titan, where water and carbon dioxide are present. Pure carbonic acid, being denser, is expected to have sunk under the ice layers and separate them from the rocky cores of these moons.[17]

Relationship to bicarbonate and carbonate

Bjerrum plot of speciation for a hypothetical monoprotic acid: AH concentration as a function of the difference between pK and pH

Carbonic acid is the formal Brønsted–Lowry conjugate acid of the bicarbonate anion, stable in alkaline solution. The protonation constants have been measured to great precision, but depend on overall ionic strength I. The two equilibria most easily measured are as follows: [math]\displaystyle{ \begin{align} \ce{CO3^{2-}{} + H+{} \lt =\gt HCO3^-} && \beta_1 = \frac{[\ce{HCO3^-}]}{[\ce{H+}][\ce{CO3^{2-}}]} \\ \ce{CO3^{2-}{} + 2H+{} \lt =\gt H2CO3} && \beta_2 = \frac{[\ce{H2CO3}]}{[\ce{H+}]^2[\ce{CO3^{2-}}]} \end{align} }[/math] where brackets indicate the concentration of specie. At 25 °C, these equilibria empirically satisfy[18][math]\displaystyle{ \begin{alignat}{6} \log(\beta_1) =&& 0&.54&I^2 - 0&.96&I +&& 9&.93 \\ \log(\beta_2) =&& -2&.5&I^2 - 0&.043&I +&& 16&.07 \end{alignat} }[/math]Note that log(β1) decreases with increasing I, as does log(β2). In a solution absent other ions (e.g. I = 0), these curves imply the following stepwise dissociation constants:[math]\displaystyle{ \begin{alignat}{3} p\text{K}_1 &= \log(\beta_2) - \log(\beta_1) &= 6.77 \\ p\text{K}_2 &= \log(\beta_1) &= 9.93 \end{alignat} }[/math] Direct values for these constants in the literature include pK1 = 6.35 and pK2 - pK1 = 3.49.[19]

To interpret these numbers, note that two chemical species in an acid equilibrium are equiconcentrated when pK = pH. In particular, the extracellular fluid (cytosol) in biological systems exhibits pH ≈ 7.2, so that carbonic acid will be almost 50%-dissociated at equilibrium.

Ocean acidification

Carbonate speciation in seawater (ionic strength 0.7 mol/dm3). The expected change shown is due to the current anthropogenic increase in atmospheric carbon dioxide concentration.

The Bjerrum plot shows typical equilibrium concentrations, in solution, in seawater, of carbon dioxide and the various species derived from it, as a function of pH.[7][8] As human industrialization has increased the proportion of carbon dioxide in Earth's atmosphere, the proportion of carbon dioxide dissolved in sea- and freshwater as carbonic acid is also expected to increase. This rise in dissolved acid is also expected to acidify those waters, generating a decrease in pH.[20][21] It has been estimated that the increase in dissolved carbon dioxide has already caused the ocean's average surface pH to decrease by about 0.1 from pre-industrial levels.

Further reading

References

  1. ↑ "Front Matter". Nomenclature of Organic Chemistry: IUPAC Recommendations and Preferred Names 2013 (Blue Book). Cambridge: The Royal Society of Chemistry. 2014. pp. P001–4. doi:10.1039/9781849733069-FP001. ISBN 978-0-85404-182-4. 
  2. ↑ 2.0 2.1 W. Hage, K. R. Liedl; Liedl, E.; Hallbrucker, A; Mayer, E (1998). "Carbonic Acid in the Gas Phase and Its Astrophysical Relevance". Science 279 (5355): 1332–5. doi:10.1126/science.279.5355.1332. PMID 9478889. Bibcode: 1998Sci...279.1332H. 
  3. ↑ 3.0 3.1 3.2 Benz, Sebastian; Chen, Da; Möller, Andreas; Hofmann, Michael; Schnieders, David; Dronskowski, Richard (September 2022). "The Crystal Structure of Carbonic Acid" (in en). Inorganics 10 (9): 132. doi:10.3390/inorganics10090132. ISSN 2304-6740. 
  4. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 310. ISBN 978-0-08-037941-8. 
  5. ↑ 5.0 5.1 5.2 Loerting, Thomas; Tautermann, Christofer; Kroemer, Romano T.; Kohl, Ingrid; Hallbrucker, Andreas; Mayer, Erwin; Liedl, Klaus R.; Loerting, Thomas et al. (2000). "On the Surprising Kinetic Stability of Carbonic Acid (H2CO3)". Angewandte Chemie International Edition 39 (5): 891–4. doi:10.1002/(SICI)1521-3773(20000303)39:5<891::AID-ANIE891>3.0.CO;2-E. PMID 10760883. 
  6. ↑ Acid-Base Physiology 2.1 – Acid-Base Balance by Kerry Brandis.
  7. ↑ 7.0 7.1 Pangotra, Dhananjai; Csepei, Lénárd-István; Roth, Arne; Ponce de León, Carlos; Sieber, Volker; Vieira, Luciana (2022). "Anodic production of hydrogen peroxide using commercial carbon materials". Applied Catalysis B: Environmental 303: 120848. doi:10.1016/j.apcatb.2021.120848. 
  8. ↑ 8.0 8.1 Andersen, C. B. (2002). "Understanding carbonate equilibria by measuring alkalinity in experimental and natural systems". Journal of Geoscience Education 50 (4): 389–403. doi:10.5408/1089-9995-50.4.389. Bibcode: 2002JGeEd..50..389A. 
  9. ↑ Loerting, Thomas; Bernard, Juergen (2010). "Aqueous Carbonic Acid (H2CO3)". ChemPhysChem (11): 2305–9. doi:10.1002/cphc.201000220. 
  10. ↑ 10.0 10.1 Winkel, Katrin; Hage, Wolfgang; Loerting, Thomas; Price, Sarah L.; Mayer, Erwin (2007). "Carbonic Acid: From Polyamorphism to Polymorphism". Journal of the American Chemical Society 129 (45): 13863–71. doi:10.1021/ja073594f. PMID 17944463. 
  11. ↑ Housecroft, C.E.; Sharpe, A.G. (2005). Inorganic Chemistry (2nd ed.). Prentice-Pearson-Hall. p. 368. ISBN 0-13-039913-2. OCLC 56834315. 
  12. ↑ Soli, A. L.; R. H. Byrne (2002). "CO2 system hydration and dehydration kinetics and the equilibrium CO2/H2CO3 ratio in aqueous NaCl solution". Marine Chemistry 78 (2–3): 65–73. doi:10.1016/S0304-4203(02)00010-5. 
  13. ↑ "Structure and mechanism of carbonic anhydrase". Pharmacology & Therapeutics 74 (1): 1–20. 1997. doi:10.1016/S0163-7258(96)00198-2. PMID 9336012. 
  14. ↑ Sander, Rolf; Acree, William E.; Visscher, Alex De; Schwartz, Stephen E.; Wallington, Timothy J. (2022-01-01). "Henry’s law constants (IUPAC Recommendations 2021)" (in en). Pure and Applied Chemistry 94 (1): 71–85. doi:10.1515/pac-2020-0302. ISSN 1365-3075. https://www.degruyter.com/document/doi/10.1515/pac-2020-0302/html. 
  15. ↑ Wang, Hongbo; Zeuschner, Janek; Eremets, Mikhail; Troyan, Ivan; Williams, Jonathon (27 January 2016). "Stable solid and aqueous H2CO3 from CO2 and H2O at high pressure and high temperature". Scientific Reports 6 (1): 19902. doi:10.1038/srep19902. PMID 26813580. Bibcode: 2016NatSR...619902W. 
  16. ↑ Stolte, Nore; Pan, Ding (4 July 2019). "Large presence of carbonic acid in CO2-rich aqueous fluids under Earth's mantle conditions". The Journal of Physical Chemistry Letters 10 (17): 5135–41. doi:10.1021/acs.jpclett.9b01919. PMID 31411889. 
  17. ↑ G. Saleh; A. R. Oganov (2016). "Novel Stable Compounds in the C-H-O Ternary System at High Pressure". Scientific Reports 6: 32486. doi:10.1038/srep32486. PMID 27580525. Bibcode: 2016NatSR...632486S. 
  18. ↑ IUPAC (2006). "Stability constants" (database).
  19. ↑ Pines, Dina; Ditkovich, Julia; Mukra, Tzach; Miller, Yifat; Kiefer, Philip M.; Daschakraborty, Snehasis; Hynes, James T.; Pines, Ehud (2016). "How Acidic Is Carbonic Acid?". J Phys Chem B 120 (9): 2440–51. doi:10.1021/acs.jpcb.5b12428. PMID 26862781. 
  20. ↑ Caldeira, K.; Wickett, M. E. (2003). "Anthropogenic carbon and ocean pH". Nature 425 (6956): 365. doi:10.1038/425365a. PMID 14508477. Bibcode: 2001AGUFMOS11C0385C. https://zenodo.org/record/1233227. 
  21. ↑ Sabine, C. L. (2004). "The Oceanic Sink for Anthropogenic CO2". Science 305 (5682): 367–371. doi:10.1126/science.1097403. PMID 15256665. Bibcode: 2004Sci...305..367S. https://www.science.org/doi/abs/10.1126/science.1097403. Retrieved 22 June 2021. 

External links

Carbonates
H2CO3 He
Li2CO3,
LiHCO3 		BeCO3 B C (NH4)2CO3,
NH4HCO3 		O F Ne
Na2CO3,
NaHCO3,
Na3H(CO3)2 		MgCO3,
Mg(HCO3)2 		Al2(CO3)3 Si P S Cl Ar
K2CO3,
KHCO3 		CaCO3,
Ca(HCO3)2 		Sc Ti V Cr MnCO3 FeCO3 CoCO3 NiCO3 CuCO3 ZnCO3 Ga Ge As Se Br Kr
Rb2CO3 SrCO3 Y Zr Nb Mo Tc Ru Rh Pd Ag2CO3 CdCO3 In Sn Sb Te I Xe
Cs2CO3,
CsHCO3 		BaCO3   Hf Ta W Re Os Ir Pt Au Hg Tl2CO3 PbCO3 (BiO)2CO3 Po At Rn
Fr Ra   Rf Db Sg Bh Hs Mt Ds Rg Cn Nh Fl Mc Lv Ts Og
↓
La2(CO3)3 Ce2(CO3)3 Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu
Ac Th Pa UO2CO3 Np Pu Am Cm Bk Cf Es Fm Md No Lr



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