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| :''Not to be confused with [[carbolic acid]], an antiquated name for [[phenol]].''
| | Database Administrator Marlon from Alert Bay, really likes models, health and fitness and sleeping. In the recent few months has paid a try to spots like Central Sikhote-Alin.<br><br>Here is my blog post: [http://www.kolna-twensa.com/blog/4455/are-you-presently-not-getting-appropriate-nutrition-try-out-these-tips/add-comment/ Best Weight Gainer Steroids] |
| :''Carbonic acid is also an archaic name for [[carbon dioxide]].''
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| {{chembox
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| | Watchedfields = changed
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| | verifiedrevid = 477313558
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| | ImageFileL1_Ref = {{chemboximage|correct|??}}
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| | ImageFileL1 = Carbonic-acid-2D.svg
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| | ImageSizeL1 = 100px
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| | ImageNameL1 = Structural formula
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| | ImageFileR1 = Carbonic-acid-3D-balls.png
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| | ImageSizeR1 = 120px
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| | ImageNameR1 = Ball-and-stick model
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| | IUPACName = Carbonic acid
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| | OtherNames = Carbon dioxide solution; Dihydrogen carbonate; acid of air; Aerial acid; Hydroxymethanoic acid
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| | Section1 = {{Chembox Identifiers
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| | KEGG_Ref = {{keggcite|correct|kegg}}
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| | KEGG = C01353
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| | InChI = 1/CH2O3/c2-1(3)4/h(H2,2,3,4)
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| | InChIKey = BVKZGUZCCUSVTD-UHFFFAOYAU
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| | ChEMBL_Ref = {{ebicite|correct|EBI}}
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| | ChEMBL = 1161632
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| | StdInChI_Ref = {{stdinchicite|correct|chemspider}}
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| | StdInChI = 1S/CH2O3/c2-1(3)4/h(H2,2,3,4)
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| | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
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| | StdInChIKey = BVKZGUZCCUSVTD-UHFFFAOYSA-N
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| | CASNo = 463-79-6
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| | CASNo_Ref = {{cascite|correct|CAS}}
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| | PubChem =
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| | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
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| | ChemSpiderID = 747
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| | ChEBI_Ref = {{ebicite|correct|EBI}}
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| | ChEBI = 28976
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| | SMILES = O=C(O)O
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| }}
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| | Section2 = {{Chembox Properties
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| | Formula = H<sub>2</sub>CO<sub>3</sub>
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| | MolarMass = 62.03 g/mol
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| | Appearance =
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| | Density = 1.668 g/cm<sup>3</sup>
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| | Solubility = Exists only in solution
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| | pKa = 6.367 (p''K''<sub>a1</sub>), 10.32 (p''K''<sub>a2</sub>)
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| | MeltingPt =
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| | BoilingPt =
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| }}
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| }}
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| | |
| '''Carbonic acid''' is the [[chemical compound]] with the [[Molecular formula|formula]] H<sub>2</sub>CO<sub>3</sub> (equivalently OC(OH)<sub>2</sub>). It is also a name sometimes given to [[solution]]s of [[carbon dioxide]] in [[water (molecule)|water]] ([[carbonated water]]), because such solutions contain small amounts of H<sub>2</sub>CO<sub>3</sub>. Carbonic acid, which is a [[weak acid]], forms two kinds of [[Salt (chemistry)|salts]], the [[carbonate]]s and the [[bicarbonate]]s. In geology, Carbonic acid causes limestone to dissolve producing calcium bicarbonate which leads to many limestone features such as [[stalactites]] and [[stalagmites]] .
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| ==Chemical equilibrium==
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| When carbon dioxide dissolves in water it exists in [[chemical equilibrium]] producing carbonic acid:<ref name=Green/>
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| :CO<sub>2</sub> + H<sub>2</sub>O {{eqm}} H<sub>2</sub>CO<sub>3</sub>
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| The [[Hydrate|hydration]] [[equilibrium constant]] at 25°C is called K<sub>h</sub>, which in the case of carbonic acid is [H<sub>2</sub>CO<sub>3</sub>]/[CO<sub>2</sub>] ≈ 1.7×10<sup>−3</sup> in pure water<ref name="HS">Housecroft and Sharpe, ''Inorganic Chemistry'', 2nd ed, Prentice-Pearson-Hall 2005, p.368.</ref> and ≈ 1.2×10<sup>−3</sup> in [[seawater]].<ref name=SB>{{Cite journal |last=Soli|first=A.L.|coauthors=R.H. Byrne |year=2002 |title=CO2 system hydration and dehydration kinetics and the equilibrium CO2/H2CO3 ratio in aqueous NaCl solution |url= |archiveurl= |archivedate= | journal=Marine chemistry |volume=78 |issue= 2–3|pages=65–73 |doi= 10.1016/S0304-4203(02)00010-5|pmid= |bibcode=}}</ref> Hence, the majority of the carbon dioxide is not converted into carbonic acid, remaining as CO<sub>2</sub> molecules. In the absence of a [[catalyst]], the equilibrium is reached quite slowly. The [[rate constant]]s are 0.039 s<sup>−1</sup> for the forward reaction (CO<sub>2</sub> + H<sub>2</sub>O → H<sub>2</sub>CO<sub>3</sub>) and 23 s<sup>−1</sup> for the reverse reaction (H<sub>2</sub>CO<sub>3</sub> → CO<sub>2</sub> + H<sub>2</sub>O). Carbonic acid is used in the making of [[soft drinks]], inexpensive and artificially carbonated sparkling wines, and other bubbly drinks. The addition of two equivalents of water to CO<sub>2</sub> would give ''[[orthocarbonic acid]]'', C(OH)<sub>4</sub>, which exists only in minute amounts in aqueous solution.
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| Addition of base to an excess of carbonic acid gives [[bicarbonate]]. With excess base, carbonic acid reacts to give [[carbonate]] salts.
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| == Role of carbonic acid in blood ==
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| Carbonic acid is an intermediate step in the transport of CO<sub>2</sub> out of the body via [[Gas exchange|respiratory gas exchange]]. The hydration reaction of CO<sub>2</sub> is generally very slow in the absence of a catalyst, but [[red blood cells]] contain [[carbonic anhydrase]], which both increases the reaction rate and dissociates a hydrogen ion (H<sup>+</sup>) from the resulting carbonic acid, leaving [[bicarbonate]] (HCO<sub>3</sub><sup>−</sup>) dissolved in the [[blood plasma]]. This catalysed reaction is reversed in the lungs, where it converts the bicarbonate back into CO<sub>2</sub> and allows it to be expelled. This equilibration plays an important role as a [[Buffer solution|buffer]] in mammalian blood.<ref>"excretion." Encyclopædia Britannica. Encyclopædia Britannica Ultimate Reference Suite. Chicago: Encyclopædia Britannica, 2010.</ref>
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| == {{anchor|Ocean}} Role of carbonic acid in ocean chemistry==
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| The oceans of the world have absorbed almost half of the CO<sub>2</sub> emitted by humans from the burning of fossil fuels.<ref name=sabine>{{cite journal|last=Sabine|first=C.L.|coauthors=et al.|year=2004|title=The Oceanic Sink for Anthropogenic CO<sub>2</sub>|url=http://www.sciencemag.org/cgi/content/short/305/5682/367"|journal=Science|volume=305|issue=5682|pages=367–371|doi=10.1126/science.1097403|pmid=15256665|format=}} {{dead link|date=May 2010}}</ref> The extra dissolved carbon dioxide has caused the ocean's average surface pH to shift by about 0.1 unit from pre-industrial levels.<ref name=unesco>{{cite web| title=Ocean Acidification Network|url=http://ioc3.unesco.org/oanet/FAQacidity.html}}</ref> This process is known as [[ocean acidification]].<ref>National Research Council. "Summary." Ocean Acidification: A National Strategy to Meet the Challenges of a Changing Ocean. Washington, DC: The National Academies Press, 2010. 1. Print.</ref>
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| ==Acidity of carbonic acid==
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| Carbonic acid is one of the [[Acid#Polyprotic acids|polyprotic acid]]s: It is [[diprotic acid|diprotic]] - it has two protons, which may dissociate from the parent molecule. Thus, there are two [[Acid dissociation constant|dissociation constants]], the first one for the dissociation into the [[bicarbonate]] (also called hydrogen carbonate) ion HCO<sub>3</sub><sup>−</sup>:
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| :H<sub>2</sub>CO<sub>3</sub> {{eqm}} HCO<sub>3</sub><sup>−</sup> + H<sup>+</sup>
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| :''K''<sub>a1</sub> = 2.5×10<sup>−4</sup> mol/litre; p''K''<sub>a1</sub> = 3.6 at 25 °C.<ref name=Green>{{Greenwood&Earnshaw2nd}}</ref>
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| Care must be taken when quoting and using the first dissociation constant of carbonic acid. In aqueous solution, carbonic acid exists in equilibrium with carbon dioxide, and the concentration of H<sub>2</sub>CO<sub>3</sub> is much lower than the concentration of CO<sub>2</sub>. In many analyses, H<sub>2</sub>CO<sub>3</sub> includes dissolved CO<sub>2</sub> (referred to as CO<sub>2</sub>(aq)), H<sub>2</sub>CO<sub>3</sub>* is used to represent the two species when writing the aqueous chemical equilibrium equation. The equation may be rewritten as follows:<ref name=Green/>
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| :H<sub>2</sub>CO<sub>3</sub>* {{eqm}} HCO<sub>3</sub><sup>−</sup> + H<sup>+</sup>
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| :''K''<sub>a</sub>(app) = 4.6×10<sup>−7</sup> mol/litre ; p''K''(app) = 6.3 at 25 °C and Ionic Strength = 0.0
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| Whereas this apparent p''K''<sub>a</sub> is quoted as the dissociation constant of carbonic acid, it is ambiguous: it might better be referred to as the acidity constant of dissolved carbon dioxide, as it is particularly useful for calculating the [[pH]] of CO<sub>2</sub>-containing solutions. A similar situation applies to [[sulfurous acid]] (H<sub>2</sub>SO<sub>3</sub>), which exists in equilibrium with substantial amounts of unhydrated [[sulfur dioxide]].
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| The second constant is for the dissociation of the [[bicarbonate]] ion into the [[carbonate]] ion CO<sub>3</sub><sup>2−</sup>:
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| :HCO<sub>3</sub><sup>−</sup> {{eqm}} CO<sub>3</sub><sup>2−</sup> + H<sup>+</sup>
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| :''K''<sub>a2</sub> = 4.69×10<sup>−11</sup> mol/litre ; p''K''<sub>a2</sub> = 10.329 at 25 °C and Ionic Strength = 0.0
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| ===pH and composition of carbonic acid solutions===
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| At a given temperature, the composition of a pure carbonic acid solution (or of a pure CO<sub>2</sub> solution) is completely determined by the [[partial pressure]] <math>\scriptstyle p_{CO_2}</math> of carbon dioxide above the solution. To calculate this composition, account must be taken of the above equilibria between the three different carbonate forms (H<sub>2</sub>CO<sub>3</sub>, HCO<sub>3</sub><sup>−</sup> and CO<sub>3</sub><sup>2−</sup>) as well as of the hydration equilibrium between dissolved CO<sub>2</sub> and H<sub>2</sub>CO<sub>3</sub> with constant <math>\scriptstyle K_h=\frac{[H_2CO_3]}{[CO_2]}</math> (see above) and of the following equilibrium between the dissolved CO<sub>2</sub> and the gaseous CO<sub>2</sub> above the solution:
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| :CO<sub>2</sub>(gas) {{eqm}} CO<sub>2</sub>(dissolved) with <math>\scriptstyle \frac{[CO_2]}{p_{CO_2}}=\frac{1}{k_\mathrm{H}}</math> where k<sub>H</sub>=29.76 atm/(mol/L) at 25 °C ([[Henry's law|Henry constant]])
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| The corresponding equilibrium equations together with the <math>\scriptstyle[H^+][OH^-]=10^{-14}</math> relation and the charge neutrality condition <math>\scriptstyle[H^+]=[OH^-]+[HCO_3^-]+2[CO_3^{2-}]</math> result in six equations for the six unknowns [CO<sub>2</sub>], [H<sub>2</sub>CO<sub>3</sub>], [H<sup>+</sup>], [OH<sup>−</sup>], [HCO<sub>3</sub><sup>−</sup>] and [CO<sub>3</sub><sup>2−</sup>], showing that the composition of the solution is fully determined by <math>\scriptstyle p_{CO_2}</math>. The equation obtained for [H<sup>+</sup>] is a cubic whose numerical solution yields the following values for the pH and the different species concentrations:
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| {|align="center" border="1" cellspacing="0" cellpadding="2" class="wikitable" style="background:#FFF;color:#000;text-align:center"
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| |-
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| !style="width:9em" scope="col"| <math>\scriptstyle p_{CO_2}</math><br /><small>(atm)</small>
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| !style="width: 5em" scope="col"| pH
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| !style="width:9em" scope="col"| [CO<sub>2</sub>]<br /><small>(mol/L)</small>
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| !style="width:9em" scope="col"| [H<sub>2</sub>CO<sub>3</sub>]<br /><small>(mol/L)</small>
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| !style="width:9em" scope="col"| [HCO<sub>3</sub><sup>−</sup>]<br /><small>(mol/L)</small>
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| !style="width:9em" scope="col"| [CO<sub>3</sub><sup>2−</sup>]<br /><small>(mol/L)</small>
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| |-
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| |scope="row"| {{0|1.0 ×}} 10<sup>−8</sup>
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| | 7.00
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| |style="color:#666"| 3.36 × 10<sup>−10</sup>
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| |style="color:#BBB"| 5.71 × 10<sup>−13</sup>
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| |style="color:#000"| 1.42 × 10<sup>−{{0}}9</sup>
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| |style="color:#666"| 7.90 × 10<sup>−13</sup>
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| |-
| |
| |scope="row"| {{0|1.0 ×}} 10<sup>−7</sup>
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| | 6.94
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| |style="color:#666"| 3.36 × 10<sup>−{{0}}9</sup>
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| |style="color:#666"| 5.71 × 10<sup>−12</sup>
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| |style="color:#000"| 5.90 × 10<sup>−{{0}}9</sup>
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| |style="color:#BBB"| 1.90 × 10<sup>−12</sup>
| |
| |-
| |
| |scope="row"| {{0|1.0 ×}} 10<sup>−6</sup>
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| | 6.81
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| |style="color:#666"| 3.36 × 10<sup>−{{0}}8</sup>
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| |style="color:#666"| 5.71 × 10<sup>−11</sup>
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| |style="color:#000"| 9.16 × 10<sup>−{{0}}8</sup>
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| |style="color:#BBB"| 3.30 × 10<sup>−11</sup>
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| |-
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| |scope="row"| {{0|1.0 ×}} 10<sup>−5</sup>
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| | 6.42
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| |style="color:#666"| 3.36 × 10<sup>−{{0}}7</sup>
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| |style="color:#666"| 5.71 × 10<sup>−10</sup>
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| |style="color:#000"| 3.78 × 10<sup>−{{0}}7</sup>
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| |style="color:#BBB"| 4.53 × 10<sup>−11</sup>
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| |-
| |
| |scope="row"| {{0|1.0 ×}} 10<sup>−4</sup>
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| | 5.92
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| |style="color:#000"| 3.36 × 10<sup>−{{0}}6</sup>
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| |style="color:#666"| 5.71 × 10<sup>−{{0}}9</sup>
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| |style="color:#666"| 1.19 × 10<sup>−{{0}}6</sup>
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| |style="color:#BBB"| 5.57 × 10<sup>−11</sup>
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| |-style="background-color:#AFF"
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| |scope="row"| {{0|}}3.5 × 10<sup>−4</sup>
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| | 5.65
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| |style="color:#000"| 1.18 × 10<sup>−{{0}}5</sup>
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| |style="color:#666"| 2.00 × 10<sup>−{{0}}8</sup>
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| |style="color:#666"| 2.23 × 10<sup>−{{0}}6</sup>
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| |style="color:#BBB"| 5.60 × 10<sup>−11</sup>
| |
| |-
| |
| |scope="row"| {{0|1.0 ×}} 10<sup>−3</sup>
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| | 5.42
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| |style="color:#000"| 3.36 × 10<sup>−{{0}}5</sup>
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| |style="color:#666"| 5.71 × 10<sup>−{{0}}8</sup>
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| |style="color:#666"| 3.78 × 10<sup>−{{0}}6</sup>
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| |style="color:#BBB"| 5.61 × 10<sup>−11</sup>
| |
| |-
| |
| |scope="row"| {{0|1.0 ×}} 10<sup>−2</sup>
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| | 4.92
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| |style="color:#000"| 3.36 × 10<sup>−{{0}}4</sup>
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| |style="color:#666"| 5.71 × 10<sup>−{{0}}7</sup>
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| |style="color:#666"| 1.19 × 10<sup>−{{0}}5</sup>
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| |style="color:#BBB"| 5.61 × 10<sup>−11</sup>
| |
| |-
| |
| |scope="row"| {{0|1.0 ×}} 10<sup>−1</sup>
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| | 4.42
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| |style="color:#000"| 3.36 × 10<sup>−{{0}}3</sup>
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| |style="color:#666"| 5.71 × 10<sup>−{{0}}6</sup>
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| |style="color:#666"| 3.78 × 10<sup>−{{0}}5</sup>
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| |style="color:#BBB"| 5.61 × 10<sup>−11</sup>
| |
| |-
| |
| |scope="row"| {{0|1.0 ×}} 10<sup>{{0|+}}0</sup>
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| | 3.92
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| |style="color:#000"| 3.36 × 10<sup>−{{0}}2</sup>
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| |style="color:#666"| 5.71 × 10<sup>−{{0}}5</sup>
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| |style="color:#666"| 1.20 × 10<sup>−{{0}}4</sup>
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| |style="color:#BBB"| 5.61 × 10<sup>−11</sup>
| |
| |-style="background-color:#AFF"
| |
| |scope="row"| {{0|}}2.5 × 10<sup>{{0|+}}0</sup>
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| | 3.72
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| |style="color:#000"| 8.40 × 10<sup>−{{0}}2</sup>
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| |style="color:#666"| 1.43 × 10<sup>−{{0}}4</sup>
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| |style="color:#666"| 1.89 × 10<sup>−{{0}}4</sup>
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| |style="color:#BBB"| 5.61 × 10<sup>−11</sup>
| |
| |-
| |
| |scope="row"| {{0|1.0 ×}} 10<sup>{{0|+}}1</sup>
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| | 3.42
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| |style="color:#000"| 3.36 × 10<sup>−{{0}}1</sup>
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| |style="color:#000"| 5.71 × 10<sup>−{{0}}4</sup>
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| |style="color:#666"| 3.78 × 10<sup>−{{0}}4</sup>
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| |style="color:#BBB"| 5.61 × 10<sup>−11</sup>
| |
| |}
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| * We see that in the total range of pressure, the pH is always largely lower than pKa<sub>2</sub> so that the CO<sub>3</sub><sup>2−</sup> concentration is always negligible with respect to HCO<sub>3</sub><sup>−</sup> concentration. In fact CO<sub>3</sub><sup>2−</sup> plays no quantitative role in the present calculation (see remark below).
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| * For vanishing <math>\scriptstyle p_{CO_2}</math>, the pH is close to the one of pure water (pH = 7) and the dissolved carbon is essentially in the HCO<sub>3</sub><sup>−</sup> form.
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| * For normal atmospheric conditions (<math>\scriptstyle p_{CO_2}=3.5\times 10^{-4}</math> atm), we get a slightly acid solution (p''H'' = 5.7) and the dissolved carbon is now essentially in the CO<sub>2</sub> form. From this pressure on, [OH<sup>−</sup>] becomes also negligible so that the ionized part of the solution is now an equimolar mixture of H<sup>+</sup> and HCO<sub>3</sub><sup>−</sup>.
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| * For a CO<sub>2</sub> pressure typical of the one in soda drink bottles (<math>\scriptstyle p_{CO_2}</math> ~ 2.5 atm), we get a relatively acid medium (p''H'' = 3.7) with a high concentration of dissolved CO<sub>2</sub>. These features contribute to the sour and sparkling taste of these drinks.
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| * Between 2.5 and 10 atm, the pH crosses the pKa<sub>1</sub> value (3.60) giving a dominant H<sub>2</sub>CO<sub>3</sub> concentration (with respect to HCO<sub>3</sub><sup>−</sup>) at high pressures.
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| * A plot of the equilibrium concentrations of these different forms of [[total inorganic carbon|dissolved inorganic carbon]] (and which species is dominant), as a function of the pH of the solution, is known as a [[Bjerrum plot]].
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| '''Remark'''
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| : As noted above, [CO<sub>3</sub><sup>2−</sup>] may be neglected for this specific problem, resulting in the following very precise analytical expression for [H<sup>+</sup>]:
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| : <math>\scriptstyle[H^+] \simeq \left( 10^{-14}+\frac {K_hK_{a1}}{k_\mathrm{H}} p_{CO_2}\right)^{1/2}</math>
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| ==Spectroscopic studies of carbonic acid==
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| Theoretical calculations show that the presence of even a single molecule of water causes carbonic acid to revert to carbon dioxide and water. In the absence of water, the dissociation of gaseous carbonic acid is predicted to be very slow, with a [[half-life]] of 180,000 years.<ref name="on_the_surprising">{{cite journal | last1 = Loerting | first1 = T. | last2 = Tautermann | first2 = C. | last3 = Kroemer | first3 = R.T. | last4 = Kohl | first4 = I. | last5 = Hallbrucker | first5 = E. | last6 = Mayer | first6 = A. | last7 = Liedl | first7 = K. R.
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| | title = On the Surprising Kinetic Stability of Carbonic Acid | journal =[[Angew. Chem. Int. Ed.]] | volume = 39 | pages = 891–895 | year = 2001 | doi = 10.1002/(SICI)1521-3773(20000303)39:5<891::AID-ANIE891>3.0.CO;2-E | pmid=10760883 | issue = 5}}</ref>
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| It has long been recognized that pure carbonic acid cannot be obtained at room temperatures (about 20 °C or about 70 °F). It can be generated by exposing a frozen mixture of water and carbon dioxide to high-energy radiation, and then warming to remove the excess water. The carbonic acid that remained was characterized by infrared spectroscopy. The fact that the carbonic acid was prepared by irradiating a solid H<sub>2</sub>O + CO<sub>2</sub> mixture may suggest that H<sub>2</sub>CO<sub>3</sub> might be found in outer space, where frozen ices of H<sub>2</sub>O and CO<sub>2</sub> are common, as are cosmic rays and ultraviolet light, to help them react.<ref name="on_the_surprising"/> The same carbonic acid polymorph (denoted ''beta''-carbonic acid) was prepared by heating alternating layers of glassy aqueous solutions of bicarbonate and acid ''in vacuo'', which causes protonation of bicarbonate, followed by removal of the solvent. ''Alpha''-carbonic acid was prepared by the same technique using methanol rather than water as a solvent.
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| ==See also==
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| * [[Carbonated water]]
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| * [[Ocean acidification]]
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| * [[Carbon dioxide]]
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| * [[Dihydroxymethylidene]] (carbonous acid)
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| == References ==
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| {{Reflist}}
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| ==Further reading==
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| *{{cite journal | last1 = Welch | first1 = M. J. | last2 = Lifton | first2 = J. F.
| |
| | last3 = Seck | first3 = J. A. | journal = [[J. Phys. Chem.]] | volume = 73 | issue = 335 | year = 1969 | doi = 10.1021/j100844a033 | title = Tracer studies with radioactive oxygen-15. Exchange between carbon dioxide and water | pages = 3351}}
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| *{{cite book | author=Jolly, W. L. | title=Modern Inorganic Chemistry (2nd Edn.) | location=New York | publisher=McGraw-Hill | year=1991 | isbn=0-07-112651-1}}
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| *{{cite journal | last1 = Moore | first1 = M. H. | last2 = Khanna | first2 = R. | title = Infrared and Mass Spectral Studies of Proton Irradiated H2O+Co2 Ice: Evidence for Carbonic Acid Ice: Evidence for Carbonic Acid | journal = [[Spectrochimica Acta]] | volume = 47A | doi =10.1016/0584-8539(91)80097-3 | pages = 255–262 | year = 1991 | issue = 2}}
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| * {{cite journal | last1 = W. Hage | first1 = K. R. Liedl | last2 = Liedl | first2 = E. | title = Carbonic Acid in the Gas Phase and Its Astrophysical Relevance | journal = [[Science (journal)|Science]] | volume = 279 | pages = 1332–1335
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| | year = 1998 | doi = 10.1126/science.279.5355.1332 | pmid = 9478889 | last3 = Hallbrucker | first3 = A | last4 = Mayer | first4 = E | issue = 5355}}
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| * {{cite journal
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| | last1 = Hage | first1 = W. | last2 = Hallbrucker | first2 = A. | last3 = Mayer | first3 = E. | title = Carbonic Acid: Synthesis by Protonation of Bicarbonate and Ftir Spectroscopic Characterization Via a New Cryogenic Technique | journal = [[J. Am. Chem. Soc.]] | volume = 115 | pages = 8427–8431 | doi = 10.1021/ja00071a061 | year = 1993
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| | issue = 18}}
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| * {{cite journal | last1 = Hage | first1 = W. | last2 = Hallbrucker | first2 = A.
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| | last3 = Mayer | first3 = E. | title = A Polymorph of Carbonic Acid and Its Possible Astrophysical Relevance | journal = [[J. Chem. Soc. Farad. Trans.]] | volume = 91 | pages = 2823–2826 | doi = 10.1039/ft9959102823 | year = 1995 | issue = 17}}
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| == External links ==
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| * [http://www.newton.dep.anl.gov/askasci/chem99/chem99661.htm Ask a Scientist: Carbonic Acid Decomposition]
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| * [http://www.wiley-vch.de/vch/journals/2002/press/200005press.html Why was the existence of carbonic acid unfairly doubted for so long?]
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| *[http://www2.iq.usp.br/docente/gutz/Curtipot_.html Carbonic acid/bicarbonate/carbonate equilibrium in water: pH of solutions, buffer capacity, titration and species distribution vs. pH computed with a free spreadsheet]
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| *[http://www.chem.usu.edu/~sbialkow/Classes/3600/Overheads/Carbonate/CO2.html How to calculate concentration of Carbonic Acid in Water]
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| {{Hydrogen compounds}}
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| {{Oxides of carbon}}
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| {{DEFAULTSORT:Carbonic Acid}}
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| [[Category:Acids]]
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| [[Category:Carbonates]]
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