Carbonic acid: synthesis by protonation of bicarbonate and FTIR spectroscopic characterization via a new cryogenic technique

Hage, Wolfgang; Hallbrucker, Andreas; Mayer, Erwin

doi:10.1021/ja00071a061

Cited by 92 publications

(132 citation statements)

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“…IR adsorbance bands in Figure 2 were attributed to the free HCO 3-anion because this anion is the predominant species at pH 28 (>97% of total C). There was essentially no neutral H2CO3 ~ present as indicated by the absence of a band near 1730 cm -1 in the spectra for C = O stretching (Hage et al 1993 2) and 1.0 M NaHCO3 (pH 7.9) solutions and 0.01 (pH 8.2), 0.1 (pH 8.2) and 1.0 M NaC1 (pH 7.9) solutions, respectively. The spectrum of NaC1 solution was subtracted from spectrum of NaHCO3 solution.…”

Section: Surface Charge At the Shear Planementioning

confidence: 98%

In Situ Infrared Speciation of Adsorbed Carbonate on Aluminum and Iron Oxides

Suarez

1997

Clays and clay miner.

254

176

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Abstract--Surface adsorption mechanisms of dissolved inorganic carbon species on soil minerals are not well understood. Traditional infrared (IR) study of adsorbed species of inorganic carbon using air-dried samples may not reveal true species in the solid/water interface in suspension. The ptu'pose of this study was to obtain information on interracial carbonate speciation between solid and aqueous phases. The interaction of bicarbonate and carbonate ions with X-ray amorphous (am) A1 and Fe oxides, gibbsite (~/-AI(OH)3 ) and goethite (a-FeOOH) was examined by electrophoresis and in situ attenuated total reflectance Fourier transform infrared (ATR-FTIR) spectroscopy. The presence of carbonate lowered the electrophoretic mobility and decreased the point of zero charge (PZC) of all minerals, implying specific adsorption. Inner-sphere complexation of bicarbonate and carbonate was supported by a lowering in the anion symmetry due to the interaction with A1 and Fe oxide surfaces. Only complexed monodentate carbonate was identified in am-Al(OH)3/aqueous solution at pH 4.1-7.8 when the solid was reacted with either NanCO 3 or Na2CO 3 solutions. Am-AI(OH)3 was transformed to a crystalline sodium aluminum hydroxy carbonate, dawsonite [NaAl(CO3)(OH)2], and bayerite (ct-AI(OH)3) after reacting with 1.0 M Na2CO3 for 24 h. Gibbsite adsorbed much less carbonate than am-AI(OH)3 such that adsorbed carbonate on gibbsite gave weak IR absorption. It is probable that monodentate carbonate is also the complexed species on gibbsite. Evidence suggesting the presence of both surface complexed bicarbonate and carbonate species in the interfacial region of am-Fe(OH)3 in suspension and the dependence of their relative distribution on solution pH is shown. Only monodentate carbonate was found in the interracial region of goethite in 1.0 M NaHCO3. A ligand exchange reaction was proposed to describe the interaction of bicarbonate and carbonate with the surface functional groups of A1 and Fe oxides.

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Section: Surface Charge At the Shear Planementioning

confidence: 98%

In Situ Infrared Speciation of Adsorbed Carbonate on Aluminum and Iron Oxides

Suarez

1997

Clays and clay miner.

254

176

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“…For studying the vapor pressure of H 2CO3 , the compound first was made by an acid-base reaction between a 1 molar solution of HBr (Sigma-Aldrich) and a 0.1 molar solution of KHCO3 (Sigma-Aldrich), similar to the technique of Hage et al (1993). A few microliters of the KHCO3 solution were injected through a septum, using a syringe, onto a KBr substrate at 10 K, attached to the tail section of a closed-cycle helium cryostat.…”

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confidence: 99%

The formation and stability of carbonic acid on outer Solar System bodies

Peeters

Hudson

Moore

et al. 2010

Icarus

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“…For a long time even the observation of intermediary formed carbonic acid appeared unlikely due to the apparently rapid decay. Despite the belief of the nonexistence of carbonic acid, chemists recently succeeded first in recognizing the stability of carbonic acid [4,5] and then in isolating and characterizing [6,7] pure carbonic acid. It was even possible to sublime and recondense the solid and therefore prove the stability of gasphase carbonic acid.…”

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confidence: 99%