H2CO32

H2CO32 is not a standard chemical formula in established nomenclature. It is likely a typographical error or a misinterpretation of carbonic acid, H2CO3, or of the carbonate system that appears in aqueous solutions. This article describes the commonly encountered chemistry associated with carbonic acid rather than a distinct compound represented by H2CO32.

Carbonic acid itself is a weak acid that exists in equilibrium with dissolved carbon dioxide in water: CO2 plus water forms H2CO3 in solution, though most dissolved CO2 is present as CO2 rather than as H2CO3. In aqueous environments, carbonic acid readily participates in acid–base equilibria that regulate pH. The first dissociation yields bicarbonate: H2CO3 ⇌ H+ + HCO3−, with a pKa around 6.35. The second dissociation yields carbonate: HCO3− ⇌ H+ + CO3^2−, with a pKa around 10.33. These equilibria form the carbonic acid–bicarbonate–carbonate buffering system.

Occurrences and significance: The carbonic acid/bicarbonate system is central to biological pH regulation, notably in blood, where it helps transport CO2 from tissues to lungs. It also governs the chemistry of seawater and plays a key role in geological and environmental processes, including carbonate mineral formation and the ongoing topic of ocean acidification as atmospheric CO2 levels rise.

Preparation and uses: Carbonic acid is typically not isolated as a pure solid; it is generated in situ in water from dissolved CO2. The system is harnessed as a buffering agent in laboratories and in various industrial applications, and its bicarbonate form is widely used in food and beverage contexts.

Safety: Carbonic acid is a weak acid and, in practice, its effects are dominated by dissolved CO2. Excess CO2 can pose asphyxiation risks in enclosed spaces, and handling should follow standard laboratory or industrial safety guidelines.