In order to create Carbonated water and other carbonated beverages, the concentration of Carbonate and bi Carbonate ions in water must be increased. This can be done either by adding carbon dioxide gas under pressure or by dissolving Carbonate or bi Carbonate salts into the water. The term is also used as a verb. The term "Carbonate" in geology and mineralogy can be used to describe both Carbonate minerals and Carbonate rock (which is primarily composed of Carbonate minerals), both of which are dominated by the Carbonate ion.
In chemically precipitated sedimentary rock, Carbonate minerals are exceedingly diverse and pervasive. The Carbonate ion, a polyatomic ion with the formula CO23, is what distinguishes a Carbonate from other salts of carbonic acid. The term "Carbonate" can also refer to an organic molecule with a Carbonate group called a Carbonate ester. The simplest Oxo carbon anion is the Carbonate ion. It has D3h molecular symmetry and is made up of one carbon atom surrounded by three oxygen atoms in a trigonal planar configuration. It has a total formal charge of 2 and a molecular mass of 60.01 g/mol. It is the conjugate base of the HCO ion, the conjugate base of H2CO3, carbonic acid, which is the hydrogen Carbonate (bi Carbonate) ion. Two (long) single bonds to negative oxygen atoms make up the Carbonate ion's Lewis structure, while a single, brief double bond to a neutral oxygen atom completes it. On heating, metal Carbonates often disintegrate, releasing carbon dioxide from the long carbon cycle into the short carbon cycle and leaving a metal oxide behind. Calx, the Latin term for quicklime or calcium oxide, CaO, which is produced by roasting limestone in a lime kiln, inspired the phrase "calcination," which refers to this process. When a positively charged ion, such as M+, M2+, or M3+, develops an electrostatic attraction with the negatively charged oxygen atoms of the ion to form an ionic compound, a Carbonate salt is created. At normal pressure and temperature, the majority of Carbonate salts are insoluble in water, with solubility constants of less than 1108. Several uranium Carbonates as well as the Carbonates of lithium, sodium, potassium, rubidium, caesium, and ammonium are exceptions. Carbonate, bi Carbonate, carbon dioxide, and carbonic acid all coexist in aqueous solution in a dynamic equilibrium. The Carbonate ion predominates in very basic environments, whereas the bi Carbonate ion predominates in slightly basic settings. Aqueous carbon dioxide, CO2(aq), which is the predominant form under more acidic conditions, is in equilibrium with carbonic acid when combined with water, H2O; the balance is substantially in favour of carbon dioxide. As a result, sodium bi Carbonate is weakly basic while carbon dioxide itself is a weak acid. Sodium Carbonate is also basic. Under pressure, CO2 dissolves in water to produce Carbonated water. The equilibrium for each form of Carbonate (Carbonate, bi Carbonate, carbon dioxide, and carbonic acid) shifts when the partial pressure of CO2 is reduced, such as when a soda can is opened, until the concentration of CO2 in the solution is equal to the solubility of CO2 at that temperature and pressure. The conversion of CO2 and carbonic acid occurs more quickly in living systems thanks to the enzyme carbonic anhydrase. While the bi Carbonate salts of most metals are soluble in water, the Carbonate salts of most metals are not. The balance between Carbonate, bi Carbonate, carbon dioxide, and carbonic acid in a solution is continually shifting due to the ambient temperature and pressure. Insoluble compounds are created when metal ions interact with insoluble Carbonates, as CaCO3. This explains how hard water causes scale to accumulate inside of pipes.
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