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Carbonic acid is a chemical compound with the chemical formula H 2 C O 3.The molecule rapidly converts to water and carbon dioxide in the presence of water. However, in the absence of water, it is quite stable at room temperature.
A carbonate is a salt of carbonic acid, (H 2 CO 3), [2] characterized by the presence of the carbonate ion, a polyatomic ion with the formula CO 2− 3.The word "carbonate" may also refer to a carbonate ester, an organic compound containing the carbonate group O=C(−O−) 2.
Numerous organic compounds have other common names, often originating in historical source material thereof. The systematic IUPAC name is not always the preferred IUPAC name , for example, lactic acid is a common, and also the preferred, name for what systematic rules call 2-hydroxypropanoic acid.
Sodium bicarbonate (IUPAC name: sodium hydrogencarbonate [9]), commonly known as baking soda or bicarbonate of soda, is a chemical compound with the formula NaHCO 3. It is a salt composed of a sodium cation (Na +) and a bicarbonate anion (HCO 3 −). Sodium bicarbonate is a white solid that is crystalline but often appears as a fine powder.
A bicarbonate salt forms when a positively charged ion attaches to the negatively charged oxygen atoms of the ion, forming an ionic compound. Many bicarbonates are soluble in water at standard temperature and pressure; in particular, sodium bicarbonate contributes to total dissolved solids, a common parameter for assessing water quality. [6]
Hydrochloric acid – HCl(aq) Hydrogen chloride – HCl; Hypochlorous acid – HOCl; Indium(I) chloride – InCl; Indium(III) chloride – InCl 3; Iodine monochloride – ICl; Iridium(III) chloride – IrCl 3; Iron(II) chloride – FeCl 2; Iron(III) chloride – FeCl 3; Lanthanum chloride – LaCl 3; Lead(II) chloride – PbCl 2; Lithium ...
Attempts to prepare compounds such as solid calcium bicarbonate by evaporating its solution to dryness invariably yield instead the solid calcium carbonate: [1] Ca(HCO 3) 2 → CO 2 (g) + H 2 O(l) + CaCO 3 (s). Very few solid bicarbonates other than those of the alkali metals (other than ammonium bicarbonate) are known to exist. [clarification ...
Note: in dilute aqueous solution the formation of the hydronium ion, H 3 O + (aq), is effectively complete, so that hydration of the proton can be ignored in relation to the equilibria. Other examples of inorganic polyprotic acids include anions of sulfuric acid , phosphoric acid and hydrogen sulfide that have lost one or more protons.