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Calcium bicarbonate, also called calcium hydrogencarbonate, has the chemical formula Ca(HCO 3) 2. The term does not refer to a known solid compound; it exists only in aqueous solution containing calcium (Ca 2+), bicarbonate (HCO − 3), and carbonate (CO 2− 3) ions, together with dissolved carbon dioxide (CO 2).
The Leblanc process was an early industrial process for making soda ash (sodium carbonate) used throughout the 19th century, named after its inventor, Nicolas Leblanc.It involved two stages: making sodium sulfate from sodium chloride, followed by reacting the sodium sulfate with coal and calcium carbonate to make sodium carbonate.
Usually the process is conducted on a brine (an aqueous solution of concentrated NaCl), in which case sodium hydroxide (NaOH), hydrogen, and chlorine result. When using calcium chloride or potassium chloride , the products contain calcium or potassium instead of sodium.
For pH control, popular chemicals include calcium carbonate, calcium oxide, magnesium hydroxide, and sodium bicarbonate. The selection of an appropriate neutralization chemical depends on the particular application. There are many uses of neutralization reactions that are acid-alkali reactions. A very common use is antacid tablets.
Hydrochloric acid has been used for dissolving calcium carbonate, e.g. such things as de-scaling kettles and for cleaning mortar off brickwork. When used on brickwork the reaction with the mortar only continues until the acid has all been converted, producing calcium chloride, carbon dioxide, and water: CaCO 3 + 2 HCl → CaCl 2 + CO 2 + H 2 O
The Mannheim process is an industrial process for the production of hydrogen chloride and sodium sulfate from sulfuric acid and sodium chloride. [1] The Mannheim furnace is also used to produce potassium sulfate from potassium chloride. [2] The Mannheim process is a stage in the Leblanc process for the production of sodium carbonate.
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
Dakin's original solution contained sodium hypochlorite (0.4% to 0.5%), prepared by treating calcium hypochlorite with sodium carbonate ("washing soda"). The solution left after removal of the insoluble calcium carbonate still contained some soda. [7] Boric acid (4%) was then added as a buffering agent to maintain a pH of between 9 and 10.