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Hard water usually contains calcium or magnesium ions. Sodium carbonate is used for removing these ions and replacing them with sodium ions. [16] Sodium carbonate is a water-soluble source of carbonate. The calcium and magnesium ions form insoluble solid precipitates upon treatment with carbonate ions:
Softened water (measured as residual sodium carbonate index) in which calcium and magnesium have been partly replaced by sodium is not suitable for irrigation use, as it tends to cause the development of alkali soils. [28] Non-chemical devices are often used in place of traditional water softening for this application.
The very pure and finely divided precipitate of calcium carbonate that is generated is a valuable by-product used in the manufacture of toothpaste. The salting-out process used in the manufacture of soaps benefits from the common-ion effect. Soaps are sodium salts of fatty acids. Addition of sodium chloride reduces the solubility of the soap salts.
A spectator ion is an ion that exists both as a reactant and a product in a chemical equation of an aqueous solution. [1] For example, in the reaction of aqueous solutions of sodium carbonate and copper(II) sulfate: 2 Na + + CO 2− 3 (aq) + Cu 2+ (aq) + SO 2− 4 (aq) → 2 Na + (aq) + SO 2− 4 (aq) + CuCO 3
For example, in the reaction between hydrochloric acid and sodium hydroxide the sodium and chloride ions, Na + and Cl − take no part in the reaction. The reaction is consistent with the Brønsted–Lowry definition because in reality the hydrogen ion exists as the hydronium ion, so that the neutralization reaction may be written as
Water-reactive substances [1] are those that spontaneously undergo a chemical reaction with water, often noted as generating flammable gas. [2] Some are highly reducing in nature. [ 3 ] Notable examples include alkali metals , lithium through caesium , and alkaline earth metals , magnesium through barium .
Sodium carbonate is used as washing soda and for softening hard water. Sodium bicarbonate (or sodium hydrogen carbonate) is used as baking soda in cooking food, for making baking powders, as an antacid to cure indigestion and in soda acid fire extinguisher. Ammonium hydroxide is used to remove grease stains from clothes
The ammonia from reaction (III) is recycled back to the initial brine solution of reaction (I). The sodium bicarbonate (NaHCO 3) precipitate from reaction (I) is then converted to the final product, sodium carbonate (washing soda: Na 2 CO 3), by calcination (160–230 °C), producing water and carbon dioxide as byproducts: