In general, it's tricky to predict for any random reaction what medium it might need. Water is a really great solvent whenever you want to have ions around. Double replacement reactions always occur in water, with the reactants in the aqueous state. Luckily, there aren't that many strong acids and bases, and you can learn morem about this from this video: Īnything that is soluble in water and dissolved (separated into individual cations and anions) is in the aqueous state. It is helpful to have the strong acids and bases memorized, since they have special reactivity. The cation (or positively charged ion) of the salt comes from the base, and the anion (or negatively charged ion) comes from the acid. ![]() If you have tried this reaction at home, you probably remember a lot of fizzing because the neutralization reaction is accompanied by a gas-producing reaction, where the carbonic acid decomposes into carbon dioxide gas-bubbles!-and water.Ī salt is generally any ionic compound, though I have also seen it defined as an ionic compound that is formed when you react an acid and a base. In the healthcare industry, it is routinely used as an effective acid neutralizer in antacid tablets and liquids.A B − C D − → A D − C B − \greenD NaCH 3 COO start text, N, a, C, H, end text, start subscript, 3, end subscript, start text, C, O, O, end text. It can also provide cost savings to paper manufacturers through the replacement of more expensive pulp fiber and optical brightening agents.ĭue to the physical and mechanical properties of calcium carbonate, its small particle size and crystal shape means that it also has many industrial uses like increasing impact strength in polymers. Here, the impurities level must be well controlled, especially the iron oxide and manganese oxide. The whiteness and brightness of precipitated calcium carbonate is very critical, especially for office (white) paper manufacturing. Specifically, paper-making requires large quantities of calcium carbonate which provides the paper with its whiteness and consistency. The National Lime Association mentions the use of precipitated calcium carbonate in the paper, polymer, and healthcare industries. It can be found as a functional additive in everything from sealants and adhesives to inks and rubber. Calcium carbonate is used in the paper industry both as a PCC filler and as a coating which allows for the paper to have such a pure white color. Precipitated Calcium Carbonate is used in several different areas of production such as the flooring, paint, and paper industry due to its mechanical and optical properties. Carmeuse is able to provide the raw materials, freight, and slaking systems to ensure that your needs are met. This can lead to downtime, not meeting your customers’ needs, additional waste, and impact your overall bottom line.Įquipment and corresponding processes may also need to be updated or replaced over time due to natural evolution of technology or normal wear and tear. Variations in quicklime quality can result in difficulties slaking and inconsistent particle size. ![]() ![]() Lime reactivity is key to achieving a finer particle size distribution and particle shape of PCC, as well as the stability of the process. ![]() An even precipitation process allows good control of the crystallization and particle size of the PCC. Precipitated calcium carbonate is produced by slaking high-calcium quicklime to create a lime slurry that is then combined with captured carbon dioxide (CO 2). The precipitated calcium carbonate production process consists of decarbonating limestone, which separates the CaO (calcium oxide) and CO 2 (carbon dioxide). Precipitated Calcium Carbonate (PCC) production requires consistent quicklime quality to produce a quality carbonate. How Is Precipitated Calcium Carbonate (PCC) Made?
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