[{"@context":"http:\/\/schema.org\/","@type":"BlogPosting","@id":"https:\/\/wiki.edu.vn\/en\/wiki24\/precipitation-chemistry-wikipedia\/#BlogPosting","mainEntityOfPage":"https:\/\/wiki.edu.vn\/en\/wiki24\/precipitation-chemistry-wikipedia\/","headline":"Precipitation (chemistry) – Wikipedia","name":"Precipitation (chemistry) – Wikipedia","description":"before-content-x4 Chemical process leading to the settling of an insoluble solid from a solution Principle of chemical precipitation in aqueous","datePublished":"2022-10-17","dateModified":"2022-10-17","author":{"@type":"Person","@id":"https:\/\/wiki.edu.vn\/en\/wiki24\/author\/lordneo\/#Person","name":"lordneo","url":"https:\/\/wiki.edu.vn\/en\/wiki24\/author\/lordneo\/","image":{"@type":"ImageObject","@id":"https:\/\/secure.gravatar.com\/avatar\/c9645c498c9701c88b89b8537773dd7c?s=96&d=mm&r=g","url":"https:\/\/secure.gravatar.com\/avatar\/c9645c498c9701c88b89b8537773dd7c?s=96&d=mm&r=g","height":96,"width":96}},"publisher":{"@type":"Organization","name":"Enzyklop\u00e4die","logo":{"@type":"ImageObject","@id":"https:\/\/wiki.edu.vn\/wiki4\/wp-content\/uploads\/2023\/08\/download.jpg","url":"https:\/\/wiki.edu.vn\/wiki4\/wp-content\/uploads\/2023\/08\/download.jpg","width":600,"height":60}},"image":{"@type":"ImageObject","@id":"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/thumb\/b\/b0\/Chemical_precipitation_diagram_multilang.svg\/220px-Chemical_precipitation_diagram_multilang.svg.png","url":"https:\/\/upload.wikimedia.org\/wikipedia\/commons\/thumb\/b\/b0\/Chemical_precipitation_diagram_multilang.svg\/220px-Chemical_precipitation_diagram_multilang.svg.png","height":"202","width":"220"},"url":"https:\/\/wiki.edu.vn\/en\/wiki24\/precipitation-chemistry-wikipedia\/","about":["Wiki"],"wordCount":4784,"articleBody":"     (adsbygoogle = window.adsbygoogle || []).push({});before-content-x4Chemical process leading to the settling of an insoluble solid from a solution  Principle of chemical precipitation in aqueous solution       (adsbygoogle = window.adsbygoogle || []).push({});after-content-x4In an aqueous solution, precipitation is the process of transforming a dissolved substance into an insoluble solid from a super-saturated solution.[1][2] The solid formed is called the precipitate.[3] In case of an inorganic chemical reaction leading to precipitation, the chemical reagent causing the solid to form is called the precipitant.[4]The clear liquid remaining above the precipitated or the centrifuged solid phase is also called the ‘supernate’ or ‘supernatant’.       (adsbygoogle = window.adsbygoogle || []).push({});after-content-x4The notion of precipitation can also be extended to other domains of chemistry (organic chemistry and biochemistry) and even be applied to the solid phases (e.g., metallurgy and alloys) when solid impurities segregate from a solid phase.Table of ContentsSupersaturation[edit]Nucleation[edit]Inorganic chemistry[edit]Precipitation in aqueous solution[edit]Reductive precipitation[edit]Precipitate colors[edit]Anion\/cation qualitative analysis[edit]Colloidal suspensions[edit]Digestion and precipitates ageing[edit]Organic chemistry[edit]Biochemistry[edit]Metallurgy and alloys[edit]Industrial processes[edit]History[edit]See also[edit]References[edit]Additional reading[edit]External links[edit]Supersaturation[edit]The precipitation of a compound may occur when its concentration exceeds its solubility. This can be due to temperature changes, solvent evaporation, or by mixing solvents. Precipitation occurs more rapidly from a strongly supersaturated solution.       (adsbygoogle = window.adsbygoogle || []).push({});after-content-x4The formation of a precipitate can be caused by a chemical reaction. When a barium chloride solution reacts with sulphuric acid, a white precipitate of barium sulfate is formed. When a potassium iodide solution reacts with a lead(II) nitrate solution, a yellow precipitate of lead(II) iodide is formed.Nucleation[edit]An important stage of the precipitation process is the onset of nucleation. The creation of a solid particle implies the formation of an interface with the solution. This involves energy changes depending on the dissolution reaction free energy (endothermic or exothermic process accompanied by an entropy increase) and the relative surface energy developed between the solid and the solution. If energy changes are not favorable, or without suitable nucleation sites, no precipitation occurs and the solution remain supersaturated.Inorganic chemistry[edit]Precipitation in aqueous solution[edit]A common example of precipitation reaction in aqueous solution is that of silver chloride. When silver nitrate (AgNO3) is added to a solution of potassium chloride (KCl) the precipitation of a white solid (AgCl) is observed.[5][6]"},{"@context":"http:\/\/schema.org\/","@type":"BreadcrumbList","itemListElement":[{"@type":"ListItem","position":1,"item":{"@id":"https:\/\/wiki.edu.vn\/en\/wiki24\/#breadcrumbitem","name":"Enzyklop\u00e4die"}},{"@type":"ListItem","position":2,"item":{"@id":"https:\/\/wiki.edu.vn\/en\/wiki24\/precipitation-chemistry-wikipedia\/#breadcrumbitem","name":"Precipitation (chemistry) – Wikipedia"}}]}]