![]() ![]() When hydrochloric acid is added, the added chloride ions shift the equilibrium position in favour of blue CoCl 4 2-ions and water. Initially, the beaker contains a red-pink solution of cobalt (II) chloride, present as Co (H 2 O) 6 2+ ions and chloride ions. Michie, A. Miller, Synthesis, 824 (1981)ī. Demonstration showing the changing equilibrium of cobalt complexes in solution. Wuts, Protective Groups in Organic Synthesis, 3rd edn. Recommended use : Laboratory chemicals Restrictions on use : Not for food, drug or household use. Use of the substance/mixture : For laboratory and manufacturing use only. This review precises chemoselective procedure for the preparation of acylals by using the metal-based Lewis acid catalysts, magnetic nanocatalysts, ionic liquids, strong protic acid and solid acids.į. Synonyms : cobalt dichloride, hexahydrate. Protection of carbonyl group of aldehydes by acetic anhydride in the presence of acid catalyst is the most convenient way. Also acylals have been used as intermediates in industry as cross-linking agents for cellulose in cotton. Beyond their protecting role, 1,1-diacetates are important precursors for the synthesis of acetoxydienes, starting materials as valuable intermediates for Diels–Alder cycloaddition reactions and neutral and basic media. As if we needed any reason at all to eat chocolate, it can help with weight loss, has a lot of nutrients, and is actually one of the best sources of dietary cobalt at up to 0.050 µg. Yes, chocolate Everyone’s favorite sweet treat is the first on this list. Among these groups, protection of aldehydes such as diacetates (acylals) has attracted more attention in the organic chemistry due to its superior applications such as commodity chemical in various fields of chemistry, their ease of preparation and their stability toward basic and neutral conditions. Here are the top 10 foods high in cobalt: 1. They are not toxic like lead or mercury compounds, though.Selective protection of carbonyl groups such as oxathioacetals, acylals, acetals and dithioacetals is the vital steps in organic chemistry. Cobalt compounds are toxic in large quantities, like any other transition metal compounds. ![]() It is a weak oxidizing agent, too weak to ignite things. It is the most common cobalt compound in the lab. It can be used to make other cobalt compounds. It is used to place cobalt into other chemical compounds. The hydrated (with water) red form can be made by reacting cobalt(II) oxide or cobalt(II) hydroxide with hydrochloric acid. The anhydrous (without water) blue form can be made by reacting cobalt with chlorine. If it is made, it just drops a Cl from CoCl 3, making CoCl 2 (cobalt(II) chloride) again. ![]() Upon heating of the hydrated form, water of crystallisation is lost and the anhydrous form is formed. The relative density of cobalt dichloride is 3.36-3.37. It can be oxidized to cobalt(III) compounds, although cobalt(III) chloride does not exist. Cobalt dichloride is typically marketed as the hexahydrate, which is a purple, odourless, crystalline, inorganic solid. Cobalt chloride can be used to test for chloride ions in this way. When it is heated, it turns more blue than when it is cooled.įor an example. Hydrochloric acid works the best, but sodium chloride can be used too. The green form is cobalt chloride reacted with a lot of hydrochloric acid.Ī different blue form is made when cobalt(II) chloride is reacted with a chemical compound that has chloride in it. Cobalt dichloride is a chemical that changes colour when exposed to changing storage levels of moisture and is commonly used in HICs for that purpose. The blue form is the color that it gives with some hydrochloric acid. The blue form will absorb water from the air and turn red again.Ĭobalt(II) chloride reacted with hydrochloric acid. It can be heated to turn it into the blue form, without water. Properties Cobalt (II) chloride is normally found in the red (or pink) form. It contains cobalt in its +2 oxidation state. It contains cobalt and chloride ions.Ĭobalt(II) chloride is normally found in the red (or pink) form. Cobalt (II) chloride, also known as cobaltous chloride and cobalt dichloride, is a chemical compound. Except where otherwise noted, data are given for materials in their standard state (at 25 ☌, 100 kPa).Ĭobalt(II) chloride hexahydrate (with six water molecules attached) Cobalt(II) chloride anhydrous (with no water molecules attached)Ĭobalt(II) chloride, also known as cobaltous chloride and cobalt dichloride, is a chemical compound. ![]()
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