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Lithium hypochlorite is a chemical compound with the chemical formula of Li O Cl. It is the lithium salt of hypochlorous acid. It consists of lithium cations (Li +) and hypochlorite anions (− OCl). It is a colorless, crystalline compound. It has been used as a disinfectant for pools, and is also used as a reagent for some chemical reactions.
Anhydrous lithium hypochlorite is stable at room temperature; however, sodium hypochlorite is explosive as an anhydrous solid. [6] The pentahydrate (NaOCl·(H 2 O) 5) is unstable above 0 °C; [7] although the more dilute solutions encountered as household bleach are more stable. Potassium hypochlorite (KOCl) is known only in solution. [4]
Lithium aluminium hydride – LiAlH 4; Lithium bromide – LiBr; Lithium borohydride – LiBH 4; Lithium carbonate (Lithium salt) – Li 2 CO 3; Lithium chloride – LiCl; Lithium hypochlorite – LiClO; Lithium chlorate – LiClO 3; Lithium perchlorate – LiClO 4; Lithium cobalt oxide – LiCoO 2; Lithium oxide – Li 2 O; Lithium peroxide ...
Hypochlorous acid is an inorganic compound with the chemical formula Cl O H, also written as HClO, HOCl, or ClHO. [2] [3] Its structure is H−O−Cl.It is an acid that forms when chlorine dissolves in water, and itself partially dissociates, forming a hypochlorite anion, ClO −.
Anhydrous sodium hypochlorite can be prepared but, like many hypochlorites, it is highly unstable and decomposes explosively on heating or friction. [5] The decomposition is accelerated by carbon dioxide at Earth's atmospheric levels - around 4 parts per ten thousand. [6] [15] It is a white solid with the orthorhombic crystal structure. [16]
Lithium perchlorate is also used as an electrolyte salt in lithium-ion batteries.Lithium perchlorate is chosen over alternative salts such as lithium hexafluorophosphate or lithium tetrafluoroborate when its superior electrical impedance, conductivity, hygroscopicity, and anodic stability properties are of importance to the specific application. [11]
Lithium chloride is a chemical compound with the formula Li Cl.The salt is a typical ionic compound (with certain covalent characteristics), although the small size of the Li + ion gives rise to properties not seen for other alkali metal chlorides, such as extraordinary solubility in polar solvents (83.05 g/100 mL of water at 20 °C) and its hygroscopic properties.
The tables below provides information on the variation of solubility of different substances (mostly inorganic compounds) in water with temperature, at one atmosphere pressure.