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Out of the four stable halogens, only fluorine and chlorine have reduction potentials higher than that of oxygen, allowing them to form hydrofluoric acid and hydrochloric acid directly through reaction with water. [17] The reaction of fluorine with water is especially hazardous, as an addition of fluorine gas to cold water will produce ...
Dichlorine monoxide is highly soluble in water, [6] where it exists in an equilibrium with HOCl. The rate of hydrolysis is slow enough to allow the extraction of Cl 2 O with organic solvents such as CCl 4, [3] but the equilibrium constant ultimately favours the formation of hypochlorous acid. [7] 2 HOCl ⇌ Cl 2 O + H 2 O K (0 °C) = 3.55x10 ...
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 −.
Evaporation under reduced pressure allows it to be concentrated further to about 40%, but then it decomposes to perchloric acid, chlorine, oxygen, water, and chlorine dioxide. Its most important salt is sodium chlorate, mostly used to make chlorine dioxide to bleach paper pulp. The decomposition of chlorate to chloride and oxygen is a common ...
dichlorine pentoxide, Cl 2 O 5 or ClOOClO 3, is hypothetical; dichlorine hexoxide or chloryl perchlorate, Cl 2 O 6 or [ClO 2] + [ClO 4] −, chlorine (V,VII) oxide; dichlorine heptoxide, Cl 2 O 7, chlorine (VII) oxide; dichlorine octoxide, chlorine (VII) oxide peroxide or dimer of chlorine tetroxide radical, Cl 2 O 8 or (OClO 3) 2; Several ions ...
The hypochlorite anion and chlorine are in equilibrium in water; the position of the equilibrium is pH dependent and low pH (acidic) favors chlorine, [11] Cl 2 + H 2 O ⇌ 2H + + Cl − + ClO −. A hypochlorite bleach can react violently with hydrogen peroxide and produce oxygen gas: H 2 O 2 (aq) + NaOCl (aq) → NaCl (aq) + H 2 O(l) + O 2 (g)
2 which dissociates in water to form hypochlorite. This reaction must be conducted in non-acidic conditions to prevent release of chlorine: 2 Cl − → Cl 2 + 2 e − Cl 2 + H 2 O ⇌ HClO + Cl − + H + Some hypochlorites may also be obtained by a salt metathesis reaction between calcium hypochlorite and various metal sulfates.
For example, it is commonly asserted that the reactivity of alkali metals (Na, K, etc.) increases down the group in the periodic table, or that hydrogen's reactivity is evidenced by its reaction with oxygen. In fact, the rate of reaction of alkali metals (as evidenced by their reaction with water for example) is a function not only of position ...