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The commercially most relevant field of application for HCl regeneration processes is the recovery of HCl from waste pickle liquors from carbon-steel pickling lines. Other applications include the production of metal oxides such as, but not limited, to Al 2 O 3 and MgO, as well as rare-earth oxides, by pyrohydrolysis of aqueous metal chloride or rare-earth chloride solutions.
Hydrochloric acid, also known as muriatic acid or spirits of salt, is an aqueous solution of hydrogen chloride (HCl). It is a colorless solution with a distinctive pungent smell. It is classified as a strong acid. It is a component of the gastric acid in the digestive systems of most animal species, including humans.
A typical mixture is 3 parts of concentrated sulfuric acid and 1 part of 30 wt. % hydrogen peroxide solution; [1] other protocols may use a 4:1 or even 7:1 mixture. A closely related mixture, sometimes called "base piranha", is a 5:1:1 mixture of water, ammonia solution ( NH 4 OH , or NH 3 (aq) ), and 30% hydrogen peroxide.
HCl + H 2 O → [H 3 O] + + Cl −. The resulting solution is called hydrochloric acid and is a strong acid. The acid dissociation or ionization constant, K a, is large, which means HCl dissociates or ionizes practically completely in water. Even in the absence of water, hydrogen chloride can still act as an acid.
McIlvaine buffer is a buffer solution composed of citric acid and disodium hydrogen phosphate, also known as citrate-phosphate buffer.It was introduced in 1921 by the United States agronomist Theodore Clinton McIlvaine (1875–1959) from West Virginia University, and it can be prepared in pH 2.2 to 8 by mixing two stock solutions.
A more convenient laboratory method involves the (reversible) dehydration of nitrous acid by HCl [4] HNO 2 + HCl → H 2 O + NOCl. By the direct combination of chlorine and nitric oxide; This reaction reverses above 100 °C. Cl 2 + 2 NO → 2 NOCl. By reduction of nitrogen dioxide with hydrogen chloride: [5] 2NO 2 + 4 HCl → 2NOCl + 2H 2 O + Cl 2
The value can, however, be estimated theoretically. For example the value of log K ≈ −6 has been estimated for hydrogen chloride in aqueous solution at room temperature. [1] A chemical compound may behave as a strong acid in solution when its concentration is low and as a weak acid when its concentration is very high.
Arsenic trioxide is an amphoteric oxide, and its aqueous solutions are weakly acidic. Thus, it dissolves readily in alkaline solutions to give arsenites. It is less soluble in acids, although it will dissolve in hydrochloric acid. [24] With anhydrous HF and HCl, it gives AsF 3 and the trichloride: [23] As 2 O 3 + 6 HX → 2 AsX 3 + 3 H 2 O (X ...