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  2. Hydrogen chloride - Wikipedia

    en.wikipedia.org/wiki/Hydrogen_chloride

    In part because of its high polarity, HCl is very soluble in water (and in other polar solvents). Upon contact, H 2 O and HCl combine to form hydronium cations [H 3 O] + and chloride anions Cl − through a reversible chemical reaction: HCl + H 2 O → [H 3 O] + + Cl −. The resulting solution is called hydrochloric acid and is a strong acid.

  3. Hydrochloric acid - Wikipedia

    en.wikipedia.org/wiki/Hydrochloric_acid

    They range from those of water at very low concentrations approaching 0% HCl to values for fuming hydrochloric acid at over 40% HCl. [ 31 ] [ 32 ] [ 33 ] Hydrochloric acid as the binary (two-component) mixture of HCl and H 2 O has a constant-boiling azeotrope at 20.2% HCl and 108.6 °C (381.8 K; 227.5 °F).

  4. Chloroform - Wikipedia

    en.wikipedia.org/wiki/Chloroform

    Phosgene reacts with water to form carbon dioxide and HCl, [77] and the carbonate salt neutralizes the resulting acid. [ 78 ] Suspected samples can be tested for phosgene using filter paper which when treated with 5% diphenylamine , 5% dimethylaminobenzaldehyde in ethanol , and then dried, turns yellow in the presence of phosgene vapour. [ 79 ]

  5. Sulfuric acid - Wikipedia

    en.wikipedia.org/wiki/Sulfuric_acid

    Although nearly 100% sulfuric acid solutions can be made, the subsequent loss of SO 3 at the boiling point brings the concentration to 98.3% acid. The 98.3% grade, which is more stable in storage, is the usual form of what is described as "concentrated sulfuric acid".

  6. Phenethylamine - Wikipedia

    en.wikipedia.org/wiki/Phenethylamine

    Phenethylamine is strongly basic, pK b = 4.17 (or pK a = 9.83), as measured using the HCl salt, and forms a stable crystalline hydrochloride salt with a melting point of 217 °C. [ 10 ] [ 21 ] Its experimental log P is 1.41.

  7. Nitrogen trifluoride - Wikipedia

    en.wikipedia.org/wiki/Nitrogen_trifluoride

    2 NF 3 + 6 HCl → 6 HF + N 2 + 3 Cl 2. However, it only attacks (explosively) organic compounds at high temperatures. Consequently it is compatible under standard conditions with several plastics, as well as steel and Monel. [6] Above 200-300 °C, NF 3 reacts with metals, carbon, and other reagents to give tetrafluorohydrazine: [13]

  8. Dry matter - Wikipedia

    en.wikipedia.org/wiki/Dry_matter

    Preparation of a sample of honey on a prism for a refractometric analysis in order to detect the percentage of dry mass. In the sugar industry the dry matter content is an important parameter to control the crystallization process and is often measured on-line by means of microwave density meters. [9]

  9. Ammonia solution - Wikipedia

    en.wikipedia.org/wiki/Ammonia_solution

    At 15.6 °C (60.1 °F), the density of a saturated solution is 0.88 g/ml; it contains 35.6% ammonia by mass, 308 grams of ammonia per litre of solution, and has a molarity of approximately 18 mol/L. At higher temperatures, the molarity of the saturated solution decreases and the density increases. [ 8 ]