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Sodium perchlorate is the precursor to ammonium, potassium and lithium perchlorate salts, often taking advantage of their low solubility in water relative to NaClO 4 (209 g/(100 mL) at 25 °C). [ 6 ] It is used for denaturating proteins in biochemistry and in standard DNA extraction and hybridization reactions in molecular biology .
Anhydrous perchloric acid is an unstable oily liquid at room temperature. It forms at least five hydrates, several of which have been characterized crystallographically. These solids consist of the perchlorate anion linked via hydrogen bonds to H 2 O and H 3 O + centers. [9] An example is hydronium perchlorate.
Sodium perchlorate (NaClO 4) is often used as a background electrolyte because of its convenient properties to fulfil this function. It is a highly soluble salt (2096 g/L at 25 °C) allowing to increase the ionic strength of a solution up to 8 M. It is not a complexing ligand, thus it does not interfere in complexation studies.
Perchlorate salts are typically manufactured through the process of electrolysis, which involves oxidizing aqueous solutions of corresponding chlorates. This technique is commonly employed in the production of sodium perchlorate, which finds widespread use as a key ingredient in rocket fuel. [5]
Sodium chlorate can be used with hydrochloric acid (or also sulfuric acid and sodium chloride, the reaction of which generates HCl) to chlorinate aromatic compounds without the use of organic solvents. In this case its function is to oxidize the HCl to obtain either HOCl or Cl 2 (depending upon the pH) in-situ which are the active chlorinating ...
The space-group assignment of the structure was resolved, with the centrosymmetric assignment of P6 3 /m confirmed. Each axial perchlorate oxygen is hydrogen bonded to three water molecules and each trigonal oxygen is hydrogen bonded to two water molecules. This interaction is the reason that the perchlorate fails to be tetrahedral.
Hydronium perchlorate is produced by the reaction of anhydrous perchloric acid and water in a 1:1 molar ratio: [2]. HClO 4 + H 2 O → [H 3 O] + ClO − 4. A more analytically reliable method was reported using the macrocyclic Schiff base of sodium 2,6-diformyl-4-methylphenolate and 2,6-diformyl-4-methylphenol as a chelating agent to sequester Cu(II): transmetallation of the macrocycle with ...
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]