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Perchloric acid is a mineral acid with the formula H Cl O 4. It is an oxoacid of chlorine . Usually found as an aqueous solution, this colorless compound is a stronger acid than sulfuric acid , nitric acid and hydrochloric acid .
4.1: Decaborane: UN 1869: 4.3: Magnesium or Magnesium alloys with more than 50 percent magnesium in pellets, turnings, or ribbons UN 1870: 4.1: Potassium borohydride: UN 1871: 5.1: Titanium hydride: UN 1872: 5.1: Lead dioxide: UN 1873: 5.1: Perchloric acid with more than 50 percent but not more than 72 percent acid, by mass UN 1874 to 1883? (UN ...
Potassium perchlorate in crystal form. Potassium perchlorate is prepared industrially by treating an aqueous solution of sodium perchlorate with potassium chloride.This single precipitation reaction exploits the low solubility of KClO 4, which is about 1/100 as much as the solubility of NaClO 4 (209.6 g/100 mL at 25 °C).
Ammonium perchlorate (AP) is produced by reaction between ammonia and perchloric acid.This process is the main outlet for the industrial production of perchloric acid.The salt also can be produced by salt metathesis reaction of ammonium salts with sodium perchlorate.
As perchloric acid is one of the strongest mineral acids, perchlorate is a weak base in the sense of Brønsted–Lowry acid–base theory. As it is also generally a weakly coordinating anion , perchlorate is commonly used as a background , or supporting, electrolyte .
Barium perchlorate is also used for the determination of small concentrations (down to 10 ppm, with an accuracy of +/- 1 ppm) of sulfate. [5] In order for the titration to be successful, a high concentration of a nonaqueous solvent, such as ethyl alcohol, 2-propanol, or methanol, must be present. Thorin is typically used as the indicator.
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Lead perchlorate trihydrate is produced by the reaction of lead(II) oxide, lead carbonate, or lead nitrate by perchloric acid: . Pb(NO 3) 2 + HClO 4 → Pb(ClO 4) 2 + HNO 3. The excess perchloric acid was removed by first heating the solution to 125 °C, then heating it under moist air at 160 °C to remove the perchloric acid by converting the acid to the dihydrate.
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