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This green color results from an intense absorption at 610 nm. In the laboratory, K 2 MnO 4 can be synthesized by heating a solution of KMnO 4 in concentrated KOH solution followed by cooling to give green crystals: [3] 4 KMnO 4 + 4 KOH → 4 K 2 MnO 4 + O 2 + 2 H 2 O. This reaction illustrates the relatively rare role of hydroxide as a ...
The purplish-black color of solid potassium permanganate, and the intensely pink to purple color of its solutions, is caused by its permanganate anion, which gets its color from a strong charge-transfer absorption band caused by excitation of electrons from oxo ligand orbitals to empty orbitals of the manganese(VII) center.
Potassium permanganate (KMnO 4) is a dark violet colored powder. Its reaction with glycerol (commonly known as glycerin or glycerine) (C 3 H 5 (OH) 3) is highly exothermic, resulting rapidly in a flame, along with the formation of carbon dioxide and water vapour:
From the point of view of Western history of chemistry, hydrochloric acid was the last of the three well-known mineral acids for which the method of its production appeared in the literature. [20] Recipes for its production started to appear in the late sixteenth century.
Side effects may include irritation of the skin and discoloration of clothing. [2] A harsh burn on a child from an undissolved tablet has been reported. [10] For treating eczema, it is recommended using for a few days at a time due to the possibility of it irritating the skin. [10]
Hydrogen chloride can protonate molecules or ions and can also serve as an acid-catalyst for chemical reactions where anhydrous (water-free) conditions are desired. Because of its acidic nature, hydrogen chloride is a corrosive substance, particularly in the presence of moisture.
The chloralkali process has been in use since the 19th century and is a primary industry in the United States, Western Europe, and Japan. [4] [5] It has become the principal source of chlorine during the 20th century. [6]
Substance Formula 0 °C 10 °C 20 °C 30 °C 40 °C 50 °C 60 °C 70 °C 80 °C 90 °C 100 °C Barium acetate: Ba(C 2 H 3 O 2) 2: 58.8: 62: 72: 75: 78.5: 77: 75