![]() ![]() The known hydrates and the approximate ranges of temperature and concentration (mass percent of NaOH) of their saturated water solutions are: nH 2O, which result in a complex solubility diagram that was described in detail by Spencer Umfreville Pickering in 1893.Sodium hydroxide can form several hydrates NaOH The viscosity of sodium hydroxide solutions plays a direct role in its application as well as its storage. The viscosity of aqueous NaOH, as with any liquid chemical, is inversely related to its service temperature, i.e., its viscosity decreases as temperature increases, and vice versa. s, that is much greater than that of water (1.0 mPa.As with other alkaline solutions, it feels slippery with skin contact due to the process of saponification that occurs between NaOH and natural skin oils.Ĭoncentrated (50%) aqueous solutions of sodium hydroxide have a characteristic viscosity, 78 m Pa The resulting solution is usually colorless and odorless. Similar to the hydration of sulfuric acid, dissolution of solid sodium hydroxide in water is a highly exothermic reaction where a large amount of heat is liberated, posing a threat to safety through the possibility of splashing. ![]() ![]() Sodium hydroxide is insoluble in ether and other non-polar solvents. It is highly soluble in water, with a lower solubility in polar solvents such as ethanol and methanol. Pure sodium hydroxide is a colorless crystalline solid that melts at 318 ☌ (604 ☏) without decomposition and with a boiling point of 1,388 ☌ (2,530 ☏). ![]() Worldwide production in 2004 was approximately 60 million tons, while demand was 51 million tons. Sodium hydroxide is used in many industries: in the making of wood pulp and paper, textiles, drinking water, soaps and detergents, and as a drain opener. The commercially available "sodium hydroxide" is often this monohydrate, and published data may refer to it instead of the anhydrous compound.Īs one of the simplest hydroxides, sodium hydroxide is frequently used alongside neutral water and acidic hydrochloric acid to demonstrate the pH scale to chemistry students.
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