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Line 1: {{More sources\|date=May 2020}} The '''alkali hydroxides''' are a class of [[chemical compound]]s which are composed of an [[alkali metal]] [[cation]] and the [[hydroxide]] anion (~~HO<sup>−</sup>~~{{chem2\|OH−}}). The alkali hydroxides are: [[Lithium hydroxide]] (LiOH) [[Sodium hydroxide]] (NaOH) Line 5 ⟶ 6: [[Rubidium hydroxide]] (RbOH) [[Caesium hydroxide]] (CsOH) [[Francium hydroxide]] (FrOH) == Production == "A strong base completely ionizes in aqueous solution to give HO<sup>−</sup> and a cation. Sodium hydroxide is an example of a strong base. The principal strong bases are the hydroxides of Group IA elements and group IIA elements."<ref>Ebbing, Darrell D & Gammon, Steven D. General Chemistry (Eighth Edition). Page 661. ISBN 0-618-39941-0</ref> Alkali hydroxides are formed in the reaction between alkali metals and water. A typical school demonstration demonstrates what happens when a piece of an alkali metal is introduced to a bowl of water. A vigorous reaction occurs, producing [[hydrogen]] gas and the specific alkali hydroxide. For example, if sodium is the alkali metal:▼ :~~Sodium~~{{chem2\|2 [[sodium\|Na]] + 2 [[water\|H2O]] → 2 [[sodium hydroxide\|NaOH]] + [[hydrogen ~~gas~~\|H2]]}}▼ The most common alkali hydroxide is sodium hydroxide, which is readily available in most hardware stores in products such as a [[drain cleaner]]. Another common alkali hydroxide is potassium hydroxide. This is available as a solution used for cleaning terraces and other areas made out of wood. [[Sodium hydroxide]] is an important industrial chemical, where it is produced by the [[chloralkali process]]. ~~All alkali hydroxides are very corrosive, being strongly [[alkaline]].~~ == Properties and uses == ▲A typical school demonstration demonstrates what happens when a piece of an alkali metal is introduced to a bowl of water. A vigorous reaction occurs, producing [[hydrogen]] gas and the specific alkali hydroxide. For example, if sodium is the alkali metal: The alkali metal hydroxides form white crystals that are [[hygroscopic]] and readily soluble in water, generating large amounts of heat upon dissolution. The solubility increases down the column as the alkali metal ions become larger and the lattice enthalpies decrease.<ref>{{cite journal\|title=Solubility of Alkali Metal Chlorides and Hydroxides in Water\|journal=Fiber Chemistry\|volume=25\|issue=6\|date=1993\|last=Skolunov\|first=A. V.\|doi=10.1007/BF00550787}}</ref> All alkali metal hydroxides are [[strong base]]s, meaning that they dissociate completely in solution to give {{chem2\|OH−}} ions. As strong bases, alkali hydroxides are highly corrosive and are used in [[cleaning product]]s. Sodium hydroxide is readily available in most hardware stores in products such as a [[drain cleaner]]. Similarly, potassium hydroxide is available as a solution used for cleaning terraces and other areas made out of wood. Both NaOH and KOH are also used in the production of soap and detergents ([[saponification]]). ▲:Sodium + water → sodium hydroxide + hydrogen gas ~~:2 Na + 2 H<sub>2</sub>O → 2 NaOH + H<sub>2</sub>~~ Due to their hygroscopic properties, alkali hydroxides are used as [[desiccant]]s. They also readily absorb carbon dioxide and are therefore used in [[carbon dioxide scrubber]]s.<ref>{{cite book\|last=Breuer\|first=D.\|last2=Heinrich\|first2=B.\|title=The MAK‐Collection for Occupational Health and Safety: Annual Thresholds and Classifications for the Workplace\|chapter=hydroxide, sodium hydroxide, potassium hydroxide, calcium hydroxide) [Air Monitoring Methods, 2003]\|date=2003\|doi=10.1002/3527600418.am131065e0008}}</ref> == Notes ==▼ ▲== ~~Notes~~See also == [[Hydroperoxide]], a peroxide analog of hydroxide [[Hydrosulfide]], a sulfur analog of hydroxide [[Sodium hydroselenide\|Hydroselenide]], a selenium analog of hydroxide [[Azanide]], a nitrogen analog of hydroxide [[Phosphanide]], a phosphorus analog of hydroxide and azanide *[[Arsanide]], an arsenic analog of hydroxide and azanide == References == {{reflist}} [[Category:Hydroxides]] [[Category:Alkali metals]]