Silicon dioxide (SiO 2) and sodium hydroxide (NaOH) mounted on alumina are examples of solid bases. Solid base: A solid base acts as a base in solid form.The acid and base share an electron pair. Neutral base: A neutral base forms a bond with a neutral acid.The strongest superbase is the ortho-diethynylbenzene dianion (C 6H 4(C 2) 2) 2. A simple example of a superbase is sodium hydride (NaH). Superbases don’t remain in aqueous solution because they are stronger bases than the hydroxide ion. They form by mixing an alkali metal (e.g., lithium, sodium) with its conjugate acid. Superbases have very weak conjugate acids. Superbase: A superbase is a Lewis base that deprotonates even better than a strong base.Other types of bases include superbases, neutral bases, and solid bases. Weak bases include the conjugate bases of acids and many other compounds, often containing hydrogen or nitrogen. Common Strong BaseĬalcium hydroxide, strontium hydroxide, and barium hydroxide only fully dissociate in solutions with concentration values of 0.01M or lower. The strong bases are classic Arrhenius bases made from alkali or alkaline earth metals and hydroxide ions. Weak base: B + H 2O ↔ BH +(aq) + OH –(aq) Weak base: BOH + H 2O ↔ B +(aq) + OH –(aq) Strong base: BOH + H 2O → B +(aq) + OH –(aq) A weak base incompletely dissociates into its ions, so that the resulting aqueous solution contains weak base, its conjugate acid, and water. Strong and Weak BasesĪ strong base is a compound that fully dissociates into its ions in aqueous solution. Water is a classic example, as it can act as a weak acid (donating a hydrogen ion or proton) or weak acid (donate OH – or accepting a proton to form H 3O +). An Arrhenius acid is an electron pair acceptor.Īcids and bases may seem like opposite species in chemical reactions, but some substances can act as either an acid or a base.
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