Base (chemistry)

Acids and bases
Acceptor number Acid Acid–base reaction Acid–base homeostasis Acid strength Acidity function Amphoterism Base Buffer solutions Dissociation constant Donor number Equilibrium chemistry Extraction Hammett acidity function pH Proton affinity Self-ionization of water Titration Lewis acid catalysis Frustrated Lewis pair Chiral Lewis acid
Acid types
Brønsted–Lowry Lewis Mineral Organic Oxide Strong Superacids Weak Solid
Base types
Brønsted–Lowry Lewis Organic Oxide Strong Superbases Non-nucleophilic Weak
v t e

In

In the more general Brønsted–Lowry acid–base theory (1923), a base is a substance that can accept hydrogen cations (H⁺)—otherwise known as protons. This does include aqueous hydroxides since OH⁻ does react with H⁺ to form water, so that Arrhenius bases are a subset of Brønsted bases. However, there are also other Brønsted bases which accept protons, such as aqueous solutions of ammonia (NH₃) or its organic derivatives (amines).^[2] These bases do not contain a hydroxide ion but nevertheless react with water, resulting in an increase in the concentration of hydroxide ion.^[3] Also, some non-aqueous solvents contain Brønsted bases which react with solvated protons. For example in liquid ammonia, NH₂⁻ is the basic ion species which accepts protons from NH₄⁺, the acidic species in this solvent.

Some other definitions of both bases and acids have been proposed in the past, but are not commonly used today.

Properties

General properties of bases include:

• Concentrated or strong bases are
  caustic
  on organic matter and react violently with acidic substances.
• Aqueous solutions
  or molten bases dissociate in ions and conduct electricity.
• Reactions with indicators: bases turn red litmus paper blue, phenolphthalein pink, keep bromothymol blue in its natural colour of blue, and turn methyl orange-yellow.
• The pH of a basic solution at standard conditions is greater than seven.
• Bases are bitter.^[5]

Reactions between bases and water

The following reaction represents the general reaction between a base (B) and water to produce a conjugate acid (BH⁺) and a conjugate base (OH⁻):^[3]

$${\displaystyle {\ce {{B}_{(aq)}+ {H2O}_{(l)}<=> {BH+}_{(aq)}+ {OH- }_{(aq)}}}}$$

${\displaystyle K_{b}={\frac {[BH^{+}][OH^{-}]}{[B]}}}$

In this equation, the base (B) and the extremely

Bases react with acids to neutralize each other at a fast rate both in water and in alcohol.[7] When dissolved in water, the strong base sodium hydroxide ionizes into hydroxide and sodium ions:

${\displaystyle {\ce {NaOH -> Na+ + OH-}}}$

and similarly, in water the acid hydrogen chloride forms hydronium and chloride ions:

${\displaystyle {\ce {HCl + H2O -> H3O+ + Cl-}}}$

When the two solutions are mixed, the H
₃O⁺
and OH⁻
ions combine to form water molecules:

${\displaystyle {\ce {H3O+ + OH- -> 2H2O}}}$

If equal quantities of NaOH and HCl are dissolved, the base and the acid neutralize exactly, leaving only NaCl, effectively

Weak bases, such as baking soda or egg white, should be used to neutralize any acid spills. Neutralizing acid spills with strong bases, such as sodium hydroxide or potassium hydroxide, can cause a violent exothermic reaction, and the base itself can cause just as much damage as the original acid spill.

Alkalinity of non-hydroxides

Bases are generally compounds that can neutralize an amount of acid. Both sodium carbonate and ammonia are bases, although neither of these substances contains OH⁻
groups. Both compounds accept H⁺ when dissolved in protic solvents such as water:

${\displaystyle {\ce {Na2CO3 + H2O -> 2Na+ + HCO3- + OH-}}}$

${\displaystyle {\ce {NH3 + H2O -> NH4+ + OH-}}}$

From this, a pH, or acidity, can be calculated for aqueous solutions of bases.

A base is also defined as a molecule that has the ability to accept an electron pair bond by entering another atom's valence shell through its possession of one electron pair.^[7] There are a limited number of elements that have atoms with the ability to provide a molecule with basic properties.^[7] Carbon can act as a base as well as nitrogen and oxygen. Fluorine and sometimes rare gases possess this ability as well.^[7] This occurs typically in compounds such as butyl lithium, alkoxides, and metal amides such as sodium amide. Bases of carbon, nitrogen and oxygen without resonance stabilization are usually very strong, or superbases, which cannot exist in a water solution due to the acidity of water. Resonance stabilization, however, enables weaker bases such as carboxylates; for example, sodium acetate is a weak base.

Strong bases

A strong base is a basic chemical compound that can remove a proton (H⁺) from (or

One advantage of this low solubility is that "many antacids were suspensions of metal hydroxides such as aluminium hydroxide and magnesium hydroxide";[9] compounds with low solubility and the ability to stop an increase in the concentration of the hydroxide ion, preventing the harm of the tissues in the mouth, oesophagus, and stomach.^[9] As the reaction continues and the salts dissolve, the stomach acid reacts with the hydroxide produced by the suspensions.^[9]

Strong bases hydrolyze in water almost completely, resulting in the leveling effect."^[7] In this process, the water molecule combines with a strong base, due to the water's amphoteric ability; and, a hydroxide ion is released.^[7] Very strong bases can even deprotonate very weakly acidic C–H groups in the absence of water. Here is a list of several strong bases:

The cations of these strong bases appear in the first and second groups of the periodic table (alkali and earth alkali metals). Tetraalkylated ammonium hydroxides are also strong bases since they dissociate completely in water. Guanidine is a special case of a species that is exceptionally stable when protonated, analogously to the reason that makes perchloric acid and sulfuric acid very strong acids.

Acids with a pK_a of more than about 13 are considered very weak, and their

Superbases

Group 1 salts of

• Butyl lithium (n-C₄H₉Li)
• Lithium diisopropylamide (LDA) [(CH₃)₂CH]₂NLi
• Lithium diethylamide (LDEA) (C
  ₂H
  ₅)
  ₂NLi
• Sodium amide (NaNH₂)
• Sodium hydride (NaH)
• Lithium bis(trimethylsilyl)amide [(CH
  ₃)
  ₃Si]
  ₂NLi

Strongest superbases are synthesised in only gas phase:

• Ortho-diethynylbenzene dianion
  (C₆H₄(C₂)₂)²⁻ (the strongest superbase ever synthesized)
• Meta-diethynylbenzene dianion
  (C₆H₄(C₂)₂)²⁻ (second strongest superbase)
• Para-diethynylbenzene dianion
  (C₆H₄(C₂)₂)²⁻ (third strongest superbase)
• Lithium monoxide anion (LiO⁻) was considered the strongest superbase before diethynylbenzene dianions were created.

Weak bases

A weak base is one which does not fully ionize in an aqueous solution, or in which protonation is incomplete. For example, ammonia transfers a proton to water according to the equation^[11]

NH₃(aq) + H₂O(l) → NH⁺
₄(aq) + OH^-(aq)

The equilibrium constant for this reaction at 25 °C is 1.8 x 10⁻⁵,^[12] such that the extent of reaction or degree of ionization is quite small.

Lewis bases

A Lewis base or electron-pair donor is a molecule with one or more high-energy lone pairs of electrons which can be shared with a low-energy vacant orbital in an acceptor molecule to form an adduct. In addition to H⁺, possible electron-pair acceptors (Lewis acids) include neutral molecules such as BF₃ and high oxidation state metal ions such as Ag²⁺, Fe³⁺ and Mn⁷⁺. Adducts involving metal ions are usually described as coordination complexes.^[13]

According to the original formulation of Lewis, when a neutral base forms a bond with a neutral acid, a condition of electric stress occurs.^[7] The acid and the base share the electron pair that formerly belonged to the base.^[7] As a result, a high dipole moment is created, which can only be decreased to zero by rearranging the molecules.^[7]

Solid bases

Examples of solid bases include:

• Oxide mixtures: SiO₂, Al₂O₃; MgO, SiO₂; CaO, SiO₂^[14]
• Mounted bases: LiCO₃ on silica; NR₃, NH₃, KNH₂ on alumina; NaOH, KOH mounted on silica on alumina^[14]
• Inorganic chemicals: BaO, KNaCO₃, BeO, MgO, CaO, KCN^[14]
• Anion exchange resins^[14]
• Charcoal that has been treated at 900 degrees Celsius or activates with N₂O, NH₃, ZnCl₂-NH₄Cl-CO₂^[14]

Depending on a solid surface's ability to successfully form a conjugate base by absorbing an electrically neutral acid, basic strength of the surface is determined.^[15] The "number of basic sites per unit surface area of the solid" is used to express how much basic strength is found on a solid base catalyst.^[15] Scientists have developed two methods to measure the amount of basic sites: one, titration with benzoic acid using indicators and gaseous acid adsorption.^[15] A solid with enough basic strength will absorb an electrically neutral acidic indicator and cause the acidic indicator's color to change to the color of its conjugate base.^[15] When performing the gaseous acid adsorption method, nitric oxide is used.^[15] The basic sites are then determined by calculating the amount of carbon dioxide that is absorbed.^[15]

Bases as catalysts

Basic substances can be used as

• Sodium hydroxide is used in the manufacture of soap, paper, and the synthetic fiber rayon.
• Calcium hydroxide (slaked lime) is used in the manufacture of bleaching powder.
• Calcium hydroxide is also used to clean the sulfur dioxide, which is caused by the exhaust, that is found in power plants and factories.^[9]
• Magnesium hydroxide is used as an 'antacid' to neutralize excess acid in the stomach and cure indigestion.
• Sodium carbonate is used as washing soda and for softening hard water.
• Sodium bicarbonate (or sodium hydrogen carbonate) is used as baking soda in cooking food, for making baking powders, as an antacid to cure indigestion and in soda acid fire extinguisher.
• Ammonium hydroxide
  is used to remove grease stains from clothes

Monoprotic and polyprotic bases

Bases with only one

When one molecule of a base via complete ionization produces one hydroxide ion, the base is said to be a monoacidic or monoprotic base. Examples of monoacidic bases are:

Diacidic bases

When one molecule of base via complete ionization produces two hydroxide ions, the base is said to be diacidic or diprotic. Examples of diacidic bases are:

Barium hydroxide, magnesium hydroxide, calcium hydroxide, zinc hydroxide, iron(II) hydroxide, tin(II) hydroxide, lead(II) hydroxide, copper(II) hydroxide, etc.

Triacidic bases

When one molecule of base via complete ionization produces three hydroxide ions, the base is said to be triacidic or triprotic. Examples of triacidic bases are:

The concept of base stems from an older alchemical notion of "the matrix":

The term "base" appears to have been first used in 1717 by the French chemist, Louis Lémery, as a synonym for the older Paracelsian term "matrix." In keeping with 16th-century animism, Paracelsus had postulated that naturally occurring salts grew within the earth as a result of a universal acid or seminal principle having impregnated an earthy matrix or womb. ... Its modern meaning and general introduction into the chemical vocabulary, however, is usually attributed to the French chemist, Guillaume-François Rouelle. ... In 1754 Rouelle explicitly defined a neutral salt as the product formed by the union of an acid with any substance, be it a water-soluble alkali, a volatile alkali, an absorbent earth, a metal, or an oil, capable of serving as "a base" for the salt "by giving it a concrete or solid form." Most acids known in the 18th century were volatile liquids or "spirits" capable of distillation, whereas salts, by their very nature, were crystalline solids. Hence it was the substance that neutralized the acid which supposedly destroyed the volatility or spirit of the acid and which imparted the property of solidity (i.e., gave a concrete base) to the resulting salt.

— William B. Jensen, The origin of the term "base"^[19]

See also

• Acid–base reactions
• Acids
• Base-richness (used in ecology, referring to environments)
• Conjugate base
• Lewis acids and bases
• Titration

References