- Brønsted–Lowry acid-base theory
In
chemistry , the Brønsted–Lowry acid-base theory is an acid-base theory. It was proposed independently byJohannes Nicolaus Brønsted andThomas Martin Lowry in 1923. In this system, anacid is defined as any chemical species (molecule or ion) that is able to lose, or "donate" ahydrogen ion (proton ), and a base is a species with the ability to gain or "accept" a hydrogen ion (proton). It follows that if a compound is to behave as an acid, donating a proton, there must be a base to accept the proton. So the Brønsted–Lowry concept can be defined by the reaction:acid + base conjugate base + conjugate acid.The conjugate base is the ion or molecule remaining after the acid has lost a proton, and the conjugate acid is the species created when the base accepts the proton. The reaction can proceed in either forward or backward direction; in each case the acid donates a proton to the base.Water is
amphoteric and can act as an acid or as a base. In the reaction betweenacetic acid , CH3CO2H, and water, H2O, water acts as a base.:CH3CO2H + H2O CH3CO2- + H3O+Theacetate ion, CH3CO2-, is the conjugate base of acetic acid and thehydronium ion , H3O+, is the conjugate acid of the base, water.Water can also act as an acid, for instance when it reacts with ammonia. The equation given for this reaction is::H2O + NH3 OH- + NH4+in which H2O donates a proton to NH3. The
hydroxide ion is the conjugate base of water acting as an acid.A strong acid, such as hydrochloric acid, dissociates completely. A weak acid, such as acetic acid, may be partially dissociated; the
acid dissociation constant , p"K"a, is a quantitative measure of the strength of the acid.A wide range of compounds can be classified in the Brønsted–Lowry framework:
mineral acid s and derivatives such assulfonate s,phosphonate s, etc.,carboxylic acid s,amine s,carbon acid s, 1,3-diketone s such asacetylacetone ,ethyl acetoacetate orMeldrum's acid and many more.A
Lewis base , defined as an electron-pair donor, can act as a Brønsted–Lowry base as the pair of electrons can be donated to a proton. This means that the Brønsted–Lowry concept is not limited to aqueous solutions. Any donor solvent, S, can act as a proton acceptor.:AH + S: A- + SH+Typical donor solvents used in acid-base chemistry, such asdimethyl sulphoxide or liquidammonia have an oxygen or nitrogen atom with a lone pair of electrons that can used to form a bond with a proton.Brønsted acidity of some Lewis acids
Some
Lewis acid s, defined as electron-pair acceptors, also act as Brønsted–Lowry acids. For example, the aluminium ion, Al3+ can accept electron pairs from water molecules, as in the reaction:Al3+ + 6H2O → Al(H2O)63+The aqua ion formed is a weak Brønsted–Lowry acid.:Al(H3O)62+ + H2O Al(H2O)5OH2+ + H3O+ .....Ka = 1.7 x 10-5The overall reaction is described as acid hydrolysis of the aluminium ion.However not all
Lewis acid s generate Brønsted–Lowry acidity. The magnesium ion similarly reacts as a Lewis acid with six water molecules:Mg2+ + 6H2O → Mg(H2O)62+but here no protons are exchanged since the Brønsted–Lowry acidity of the aqua ion is negligible (Ka ~ 10-12).Boric acid also exemplifies the usefulness of the Brønsted–Lowry concept for an acid which does not dissociate, but does effectively donate a proton to the base, water. The reaction is:B(OH)3 + 2H2O B(OH)4- + H3O+Here boric acid acts as a Lewis acid and accepts an electron pair from the oxygen of one water molecule, which in turn donates a proton to a second water molecule and therefore acts as a Brønsted acid.ee also
*
Acid
*Acid-base reaction theories
*Base (chemistry)
*Lewis acid
*Lewis base
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