Bases Bronsted-Lowry base

Bronsted base (Bronsted-Lowry base) A molecular entity capable of accepting a hydron from an acid (i.e., a hydron acceptor ) or the corresponding chemical species. For example OH-, H20, CH3C02", HSO4-, SO42-, and Cl". [Pg.34]

Bronsted-Lowry base (Section 2.7) A substance that accepts H+ from an acid. [Pg.1237]

Backbone (protein), 1028 Backside displacement. reaction and.363-364 von Baeyer, Adolf, 113 Baeyer strain theory, 113-114 Bakelile, structure of, 1218 Banana, esters in, 808 Barton, Derek, H. R., 389 Basal metabolic rate, 1169 Basal metabolism. 1169-1170 Base, Bronsted-Lowry, 49 Lewis, 57, 59-60 organic, 56-57 strengths of, 50-52 Base pair (DNA), 1103-1105 electrostatic potential maps of. [Pg.1287]

Bronsted-Lowry bases (right column) can be divided similarly ... [Pg.371]

Barrier-layer cells 658 Baryta see Barium hydroxide Bases. Bronsted-Lowry theory of, 21 dissociation constants of, (T) 833 hard, 54 ionisation of, 21... [Pg.857]

Bromides, D. of as silver bromide, (g) 491 by EDTA, (ti) 339 by mercury(I), (cm) 542 by oxygen flask, 113 by silver ion, (cm) 546 by silver nitrate, (ti) 351 by Volhard s method, (ti) 356 with iodide, (ti) 352 4-Bromomandelic acid 473 Bromophenol blue 265, 267 Bromopyrogallol red 182, 319 Bronsted-Lowry bases titration with strong acids, 277... [Pg.858]

These species are Bronsted-Lowry bases in water (none are Arrhenius bases) since they are proton acceptors and OH" ions are produced NH3, HS, CH3COO and O2. ... [Pg.148]

Bronsted-Lowry bases NH3, H20 and H in ionic NaH Bronsted-Lowry acids H20, HF... [Pg.150]

Proton acceptor (Bronsted-Lowry base) example amine... [Pg.1]

A base is a substance that can accept a proton. (Some chemists describe Bronsted-Lowry bases as proton-acceptors. )... [Pg.380]

Table 8.3 lists the base dissociation constants for several weak bases at 25°C. Nitrogen-containing compounds are Bronsted-Lowry bases, because the lone pair of electrons on a nitrogen atom can bond with H+ from water. The steps for solving problems that involve weak bases are similar to the steps you learned for solving problems that involve weak acids. [Pg.404]

Amines cire both Bronsted-Lowry bases (they accept hydrogen ions from acids) and Lewis bases (they furnish an electron pair to Lewis acids). As Bronsted-Lowry bases they have values. Aliphatic amines have values of approximately 1(H, and aromatic amines have values near 10 °. (These values compare to a value of =10" for ammonia.)... [Pg.226]

Primary, secondary, and tertiary amines behave as Bronsted-Lowry bases. These amines react like ammonia, adding H to produce an ammonium ion. [Pg.233]

Generalizing from the data, one notes the following not unexpected results about 10% of the course is devoted to the introductory concepts of stoichiometry and chemical equations more than 20% of the course is devoted to the study of structure of matter and chemical bonding acids and bases (Bronsted-Lowry) and equilibrium are the most extensively covered topics among the remaining content areas. [Pg.140]

In this reaction, hydrochloric acid (HCl) donates a proton to water (H2O), making it the Brpnsted-Lowry acid. Water, which accepts the proton, is the Bronsted-Lowry base. This makes hydronium (H3O+) the conjugate acid and chloride (Cl ) the conjugate base. Water can act as the base in this reaction and as an acid in the example problem because it s composed of both a hydrogen ion and a hydroxide ion therefore, it can either accept or donate a proton. [Pg.233]

Brensted-Lowry acid proton donor Bronsted-Lowry base proton acceptor J. N. Bronsted of the University of Copenhagen published his definition of acids and bases in 1923. [Pg.105]

Bronsted-Lowry base A substance that can accept H+... [Pg.612]

When a Bronsted-Lowry base such as NH3 dissolves in water, it accepts a proton from the solvent, which acts as an acid. The products are the hydroxide ion, OH (the conjugate base of water), and the ammonium ion, NH4+ (the conjugate acid of NH3). In the reverse reaction, NH4+ acts as the proton donor, and OH-acts as the proton acceptor ... [Pg.613]

For a molecule or ion to accept a proton, it must have at least one unshared pair of electrons that it can use for bonding to the proton. As shown by the following electron-dot structures, all Bronsted-Lowry bases have one or more lone pairs of electrons ... [Pg.613]

PROBLEM 15.2 What is the conjugate acid of each of the following Bronsted-Lowry bases ... [Pg.614]

Give three examples of molecules or ions that are Bronsted-Lowry bases but not Arrhenius bases. [Pg.656]

Because ammonia is a Bronsted-Lowry base (Section 15.1), its aqueous solutions are weakly alkaline ... [Pg.835]

The theory explains why a pure acid behaves differentiy from its aqueous solution, since for an acid to behave as an H+ ion donor it must have another substance present to accept the H+ ion. So the water, in the aqueous acid solution, is behaving as a Bronsted-Lowry base and accepting an H+ ion. Generally ... [Pg.130]

The amide anion functions as a Bronsted-Lowry base. It accepts a proton from a terminal acetylene, which functions as a Bronsted-Lowry acid. [Pg.128]

According to the Lewis definition, an acid is an electron pair acceptor and a base is an electron pair donor. All Bronsted-Lowry bases are also Lewis bases. However, Lewis acids include many species that are not proton acids instead of H+, they have some other electron-deficient species that acts as the electron pair acceptor. An example of a Lewis acid-base reaction is provided by the following equation. In this reaction the boron of BF3 is electron/deficient (it has only six electrons in its valence shell). The oxygen of the ether is a Lewis base and uses a pair of electrons to form a bond to the boron, thus completing boron s octet. [Pg.106]

A Bronsted-Lowry base is a substance that accepts a proton from another substance. This is a significant change from the Arrhenius definition. Arrhenius bases possess an OH, whereas Bronsted-Lowry bases need not. In the example below, notice how ammonia increases the concentration of hydroxide ion in the resulting solution without donating a OH- ion. It does so by accepting a proton from water ... [Pg.316]

One very important thing to remember is that an acid and base are always present in these reactions. In order for a molecule or ion to donate a proton, there has to be another ion or molecule to receive it. In addition, in reversible acid-base reactions, the roles of the substances as proton donor or acceptor will switch in the reverse reaction. In the example below, note how water (a Bronsted-Lowry base in this reaction) accepts a proton to form a hydronium ion in the forward reaction. In the reverse reaction, the hydronium ion (Bronsted-Lowry acid) donates a proton and, after losing the proton, becomes the water molecule once again ... [Pg.317]

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