Brpnsted-Lowry

A more general theory of acids and bases was devised independently by Johannes Br0n sted (Denmark) and Thomas M Lowry (England) m 1923 In the Brpnsted-Lowry approach an acid is a proton donor, and a base is a proton acceptor The reaction that occurs between an acid and a base is proton transfer... [Pg.33]

The acid dissociation constant has the same form m Brpnsted-Lowry as m the Arrhenius approach but is expressed m the concentration of H30" rather than The concentration terms [H30" ] and [H" ] are considered equivalent quantities m equilibrium constant expressions... [Pg.35]

Analyzing acid-base reactions according to the Brpnsted-Lowry picture provides yet another benefit Table 1 7 which lists acids according to their strength m descending... [Pg.44]

The same G N Lewis who gave us electron dot formulas also suggested a way of think mg about acids and bases that is more general than the Brpnsted-Lowry approach Where Brpnsted and Lowry viewed acids and bases as donors and acceptors of protons (positively charged) Lewis took the opposite view and focused on electron pairs (negatively charged) According to Lewis an acid is an electron pair acceptor and a base is an electron pair donor... [Pg.45]

This chapter sets the stage for all of the others by reminding us that the relationship between structure and properties is what chemistry is all about It begins with a review of Lewis structures moves to a discussion of the Arrhenius Brpnsted-Lowry and Lewis pictures of acids and bases and the effects of structure on acidity and basicity... [Pg.47]

Section 1 13 According to the Brpnsted-Lowry definitions an acid is a proton donor and a base is a proton acceptor... [Pg.49]

Basicity constants are not necessary in the Brpnsted-Lowry approach Basicity is measured according to the pA of the conjugate acid The weaker the conjugate acid the stronger the base... [Pg.50]

This IS a very useful relationship You should practice writing equations according to the Brpnsted-Lowry definitions of acids and bases and familiarize yourself with Table 1 7 which gives the s of various Br0n sted acids... [Pg.50]

Base According to the Arrhenius definition (Section 1 12) a substance that ionizes in water to produce hydroxide ions According to the Brpnsted-Lowry definition (Section 1 13) a substance that accepts a proton from some suitable donor According to the Lewis definition (Section 1 17) an electron pair donor... [Pg.1277]

A Br0nsted-Lowry base is to a hydrogen-ion acceptor as a Brpnsted-Lowry acid is to —... [Pg.37]

According to Brpnsted-Lowry theory, a water molecule can accept a proton, thereby becoming a hydronium ion. In this case, water is acting as a base (proton acceptor). [Pg.394]

When water acts as a Brpnsted-Lowry acid, it donates a proton to another species, thereby converting to the hydroxide ion. [Pg.394]

At the microscopic level, the Arrhenius theory defines acids as substances which, when dissolved in water, yield the hydronium ion (H30+) or H+(aq). Bases are defined as substances which, when dissolved in water, yield the hydroxide ion (OH). Acids and bases may be strong (as in strong electrolytes), dissociating completely in water, or weak (as in weak electrolytes), partially dissociating in water. (We will see the more useful Brpnsted-Lowry definitions of acids and bases in Chapter 15.) Strong acids include ... [Pg.54]

The hydrogen ion accepts the lone pair of electrons from the ammonia to form the ammonium ion. The hydrogen ion, because it accepts a pair of electrons, is the Lewis acid. The ammonia, because it donates a pair of electrons, is the Lewis base. This reaction is also a Brpnsted-Lowry acid-base reaction. This illustrates that a substance may be an acid or a base by more than one definition. All Brpnsted-Lowry acids are Lewis acids, and all Brpnsted-Lowry bases are Lewis bases. However, the reverse is not necessarily true. [Pg.227]

All Brpnsted-Lowry and Arrhenius acids contain hydrogen. The formation or transfer of hydrogen ions is the key to the behavior of all acids. You may wish to review the behavior of acids in Chapters 4 and 15. [Pg.282]

Comparar entre los modelos de acidos y bases de Arrhenius y Brpnsted-Lowry. [Pg.49]

Cuando un actdo de Brpnsted-Lowry dona un ton htdrogeno, se forma una base conjugada. Cuando una base de Brpnsted-Lowry acepta un ton htdrogeno, se forma un actdo conjugado. [Pg.51]

What is the value of when water acts as a Brpnsted-Lowry acid Write the expression for if water acts as a diprotic acid. [Pg.403]

A particularly important concept in chemistry is that associated with proton loss and gain, i.e. acidity and basicity. Acids produce positively charged hydrogen ions H+ (protons) in aqueous solution the more acidic a compound is, the greater the concentration of protons it produces. In water, protons do not have an independent existence, but become strongly attached to a water molecule to give the stable hydronium ion H3O+. In the Brpnsted-Lowry definition ... [Pg.121]

The carboxylic acids, like all Brpnsted-Lowry acids, can lose a hydrogen ion. The result is a carboxylate ion, shown in Figure 9-4. [Pg.125]

Method 2 Brpnsted-LoWri tackles bases u/ithout a ht dromde ion... [Pg.225]

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]

The Brpnsted-Lowry definition does not require that H30+ be formed. This definition can therefore be extended to nonaqueous solvents and even to the gas phase ... [Pg.105]

Brpnsted-Lowry acids are proton donors, and Br0nsted-Lowry bases are proton acceptors. An acid increases the concentration of H,0+ in aqueous solution, and a base increases the concentration of OH. An acid-base pair related through the gain or loss of a single proton is described as conjugate. When a proton is transferred... [Pg.116]

Distinguish Lewis acids and bases from Brpnsted-Lowry acids and bases. Give an example of each. [Pg.119]

Identify the Brpnsted-Lowry acids among the reactants in the following reactions ... [Pg.119]

Brpnsted-Lowry acid A proton (hydrogen ion) donor. [Pg.687]

Brpnsted-Lowry definition does not differ appreciably from the Arrhenius definition of hydrogen ions (acids) and hydroxide ions (bases) ... [Pg.705]

In the Brpnsted-Lowry view, an acid doesn t dissociate in water it transfers a proton to water. Water acts as a base. [Pg.41]

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