Acids and bases Br0nsted

Harrison [57] distinguishes Br0nsted acid and base chemical ionisation, charge exchange (CE) and electron capture chemical ionisation (ECCI). 

Because the reactions of Br0nsted acids and bases with water are equilibrium reactions, we can write equilibrium constant expressions for these ionizations or dissociations. For example, the dissociation of nitrous acid in water and its equilibrium constant expression are as follows ... 

Periodic Table Correlations. When comparing Br0nsted acids and bases that differ in the position of an element in the periodic table ... 

I See the Saunders Interactive General Chemistry CD-ROM, Screen 1 7.2, Br0nsted Acids and Bases. 

Of course, decomposition is a chemical phenomenon and depends on the nature of the ions that compose the IL. Angell et al. [9, 12] have investigated the decomposition behavior of various binary ILs that can be formed by the proton transfer that occurs between neat Br0nsted acids and bases [Eq. (2)]. 

Transesterification of triglycerides can be facilitated by both Br0nsted acid and base catalysts [204, 205]. Essential steps over each catalyst types are shown in Scheme 6.30 and Scheme 6.31, respectively. Reaction over acid catalysts first requires triglyceride adsorption, whereas the reaction over base catalysts is initiated by alcohol adsorption. Thereafter, the carbonyl moiety in the glyceride molecule is attacked to produce the alkyl esters. These steps occur consecutively to form the diglyceride and monoglyceride esters, with three molecules of fatty acid alkyl esters produced for every molecule of glycerol. 

Define Br0nsted acids and bases. Give an example of a conjugate pair in an acid-base reaction. 

Both the amide ion (NH2) and the nitride ion (N ) are strongo- bases than the hydroxide ion and hence do not exist in aqueous solutions, (a) Write equations showing the reactions of these ions with water, and identify the Br0nsted acid and base in each case, (h) Which of the two is the stronger base ... 

Following is another example of adding a proton. Here, the proton is added across the pi bond of the C — C double bond. The compounds below are labeled as proton donor and proton acceptor, terms used to describe Br0nsted acids and bases. They can also be labeled according to Lewis acid-base theory as electrophile and nucleophile. ... 

The cation and anion of a salt may have the same or different Br0nsted acid and base strengths. When they are the same, solutions of the salt have a pH of 7. When they are different, salt solutions have and OH concentrations that are unequal and pH values different than 7. The reactions of salt ions with water that cause these results are called hydrolysis reactions. 

Lewis Acids and Bases A more general definition of acids and bases characterizes an acid as a substance that can accept a pair of electrons and a base as a substance that can donate a pair of electrons. All Br0nsted acids and bases are Lewis acids and bases. 

Although in this chapter we are mainly concerned with Br0nsted acids and bases, it is important not to lose sight of the definition of Lewis acids and bases. Relevant to this chapter is the fact that water functions as a Lewis base when it acts as a solvent. 

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