Acids proton donors and

On the Brpnsted theory (p. 51), solutions with concentrations of H3O+ greater than that in pure water are acids (proton donors), and solutions rich in OH are bases (proton acceptors). The same classifications follow from the solvent-system theory of acids and bases... 

C) The Bronsted-Lowry or proton theory interprets the acid-base reaction as a mere proton exchange between the acid (proton donor) and the base (proton acceptor) however, the Lewis theory or electron theory interprets the reaction as a donation and acceptance of a lone pair of electrons, where the... 

The acids (proton donors) and bases (proton acceptors) are labeled below their formulas. Remember that a proton, in Bransted-Lowry acid-base theory, is H+. 

The Robinson annulation of ethyl acetoacetate and tra i -chalcone was investigated with pulverized NaOH in [BMIMjPFg as the base catalyst at 100°C 110). The mixture was neutralized before extraction with toluene. The product, 6-ethoxycarbonyl-3,5-diphenyl-2-cyclohexenone, was obtained by purification in a silica gel chromatography column. A yield of 48% was obtained (Scheme 7). The ionic liquid could be recycled and reused with no diminution of product yield. The C2 position in imidazolium cations is an acidic proton donor and may have reacted... 

This reaction is a proton transfer from HC1 to the C=0 group of acetaldehyde. Therefore, it is a Br0nsted-Lowry acid-base reaction, with HC1 acting as the acid (proton donor) and acetaldehyde acting as the base (proton acceptor). Before drawing any curved... 

Thus, water acts as an acid (proton donor) and a base (proton acceptor) in what is called the autoionization of water. The autoionization of water can be simplified as follows ... 

Many features of acid sites in solids closely parallel those in solution. Materials that are Bronsted acids (proton donors) and Lewis acids (electron acceptors) are known. Typically, Bronsted acid sites in mixed metal oxides occur where the oxygen atoms of a hydroxyl attached to a metal atom of one kind are coordinating (acting as a Lewis base) to atoms of a different kind, resulting in the proton becoming more acidic (Scheme 8.5). Lewis acid sites are usually associated with incompletely coordinated cations that can accept electrons. The criteria for solid acidity are widely met by mixed metal oxides and oxo-salts, the varied chemistry of which gives rise to solids with acidities up to that of concentrated sulfuric acid and, in some cases, beyond. 

Acid catalysis finds very wide industrial application in refinery operations and chemicals production. Both Bronsted acids (proton donors) and Lewis acids... 

Alcohols can function as both weak acids (proton donors) and weak bases (proton acceptors). Table 10.2 lists the acid ionization constants for several low-molecular-weight alcohols. 

The substance that donates the proton is the acid (proton donor) and becomes the conjugate base (as a product). The substance that accepts the proton (proton acceptor) is the base and becomes the conjugate acid (as a product). 

The HNO3 molecule is an acid (proton donor) and H2O is a base (proton acceptor). Note that H2O may function as an acid or a base, depending on the other reactant. 

Studies of chemical attack on nitrile rubber by fluids encountered in sealing applications in the oil industry are reported. The results showed that excessive hardening of nitrile rubber in the downhole oilfield environment occurs at the acrylonitrile sites, and that it could be due to either hydrolysis or reduction of the cyano group. Hydrolysis is driven by Bronsted acids (proton donors) and reduction by Lewis acids (electron donors). Catalysis by metal ions could possibly cause these reactions to occur at a greatly reduced activation energy. Oxidative attack at the butadiene sites is the primary cause of hardening in aboveground applications of nitrile rubber. 12 refs. 

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