Benzoate anion

Electrostatic potential map for benzoate anion shows most negatively-charged regions (in red) and less negatively-charged regions (in blue). 

The equilibrium constant for the proton transfer reaction of benzoic acid, determined in Example, is 6.4 X 10. Calculate the equilibrium concentration of benzoic acid and benzoate anions in a 5.0 X 10 M aqueous solution of the acid. 

Completing the table requires an appropriate unknown. If we let x represent the change in concentration of H3 O during the reaction, the changes in the other concentrations are -X for benzoic acid and +X for benzoate anion. Then we apply Equation to each column and complete the table ... 

Sodium benzoate is a common food preservative. This salt dissolves in water to produce benzoate anions, which accept protons from water ... 

Under initial conditions, three chemical species are present benzoate anions, Na , and H2 O. 

The net reaction is given. A proton is transferred from a water molecule to a benzoate anion. A small amount of benzoic acid forms as the reaction reaches equilibrium. Notice that Na ions do not participate in the net reaction. 

The isolated double bonds in the dihydro product are much less easily reduced than the conjugated ring, so the reduction stops at the dihydro stage. Alkyl and alkoxy aromatics, phenols, and benzoate anions are the most useful reactants for Birch reduction. In aromatic ketones and nitro compounds, the substituents are reduced in preference to the Dissoiving-Memi... 

Scheme 3.37 describes gas-phase generation of m-benzyne anion (the distonic anion-biradical) from m-bis(trimethylsilyl) benzene (Wenthold et al. 1994, 1996 Wenthold and Squires 1998). The same anion-biradical is formed from isophthalic acid under the same conditions (Reed et al. 2000). Particularly, the reaction of m-bis(trimethylsilyl) benzene with fluoride ion, followed by treatment of the formed trimethylsilyl phenyl anion with fluorine in helium, produces the anion-biradical mentioned. The latter is transformed into the corresponding nitro benzoate anion through the addition of CO2 and NO2 (Scheme 3.37). 

A para-substituent may stabilize mesomerically either the conjugate acid of an acid-base pair rather more than it stabilizes benzoic acid, or it may stabilize the conjugate base rather more than it stabilizes the benzoate anion. The first situation is found in car-boxonium ions [13], where the delocalization of the positive charge on to a mesomerically electron-donating substituent stabilizes the cation. A similar resonance in the benzoic acid molecule [14] involves a separation of charge and affects the binding of the proton... 

Conversely, if a. para substituent stabilizes the conjugate base of an acid-base pair rather more than it stabilizes the benzoate ion, more positive substituent constants are required to achieve linearity in Hammett plots. Examples of this are acid dissociations of phenols and anilinium ions, where mesomerically electron-withdrawing substituents (Y = —NO2, —C N) are more effective in enhancing acid strength than they are in benzoic acid, because charge delocalization of the type [15] is not possible in the benzoate anion. 

Taste. Of the fundamental tastes, bitter is unique in showing human genetic differences in sensitivity. Six decades ago, it was reported tiiat phenylthiocarbamide (PTC) tasted extremely bitter to some individuals while being almost tasteless to others (45). Tlie ability to taste PTC was found to be a dominant genetic trait which occurs across gender, age and culture, with 70% of the American pulation carrying the dominant trait (46). Sensitivity to PTC and propylthiouracil (PROP) are correlated with sensitivities to otiier bitter tasting compounds, such as caffeine, saccharin (after-taste) and salts of i tassium cations and benzoate anions (47,48,49 0). However, in a reexamination of the sensitivity to NaQ and KQ, no differences were found between tasters and nontasters to non-PTC type compounds, and the statistical methods that showed differences were questioned (51). Individuals who do not respond to PTC are not necessarily insensitive to quinine, another intensely bitter compound (49,50,52). 

In the presence of a large excess of EtO ion, the bimetallic catalyst is fully saturated with EtO as shown by structure I in Scheme 5.3. Incremental additions of a carboxylate substrate would cause the gradual conversion of I into the 1 1 productive complex II, but further additions would yield the unproductive complex III. As expected from this mechanism a bell-shaped profile is observed in a plot of initial rate versus substrate concentration related to the catalyzed ethanolysis of 16 (Figure 5.5). The fairly good quality of the fit supports the validity of Scheme 5.3. Further confirmation comes from the finding that benzoate anions behave as competitive inhibitors of the reaction. Since the reaction product of the ethanolysis of 16 is also a benzoate anion, product inhibition is expected. Indeed, only four to five turnovers are seen in the ethanolysis of 16 before product inhibition shuts down the reaction. The first two turnovers are shown graphically in Figure 5.6. 

For a monoprotic system, the basic species, A-, is the predominant form when pH > P a. The acidic species, HA, is the predominant form when pH < pKa. The predominant form of benzoic acid at pH 8 is the benzoate anion, C6H5C02. 

Thus a quantitative ion-exchange reaction was confirmed to take place by a simple precipitation of a THF solution of lc and l c into aqueous solution containing a benzoate anion, and the subsequent ring-opening reaction of the pyrrolidinium salt groups was found to proceed by the heating treatment at 100°C. 

Benzoate anion was used as an oxygen nucleophile for imidazylates 4,12, 41,43 acetate ion was used for imidazylate 19 (acetate), and nitrite ion for imidazylate 22. 

Perbenzoic acid fcrf-butjl ester (51) is the source — under copper I) bromide catalysis —of a benzoate anion (52) and radical 53. Radical 53 subsequently abstracts a hydrogen atom selective ) from the 11 -position of 55 in a homolytic bond cleavage to give a buta diene system with opening of the cyclopropane ring.Jn... 

The effect of the anion on the copolymerization rate is controversial. Hilt et al.41 established for different sodium halides the following order of efficiency F < Cl < Br < J . This order was interpreted on the basis of the increase in nucleophilicity or polarizability of the anions. Sfluparek and Mleziva 43) observed that the reaction rate of the benzoate anion was about twice as high as that of the bromide anion in the copolymerization of epichlorohydrine with phthalic anhydride. On the other hand, Luston and Manasek56) did not detect any effect of the anion size on the copolymerization rate initiated by tetramethylammonium and tetrabutylammonium halides. 

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