Acetic acid acetate ion

The most common charge types for the acid HB and its conjugate base B are CH3COOH = H+ -f CH3C00 (acetic acid, acetate ion)... 

Calculate the equilibrium concentrations of acetic acid, acetate ion, and hydronium ion in a 2.5 M solution of acetic acid. 

In accordance with this view, the occurrence of the unusual peaks on the cyclic voltammograms observed in acetic acid/acetate system was ascribed to a one-electron transfer process of acetic acid/acetate ions according to the equations [180] ... 

The irreversible A-Se2 mechanism was observed in dilute hydrochloric acid solution when there was no substituent at C-7 and when both syn- and 3f n -isopropyl and -butyl groups were at carbon-7. The reversible mechanism was only found when an isopropyl or /-butyl group was syn to the diazo group and the reaction was carried out in the acetic acid-acetate ion buffer. 

Figure 61 shows the pH-logCj diagram of the corresponding acid-base pair acetic acid/acetate ions. 

Sulfurous acid Sulfite ion Boric acid Borate ion Acetic acid Acetate ion... 

All of the previous acid-base examples dealt with situations in which an acid and its conjugate base were close to equilibrium. In the following example, we consider the addition of a strong acid to an acetic acid/acetate ion buffer. Hydro-nium ion reacts with the conjugate base (acetate ion) in the buffer, so that the con-centtations of species in solution change markedly from their initial value. (If you add a strong base to this buffer, hydroxide ion reacts with acetic acid in the buffer.)... 

In the case of our acetic acid (1.0 A/) and sodium acetate (1.0 A/) buffer, the concentrations of weak acid and conjugate base are equal. When this is true, the log term in the Henderson-Hasselbalch equation is zero and the pH is numerically equal to the pAa. In the case of an acetic acid-acetate ion buffer, pAa = -log 1.8 X 10 = 4.74. 

Q How does this acetic acid/acetate ion buffer maintain pH ... 

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