Acetic acid and sodium hydrogen carbonate, NaHCO₃, are mixed in water. Write a balanced equation for the acid–base reaction that could, in principle, occur. Using Table 16.2, decide whether the equilibrium lies predominantly to the right or to the left.

Data given in Table 16.2

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Increasing Acid Strength TABLE 16.2 Acid Name Perchloric acid Sulfuric acid Hydrochloric acid Nitric acid Ionization Constants for Some Acids and Their Conjugate Bases at 25 °C K₂ Large Large Large Large 1.0 1.2 x 10-2 1.2 x 10-2 7.5 x 10-3 6.3 x 10-³ 7.2 x 10-4 4.5 x 10-4 1.8 x 10-4 Hydronium ion Sulfurous acid Hydrogen sulfate ion Phosphoric acid Hexaaquairon (111) ion Hydrofluoric acid Nitrous acid Formic acid Benzoic acid Acetic acid Propanoic acid Hexaaquaaluminum ion Carbonic acid Hexaaquacopper(11) ion Acid HCIO4 H₂SO4 HCI HNO3 H₂O+ H₂SO3 HSOA™ H3PO4 [Fe(H₂O)]³+ HF HNO₂ HCO₂H C6H5CO₂H CH3CO,H CH3CH₂CO₂H [AI(H₂O)]³+ H₂CO3 [Cu(H₂0)]²+ Hydrogen sulfide H₂S Dihydrogen phosphate ion H₂PO4 Hydrogen sulfite ion HSO3 Hypochlorous acid HCIO Base CIO4 HSO4 CI- NO3 H₂O HSO3 SO4²- H₂PO4 [Fe(H₂0)50OH]²+ F- NO₂™ HCO₂ C6H5CO₂ CH3CO, CH3CH₂CO₂ [AI(H₂O)5OH]²+ HCO3 [Cu(H₂0); OH]+ HS- 6.2 x 10-8 HPO4²- 6.2 x 10-8 SO3²- 3.5 x 10-8 CIO 6.3 x 10-5 1.8 × 10-5 1.3 x 10-5 7.9 x 10-6 4.2 x 10-7 1.6 x 10-7 1 x 10-7 K₂ Very small Very small Very small Very small 1.0 x 10-14 8.3 x 10-13 8.3 x 10-13 1.3 x 10-12 1.6 x 10-12 1.4 x 10-11 2.2 x 10-¹¹ 5.6 x 10-¹1 1.6 x 10-10 5.6 x 10-10 7.7 x 10-10 1.3 x 10- 2.4 x 10-8 6.3 x 10-8 1 x 10-7 1.6 x 10-7 1.6 x 10-7 2.9 x 10-7 Base Name Perchlorate ion Hydrogen sulfate ion Chloride ion Nitrate ion Water Hydrogen sulfite ion Sulfate ion Dihydrogen phosphate ion Pentaaquahydroxoiron (III) ion Fluoride ion Nitrite ion Formate ion Benzoate ion Acetate ion Propanoate ion Pentaaquahydroxoaluminum ion Hydrogen carbonate ion Pentaaquahydroxocopper(11) ion Hydrogen sulfide ion Hydrogen phosphate ion Sulfite ion Hypochlorite ion Increasing Base Strength