For each of the following ions, write two equations—one showing its ionization as an acid and the other as a base: 

(a) HSO₃^-; 

(b) HS^-; 

(c) HPO₄^-. 

Then use data from Table 16.5 to predict whether each ion makes the solution acidic or basic.

Table 16.5

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TABLE 16.5 lonization Constants of Some Polyprotic Acids Acid lonization Equilibria Hydrosulfurica Carbonicb Citric Phosphoric Oxalic Sulfurousc Sulfuricd H₂S + H₂O HS + H₂O H₂CO3 + H₂O HCO3 + H₂0 H₂PO4+H₂O H₂PO4¯ + H₂0 — HPO42- + H₂O → H₂C₂O4 + H₂0 HC,O4 + H,O H₂SO3 + H₂O — HSO3 + H₂0 H₂O+ + HS¯ H₂O+ + S²- — H₂0+ + HCO3- H3O+ + CO3²- Kaj K₁₂ = 4.7 x 10-11 H₂CH₂O + H₂O H₂O+ + H₂CH₂O₂K₁₁ = 7.5 × 10-4 H₂CH₂O₂ + H₂O H₂O+ + HC6H₂0,²- K₁₂ = 1.7 x 10-5 HC₂H₂0₂² + H₂0 — H3O+ + C¿H²0,³- Kaz = 4.0 x 10-7 K₁₁ = 7.1 × 10-3 K₁₂ = 6.3 × 10-8 = 4.2 X 10-13 Kaz Ka₁ = 5.6 x 10-2 Kaz H₂O+ + H₂PO4¯ H3O+ + HPO ²− H₂0+ + PO4³- H30+ + HC₂04- H₂O+ + C₂0₂²- H3O+ + HSO3- H3O+ + SO3²- lonization Constants, K = 1.0 × 10-7 H₂SO4+H₂O → H3O+ + HSO4- HSO4+H₂O H₂O+ + SO4²- Kaj Kaz Kay Kaz = 1 × 10-19 Kaz = 4.4 x 10-7 = 5.4 x 10-5 = 1.3 x 10-2 = 6.2 × 10-8 Kaj very large = 1.1 x 10-2 pk pka₁ = 7.00 pka2 pkal pka2 = 10.33 PK₁₁ = 3.12 PK₁₂ = 4.77 = 19.0 = 6.36 pK₁3 = 6.40 pK₁₁ = 2.15 PK₁₂ = 7.20 pk az pka₁ pKaz = 12.38 pK₁₁ = 1.25 pka₂ = 4.27 pka₁ = 1.89 pka₂ = 7.21 <0 = 1.96 Acid strength