Phosphoric acid can supply one, two, or three H₃O+ ions in aqueous solution. Write balanced equations (like those for sulfuric acid on page 142) to show this successive loss of hydrogen ions.

Data given in page 142

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Hydrochloric acid, a strong acid. 100% ionized. Equilibrium strongly favors products. + H₂O(l) H₂0+ (aq) + CL-(aq) HCl(aq) hydrochloric acid strong electrolyte = 100% ionized water CH3CO₂H(aq) acetic acid In contrast, CH3CO₂H, a weak electrolyte and weak acid, ionizes only to a small extent. Acetic acid, a weak acid, << 100% ionized. Equilibrium favors reactants. + H₂O(l) CH3CO₂ (aq) + hydronium ion Strong acid: H₂SO4 (aq) + H₂O(l) sulfuric acid 100% ionized Weak acid: HSO (aq) + H₂O(C) hydrogen sulfate ion <100% ionized water acetate ion hydronium ion Sulfuric acid, a diprotic acid (an acid capable of transferring two H+ ions), reacts with water in two steps. The first step strongly favors products, whereas the second step is reactant-favored. H₂0+ (aq) + hydronium ion chloride ion HSO₂ (aq) hydrogen sulfate ion H₂0+ (aq) + SO² (aq) hydronium ion sulfate ion H3O+(aq)