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Acids and Bases. Definitions. Bronsted -Lowry: Acids donate protons (H + ) Bases accept protons (H + ) Arrhenius: Acids produce hydronium in water (H 3 O + ) Bases produce hydroxide in water (OH - ). Properties of acids and bases. What is the acid ?.
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Definitions • Bronsted-Lowry: • Acids donate protons (H+) • Bases accept protons (H+) • Arrhenius: • Acids produce hydronium in water (H3O+) • Bases produce hydroxide in water (OH-)
What is the acid? HNO3(aq) + NH3(aq) → NO3-(aq) + NH4+(aq) PO43- + CH3COOH → HPO42-+ CH3COO- H2O + NH4+ → H3O+ + NH3 What is the base? What is the conjugatebase? What is the conjugate acid?
Strong vs. Week • Strong acids and bases ionize or dissociate completely (100%) • Ex: HCl + H2O→ Cl- + H3O+ NaOH → Na+ + OH- (all of the acid and base become products) • Weak acids and bases ionize or dissociate only partially (<100%). The reach equilibrium. • Ex: HNO2 + H2O ↔ NO2- + H3O+ NH3 + H2O ↔ NH4+ + OH- (only some of the acid and base become products)
Strong Acids • HCl: hydrochloric acid • HBr: hydrobromic acid • HI: hydroiodic acid • HNO3: nitric acid • H2SO4: sulfuric acid • HClO4: perchloric acid Hydrogen Halides Oxyacids
Strong bases • LiOH • NaOH • KOH • RbOH • CsOH • Sr(OH)2 • Ba(OH)2