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Acids & Bases

Acids & Bases. Characteristics Acid Tastes Sour (orange juice) Low pH (1-7) Usually have a H (ex. HCl ) Base Tastes Bitter (Tonic Water) High pH (7-14) Usually have a OH (ex. NaOH ). Definitions of acids/bases. Arrhenius Acid/Base (oldest one) Gives up Hydronium/Gives up Hydroxide

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Acids & Bases

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  1. Acids & Bases • Characteristics • Acid • Tastes Sour (orange juice) • Low pH (1-7) • Usually have a H (ex. HCl) Base • Tastes Bitter (Tonic Water) • High pH (7-14) • Usually have a OH (ex. NaOH)

  2. Definitions of acids/bases • Arrhenius Acid/Base (oldest one) • Gives up Hydronium/Gives up Hydroxide • Bronsted-Lowrey Acid/Base (more modern) • Gives up proton/Accepts proton

  3. Conjugate Base Acid Conjugate Acid Base Parts of Reactions • Remember, Acids give up protons and Bases take ‘em! • HF + H2O  H3O+ + F-

  4. Acid Dissociations • Strong Acid + Water • When strong acids (HCl, HI, HBr, HNO3, HClO4 & H2SO4) are added to water they dissociate completely making hydronium and the anion of the acid. • HCl + H2O  H3O+ + Cl- • Weak Acid + Water • When a weak acid is added to water, only a small portion of it dissociates (double arrow) making hydronium and the anion of the acid. • HF + H2O  H3O+ + F-

  5. Base Dissociations • Strong/Weak Bases • When a strong base (OH’s of 1st Column and Ca2+, Sr2+ & Ba2+) or weak base that is a hydroxide is added to water it breaks apart. Since the water does not actually change in the reaction, it is put over the arrow. • NaOH --> Na+ + OH- • Be(OH)2 --> Be2+ + 2OH-

  6. Acid + Base • When an acid reacts with a base, salt and water are produced. The acid and base neutralize each other and it doesn’t matter if they are strong or weak! • HCl + NaOH  NaCl + H2O • This is called a neutralization reaction

  7. [H3O+] The pH Scale [H3O+] = [OH-] [OH-]

  8. Calculate the pH's of strong acids from Molarity of Strong Acids. • [H+] = 1 x 10-7 M • [OH-] = 1x 10-7 M So what is the pH of distilled water?

  9. Titrations • This is a lab technique that uses neutralization math that enables the user to find the pH of an unknown acid or base.

  10. Reaction Equilibrium

  11. Le Chatlier’s Principle… • This principle says that for any change you make to a system at equilibrium, the system will shift to “undo” that change. • PCl5 (g)  PCl3 (g) + Cl2 (g) • This reaction is endothermic… • Which way will the reaction shift if • Cl2 (g) is added? • Pressure is increased? • Reaction vessel is cooled down? • PCl3 is removed as it is formed?

  12. Another Problem… • C (s) + H2O (g)  CO (g) + H2 (g) • Reaction is Endothermic… • Which way will the reaction shift if • The reaction vessel is heated up? • Pressure is decreased? • More solid carbon is added? • Carbon monoxide is taken out?

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