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Understanding Acids and Bases: Definitions and Behavior

Explore the definitions of acids and bases through Arrhenius and Brønsted-Lowry theories. Learn how they behave on a particulate level and differentiate between strong and weak forms.

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Understanding Acids and Bases: Definitions and Behavior

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  1. Living By ChemistrySECOND EDITION Unit 4: TOXINS Stoichiometry, Solution Chemistry, and Acids and Bases

  2. Lesson 85: Pass the Proton • Acid-Base Theories

  3. ChemCatalyst • Which of these four solutions conduct electricity: 0.10 M HCl (hydrochloric acid), 0.10 M CH3COOH (acetic acid), 0.10 M NaCl (sodium chloride),0.10 M C12H22O11 (sugar)? Explain.

  4. Key Question • How are acids and bases defined?

  5. You will be able to: • define Arrhenius and Brønsted-Lowry acids and bases • explain the behavior of acids and bases on a particulate level • explain the difference between strong and weak acids and bases

  6. Prepare for the Activity Work in groups of four.

  7. Discussion Notes • Acids are substances that add H+ to solution. • Bases are substances that add OH- to solution. • Neutral substances do not add H+ or OH- to solution. • The definitions of acids and bases have changed over time.

  8. Discussion Notes (cont.) • Arrhenius Definition of Acids and Bases: • An acid is any substance that adds hydrogen ion (H+) to solution. • A base is any substance that adds hydroxide ion (OH-) to solution.

  9. Discussion Notes (cont.) • Brønsted-Lowry Definition of Acids and Bases: • An acid is a proton donor. • A base is a proton acceptor. • Acids and bases that break apart (dissociate) completely in solution are called strong acids and strong bases. • Acids and bases that do not dissociate completely in solution are called weak acids and weak bases.

  10. Wrap Up • How are acids and bases defined? • According to the Arrhenius definition, an acid is a substance that adds hydrogen ions, H+, to an aqueous solution. • According to the Arrhenius definition, a base is a substance that adds hydroxide ions, OH–, to an aqueous solution.

  11. Wrap Up (cont.) • Some substances add OH– by removing H+ from water. Brønsted and Lowry define an acid as a proton (H+)donor and a base as a proton (H+) acceptor. • Strong acids and strong bases dissociate completely into ions, while weak acids and weak bases do not.

  12. Check-In • Which substances do you expect will conduct electricity: hydrocyanic acid, HCN; magnesium hydroxide, Mg(OH)2; methanol, CH3OH? Explain your thinking.

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