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Definitions of Acids and Bases

Explore the definitions, characteristics, and examples of acids and bases. Learn about Arrhenius, Bronsted-Lowry, and Lewis definitions, conjugates, and models. Discover the properties of common acids and bases.

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Definitions of Acids and Bases

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  1. Definitions of Acids and Bases Chemistry Mrs. Coyle

  2. Common Acids Vinegar (acetic or ethanoic acid) Citric Acid

  3. Characteristics of Acids • Sour taste (for edible acids) • May burn your skin • Turn litmus paper from blue to red.

  4. Examples of Acids • HCl Hydrochloric Acid • H2SO4 Sulfuric Acid • HNO3 Nitric Acid • CH3COOH Acetic Acid (Vinegar)

  5. Common Bases Ammonia

  6. Characteristics of Bases • Bitter taste (for edible bases only) • Can be poisonous and corrosive. • Turn litmus from red to blue.

  7. Examples of Bases • Sodium Hydroxide NaOH • Potassium Hydroxide KOH • Magnesium Hydroxide Mg(OH)2 • Ammonia NH3

  8. Three Definitions of Acids and Bases • Svante Arrhenius (Swedish 1887) • Bronsted- Lowry (Danish and English 1923 independently proposed definition) • Gilbert Lewis (American 1920’s)

  9. Arrhenius Definition of Acids and Bases • Acids produce hydrogen ions (H+) in an aqueous solution, while bases produce hydroxide ion (OH-). Acid: HCl (aq) H+ (aq) + Cl- (aq) Base: NaOH(aq) Na+(aq) + OH-(aq)

  10. Acids can have more than one ionizable hydrogen.

  11. Bronsted- Lowry Definition of Acids and Bases • An acid is a proton (H+) donor. • A base is a proton (H+) acceptor. • Example: HF + H2O H3O+ + F- Acid Base H3O+ : hydronium ion

  12. Conjugate Acids and Bases • General expression: HA (aq) + H2O (l) H3O+ (aq) + A- (aq) Acid Base Conjugate Conjugate Acid Base

  13. Conjugate Acids and Bases • Conjugate acid is the particle formed that has received the proton. (ex: H3O+) • Conjugate base is the particle left from the acid once it has donated the proton.

  14. Ammonia NH3(aq) + H2O (l)  NH4 + (aq) + OH- (aq) Base Acid Conjugate Conjugate Acid Base

  15. Note • Water acts as an acid and as a base. It is amphoteric.

  16. Lewis Acids and Bases • An acid accepts a pair of electrons. • A base donates a pair of electrons. • This is a more general definition than the previous two.

  17. Example of a Lewis Acid and Base :NH3 + H+  NH4+

  18. Three Models of Acids and Bases

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