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Definitions of Acids and Bases

Definitions of Acids and Bases. Chemistry Mrs. Coyle. Common Acids. Vinegar (acetic or ethanoic acid). Citric Acid. Characteristics of Acids. Sour taste (for edible acids) May burn your skin Turn litmus paper from blue to red. Examples of Acids. HCl Hydrochloric Acid

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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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