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Acids and Bases

This section explores the fundamental characteristics of acids and bases, covering their properties, behaviors, and the differences between strong and weak varieties. Acids, known for their sour taste, ionize in water to produce hydrogen cations (H+) and hydronium ions (H3O+), while bases, which taste bitter and feel slippery, generate hydroxide ions (OH-) in solution. The pH scale ranging from 0 to 14 indicates the acidity or basicity of a solution, with 7 being neutral. This overview serves as a guide to understanding these essential chemical concepts.

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Acids and Bases

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  1. Acids and Bases (p. 256-261, 264-265)

  2. Acids • Taste sour

  3. Acids • Ionize when dissolved in water (they dissociate into their ions; +, -). • This allows the water to conduct electricity (which means they are electrolytes). • Ex- HCl is an acid…when placed in water, it becomes H+ and Cl-

  4. Acids • Acids produce Hydrogen Cations • Therefore, the formula for an acid must have H in it (usually it will be at the beginning of the chemical formula only) • Ex. HCl, H2SO4

  5. Acids • The H+ will attach to H2O to form Hydronium ions (H3O+) • Acids produce H3O+ in water

  6. Strong vs. Weak AcidsSee Table on p. 258 Strong Acid • Ionize completely • HNO3+ H2O  H3O+ + NO3- • strong electrolytes • (can conduct electricity well) Weak Acid • Don’t ionize completely (don’t produce as many ions) • CH3COOH + H2O  H3O+ + CH3COO- • weak electrolytes

  7. BASES • Taste Bitter and Soapy • Feel Slippery

  8. Bases • Some contain hydroxide ions, OH- , in their formulas, others don’t. • Those that don’t have OH in the formula will react with water to produce OH- ions. • All produce hydroxide ions, OH- , in water & conduct electricity (electrolytes).

  9. Strong vs. Weak Bases Strong Bases • Have OH and a metal atom in their formula • (ex-NaOH) • Dissociate in water to give: OH- & metal ion • ex. NaOH OH- + Na+ • Strong electrolyte Weak Bases • Don’t have OH in their formula • (ex-NH3) • ionize in water to produce OH- (water gives up an H), but doesn’t ionize completely • ex. NH3 + H2O  NH4++ OH- • Weak electrolyte

  10. pH Scale • Ranges from 0-14 • 7=neutral (not acidic nor basic), • Amount of H3O+ is equal to amount of OH- • Low pH (0-<7) = acidic • Amount of H3O+ is greater than the amount of OH- • pH of 3 is more acidic than a pH of 5 • High pH (>7-14)= basic • Amount of H3O+ is less than the amount of OH- • pH of 13 is more basic than a pH of 10

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