ACIDS AND BASES

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ACIDS AND BASES

• Acidic H ions and basic OH- ions

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SOLUTIONS

• All aqueous solutions (water) contain Hydrogen
  ions H and Hydroxide ions (OH-. The relative
  amounts of the two ions determine whether an
  aqueous solution is acidic, basic or neutral.

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SOLUTIONS

• ACIDIC contains more H ions than (OH- ions
• BASIC contains more (OH- ions than H ions
• NEUTRAL has and equal amount of both

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TYPES OF ACIDS

• Arrhenius Model an acid is a substance that
  contains hydrogen and ionizes in aqueous
  solutions to produce hydrogen ions. A base is a
  substance that contains a hydroxide group and
  dissociates in aqueous solutions to produce
  hydroxide ions

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• Bronsted-Lowery model and acid is a hydrogen
  ion donor and a base is a hydrogen ion acceptor.
  When a Bronsted-Lowery acid donates a hydrogen
  ion a conjugate base is formed and vice versa
  when it accepts a hydrogen ion a conjugate acid
  is formed. Th two combined form a conjugate
  acid-base pair

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• Monoprotic Acid an acid that can donate only 1
  H ion. Like HCl
• Polyprotic acid an acid that can donate more
  than 1 H ion. Like H2SO4.

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STRENGTHS

• An acid that ionizes completely in dilute aqueous
  solution is a strong acid Like HCl, H2SO4, HNO3
• A weak acid ionizes only partially Like H3CO3,
  H3PO4, H3BO3, H3PO4
• You can use Keq to determine this

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• Bases Metallic Hydroxides are strong bases
• Weak bases are generally non-metallic hydroxides

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pH

• Equals the negative logarithm of the hydrogen ion
  concentration
• pH -Log H
• pOH is the negative logarithm of the hydroxide
  concentration
• pOH - Log OH-
• pH pOH 14