14.3: Acid and Base Strengths, Ka, Kb, Acid-Base Equilibria

• Is k temperature dependent?

  yes
• Do catalysts impact k?

  No, they change how fast equilibrium is reacted but do not change equilibrium position
• What are examples of strong acids?

  HCl, HNO3, first proton on H2O4
• What are strong acids?

  Acids that completely dissociate in water to produce a high concentration of H+ ions.
• Are most acids strong or weak?

  weak
• What is an example of weak acids

  CH3COOH
• What are weak acids?

  Acids that do not completely dissociate in water.
• What are some examples of strong bases

  NaOH, KOH3, Ca(OH)2
• What are strong bases?

  bases that completely dissociate in water
• What are some examples of weak bases?

  Ammonia, sodium bicarbonate
• What do acids release in water?

  H+
• What do bases release in water?

  OH-
• What is the bronsted-Lowry Model

  an acid is a proton (H⁺) donor, and a base is a proton acceptor.
• Conjugate of a ___ is a weak ___

  strong X (acid or base), weak y (base or acid)
• What does it mean that water is amphoteric

  Can act as an acid or base
• pH + pOH =

  14.00
• pH = -

  log()
• (___)= 10

  ^-pH
• Stronger acids (____) generate higher [H+]

  larger ka
• stronger bases (___) generates higher [OH-]

  larger kb
• What is the percent dissociation equation

  (concentration of acid solute)/(concentration of acid ionized)​x100%
• For acids: a particular non-metal oxide species, the one with ___ oxygen will form a stronger acid

  oxygen
• Higher oxidation state of central = ___ acid

  stronger
• The same number of O: compare most ____ atom (don't use for binary acids)

  electronegative
• What is the most electronegative element

  Fluorine

  
• Most electronegative atom = ___ acid

  stronger acid