Acid-Base Chemistry Flashcards
3 ways to define Acid:
Arrhenius: dissociate to form H+ ions
B-L: Acid is a proton donor
Lewis: Acid is electron acceptor
Lewis: Acid acceptor
3 ways to define Base:
Arrhenius: dissociate to form OH- ions
B-L: Base is proton acceptor
Lewis: Base is electron donor
What is amphoteric and what are some EX
- either accept or donate a proton
- EX: water, amino acids
What is Kw?
1E-14: only at room temp, 35C
- temp dependent
- directly prop to temp, however H+ and OH- are equal in water
- water is neutral at any temp, however its pH might not be 7
Why does large Ka or Kb relate ot strong acid or base respectively?
parent acid or base is in denominator
- ions are the numerator
Ka = H+ A- / HA
- thus a large Ka has ion products in higher concentrations > dissociates more readily
- dissociate less readily, hold on to proton
Strong acids
HBR, I, HCl (halogens)
HNO3 and H2SO4
HClO3 and HClO4
Strong bases
OH of alkali earth metals: NaOH, KOH, Ca(OH2)
- NH2-, H-, CH3O-, CH3CH2O0, (CH3)3CO-, C2H5ONa
Acid-Base Common Ion Effect
Acid to Acid: Acid ionizes less
Acid to base: Acid ionizes more
Base to Base: Base ionizes less
Base to Acid: base ionizes more
what does “-p”
-log
Pka + pkb =
14