Acid-Base Chemistry (5/10) Flashcards
Arrhenius
Acids and bases dissociate in certain solutions for form ions
acids: H+
bases: OH-
Arrhenius acids and bases
Acids must have H+ in it
Bases must have OH- in it
(not very broad, limiting)
Bronsted-Lowrey
An acid is a proton donor
A base is a proton acceptor
-MCAT mostly refers to Brownsted
for Bronsted, once acid loses proton…
Once proton is lost= conjugate base of undissociated proton
Lewis
Acids= electron acceptors Base= electron donor
Difference in Lewis to other two
Addresses problems to make it most broad and includes (helps with oxidation and reduction)
Amphoteric species
Can either accept or donate a proton
EX) water, amino acids
Acid-base Equilibria
Protons are gained and lost
Keq
Equilibrium constant
- general term
- reflects the relative [] of products and reactants
Kw
For water Water auto
- ionization equilibrium constant
- reaction of water with itself to form ions
Kw value
[H3O][OH]
1x 10^-14
temperature dependent !
Temperature effect on Kw
not at standard temp, very low temperature= lower [H3O+], raises pH (basic from being in a cold room)
As long as both concentrations are equal though, concentrations are still equal and pH is just not always 7
Kb
base dissocation constant
Ka
acid dissociation constant
High Ka
dissociates more readily and forms more products
