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
Acid strength
stronger acid= dissociates almost completely and has a high Ka
Base strength
Has a high Kb
7 strong acids
HI HBr HCl HNO3 H2SO4 HClO3 HClO4
Strong bases
NaOH KOH Ca(OH)2 NH2- H- CH3O- CH3CH2O- (CH3)3CO-
ACid and bases with common ion effect
Add acid to acid solution then we go to left and we wont ionize as much
Add acid to basic solution, we shift to the right and go more to products
pH scale
pH=-log[H3O+]
pOH= -log[OH-]
Kw
-log Kw =14
pH + pOH
=14
Pka and Ka realtionship
low pKa means high Ka and this means a strong acid.
pKa and Ka have an inverse relationship
Ka x Kb (acid and conjugate base)
= Kw or 1.0 x 10^-14 at 25 C
Organic acid naming
Derived from organic compounds (contains carbons)
EX) carboxylic acids
Inorganic acids
Does not contain carbon
EX) HI or hydroiodic acid
Oxyacids
Inorganic, name depends on number of oxygen atoms present
Names of oxyacids
ClO- hypochlorite
ClO2- chlorite
ClO3- chlorate
ClO4- perchlorate
HClO hypochlorous acid
HClO2- chlorus acid
HClO3 chloric acid
HClO4 perchloric acid
