Acid-Base Chemistry (5/10)

Acids and bases dissociate in certain solutions for form ions acids: H+ bases: OH-

Acids must have H+ in it Bases must have OH- in it (not very broad, limiting)

An acid is a proton donor A base is a proton acceptor -MCAT mostly refers to Brownsted

Once proton is lost= conjugate base of undissociated proton

Acids= electron acceptors Base= electron donor

Addresses problems to make it most broad and includes (helps with oxidation and reduction)

Can either accept or donate a proton EX) water, amino acids

Protons are gained and lost

Equilibrium constant • general term • reflects the relative [] of products and reactants

For water Water auto • ionization equilibrium constant • reaction of water with itself to form ions

[H3O][OH] 1x 10^-14 temperature dependent !

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

base dissocation constant

acid dissociation constant

dissociates more readily and forms more products

stronger acid= dissociates almost completely and has a high Ka

Has a high Kb

HI HBr HCl HNO3 H2SO4 HClO3 HClO4

NaOH KOH Ca(OH)2 NH2- H- CH3O- CH3CH2O- (CH3)3CO-

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=-log[H3O+] pOH= -log[OH-]

-log Kw =14

=14

low pKa means high Ka and this means a strong acid. pKa and Ka have an inverse relationship