Question | Answer |
Arrhenius acid | yields H3O+ when hadded to H2O |
Arrhenius base | yields OH- when added to H2O |
Bronsted-Lowry acid | Proton donor |
Bronsted-Lowry base | Proton acceptor |
Lewis acid | Electron pair acceptor |
Lewis base | Electron pair donor |
Amphoteric | Can act as either an acid or a base |
Hydronium concentration @ 25C | 1x10-7M ph=7 |
Ka | [H3O+][A-]/[HA] |
pKa | pKa -log(Ka) |
Ka from pKa | Ka = 10^-pKa |
Dissociation | acids dissociate in water |
Hydrolysis | bases under go hydrolysis in water |
Equation relating pKa(HA) and pKb(A-) | pKa(HA) + pKb(A-) = 14 |
pKa and Ka as acid strength increases | pKa goes down, Ka goes up |
Strong acids | HCl, HBr, HI, H2SO4, HNO3, HClO4 |
Strong bases | LiOH, KOH, NaOH, Ca(OH)2, KOCH3, NaNH2, Li(CH2)3CH3 |
Weak acid | 0 < pKa < 14 |
Very weak acid | pKa > 14 |
Kw | 1x10^-14 |
Haloacid trends | * As halogen size increases, acid strength increases
* Within a period, acidity increases with increasing electronegativity of halogen |
Haloacid | Of the form HX |
Oxyacids | Hydrogen dissociates from oxygen |
Oxyacids trends | * More oxygens bonded to central atom means more acidic (most important trend)
* If same number of O's, increasing electronegativty of central atom increases acidity |
For oxyacids, change in pKa with each additional O | pKa decreases by approximately 5 for every O gained |
Metal oxides | lewis base |
metal hydroxides | bronsted-lowry base |
pKa Carboxylic acid | 3-5, (2-3 in amimo acid) |
pKa phenol | 9.5-10.5 |
pKa alkyl ammonium cation | 9-11 (9-10 in amino acid) |
non-metal oxides | lewis acid |
non-metal hydroxides | bronsted-lowry acids |
Normality | moles of equivalents per liter solution. 1.0 molar diprotic acid is 2.0N |
pH formula | pH = -log[H3O+] |
relating pH and pOH | pH + pOH = 14 |
log(2) | 0.3 |
log(3) | 0.48 |
log(a*b) | log(a) + log(b) |
log(a/b) | log(a) - log(b) |
-log(a x 10^-b) | b - log(a) |
relationship between Ka and Kb | Ka*Kb = 10^-14 |
Formula for pH estimation | pH = (1/2)*pKa - (1/2)*log[HA] |
Formula for pOH estimation | pOH = (1/2)*pKb - (1/2)*log[A-] |
pH > pKa (protonated or deprotonated) | deprotonated |
pH < pKa (protonated or deprotonated) | protonated |
HH equation for buffers | pH = pKa + log([base]/[acid])
works for both concentrations and moles |