Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
BR Chem Ch4
Flashcards from chapter 4 of Berkley Review's chemistry book (2010)
| 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 |
Created by:
kcurtiss
Popular MCAT sets