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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
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