Acid - Base Equilibrium
Terms
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- Bronsted-Lowry Acid and Base Theory
- Acid: proton donor, Base: proton acceptor
- [H+] equation
- [H+] = 10^ -pH
- Arrhenius Acid and Base Theory
- Acids produce H+, Bases produce OH-
- pOH equation
- pOH = -log{OH-]
- Strong acids and bases
- dissociates completely in water, large K values, strong electrolytes
- Autoionization of water Reaction:
- 2 H2O <-> H3O+ + OH-
- How atomic size affect strength?
- the bigger radius / MM, the higher strength (harder to break bonds)
- Lewis Acid and Base Theory
- Acid: accept e-, Base: donate e-
- pH equation
- pH = -log{H+]
- Weak Acid ions
- HSO4-, HSO3-, H2PO4-, NH4+
- [OH-] equation
- [OH-] = 10^ -pOH
- Weak acids and bases
- don't dissociate in water, small K value, weak electrolytes
- How Oxygen affect strength?
- the more O, the more strength
- Properties of Bases
- bitter, pH>7, produce OH- in solution, slippery
- pKw, pKa, pKb equations
- pKa = -log[Ka] pKb
- Strong Bases
- LiOH, NaOH, KOH, Ba(OH)2, Sr(OH)2, Ca(OH)2 (CaSr Na BALiK)
- % Dissociation equation
- (x/original conc) x 100%
- Electronegativity patern on periodic table?
- HF is highest EN
- Weak Bases ions
- C2H3O2-, HS-, HPO4 2-, CN-, CO3 2-, PO4 3-, S2-
- BAses strength on periodic table?
- top right (ClOH) strongest
- Strong Acids
- HI, HBr, HCl, HNO3, H2SO4 (BrICl NO SO)
- Kwater value and equation?
- Kw = 1x10^ -14 ; Kw = Ka x Kb
- Properties of acids
- sour, pH<7, produce H+ in solution
- Acid strength on periosdic table?
- bottom left (HFr) strongest