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