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16 Cards in this Set
- Front
- Back
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K > Q |
Forward reaction, reactants into products |
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K < Q |
Backwards reaction, products into reactants |
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K = Q |
Reaction is at equilibrium |
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Auto-Ionization Constant of Water |
Kw = [H3O+][OH-] |
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pH equation |
pH = -log[H3O+] |
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Amphoteric |
Able to be both an acid and a base (Water) |
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Bronsted-Lowry Theory |
Mixing an acid and base together forms weaker conjugate acid and bases through the exchange of a proton |
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Polyprotic Acids Kan rule |
Ka1 > Ka2 > Ka3 because each ionization becomes more difficult to remove an H+ due to increased negative charge |
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Reaction Quotient Equation |
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Saturation of a solution |
Saturated = at equilibrium Supersaturated = excess solute Undersaturdated = not enough solute |
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What determines the strength of the acid? |
Larger difference in electronegativityeans stronger acid |
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[OH-] or [H3O+] Equation |
10^-14 / [H3O+] |
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pH + pOH = |
pH + pOH = 14 |
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pKa equation |
pKa = -log(Ka) |
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pKa relation to acid strength |
The larger the pKa value, the weaker the acid |
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Ka * Kb = |
Ka * Kb = Kw |
