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17 Cards in this Set
- Front
- Back
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Acid
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proton (H+) donor
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Base
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proton (H+) acceptor
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Conjugate base
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acid after it has donated a proton
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Conjugate acid
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base after it has accepted a proton
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Acid dissociation constant (Ka)
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numerical measure of acid strength; how readily H+ is released when an acid is dissolved in water
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Ka=
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[H+][A-]/[HA]
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Smaller pKa=
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stronger acid
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Kw=
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[H+][OH-] = 10E-7 X 10E-7 = 10E-14
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pH=
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-log10 * [H+]
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pKa=
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-log10 * Ka
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Titration curve
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used to determine at what pH value, an acid donates its H+
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Equivalence point
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Where acid is neutralized
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Inflection point
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midpoint where no change in pH is observed due to addition of base to an acid
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If pH>pKa
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then acid mostly deprotonated
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If pH<pKa
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then acid mostly protonated
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Henderson-Hasselbalch
pH= |
pKa + log [A-]/[HA]
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If pH=pKa
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then acid = base
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