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33 Cards in this Set
- Front
- Back
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Arrhenius |
Acid- hydrogen ions |
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Arrhenius
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Acid- hydrogen ions
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Arrhenius |
Acid- hydrogen ions |
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Arrhenius |
Acid- hydrogen ions, Base- hydroxide ions; |
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Brønsted-Lowry
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Acid- donates proton (hydrogen ion), Base- accepts proton, Conjugate pairs
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Lewis
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Acid- accepts an electron pair, Base- donates an electron pair
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pH=
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-log [H ]
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pOH=
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-log [OH-]
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pKa=
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-log Ka
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pKb=
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-log Kb
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[H ] = [OH-], the solution is...
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NEUTRAL!
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[H ] > [OH-], the solution is...
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Acidic
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[H ] < [OH-], the solution is...
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Basic
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pH=7
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Neutral
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pH<7
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Acid
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pH>7
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Basic
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What defines a weak acid?
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When placed in water, only a small fraction of its molecules will dissociate into hydrogen ions and conjugate base ions. Most of the molecules will remain in solution as undissociated aqueous particles.
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Strong acids/bases have (low / high) K values.
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High
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6 strong acids |
HCl, HBr, HI, HNO3, HClO4, H2SO4
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5 strong bases
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LiOH, NaOH, KOH, Ba(OH)2, Sr(OH)2
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Oxoacids
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Acids that contain oxygen, the greater the number of oxygen atoms in a molecule, the stronger the acid, more oxygen attractions in an atom weakens the attraction of the central atom for the H
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Polyprotic acids
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Acids that can give up more than one H
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Amphoteric substances
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Substances that can act as either acids or bases
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Acid anhydride
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Combines with water to form an acid; usually a nonmetal
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Basic anhydride
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Combines with water to form a base; usually metals
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Equivalence point
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Point in titration when exactly enough base has been added to neutralize all the acid that was initially present (or vice versa)
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Half-equivalence point
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Point when enough base has been added to convert half of the acid into conjugate base; [acid]=[conjugate base] pH=pKa
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Dissociation
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decomposes to ions
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Hydrolysis
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Reacts with water
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@ 1/2 equivalence point, kPa=
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pH
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How to find Ka from pKa
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10^-kPa
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Buffer equation to memorize
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[H+]=Ka ( [A] / [B] )
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End point |
when the indicator changes color |
