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22 Cards in this Set
- Front
- Back
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Arrhenius acids dissociate to form |
An excess of H+ in solution |
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Arrhenius Basra dissociate ti for an excess of |
OH- in solution |
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Brønsted-Lowry acids |
Donate protons BAD (+) |
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Brønsted-Lowry bases |
Accept protons BBA (+) |
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Examples of bronsted bases and Arrhenius bases |
OH-, NH3, and F- are bronsted bases because they can accept protons NH3 and F- can’t be Arrhenius bars because they can’t donate OH |
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Lewis acids accept |
Electrons LAA(-) |
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Lewis bases |
Donate electrons LBD(-) |
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Coordinate covalent bonds and nucleophile/electrophile interactions are examples if |
Lewis acids and bases |
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Amphoteric species |
Can act as an acid in basic environments or bases in acidic environments |
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Name the amphoteric species in the reaction H2SO4-> HSO4- -> SO42- |
HSO4- |
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If pH=pka, then |
[HA]=[A-] |
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If pH=pka, then |
[HA]=[A-] |
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If pH>pka, then |
[HA]<[A-] |
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If pH=pka, then |
[HA]=[A-] |
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If pH>pka, then |
[HA]<[A-] |
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If pH |
[HA]>[A-] |
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pOH formula |
pOH = -log[OH] or log 1/[OH] |
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pH formula |
pH = -log[H] or log 1/[H] |
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Can temperature affect Kw? |
Yes. At temperatures above 298, Kw increases |
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All equilibrium constants depend on |
Temperature |
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If Ka or Kb is smaller than 1, then the acid or base is considered |
Weak |
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Nonionic weak bases are typically |
Amines |
