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28 Cards in this Set
- Front
- Back
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Arrhenius definition of acid/base
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Acids ionize in water to produce H+ ions
bases ionize in water to produce OH- |
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Bronsted-Lowry definition of acid/base
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Acids are proton donors, bases are proton acceptors
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Lewis acid/base
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lewis acid - e-n pair acceptor
lewis base - e-n pair donor |
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Strong acids
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HI, HBr, HCl, HClO4, HClO3, H2SO4, HNO3
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Amphoteric substance
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Substance that can act both as acid and base
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Kw
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[H3O][OH-], Kw= 1.0*10^-14
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pH
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-log [H+]
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pH+pOH
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14
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pOH
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-log [OH]
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KaKb
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Kw
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What is concentration [H+] in sstrong acid?
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same as acid, dissociates completely
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pH calculation in weak acid
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[HA]= 0.2
Ka= [H+][A-]/[HA]= x^2/0.2 |
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pKa
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-logKa
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pKb
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-log Kb
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pKa+pKb
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14
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Neutralization reaction
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Reaction of acid and base that produces salt and water
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Indicator
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weak acid that undergoes a color change when it is converted to conjugate base
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Salt
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ionic compound that consists of anion and cation
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Buffer
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Solution that resists changes in pH when small amount of acid/base is added
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Henderson-Hasselbalch equation
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pH= pKa - log [weak acid]/conjugate base
pH= pKa+ log [conjugate base/weak acid] |
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In designing buffer what should be acid's pKa?
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should be as close as possible to pH
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Henderson Hasselbalch equation for base
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pOH= pKb - log [weak base/conjugate acid]
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Acid Base titration
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Experimental technique used to determine identity of unknown weak acid/base by determining pKa (pKb)
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Titration curve weak acid/strong base
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equivalence point at pH>7
starts low, goes up |
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Titration curve weak base/strong acid
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equivalence point at pH <7, starts high, goes down
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Titration curve for polyprotic acid
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multiple equivalence points
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Buffering region
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Section of the titration curve where pH changes very gradually
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Equivalence point
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point during drastic pH change when enough base is added to neutralize all acid
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