Chapter 9: Acids and Bases

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34 Terms

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Ka=

acids

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Kb=

bases

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Ksp=

solids

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titrations

analytical technique to calculate something

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endpoint of titration

when moles of acid equals mols of base

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indicator in titrations

pH dependent and cause a color change

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standardize titration

determines molarity

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Acid=

proton donor

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base

proton acceptor

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an acid has a

conjugate base pair

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a base has a

conjugate acid pair

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pH can be calculated directly from

Ka

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pOH can be calculated directly from

Kb

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amphoteric

both acid and base

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pH=

-log[H3O+]

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pOH=

-log[OH-]

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Kw=

[H3O+][OH-]

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Kw=

1.0×10-14

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pKw=

-log(Kw)

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pKw=

14

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pH+pOH=

pKw

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pH+pOH=

14

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weak acid Ka=

x2/y

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OH- means that

base is present

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H3O+ means that

acid is present

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weak base Kb=

x2/y

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pKa=

-log(Ka)

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pKb=

-log(Kb)

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Ka=

10-pKa

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Kb=

10-pKb

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buffers equation

(z)(x)/(y)

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buffers resist

pH changes

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Steps for buffer equations

  1. ICE tables

  2. IRNI table

  3. NICE table

34
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Buffers contain a

weak acid and its conjugate base or a weak base and its conjugate acid