Kaplan General Chemistry: Chapter 10 Acids and Bases Flashcards

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1
Q

pka is the PH where:

A

HA = A-

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2
Q

low pka means

A

more acidic

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3
Q

low ka means

A

less acidic

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4
Q

high ka means

A

more acidic

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5
Q

formula for pka

A
pka = -log(Ka)
pka= -log (n x10^m)
pka = m-0.n
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6
Q

ka x kb = kw =

A

10^-14

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7
Q

equation for the equivalence point

A

NaVa = NbVb

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8
Q

Henderson-Hasselbach equation

A

pH = pka + log[A-]/[HA]

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9
Q

phosphorous acid compound. What is the conjugate base?

A

phosphorus acid : H3PO3

conjugate base: phosphite

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10
Q

phosphoric acid compound. what is the conjugate base

A

phosphoric acid H3PO4

conjugate base: phosphate

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11
Q

hypophosphorous acid

A

H3PO2

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12
Q

perphosphoric acid

A

H3PO5

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13
Q

How can PI be obtained for acidic amino acids? basic amino acids?

A

PI can be obtained by averaging 2 acidic pka values for acidic AAs, or 2 basic pka values for basic AAs.

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14
Q

what is the equivalence point for a strong acid and strong base titration?

A

7

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15
Q

equivalence point for strong acid and weak base equivalence point

A

less than 7

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16
Q

equivalence point for weak acid and strong base equivalence point

A

over 7

17
Q

an indicator must be ___ than the acid or base being titrated

A

must be weaker

18
Q

an indicator chosen for a titration should have a pka:

A

close to the pH of the expected equivalence point

19
Q

when a solution is optimally buffered, what does ph equal to?

A
ph = pka
pOH = pkb.
20
Q

what is the equality at the equivalence point? at half the equivalence point?

A

at equivalence point: [HA]=[A-]

at HALF the equivalence point: pka = pH