Acids and Bases Flashcards

1
Q

Solutions that are acidic tend to have pHs ____ than 7.

A

Less

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2
Q

Solutions that are basic tend to have pHs ______ than 7.

A

Greater

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3
Q

At 25°C only, the pH of pure water is

A

7.

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4
Q

What do acids do in acid/base reactions?

A

Donate H+

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5
Q

What do bases do in acid/base reactions?

A

Accept H+

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6
Q

In math equations, H+ can be replaced with

A

H3O +.

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7
Q

What are the strong acids?

A

HCl
HBr
HI
HNO3
H2SO4
HClO4

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8
Q

What are the strong bases?

A

Group 1A and 2A metals bonded to OH-

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9
Q

For solutions containing weak acids only, a useful formula is

A

[H+] = sqrt([weak acid]•Ka)

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10
Q

For solutions containing weak bases acids only, a useful formula is

A

[OH-] = sqrt([weak base]•Kb)

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11
Q

Percent ionization/dissociation for weak acid formula

A

% Diss = [H+]/[weak acid]o • 100%

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12
Q

As you dilute a weak acid or weak base, the percent ionization of the weak acid or weak base

A

Increases.

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13
Q

If a salt contains a weak acid, it will make a(n) _______ solution when dissolved into.

A

Acidic

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14
Q

If a salt contains a weak base, it will make a(n) _______ solution when dissolved in water.

A

Basic

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15
Q

Electronegative atoms make weak acids _________

A

Stronger.

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16
Q

CxHy groups make weak acids

17
Q

Electronegative atoms make weak bases

18
Q

CxHy groups make weak bases

19
Q

Resonance makes a conjugate base ________ stable.

20
Q

Buffer solutions must contain a ___________________.

A

Weak conjugate acid/base pair

Ex. HCOOH and HCOO-

21
Q

pH at equivalence point in a strong acid/weak base titration

A

pH < 7 (due to CA of weak base)

22
Q

pH at equivalence point in a weak acid/strong base titration

A

pH > 7 (due to CB of weak acid)

23
Q

pH at equivalence point in a strong acid/strong base titration

24
Q

pH at equivalence point in a weak acid/weak bad titration

A

pH could be greater than, less than, or equal to 7. Determined by whichever conjugate is stronger.

25
pH = p*K*a when
[HA] = [A-] (half-equivalence point)
26
Greater buffer capacity is related to having
more moles of weak acid or weak base in buffer solution.
27
An indicator should be selected for titration that has a p*K*a close to the pH at
the equivalence point.