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CHM 1040 > ch 16 > Flashcards

ch 16 Flashcards

1
Q

Arrhenius

A

Scientist who postulated that acids produce H+ions in aqueous solution, whereas bases produce OH–ions

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2
Q

Brønsted–Lowry model

A

States that acids are proton (H+) donors, bases are proton acceptors
HCl (acid) + H2O (base) → Cl–+ H3O+

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3
Q

Conjugate base

A

everything that remains of the acid molecule after a proton is lost

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4
Q

Conjugate acid

A

formed when a proton is transferred to the base

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5
Q

Conjugate acid–base pair

A

Consists of two substances related to each other by the donating and accepting of a single proton

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6
Q

acids in water

A

Water acts as a base accepting a proton from the acid

- Forms hydronium ion (H3O+)

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7
Q 
Which of the following pairs represents a conjugate acid–base pair? 
a) HCl, HNO3
b )H3O+, OH–
c) H2SO4, SO42–
d) HCN, CN–
A

d) HCN, CN–

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8
Q

strong acid

A
  • Completely ionized or completely dissociated HA(aq) + H2O(l) → H3O+(aq) + A–(aq)
  • breaks apart 100%
  • forward rxn predominates
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9
Q

weak acid

A
  • Most of the acid molecules remain intact HA(aq) + H2O(l) ← H3O+(aq) + A–(aq)
  • A- is a much stronger base than H2O
  • strength of the conjugate base compared with that of water
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10
Q

Strong acids contain relatively __ conjugate bases

A

weak

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11
Q

what makes up a base?

A

type 1 and 2 metals + OH-

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12
Q

common strong acids

A
  • Sulfuric acid, H2SO4
  • Hydrochloric acid, HCl
  • Nitric acid, HNO3
  • Perchloric acid, HClO4
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13
Q

Oxyacids

A

Acidic proton is attached to an oxygen atom

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14
Q

Organic acids

A
  • Have a carbon atom backbone and commonly contain the carboxyl group
  • typically weak acids
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15
Q

weak acids have a __ base

A

strong

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16
Q 
Consider a 1.0 M solution of HCl
• Order the following from strongest to weakest base and explain your answer
– H2O(l)
– A–(aq) (from weak acid HA) 
– Cl–(aq)
A

A-, H2O, Cl-

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17
Q

water is _

A

amphoteric

- can be both an acid (H3O+) and a base (OH-)

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18
Q

at 25ºC, Kw =

A

Kw = [H+] [OH-] = 1.0 x 10^-14

*no matter what the solution contains

19
Q

[H+] = [OH–]

A

neutral solution

20
Q

[H+] > [OH–]

A

acidic solution

21
Q

[H+] < [OH–]

A

basic solution

22
Q

in an acidic, basic, or neutral solution Kw always equals

A

Kw = [H+][OH–] = 1.0 × 10^-14

23
Q

In the context of an acidic aqueous solution, which of the following statements is correct?

a) [H+] < 1.0 × 10^-7 M
b) [H+] > 1.0 x 10^-7 M
c) [OH–] > 1.0 × 10^-7 M
d) [H+] < [OH-]

A

b

24
Q

an acid/base reaction is also called a

A

neutralization reaction

25
Q

pH =

A

− log [H+]

26
Q

pH scale

A

Provides a convenient way to represent solution acidity

27
Q

as [H+] increases, pH __

A

decreases

28
Q

sig figs

A

The number of decimal places in the log is equal to the number of significant figures in the original number

29
Q

pH range

A

7 is neutral
> 7 is basic
< 7 is acidic
*The lower the pH, the more acidic the solution

30
Q

pH scale

A

scale is from 0-14

  • acidic: 0-6.9
  • neutral: 7
  • basic: 7.1-14
31
Q

pOH =

A
  • log [OH-]
32
Q

[H+] =

A

10^-pH

33
Q

[OH-] =

A

10^-pOH

34
Q

pH + pOH =

A

14

35
Q

[H+] [OH-] =

A

1.0 x 10^ -14

36
Q

calculate the pH for 1.0×10^-4 M H+

A

4.00

pH = –log[H+] = –log(1.0 × 10–4 M) = 4.00

37
Q

calculate the pH for 0.040 M OH–

A

12.60

38
Q

The pH of a solution is 5.85. What is the [H+] for this solution?

A

[H+] = 1.4 × 10^-6 M

39
Q

calculate the pOH for 1.0×10^-4 M H+

A

10.00

40
Q

calculate the pOH for 0.040 M OH–

A

1.40

41
Q

The pH of a solution is 5.85. What is the [OH–] for this solution?

A

7.1 × 10^-9 M

42
Q

Consider an aqueous solution of 2.0 ×10–3 M HCl. What is its pH?

A

2.70

43
Q

Calculate the pH of a 1.5 ×10–11 M solution of HCl

A

7.00

44
Q

Calculate the pH of a 1.5 ×10–2 M solution of HNO3

A

1.82

CHM 1040 (6 decks)

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