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Chem 23 > Acid-Base Titrations > Flashcards

Acid-Base Titrations Flashcards

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1
Q

pH meter measures the _______ produced in the solution

A

voltage

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2
Q

blue paper turns red at pH?

A

<5

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3
Q

They defined acid-base reactions as processes that involve the transfer of proton (H+) from one substance to another. The one which donates the proton is the acid while the one that accepts the proton is the base.

A

Johannes Brønsted and Thomas Lowry

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4
Q

red paper turns blue at pH?

A

8

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5
Q

These are aqueous systems that tend to resist changes in pH when small amounts of acid (H⁺) or base (OH⁻) are added

A

Buffers

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6
Q

are important because it tells you the pH of the solution at the equivalence point

A

Titration Curves

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7
Q

CH3COOH has a conjugate base pair

A

CH3COO-

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8
Q

If [H3O+] is higher, then it is

A

acidic

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9
Q

Weak acid and a Conjugate base in a sol’n will give you

A

Buffer Solution

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10
Q

For less accurate method, one can use this to measure the pH of a solution

A

litmus papers

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11
Q

For more accurate measurements, a ___________ is used which measures the voltage produced in the solution.

A

pH meter

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12
Q

The one that accepts the proton is the

A

Base

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13
Q

What happens to pH at equivalence point?

A

changes drastically so the curve is somewhat vertical at equivalence point

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14
Q

have two ionizable protons

A

Diprotic acids

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15
Q

Since strong acids and bases completely dissociates in solution, the equilibrium concentrations of H3O+ (for acids) and OH- (for bases) are?

A

equal to their initial concentrations

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16
Q

pH range where the buffer is most effective in resisting pH change

A

Buffer Range

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17
Q

The only difference between conjugate pairs is the transfer of

A

H+

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18
Q

The one which donates the proton is the

A

Acid

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19
Q

One common example of amphiprotic substances

A

water

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20
Q

A solution in which [H3O+] is equal to [OH-] is called

A

Neutral

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21
Q

encompass all acids containing more than one ionizable H

A

polyprotic acids

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22
Q

This property of water where it can act as either a Bronsted-Lowry acid or a Bronsted-Lowry base is called

A

autoionization

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23
Q

He defined acids as substances that, when dissolved in pure water, increase the concentration of H+ ions, and bases are those that increase the concentration of OH− ions.

A

Svante Arrhenius

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24
Q

It completely dissociates in solution

A

strong acids and strong bases

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25
Q

plots the pH of the solution against the volume of titrant added

A

Titration Curves

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26
Q

acids as substances, when dissolved in pure water, increase the concentration of H+ ions, and bases are those that increase the concentration of OH− ions.

A

Arrhenius Definition

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27
Q

They proposed a more general description for acids and bases.

A

Johannes Brønsted and Thomas Lowry

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28
Q

indicates the end point of the titration

A

Acid-Base Indicators

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29
Q

The equilibrium constant of the weak base is therefore called the

A

base-dissociation constant, Kb

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30
Q

A proton donor and its corresponding proton acceptor make up a

A

conjugate acid-base pair

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31
Q

The buffering power at midpoint is

A

maximal

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32
Q

acts in the cytoplasm of all cells

A

Phosphate buffer system

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33
Q

at half equivalence point, you will have

A

Buffer Solution

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34
Q

There are substances that are capable of donating and accepting protons called

A

Amphiprotic substances

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35
Q

This equilibrium constant of weak acid is called the

A

acid-dissociation constant, Ka

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36
Q

higher [OH-] is considered

A

basic

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37
Q

NH3 has a conjugate acid pair

A

NH4+

38
Q

These are mixtures of weak acids and their conjugate bases

A

Buffer systems

39
Q

In all acid-base reactions, the products will always be the ________________ of the other

A

conjugate pair

40
Q

The pH range of your indicator must be near the _____________________

A

Equivalence Point

41
Q

The higher the value of Ka

A

the stronger the acid

42
Q

This property of water where it can act as either a

A

Bronsted-Lowry acid or a Bronsted-Lowry base

43
Q

solutions containing a weak acid and its conjugate base, or a weak base and its conjugate acid

A

Acid-Base Indicators

44
Q

pH of an acidic solution

A

< 7.00

45
Q

pH of a neutral solution

A

= 7.00

46
Q

pH of a basic solution

A

> 7.00

47
Q

[H+][(M) of an acidic solution

A

> 1.0 x 10^-7

48
Q

[H+][(M) of a neutral solution

A

= 1.0 x 10^-7

49
Q

[H+][(M) of a basic solution

A

< 1.0 x 10^-7

49
Q

[OH-][(M) of an acidic solution

A

< 1.0 x 10^-7

50
Q

[OH-][(M) of a basic solution

A

> 1.0 x 10^-7

51
Q

[OH-][(M) of a neutral solution

A

= 1.0 x 10^-7

52
Q

pH + pOH = pKw= ?

A

14

53
Q

the equilibrium concentrations of H3O+ (for acids) and OH- (for bases) are equal to their

A

initial concentrations

54
Q

The higher the value of Ka, the __________ the acid.

A

stronger

55
Q

where HA is a weak acid and its conjugate base is A-, the equilibrium constant is called the?

A

acid-dissociation constant, Ka

56
Q

where HB is the conjugate acid of the base, the equilibrium constant expression is called the

A

base-dissociation constant, Kb

57
Q

the higher the value of Kb, the __________ the base

A

stronger

58
Q

have two ionizable protons

A

diprotic acids

59
Q

encompass all acids containing more than one ionizable H

A

polyprotic acids

60
Q

The stronger the acid, the __________ its pKa

A

lower

61
Q

the stronger the base, the ___________ its pKa

A

higher

62
Q

examples of strong acids

A

Perchloric acid
Chloric acid
Hydrobromic acid
Hydrochloric acid
Hydroiodic acid

63
Q

examples of strong bases

A

Potassium hydroxide
Lithium hydroxide
Rubidium hydroxide
Sodium hydroxide
Strontium hydroxide

64
Q

These are aqueous systems that tend to resist changes in pH when small amounts of acid (H⁺) or base (OH⁻) are added

A

Buffers

65
Q

where the buffer is most effective in resisting pH change

A

Buffer range - pH range

65
Q

These are mixtures of weak acids and their conjugate bases.

A

Buffer systems

66
Q

The buffering power at midpoint is

A

maximal

67
Q

A proton donor and its corresponding proton acceptor make up a

A

conjugate acid-base pair

68
Q

The only difference between conjugate pairs is the transfer of

A

H+

68
Q

In all acid-base reactions, the products will always be the ____________________ of the other.

A

conjugate pair

69
Q

expression that relates pH, pKa, and buffer concentration

A

Henderson-Hasselbalch Equation

69
Q

these are equal at midpoint

A

pH and pKa

69
Q

Henderson-Hasselbalch equation also allows us to calculate ________, given pH and the molar ratio of proton donor and acceptor

A

pKa

70
Q

Henderson-Hasselbalch equation also allows us to calculate ________, given pKa and the molar ratio of proton donor and acceptor

A

pH

70
Q

Henderson-Hasselbalch equation also allows us to calculate the __________________________, given pH and pKa

A

molar ratio of proton donor and acceptor

71
Q

__[buffer], ↓ΔpH, ↑ buffer capacity

A

↑

71
Q

factors affecting buffer capacity

A
  1. concentration of the two buffer components
  2. pH
72
Q

↑[buffer], __ΔpH, ↑ buffer capacity

A

↓

73
Q

↑[buffer], ↓ΔpH, __buffer capacity

A

↑

74
Q

buffer is most effective (ΔpH) when the acid is ________ since it gives greater capacity to neutralize the added base

A

higher

75
Q

buffer is most effective (ΔpH) when the acid is higher since it gives ___________________ to neutralize the added base

A

greater capacity

76
Q

acts in the cytoplasm of all cells, consists of H2PO4⁻ as proton donor and HPO42−as proton acceptor:

A

phosphate buffer system

76
Q

Blood plasma is buffered in part by the bicarbonate system, consisting of carbonic acid (H2CO3) as proton donor and bicarbonate (HCO3⁻) as proton acceptor

A

bicarbonate system

76
Q

these are two especially important biological buffers

A
  1. Phosphate buffer system
  2. Bicarbonate system
77
Q

proton donor in phosphate buffer system

A

H2PO4-

78
Q

proton acceptor in phosphate buffer system

A

HPO4^2-

79
Q

proton donor in bicarbonate system

A

H2CO3

80
Q

proton acceptor in bicarbonate system

A

HCO3-

81
Q

Titration curves are important because it tells you the pH of the solution at the?

A

equivalence point

82
Q

solutions containing a weak acid and its conjugate base, or a weak base and its conjugate acid

A

acid-base indicators

83
Q

The pH range of your indicator must be near the?

A

equivalence point

Chem 23 (7 decks)

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