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Chemistry I > Aqueous Ionic Equilibrium > Flashcards

Aqueous Ionic Equilibrium Flashcards

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1
Q

Acidosis:

A

a conditions in which the acid affects the equilibrium between hemoglobin and oxygen

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2
Q

A buffer resists:

A

pH change

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3
Q

How does a buffer resist pH change

A

it neutralizes added acid or added base

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4
Q

a buffer contains

A

significant amounts of weak acid/weak base and its conjugate base/acid

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5
Q

in a buffer, the acid does what

A

neutralizes added base

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6
Q

common ion affect

A

tendency for a common ion to decrease the solubility of an ionic compound or to decrease the ionization of a weak acid or base

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7
Q

why is “x is small” approximation valid

A

so little of a weak acid ionizes compared to its initial concentration

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8
Q

in a solution in which acid and conjugate base concentrations are equal, [H3O+] is equal to what?

A

Ka

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9
Q

Henderson-Hasselbalch equation:

A

pH=pKa+log([bas]/[acid])

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10
Q

the pH of a buffer increases with an increase in…

A

in the amount of base relative to the amount of acid

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11
Q

Henderson-Hasselbalch equation only works if:

A

the x is small approximation is valid

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12
Q

x is small approximation applies when what 2 things are true

A

1) the initial concentrations of acids (and/or bases) are not too dilute
2) the equilibrium constant is fairly small

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13
Q

for x is small approximations, initial concentrations of acids and conjugate bases should be at least how much greater than the equilibrium constant?

A

10^2-10^3

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14
Q

calculating the pH of buffer solution requires breaking the problem into what 2 parts:

A

1) stoich calculation
2) equilibrium calculation

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15
Q

in a single buffer solution, BLANK is the same for boht the acid and the base

A

volume

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16
Q

adding a small amount of strong acid to a buffer converts a stoichiometric amount of the base to the conjugate acid and does what to the pH of the buffer?

A

decreases the pH of the buffer (adding acid decreases the pH)

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17
Q

adding a small amount of strong base to a buffer converts a stoichiometric amount of the acid to the conjugate base and does what to the pH?

A

increases the pH of the buffer (adding base increases the pH)

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18
Q

adding acid creates more BLANK, adding base creates more BLANK

A

acid, base

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19
Q

capacity of buffer:

A

how much added acid or base it can effectively neutralize

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20
Q

range of a buffer

A

the pH range over which a particular acid and its conjugate base can be effective

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21
Q

when is a buffer most effective? (in terms of relative concentrations)

A

when concentrations of acid and conjugate base are equal

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22
Q

For a buffer to be reasonably effective, relative concentrations of acid and conjugate base should not differ by..

A

more than a factor of 10

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23
Q

when can be said of a buffer solution when concentrations of acids and bases are high?

A

the buffer is effective

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24
Q

the more dilute the buffer components..

A

the less effective the buffer

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25
Q

the lowest pH for an effective buffer occurs when?

A

the base is one tenth as concentrated as the acid

26
Q

the highest pH for an effective buffer occurs when?

A

the base is ten times as concentrated as a acid

27
Q

what would be an effective buffering range system for a weak acid with pKa of 5.0?

A

4.0-6.0

28
Q

buffer capacity increases with:

A

increasing absolute concentrations of buffer components

29
Q

Equivalence point

A

the point in the titration when the number of moles of base is stoichiometrically equal to the number of moles of acid; neither reactant is in excess

30
Q

when titrating a weak acid with a strong base, between the initial pH and the equivalence point, what happens to the solution?

A

it becomes a buffer

31
Q

for the titration of a weak acid with strong base, what occurs at exactly the half-way equivalence point?

A

pH=pKa

32
Q

for the titration of weak acid with strong base, what happens at the equivalence point?

A

the acid has been converted into its conjugate base

33
Q

what is Ksp

A

the measure of the solubility of a compound

34
Q

what is molar solubility?

A

solubility in units of moles per liter

35
Q

True/False: Ksp is the molar solubility

A

FALSE: Ksp is the solubility product constant

36
Q

True/False: Ksp is dependent on temperature

A

true

37
Q

true/false: solubility depends on the kind of solution

A

true

38
Q

relationship between Ksp nd molar solubility depends on:

A

the stoichiometry of the dissociation reaction

39
Q

the solubility of an ionic compound is BLANK in a solution containing a common ion than in pure water

A

lower

40
Q

if pH is high, the rxn will shift:

A

left

41
Q

if pH is low, rxn will shift:

A

right

42
Q

the solubility of an ionic compound with a strongly basic or weakly basic anion BLANK with increasing acidity

A

increases

43
Q

BLANK, BLANK, and BBLANK are more soluble in acidic water than in pure water

A

hydroxides, sulfides, and carbonates

44
Q

what is the differemce between Q and Ksp

A

is the value of this product at equilibrium only, whereas Q is the value of the product under any conditions

45
Q

If more solid is added to an unsaturated solution, what will happen?

A

it will dissolve

46
Q

Selective Precipitation:

A

a process involving the addition of a reagent that forms a precipitate with one of the dissolved cations but not the others

47
Q

The difference in values required for selective precipitation is:

A

at least 10^3

48
Q

what can selective precipitation be used for?

A

to determine which metal ions are present in an unknown solution

49
Q

Qualitative analysis involves:

A

finding the kind of ions present in the solution

50
Q

quantitative analysis:

A

amounts of substances in a solution or mixture.

51
Q

Transition metal ions tend to be good

A

electron acceptors (Lewis acid)

52
Q

complex ion:

A

ontains a central metal ion bound to one or more ligands

53
Q

ligand:

A

neutral molecule or ion that acts as a Lewis base with the central metal ion

54
Q

formation constant (Kf) :

A

The equilibrium constant associated with the reaction for the formation of a complex ion

55
Q

if Kf is large, then:

A

formation of the complex ion is highly favored

56
Q

the solubility of an ionic compound containing a metal cation that forms complex ions BLANK in the presence of Lewis bases that complex with the cation

A

increases

57
Q

what are the most common Lewis bases that increase the solubility of metal cations?

A

NH3, CN-, OH-

58
Q

why do metal hydroxides become more soluble in acidic solutions?

A

they can act as bases and react with H3O+

59
Q

The ability of an amphoteric metal hydroxide to act as an acid does what to its solubility in basic solution?

A

increases

60
Q
A

Chemistry I (16 decks)

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