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chemistry 1302 gen chem 2 > chapter 14: acid base eqilibrium > Flashcards

chapter 14: acid base eqilibrium Flashcards

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1
Q

what are water-soluble ionic compounds

A

salts

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2
Q

nearly all salts are what

A

strong electrolytes

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3
Q

what is hydrolysis

A

when ions are able to react w/ water to generate H+ or OH- ions

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4
Q

how can the pH of an aqueous salt solution can be predicted

A

qualitatively by considering the ions of which the salt compos

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5
Q

what is an anion, X^-

A

conjugate base of an acid

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6
Q

what will a strong acid or base do to the pH

A

they will have no effect on the pH ( and make sure to cancel them out

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7
Q

if you have a weak acid then what is the strength of its conjugate base

A

the base is also weak

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8
Q

to what extent will acetate ion react with water and what does it do to the pH

A

react to a small extent
- increases the pH and makes it basic

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9
Q

anions w/ ionizable protons are what

A

amphoteric

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10
Q

the behavior w/ water is determined by what

A

the magnitude of Ka or Kb

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11
Q

if Ka > Kb

A

ion will cause the solution to be acidic

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12
Q

if Kb> Ka

A

the solution will be basic

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13
Q

polyatomic cations that contain one or more protons can be considered what

A

conjugate acids of weak bases

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14
Q

what can metal ions react with that will affect the pH

A

react with water to decrease the pH of an aqueous solution

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15
Q

what other ions do not affect pH

A
  • ions of alkali metals
  • heavier alkaline earth metals
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16
Q

what can cause a shift of the electron density in water

A

attraction between nonbonding electrons on O2 and and the metal

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17
Q

greater charge =

A

smaller size = more acidic

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18
Q

strong electron interaction characteristics

A
  • greater charge and smaller size
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19
Q

weak electrostatic interactions

A
  • smaller charge = larger size
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20
Q

cation is from a strong base; anion is from a strong acid

A

pH is neutral

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21
Q

cation is from a strong base; anion is from weak acid

(NaC2H3O2)

A

basic soln

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22
Q

cation is a conjugate acid of weak base; anion is from strong acid
NH4CL

A

acidic

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23
Q

what is the formula for a solution

A

cation + anion

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24
Q

cation is highly charged metal ion; anion is from strong acid
Al(NO3)

A

acidic

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25
Q

what happens when NaC2H3O2 is added to a solution

A
  • NaC2H3O2 dissociates completely
  • increase in C2H3 O2 ions
26
Q

what does an increase in C2H3O2 ions cause
HC2H3O2—> H+ + C2H3 O2

A
  • equilibrium will shift to the left
  • makes more acid
27
Q

what is the common ion effect

A

extent of the ionization of a weak electro. is decreased by adding a strong electrolyte that has an ion in common

28
Q

if you have a concentratoin of a strong acid then what is that concentration also equal to

A
  • H3O + concentration
  • use this conc. to calculate pH directly
29
Q

what is a buffer solution

A

weak conjug. acid/base pair that resist drastic changes in ph

30
Q

what can a buffer neutralization not do

A

consume one another that is why we use weak acids and bases

31
Q

what pH can you buffer a solution

A
  • at any pH
32
Q

what are the 3 ways to make an effective buffer

A
  • weak acid and salt contains conjugate weak base
  • weak base and salt that contains conjugate weak acid
  • two salts that contain different anions that correspond to the same polyprotic acid
    NaHCo3 and Na2CO3
    HCo3 = was and CO3 is wb
33
Q

what is the henderson hassbelbalch equation and what is is used for

A

pH = pKa + log (base/acid)
- calculates pH of a buffer from Ka and initial concs of the weak acid and salt of the conjug base

34
Q

what happens when a strong acid is added to a buffer

A

the H+ is consumed by X- to produce HX

35
Q

what happens when a strong base is added to a buffer

A

OH is consumed by HX to produce X

36
Q

what is buffer capacity

A

the amount of acid to base the buffer can neutralize before the pH begins to change

37
Q

what does buffer capacity depend on

A

the amount of acid and base from which the buffer is made

38
Q

if you have large amounts of conjugate acid-base pair what happens

A

the more resistant the pH is to change

39
Q

what is the pH range

A

range over which the buffer acts effectively

40
Q

when do buffers most effectively resist change

A

when the conc. of the weak acid and conjug. base are about the same
- pH = pKa

41
Q

when ph= pka what does it mean

A
  • optimal pH of any biffer
42
Q

what is a titration

A

analytical technique to calculate the conc. of a solute in a solution

43
Q

what is the standard solution

A

solution of a known concentration

44
Q

what is the equivalence point

A

point at which the two different solutions (known + unknown) are at stoichiometrically equivalent quantitties

45
Q

what are indicators

A

dyes that show a color change right past the equivalence point

46
Q

is the equivalence point found? if not what is found

A

no, the endpoint is found

47
Q

what are most indicators

A

weak acids

48
Q

what can be used to monitor the progression of a titration curve

A

a pH meter

49
Q

what are some characteristics of a strong acid-base titration

  1. how to measure pH before the addition of the base?
A
  1. before base: pH can be calculated from the conc. of the strong acid (-log)
  2. initial acid conc. starts closer to 1 and is very low and base pH is high
  3. base is added pH increases and is rapid near the equivalence point
50
Q

what is the equivalence point and what is the pH

A

moles of acid = moles of base

  • the pH = 7.00
51
Q
A
52
Q

in a strong acid-base titration what happens as more base is added, how do you find the pH

A
  • the pH levels off and pH is determined by the conc. of the excess base
53
Q

what is the end point

A

the point where the indicator changes color( approx. the equivalence point)

54
Q

what are some characteristics of a weak acid-strong base titration

A
  • initial acid starts at a higher pH
  • base is at a high pH
55
Q

in a WA-SB titration how do you determine the pH

A

the pH is determined by the acid but since it is a weak acid we need to know the Ka

56
Q

what happens prior to the equivalence point of a WA-SB titration and what happens after

A
  1. weak acid is neutralized to the weak base and the solution contains a mixture of the WA and CB
  2. after we are left with the conjugate of the WA
57
Q

what happens at the equivalence point of WA-SB

A

moles acid = moles of base

  • base reacts with acid to form a salt

pH >7 because Na+ doesn’t have an effect on pH

58
Q

what are some titration curve comparisons

A
  1. weak acid solns have a higher initial pH than strong acid of the same conc.
  2. pH change at the rapid rise near the equiv. point is smaller for a weak acid
  3. pH @ Equiv is >7 for weak acids and 7 for strong acids
59
Q

why is Ka an important factor in weak acid titrations

A
  • strength of weak acids has an effect on pH curve
  • weaker the acid = greater pH value @ equivalence point= shorter vertical region
60
Q

what are some characteristics of a strong acid-weak base titration

A
  1. goes in the other direction
  2. the initial acid pH is low and base is not that high
  3. pH @ equivalence is less than 7.00

chemistry 1302 gen chem 2 (10 decks)

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