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CHM135 > Unit 8 Acids and Bases > Flashcards

Unit 8 Acids and Bases Flashcards

1
Q

What is a bronsted Lowry acid?

A

a substance that gives hydrogen atom known as a proton donor

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2
Q

What is a bronsted Lowry base?

A

substance that receives hydrogen called proton acceptor

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3
Q

Do acids have a plus or minus sign?

A

plus sign

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4
Q

Do bases have a plus of minus sign?

A

minus sign

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5
Q

How do you identify Conjugate acid-base pairs?

A
  1. Identify two elements that look similar and underline them
  2. Identify the acid and the base, the acid usually has an H in the front, the base will have a minus sign
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6
Q

What does Acid dissociation as an equilibrium mean?

A

when the concentration of an acid and its conjugate base does not change because the forward and reverse reactions are happening at the same rate

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7
Q

What is the Ka expression used for?

A

reaction of acid in the solvent-base water

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8
Q

What is the format of the Ka expression?

A

ka=[H3O+][A-]\HA

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9
Q

What is Ka?

A

the extent to which an acid dissociates in a solution

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10
Q

How is acid strength associated with Ka?

A

A stronger acid will give a larger Ka value

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11
Q

What is Kb?

A

the extent of ionization of a weak base

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12
Q

How are base strength and Kb related?

A

the stronger the base, the stronger the Kb value

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13
Q

What does it mean by water is amphiprotic?

A

can accept and donate protons

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14
Q

Describe the chemical equation of autoionization.

A

two waters as reactants make an hydronium and a hydroxide

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15
Q

what is the kw expression?

A

Kw=[H3O+][OH-]=(1.0 x 10-7)(1.0 x 10-7) = 1.0 x 10-14

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16
Q

What is the Kw value?

A

1.0 x 10-14

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17
Q

What is a strong acid?

A

an acid that fully dissociates in water

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18
Q

What is the condition of ka value of a strong acid?

A

must be greater than 1

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19
Q

What is a weak acid?

A

acid that does not dissociate much in water

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20
Q

What is the condition of ka value of a weak acid?

A

must be less than 1

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21
Q

what is the generic formula for ka?

A

Ka=[H3O+][A-]/[HA]

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22
Q

What is the generic formula for Kb?

A

Kb=[OH-][BH+][B]

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23
Q

How are Ka and Kb related in terms of proportionality?

A

Ka and Kb are inversely proportional

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24
Q

what happens to the reaction when the base concentration is deficient?

A

the reaction will not proceed, not considered a base anymore

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25
Q

What is the conjugate of a strong acid?

A

weak base

26
Q

What is the congugate of a weak acid?

A

a strong base

27
Q

What is the congugate of a weak base?

A

strong acid

28
Q

What is the congugate of a strong base?

A

weak acid

29
Q

what is the strategy to solve this Problem: If equal concentrations of reactants and products were mixed, in which direction would the reaction proceed?

A

Strategy: figure out which side has the strongest acid. the reaction will move the opposite side of where the strong acid is

30
Q

How does polarity affect acid strength?

A

The more polar and acid is the stronger it is

31
Q

what are the trends of increased electronegativity of the periodic table?

A

the left to right and from bottom to top

32
Q

how does atom size affect acid strength?

A

the bigger the element the hydrogen atom is connected to, the more polar the bond will be and the more the acid will dissociate

33
Q

what does the degree of polarity depend on?

A

the electronegativity of the element the hydrogen atom is bonded to

34
Q

How does the number of oxygens affect acidity strength? why?

A

Acidity increases with the number of oxygen atoms because it is very electronegative

35
Q

When OH is bonded to another element called y, how does the electronegativity of y affect the acidity of the acid?

A

When OH is bonded to another element call it y, the more electronegative y is, the more acidic the acid will be

36
Q

What is the formula for the pH?

A

ph=-log[H+]

37
Q

What is the formula for the pOH?

A

pOH=-log[OH-]

38
Q

If I rearrange the pH scale formula for H+ what will it look like?

A

[H+]=10-ph

39
Q

If I rearrange the pOH scale formula for OH- what will it look like?

A

[OH-]=10-pOH

40
Q

what is pH

A

the measure of acidity

41
Q

what is the pH of the neutral solution?

A

7

42
Q

what is the pH Acidic solution?

A

less than 7

43
Q

what is the pH of a Basic solution?

A

has a pH greater than 7

44
Q

what is the formula to find pH or pOH given the value of one?

A

14=pH+pOH

45
Q

is the solution an acid or base with pOH is less than 7

A

a base

46
Q

is the solution an acid or base with pOH is greater than 7

A

an acid

47
Q

What is the formula to find the pKa?

A

pka=-log(Ka)

48
Q

What is the formula to find the pKb?

A

pkb=-log(kb)

49
Q

What is the relationship between acid strength and pKa?

A

Stronger acids give a negative or lower pKa

50
Q

What is the Leveling affect?

A

Any two strong acids will differ in acid strength, but in water, they will exhibit the same acid strength as hydronium. Same for base, instead they will inhibit the same strength as hydroxide

50
Q

What is the formula to find the kb given pkb?

A

kb=10^-pkb

50
Q

What is the formula to find the pkb?

A

pkb=-log(kb)

51
Q

What do ions of weak acids reacting with water to form?

A

Ions of weak acids react with water to form OH-

52
Q

What is salt (ionic compounds) hydrolysis?

A

when the ion reacts with water. The water molecule splits into H+ and OH-

53
Q

What do ions of strong acids react with water to form?

A

Ions of strong acids and bases do not influence pH

54
Q

What do ions of strong bases react with water to form?

A

Ions of strong acids and bases do not influence pH

55
Q

What are poor enough acids and bases considered?

A

they are not considered acids or bases at all

56
Q

Will a salt derived from a strong acid and weak base will be acidic or basic? Explain

A

A salt derived from a strong acid and weak base will be acidic due to the presence of strong acid because there are more hydronium than hydroxide ions

57
Q

If ka>kb what is the pH and the strength of the acid and the base?

A

pH<7 acid stronger than base

58
Q

If Ka<kb what is the pH and the strength of the acid and the base?

A

Ka<kb>7 base stronger than acid</kb>

59
Q

If Ka=KB, what is the pH and the strength of the acid and the base?

A

Ka=KB then pH~7

60
Q

what is the relationship between Ka and Kb?

A

they are inversely proportional

CHM135 (15 decks)

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