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Chemistry R120 > Chapter 16 Acid-Base Equilibria > Flashcards

Chapter 16 Acid-Base Equilibria Flashcards

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1
Q

Who is Svante Arrhenius?

A

Swedish Chemist who had his own way of defining acids and bases

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2
Q

Who defined acid-base reactions as involving the transfer of H+ ions from one substance to another?

A

Johannes Bronsted and Thomas Lowry

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3
Q

What is a hydronium ion?

A

formed by the interaction between a H+ (proton) with a water molecule = this interacts with water molecules via hydrogen bonding

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4
Q

What is amphiprotic?

A

substance that is capable of acting as an acid and a base

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5
Q

How does an amphiprotic substance act as an acid?

A

when combined with something MORE strongly basic than itself

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6
Q

How does an amphiprotic substance act as a base?

A

when combined with something MORE strongly acidic than itself

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7
Q

What are conjugate acid-base pairs?

A

acids and bases that only differ in the presence or absence of a proton

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8
Q

How is a conjugate base formed?

A

by removing a proton FROM the acid

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9
Q

How is a conjugate acid formed?

A

by adding a proton TO the base

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10
Q

What kind of conjugate base (CB) does an acid have as it becomes stronger?

A

weaker conjugate base = more easily an acid gives up a proton = less likely its conjugate base accepts the proton again

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11
Q

What kind of conjugate acid (CA) does a base have as it becomes stronger?

A

weaker conjugate acid = more easily a base accepts a proton = less likely its conjugate acid will give it up again

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12
Q

What are weak acids?

A

only partially dissociates in aqueous solutions

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13
Q

What is the leveling effect?

A

phenomenon where strong acids react with water to form H3O+ ions and strong bases react with water for form OH- ions

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14
Q

What are the 3 strong bases?

A

O2- | H- | CH3-

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15
Q

What is auto-ionization of water?

A

water spontaneously forms low concentrations of H+ ions and OH- ions by proton transfer from one water molecule to another

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16
Q

What is the equilibrium constant expression for the auto ionization of water?

A

Kw = [H3O+] [OH-}

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17
Q

What is the ion product constant?

A

Kw

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18
Q

What is the value of Kw?

A

1.00 x 10^-14

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19
Q

What is the relative concentration of ions in a basic solution?

A

[H+] < [OH-]

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20
Q

What is the relative concentration of ions in an acidic solution?

A

[H+] > [OH-]

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21
Q

What is the relative concentration of ions in a neutral solution?

A

[H+] = [OH-]

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22
Q

What is pH?

A

method of reporting H+ ion concentration

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23
Q

What is the pH range of a basic solution?

A

pH > 7

24
Q

What is the pH range of an acidic solution?

A

pH < 7

25
Q

What is the pH range of a neutral solution?

A

pH = 7

26
Q

What does “p” mean in pH?

A

to take the “-log” of

27
Q

What are 2 ways to measure pH?

A

pH indicators and pH meters

28
Q

What are pH indicators?

A

less accurate measurements; one color in its acid form differs from the color in its basic form

29
Q

What is a pH meter?

A

accurate measurement of pH; electrodes indicate small changes in voltage within the solution

30
Q

What is the acid dissociation constant?

A

(Ka) = equilibrium constant for the ionization of an acid

31
Q

What is indicated about the acid in solution if the Ka increases?

A

acid in solution = strong acid

32
Q

When calculating pH using ice tables, when can “-x” be negligible?

A

x > 5% of initial concentration

33
Q

What is the base dissociation constant?

A

Kb = dissociation constant for WEAK bases

34
Q

What are the 2 categories of weak bases?

A

neutral substances with an atom with a non-bonding e- pair that can accept an H+ ion | anions of weak acids

35
Q

What are the 3 anions of weak acids?

A

ClO- | HS- | CO3-

36
Q

What is hydrolysis?

A

reaction between ions and water to create OH- or H+

37
Q

How can we determine if a salt is an acid or base?

A

looking at the cation and anion separately

38
Q

Would an anion of a strong acid be basic, acidic, or neutral?

A

neutral because it won’t react with water (ie: Cl-)

39
Q

Would an anion of a weak acid be basic, acidic, or neutral?

A

basic because it will react with water to produce OH-

40
Q

Would protonated anions of a polyphonic acid be basic, acidic, or neutral?

A

Ka > Kb = acidic anion | Ka < Kb = basic anion

41
Q

Would a cation of a strong base (Group 1A and 2A) be basic, acidic, or neutral?

A

neutral

42
Q

Would a polyatomic cation of a weak base be basic, acidic, or neutral?

A

acidic

43
Q

Would a metal cation (transition/post-transition) be basic, acidic, or neutral?

A

acidic = no H atoms in these cations

44
Q

Would a Group1A/2A cation with a strong acid anion be basic, acidic, or neutral?

A

neutral

45
Q

Would a Group1A/2A cation with a weak acid anion be basic, acidic, or neutral?

A

basic (like the anion)

46
Q

Would a polyatomic or metal cation (transition/post-transition) with a strong acid anion be basic, acidic, or neutral?

A

acidic (like the cation)

47
Q

Would a polyatomic or metal cation (transition/post-transition) with a weak acid anion be basic, acidic, or neutral?

A

Ka > Kb = acidic | Ka < Kb = basic`

48
Q

What are the 3 factors that affect acid strength?

A

HA bond polarity | bond strength | conjugate base (A-) stability

49
Q

What is HA bond polarity?

A

must be polarized with a partial (+) on H and partial (-) on A

50
Q

How does an increase in HA bond polarity affect acid strength?

A

draws more electron density from H = stronger the acid

51
Q

What is bond strength?

A

weaker bonds are broken more easily = makes acid stronger

52
Q

How does an decrease in bond strength affect acid strength?

A

stronger the acid

53
Q

How does conjugate base (A-) stability affect acid strength?

A

more stable anion = stronger the acid (as it can easily give up the H+)

54
Q

What are binary acids?

A

H–A

55
Q

What are oxyacids?

A

H, O, and another nonmetal element as the central atom (like HClO4)

56
Q

How does an oxidation number of an oxyacid affect acid strength?

A

as oxidation number increases = stronger the acid

Chemistry R120 (18 decks)

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