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Chemistry R120 > Chapter 16 Acid-Base Equilibria > Flashcards

Chapter 16 Acid-Base Equilibria Flashcards

(56 cards)

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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?

24
Q

What is the pH range of an acidic solution?

25
What is the pH range of a neutral solution?
pH = 7
26
What does "p" mean in pH?
to take the "-log" of
27
What are 2 ways to measure pH?
pH indicators and pH meters
28
What are pH indicators?
less accurate measurements; one color in its acid form differs from the color in its basic form
29
What is a pH meter?
accurate measurement of pH; electrodes indicate small changes in voltage within the solution
30
What is the acid dissociation constant?
(Ka) = equilibrium constant for the ionization of an acid
31
What is indicated about the acid in solution if the Ka increases?
acid in solution = strong acid
32
When calculating pH using ice tables, when can "-x" be negligible?
x > 5% of initial concentration
33
What is the base dissociation constant?
Kb = dissociation constant for WEAK bases
34
What are the 2 categories of weak bases?
neutral substances with an atom with a non-bonding e- pair that can accept an H+ ion | anions of weak acids
35
What are the 3 anions of weak acids?
ClO- | HS- | CO3-
36
What is hydrolysis?
reaction between ions and water to create OH- or H+
37
How can we determine if a salt is an acid or base?
looking at the cation and anion separately
38
Would an anion of a strong acid be basic, acidic, or neutral?
neutral because it won't react with water (ie: Cl-)
39
Would an anion of a weak acid be basic, acidic, or neutral?
basic because it will react with water to produce OH-
40
Would protonated anions of a polyphonic acid be basic, acidic, or neutral?
Ka > Kb = acidic anion | Ka < Kb = basic anion
41
Would a cation of a strong base (Group 1A and 2A) be basic, acidic, or neutral?
neutral
42
Would a polyatomic cation of a weak base be basic, acidic, or neutral?
acidic
43
Would a metal cation (transition/post-transition) be basic, acidic, or neutral?
acidic = no H atoms in these cations
44
Would a Group1A/2A cation with a strong acid anion be basic, acidic, or neutral?
neutral
45
Would a Group1A/2A cation with a weak acid anion be basic, acidic, or neutral?
basic (like the anion)
46
Would a polyatomic or metal cation (transition/post-transition) with a strong acid anion be basic, acidic, or neutral?
acidic (like the cation)
47
Would a polyatomic or metal cation (transition/post-transition) with a weak acid anion be basic, acidic, or neutral?
Ka > Kb = acidic | Ka < Kb = basic`
48
What are the 3 factors that affect acid strength?
HA bond polarity | bond strength | conjugate base (A-) stability
49
What is HA bond polarity?
must be polarized with a partial (+) on H and partial (-) on A
50
How does an increase in HA bond polarity affect acid strength?
draws more electron density from H = stronger the acid
51
What is bond strength?
weaker bonds are broken more easily = makes acid stronger
52
How does an decrease in bond strength affect acid strength?
stronger the acid
53
How does conjugate base (A-) stability affect acid strength?
more stable anion = stronger the acid (as it can easily give up the H+)
54
What are binary acids?
H--A
55
What are oxyacids?
H, O, and another nonmetal element as the central atom (like HClO4)
56
How does an oxidation number of an oxyacid affect acid strength?
as oxidation number increases = stronger the acid

Chemistry R120 (18 decks)

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