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CH 101 > Chapter 12: Introduction to Acids and Bases > Flashcards

Chapter 12: Introduction to Acids and Bases Flashcards

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1
Q

acids tend to

A

taste sour, react with active metals to produce H2 (g), and turn litmus red

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2
Q

bases tend to

A

taste bitter, produce solutions that feel slippery, and turn litmus blue

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3
Q

acid/base indicators

A

chemical compounds that change color in acidic, basic, or neutral environments

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4
Q

both acids and bases dissociate to form ions in aqueous solution, therefore they are

A

electrolytes

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5
Q

acids and bases that completely ionize/dissociate (100%) are

A

strong

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6
Q

acids and bases that do not completely ionize in aqueous solution are

A

weak

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7
Q

Arrhenius definition (acid)

A

an acid is a hydrogen-containing substance that dissociates to produce hydrogen ions (H+), which are typically present as H3O+ in water

acidic solutions have a higher [H3O+]

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8
Q

Arrhenius definition (base)

A

a base is a substance that dissociates to produce hydroxide ions (OH-) in aqueous solution

basic solutions have a higher [OH-]

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9
Q

neutral solutions have

A

[H3O+] = [OH-]

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10
Q

H2O can function as

A

both an acid and a base; water is essentially a non-electrolyte, but there is a small amount of dissociation

allows for the autoionization of water

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11
Q

polyprotic acids

A

can release more than one H+ into aqueous solution

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12
Q

acids that can only release one proton into solution are

A

monoprotic acids (e.g., hydrochloric acid, hydrobromic acid, and nitric acid)

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13
Q

diprotic acids such as sulfuric acid and carbonic acid can release

A

two protons

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14
Q

triprotic acids such as phosphoric acid can release

A

three protons

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15
Q

Bronsted-Lowry definition (acid)

A

an acid is a proton donor

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16
Q

Bronsted-Lowry definition (base)

A

a base is a proton acceptor

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17
Q

the ionization of weak acids is an example of an

A

equilibrium reaction

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18
Q

when describing an acid-base equilibrium, we refer to the acid and base on the right-hand side of the chemical equation as the

A

conjugate acid and conjugate base

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19
Q

the conjugate acid is formed when

A

a base gains a proton (H+); it’s what forms when a base accepts a proton

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20
Q

the conjugate base is formed when

A

an acid loses a proton; it is what remains of the acid after it has donated a proton

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21
Q

the conjugates of weak acids are

A

basic; they can act as a weak base and accept protons from water and increase the OH- concentration

22
Q

in acid-base neutralization reactions, an acid and a base combine to produce

A

water and an ionic compound (salt); the formation of water is the driving force for the neutralization reaction

double-displacement reaction

23
Q

acids react with pure metals to produce

A

hydrogen gas (single-displacement reaction)

precious metals (silver, gold, and platinum) do not react with acid

24
Q

nonmetal oxides

A

compounds that contain a nonmetal covalently bonded to one or more oxygen atoms; typically react with water to form acidic solutions

25
Q

metal oxides

A

compounds that consist of a metal element chemically bonded to oxygen; reacts with water to form basic solutions

26
Q

acids react with carbonates to produce

A

water, carbon dioxide, and a salt

27
Q

autoionization of water

A

the process in which water molecules spontaneously dissociate into hydronium ions and hydroxide ions

a water molecule donates a proton to another water molecule to form ions

28
Q

the autoionization of water yields

A

the same number of hydronium and hydroxide ions; [H3O+] and [OH-] = 1.0 x 10^-7 M

29
Q

the equilibrium constant expression for the autoionization of water is

A

Kw; Kw = [H3O+][OH-] = 1 x 10^-14 M at 25 C

30
Q

a common way to express acidity and basicity is

A

pH

31
Q

pH is a measure of

A

[H3O+] aka [H+]; pH = -log[H3O+]

-log[1.00 x 10^-7] = 7 (neutral)

32
Q

pOH =

A

-log[OH-]; since [OH-] = 1.0 x 10^-7 M, pOH = 7 (neutral)

33
Q

pH + pOH =

A

14

34
Q

if the pH decreases, the [H3O+]

A

increases; the solution is more acidic than neutral water

remember: pH is the negative logarithm of the [H3O+]

35
Q

pH < 7.00

A

the solution is acidic

36
Q

pH = 7.00

A

the solution is neutral

37
Q

pH > 7.00

A

the solution is basic

38
Q

a change of 1 pH represents

A

a tenfold change in [H3O+]; a decrease in pH by 1 unit increases [H3O+] by a factor of 10 & an increase in pH by 1 unit decreases [H3O+] by a factor of 10

39
Q

because strong acids dissociate completely, the acid molecules break apart to form

A

hydronium ions and anions (conjugate base); thus, [strong acid] is the same as [H3O+]

40
Q

titration

A

an analytical technique used to precisely determine the concentration of an acid or base by measuring the volume required for a neutralization to occur

used to determine the molarity of an unknown acid or base

41
Q

buffer

A

a solution containing a mixture of acidic and basic components that resists changes in pH; adding acid or base in a buffered solution causes a smaller pH change

42
Q

two common combinations of buffers are

A

a mixture of a weak acid and its conjugate base & a weak base and its conjugate acid

43
Q

the pH of a buffer solution depends on

A

the relative amounts of the acid and base components

44
Q

the weaker the acid,

A

the stronger the conjugate base

weak acids leave a conjugate base w/ a greater ability to accept protons

45
Q

the stronger the acid,

A

the weaker the conjugate base

46
Q

there is no reverse reaction with a strong acid because

A

the strong acid completely dissociates, going all the way to the right side of the reaction; dissociation is essentially irreversible because of the strong tendency to donate a proton

47
Q

the salt of a strong acid forms a

A

neutral solution because the conjugate base is very weak and does not interact with water in a way that would alter the pH

48
Q

the salt of a weak acid forms a

A

basic solution because the conjugate base is strong enough to react with water and increase the [OH-], thus increasing the pH

49
Q

since the salt of a weak acid is basic, a neutralization reaction can take place with

A

an acid; the conjugate base of the weak acid (present in the salt) can neutralize the H⁺ ions from the acid, reforming the weak acid in hydrolysis

50
Q

hydrolysis

A

a chemical reaction in which a substance reacts with water to produce either H+ or OH- ions, affecting the pH (acidic, basic, or neutral hydrolysis)

CH 101 (19 decks)

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