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Acid-Base Flashcards

1
Q

This is the earliest acid-base definition, which classifies these substances in terms of their behavior in water

A

ARRHENIUS ACID-BASE DEFINITION

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2
Q

is a substance with H in its formula that dissociates to yield H₃O⁺

A

acid - according to arrhenius

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3
Q

is a substance with OH in its formula that dissociates to yield OH⁻

A

base - according to arrhenius

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4
Q

is a substance that dissociates in aqueous medium to form or yield hydronium ions, H3O+ .

A

Arrhenius acid

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5
Q

HCl(aq) + H2O(l) → H𝟑O(aq) + Cl-

HCl is an?

A

Arrhenius acid

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6
Q

is a substance that ionizes in aqueous medium to produce hydroxide ions.

A

Arrhenius base

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7
Q

_____ acid dissociates completely into ions in water:

A

strong acid

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8
Q

A dilute solution of a strong acid contains no ____ molecules.

A

HA

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9
Q

A strong acid yields

A

→ H3O+(aq) + A-(aq)

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10
Q

A _____ acid dissociates slightly to form ions in water:

A

weak acid

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11
Q

Weak acid yields

A

⇌ H3O+(aq) + A-(aq)

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12
Q

In a dilute solution of a weak acid, most HA molecules are _________.

A

undissociated

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13
Q

Strong acid: HA(g or l) + H2O(l) → H3O+(aq) + A-(aq)

There are no ____ molecules in solution.

A

HA

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14
Q

Weak acid: HA(aq) + H2O(l) ⇌ H3O+(aq) + A-(aq)

Most HA molecules are ________.

A

undissociated (always remember na sa weak acid, reversible ang reaction kay hindi completely dissociated and HA)

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15
Q

The value of ____ is an indication of acid strength.

A

Ka

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16
Q

A large value of K means that the reaction favors the formation of

A

product (s)

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17
Q

A small value of K means that the reaction favors the

A

reactants

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18
Q

If Ka > 1, then the acid is

A

strong

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19
Q

If Ka<1,then the acid is

A

Weak

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20
Q

If Kb > 1, then the base is

A

strong

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21
Q

If Kb<1,then the base is

A

weak

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22
Q

(HCl, HBr, and HI) are strong or weak? Why?

A

STRONG. Because they are hydrohalic acids

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23
Q

oxoacids in which the number of O atoms exceeds the number of ionizable protons by two or more (strong or weak?)

A

Strong

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24
Q

HNO3

A

3-1=2 ; STRONG

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25
H2SO4
4-2=2 ; STRONG
26
HClO4
4-1=3 ; STRONG
27
It is the only hydrohalic acid that is weak
HF
28
acids in which H is not bonded to O or to a halogen
Weak acids
29
HCN
Weak acid (not bonded to O or halogen)
30
oxoacids in which the number of O atoms equals or exceeds the number of ionizable protons by one
Weak
31
HClO
1=1 ; Weak
32
HNO2
2-1=1 ; weak
33
carboxylic acids, which have the general formula RCOOH
Weak acids
34
CH3COOH
Weak because of COOH
35
C6H5COOH
Weak because of COOH
36
water-soluble compounds containing O2- or OH- ions. (Strong or weak)
Strong base
37
M2O or MOH, where M = Group 1A(1) metal (Strong or Weak Base)
Strong
38
Group 1A(1) metals
(Li, Na, K, Rb, Cs)
39
MO or M(OH)2 where M = group 2A(2) metal ( Strong or weak base)
STRONG BASE
40
group 2A(2) metal
(Ca, Sr, Ba)
41
ammonia (NH3) - strong or weak base?
Weak
42
amines - strong or weak base?
Weak base
43
A _______ completely transfers its protons to water, leaving essentially no undissociated molecules in solution. Its conjugate base has a negligible tendency to accept protons in aqueous solution.
strong acid
44
(The conjugate base of a ______ acid shows negligible basicity.)
strong acid
45
A ________only partially dissociates in aqueous solution and therefore exists in the solution as a mixture of the undissociated acid and its conjugate base.
weak acid
46
The conjugate base of a _______ shows a slight ability to remove protons from water.
weak acid
47
The conjugate base of a weak acid is a ____ base.
weak base
48
A substance with ________ contains hydrogen but does not demonstrate any acidic behavior in water
negligible acidity
49
The conjugate base of a substance with negligible acidity is a ______
strong base
50
means a substance can act as either an acid or a base
Amphiprotic
51
It is amphiprotic based on the concept of
Bronsted-Lowry theory
52
Also called “self-ionization of water”
Autoionization of Water
53
an ionization reaction in pure water or in an aqueous solution, in which a water molecule, H2O, deprotonates (loses the nucleus of one of its hydrogen atoms) to become a hydroxide ion, OH−.
Autoionization of Water
54
means the ability of a substance to react either as an acid or as a base.
Amphoteric
55
amphoteric based on the concept of
Lewis theory
56
Kw = [H3O+][OH-] = _______ (at 25°C)
1.0x10^-14
57
T or F | A change in [H3O+] causes an inverse change in [OH-], and vice versa.
Truee
58
[H3O] > [OH-]
acidic solution
59
[H3O] = [OH]
neutral solution
60
[H3O] < [OH]
basic solution
61
The ___ of a solution indicates its relative acidity:
pH
62
pH < 7.00
acidic solution
63
pH = 7.00
neutral solution
64
pH > 7.00
basic solution
65
The higher the pH, the lower the [H3O] and the less ___ the solution.
acidic
66
scales express the acidity and basicity of dilute aqueous solutions.
pH and pOH
67
is known as the power of hydrogen or the measure of hydrogen ion [H+] or hydronium ion [H3O+] concentration.
pH
68
is the measure of hydroxide ion [OH-] concentration.
pOH
69
• These expressions are analogous to the expression for pH. We derived it to express the concentrations in a more convenient way using whole numbers.
pKa and pKb
70
• pKa =
-log Ka
71
• pKb =
-log Kb
72
• The smaller the value of pKa, the ______ the acid
stronger
73
The smaller the value of pKb, the ______ the base.
stronger
74
An acid is a proton donor, any species that donates an H+ ion. • An acid must contain H in its formula.
Brønsted-Lowry Acid
75
A base is a proton acceptor, any species that accepts an H+ ion. • A base must contain a lone pair of electrons to bond to H+.
Brønsted-Lowry Base
76
An acid-base reaction is a ______-transfer process (Bronsted Lowry)
proton
77
• is a substance that is a proton donor.
Brønsted-Lowry acid
78
is a substance that is a proton acceptor.
Brønsted-Lowry base
79
A ______ is any species that donates an electron pair to form a bond.
Lewis base
80
A _____ is any species that accepts an electron pair to form a bon
Lewis acid

Anachem (4 decks)

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