Chemistry Unit #8: Acids and Bases .............. Test on April 19, 2017 Flashcards
1
Q
What is the acid name of H₃PO₄?
A
Phosphoric acid
2
Q
Is F⁻ an acid or a base? (In terms of Brønsted-Lowry)
A
A base because it can accept a proton?
3
Q
Define hydroxonium ion
A
When H⁺ reacts with water to create the hydrate H₃O⁺
H⁺ + H₂O ⇌ H₃O⁺
H⁺ or H₃O⁺ is a hydroxonium/hydronium ion
4
Q
Who wrote “Experimental History of Colours”
A
Robert Doyle wrote “Experimental History of Colours”
5
Q
Is HF a strong or weak acid/base?
A
Weak acid
6
Q
Is HNO₂ a strong or weak acid/base?
A
Weak acid
7
Q
Weak bases are _____ electrolytes
A
weak
8
Q
What is the acidic name of HNO₂?
A
nitrous acid
9
Q
What are problems associated with using indicators? 4
A
People do not always agree on colours
Most people only detect 1:10 colour ratio changes
Adding yellow to red will not be detectable until you have 1 part yellow to 9 parts red
Samples tested must be in solution
Adding too much will change the pH
Solutions must be clear and colourless
Coloured solutions affect indicator colour
Some indicators may react with sample
Change in composition will change colour
10
Q
Strong acids are _____ electrolytes
A
strong
11
Q
Define electrolyte
A
When an ionic substance creates an ion in a solution
12
Q
A
13
Q
Define Alkali
A
A base that is soluble in water
14
Q
Metal oxides mixed with water form……?
A
bases
15
Q
Is this chemical reaction, is the acid monoprotic or diprotic?
H₂SO₄(aq) ⇒ 2H⁺(aq) + SO₄²⁻(aq)
A
Diprotic because when it dissociated, the acid released 2 H⁺
16
Q
For diprotic acids, the second proton released is always ____ than the first.
A
Weaker
17
Q
When acids undergo a neutralization reaction with bases, what forms when the base is a carbonate?
A
Salt, carbon dioxide and water
18
Q
In the chemical equation of NH₃ + H₂O ⇒ NH₄ + OH⁻, since NH₄ is the CA, that makes NH₃ the ____
A
Base. Water is then the acid.
19
Q
A pH of 1 is ______ times stronger than a pH of 3
A
A pH of 1 is 100 times stronger than a pH of 3
20
Q
People do not always agree on colours. Most people only detect _____ ratio colour ratio changes
A
People do not always agree on colours. Most people only detect 1:10 colour ratio changes
21
Q
Define Strong Acids 2
A
Strong bases completely dissociate (split up) into ions in an aqueous solution
They release hydroxide ions in an aqueous solution
NaOH ⇒ Na⁺ + OH⁻
22
Q
A pH of 1 is _____ times stronger than a pH of 2
A
A pH of 1 is 10 times stronger than a pH of 2
23
Q
What is the points for Temperature as one of the ways we can distinguish between a strong and a weak acid?
A
Temperature
A reaction between an acid and a substance like a reactive metal is exothermic and the strong acid will release more energy.
24
Q
Is the chemical reaction of BF₃ + NH₃ a Lewis definition or a Brønsted-Lowry definition?
A
a Lewis definition because the BF₃ acid’s valence electron and the NH₃ base’s valence electron is already full.
25
What is a pH scale? 2 - 4
A pH scale is a way of expressing the strengths of acids and bases.
Instead of using very small numbers, we just use the NEGATIVE power of 10 on the Molarity of the H⁺ (or OH⁻) ion.
A pH of 1 is 10 times stronger than a pH of 2
A pH of 1 is 100 times stronger than a pH of 3
26
27
28
What is the equilibrium constant of water, {H₂O(l) ⇌ H⁺(aq) + HO⁻(aq)}?
Kc = 1 \* 10⁻¹⁴
29
All acids release _______ \_\_\_\_\_ into solution
Hydrogen ions
30
Brønsted-Lowry Acids and Bases contain \_\_\_\_\_-bonding pair of electrons
Non
31
32
Strong acids have _____ conductivity
strong
33
An acid of pH = 2 release _______ H⁺ into the solution than an acid of pH = 3
An acid of pH = 2 release more H⁺ into the solution than an acid of pH = 3
34
What is the Lewis definition of an Acid?
A substance that can accept an electron pair
35
How do you calculate pH? 1 - 3
pH = -log [H⁺(aq)]
Or When working backwards;
[H⁺(aq)] = antilog (-pH)
Or
[H⁺(aq)] = 10⁻ᵖᴴ
36
What are the indicators inside the Universal indicator? 4
Methyl orange
Methyl red
Bromothymol blue
Phenolphthalein
37
Define Arrhenius Acid
Substance that increases the concentration of H⁺ in aqueous solution.
38
Adding yellow to red will not be detectable until you have 1 part yellow to __ parts red
Adding yellow to red will not be detectable until you have 1 part yellow to 9 parts red
39
Is this chemical reaction, is the acid monoprotic or diprotic?
HCI(aq) ⇒ H⁺(aq) + CI⁻(aq)
Monoprotic because when it dissociated, the acid could only release 1 H⁺
40
What is the Brønsted-Lowry definition of an Acid?
A proton (H⁺) donor
The proton is really just a hydrogen atom that has lost it's electron!
41
What are the 5 common examples of strong monoprotic acid?
HNO₃,
HBr,
HI,
HCIO₄
and H₂SO₄
42
Weak bases can react with water to form ______ ions in solution
Hydroxide
43
What is the Brønsted-Lowry definition of an Base?
A proton (H⁺) acceptor
The proton is really just a hydrogen atom that has gained it's electron!
44
Most acids consist of hydrogen and an \_\_\_\_\_\_
anion
45
Is a Lewis acid an electrophile or nucleophile?
a Lewis acid is an electrophile because the H⁺ is positive and it is attracted to the negative compound like CI⁻
46
Strong acids ________ dissociate
Completely (Note the yield arrow: We use ⇒)
47
Most bases consist of a ______ with a hydroxide
Most bases consist of a cation (metal positively charged ion) with a hydroxide
48
Define Equimolar
Refers to when two solutions containe the same number of moles
49
Is a Lewis base an electrophile or nucleophile?
a Lewis base is a nucleophile because the OH⁻ is negative and it is attracted to the positive compound like Na⁺
50
Is H₂SO₄ a strong or weak acid/base?
Strong acid
51
Name two natural acid-base indicators
Red cabbage juice
Various teas
52
[H⁺] = [HO⁻] = ______ M for pure water
Kc = 1 \* 10⁻⁷
53
When acids react with precious metals, what forms?
Nothing because precious metals do not react with the acid
54
Strong bases have _____ conductivity
strong
55
What is the Lewis definition of a Base?
A substance that can donate an electron pair
56
Is HBr, a strong or weak acid/base?
Strong acid
57
When acids undergo a neutralization reaction with bases, what forms when the base is a hydroxide?
Salt and water
58
Is ammonia a strong or weak acid/base?
Weak base
59
When acids and bases were identified by taste, what do bases taste like?
bitter
60
61
[H⁺] = [\_\_\_\_] = Kc = 1 \* 10⁻⁷ M for pure water
HO⁻
62
Define Weak Bases
Weak bases slightly dissociate (split up) into ions in an aqueous solution
63
64
Identify the acid, base, conjugate acid and conjugate base. H₂PO₄⁻ + HCO₃⁻ ⇌ HPO₄⁻² + H₂CO₃
H₂PO₄⁻ ----- A
HCO₃⁻ ----- B
HPO₄⁻² ----- CB
H₂CO₃ ----- CA
65
Are group 1 hydroxides, metal hydroxides with one valence electron, like NaOH a strong or weak acid/base?
Strong base
66
Is NaH an ionic acid?
No because it will release H⁻
67
68
Most acids consist of ________ and an anion
hydrogen
69
In equimolar solutions, which has a higher pH? A weak or strong acid?
A weak acid has a higher pH than a strong acid of equal concentration because not all of the hydrogen ions have dissociated
70
71
Strong bases are _____ electrolytes
strong
72
Define Arrhenius base 2
Substance that increases the concentration of OH⁻ in aqueous solution.
Substance that neutralizes an acid by removing H⁺ in aqueous solution.
73
What metals do not react with acids?
Cu(s), Ag(s), Au(s) They are called 'noble metals'
74
What is the points for Conductivity as one of the ways we can distinguish between a strong and a weak acid?
Conductivity
A weak acid does not conduct electricity as well as a strong acid.
A dimly lit bulb will mean it is a weak acid because a strong acid will a have brightly dim bulb because it has more ions.
75
What are the ways we can distinguish between a strong and a weak acid? 4
Temperature
A reaction between an acid and a substance like a reactive metal is exothermic and the strong acid will release more energy.
Bubbling
A reaction between an acid and a substance like metal will bubble, releasing hydrogen and the strong acid will bubble more and release hydrogen.
Reaction time
A weak acid reacts more slowly than a strong acid.
A strong reacts more faster than a weak acid.
Conductivity
A weak acid does not conduct electricity as well as a strong acid.
A dimly lit bulb will mean it is a weak acid because a strong acid will a have brightly dim bulb because it has more ions.
76
Since acids are ionic substances, they _______ in water.
Since acids are ionic substances, they dissociate in water.
77
Strong acids have conjugate bases that will….. 2
Strong acids have conjugate bases that will not reform the acid
The conjugate bases will act neutral
78
What yield arrow do we use when there is a weak acid/base reacting?
⇌
79
When acids undergo a neutralization reaction with bases, what forms when the base is an ammonia?
salt
80
81
82
Are amines a strong or weak acid/base?
Weak base
83
Identify the acid, base, conjugate acid and conjugate base. KHCO₃ + KH₂PO₄ ⇌ H₂CO₃ + K₂HPO₄
KHCO₃ ----- B
KH₂PO₄ ----- A
H₂CO₃ ----- CA
K₂HPO₄ ----- CB
84
Is C₁₂H₂₂O₁₁ an ionic base?
No
85
[\_\_\_\_\_] = [HO⁻] = Kc = 1 \* 10⁻⁷ M for pure water
--\>
H⁺
86
Most bases consist of a cation (metal positively charged ion) with a \_\_\_\_\_\_\_
Most bases consist of a cation (metal positively charged ion) with a hydroxide
87
Is CH₃OH an ionic base?
No
88
When acids undergo a neutralization reaction with bases, what forms when the base is a metal oxide?
Salt and water
89
90
What is the products of CO₃(aq) + H₂O(l) ⇌
CO₃(aq) + H₂O(l) ⇌ HCO₃⁻(aq) + OH⁻(aq)
91
What was lichen Rocella could be used as? 3
A purple dye
Add fermented urine (base) to produce an orchid blue dye
Acidified to produce a red dye
92
What is chemical formula of phosphoric acid?
H₃PO₄
93
Weak bases have _____ conductivity
weak
94
Pure water _____ dissociates
Slightly
95
If H₂CO₃ is a weak acid, that makes HCO₃⁻¹ a strong or weak acid?
Weaker acid
96
What is the points for Reaction time as one of the ways we can distinguish between a strong and a weak acid? 2
Reaction time
A weak acid reacts more slowly than a strong acid.
A strong reacts more faster than a weak acid.
97
# Define Nucleophile 2-3
Substance that donates the e- pair in an organic chemical reaction.
A nucleophile is also a Lewis base.
Typical nucleophiles are CN-, OH- and NH3.
98
When acids react with reactive metals, what forms?
Salt and hydrogen gas
99
100
Identify the acid, base, conjugate acid and conjugate base. NH₃ + C₆H₅COOH ⇌ NH₄⁺ + C₆H₅COO⁻
NH₃ ----- B
C₆H₅COOH ----- A
NH₄⁺ ----- CA
C₆H₅COO⁻ ----- CB
101
What did Robert Doyle write?
Robert Doyle wrote "Experimental History of Colours"
102
103
Define Amphoteric? 1 - 3
A substance that can act both as an acid or a base
e.g. Al₂O₃ and H₂O
Al₂O₃ as a base: Al₂O₃ + 6HCI ⇒ 2AlCI₃ + 3H₂O
Al₂O₃ as an acid: Al₂O₃ + 2NaOH + 3H₂O ⇒ NaAl(OH)₄
104
What is the products of NH₃(aq) + H₂O(l) ⇌
NH₃(aq) + H₂O(l) ⇌ NH₄⁺(aq) + OH⁻(aq)
105
Weak acids ________ dissociate
Partially (Note the yield arrow: We use ⇌)
106
Define Monoprotic
Where one mole of the acid produces one mole of hydrogen ions, e.g. HCl.
107
Define Strong Acids
Strong acids completely dissociate (split up) into ions in an aqueous solution
108
What is the signification of Pka?
Pka is the pH at which the indicator is in the middle of its colour transition
109
All acids release _______ ions into solution
Hydrogen
110
What does pH stand for?
"Power of Hydrogen"
111
Weak acids have _____ conductivity
weak
112
[H⁺] = [HO⁻] = Kc = 1 \* 10⁻⁷ M for \_\_\_\_\_\_\_
pure water
113
What type of bond do Lewis Acids and Bases make?
A coordinated dative bond
114
How do you calculate [H⁺(aq)]? 2
[H⁺(aq)] = antilog (-pH)
Or
[H⁺(aq)] = 10⁻ᵖᴴ
Or When working backwards;
pH = -log [H⁺(aq)]
115
116
How do you accurately determine the pH of a solution?
Using a pH meter
117
What is the compound name of HNO₂?
hydrogen nitrite
118
Since acids are ionic substances, they; 2 (3)
They dissociate in water. And They also conduct electricity in water Called electrolyte
119
Weak acids have weak conjugate bases that will….
Weak acids have weak conjugate bases that will reform back to the original weak acid
120
What two factors affect the [H₃O⁺] for an acid. 2
The labelled concentration of the acid
The strength of the acid
121
When water acts as proton acceptor with HF but as a proton donator, an acid, with ammonia, what is this property called?
Amphoteric
122
Define dissociate
When molecules separate or split into smaller particles such as ions
123
Define Weak Acids
Weak acids slightly dissociate (split up) into ions in an aqueous solution
124
Is H₂O a strong or weak acid/base?
Weak acid
125
# Define Amphiprotic 2
A type of amphoteric substance that specifically can act as neither an acid or base by accepting or donating hydrogen ions.
E.g. water and diprotic acids.
126
Is HCN a strong or weak acid/base?
Weak acid
127
Non-metal oxides mixed with water form……?
acids
128
What is special about the Lewis definition of acids?
There is no requirement for Lewis acids to contain hydrogen
129
What is the points for Bubbling as one of the ways we can distinguish between a strong and a weak acid?
Bubbling
A reaction between an acid and a substance like metal will bubble, releasing hydrogen and the strong acid will bubble more and release hydrogen.
130
Is the chemical reaction of H⁺ + H₂O ⇒ H₃O a Lewis definition or a Brønsted-Lowry definition?
It a Lewis definition and a Brønsted-Lowry definition because H⁺ acid is an electrophile and the H₂O base is a nucleophile making it a Lewis definition. The H⁺ acid is also a proton donor and the H₂O base is a prton acceptor making it a Brønsted-Lowry definition.
131
Is HNO₃, a strong or weak acid/base?
Strong acid
132
Identify the acid, base, conjugate acid and conjugate base. CH₃COOH + OH⁻ ⇌ H₂O + CH₃COO⁻
CH₃COOH ----- acid
OH⁻ ------ base
H₂O ------ CA
CH₃COO⁻ ------ CB
133
[H₃O⁺] = ____________ M for neutral solution
[H₃O⁺] = 1 \* 10⁻⁷ M for neutral solution
134
Identify the acid, base, conjugate acid and conjugate base. NaHSO₄ + NaOH ⇌ Na₂SO₄ + H₂O
NaHSO₄ ----- A
NaOH ----- B
Na₂SO₄ ----- CB
H₂O ----- CA
135
[H₃O⁺] = ____________ M for acidic solution
[H₃O⁺] = 1 \* 10⁻⁷ M for acidic solution
136
137
Weak acids are _____ electrolytes
weak
138
What yield arrow do we use when there is a weak acid/base reacting?
⇒
139
140
What is the fancy name of bubbling?
effervescence
141
Names 3 bases that is a base that doesn't consist of a cation (metal positively charged ion) with a hydroxide
Ammonia, NH₃ and organic amines, R-NH₂
142
When acids and bases were identified by taste, what do acids taste like?
Sour (like most fruits)
143
Is HI, a strong or weak acid/base?
Strong acid
144
145
Is HCIO₄ a strong or weak acid/base?
Strong acid
146
147
Adding yellow to red will not be detectable until you have __ part yellow to 9 parts red
Adding yellow to red will not be detectable until you have 1 part yellow to 9 parts red
148
[H₃O⁺] = ____________ M for alkaline solution
[H₃O⁺] = 1 \* 10⁻⁷ M for alkaline solution
149
What is a hydronium ion?
H₃O⁺
150
After the lichen Rocella, what came as a way to test acids and bases
The litmus test
151
