Reactions in Water Flashcards
1
Q
Describe acid
A
A substance that can donate a proton to a base
2
Q
Describe base
A
A substance with a pH greater than 7
3
Q
Provide a common use of nitric acid
A
Etch copper and manufacture fertiliser
4
Q
Provide the chemical formulae of nitric acid
A
HNO3
5
Q
Provide a common occurence and use of hydrochloric acid
A
Produced in the stomach and used to clean bricks and concrete
6
Q
Provide the chemical formulae of hydrochloric acid
A
HCl
7
Q
Provide a common use of sulfuric acid
A
Used in car batteries, plastics, insecticides, detergents and pharmaceuticals
8
Q
Provide the chemical formulae of sulfuric acid
A
H2SO4
9
Q
Provide a common occurrence of ethanoic acid
A
Found in vinegar
10
Q
Provide the chemical formulae of ethanoic acid
A
CH3COOH
11
Q
Provide a common occurrence of citric acid
A
Found in lemon juice
12
Q
Provide the chemical formulae of citric acid
A
C6H8O7
13
Q
Provide the common occurrence of carbonic acid
A
Found in soft drinks
14
Q
Provide the chemical formulae of carbonic acid
A
H2CO3
15
Q
Provide the common use of lactic acid
A
Makes milk sour
16
Q
Provide the chemical formulae of lactic acid
A
C3H6O3
17
Q
Provide the common occurrence of ascorbic acid
A
Found in citrus fruit
18
Q
Provide the chemical formulae of abscorbic acid
A
C3H8O6
19
Q
State the key to diluting concentrated acids
A
Always add acid to water
20
Q
State the 5 properties of acids
A
- taste sour
- corrosive
- molecular in structure and dissolve in water to produce an electrolyte
- affect the colour of certain natural and synthetic dyes
- neutralised by bases
21
Q
State what acids can be neutralised by
A
Bases
22
Q
State what acids dissolve in water to produce
A
Elecytrolytes
23
Q
Describe electrolytes
A
Substance that conducts electricity
24
Q
State the common products of acid+metal
A
salt+hydrogen gas
25
State the common products of acid+metal carbonate
salt+carbon dioxide gas+water
26
State the common products of acid+metal hydrogen carbonate
salt+carbon dioxide gas+water
27
State the common products of acid+metal sulfite
salt+sulfur dioxide gas+water
28
State the common products of acid+metal sulfide
salt+hydrogen sulfide gas
29
State the common products of acid+metal oxide
salt+water
30
State the common products of acid+base
salt+water
31
State what reactants produce salt+hydrogen gas
acid+metal
32
State what two sets of reactants produce salt+carbon dioxide gas+water
acid+metal carbonate
| acid+metal hydrogen carbonate
33
State what reactants produce salt+sulfur dioxide gas+water
acid+metal sulfite
34
State what reactants produce salt+hydrogen sulfide gas
acid+metal sulfide
35
State what reactants produce salt+water
acid+base
36
State 8 properties of bases
1. bitter taste
2. feel slippery
3. turn litmus from red to blue
4. electrolytes
5. corrosive
6. generally ionic substances
7. oxides/hydroxides of metals
8. usually insoluble in water
37
State what colour litmus turns in the presence of a base
Red to blue
38
State what colour litmus turns in the presence of an acid
Blue to red
39
Provide the chemical formulae for ammonia
NH4
40
Provide a common use of ammonia
Fertilisers and detergents
41
Provide the chemical formulae for sodium hydroxide
NaOH
42
Provide a common use of sodium hydroxide
Soaps and detergents
43
Provide the chemical formulae for sodium carbonate
Na2CO3
44
Provide a common use of sodium carbonate
Manufacture of glass, washing powder and detergent
45
Provide the chemical formulae for calcium oxide
CaO
46
Provide a common use of calcium oxide
Bricklayers mortar
47
Provide the chemical formulae for lead (II) oxide
PbO
48
Provide a common use of lead (II) oxide
House paint
49
Provide the chemical formulae for calcium hydroxide
Ca(OH)2
50
Provide the common use of calcium hydroxide
Garden lime, plaster and cement
51
Provide the chemical formulae for ammonium hydroxide
NH4OH
52
Provide the common use of ammonium hydroxide
Cleaning agents
53
Provide the chemical formulae for magnesium hydroxide
Mg(OH)2
54
Provide the common use of magnesium hydroxide
Milk of magnesia (for treatment of indigestion)
55
State the 2 major statements of the Bronsted-Lowry theory
- An acid is a proton donor
| - A base is a proton acceptor
56
State what a reaction between an acid and a base involves
Proton transfer from the acid to the base
57
State the only time when a proton is transferred from the acid to a base in a reaction
When both the acid and base are present
58
Describe ionisation
Reaction in which substances react with water to produce ions
59
Describe hydrolysis
A reaction in which a substance reacts with water to form OH- or H3O+ ions
60
State what occurs when ionic bases dissolve in water
They dissociate or separate into their constituent ions
61
State whether or not ionic bases ionise when they are introduced to water
They do not ionise since they do not actually react with the water to produce ions as acids do
62
State what is generally produced when an acid and base react with one another
A salt and water are produced
63
Describe spectator ions
Ions that do not take part in a reaction but maintain electrical neutrality in a solution
64
State an alternative formation of an acid-base reaction
Conjugate acid and bases which form
65
Describe conjugate acid-base pairs
Pairs differ by a proton.
66
Provide instructions on how to find the conjugate base of an acid
Subtract 1 H+
67
Provide instructions on how to find the conjugate acid of a base
Add 1 H+
68
State whether or not a conjugate acid and base can reform the original acid and base and if so, how they might do this
Yes. Transfer a proton in a 'backwards' reaction
69
Describe a polyprotic acid
Acids that can donate more than one proton per molecules of acid
70
Describe a diprotic acid
Acids that can donate two protons
71
Describe a monoprotic acid
Acids that can donate one proton
72
Describe a triprotic acid
Acids that can donate three protons
73
State what substances that can donate or accept electrons are referred to as
Amphiprotic
74
Describe amphiprotic substances
Substances that can donate or accept electrons
75
Describe ampholytes
Ionic amphiprotic substances
76
State to what the strength of an acid or base is related to
The ease with which it donates or accepts a proton
77
State what a strong acid will readily donate
Protons
78
State what a strong base will readily accept
Protons
79
State what a strong acid will readily do
Donate protons
80
State what a strong base will readily do
Accept protons
81
State whether or not all strong acid react completely with water
Yes.
82
State whether or not the anions of strong acids have the ability to attract protons
No.
83
State whether or not oxide ions exist in water
No.
84
State why oxide ions do not exist in water
Because they always revert to hydroxide ions
85
State whether or not the strength and concentration of an acid differ from one another
Yes. The strength and concentration of an acid differ
86
State what the strength of a solution is determined by
The number of ions present
87
State what will occur to a strong acid when it is placed in a solution
It will become completely ionised
88
State what will occur to a weak acid when it is placed in a solution
Contains a large number of molecules when compared with the number of ions produced in solution
89
Describe concentration
Refers to the amount of acid or base that is dissolved in a given volume of water
90
State what the concentration and strength of an acid or base solution determine
The number of ions present in the solution
91
Describe the pH scale
A pH scale that is applied over a range from 1-14
92
State what a neutral solution has a pH of
7
93
State what values lower than 7 on the pH scale indicate
Acidic solution
94
The stronger the acid, the lower the
pH value
95
State what is stronger a pH of 3 or a pH of 4
A pH of 3
96
State what values greater than 7 on the pH scale indicate
Basic solution
97
State what the pH of a solution is defined by
-log[H3O+]
98
Describe dilution
Process of adding water to a solution
99
State what dilution may affect in acidic or basic solutions
The concentration of H3O+ ions that are present
100
Describe indicators
Dyes that are usually themselves weak acids or bases
101
State what indicators show
Different colours that allow acidic or basic solutions to be differentiated from one another
102
State what indicators can be used to determine
Whether a substance is acidic or basic and also how acidic or basic it is
103
State the 4 most commonly used indicators
1. Litmus
2. Phenolphthalein
3. Methyl orange
4. Universal indicator
104
Describe what the universal indicator is
A mixture of several different indicators that changes colour gradually from red, to green, to violet
105
State whether or not normal rain is slightly acidic
Yes
106
State why normal rain is slightly acidic
Dissolution of carbon dioxide in water
107
State what the product of CO2+H2O in rain is
Weak carbonic acid (H2CO3)
108
State what carbonic acid reacts slightly with water to produce
Hydronium ions
109
State what the affect of overall acidic rain may be
- defoliation of significant forest areas
- lunar landscape in Queenstown
- run off into lakes has resulted in them being unable to sustain life
110
State whether or not other gases can contribute to the acid rain phenomenon
Yes.
111
State the 5 major responses that have been launched to tackle acid rain
1. catalytic converters of car exhausts to change nitrogen oxides to nitrogen and oxygen
2. use of natural gas a fuels
3. switching to coal with a low sulfur content
4. taking measures to assist the disperal of SO2 (e.g. buying taller chimney stacks)
5. treating exhaust gases to remove undesirable emissions
112
State what dissolves in water to produce carbonic acid
Carbon dioxide
113
State what acidity the oceans have
They are slightly alkaline
114
State from what pH the oceans have dropped to since the Industrial Revolution
Dropped from 8.2 to 8.1
115
State the 4 major issues that could result from acidification
1. coral bleaching
2. interference with marine organisms
3. reproductive disorders
4. interference with shell building
116
State what may occur if the carbonate ion concentration is lowered too much
Calcium carbonate in the shells of marine organisms may dissolve in an attempt to replace the removed carbonate ions
