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Chemistry > Acids & Alkalis > Flashcards

Acids & Alkalis Flashcards

(87 cards)

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1
Q

Neutralisation

A

When an acid reacts with a alkali to produce a neutral solution of a salt and water

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2
Q

Indicator and examples

A

Something that changes colour due to a change in pH

E.g. Litmus, methyl orange, phenolphthalein

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3
Q

Hydrochloric acid formula

A

HCl

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4
Q

Sulfuric acid formula

A

H2SO4

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5
Q

Nitric acid formula

A

HNO3

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6
Q

All acids contain… The more concentrated the H+ ions…

A

All acids contain hydrogen atoms. When acids dissolve in water they form H+ ions. Therefore the pH of the acid will be lower

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7
Q

aq

A

Aqueous solution = dissolved in water

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8
Q

All alkaline solutions contain… the more concentrated the OH- ions…

A

Contain OH- ions (hydroxide ions). The higher the pH of the alkali

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9
Q

Concentration def

A

How many particles are dissolved in a given volume of liquid

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10
Q

Strength of an acid/alkali is determined by

A

Concentration, ability to donate hydrogen (protons) - more protons mean more dangerous means reactive

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11
Q

High concentration means

A

Weak acid - partially dissociate

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12
Q

Low concentration means

A

Strong acid - completely dissociate

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13
Q

More hydrogen ions (protons) do…

A

More damage

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14
Q

Work out concentration

A

Amount dissolved (g) / volume (dm3)

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15
Q

1dm3

A

1000cm3

1l

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16
Q

By increasing volume, the concentration

A

Decreases

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17
Q

Mole

A

6.02x10^23

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18
Q

Strong acid

A

Higher concentration of H+ ions and ability to donate protons

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19
Q

Increase pH

A

Decrease concentration of hydrogen ions

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20
Q

Base + acid —>

A

Salt + water

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21
Q

pH probe attached to a pH meter

A

More accurate than universal indicator as it gives a numerical value

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22
Q

Which ion is produced by an acid in aqueous solution

A

H+

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23
Q

Ethanoic/Acetic acid formula

A

CH3COOH

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24
Q

Citric acid formula

A

C6H8O7

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25
Carbonic acid formula
H2CO3
26
Strong (good proton donors) acids to weak acids
Sulphuric, hydrochloric, nitric, citric, ethanoic, carbonic
27
Dissociate
Breaking down of hydrogen ions and separating of anions
28
Dynamic equilibrium
Forward and back at the same rate
29
Tip for doing ionic equations
Start with the H+ ions first and don't forget about group ions and their charges
30
SO4 charge
2-
31
NO3 charge
1-
32
CO3 charge
2-
33
Partially dissociate citric acid
3H+ + C6H5O7 3-
34
Bases end in
Oxides, hydroxides, carbonates
35
Alkali is a
Soluble base
36
Concentrated vs dilute
More acid molecules per cm3 vs less
37
Anhydrous solution
Water is driven out
38
Base is
Any chemical that neutralises acids to make a salt and water only
39
Sodium hydroxide formula
NaOH
40
Potassium hydroxide formula
KOH
41
Calcium hydroxide formula
Ca(OH)2
42
Lithium hydroxide
LiOH
43
Strong acids ( in terms of ions)
Strong completely dissociate into ions in solutions
44
Weak acids (in terms of ions)
Partly break up into ions
45
A concentrated solution
Contains lots of solute compared to the volume of solvent
46
Dilute solution
Contains small amounts of solute compared to the volume of solvent
47
Safety when making copper sulfate
Eye protection e.g. goggles, copper oxide is harmful especially when in eyes and scratch then, sulphuric acid is irritant
48
How to make copper sulfate
Pour 20cm3 of dilute sulphuric acid into the conical flask. Warm the acid to 50°C using a water bath. Use a spatula to add a little copper oxide to the acid and stir using a glass rod. Keep repeating until all acid has reacted. Filter mixture and transfer to evaporating dish. Heat mixture over water bath until crystals start to form. Then leave in sun to evaporate water
49
Titration
When an acid is added from a burette to a fixed volume of alkali in a comical flask to obtain a neutral solution
50
Burette
A tall piece of glassware used to release small drops of liquid to obtain an accurate volume to neutralise a solution
51
Titration experiment
Use a pipette to measure the alkali. Use single indicators such as phenolphthalein or methyl orange as they have obvious colour changes to give a sharper endpoint. Use a white tile to make the colour change easier to see
52
When to use methyl orange and colour change
Strong acid + weak alkali (turns red in acid and yellow/orange in alkali)
53
When to use phenolphthalein and colour change
Weak acid and strong alkali (turns colourless in acid and pink in alkali)
54
Safety precaution with titration experiment
Fill burette below eye level. It can spill into your eyes and cause harm
55
Concentration formula in terms of moles
Number of moles divided by volume
56
If the concentration of hydrogen ions increases by a factor of 10, the pH…
Decreases by 1
57
What happens during neutralisation
Hydrogen ions in the acid combine with oxide ions to form water. This removes the hydrogen ions and so the pH increases by becoming more neutral. The salts are produced by replacing the hydrogen ions with metal ions
58
Ionic equation for hydrochloric acid
HCl --> H+ + Cl-
59
Ionic equation for sulphuric acid
H2SO4 --> 2H+ + SO4 2-
60
Ionic equation for nitric acid
HNO3 --> H+ + NO3-
61
Ionic equation for ethanoic acid
CH3COOH H+ + CH3COO-
62
Ionic equation for calcium hydroxide
Ca(OH)2 --> Ca2+ + 2OH-
63
How to make soluble salt that isn't contaminated
Use a pH meter to check its neutral
64
Titre
Initial volume - final reading
65
Titration experiment
Tie long hair back and put on goggles. Measure using a pipette the alkali into the conical flask and add phenol. Place white tile under flask. Fill burette and remove the funnel. Add initial reading to table measuring under meniscus. Add acid slowly and swirl gently. Once colour change is permanent record final reading. Note the titre reading
66
What observations can be seen during a reaction between an acid and a metal
Fizzing and dissolving
67
What is produced from reacting metal and acid together
Metal + acid --> salt + hydrogen
68
How to test for hydrogen
Squeaky pop test. A lot splint will go out and make a popping sound in the presence of hydrogen gas
69
Carbonate + acid
--> salt + water + carbon dioxide
70
What observation can be seen when reacting metal carbonates with acids
Dissolving
71
Test for carbon dioxide
Clear limewater goes cloudy when carbon dioxide is added
72
Metal reactivity series
Potassium Sodium Calcium Magnesium Aluminium (carbon) Zinc Iron Tin Lithium Copper Silver Gold Platinum
73
OILRIG
Oxidation is Loss, Reduction is Gain
74
Half equation for metal
E.g. Na --> Na+ + e-
75
Half equation for non metal
Cl + e- --> Cl-
76
(Solubility) most chlorides
Soluble
77
(Solubility) most sulfates
Soluble
78
(Solubility) Most carbonates
Insoluble
79
(Solubility) Most hydroxides
Insoluble
80
(Solubility) all nitrates
Soluble
81
Silver and lead chloride (Solubility)
Insoluble
82
Lead, barium, calcium sulfate (Solubility)
Insoluble
83
Sodium, potassium, ammonium carbonates (Solubility)
Soluble
84
Sodium, potassium, ammonium hydroxide (Solubility)
Soluble
85
Solubility def
A measure of how much of a substance will dissolve in a litre of water
86
Precipitate reaction
2 aqueous solutions make a solid product
87
Precipitate experiment
Mix two aqueous solutions together in equal amounts to make a neutral homogeneous solution. Pour through filter paper onto a conical flask. Keep the filtrate. Wash with distilled water to dissolve soluble ions to make it pure. Leave to dry and evaporate water

Chemistry (10 decks)

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