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Chemistry > Acids & Alkalis > Flashcards

Acids & Alkalis Flashcards

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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
Q

Carbonic acid formula

A

H2CO3

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26
Q

Strong (good proton donors) acids to weak acids

A

Sulphuric, hydrochloric, nitric, citric, ethanoic, carbonic

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27
Q

Dissociate

A

Breaking down of hydrogen ions and separating of anions

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28
Q

Dynamic equilibrium

A

Forward and back at the same rate

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29
Q

Tip for doing ionic equations

A

Start with the H+ ions first and don’t forget about group ions and their charges

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30
Q

SO4 charge

A

2-

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31
Q

NO3 charge

A

1-

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32
Q

CO3 charge

A

2-

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33
Q

Partially dissociate citric acid

A

3H+ + C6H5O7 3-

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34
Q

Bases end in

A

Oxides, hydroxides, carbonates

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35
Q

Alkali is a

A

Soluble base

36
Q

Concentrated vs dilute

A

More acid molecules per cm3 vs less

37
Q

Anhydrous solution

A

Water is driven out

38
Q

Base is

A

Any chemical that neutralises acids to make a salt and water only

39
Q

Sodium hydroxide formula

A

NaOH

40
Q

Potassium hydroxide formula

A

KOH

41
Q

Calcium hydroxide formula

A

Ca(OH)2

42
Q

Lithium hydroxide

A

LiOH

43
Q

Strong acids ( in terms of ions)

A

Strong completely dissociate into ions in solutions

44
Q

Weak acids (in terms of ions)

A

Partly break up into ions

45
Q

A concentrated solution

A

Contains lots of solute compared to the volume of solvent

46
Q

Dilute solution

A

Contains small amounts of solute compared to the volume of solvent

47
Q

Safety when making copper sulfate

A

Eye protection e.g. goggles, copper oxide is harmful especially when in eyes and scratch then, sulphuric acid is irritant

48
Q

How to make copper sulfate

A

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
Q

Titration

A

When an acid is added from a burette to a fixed volume of alkali in a comical flask to obtain a neutral solution

50
Q

Burette

A

A tall piece of glassware used to release small drops of liquid to obtain an accurate volume to neutralise a solution

51
Q

Titration experiment

A

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
Q

When to use methyl orange and colour change

A

Strong acid + weak alkali (turns red in acid and yellow/orange in alkali)

53
Q

When to use phenolphthalein and colour change

A

Weak acid and strong alkali (turns colourless in acid and pink in alkali)

54
Q

Safety precaution with titration experiment

A

Fill burette below eye level. It can spill into your eyes and cause harm

55
Q

Concentration formula in terms of moles

A

Number of moles divided by volume

56
Q

If the concentration of hydrogen ions increases by a factor of 10, the pH…

A

Decreases by 1

57
Q

What happens during neutralisation

A

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
Q

Ionic equation for hydrochloric acid

A

HCl –> H+ + Cl-

59
Q

Ionic equation for sulphuric acid

A

H2SO4 –> 2H+ + SO4 2-

60
Q

Ionic equation for nitric acid

A

HNO3 –> H+ + NO3-

61
Q

Ionic equation for ethanoic acid

A

CH3COOH H+ + CH3COO-

62
Q

Ionic equation for calcium hydroxide

A

Ca(OH)2 –> Ca2+ + 2OH-

63
Q

How to make soluble salt that isn’t contaminated

A

Use a pH meter to check its neutral

64
Q

Titre

A

Initial volume - final reading

65
Q

Titration experiment

A

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
Q

What observations can be seen during a reaction between an acid and a metal

A

Fizzing and dissolving

67
Q

What is produced from reacting metal and acid together

A

Metal + acid –> salt + hydrogen

68
Q

How to test for hydrogen

A

Squeaky pop test. A lot splint will go out and make a popping sound in the presence of hydrogen gas

69
Q

Carbonate + acid

A

–> salt + water + carbon dioxide

70
Q

What observation can be seen when reacting metal carbonates with acids

A

Dissolving

71
Q

Test for carbon dioxide

A

Clear limewater goes cloudy when carbon dioxide is added

72
Q

Metal reactivity series

A

Potassium Sodium Calcium Magnesium Aluminium (carbon) Zinc Iron Tin Lithium Copper Silver Gold Platinum

73
Q

OILRIG

A

Oxidation is Loss, Reduction is Gain

74
Q

Half equation for metal

A

E.g. Na –> Na+ + e-

75
Q

Half equation for non metal

A

Cl + e- –> Cl-

76
Q

(Solubility) most chlorides

A

Soluble

77
Q

(Solubility) most sulfates

A

Soluble

78
Q

(Solubility) Most carbonates

A

Insoluble

79
Q

(Solubility) Most hydroxides

A

Insoluble

80
Q

(Solubility) all nitrates

A

Soluble

81
Q

Silver and lead chloride (Solubility)

A

Insoluble

82
Q

Lead, barium, calcium sulfate (Solubility)

A

Insoluble

83
Q

Sodium, potassium, ammonium carbonates (Solubility)

A

Soluble

84
Q

Sodium, potassium, ammonium hydroxide (Solubility)

A

Soluble

85
Q

Solubility def

A

A measure of how much of a substance will dissolve in a litre of water

86
Q

Precipitate reaction

A

2 aqueous solutions make a solid product

87
Q

Precipitate experiment

A

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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