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IGCSE Chemistry > 7.1 Acids And Bases > Flashcards

7.1 Acids And Bases Flashcards

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1
Q

What is another name for oxonium

A

Hydronium
H3O+

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2
Q

Name 7 examples of acids

A

Hydrochloric
Nitric
Sulfuric
Sulfurous
Carbonic
Nitrous
Ethanoic

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3
Q

Formula of the following acids:
hydrochloric
Nitric
Sulfuric
Sulfurous
Carbonic
Nitrous
Ethanoic/acetic

A

HCl
HNO3
H2SO4
H2SO3
H2CO3
HNO2
CH3COOH

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4
Q

Name 3 strong acids+uses

A

Hydrochloric-stomach acid/clean metal surfaces
Nitric-fertilizer/explosives
Sulfuric-car batteries+paint

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5
Q

Name 4 weak acids+uses

A

Sulfurous-acid rain
Nitrous-atmosphere
Ethanoic-major compound in vinegar
Carbonic-fizzy drinks

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6
Q

Name 5 indicators + their colours in bases

A

Litmus- blue
Phenolphthalein- pink
Methyl orange - orange yellow
Thymolphthalein - blue
Bromothymol blue - blue

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7
Q

Name 5 indicators+their colours in acids

A

Litmus - red
Phenolphthalein - colour less
Methyl orange - pink/red
Thymolphthalein - colour less
Bromothymol blue - yellow

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8
Q

Acid reacting with metal

A

Acid + metal -> salt + hydrogen gas

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9
Q

Acid/metal reacting with bases(3)

A

Acid+base -> salt+water
Acid+metal oxide->salt+water
Metal+hydroxide=salt+water

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10
Q

Is a metal hydroxide an acid or a base

A

Base

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11
Q

Acid reacting with metal carbonate

A

Acid+metal carbonate->salt+carbon dioxide+water

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12
Q

Acid reacting with ammonia

A

Acid+ammonia->ammonium salt

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13
Q

What diprotic acids

A

Acids that have 2 hydrogens (protons) and are able to donate?
React with 2 waters to form 2 oxonium ions and the other ion has a -2 charge

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14
Q

What happens when acids react with water

A

They undergo a process called ionisation
The acid releases an H+ ion which joins to water to form an oxonium ion (positive)(the other ion will always be negative)

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15
Q

What is oxonium formula

A

H30+
(Always positive)

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16
Q

What are acids

A

Proton donors which produce an excess of H+ ions that react with bases to form water

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17
Q

What is responsible for the properties of acids+ the properties

A

The H+ ion
-Sour taste
-pH below 7
-Soluble in water

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18
Q

Why can acids form aqueous solutions

A

Because acids are soluble in water

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19
Q

4 examples of alkalis+formula+uses

A

NaOH- caustic soda-clean drains
KOH- caustic potash-defoam in manufacture of paper
NH4OH- cloudy ammonia-cleaning+manufacture HNO3
Ca(OH)2-lime water-improve soils, cement, neutralisation of acids

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20
Q

What is a base

A

Proton acceptors that react with H+ ions of acids to form water
(Any compound that can neutralize an acid)
Hydroxides/oxides of metals

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21
Q

What are alkalis+eg

A

Soluble bases which have an excess of OH ions
NaOH

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22
Q

Do bases always dissolve in water

A

No

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23
Q

Name 5 bases

A

Metal oxides
Metal hydroxides
Metal carbonate
Metal hydrogen carbonate
Ammonia solutions

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24
Q

What can be used to test pH

A

Universal indicator

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25
Q

What is the difference between strong and weak acids

A

Strong acids completely dissolve in water, meanwhile weak acids only partially ionise/dissociates in water+ are reversable

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26
Q

What is concentration

A

The quantity of solute dissolved in a litre of aqueous solution

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27
Q

What is
Concentrated acid
Dilute acid

A

A lot of acid, small volume of water
Small amount of acid, relatively large volume of water

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28
Q

Properties of alkalis

A

Soapy feeling
Turns litmus paper blue
Neutralizes acids

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29
Q

What does an acid and a base equal

A

Salt and water

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30
Q

What happens to alkalis in water

A

They dissociate to form hydroxide ions (OH-)

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31
Q

What are strong alkalis

A

Alkalis that dissociate completely in aqueous solutions

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32
Q

What are weak alkalis

A

Alkalis that partially dissociate in aqueous solution

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33
Q

What is the Brønsted-Lowry Theory

A

Defines acids and bases in terms of proton transfer between chemical compounds

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34
Q

What is a Brønsted-Lowry acid

A

A proton donor

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35
Q

Brønsted-Lowry base

A

A proton acceptor

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36
Q

What are amphoteric substances
2 eg.s

A

Substances that can act as both acids and bases depending on the reaction
Oxides that react with acids and bases to produce salt and water
ZnO
Al2O3

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37
Q

What is a conjugate acid

A

The substance forms when a base gains an H+ion

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38
Q

What is a conjugate base

A

Substance formed when an acid loses an H+ ion

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39
Q

What are the types of oxides + eg

A

Metal oxides-basic/alkaline producing CuO,CaO,NaOH,KOH
Non-metal oxides-acidic, produce acidic aqueous SO2,CO2
Amphoteric oxides Al2O3,ZnO

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40
Q

What are oxides called if they do not react + eg

A

Neutral
N2O,NO,CO

41
Q

What is a neutral substance and neutralization (what do they do)

A

It doesn’t affect the colour of litmus paper
Chemical reaction between acid and alkali to produce a solution of salt and water

42
Q

What are the 3 types of oxides

A

Metal oxides
Amphoteric oxides
Non-metal oxides

43
Q

Features of metal oxides and 4 examples

A

Basic
Produce alkaline aqueous solution
1-copper oxide (CuO)
2-calcium oxide (CaO)
3-sodium hydroxide (NaOH_
4-potassium hydroxide (KOH)

44
Q

What do metal oxides react with and what is the product

A

Acids, Salt and water

45
Q

What are the features of non-metal oxides and 2 eg

A

Acidic
Produce acidic aqueous solutions
1-Sulfur dioxide (SO2)
2.-Carbon dioxide (CO2)

46
Q

What do non-metal oxides reacts with and what is the product

A

Bases, salt and water

47
Q

What are the features of amphoteric oxides +2 egs

A

Can be acidic or basic
1- Aluminium Oxide (Al2O3)
2.Zinc Oxide (ZnO)

48
Q

What do amphoteric oxides react with and what is the product

A

Acid or bases
Salt and water

49
Q

What does it mean if something is neutral/a neutral substance

A

Doesnt react with acid or base
Doesnt affect the colour of litmus paper

50
Q

What is neutralisation

A

The reaction between an acid and a base to form a solution of salt and water

51
Q

What are spectator ions

A

Ions that do not participate in chemical reactions and are present/remain the saame on both sides of the equations

52
Q

4 examples of neutralisation reactions

A

Insect stings
Indigestion
Soil treatment
Tooth decay

53
Q

Insect stings and what can neutralise them

A

Bee= acidic, baking soda (NaHCO3)
Wasp=basic, acetic acid/ vinegar (CH3COOH)

54
Q

What is an alkali

A

A base that dissolves in water

55
Q

What causes idigestion and what neutralises it

A

Excess HCl in the stomach
Antacids-milk of magnesia- Mg(OH)2,NaHCO3

56
Q

Explain soil treatment

A

Plants like to grow in neutral soil, so quicklime(CaO), slaked lime (Ca(OH)2))or chalk (CaCO3)

57
Q

Explain tooth decay and how it is neutralised

A

Bacteria produces an acid that eats the enamel on your teeth, toothpaste is an alkaline used to neutralise

58
Q

What are neutral oxides+3 egs

A

Oxides that do not react with acids or bases
Nitrogen dioxide (N2O)
Nitrogen monoxide (NO)
Carbon monoxide (CO)

59
Q

What is the mail neutralisation reaction

A

HCl+NaOH=HOH+NaCl

60
Q

What salt does:
Nitric acid
Hydrochloric acid
Sulphuric acid
Produce

A

Nitrate
Chloride
Sulphate

61
Q

What are salts

A

Compounds formed when the hydrogen atom in an acid is replaced by a metal from the base/alkali

62
Q

How to you select a method of salt preparation

A

Decide whether the salt is soluble or insoluble
If soluble, then titration or crystallisation
If insoluble, then precipitation

63
Q

What is the “formula” for titration and 3 common acids and the bases

A

Soluble acid+soluble base
HCl,H2SO4,HNO3
All the oxides

64
Q

What are the apparatus needed for titration

A

Burette
Pippette
Safety burette filler
Conical flask

65
Q

describe the process of titration

A

Pippette 25cm3 of acid into conical flask
Add a few drops of indicator to flask
Fill burette with alkali
Slowly add alkali to acid until colour changes
Repeat titration without indicator
Evaporation:heat solution until all water evaporates and only salt remains

66
Q

Explain evaporation process

A

Solution is placed in a evaporating basin and is heated with a bunsen burner, the solution becomes more concentrated as it evaporates, once all the solution has evaporated, only the crystal solute will remain.

67
Q

what is the water of crystallisation

A

Water molecules present in hydrated crystals
CuSO4
5H20
CoCl2
6H2O

68
Q

What is a saturated solution

A

A solution that contains the maximun amount of solute that can be dissolved under the condition the solvent exhists.

69
Q

What is the “formula” for crystallisation and 2 common compounds used

A

Insoluble base+acid
CuO, MgO

70
Q

Describe the steps of crystallisation(6)

A

Add excess insoluble base to acid and allow to react
Separate excess solid from filtrate by filtration
Heat filtrate gently to form a saturated solution
Cool saturated solutions to allow for crystallisation
Dry the crystals between pages of filter paper

71
Q

What are waters of crystallisations

A

Water molecules present in hydrated crystals
(Formulas separated by a dot) that can be hydrated to different degrees.
If there is no wtaer in the structure, it is an anhydrous compound, these can be formed/reversed by heating the hyrdrated compound

72
Q

What is the “formula” for precipitation and what can be used(3)

A

Soluble+soluble->insoluble
AgNO3,PbNO3 or BaCl2

73
Q

What are the steps for precipitation

A

Add solution(soluble salt) to AgNO3,PbNO3, BaCl2
Filter
Wash
Allow precipitate to dry on filter paper

74
Q

What is ionisation of acids

A

When acids react with water and the acid releases an H+ which joins with water to from an oxonium ion.

75
Q

What is an indicator

A

An organic dye which changes colour based on the change of H+ ions in a solution

76
Q

Why do you repeat titration without the indicator

A

The indicator contaminâtes the salt, repeating it will allow for a pure salt.

77
Q

Why do you add excess insoluble bases in crystallization

A

So that all of the insoluble base reacts with all the acid. You can filter out base, but not acid.

78
Q

What is the difference between the products of crystallization and precipitation and how they are prepared

A

Crystallization forms crystals
Precipitation forms precipitate
Precipitate is washed, crystals arent

79
Q

What metallic oxides acidic or basic?

A

Basic

80
Q

Are non metallic oxides acidic or basic

A

Acidic

81
Q

What is an ionic equation

A

An equation showing all the separate ions partaking in a reaction

82
Q

What is the most common indicator used for titrations

A

Phenolphthalien

83
Q

What does crystallisation form vs precipitation

A

Insoluble salt/crystal
Insoluble salt/base

84
Q

What 3 compounds are solutions added to in precipitation

A

AgNO3
PbNO3
BaCl

85
Q

What are the solubility rules(5)

A
  1. All common salts of the Group 1A elements and ammonium are soluble.
  2. All common acetates and nitrates are soluble.
  3. All binary compounds of Group VIIA elements (other than F) with metals are soluble except those of silver, mercury (1), and lead.
  4. All sulfates are soluble except those of barium, strontium, lead, calcium, silver, and mercury(1).
  5. Except for those in Rule 1, carbonates, hydroxides, oxides, and phosphates are insoluble
86
Q

Describe an experiment to show that aluminum oxide is amphoteric

A

add a named acid, e.g. HCI and a named alkali, e.g. NaOH;
Al203 will react with /neutralises both reagents;
and so it will dissolve into the reagent /form a solution;

87
Q

Physical properties of silicon (IV) oxide

A

high melting point/ high boiling point;
poor conductor (of electricity);
hard;
insoluble;

88
Q

What oxides do metals form

A

Basic

89
Q

What is an oxide

A

Chemical compound containing at least one oxygen atom and another element

90
Q

Dissociation of ethanoic acid

A
91
Q

Dissociation of HCL

A

HCl -> H+ +Cl-

92
Q

What does an aqueous solution of acids contain

A

H+ ions

93
Q

What does an aqueous solution of alkalis contain

A

OH- ions

94
Q

Can acids and bases conduct electricity

A

Yes because they contain dissolved ions (they are electrolytes)

95
Q

Base and ammonium salt reaction

A

Salt, ammonia gas and water

96
Q

How does metallic character relate to oxides being acidic or basic

A

Metals are basic in nature, and metallic character decreases from left to right on the periodic table meaning the oxides become acidic as you move to the right

97
Q

Hydrated substance

A

Substance that is chemically combined with water

98
Q

Anhydrous substance

A

Substance containing no water

99
Q

CuCl2 anhydrous and hydrated colours

A

Yellow
Green

IGCSE Chemistry (21 decks)

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