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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
What is the difference between strong and weak acids
Strong acids completely dissolve in water, meanwhile weak acids only partially ionise/dissociates in water+ are reversable
26
What is concentration
The quantity of solute dissolved in a litre of aqueous solution
27
What is Concentrated acid Dilute acid
A lot of acid, small volume of water Small amount of acid, relatively large volume of water
28
Properties of alkalis
Soapy feeling Turns litmus paper blue Neutralizes acids
29
What does an acid and a base equal
Salt and water
30
What happens to alkalis in water
They dissociate to form hydroxide ions (OH-)
31
What are strong alkalis
Alkalis that dissociate completely in aqueous solutions
32
What are weak alkalis
Alkalis that partially dissociate in aqueous solution
33
What is the Brønsted-Lowry Theory
Defines acids and bases in terms of proton transfer between chemical compounds
34
What is a Brønsted-Lowry acid
A proton donor
35
Brønsted-Lowry base
A proton acceptor
36
What are amphoteric substances 2 eg.s
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
37
What is a conjugate acid
The substance forms when a base gains an H+ion
38
What is a conjugate base
Substance formed when an acid loses an H+ ion
39
What are the types of oxides + eg
Metal oxides-basic/alkaline producing CuO,CaO,NaOH,KOH Non-metal oxides-acidic, produce acidic aqueous SO2,CO2 Amphoteric oxides Al2O3,ZnO
40
What are oxides called if they do not react + eg
Neutral N2O,NO,CO
41
What is a neutral substance and neutralization (what do they do)
It doesn’t affect the colour of litmus paper Chemical reaction between acid and alkali to produce a solution of salt and water
42
What are the 3 types of oxides
Metal oxides Amphoteric oxides Non-metal oxides
43
Features of metal oxides and 4 examples
Basic Produce alkaline aqueous solution 1-copper oxide (CuO) 2-calcium oxide (CaO) 3-sodium hydroxide (NaOH_ 4-potassium hydroxide (KOH)
44
What do metal oxides react with and what is the product
Acids, Salt and water
45
What are the features of non-metal oxides and 2 eg
Acidic Produce acidic aqueous solutions 1-Sulfur dioxide (SO2) 2.-Carbon dioxide (CO2)
46
What do non-metal oxides reacts with and what is the product
Bases, salt and water
47
What are the features of amphoteric oxides +2 egs
Can be acidic or basic 1- Aluminium Oxide (Al2O3) 2.Zinc Oxide (ZnO)
48
What do amphoteric oxides react with and what is the product
Acid or bases Salt and water
49
What does it mean if something is neutral/a neutral substance
Doesnt react with acid or base Doesnt affect the colour of litmus paper
50
What is neutralisation
The reaction between an acid and a base to form a solution of salt and water
51
What are spectator ions
Ions that do not participate in chemical reactions and are present/remain the saame on both sides of the equations
52
4 examples of neutralisation reactions
Insect stings Indigestion Soil treatment Tooth decay
53
Insect stings and what can neutralise them
Bee= acidic, baking soda (NaHCO3) Wasp=basic, acetic acid/ vinegar (CH3COOH)
54
What is an alkali
A base that dissolves in water
55
What causes idigestion and what neutralises it
Excess HCl in the stomach Antacids-milk of magnesia- Mg(OH)2,NaHCO3
56
Explain soil treatment
Plants like to grow in neutral soil, so quicklime(CaO), slaked lime (Ca(OH)2))or chalk (CaCO3)
57
Explain tooth decay and how it is neutralised
Bacteria produces an acid that eats the enamel on your teeth, toothpaste is an alkaline used to neutralise
58
What are neutral oxides+3 egs
Oxides that do not react with acids or bases Nitrogen dioxide (N2O) Nitrogen monoxide (NO) Carbon monoxide (CO)
59
What is the mail neutralisation reaction
HCl+NaOH=HOH+NaCl
60
What salt does: Nitric acid Hydrochloric acid Sulphuric acid Produce
Nitrate Chloride Sulphate
61
What are salts
Compounds formed when the hydrogen atom in an acid is replaced by a metal from the base/alkali
62
How to you select a method of salt preparation
Decide whether the salt is soluble or insoluble If soluble, then titration or crystallisation If insoluble, then precipitation
63
What is the “formula” for titration and 3 common acids and the bases
Soluble acid+soluble base HCl,H2SO4,HNO3 All the oxides
64
What are the apparatus needed for titration
Burette Pippette Safety burette filler Conical flask
65
describe the process of titration
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
Explain evaporation process
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
what is the water of crystallisation
Water molecules present in hydrated crystals CuSO4 5H20 CoCl2 6H2O
68
What is a saturated solution
A solution that contains the maximun amount of solute that can be dissolved under the condition the solvent exhists.
69
What is the “formula” for crystallisation and 2 common compounds used
Insoluble base+acid CuO, MgO
70
Describe the steps of crystallisation(6)
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
What are waters of crystallisations
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
What is the “formula” for precipitation and what can be used(3)
Soluble+soluble->insoluble AgNO3,PbNO3 or BaCl2
73
What are the steps for precipitation
Add solution(soluble salt) to AgNO3,PbNO3, BaCl2 Filter Wash Allow precipitate to dry on filter paper
74
What is ionisation of acids
When acids react with water and the acid releases an H+ which joins with water to from an oxonium ion.
75
What is an indicator
An organic dye which changes colour based on the change of H+ ions in a solution
76
Why do you repeat titration without the indicator
The indicator contaminâtes the salt, repeating it will allow for a pure salt.
77
Why do you add excess insoluble bases in crystallization
So that all of the insoluble base reacts with all the acid. You can filter out base, but not acid.
78
What is the difference between the products of crystallization and precipitation and how they are prepared
Crystallization forms crystals Precipitation forms precipitate Precipitate is washed, crystals arent
79
What metallic oxides acidic or basic?
Basic
80
Are non metallic oxides acidic or basic
Acidic
81
What is an ionic equation
An equation showing all the separate ions partaking in a reaction
82
What is the most common indicator used for titrations
Phenolphthalien
83
What does crystallisation form vs precipitation
Insoluble salt/crystal Insoluble salt/base
84
What 3 compounds are solutions added to in precipitation
AgNO3 PbNO3 BaCl
85
What are the solubility rules(5)
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
Describe an experiment to show that aluminum oxide is amphoteric
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
Physical properties of silicon (IV) oxide
high melting point/ high boiling point; poor conductor (of electricity); hard; insoluble;
88
What oxides do metals form
Basic
89
What is an oxide
Chemical compound containing at least one oxygen atom and another element
90
Dissociation of ethanoic acid
91
Dissociation of HCL
HCl -> H+ +Cl-
92
What does an aqueous solution of acids contain
H+ ions
93
What does an aqueous solution of alkalis contain
OH- ions
94
Can acids and bases conduct electricity
Yes because they contain dissolved ions (they are electrolytes)
95
Base and ammonium salt reaction
Salt, ammonia gas and water
96
How does metallic character relate to oxides being acidic or basic
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
Hydrated substance
Substance that is chemically combined with water
98
Anhydrous substance
Substance containing no water
99
CuCl2 anhydrous and hydrated colours
Yellow Green

IGCSE Chemistry (21 decks)

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