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CHEMISTRY Module 2: Foundation In Chemistry > 2.1.4 Acids 2.1.5 Redox > Flashcards

2.1.4 Acids 2.1.5 Redox Flashcards

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1
Q

Name the common acids

A

HCl
H2SO4
HNO3
CH3COOH

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2
Q

Name the common alkalis

A

NaOH
KOH
NH3

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3
Q

What do acids do when dissolved in water

A

Release hydrogen ions as protons H+

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4
Q

What do alkalis do when dissolved in water

A

Release hydroxide ions, OH-

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5
Q

What is a strong acid

A

Completely dissociates/ionises in aqueous solution, releases all its hydrogen atoms into solution.

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6
Q

Examples of strong acids

A

HCl
H2SO4
HNO3

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7
Q

What is a weak acid

A

Partially dissociates/ionises in aqueous solution, only releases small proportion of available H atoms into solution as H+

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8
Q

Examples of weak acids

A

CH3COOH

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9
Q

Examples of bases

A

Metal oxides
Metal hydroxides
Metal carbonates
Ammonia

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10
Q

What is a neutralisation reaction?

A

H+ and OH- react to form H20
Reaction between acid and base to form salts

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11
Q

What does acid + metal oxide make

A

Salt + water

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12
Q

What does metal hydroxide + acid make

A

Salt + water

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13
Q

What does acid + alkali make

A

Salt + water

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14
Q

What does acid + metal carbonate make

A

Salt + water + carbon dioxide

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15
Q

What can titrations be used for

A

Finding concentration of a solution
Identification of unknown chemicals
Finding purity of a substance

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16
Q

How to prepare a standard solution

A

Weigh solid accurately
Dissolve solid in beaker using distilled water, less than needed to fill volumetric flask
Transfer solution to volumetric flask
Rinse beaker into flask
Fill flask to graduation line, bottom of meniscus lines up with mark, view from eye level
Slowly invert flask to mix solution

17
Q

How to carry out an acid-base titration

A

Add measured volume of one solution to conical flask using a pipette
Add other solution to burette, record initial reading
Add a few drops of indicator to solution in the conical flask
Run solution in the burette into conical flask, swirl flask throughout.
Indicator changes colour at the end point of the titration.
Record final burette reading, work out titre.
Repeat titration accurately, adding solution drop wise as end point is approached.
Further titrations carried out until 2 accurate titres are concordant (within 0.10cm3)

18
Q

What is the oxidation number for elements

A

0

19
Q

What is the oxidation number for oxygen in compounds

A

-2

20
Q

What is the oxidation number for hydrogen in compounds

A

+1

21
Q

What is the oxidation number for fluorine in compounds

A

-1

22
Q

What is the oxidation number for ions

A

The same as the ionic charge

23
Q

What are the exceptions for the oxidation number rules in compounds

A

Hydrogen is -1 in metal hydrides
Oxygen is -1 in peroxides
Oxygen is +2 when bonded to fluorine

24
Q

What is the sum of oxidation numbers in a compound

A

The total charge

25
Q

Oxidation in terms of electron transfer

A

Loss of electrons

26
Q

Reduction in terms of electron transfer

A

Gain of electrons

27
Q

Oxidation in terms of oxidation number

A

Increase in oxidation number

28
Q

Reduction in terms of oxidation number

A

Decrease in oxidation number

29
Q

Redox reaction of zinc and dilute hydrochloric acid

A

Zn(s) + 2HCl (aq) -> ZnCl2(aq) + H2 (g)

Zinc goes from 0 to +2, oxidation
Hydrogen goes from 1+ to 0, reduction

30
Q

Redox reaction of aluminium with dilute sulfuric acid

A

2Al (s) + 3H2SO4 (aq) -> Al2(SO4)3 (aq) + 3H2 (g)
Aluminium goes from 0 to +3, oxidation
Hydrogen goes from +1 to 0, reduction

CHEMISTRY Module 2: Foundation In Chemistry (5 decks)

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