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AS level - Chemistry > Chapter 4 - Acids and redox > Flashcards

Chapter 4 - Acids and redox Flashcards

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1
Q

What is a Bronsted- Lowry Acids

A

They are defined to be proton donors.

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2
Q

What is a Bronsted-Lowry Base

A

They are defined to the proton acceptors

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3
Q

Give 3 examples of strong acids

A 
Sulfuric acid (H2SO4)
Hydrochloric acid (HCl)
Nitric acid (HNO3)
Because they are all inorganic acids (or minerals)
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4
Q

Give an example of a weak acid

A 
Ethanoic acid (CH3COOH)
Just carboxylic acids in general because they are organic acids.
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5
Q

What is the difference between an alkali and a base

A

An alkali is any soluble base.

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6
Q

3 examples of strong alkalis

A

NaOH
KOH
Ca(OH)2

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7
Q

1 example of a weak acid

A

NH4OH

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8
Q

acid + alkali –>

A

salt and water

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9
Q

acid + carbonate –>

A

salt + water + carbon dioxide

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10
Q

Ionic equation for neutralisation

A

H+(aq) + OH-(aq) –> H20 (l)

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11
Q

Explain sulfuric acid’s strength

A

It has 2 hydrogen atoms, but it is only strong for one of them. So it fully dissociates with 1, and then partially dissociates in the other.
H2SO4(aq) –> H+(aq) + HSO4-(aq)
HSO4-(aq) H+(aq) + SO4 2- (aq)

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12
Q

ionic equation for acid and oxides

A

2H+ + O2- –> H20

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13
Q

ionic equation for acid and carbonates

A

2H+ + CO3 2- –> H2O + CO2

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14
Q

ionic equation for when water mixes with hydrogen

A

H+(aq) + H2O(l) –> H3O+(aq)
This happens by a dative covalent bond because the oxygen had 2 lone pairs, one of which it now shares with this third hydrogen.
The new compound is called hydroxonium.

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15
Q

What is titration

A

A technique used to accurately measure the volume of an unknown solution that reacts exactly with another known solution.

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16
Q

What can titrations be used for

A

finding the concentration of a solution
identification of unknown chemicals
finding the purity of a substance

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17
Q

Explain diprotic molecule

A

It is a molecule that has 2 hydrogens. Immediately, this is the stronger acid because it has more hydrogen ions to release and carry the charge.

18
Q

As a solution is diluted, what happens to its current flow

A

If a solution is diluted, the concentration of H+ ions decreases. If there is less ions to carry the charge, the electrical conductivity will decrease.

19
Q

Why does a stronger acid have a higher electrical conductivity?

A

A stronger acid can ionise fully and release more ions per unit of volume of solution to carry the charge through the electrolyte.

20
Q

Rule for halogens

A

They are usually -1.

But they are positive with oxygen and fluorine

21
Q

Rule for hydrogen with metals

A

-1 oxidation number

22
Q

Rule for hydrogen with non- metals

A

+1 oxidation number

23
Q

Rule for oxygen

A

Usually -2

But -1 is peroxide (H2O2)

24
Q

Rule for fluorine

A

Always -1

25
Q

How to calculate percentage uncertainty

A

uncertainty/ capacity * 100%

26
Q

What is the % uncertainty on a 100cm3 volumetric flask

A

+- 0.20cm3

27
Q

What is the % uncertainty on a 250cm3 volumetric flask

A

+- 0.30cm3

28
Q

Effect on titre if the pipette has an air bubble

A

creates a smaller titre because there is actually less volume

29
Q

Effect on the titre if the burette reading are taken from the top, rather than the bottom of the meniscus

A

Wouldn’t be affected because the change in volume would still be the same.

30
Q

when do you multiply the number by 2 when calculating the % uncertainty

A

if you have used that object twice

31
Q

Uncertainty of a 10cm3 pipette

A

+- 0.04 cm3

32
Q

Uncertainty of a 25cm3 pipette

A

+- 0.06cm3

33
Q

Uncertainty of a 50cm3 pipette

A

+- 0.10cm3 (0.05 * 2 because its read twice)

34
Q

oxidation numbers:

reduction

A

decrease in oxidation number

35
Q

oxidation numbers:

oxidation

A

increase in oxidation numbers

36
Q

H in metal hydrides

A

-1

37
Q

O in peroxide (H2O2)

A

-1

38
Q

O is bonded to F

A

+2

39
Q

nitrite

A

no2 +3

40
Q

nitrate

A

no3 +5

AS level - Chemistry (19 decks)

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