Acids & Bases

Question 1

Define acid in terms of the Lowry-Brønsted model

Question 2

Define bases in terms of the Lowry-Brønsted model

Question 3

ionisation

Question 4

strong acid + name & formula of common ones
(HCℓ – hydrochloric acid, H2SO4 – sulfuric acid and HNO3 – nitric acid)

Question 5

Classify acids (other than the 3 listed above) as strong when given
sufficient information, e.g. Ka values

Question 6

weak acid + name & formula of common ones
(HF – hydrofluoric acid, H3PO4 – phosphoric acid, H2SO3 – sulfurous acid, (COOH)2 – oxalic acid, CH3COOH – ethanoic acid, and other carboxylic acids)

Question 7

polyprotic acids

Question 8

Distinguish between monoprotic, diprotic and triprotic acids and
give examples of each

Question 9

dissociation

Question 10

strong base + name & formula of common ones
(group 1 hydroxides only)

Question 11

weak base + name & formula of common ones
(NH3(aq) or NH4OH(aq) and know that it is a weak base which only ionises partially in aqueous solution)

Question 12

Know that metal carbonates and metal hydrogen carbonates are
weak base salts (see hydrolysis of a salt)

Question 13

concentrated acid

Question 14

concentrated base

Question 15

dilute acid

Question 16

dilute base

Question 17

amphoteric (or amphiprotic) substance

Question 18

Identify conjugate acid-base pairs for given compounds or
reactions

Question 19

Know that a strong acid has a very weak conjugate base and a
strong base has a very weak conjugate acid

Question 20

Kw, Ka, Kb and pH

Question 21

Explain how conductivity can be used as a measure of acid
strength

Question 22

Explain the auto-ionisation (autoprotolysis) of water

Question 23

Define Kw for water at 25 °C as Kw = [H3O+][OH-]

Question 24

Explain the pH scale as the measure of hydronium ion (H3O+)
concentration in water at 25 °C

Question 25

Explain qualitatively the pH range of 0 to 14

Question 26

salt

Question 27

Write balanced chemical equations representing acid reactions:
- acid + active metal → salt + hydrogen (NB: A redox reaction)
- acid + metal oxide → salt + water
- acid + metal hydroxide → salt + water
- acid + metal carbonate → salt + carbon dioxide + water
- acid + metal hydrogen carbonate → salt + carbon dioxide + water

Question 28

Identify the acid and base (metal or ammonium hydroxide) that could react to produce a given salt

Question 29

hydrolysis of a salt

Question 30

Determine which cation or anion (if any) from a given salt will
undergo hydrolysis and write an equation for this reaction and
hence predict the approximate pH range of the salt solution

Question 31

Predict that the conjugate ions of strong acids and bases do not
undergo hydrolysis,

Question 32

neutralisation

Question 33

standard solution

Question 34

Describe quantitatively and qualitatively how to make up a
standard solution

Question 35

Describe and explain the physical process of performing a titration
to ensure the appropriate precision

Question 36

Select suitable indicators for the relevant titrations from a table of
given indicators and their pH ranges. Titrations between strong
acid/strong base; strong acid/weak base; weak acid/strong base
are considered to be relevant

Question 37

Identify indicators as weak acids and use Le Châtelier’s principle
to predict and explain the colour of the indicator in different acidic
and basic media