1.30 recall the charges of common ions in this specification

K +
Na +
Li +
H +

Mg 2+
Ca 2+

Al 3+

Cl-
Br-
I-
F-
OH-

NO3-

SO4 2-

CO3 2-

5.31 describe important uses of sodium hydroxide, including the manufacture of bleach, paper and soap; and of chlorine, including sterilising water supplies and in the manufacture of bleach and hydrochloric acid.

Sodium Hydroxide: Bleach; paper; soap

Chlorine: sterilising water; bleach; hydrochloric acid

5.30 write ionic half-equations for the reactions at the electrodes in the diaphragm cell

2 Cl- > Cl2 + 2e-
2 H+ + 2e- > H2

Really useful video:
http://www.youtube.com/watch?v=BUvnwUdtwqo

5.29 describe the manufacture of sodium hydroxide and chlorine by the electrolysis of concentrated sodium chloride solution (brine) in a diaphragm cell

Brine is NaCl solution.
In electrolysis, chlorine is created at the anode, hydrogen is created at the cathode, sodium hydroxide is left in the solution.

2NaCl + 2H2O > 2NaOH + H2 + Cl2

This happens in a diaphragm cell.

5.28 describe the use of sulfuric acid in the manufacture of detergents, fertilisers and paints

Detergents: used to 'sulphonate' products (apperently.)
Fertilisers: reacted to make phosphates soluble to plants: reacted to make ammonia easier to handle.
Paints: reacted with titanium ore to make a main pigment in paint.

http://bscstriplescience.wikispaces.com/file/view/C3_4_12+Why+is+sulphuric+acid+important.pdf

5.27 describe the manufacture of sulfuric acid by the contact process, including the essential conditions

(stage 1) S + O2 > SO2 
(stage 2) SO2 + O > SO3
(satge 3) SO3 + H2O > H2SO4

freewebs

i) a temperature of about 450C

ii) a pressure of about 2 atmospheres

iii) a vanadium(V) oxide catalyst (in stage 2)

Very helpful source:
http://namedorganicreactions.co.uk/Sulphuric.pdf

5.26 recall the raw materials used in the manufacture of sulfuric acid

Sulphur (sulphur is found in rocks and some natural gasses) and oxygen from the air and water.